Structure 2.3 Flashcards

1
Q

Process of removing electrons from metals is …thermic

A

Endothermic

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

Do metals or nonmetals require more energy to remove electrons?

A

Non metals

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

Electrical conductivity caused by

A

Movement of charged particles

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

Why are metals good conductors of electricity?

A

As current is carried by the delocalised electrons and there is low electrical resistance

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

Why do metals have a low electrical resistance?

A

Delocalised electrons can move freely

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

Why are metals good conductors of heat?

A

Delocalised electrons can carry heat, the friction caused by their movement causes the metal to heat up.

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

What is the strength of a metallic bond determined by?

A
  • The number of delocalised electrons
  • The charge of the cation
  • The radius of the cation
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Across a period, size

A

Decreases as electrostatic attraction pulls electrons closer to the nucleus.

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

Metallic bonding is

A

Very strong due to high melting points

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

Only liquid metal at room temp

A

Mecury

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

When a series of metals form cations with the same charges, the larger the cation…

A

The weaker the metallic bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

As an atom increases, the attraction between the cation and the delocalised electrons…

A

Decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Across a period, what happens to the charge of a cation and the radius of a cation?

A

Charge increases, radius decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Malleable

A

Can be beaten into shape with a hammer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Ductile

A

Can be drawn into a wire

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Why are metals malleable and ductile?

A

Close packed layers of cations can slide over each other without breaking, movement of the delocalised electrons are non-directional and random

17
Q

D block elements are all metals - what is the trend with their atomic radius and their melting points?

A

Atomic radius decreases slightly moving across period, no pattern in melting points

18
Q

Transition metals conductivity

A

All good conductors of heat and electricity

19
Q

Why are transition metals good conductors?

A

They have a large number of s and d valence electrons which can delocalise

20
Q

Transition element

A

Element with a d subshell that is partially filled

21
Q

Process of removing an electron is

A

Endothermic (higher energy in metals)

22
Q

Transition metal melting points trend

A

No clear trend, however it is very high compared to the s and p block metals