Metallic Bonding/Properties of Metals [C]

Question 1

What is metallic bonding?

Answer 1

Metallic bonding is when atoms are surrounded by a sea of delocalised electrons

Question 2

How does attraction change between the atoms and electrons in metallic bondings?

Answer 2

As the electrons become delocalised, the atoms become positive ions.
The electrons attract the +ions and the +ions attract to the electrons

Question 3

What are some properties of metals?

Answer 3

They are:
- Shiny
- Ductile
- Malleable
- High melting point
- Good heat/electricity conductor

Question 4

Why does melting point decrease as we go down group 1?

Answer 4

As we go down the group, the melting point decreases.

This is because the electrons gets shielded from the nuclear charge which weakens the pull.
The atomic radius also gets bigger which weakens the attraction.

Question 5

How does the melting point change across a period? Why is this?

Answer 5

Melting points increase across a period.

As we go across the period, the pull force on the delocalised electron increases which causes a stronger bond

Question 6

Why are metals conductive and ductile?

Answer 6

The sea of delocalised electrons can carry the current which makes them conductive

The atoms are arranged in layers which can be pulled from over each other which allows them to be ductile.