3.1.3.3 Metallic bonding

Question 1

What is metallic bonding?

Answer 1

The electrostatic force of attraction between positive metal ions and a sea of delocalised electrons

Question 2

What are the properties of metallic compounds?

Answer 2

High m.p./b.p.
Good conductors of heat/ electricity
Malleable and ductile

Question 3

Why do metals have a high melting/boiling point?

Answer 3

Strong electrostatic attraction between positive metal ions and the sea of delocalised electrons

Question 4

What is the trend of boiling points down a group for metallic compounds?

Answer 4

Decreases
- delocalised electrons are further away from positive ions as you move down the group since
number of electrons shells increase. So attraction between positive ions and delocalised electrons gets weaker

Question 5

What is the trend of boiling points across a period for metallic compounds?

Answer 5

Increases
- Number of delocalised electrons increases as the charge of the metal ion becomes bigger, so the attraction between the delocalised electrons and the metal ions increases, so more energy to break bond.

Question 6

What determines the strength of a metallic bond?

Answer 6

Number of delocalised electrons
Charge on the cation
Radius of the cation

Question 7

Why are metals good conductors of heat?

Answer 7

Delocalised electrons free to move so they transfer thermal energy through the structure

Question 8

Why are metals good conductors of electricity?

Answer 8

Ions are free to move so carry charges.
Delocalised electrons are free to move so carry charges

Question 9

Why are metals malleable and ductile?

Answer 9

Layers of atoms can slide over eachother