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Water as a solvent VCE Chemistry Unit 2.1

Published byNicholas Newman Modified over 4 years ago


Presentation on theme: "Water as a solvent VCE Chemistry Unit 2.1"— Presentation transcript:

1 Water as a solvent VCE Chemistry Unit 2.1

2 Put sound on

3 Water Is essential to life.
Covers 70% of earth’s crust, but only 1% is drinkable. In ocean, atmosphere and on land. Found naturally as gas, liquid or solid. 67% of our body.

4 What do you know already about
Physical properties? Structure and bonding?

5 Physical Properties Colourless,odourless liquid at 25oC
Relatively high melting(0oC) and boiling temperature(100oC) High heat capacity - Requires a lot of energy to heat it up High latent heat Water expands when frozen Density of ice less than water Non-conductor Good solvent for polar compounds

6 covalent intramolecular bonding
Polar molecule Discrete molecular compound covalent intramolecular bonding bent

7 Bonding Between Water Molecules
Most properties can be explained because of the hydrogen bonding between the molecules. (Intermolecular)

8 Bonding Between Water Molecules
Oxygen is much more electronegative than hydrogen. Water forms polar molecules because electrons are more strongly attracted to the oxygen atom.

9 Hydrogen Bonding

10 Melting and Boiling Temperatures
Are higher than similar substances. This is because of the relatively high hydrogen bonding forces.

11 Specific Heat Capacity
= energy needed to raise the temperature of 1g of the substance by 1oC. It takes 4.19 J to raise the temperature of 1g water by 1oC. Water requires a large amount of heat to increase its temperature because energy is needed to overcome the H-bonds.

12 Latent Heat Amount of heat needed to change the state of a substance.
E.g. When heating ice the temperature remains constant until the ice is melted. Water has a high latent heat because of the hydrogen bonding holding the molecules together.

13 Latent Heat Latent heat of fusion. Energy needed to melt a substance.
Latent heat of vaporisation. Energy needed to vaporize a substance.

14 Expansion on Freezing The regular arrangement of water molecules in ice takes up more space than the irregular arrangement in liquids. Density of ice < density of water.

15 Water Molecules in Ice

16 Water As a Solvent Water will dissolve many substances
Solutions in water are aqueous solutions (aq).

17 Solution Chemistry In order for substance to dissolve:
The particles of the solute are separated from each other. The particles of the solvent are separated from each other. The solvent and solute particles attract each other.

18 Substances That Dissolve
1. Molecular compounds that A) form hydrogen bonds B) ionise 2. Ionic compounds that dissociate

19 Molecular Substances 1 A.Those that can form hydrogen bonds with water.E.G. Ethanol Both water and ethanol are polar molecules. They are able to mix freely forming hydrogen bonding between the molecules

20 water hydrogen bonding ethanol
Animation (long): hydrogen bonding ethanol


22 Molecular Substances 2 B.Those that ionise in water. E.g. hydrogen chloride HCl has a highly polarised bond which breaks in water. This is due to the force of attraction of the water molecules. Two ions are formed

23 Ionisation This process is known as IONISATION.
The ions are said to be hydrated. HCl(g) + H20(l) H30+(aq) + Cl –(aq) Hydronium ion

24 Ionic Compounds E.g. NaCl
The water molecules are attracted to the ions. They pull the sodium and chloride ions into the surrounding solution.

25 Sodium Chloride

26 Dissolving Salt H2O is a polar molecule.
The charged regions are attracted to ions with the opposite charge. Hence, the positively charged regions of water molecules are attracted to Cl- ions, and the negatively charged regions of water molecules are attracted to Na+ ions.



29 When several water molecules surround an ion in the crystal, the sum of the attractive forces between the water molecules and the ion may become strong enough to overcome the attractive forces between the cations and anions in the NaCl crystal.

30 Salt dissolving

31 http://ithacasciencezone. com/chemzone/lessons/03bonding/dissociate
Good animations of salt dissolving

32 Hydration of Ions The ions are now hydrated.
This is ion-dipole attraction. When positive and negative ions are separated from one another this called DISSOCIATION.

33 NaCl in Water

34 Hydration of Chloride ion

35 Hydration of Sodium Ion

36 Would you expect these molecules to be polar?

37 Solubility The maximum amount of a solute that will dissolve in a given quantity of solvent at a particular temperature. Usually measured as mass of solute in 100 g of water. A solution in which no more solute will dissolve is called a saturated solution.

38 Solubility Curves The relationship between solubility and temperature can be represented by a solubility curve. Each point on the curve represents as saturated solution. No more solute can be dissolved at that temperature. Saturated solution animation Demo

39 Solubility Curves

40 Solubility Rules

41 References Solubility
Great site

Download ppt "Water as a solvent VCE Chemistry Unit 2.1"
 Water – The Unique Substance Water and solutions Water Polarity Solubility (like dissolves like) Types of chemical compounds Chemical Bonding. Physical Properties of Ionic and Covalent Compounds Ionic Bonding and Ionic Compounds. Atoms and Ions  Atoms are the building blocks of matter (solids, liquids and gases).  For example:  Copper wire. By: Racquel Cantu & Nicole Keeler(:. Formation of Ions *An atom that has a net positive or negative electric charge is called an ion. *An ion with a negative. Chemistry Test Part 2 Review 1 Liquids and Solids Chapter Water Colorless, odorless and tasteless Density of ice < than density of liquid water –Not the normal trend –For equal.  Water molecule dipole moment.  The polarity of water affects its properties –Causes water to remain liquid at higher temperature –Permits ionic compounds. Chapter 13.1 Objectives Demonstrate the uniqueness of water as a chemical substance. Demonstrate the uniqueness of water as a chemical substance. Model. Metallic Solids Metals are not covalently bonded, but the attractions between atoms are too strong to be van der Waals forces In metals valence electrons. Cell Biology: Cell Compounds and Biological Molecules Ionic Bonding Structure and properties of ionic substances. Intermolecular Forces: relationships between molecules Basic Chemistry Copyright © 2011 Pearson Education, Inc. Chapter 10 Structures of Solids and Liquids 10.4 Attractive Forces between Particles 1. The Wonder of Water.

  SWBAT summarize what causes surface tension in water.  SWBAT define solution, solute, solvent and polar molecule.  SWBAT summarize the steps of dissolving.