Metallic Bonding and Properties

Question 1

What is metallic bonding?

Answer 1

Metallic bonding is a strong electrostatic force of attraction between metal ions and delocalised electrons.

Question 2

Why does every metal conducts electricity?

Answer 2

This is due to the metallic bonding find with in metal elements. In metallic bonding the outer electrons delocalised (free to move). This produces an electrostatic force of attraction between positively charged metal ions and negatively charged delocalised electron.

Question 3

What are the properties of metals?

Answer 3

High melting points
Good conductors of electricity
Good conductors of heat
High density

Question 4

Some metals have properties that are not typical what are they?

Answer 4

Mercury has a low melting point exists as a liquid at room temperature
Elements in group one have low melting points but also low densities

Question 5

What is the boiling point/melting points, state at room temperature and conduction of electricity in ionic lattice’s, covalent networks, discrete covalent molecules and metallic?

Answer 5

Ionic lattices have a high melting/boiling points, they are a solid at room temperature and only conduct electricity when molten or in solution
Covalent networks have a very high melting and boiling point and are solid at room temperature and
never conduct electricity except from graphite
Discreete covalent molecules have low boiling and melting point, are a liquid or gas at room temperature and they never conduct electricity
Metallic have high melting and boiling points they’re solid at room temperature except from Mercury which is a liquid and they conduct Electricity