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FAQ: What Is A Primary Health Care Center?
Home > Health Center > FAQ: What Is A Primary Health Care Center?
1 What is meant by primary health Centre?
2 What are examples of primary health care?
3 What is the role of primary health Centre?
4 What are the 7 principles of primary health care?
5 What are the 8 elements of primary health care?
6 What is the difference between primary health care and primary care?
7 What are the 10 components of primary healthcare?
8 How is primary health care delivered?
9 Why is primary care so important?
10 What are the disadvantages of primary health care?
11 What are the four pillars of primary health care?
12 Who is the father of PHC?
13 What are the basic principles of primary health care?
What is meant by primary health Centre?
DEFINITION The primary health center (PHC) is the basic structural and functional unit of the public health services in developing countries, to provide accessible, affordable, and available primary health care to people. OR "Primary health centers some times referred to as public health centers.
What are examples of primary health care?
Primary health care services may also target specific conditions and health care needs, like sexual health, drug and alcohol treatment, oral health, cardiovascular disease, asthma, diabetes, mental health, and obesity.
What is the role of primary health Centre?
Primary Health Centres (PHCs) comprise the second tier in rural healthcare structure envisaged to provide integrated curative and preventive healthcare to the rural population with emphasis on preventive and promotive aspects.
What are the 7 principles of primary health care?
The principles of primary health care are accessibility, public participation, health promo- tion, appropriate technology and intersectoral cooperation. Accessibility means that the five types of health care are universally available to all clients regardless of geo- graphic location.
You might be interested: Often asked: Pocket Mortys How To Return To Health Center?
What are the 8 elements of primary health care?
8 Components of Primary Health Care
Public Education.
Proper Nutrition.
Clean Water & Sanitation.
Maternal & Child Health Care.
Immunization.
Local Disease Control.
Accessible Treatment.
Drug Provision.
What is the difference between primary health care and primary care?
Primary Health Care is a broader term which derives from core principles articulated by the World Health Organization and which describes an approach to health policy and service provision that includes both services delivered to individuals (Primary Care services) and population-level "public health-type" functions.
What are the 10 components of primary healthcare?
Point out elements of primary health care as drafted by Alma Ata conference.
Provision of balance diet and maintain cleanliness and sanitation.
Prevention and control of local endemic diseases.
Immunization against major infectious diseases.
Maternal and child health care.
Provision of essential drugs supply.
How is primary health care delivered?
Primary health care services are delivered in settings such as general practices, community health centres, allied health practices, and via communication technologies such as telehealth and video consultations. almost 1 in 5 (18%) saw 3 or more health professionals for the same health condition [2].
Why is primary care so important?
A primary care physician is essential to help an individual navigate to good health and stay healthy; preventing disease by identifying risk factors; coordinating and managing chronic disease care for longevity and a better quality of life.
What are the disadvantages of primary health care?
Challenges in Primary Care
Lack of Choice. Each general practitioner has a particular way of working with patients and promoting their health, which is more compatible with some patients than others.
Variable Quality.
Reactive vs.
Physician Shortage.
Addressing the Challenges.
Further Reading.
You might be interested: Readers ask: When Was Unt Health Science Center Established?
What are the four pillars of primary health care?
The four major pillars of primary health care are as follows:
Community Participation.
Inter-sectoral Coordination.
Appropriate Technology.
Support Mechanism Made Available.
Who is the father of PHC?
Grant was the father of primary health care. John Grant was a very distinguished physician who worked with the Rockerfeller Foundation in a number of countries, but his most important contribution was his work in China back in the 1930s.
What are the basic principles of primary health care?
EFFECTIVE HEALTH CARE EQUALS PRIMARY HEALTH CARE (PHC) The five principles of primary health care are: – Accessibility; – Public participation; – Health promotion; – Appropriate skills and technology; and – Intersectoral cooperation.


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Abstract: 8-K filed by Allegiance Bancshares Inc. (ABTX) covering Results of Operations and Financial Condition and Financial Statements and Exhibits.
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8-K 8-K 10/1/2019 9/27/2019
Abstract: 8-K filed by Allegiance Bancshares Inc. (ABTX) covering Entry into a Material Definitive Agreement; Creation of a Direct Financial Obligation or an Obligation under an Off-Balance Sheet Arrangement of a Registrant; and Financial Statements and Exhibits.
Abstract: Registrant reported that on Sept. 20, it entered into an underwriting agreement for the sale of $60 million of its 4.70% fixed- to floating-rate subordinated notes due Oct. 1, 2029. The underwriting agreement was included by exhibit.
Prospectus 424B5 9/23/2019
Abstract: Registrant reported that it made available the fixed income investor presentation. The presentation was included by the exhibit.
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Abstract: Registrant reported that effective Sept. 11, Roland Williams resigned from his position as a member of the board of directors of Allegiance Bank and will no longer serve as executive vice chairman of the bank.
Abstract: On July 26, registrant announced that its board of directors authorized a stock repurchase program on July 25 to repurchase up to 1 million shares of its outstanding common stock at the discretion of management through July 31, 2020.
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Abstract: Registrant filed a registration statement for up to 1.3 million shares of common stock in an offering valued at approximately $45.3 million offered through its 2019 amended and restated stock awards and incentive plan.
Abstract: 8-K filed by Allegiance Bancshares Inc. (ABTX) covering Departure of Directors or Principal Officers; Election of Directors; Appointment of Principal Officers; Submission of Matters to a Vote of Security Holder; and Financial Statements and Exhibits.
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Abstract: Registrant filed a registration statement for up to 100,000 shares of common stock in an offering valued at approximately $3.5 million offered through its 2019 amended and restated employee stock purchase plan.
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Provocative David Cerny 'Flips Off' Czech Communists
World | October 22, 2013, Tuesday // 12:08
Czech artist David Cerny has floated a giant purple middle finger statue down Prague's Vltava River, pointing at Prague Castle, the seat of President Milos Zeman. Photo EPA/BGNES
David Cerny, "l'enfant terrible" of Czech art, has created and mounted yet another bold street installation in the very heart of Prague.
The famous and controversial artist, known for his strong anti-communist stance, floated a huge purple statue of an extended middle finger down the River Vltava.
The installation comes in the eve of Friday's general elections in the country, where polls forecast that the Communists might enter its rule "through the back door" for the first time ever since the fall of the Berlin Wall in 1989.
The giant purple hand has been mounted on a barge floating on the river and is pointed at Prague Castle, the seat of President Milos Zeman.
Zeman supports a post-election plan to have the left-wing Social Democrats form a minority government, which is said to enjoy the tacit support of the Czech communists. If this happens, the communists, albeit indirectly, will find themselves back in power for the first time since the Velvet Revolution.
Cerny is known for always defying authority and officials through his art and views. His latest piece is seen as a clear message to the leftist President and the political party recently set up by his supporters.
It is unknown if the finger is to stay floating on Vlatava or be removed. Zeman was on an official trip to the Ukraine Monday, when the installation was mounted.
The Czech parliament was dissolved in August following weeks of turmoil in Czech politics.
Prime Minister Petr Necas's government collapsed in June amid a bribery scandal, and a government of technocrats, formed by President Zeman in July and opposed by the main political parties, resigned in August.
David Cerny often makes headlines in Bulgaria as well.
In January 2009, his satire of European stereotypes in an eight-ton mosaic of the bloc's then-27 nations, called "Entropa," caused quite of a scandal, particularly in Bulgaria.
The piece, which was installed at the European Council building in Brussels, was supposed to proudly display unique traits of each country in the union. Instead, it depicted Bulgaria as a Turkish squat toilet, Catholic Poland as a group of priests raising a gay flag and Germany as a network of motorways eerily resembling a swastika.
Only Bulgaria, however, censored the installation, as it protested against the way it has been presented, which resulted in the toilet being draped in a black veil, making it even more visible.
As recently as August 21, the controversial monument of the Soviet Army in the downtown of the Bulgarian capital Sofia was colored in honor of the Prague Spring.
The unnamed street artists sprayed the monument with pink color in an artistic apology to the Czech for the Warsaw Pact invasion and in a tribute to Cerny, who in 1991 painted pink a Soviet tank in Prague, mounting an erected middle finger on top.
An exclusive interview for Novinite.com read HERE.
Tags: tank, Pink, Soviet Army Monument, sofia, squat toilet, Entropa, Petr Necas, communist, leftist, general elections, Milos Zeman, president, Vltava River, Prague, statue, middle finger, purple, David Cerny, artist, Czech, Prague Spring
» Restaurants in Sofia Boycotted the New Measures last night
» Sofia Airport Recorded a Decline of 3.8 Million Passengers compared to Pre-COVID levels
» COVID Restrictions on Restaurants in Sofia in Force from Today - They will be Boycotted
» Sofia: How Warm is it in Electric Buses during Winter
» Bulgarian President to PM of North Macedonia: Let's Make Progress on Important Topics


At present many countries in the region have carried out their digital strategy including Việt Nam. But China and Singapore are the two leading nations.
In our country, an e-Government system was launched several years ago, but the national system still needs further improvements.
More recently, Prime Minister Nguyễn Xuân Phúc signed a decree on advancing the campaign to bring Industry 4.0 to life. But I'm sorry to say there remain many things to be done. When we talk about the digital economy, for many Vietnamese, that economy seems alien. But in real life, the internet of things has penetrated all corners of our socio-economic life.
The foundation for digital transformation is the data, but I have to admit our current data system is still weak. Electronic data of Government agencies at present simply focus on the State management performance of each agency, not on sharing information. This leads to waste of finances and human resources.
It is time for us to improve the operational quality of all public agencies. To achieve this goal, we need to change our current thinking and adopt a suitable management method. That means we need to improve the efficiency and effectiveness of online public services for people and enterprises. Last but not least, the application of technology must go hand in hand with administrative reform and the development of online public services.
In my opinion, the most important thing in the course of digitalisation is the effectiveness of information sharing.
To my knowledge, a digital economy is closely associated with informatics, automation and cloud computing, the internet and others. In the field of agriculture, digitalisation is used in remote control or automation. That's why when we want to apply digitalisation in our agriculture industry we should start from need assessments.
But, in my opinion, it is too early for us to talk about the application of digitalisation in agriculture with a very simple reason: we have not completed the mechanisation revolution while we have abundant labourers in the field of agriculture.
It is indisputable that we need a very good foundation for information technology in an advanced agriculture coupled by the farmers' strong knowledge and skills. But, I'm sorry to say that at present we're facing a lot of difficulties in our basic infrastructure.
So, in my opinion, the most challenging area that Việt Nam faces is digitalisation in our primary industry – agriculture. No doubt, when Industry 4.0 is applied to agriculture, it means manual work will be replaced by machines.
As a result many people will be out of work. This is a big challenge for Việt Nam. And Việt Nam has to change its growth model. Agriculture must be then closely associated with industry, as is the countryside and towns and cities. What's more important is the change of the cluster growth model toward the goal of harmonisation and opportunities for everyone.


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UPLB Perspective
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COVID-19 Watch News
Youth groups slam gov't on handling pandemic, forward agenda that amplifies public's demands
by Alvin James Magno
Several youth groups criticize the actions made by the Duterte administration on the implemented policies regarding the Luzon lockdown and the misappropriation of the P 27.1 B emergency fund fighting the pandemic, thus creating two sets of agenda that will address the current problems faced by the country.
According to the College Editors Guild of the Philippines (CEGP) President Daryl Angelo Baybayado, the guild acknowledges the allocation of the budget for the affected sectors; however, the fund given to the health care sector is not enough on solving the soaring number of COVID-19 patients.
"If the government is sincere in serving the needs of the Filipino people, Duterte must prioritize the funding for the health sector and coronavirus test kits to immediately combat the disease," he said.
To give a brief background, the Duterte Administration's economic team rolls out the P 27.1 billion budget on Monday to target the severities inflicted by the pandemic in the country. Instead of it being commended, it was lambasted by the public because half of it or P14 billion was given to the tourism sector. Meanwhile, the health sector was allocated with only P3.1 billion to purchase test kits.
Moreover, the guild's president added that despite of the administration's allotment of budget for workers, especially the farmers who are distressed by the rice liberalization law, it will not properly support their family's day-to-day needs. Baybayado also stated that as millions of them are affected, the P2 billion financial assistance for displaced workers, P1.2 social security benefits, and P2.8 billion loan for farmers will not be sufficient.
Meanwhile, the National Union of Students of the Philippines (NUSP) condemns the actions made by the government to the repressive policies set down to the public.
"The incompetence of national public officials in responding to health crises also worsens the situation. Instead of focusing their attention and resources to solve the socio-economic reasons that underpin the crisis, they are instead prioritizing draconian measures of imposing restrictive lockdown measures," NUSP said.
The call for public health demands
With the problems at hand, CEGP, alongside other youth groups and mass organizations, made a 7-point public health demands to address the rising number of individuals contracted COVID-19.
"The 7-point public health demands are urgent and imperative measures from the worsening disease given the Duterte regime's blatant negligence. The lack of support and how unprepared our public officials in our country reveals something deeply rotten about our healthcare system," CEGP's Baybayado said.
The said public health demands mostly compromise health measures and the prioritization of the welfare of the Filipinos. The demands are to pass immediate medical solutions instead of military actions; support local scientists and frontline health workers and professionals; ensure the assistance to the affected workers; rechannel the allocated budget of the Office of the President, National Task Force, and Oplan Tokhang to basic social services; stop the increase in prices amid the crisis; ensure the regulation of food, medicine, and other basic products; and, ensure the protection of human rights and civil liberties of all sectors.
Furthermore, the said guild called out the current administration to prioritize the interest of millions of Filipinos affected by the crisis.
"In these trying times, the welfare of the Filipino people should be the utmost priority of the administration… He must listen to his constituents," Baybayado said.
Additionally, CEGP tasked all student publications to stand with its pro-people agenda and report the current conditions happening not only in the country, but also in the community.
The students' demands
On the other hand, NUSP, in partnership with Kabataan Partylist (KPL), crafted a 5-point student demands to amplify the concerns of the students and the calls of its student councils to free and accessible education for all during the crisis.
"The struggle for the 5-point Student Demands — made possible through the efforts of student leaders all over the country — continues the historic role of student councils in achieving a free and inclusive society for the youth," NUSP Deputy Secretary General Joshua Marcial said.
The said demands of the union are inclusive educational alternative, which calls for the suspension of online classes and to resume classes if the government successfully mitigated the spreading of virus; refund unused fees and stop impending tuition and other school fees increase; sustain teaching and non-teaching staff salaries; stop rail-roading anti-student repressive policies; and, preserve student representation through genuine student councils.
The organization also commends and continues the support of the work of medical front liners, further demanding the government to stop the militarization of communities, and transfer billions of confidential funds for mass testing, disinfection, and other medical-related solutions to combat the pandemic.
"The solution should not just favor the convenience of the few but should serve also the marginalized individuals," NUSP stated. [P]
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About Alvin James Magno
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RSVP for Geelong Monthly Breakfast Sun 27 May - new riders welcome to add comments!
It's all about being central for the members, the display of our beautiful vespas, and being seen therefor promoting the club.
The Esplanade as the location ticks the boxes and perhaps a conversation with The Edge is due again.
Let's see what responses you get.
Tufan, after the discussion had at the last breakfast about returning to The Edge, just wanting to know if this breakfast is going to be changed back to The Edge or are you still having it at Pako Raw?


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Important News About Houston Dressage Society Members
Mary "Molly" Wallin
Molly Wallin and Brambletyne Valor
Molly Wallin, 80, of Tomball, Texas, entered into Heaven August 4, 2001. Although originally from the horse-crazy state of Virginia, Molly's love for horses was first allowed to blossom when the uncle of her husband, Burt, first introduced her to his mixed herd in Texas well over 50 years ago. His horses were Arabian, Quarter Horses and Thoroughbreds. Molly immediately immersed herself in the horses while still caring for her family and other duties.
From an accomplished Arabian competitor and judge to a successful FEI dressage competitor, Molly inspired many with her exacting requirements for quality, remarkable dignity and ability to maintain a healthy balance between her marriage and her infatuation with horses. Molly was unstinting in her praise AND her critiques. Whether one was an amateur or professional made no difference in her standards --although she was known to say that professionals should adhere to the strictest standards in all their actions. In all her endeavors Molly emphasized the functional usefulness, the beauty and the talent of the horse. The well being of her horses was always more important than competition. Throughout her life, Molly received many equine related awards and recognitions, the latest being USDF Region 9 Horseperson of the Year 2000. Molly's last partner, Brambletyne Valor +\, will continue sharing Molly's spirit as he "teaches" future FEI riders.
Molly spent her years while on this earth sharing her love, compassion and forgiveness with her family, many, many friends, Christian brothers and sisters, as well as, with acquaintances. When repeatedly faced with personal adversity, Molly continued to do the next right thing, taking every day on a day-by-day basis, never losing her care for those others around her. Molly's fight with cancer never dimmed her vivacity nor lessened her interest in people. As a horsewoman passionate about horses and dressage and passionate about furthering the art for her own benefit, as well as, that of her friend Valor, while still being passionate in helping "people" friends, Molly Wallin exemplified what we should all try to emulate.
She is survived by her husband Burton, 4 children, Burton, Jr., Susan Inman, Kent and Kirk, 13 grandchildren and 5 great grandchildren. Memorial gifts may be sent to the Walk to Emmaus Ministry, (Luke 23:13-32) P.O. Box 73167, Houston, Texas 77090.
There are special people who touch our lives in a certain way and having known them we will never be the same.
Sadly submitted by Tevia McLaren
Photos by Olva Stewart Pharo taken at the last HDS Show at Bear Creek
This site is managed by Calaveras County Equestrian Management & Promotional Services,
publisher of the Texas Horseman's Directory.
For comments or information email: directory@texhorseman.com
Last update: 8 October, 2005


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Life at Alcidion
We are Optimistic – Alcidion's values in action
July 5, 2021 | Culture
This is the third article in a series of blog posts that explores Alcidion's core values in action and how they influence our work, products and culture. In this blog, UK Managing Director Lynette Ousby takes a look at how we live the value "We are optimistic".
At Alcidion we believe that technology can truly assist in contributing to safer, more effective outcomes in healthcare. Adopting innovative technology can be a daunting prospect however the benefits that can be achieved by implementing Alcidion's smart solutions can improve not just the burden on clinicians but also enact a workflow that provides safer care for patients.
The adoption of Alcidion's products in the UK has been an exciting trajectory and I'm pleased to share our successes following the launch of Miya Precision and how we embrace the 'we are optimistic' value in everything that we do.
Miya Precision entered the UK market in July 2020 providing the NHS with a clinical decision support tool to quickly adopt new and emerging smart technologies as well as address NHS strategic priorities. Alcidion were optimistic that we could offer a solution that would remove system roadblocks for the NHS and significantly improve patient safety and care delivery.
Alcidion are proud that we have now partnered with 27 National Health Service (NHS Trusts) to implement digital solutions across the UK and that our customers are achieving results that are positively impacting the way that they deliver care. Smartpage, Miya Observations and Miya Assessments (Patientrack) have enjoyed significant success in the United Kingdom. The ability of Smartpage to integrate with existing IT systems across the trusts has provided Alcidion a gateway in reaching new customers and inviting them to realise the benefits of Alcidion's product offering and hero product – Miya Precision.
We are developing partnerships
In 2019, Dartford and Gravesham NHS Trust announced a five year contract to implement Alcidion's Miya Precision platform, Smartpage and Patientrack solutions. This agreement also included implementation of and Better Meds Electronic Prescribing and Medications Administration (ePMA), Alcidion's first deployment of that product. This contract has been a significant one for us to be able to manage the implementation of digital solutions from start to finish and use the successes Dartford and Gravesham NHS Trust achieve as a benchmark in the industry, providing other NHS Trusts with insights into why adopting Alcidion's innovative solutions can assist in executing the NHS Long Term Plan and improve patient care now and into the future.
Alcidion is implementing Miya Precision, Patientrack and the Better Meds system at South Tees Hospitals NHS Foundation Trust (South Tees). We extended our partnership with them to include Smartpage, cloud hosting and change management tools in November 2020. The extension of the South Tees contract was a significant milestone for Alcidion in the UK market and we look forward to watching these tools increase their productivity and patient care techniques.
We were delighted to recently announce a five year deal with East Lancashire Hospitals NHS Trust (East Lancashire Trust) to implement Patientrack (now Miya Observations and Miya Assessments) and Smartpage in March 2021. This capability accompanied by Smartpage will be an important part of East Lancashire Hospitals Trust's digital roadmap and the deployment reaching thousands of NHS professionals across five hospitals in East Lancashire will benefit clinicians to use these smart solutions to monitor and respond to patients in need of urgent attention.
The success of Smartpage has been its ability to work with existing systems and this continues to be recognised with our recent agreement to deploy the solution to meet the needs of busy healthcare staff at Five NHS trusts and the Isle of Man's Department of Health and Social Care. Not to mention aligning with health and social care secretary Matt Hancock's campaign for the NHS to phase out pagers by the end of 2021.
We are optimistic that the implementations of these solutions and the positivity within the UK healthcare market shows that Alcidion can deliver on the promises we make, instilling a partnership with customers that believe technology solutions can deliver safer and time saving results.
We are growing
To be able to achieve these wins, you need a great team! Since January we have welcomed Clinical Consultant Katy Cain, Programme Manager Harvey Hanson, Managed Services Consultant Jamie Longmore, Clinical Product Specialist Kate Gaunt, Service Desk Manager Kal Johal and Project Manager Louise Clowes to the team with Kerry Kelly joining us in June as Business Operations Assistant, bringing the UK Team to 35.
A senior nurse with more than 20 years' experience, Katy joins the team from East Lancashire Hospitals NHS Trust and will be instrumental in helping us to listen to the needs of NHS professionals.
Harvey brings with him 15 years of healthcare experience working on a variety of business change and transformational programmes of work including the National Programme for IT, Gibraltar EPR Programme and Doncaster and Bassetlaw PAS and ED replacement.
With 15 years of experience in IT, having previously spent 5 years working for the NHS as an infrastructure support / projects engineer, Jamie will contribute to our global support team with particular focus on local technical support for our Miya Precision, ePMA and Smartpage products.
Kate Gaunt is an experienced healthcare professional with a background in theatres, emergency care and resuscitation. As a super user, Kate will be working closely with our customers to deploy Miya Precision to a clinical setting.
Project Manager Louise Clowes brings over 10 years of valuable experience to Alcidion, having delivered complex Healthcare IT solutions to a number of UK Trusts focused on PAS, EPR, ED and integration.
Kal has a wealth of customer service leadership experience in Healthcare IT, with a proven track record in creating something new or improving processes to maintain high standards of support to clinical applications.
With over 20 years of experience working in finance, Kerry Kelly will assist the Burnley office in financial administration, office management and supporting sales and marketing functions.
Recently Alcidion welcomed ExtraMed, a UK patient flow software company to the Group. For 20 years, ExtraMed have been providing patient flow software and command centre communications to a number of NHS Trusts. We are excited to have the ExtraMed team of 11 staff on board and look forward to combining the teams and services to continue to provide innovative and exciting services to ExtraMed and Alcidion customers.
The growth and investment in the UK team has allowed us to open a new office in Burnley. Having been raised in Padiham, it is exciting to join the North West community and develop career opportunities at Alcidion within these regions. Please visit our career page for upcoming positions!
It is a busy time for Alcidion but we believe that implementing innovative technology can impact healthcare delivery in revolutionary ways, saving clinician's time by providing them with actionable insights to improve patient outcomes. We are optimistic in continuing to develop our relationships and expanding Alcidion's footprint across the United Kingdom.
Lynette Ousby is the UK Managing Director at Alcidion
Get to know our team – Chief Financial Officer Matthew Gepp
Evidenced Based Project Management


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Postrzelone bliźniaki (ang. Meet the Deedles) - amerykańska komedia filmowa z 1998 roku. W tytułowych rolach występują Paul Walker (Szybcy i wściekli) oraz Steve Van Wormer (Strażnik czasu 2: Decyzja).

Fabuła
Film opowiada o dwóch braciach, Philu i Stevie Deedlesach, których ojciec wysyła na nudny obóz survivalowy. Niesforni bracia nie zamierzają poddać się instytucji i przewracają kemping do góry nogami.

Amerykańskie filmy z 1998 roku
Amerykańskie filmy komediowe
Filmy w reżyserii Steve'a Boyuma
Filmy Disneya

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RDN: Tell us about Oceanpower and Oceanpower America. What do you do?
WH: Although 'Oceanpower' may sound new to some distributors, dealers and operators in North America, it started to export ice cream equipment to US under various trade names as early as 2007. The company itself started to manufacture ice cream equipment in 1996 and now exports ice cream machines and powder mixes to almost every corner of the world. To better serve our customers in North America, we recently established Oceanpower America and we will keep our audience updated with our progress.
RDN: How does Oceanpower standout against other competitors?
WH: Oceanpowerhas been able to distinguish itself from other competitors by continuing to innovate in the food service industry, not only in terms of products, but also the business as a whole. When the company started to make ice cream equipment nearly twenty years ago, the first line of products were very simple, of small capacity. As business grew, we started to improve our products and export them to other areas such as Middle East, Europe, Africa and North America. During the course of global expansion, we had to adopt a 'complex global' strategy to cope with specific needs and restraintsfrom customers in each different geographic territory. For example, in many emerging markets, voltage instability could severely impact machine's performance; therefore, our engineering team had to make the system more robust and stable. Simply put, our customers' continued request for better products prompted us to revolutionize our product lines. In addition, due to customers' strong interest in quality, affordable ice cream powder and cone products, we imported three state-of-the-art assembly lines from Austria and invested millions of dollars in a food processing facility, FDA and HACCP approved.
RDH: What products are you presenting to the audience at the show this year, any new products?
WH: We brought almost our entire product line to the show this year to demonstrate our hard work for the past several years. Nearly all products are new. Our product portfolio encompasses mini ice cream machine models Sunny A6 and A 12, classic counter top and floor standing ones, the flag-ship 165 series, and the classic OPH42 batch freezer. Each product line targets a specific customer segment. Priced very competitively, mini machines are ideal for mom-and-pop shops and catering venues, etc. while the 165 series would be indispensable for locations with heavy foot traffic demanding absolute continuous dispensing performance. In addition, to boost overrun and profitability, customers also have the option to include air pump as an option when ordering.
WH: As part of our global strategy, we hope to build a strong and resilient supply chain in North America within the next few years. Oceanpower in on its to become a real American company.
Oceanpower's new flagship DW series soft serve freezers recently made their debut in North America, symbolizing the company's new push for its strategic global expansion. The new models will rank the company among the top-tier foreign ice cream equipment manufacturers in the US market.
Running on either single-phase or three-phase power, the new DW series features dramatic upgrades from Oceanpower's existing line of soft serve machines. The series runs on an industry-leading patented Triple-Control system in that the machine is able to switch between Current, Temperature, and Timing modes in case one or two modes fail, ensuring maximum reliability and protection against potentially destructive events such as cylinder-freezing. The series is also equipped with either two or three-horsepower American-brand Tecumseh compressors well known for their quality consistency, superior refrigeration capacity and wide range of operating voltage. The super continuous dispensing capability now positions the models among the top candidates for business with heaviest foot traffic. The first-dispensing time is now reduced to between eight and ten minutes once the compressor starts. In addition, sparing an extra compressor, the model now operates on one powerful American-brand Tecusmeh compressor for both ice cream making and hopper refrigeration, cooling the hopper at a much faster speed for maximum mix freshness. The one compressor system also simplifies the machine design for easier service and higher level of reliability. The ice cream making process is also aided by the 1.5 horsepower Regal-Beloit joint venture-made AC beater-motor, which suits a wide range of viscotiy for all types of soft serve mixes. On top of all these features, the models offer other value-added features such as Oceanpower's new generation air pump that is able to raise overrun to 50% to 60% (which is virtually indispensible for businesses serving customers with such taste preference), the durable motor-propelled magnetic hopper agitators, infra-red remote control, and acrylic soft touch pads for smooth touch control, and a new automatic-return dispenser door for better handling and insulation.
The biggest plus for the series is that pasteurization is available on the three-phase model. The patented pasteurization mechanism is able to raise the mix in the cylinders and hoppers to 167 Fahrenheit within 20 minutes of heating and maintain the temperature for 15 seconds, killing 95% of germs, before the ice cream making progress begins. Operators are free to run the feature at intervals at their choice, such as at business open and close. This optional feature greatly enhances food safety for operators and consumers. Together with the standby function, pasteurization relieves the operators from the burden of disassembling the dispenser and washing the machine every night.
Big box, powerful soft serve freezers are pretty much the norm for the North American ice cream equipment market. These high-capacity machines have not let the operators down. Yet the smallest-sized market segments have typically been neglected by the manufacturers. Traditional America mom-and-pop shops and country side convenience stores have their soft serve needs as well, probably not for the big box type. Not until recently did major manufacturers start to pay attention to this specifc market segment and make small-capacity models for the operators.
Oceanpower's new Sunny series mini soft serve freezers immediately caught attention from dealers and operations once they became available in the market last year. Deployed in many small coffee shops, the new series has already met initial success in the European market. These are machines are making their debut in the 2015 NRA Show. What immediately catches the audience eye balls is the chic, patented design. The size of a regular desk-top computer, the body of the series comes with a variety of features, shapes and designs such as color-coded distribution handle, rainbow strip body pattern, removable hopper for easier overnight storage in refrigerator, built-in logo banner, and even a clip-on blue-tooth music player. These add-on features will greatly enhance the appeal of the machine and the ambient environment, making the serving atmosphere much cozier and friendlier.
In essence, the series comes with two hopper sizes, two quarts and 13 quarts, matching operators' different foot traffic needs. Clad in the exquisiteness are the core offerings, the 0.6 horsepower Spain-made Cubigel compressor and a one-third horsepower Japanese brand two-in-one beater motor and gear box. Despite its mini size, the machine is able to turn out ten quarts of production, or roughly 100 to 120 cones per hour. This series is expected to hit with great success in North America.
In the meantime, Oceanpower is introducing its batch freezers and pasteurizers for gelato lovers on this continent. The flexible batch freezer series feature the following capabilities, concurrent or consecutive pasteurizing and gelato making, proprietary beater design for smoother gelato texture and higher overrun, multiple discharge temperature selection, dual-speed gelato making and dispensing for different preferences, accurate sensing for precise discharge temperature, and both air and water cooling options. Plus, the built-in frequency inverter allows the machine to run at much lower noise level.


KODAK enter the U.K. Smart Home market, via a new licensing deal with Liz Invest. Their first product is the Kodak Smart Security System.
The range comprises of two indoor and outdoor motorised cameras as well as sensors. Both cameras deliver 1080p HD video with the indoor also featuring two way audio. All recordings can either be saved on an internal SD or on Google Cloud, all without a subscription.
The system allows customers to create their own secure home network. The network can be controlled and viewed via a free app – KODAK Security mobile app. The app is available on iOS and Android.
Unlike other home camera systems the cameras can connect to sensors. Once triggered the camera rotates to point to the sensor.
The cameras either come as standalone units or as starter kits. The standard kit includes one door sensor and a remote control. The premium starter kit includes two sensors, one motion sensor and a remote.
The indoor camera has a RRP of £129, the outdoor camera £169.99. The Starter kit has a RRP £149.99 or £199.99 for the premium kit.


text:
Metals (particularly those in groups 1 and 2) tend to lose the number of electrons that would leave them with the same number of electrons as in the preceding noble gas in the periodic table. By this means, a positively charged ion is formed. Similarly, nonmetals (especially those in groups 16 and 17, and, to a lesser extent, those in Group 15) can gain the number of electrons needed to provide atoms with the same number of electrons as in the next noble gas in the periodic table. Thus, nonmetals tend to form negative ions. Positively charged ions are called cations, and negatively charged ions are called anions. Ions can be either monatomic (containing only one atom) or polyatomic (containing more than one atom). Compounds that contain ions are called ionic compounds. Ionic compounds generally form from metals and nonmetals. Compounds that do not contain ions, but instead consist of atoms bonded tightly together in molecules (uncharged groups of atoms that behave as a single unit), are called covalent compounds. Covalent compounds usually form from two nonmetals. Atoms gain or lose electrons to form ions with particularly stable electron configurations. The charges of cations formed by the representative metals may be determined readily because, with few exceptions, the electronic structures of these ions have either a noble gas configuration or a completely filled electron shell. The charges of anions formed by the nonmetals may also be readily determined because these ions form when nonmetal atoms gain enough electrons to fill their valence shells. Covalent bonds form when electrons are shared between atoms and are attracted by the nuclei of both atoms. In pure covalent bonds, the electrons are shared equally. In polar covalent bonds, the electrons are shared unequally, as one atom exerts a stronger force of attraction on the electrons than the other. The ability of an atom to attract a pair of electrons in a chemical bond is called its electronegativity. The difference in electronegativity between two atoms determines how polar a bond will be. In a diatomic molecule with two identical atoms, there is no difference in electronegativity, so the bond is nonpolar or pure covalent. When the electronegativity difference is very large, as is the case between metals and nonmetals, the bonding is characterized as ionic.
Keywords: Atom, Bonding, Electron Configurations, Periodic Table
13.1 Ionic and Molecular Compounds
Define ionic and molecular (covalent) compounds
Predict the type of compound formed from elements based on their location within the periodic table
Determine formulas for simple ionic compounds
In ordinary chemical reactions, the nucleus of each atom (and thus the identity of the element) remains unchanged. Electrons, however, can be added to atoms by transfer from other atoms, lost by transfer to other atoms, or shared with other atoms. The transfer and sharing of electrons among atoms govern the chemistry of the elements. During the formation of some compounds, atoms gain or lose electrons, and form electrically charged particles called ions (Figure 13.1).
(a) A sodium atom (Na) has equal numbers of protons and electrons (11) and is uncharged. (b) A sodium cation (Na+) has lost an electron, so it has one more proton (11) than electrons (10), giving it an overall positive charge, signified by a superscripted plus sign.
You can use the periodic table to predict whether an atom will form an anion or a cation, and you can often predict the charge of the resulting ion. Atoms of many main-group metals lose enough electrons to leave them with the same number of electrons as an atom of the preceding noble gas. To illustrate, an atom of an alkali metal (group 1) loses one electron and forms a cation with a 1+ charge; an alkaline earth metal (group 2) loses two electrons and forms a cation with a 2+ charge, and so on. For example, a neutral calcium atom, with 20 protons and 20 electrons, readily loses two electrons. This results in a cation with 20 protons, 18 electrons, and a 2+ charge. It has the same number of electrons as atoms of the preceding noble gas, argon, and is symbolized Ca2+. The name of a metal ion is the same as the name of the metal atom from which it forms, so Ca2+ is called a calcium ion.
When atoms of nonmetal elements form ions, they generally gain enough electrons to give them the same number of electrons as an atom of the next noble gas in the periodic table. Atoms of group 17 gain one electron and form anions with a 1− charge; atoms of group 16 gain two electrons and form ions with a 2− charge, and so on. For example, the neutral bromine atom, with 35 protons and 35 electrons, can gain one electron to provide it with 36 electrons. This results in an anion with 35 protons, 36 electrons, and a 1− charge. It has the same number of electrons as atoms of the next noble gas, krypton, and is symbolized Br−. (A discussion of the theory supporting the favored status of noble gas electron numbers reflected in these predictive rules for ion formation is provided in a later chapter of this text.)
Note the usefulness of the periodic table in predicting likely ion formation and charge (Figure 13.2). Moving from the far left to the right on the periodic table, main-group elements tend to form cations with a charge equal to the group number. That is, group 1 elements form 1+ ions; group 2 elements form 2+ ions, and so on. Moving from the far right to the left on the periodic table, elements often form anions with a negative charge equal to the number of groups moved left from the noble gases. For example, group 17 elements (one group left of the noble gases) form 1− ions; group 16 elements (two groups left) form 2− ions, and so on. This trend can be used as a guide in many cases, but its predictive value decreases when moving toward the center of the periodic table. In fact, transition metals and some other metals often exhibit variable charges that are not predictable by their location in the table. For example, copper can form ions with a 1+ or 2+ charge, and iron can form ions with a 2+ or 3+ charge.
Some elements exhibit a regular pattern of ionic charge when they form ions.
Composition of Ions
An ion found in some compounds used as antiperspirants contains 13 protons and 10 electrons. What is its symbol?
Because the number of protons remains unchanged when an atom forms an ion, the atomic number of the element must be 13. Knowing this lets us use the periodic table to identify the element as Al (aluminum). The Al atom has lost three electrons and thus has three more positive charges (13) than it has electrons (10). This is the aluminum cation, Al3+.
Give the symbol and name for the ion with 34 protons and 36 electrons.
Se2−, the selenide ion
Formation of Ions
Magnesium and nitrogen react to form an ionic compound. Predict which forms an anion, which forms a cation, and the charges of each ion. Write the symbol for each ion and name them.
Magnesium's position in the periodic table (group 2) tells us that it is a metal. Metals form positive ions (cations). A magnesium atom must lose two electrons to have the same number electrons as an atom of the previous noble gas, neon. Thus, a magnesium atom will form a cation with two fewer electrons than protons and a charge of 2+. The symbol for the ion is Mg2+, and it is called a magnesium ion.
Nitrogen's position in the periodic table (group 15) reveals that it is a nonmetal. Nonmetals form negative ions (anions). A nitrogen atom must gain three electrons to have the same number of electrons as an atom of the following noble gas, neon. Thus, a nitrogen atom will form an anion with three more electrons than protons and a charge of 3−. The symbol for the ion is N3−, and it is called a nitride ion.
Aluminum and carbon react to form an ionic compound. Predict which forms an anion, which forms a cation, and the charges of each ion. Write the symbol for each ion and name them.
Al will form a cation with a charge of 3+: Al3+, an aluminum ion. Carbon will form an anion with a charge of 4−: C4−, a carbide ion.
The ions that we have discussed so far are called monatomic ions, that is, they are ions formed from only one atom. We also find many polyatomic ions. These ions, which act as discrete units, are electrically charged molecules (a group of bonded atoms with an overall charge). Some of the more important polyatomic ions are listed in Table 13.1. Oxyanions are polyatomic ions that contain one or more oxygen atoms. At this point in your study of chemistry, you should memorize the names, formulas, and charges of the most common polyatomic ions. Because you will use them repeatedly, they will soon become familiar.
Common Polyatomic Ions
Related Acid
ammonium NH4+NH4+
hydronium H3O+H3O+
peroxide O22-O22-
hydroxide OH-OH-
acetate CH3COO−CH3COO− acetic acid CH3COOH
cyanide CN− hydrocyanic acid HCN
azide N3-N3- hydrazoic acid HN3
carbonate CO32-CO32- carbonic acid H2CO3
bicarbonate HCO3-HCO3-
nitrate NO3−NO3− nitric acid HNO3
nitrite NO2−NO2− nitrous acid HNO2
sulfate SO42−SO42− sulfuric acid H2SO4
hydrogen sulfate HSO4−HSO4−
sulfite SO32−SO32− sulfurous acid H2SO3
hydrogen sulfite HSO3−HSO3−
phosphate PO43−PO43− phosphoric acid H3PO4
hydrogen phosphate HPO42−HPO42−
dihydrogen phosphate H2PO4−H2PO4−
perchlorate ClO4−ClO4− perchloric acid HClO4
chlorate ClO3−ClO3− chloric acid HClO3
chlorite ClO2−ClO2− chlorous acid HClO2
hypochlorite ClO− hypochlorous acid HClO
chromate CrO42−CrO42− chromic acid H2CrO4
dichromate Cr2O72−Cr2O72− dichromic acid H2Cr2O7
permanganate MnO4−MnO4− permanganic acid HMnO4
Note that there is a system for naming some polyatomic ions; -ate and -ite are suffixes designating polyatomic ions containing more or fewer oxygen atoms. Per- (short for "hyper") and hypo- (meaning "under") are prefixes meaning more oxygen atoms than -ate and fewer oxygen atoms than -ite, respectively. For example, perchlorate is ClO4−,ClO4−, chlorate is ClO3−,ClO3−, chlorite is ClO2−ClO2− and hypochlorite is ClO−. Unfortunately, the number of oxygen atoms corresponding to a given suffix or prefix is not consistent; for example, nitrate is NO3−NO3− while sulfate is SO42−.SO42−. This will be covered in more detail later in the module on nomenclature.
The nature of the attractive forces that hold atoms or ions together within a compound is the basis for classifying chemical bonding. When electrons are transferred and ions form, ionic bonds result. Ionic bonds are electrostatic forces of attraction, that is, the attractive forces experienced between objects of opposite electrical charge (in this case, cations and anions). When electrons are "shared" and molecules form, covalent bonds result. Covalent bonds are the attractive forces between the positively charged nuclei of the bonded atoms and one or more pairs of electrons that are located between the atoms. Compounds are classified as ionic or molecular (covalent) on the basis of the bonds present in them.
Ionic Compounds
When an element composed of atoms that readily lose electrons (a metal) reacts with an element composed of atoms that readily gain electrons (a nonmetal), a transfer of electrons usually occurs, producing ions. The compound formed by this transfer is stabilized by the electrostatic attractions (ionic bonds) between the ions of opposite charge present in the compound. For example, when each sodium atom in a sample of sodium metal (group 1) gives up one electron to form a sodium cation, Na+, and each chlorine atom in a sample of chlorine gas (group 17) accepts one electron to form a chloride anion, Cl−, the resulting compound, NaCl, is composed of sodium ions and chloride ions in the ratio of one Na+ ion for each Cl− ion. Similarly, each calcium atom (group 2) can give up two electrons and transfer one to each of two chlorine atoms to form CaCl2, which is composed of Ca2+ and Cl− ions in the ratio of one Ca2+ ion to two Cl− ions.
A compound that contains ions and is held together by ionic bonds is called an ionic compound. The periodic table can help us recognize many of the compounds that are ionic: When a metal is combined with one or more nonmetals, the compound is usually ionic. This guideline works well for predicting ionic compound formation for most of the compounds typically encountered in an introductory chemistry course. However, it is not always true (for example, aluminum chloride, AlCl3, is not ionic).
You can often recognize ionic compounds because of their properties. Ionic compounds are solids that typically melt at high temperatures and boil at even higher temperatures. For example, sodium chloride melts at 801 °C and boils at 1413 °C. (As a comparison, the molecular compound water melts at 0 °C and boils at 100 °C.) In solid form, an ionic compound is not electrically conductive because its ions are unable to flow ("electricity" is the flow of charged particles). When molten, however, it can conduct electricity because its ions are able to move freely through the liquid (Figure 13.3).
Sodium chloride melts at 801 °C and conducts electricity when molten. (credit: modification of work by Mark Blaser and Matt Evans)
To see salts melt and conduct electricity, watch this video that illustrates the conductivity of molten salt.
In every ionic compound, the total number of positive charges of the cations equals the total number of negative charges of the anions. Thus, ionic compounds are electrically neutral overall, even though they contain positive and negative ions. We can use this observation to help us write the formula of an ionic compound. The formula of an ionic compound must have a ratio of ions such that the numbers of positive and negative charges are equal.
Predicting the Formula of an Ionic Compound
The gemstone sapphire (Figure 13.4) is mostly a compound of aluminum and oxygen that contains aluminum cations, Al3+, and oxygen anions, O2−. What is the formula of this compound?
Although pure aluminum oxide is colorless, trace amounts of iron and titanium give blue sapphire its characteristic color. (credit: modification of work by Stanislav Doronenko)
Because the ionic compound must be electrically neutral, it must have the same number of positive and negative charges. Two aluminum ions, each with a charge of 3+, would give us six positive charges, and three oxide ions, each with a charge of 2−, would give us six negative charges. The formula would be Al2O3.
Predict the formula of the ionic compound formed between the sodium cation, Na+, and the sulfide anion, S2−.
Na2S
Many ionic compounds contain polyatomic ions (Table 13.1) as the cation, the anion, or both. As with simple ionic compounds, these compounds must also be electrically neutral, so their formulas can be predicted by treating the polyatomic ions as discrete units. We use parentheses in a formula to indicate a group of atoms that behave as a unit. For example, the formula for calcium phosphate, one of the minerals in our bones, is Ca3(PO4)2. This formula indicates that there are three calcium ions (Ca2+) for every two phosphate (PO43−)(PO43−) groups. The PO43−PO43− groups are discrete units, each consisting of one phosphorus atom and four oxygen atoms, and having an overall charge of 3−. The compound is electrically neutral, and its formula shows a total count of three Ca, two P, and eight O atoms.
Predicting the Formula of a Compound with a Polyatomic Anion
Baking powder contains calcium dihydrogen phosphate, an ionic compound composed of the ions Ca2+ and H2PO4−.H2PO4−. What is the formula of this compound?
The positive and negative charges must balance, and this ionic compound must be electrically neutral. Thus, we must have two negative charges to balance the 2+ charge of the calcium ion. This requires a ratio of one Ca2+ ion to two H2PO4−H2PO4− ions. We designate this by enclosing the formula for the dihydrogen phosphate ion in parentheses and adding a subscript 2. The formula is Ca(H2PO4)2.
Predict the formula of the ionic compound formed between the lithium ion and the peroxide ion, O22−O22− (Hint: Use the periodic table to predict the sign and the charge on the lithium ion.)
Li2O2
Because an ionic compound is not made up of single, discrete molecules, it may not be properly symbolized using a molecular formula. Instead, ionic compounds must be symbolized by a formula indicating the relative numbers of its constituent ions. For compounds containing only monatomic ions (such as NaCl) and for many compounds containing polyatomic ions (such as CaSO4), these formulas are just the empirical formulas introduced earlier. However, the formulas for some ionic compounds containing polyatomic ions are not empirical formulas. For example, the ionic compound sodium oxalate is comprised of Na+ and C2O42−C2O42− ions combined in a 2:1 ratio, and its formula is written as Na2C2O4. The subscripts in this formula are not the smallest-possible whole numbers, as each can be divided by 2 to yield the empirical formula, NaCO2. This is not the accepted formula for sodium oxalate, however, as it does not accurately represent the compound's polyatomic anion, C2O42−.C2O42−.
Molecular Compounds
Many compounds do not contain ions but instead consist solely of discrete, neutral molecules. These molecular compounds (covalent compounds) result when atoms share, rather than transfer (gain or lose), electrons. Covalent bonding is an important and extensive concept in chemistry, and it will be treated in considerable detail in a later chapter of this text. We can often identify molecular compounds on the basis of their physical properties. Under normal conditions, molecular compounds often exist as gases, low-boiling liquids, and low-melting solids, although many important exceptions exist.
Whereas ionic compounds are usually formed when a metal and a nonmetal combine, covalent compounds are usually formed by a combination of nonmetals. Thus, the periodic table can help us recognize many of the compounds that are covalent. While we can use the positions of a compound's elements in the periodic table to predict whether it is ionic or covalent at this point in our study of chemistry, you should be aware that this is a very simplistic approach that does not account for a number of interesting exceptions. Shades of gray exist between ionic and molecular compounds, and you'll learn more about those later.
Predicting the Type of Bonding in Compounds
Predict whether the following compounds are ionic or molecular:
(a) KI, the compound used as a source of iodine in table salt
(b) H2O2, the bleach and disinfectant hydrogen peroxide
(c) CHCl3, the anesthetic chloroform
(d) Li2CO3, a source of lithium in antidepressants
(a) Potassium (group 1) is a metal, and iodine (group 17) is a nonmetal; KI is predicted to be ionic.
(b) Hydrogen (group 1) is a nonmetal, and oxygen (group 16) is a nonmetal; H2O2 is predicted to be molecular.
(c) Carbon (group 14) is a nonmetal, hydrogen (group 1) is a nonmetal, and chlorine (group 17) is a nonmetal; CHCl3 is predicted to be molecular.
(d) Lithium (group 1) is a metal, and carbonate is a polyatomic ion; Li2CO3 is predicted to be ionic.
Using the periodic table, predict whether the following compounds are ionic or covalent:
(a) SO2
(b) CaF2
(c) N2H4
(d) Al2(SO4)3
(a) molecular; (b) ionic; (c) molecular; (d) ionic
13.2 Ionic Bonding
Explain the formation of cations, anions, and ionic compounds
Predict the charge of common metallic and nonmetallic elements, and write their electron configurations
As you have learned, ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell.
Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions. The properties of ionic compounds shed some light on the nature of ionic bonds. Ionic solids exhibit a crystalline structure and tend to be rigid and brittle; they also tend to have high melting and boiling points, which suggests that ionic bonds are very strong. Ionic solids are also poor conductors of electricity for the same reason—the strength of ionic bonds prevents ions from moving freely in the solid state. Most ionic solids, however, dissolve readily in water. Once dissolved or melted, ionic compounds are excellent conductors of electricity and heat because the ions can move about freely.
Neutral atoms and their associated ions have very different physical and chemical properties. Sodium atoms form sodium metal, a soft, silvery-white metal that burns vigorously in air and reacts explosively with water. Chlorine atoms form chlorine gas, Cl2, a yellow-green gas that is extremely corrosive to most metals and very poisonous to animals and plants. The vigorous reaction between the elements sodium and chlorine forms the white, crystalline compound sodium chloride, common table salt, which contains sodium cations and chloride anions (Figure 13.5). The compound composed of these ions exhibits properties entirely different from the properties of the elements sodium and chlorine. Chlorine is poisonous, but sodium chloride is essential to life; sodium atoms react vigorously with water, but sodium chloride simply dissolves in water.
(a) Sodium is a soft metal that must be stored in mineral oil to prevent reaction with air or water. (b) Chlorine is a pale yellow-green gas. (c) When combined, they form white crystals of sodium chloride (table salt). (credit a: modification of work by "Jurii"/Wikimedia Commons)
The Formation of Ionic Compounds
Binary ionic compounds are composed of just two elements: a metal (which forms the cations) and a nonmetal (which forms the anions). For example, NaCl is a binary ionic compound. We can think about the formation of such compounds in terms of the periodic properties of the elements. Many metallic elements have relatively low ionization potentials and lose electrons easily. These elements lie to the left in a period or near the bottom of a group on the periodic table. Nonmetal atoms have relatively high electron affinities and thus readily gain electrons lost by metal atoms, thereby filling their valence shells. Nonmetallic elements are found in the upper-right corner of the periodic table.
As all substances must be electrically neutral, the total number of positive charges on the cations of an ionic compound must equal the total number of negative charges on its anions. The formula of an ionic compound represents the simplest ratio of the numbers of ions necessary to give identical numbers of positive and negative charges. For example, the formula for aluminum oxide, Al2O3, indicates that this ionic compound contains two aluminum cations, Al3+, for every three oxide anions, O2− [thus, (2 ×× +3) + (3 ×× –2) = 0].
It is important to note, however, that the formula for an ionic compound does not represent the physical arrangement of its ions. It is incorrect to refer to a sodium chloride (NaCl) "molecule" because there is not a single ionic bond, per se, between any specific pair of sodium and chloride ions. The attractive forces between ions are isotropic—the same in all directions—meaning that any particular ion is equally attracted to all of the nearby ions of opposite charge. This results in the ions arranging themselves into a tightly bound, three-dimensional lattice structure. Sodium chloride, for example, consists of a regular arrangement of equal numbers of Na+ cations and Cl– anions (Figure 13.6).
The atoms in sodium chloride (common table salt) are arranged to (a) maximize opposite charges interacting. The smaller spheres represent sodium ions, the larger ones represent chloride ions. In the expanded view (b), the geometry can be seen more clearly. Note that each ion is "bonded" to all of the surrounding ions—six in this case.
The strong electrostatic attraction between Na+ and Cl– ions holds them tightly together in solid NaCl. It requires 769 kJ of energy to dissociate one mole of solid NaCl into separate gaseous Na+ and Cl– ions:
NaCl(s)⟶Na+(g)+Cl–(g)ΔH=769kJNaCl(s)⟶Na+(g)+Cl–(g)ΔH=769kJ
Electronic Structures of Cations
When forming a cation, an atom of a main group element tends to lose all of its valence electrons, thus assuming the electronic structure of the noble gas that precedes it in the periodic table. For groups 1 (the alkali metals) and 2 (the alkaline earth metals), the group numbers are equal to the numbers of valence shell electrons and, consequently, to the charges of the cations formed from atoms of these elements when all valence shell electrons are removed. For example, calcium is a group 2 element whose neutral atoms have 20 electrons and a ground state electron configuration of 1s22s22p63s23p64s2. When a Ca atom loses both of its valence electrons, the result is a cation with 18 electrons, a 2+ charge, and an electron configuration of 1s22s22p63s23p6. The Ca2+ ion is therefore isoelectronic with the noble gas Ar.
For groups 13–17, the group numbers exceed the number of valence electrons by 10 (accounting for the possibility of full d subshells in atoms of elements in the fourth and greater periods). Thus, the charge of a cation formed by the loss of all valence electrons is equal to the group number minus 10. For example, aluminum (in group 13) forms 3+ ions (Al3+).
Exceptions to the expected behavior involve elements toward the bottom of the groups. In addition to the expected ions Tl3+, Sn4+, Pb4+, and Bi5+, a partial loss of these atoms' valence shell electrons can also lead to the formation of Tl+, Sn2+, Pb2+, and Bi3+ ions. The formation of these 1+, 2+, and 3+ cations is ascribed to the inert pair effect, which reflects the relatively low energy of the valence s-electron pair for atoms of the heavy elements of groups 13, 14, and 15. Mercury (group 12) also exhibits an unexpected behavior: it forms a diatomic ion, Hg22+Hg22+ (an ion formed from two mercury atoms, with an Hg-Hg bond), in addition to the expected monatomic ion Hg2+ (formed from only one mercury atom).
Transition and inner transition metal elements behave differently than main group elements. Most transition metal cations have 2+ or 3+ charges that result from the loss of their outermost s electron(s) first, sometimes followed by the loss of one or two d electrons from the next-to-outermost shell. For example, iron (1s22s22p63s23p63d64s2) forms the ion Fe2+ (1s22s22p63s23p63d6) by the loss of the 4s electrons and the ion Fe3+ (1s22s22p63s23p63d5) by the loss of the 4s electron and one of the 3d electrons. Although the d orbitals of the transition elements are—according to the Aufbau principle—the last to fill when building up electron configurations, the outermost s electrons are the first to be lost when these atoms ionize. When the inner transition metals form ions, they usually have a 3+ charge, resulting from the loss of their outermost s electrons and a d or f electron.
Determining the Electronic Structures of Cations
There are at least 14 elements categorized as "essential trace elements" for the human body. They are called "essential" because they are required for healthy bodily functions, "trace" because they are required only in small amounts, and "elements" in spite of the fact that they are really ions. Two of these essential trace elements, chromium and zinc, are required as Cr3+ and Zn2+. Write the electron configurations of these cations.
First, write the electron configuration for the neutral atoms:
Zn: [Ar]3d104s2
Cr: [Ar]3d54s1
Next, remove electrons from the highest energy orbital. For the transition metals, electrons are removed from the s orbital first and then from the d orbital. For the p-block elements, electrons are removed from the p orbitals and then from the s orbital. Zinc is a member of group 12, so it should have a charge of 2+, and thus loses only the two electrons in its s orbital. Chromium is a transition element and should lose its s electrons and then its d electrons when forming a cation. Thus, we find the following electron configurations of the ions:
Zn2+: [Ar]3d10
Cr3+: [Ar]3d3
Potassium and magnesium are required in our diet. Write the electron configurations of the ions expected from these elements.
K+: [Ar], Mg2+: [Ne]
Electronic Structures of Anions
Most monatomic anions form when a neutral nonmetal atom gains enough electrons to completely fill its outer s and p orbitals, thereby reaching the electron configuration of the next noble gas. Thus, it is simple to determine the charge on such a negative ion: The charge is equal to the number of electrons that must be gained to fill the s and p orbitals of the parent atom. Oxygen, for example, has the electron configuration 1s22s22p4, whereas the oxygen anion has the electron configuration of the noble gas neon (Ne), 1s22s22p6. The two additional electrons required to fill the valence orbitals give the oxide ion the charge of 2– (O2–).
Determining the Electronic Structure of Anions
Selenium and iodine are two essential trace elements that form anions. Write the electron configurations of the anions.
Se2–: [Ar]3d104s24p6
I–: [Kr]4d105s25p6
Write the electron configurations of a phosphorus atom and its negative ion. Give the charge on the anion.
P: [Ne]3s23p3; P3–: [Ne]3s23p6
13.3 Covalent Bonding
Describe the formation of covalent bonds
Define electronegativity and assess the polarity of covalent bonds
Ionic bonding results from the electrostatic attraction of oppositely charged ions that are typically produced by the transfer of electrons between metallic and nonmetallic atoms. A different type of bonding results from the mutual attraction of atoms for a "shared" pair of electrons. Such bonds are called covalent bonds. Covalent bonds are formed between two atoms when both have similar tendencies to attract electrons to themselves (i.e., when both atoms have identical or fairly similar ionization energies and electron affinities). For example, two hydrogen atoms bond covalently to form an H2 molecule; each hydrogen atom in the H2 molecule has two electrons stabilizing it, giving each atom the same number of valence electrons as the noble gas He.
Compounds that contain covalent bonds exhibit different physical properties than ionic compounds. Because the attraction between molecules, which are electrically neutral, is weaker than that between electrically charged ions, covalent compounds generally have much lower melting and boiling points than ionic compounds. In fact, many covalent compounds are liquids or gases at room temperature, and, in their solid states, they are typically much softer than ionic solids. Furthermore, whereas ionic compounds are good conductors of electricity when dissolved in water, most covalent compounds are insoluble in water; since they are electrically neutral, they are poor conductors of electricity in any state.
Formation of Covalent Bonds
Nonmetal atoms frequently form covalent bonds with other nonmetal atoms. For example, the hydrogen molecule, H2, contains a covalent bond between its two hydrogen atoms. Figure 13.7 illustrates why this bond is formed. Starting on the far right, we have two separate hydrogen atoms with a particular potential energy, indicated by the red line. Along the x-axis is the distance between the two atoms. As the two atoms approach each other (moving left along the x-axis), their valence orbitals (1s) begin to overlap. The single electrons on each hydrogen atom then interact with both atomic nuclei, occupying the space around both atoms. The strong attraction of each shared electron to both nuclei stabilizes the system, and the potential energy decreases as the bond distance decreases. If the atoms continue to approach each other, the positive charges in the two nuclei begin to repel each other, and the potential energy increases. The bond length is determined by the distance at which the lowest potential energy is achieved.
The potential energy of two separate hydrogen atoms (right) decreases as they approach each other, and the single electrons on each atom are shared to form a covalent bond. The bond length is the internuclear distance at which the lowest potential energy is achieved.
It is essential to remember that energy must be added to break chemical bonds (an endothermic process), whereas forming chemical bonds releases energy (an exothermic process). In the case of H2, the covalent bond is very strong; a large amount of energy, 436 kJ, must be added to break the bonds in one mole of hydrogen molecules and cause the atoms to separate:
H2(g)⟶2H(g)ΔH=436kJH2(g)⟶2H(g)ΔH=436kJ
Conversely, the same amount of energy is released when one mole of H2 molecules forms from two moles of H atoms:
2H(g)⟶H2(g)ΔH=−436kJ2H(g)⟶H2(g)ΔH=−436kJ
Pure vs. Polar Covalent Bonds
If the atoms that form a covalent bond are identical, as in H2, Cl2, and other diatomic molecules, then the electrons in the bond must be shared equally. We refer to this as a pure covalent bond. Electrons shared in pure covalent bonds have an equal probability of being near each nucleus.
In the case of Cl2, each atom starts off with seven valence electrons, and each Cl shares one electron with the other, forming one covalent bond:
Cl+Cl⟶Cl2Cl+Cl⟶Cl2
The total number of electrons around each individual atom consists of six nonbonding electrons and two shared (i.e., bonding) electrons for eight total electrons, matching the number of valence electrons in the noble gas argon. Since the bonding atoms are identical, Cl2 also features a pure covalent bond.
When the atoms linked by a covalent bond are different, the bonding electrons are shared, but no longer equally. Instead, the bonding electrons are more attracted to one atom than the other, giving rise to a shift of electron density toward that atom. This unequal distribution of electrons is known as a polar covalent bond, characterized by a partial positive charge on one atom and a partial negative charge on the other. The atom that attracts the electrons more strongly acquires the partial negative charge and vice versa. For example, the electrons in the H–Cl bond of a hydrogen chloride molecule spend more time near the chlorine atom than near the hydrogen atom. Thus, in an HCl molecule, the chlorine atom carries a partial negative charge and the hydrogen atom has a partial positive charge. Figure 13.8 shows the distribution of electrons in the H–Cl bond. Note that the shaded area around Cl is much larger than it is around H. Compare this to Figure 13.7, which shows the even distribution of electrons in the H2 nonpolar bond.
We sometimes designate the positive and negative atoms in a polar covalent bond using a lowercase Greek letter "delta," δ, with a plus sign or minus sign to indicate whether the atom has a partial positive charge (δ+) or a partial negative charge (δ–). This symbolism is shown for the H–Cl molecule in Figure 13.8.
(a) The distribution of electron density in the HCl molecule is uneven. The electron density is greater around the chlorine nucleus. The small, black dots indicate the location of the hydrogen and chlorine nuclei in the molecule. (b) Symbols δ+ and δ– indicate the polarity of the H–Cl bond.
Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity. Electronegativity is a measure of the tendency of an atom to attract electrons (or electron density) towards itself. It determines how the shared electrons are distributed between the two atoms in a bond. The more strongly an atom attracts the electrons in its bonds, the larger its electronegativity. Electrons in a polar covalent bond are shifted toward the more electronegative atom; thus, the more electronegative atom is the one with the partial negative charge. The greater the difference in electronegativity, the more polarized the electron distribution and the larger the partial charges of the atoms.
Figure 13.9 shows the electronegativity values of the elements as proposed by one of the most famous chemists of the twentieth century: Linus Pauling (Figure 13.10). In general, electronegativity increases from left to right across a period in the periodic table and decreases down a group. Thus, the nonmetals, which lie in the upper right, tend to have the highest electronegativities, with fluorine the most electronegative element of all (EN = 4.0). Metals tend to be less electronegative elements, and the group 1 metals have the lowest electronegativities. Note that noble gases are excluded from this figure because these atoms usually do not share electrons with others atoms since they have a full valence shell. (While noble gas compounds such as XeO2 do exist, they can only be formed under extreme conditions, and thus they do not fit neatly into the general model of electronegativity.)
The electronegativity values derived by Pauling follow predictable periodic trends, with the higher electronegativities toward the upper right of the periodic table.
Electronegativity versus Electron Affinity
We must be careful not to confuse electronegativity and electron affinity. The electron affinity of an element is a measurable physical quantity, namely, the energy released or absorbed when an isolated gas-phase atom acquires an electron, measured in kJ/mol. Electronegativity, on the other hand, describes how tightly an atom attracts electrons in a bond. It is a dimensionless quantity that is calculated, not measured. Pauling derived the first electronegativity values by comparing the amounts of energy required to break different types of bonds. He chose an arbitrary relative scale ranging from 0 to 4.
Linus Pauling
Linus Pauling, shown in Figure 13.10, is the only person to have received two unshared (individual) Nobel Prizes: one for chemistry in 1954 for his work on the nature of chemical bonds and one for peace in 1962 for his opposition to weapons of mass destruction. He developed many of the theories and concepts that are foundational to our current understanding of chemistry, including electronegativity and resonance structures.
Linus Pauling (1901–1994) made many important contributions to the field of chemistry. He was also a prominent activist, publicizing issues related to health and nuclear weapons.
Pauling also contributed to many other fields besides chemistry. His research on sickle cell anemia revealed the cause of the disease—the presence of a genetically inherited abnormal protein in the blood—and paved the way for the field of molecular genetics. His work was also pivotal in curbing the testing of nuclear weapons; he proved that radioactive fallout from nuclear testing posed a public health risk.
Electronegativity and Bond Type
The absolute value of the difference in electronegativity (ΔEN) of two bonded atoms provides a rough measure of the polarity to be expected in the bond and, thus, the bond type. When the difference is very small or zero, the bond is covalent and nonpolar. When it is large, the bond is polar covalent or ionic. The absolute values of the electronegativity differences between the atoms in the bonds H–H, H–Cl, and Na–Cl are 0 (nonpolar), 0.9 (polar covalent), and 2.1 (ionic), respectively. The degree to which electrons are shared between atoms varies from completely equal (pure covalent bonding) to not at all (ionic bonding). Figure 13.11 shows the relationship between electronegativity difference and bond type.
As the electronegativity difference increases between two atoms, the bond becomes more ionic.
A rough approximation of the electronegativity differences associated with covalent, polar covalent, and ionic bonds is shown in Figure 13.11. This table is just a general guide, however, with many exceptions. For example, the H and F atoms in HF have an electronegativity difference of 1.9, and the N and H atoms in NH3 a difference of 0.9, yet both of these compounds form bonds that are considered polar covalent. Likewise, the Na and Cl atoms in NaCl have an electronegativity difference of 2.1, and the Mn and I atoms in MnI2 have a difference of 1.0, yet both of these substances form ionic compounds.
The best guide to the covalent or ionic character of a bond is to consider the types of atoms involved and their relative positions in the periodic table. Bonds between two nonmetals are generally covalent; bonding between a metal and a nonmetal is often ionic.
Some compounds contain both covalent and ionic bonds. The atoms in polyatomic ions, such as OH–, NO3−,NO3−, and NH4+,NH4+, are held together by polar covalent bonds. However, these polyatomic ions form ionic compounds by combining with ions of opposite charge. For example, potassium nitrate, KNO3, contains the K+ cation and the polyatomic NO3−NO3− anion. Thus, bonding in potassium nitrate is ionic, resulting from the electrostatic attraction between the ions K+ and NO3−,NO3−, as well as covalent between the nitrogen and oxygen atoms in NO3−.NO3−.
Electronegativity and Bond Polarity
Bond polarities play an important role in determining the structure of proteins. Using the electronegativity values in Figure 13.9, arrange the following covalent bonds—all commonly found in amino acids—in order of increasing polarity. Then designate the positive and negative atoms using the symbols δ+ and δ–:
C–H, C–N, C–O, N–H, O–H, S–H
The polarity of these bonds increases as the absolute value of the electronegativity difference increases. The atom with the δ– designation is the more electronegative of the two. Table 13.5 shows these bonds in order of increasing polarity.
Bond Polarity and Electronegativity Difference
ΔEN
C–H 0.4 Cδ−−Hδ+Cδ−−Hδ+
S–H 0.4 Sδ−−Hδ+Sδ−−Hδ+
C–N 0.5 Cδ+−Nδ−Cδ+−Nδ−
N–H 0.9 Nδ−−Hδ+Nδ−−Hδ+
C–O 1.0 Cδ+−Oδ−Cδ+−Oδ−
O–H 1.4 Oδ−−Hδ+Oδ−−Hδ+
Silicones are polymeric compounds containing, among others, the following types of covalent bonds: Si–O, Si–C, C–H, and C–C. Using the electronegativity values in Figure 13.9, arrange the bonds in order of increasing polarity and designate the positive and negative atoms using the symbols δ+ and δ–.
Electronegativity Difference
C–C 0.0 nonpolar
Si–C 0.7 Siδ+−Cδ−Siδ+−Cδ−
Si–O 1.7 Siδ+−Oδ−Siδ+−Oδ−


text:
Q: graphics.beginStroke not working in IE11 or edge I'm painting a ruler to the canvas. The ruler paints in chrome but not in IE or Edge.
The tick marks of the ruler are not painting. I think my problem is in set stroke. Does IE not support set stroke?
Any idea what I'm doing wrong?
I think the problem is in these two lines but I'm unsure.
division.graphics.setStrokeStyle(0.5).beginStroke("black");
backgroundOfDivision.graphics.drawRect(-pixelsPerDivision / 2, 200, pixelsPerDivision, divisionHeight).endStroke();
Link to the ruler game
      function createRuler(lengthInInches, start) {

        var ruler = new createjs.Container();

        var pixelsPerDivision = settings.ruler.pixelsPerDivision;

        var totalDivisions = settings.ruler.divisionsPerInch * (lengthInInches);

        var cmPerInch = 2.54;
        var mmPerInch = cmPerInch * 10;

        var rectangle = new createjs.Shape();
        var rulerHeight = 200;
        rectangle.graphics.beginStroke("black").beginFill("white").drawRect(0, 200, totalDivisions * pixelsPerDivision, rulerHeight);

        ruler.addChild(rectangle);

        var divisionContainer;
        var backgroundOfDivision;

        var division, divisionHeight, numberText;

        var end = start + totalDivisions;

        var startDivision = start * settings.ruler.divisionsPerInch;

        //Paint Standard Ruler
        for (var i = 0; i <= totalDivisions; ++i) {

            divisionContainer = new createjs.Container();
            divisionContainer.value = i * (1 / settings.ruler.divisionsPerInch) + start;
            divisionContainer.unit = "in";
            backgroundOfDivision = new createjs.Shape();

            division = new createjs.Shape();
            division.x = i * pixelsPerDivision
            division.graphics.setStrokeStyle(0.5).beginStroke("black");

            if ((i + startDivision) % 32 == 0) {
                // make big line
                divisionHeight = 70;

                if ((i + startDivision) > 0) {
                    var numberText = new createjs.Text(((i + startDivision) / 32).toString(), "32px Arial", "black");

                    numberText.x = division.x;
                    numberText.y = divisionHeight + 200;
                    numberText.textAlign = "center";

                    divisionContainer.addChild(numberText);
                }

            }
            else if ((i + startDivision) % 8 == 0) {
                // make 1/4 inch line
                divisionHeight = 60;
            }
            else if ((i + startDivision) % 4 == 0) {
                // make 1/8 inch line
                divisionHeight = 45;
            }
            else if ((i + startDivision) % 2 == 0) {
                // make 1/16 inch line
                divisionHeight = 30;
            }
            else {
                // make 1/32 inch line
                divisionHeight = 15;

            }
            backgroundOfDivision.graphics.setStrokeStyle(0.5).beginStroke("Green").beginFill("Green");
            backgroundOfDivision.alpha = 0.0;
            backgroundOfDivision.graphics.drawRect(-pixelsPerDivision / 2, 200, pixelsPerDivision, divisionHeight).endStroke();
            backgroundOfDivision.x = i * pixelsPerDivision;

            division.graphics.drawRect(0, 200, 0, divisionHeight).endStroke();
            divisionContainer.divisionHeight = divisionHeight;
            divisionContainer.division = division;
            divisionContainer.backgroundOfDivision = backgroundOfDivision;

            divisionContainer.addChild(backgroundOfDivision);
            divisionContainer.addEventListener("rollover", function (e) {

                createjs.Tween.get(e.currentTarget.backgroundOfDivision).to({ alpha: 1.0 }, 500);
            });
            divisionContainer.addEventListener("rollout", function (e) {

                createjs.Tween.get(e.currentTarget.backgroundOfDivision, { override: true }).to({ alpha: 0.0 }, 250);
            });
            divisionContainer.addEventListener("mousedown", function (e) {
                if (clickedAnswerNowWait == false) {
                    btnClick();
                    clickedAnswerNowWait = true;
                    CheckAnswer(e.currentTarget)
                }
            });

            divisionContainer.addChild(division);
            ruler.addChild(divisionContainer);
            allTheDivisions.push(divisionContainer);
        }
}

A: The issue here is not with EaselJS beginStroke, but rather how browsers handle a 0-width rectangle.
To draw your ticks on your ruler, you are using:
division.graphics.beginStroke("green")
  .drawRect(0, 200, 0, divisionHeight);

In Chrome, this will show the stroke, however IE/Edge does not. To illustrate this, I created a simple demo that just does a stroke on a raw canvas:
var c=document.getElementById("canvas");
var ctx=c.getContext("2d");
ctx.rect(20,20,0,100);
ctx.stroke();

In Chrome, this shows a stroke, and IE/Edge it does not.
I would recommend instead using a stroke. It has the benefit of auto-centering as the stroke grows, and you can control the lineCap as well. If you want ticks that have a different fill/stroke, then rectangles are the way to go, as long as they are wider than 0.
Hope that helps!

redpajama_set_name: RedPajamaStackExchange


Missed the 1:1 (actual size) Gundam in Odaiba last year? Here's your chance to see it again.
The 18-meter Gundam statue is now located at East Shizuoka Square (north east of JR Shizuoka Station/Naganuma, Aoi-ku, Shizuoka City). It will be on display from July 24th, 2010 till January 10th, 2011.
The production factory for Bandai's Gundam plastic models is actually located in Shizuoka. So, that place is really significant when it comes to the world of Gundam.
Jump into the world of Dragon Ball and play as Goku and his friends in search of the seven mystical Dragon Balls! Dragon Ball: Origins 2 is an all-new action-adventure game encompassing Goku's battle against the Red Ribbon Army featuring a humorous and memorable story taken from the original anime series. Battle alone or with a friend on Goku's continuing quest with engaging controls and a fun mix of fierce fighting, dynamic action, exploration and puzzles!
In the Toy Story 3: The Video Game help Buzz, Woody and the rest of the Toys ensure no toy gets left behind. Dive into to all new heroic adventures in Story Mode or let your imagination run wild in the exiting new open world of Toy Box Mode! Come and play to infinity…and beyond.
More songs, more adventures and more fun. After defeating opponents from other dojos, the Taikos have embarked on a new journey to defeat the yokai (or devils). Win outfits and level up when you beat them.
This version will feature anime theme songs such as Totoro and Ponyo, Jpop songs such as Choo Choo train and rearranged classics such as Beethoven's symphonies. Taikos could play everything, and so do you.
With just one game software, a maximum of four people could join the party, you just need to turn on the Wi Fi control. Take part in the "Every Day Challenge" daily to see how much your taiko skills improved, win points and unlock new songs.
Players engage in nonstop shooter action as they're propelled through this on-rails game. Isa and Kachi are being hunted. They go on the run and on the defensive. And they shoot everything.
Sin & Punishment 2 is the long-awaited sequel to the Japanese Nintendo 64 cult-classic shooter. It brings a frantic arcade sensibility to a post-apocalyptic world. Fans who can't wait for the sequel can replay the original game by downloading it from the Virtual Console section of the Wii Shop Channel.
The Tamagotchis went to Chibichibi Island for vacation, and they have so much fun they almost didn't want to go home. And conveniently, they lost their tickets. So, the four extended their stay there. By helping the locals with their work, they will earn Gotchi points for their return trip.
Old mini games of course, are still available, along with new ones such as fishing and farming. Sail your boat into the waters and chase after the fish in the fishing games, or sow seeds, water the plants and harvest in the farming games. Small pests and insects may be attracted to your land, chase them away with the whistle to protect your hard work.
Rico Rodriguez is back but this time he's on a mission to go after the man who knows him best, his former commanding officer, mentor and friend. Tom Sheldon has gone rogue and disappeared with millions of agency cash and top secret intel. His last known whereabouts – the South East Asian island of Panau. Align with factions, take over military strongholds, gain influence within the island and ultimately cause chaos to destabilize the hostile government to locate your target and eliminate him.
The once great Kingdom of Brimthule is in despair following the loss of its lord and champion. King Leroy sacrificed himself to entomb the great beast Ragnakore in a body of stone. Without its leader, the kingdom has split into baronies and is beset by curses, monsters, and misfortunes, with some believing Ragnakore, though trapped, is responsible. The time has come for new heroes to stand tall against the realm's greatest foes, the time has come for the Dawn of Heroes.
Join the Fairy Tail guild and clear missions. Those who watch the anime or read the manga already know that the guild sends wizards to do all sorts of things; some times it's treasure hunting, some times it's rescuing, but all of them involve fantastic adventures, come get your magic circle and fight some bad guys.
Form a tag team like the ones in the anime, you take two people to the battlefield in the single player mode and a team of four people in the multi-player mode. Be sure to make use of the Wireless LAN, some of the monsters you fight are massive and you need 4 powerful wizards to subdue them.


text:
At the Kelly Gallery
by kellygallery
The Kelly Gallery's summer season of new graduate shows is well underway, and at the opening of the latest exhibition Black and Blue Part 2 featuring works by GSA graduates, the artists all agreed that having their work showcased by the RGI is a huge encouragement; a bridge between the adrenalin fuelled degree shows, and the challenge of finding work.
Lee Hutchinson who studied Fine Art Photography at GSA said:
"When the email came through from Lynne and Amy that my work had been selected for the new graduates' show, it was such a confidence boost. I came to last year's exhibition at the Kelly to view my friend's work and now it's a great feeling to be part of this year's show."
Originally from Newcastle, Lee is staying on in Glasgow as he feels the city's art scene is so vibrant. It's encouraging that the RGI's commitment to emerging talent is making a contribution to city's reputation as an arts hub.
The current show which runs until August 4, is followed by Cartel, an exhibition of selected works produced by BA Visual Arts gradates from North Glasgow College. Then Assembly with works by photographers from Glasgow's City College and UWS.
The private views are always an ideal opportunity for new graduates to meet and receive encouragement from established artists as well as members of the public. Amidst all this emerging talent, could well be the Turner Prize winners of the future.
Cartel: Artists from Glasgow's North College. 7 – 18 August 2012
Assembly: Photography from Glasgow's City College and UWS. 21 August – 1 September
A selection of works can be viewed online
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