Metallic Bonding Flashcards

1
Q

Metallic Bonding

A

Bonding between the sea of delocalised electrons and positive ions arranged in a lattice.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Metal elements structures

A

Giant Metallic Lattice Structure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Describe structure of metallic bonding

A

The outermost shell of electrons of a metal atom is delocalised- the electrons are free to move about the metal leaving a positive metal ion.

The positive metal ions are attracted to the delocalised negative electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Explain why metals have high melting points

A

Because of the strong electrostatic attractions between the positive metal ions and the delocalised sea of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Explain why the number of delocalised electrons per atom affects the melting point

A

The more delocalised electrons there are, the stronger the bonding will be and the higher the melting point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Explain why metals are good thermal conductors

A

The delocalised electrons can pass kinetic energy to each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Explain why metals are good electrical conductors

A

The delocalised electrons can move and carry a current

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Explain why metals are insoluble

A

Because of the strength of the metallic bonds

except in liquid metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly