Metals & Ions- T3

Question 1

What structure is an ionic compound held in?

Answer 1

A giant lattice structure.

Question 2

How is the lattice structure held together in an ionic compound?

Answer 2

By strong electrostatic attraction between oppositely charged ions.

Question 3

Why do ionic compounds have high melting and boiling points?

Answer 3

Due to strong electrostatic forces of attraction between oppositely charged ions which need lots of energy to overcome.

Question 4

When will ionic compounds conduct electricity and why?

Answer 4

When it is molten/ dissolved (aqueous)
Ions are free to move and carry the charge

Question 5

Why are ionic compounds soluble in water?

Answer 5

Water is polar so will attract the ions of either charges and pull the lattice apart.

Question 6

So.. what are the 4 properties of ionic compounds?

Answer 6

1) High melting and boiling points. 2) Soluble in water. 3) Conduct electricity when molten. 4) Doesn’t conduct electricity when solid.

Question 7

What 2 things affect the melting and boiling points of ionic lattices?

Answer 7

Ion size and charge.

Question 8

How are metals arranged?

Answer 8

Lattice of positive metal ions surrounded by a ‘sea’ of delocalised electrons.

Question 9

4 properties of metals and reasons:

Answer 9

1) Malleable (layers can slide over each other). 2) Insoluble (due to strong metallic bonds). 3) Conducts heat & electricity (delocalised electrons are free to move to carry the charge). 4) High melting point and boiling points (strong electrostatic attraction between +ve metals and delocalised electrons).

Question 10

What 2 things determine the strength of a metallic bond?

Answer 10

Charge on the ion and size.

Question 11

Weakest to strongest bonds: (covalent, metallic and ionic)

Answer 11

(weakest) Metallic– Ionic— Covalent (strongest)