Structure and Bonding

The bond described as the electrostatic attraction between two positive nucleii and a shared electron pair.

• Ionic bond

• Covalent bond

• Metallic bond

• Intermolecular force

The bonding described as the electrostatic attraction between positive ions and delocalised electrons.

• Ionic bonding

• Covalent bonding

• Metallic bonding

• Intermolecular forces

The bonding described as the electrostatic attraction between oppositely charged ions.

• Ionic bonding

• Covalent bonding

• Metallic bonding

• Intermolecular forces

Choose ALL the correct statements: Ionic compounds form...

• Small molecules

• Between metals and non-metals

• Between two non-metals

• Liquids at room temperature

• Giant lattice structures

Pick the best answer - Metals conduct electricity because

• The ions can move around

• The free electrons can move through the structure

• The delocalised electrons can move through the structure

• The delocalised electrons can vibrate

Hydrogen chloride is an example of a molecular substance, it has a low boiling point because...

• It only has on covalent bond per molecule, this makes it easy to break.

• It only has two atoms in the molecule and so it's bonds are weak.

• To boil only weak intermolecular forces need to be broken.

• To boil it is easy to break the intermolecular forces and covalent bonds because they are both weak.

Select all relevant points - Graphite can conduct electricity because...

• Each carbon only has three covalent bonds

• It is a metallic substance

• It's ions can move freely

• It has delocalised electrons that can move

• It is ionic

Diamond has a high melting point because

• It has many strong ionic bonds that require lots of energy to overcome.

• It is a giant metallic structure with strong electrostatic attractions that requires lots of energy to overcome.

• It has many strong covalent bonds that require lots of energy to overcome.

• There are lots of carbon atoms and so there are many intermolecular forces which requires lots of energy to overcome.

Select all correct answers - When would we expect ionic substances to be able to conduct electricity?

• Never

• Always

• As a liquid

• In solution

• As a solid

Sodium chloride has a high melting point, how would you expect the melting point of magnesium oxide to compare?

• Higher because it is a covalent compound, covalent bonds are stronger than ionic bonds and so more energy will be required to break the bonds.

• Higher because they have a 2+ and a 2- charge, which will create a stronger electrostatic attraction so more energy will be required to break the ionic bonds

• Lower because it is a covalent compound, covalent bonds are weaker than ionic bonds and so less energy will be required to break the bonds.

• Lower because because they have a 2+ and a 2- charge, which will create a weaker electrostatic attraction so less energy will be required to break the ionic bonds