Metallic Ionic Giant Covalent Simple Molecular Present Metals only Metals and Non-metals Non-metals only Non-metals only Bonding Metallic Ionic Covalent Covalent Structure Giant lattice Giant lattice Giant lattice Simple molecular Made up of Positive metal ions and Positive metal ions and negative Atoms Molecules delocalized electrons ions Diagram See specific examples of diamond, graphite and silicon dioxide Properties 1.High melting and boiling point 1.High melting and boiling point 1. High melting and 1. Low melting and boiling 2. Good conductor of electricity 2. Good conductor of electricity when boiling points points 3. Malleable (easy to be bent and dissolved in water or molten 2. Most do not conduct 2. Do not conduct electricity shaped) (the exception is Graphite) 1. Lots of energy needed to break 1. Lots of energy needed to break the 1. Lots of energy 1. Weak intermolecular forces of strong metallic bonds strong bonds between the positive needed to overcome that require very little energy to properties 2. Metals have delocalized and negative ions. the strong covalent be broken. electrons that are free to move 2. When Ionic compounds dissolve or bonds. 2. No free electrons throughout and carry an electric melt the ions are free to move and 2. No free electrons current carry an electric current. (except in graphite) 3. Metal atoms are arranged in layers that are able to slide over each other. Examples gold, platinum, iron sodium chloride, potassium flouride, diamond, graphite, chlorine, oxygen, magnesium oxide silicon dioxide hydrogen, helium
Metallic Ionic Giant Covalent Simple Molecular Present Metals only Metals and Non-metals Non-metals only Non-metals only Bonding Metallic Ionic Covalent Covalent Structure Giant lattice Giant lattice Giant lattice Simple molecular Made up of Positive metal ions and delocalized electrons Positive metal ions and negative ions Atoms Molecules Diagram See specific examples of diamond, graphite and silicon dioxide Properties 1.High melting and boiling point 2. Good conductor of electricity 3. Malleable (easy to be bent and shaped) 1.High melting and boiling point 2. Good conductor of electricity when dissolved in water or molten 1. High melting and boiling points 2. Most do not conduct (the exception is Graphite) 1. Low melting and boiling points 2. Do not conduct electricity of properties 1. Lots of energy needed to break strong metallic bonds 2. Metals have delocalized electrons that are free to move throughout and carry an electric current 3. Metal atoms are arranged in layers that are able to slide over each other. 1. Lots of energy needed to break the strong bonds between the positive and negative ions. 2. When Ionic compounds dissolve or melt the ions are free to move and carry an electric current. 1. Lots of energy needed to overcome the strong covalent bonds. 2. No free electrons (except in graphite) 1. Weak intermolecular forces that require very little energy to be broken. 2. No free electrons Examples gold, platinum, iron sodium chloride, potassium flouride, magnesium oxide diamond, graphite, silicon dioxide chlorine, oxygen, hydrogen, helium
Structure-bonding-and-properties-of-ionic-meallic-and-covalent-.docx