Bonding

Question 1

Describe Ionic bonding

Answer 1

Electrons are transferred from a metal atom to a non-metal atom producing ions

Question 2

Describe simple covalent bonding

Answer 2

A shared pair of electrons between 2 non-metals

Question 3

Describe giant covalent bonding

Answer 3

A shared pair of electrons between 2 non-metals

Question 4

Describe metallic bonding

Answer 4

Positive Metal ions in a lattice structure surrounded by a sea of delocalised electrons

Question 5

Describe the melting points of ionic bonding

Answer 5

Have very high melting points as there are strong electrostatic forces of attraction between oppositely charged ions. These electrostatic forces of attraction require lots of energy to break.

Question 6

Describe melting points of simple covalent bonds

Answer 6

Have low melting points as there are weak intermolecular forces between molecules which don’t require much energy to break. These substances are liquid or gas at room temperature.

Question 7

Describe melting points of giant covalent bonds

Answer 7

Have very high melting points due to the many strong covalent bonds between atoms which require lots of energy to break.

Question 8

Describe melting points of metallic bonding

Answer 8

Have very high melting points due to the strong electrostatic forces of attraction between the positive metal ions and the negative delocalised electrons. These electrostatic forces of attraction require lots of energy to break.

Question 9

Describe the conductivity of ionic bonding

Answer 9

Only conduct when molten or in solution as the ions need to be free to move to carry charge. In a solid the ions are held in a fixed lattice structure and cannot move.

Question 10

Describe the conductivity of simple covalent bonds

Answer 10

Do not conduct electricity as the molecules have no overall charge

Question 11

Describe the conductivity of giant covalent bonds

Answer 11

Graphite conducts electricity as it has delocalised electrons which can move throughout the structure and carry charge. Diamond does not conduct electricity as it does not have any delocalised electrons. Each carbon in diamond is covalently bonded to 4 others.

Question 12

Describe the conductivity of metallic bonding

Answer 12

Conduct electricity as there are delocalised electrons which can move throughout the structure and carry charge.

Question 13

Describe the ionic bonding of Cl and L

Answer 13

L loses 1 electron to become L+ 2.
Cl gains 1 electron to become Cl- 2.8.8
1:1 ratio