U11 - metallic bonding Flashcards

1
Q

Def: Metallic bonds

A

Metal lattice of positive ions, surrounded by a sea of delocalised electrons

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

Explain the structure of the metal lattices, zinc and sodium

A

Coulomb forces between the negatively charged electrons attract the positively charged ions in a giant metallic structure.
The electrostatic forces between the positive and negatively charged particles are strong

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

How many electrons does sodium aluminium and magnesium lose

A

Sodium - 1 e
Aluminium - 3 e
Magnesium - 2 e

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

Why does aluminium have a higher melting and boiling point than sodium

A

Aluminium has the stronger electrostatic forces i.e. +3 and -3, and will therefore have the higher melting and boiling point than sodium that only has +1 and -1 charges holding the particles together

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

Properties of metals

A

shiny
malleable
sonorous
good conductor of electricity
good conductor of heat

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

Def: shiny

A

he delocalised electrons on the surface reflect light

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

Def: Malleable

A

the positive atomic rests occur in layers, the layers are held together
by strong forces and can slide over each other without breaking apart.
The delocalised electrons maintain attraction between the layers of positive ions.

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

Def: Sonorous

A

when struck, metals make a ringing sound, because the
vibration is carried through the metal by the delocalised electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Why is metals good conductors of electricity

A

The delocalised electrons are free to move and
therefore carry charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Why are metals good conductors of heat

A

The metal ions are closely packed in the ionic lattice (dense)
which allow the ions to bump into each other, transferring energy from one particle to the next.
The delocalised electrons are also able to take the energy and travel through the metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Why are metals good conductors of heat

A

The metal ions are closely packed in the ionic lattice (dense)
which allow the ions to bump into each other, transferring energy from one particle to the next.
The delocalised electrons are also able to take the energy and travel through the metal

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