Bonding - State Of Matter

Question 1

Metallic bonding and electrons

Answer 1

Metals are giant structures of atoms.
The electrons in the outer shell are free to move around (delocalised)
Strong forces of electrostatic attraction between the positive metal ions and the shared negative ions
These forces of attraction are known as metallic bonds
They hold atoms together in a regular pattern.

Question 2

How does the bonding in metals affect their properties?

Answer 2

Metallic bonds are strong - lots of energy required to break them
This means that most substandes with metallic bonds hage very high melting and boiling pointe
Theyre usuallt solid at room temperature
The delocalised electrons in the metal are free to move
These electrons carry electrical charge and thermal energy through whole structure
This means metals are good conductors of electricity and heat
The layers in atoms can slide over eachither
Because of this, metals can be bent or formed into different shapes (malleable and ductile)

Question 3

Metallic bonding found in alloys

Answer 3

Pure metals are often soft
Most of the metals we use are allots
An alloy is a mixture or two or more metals, or a metal and another element
Mixing another element with a pure metal causes the layers of metal atoms to lose their shape. This is because different elements have different sized atoms.
It becomes more difficult for the atoms to slide over each other.
This makes alloys harder, and so more useful than pure metals.