Properties of substances Flashcards

You may prefer our related Brainscape-certified flashcards:
1
Q

What is ionisation energy?

A

Energy required to remove an electron from an atom in the gas state

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

What is the trend in ionisation energy?

A

Increases across a period left to right
Decreases down a group

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

How does the atomic radius affect the ionisation energy?

A

Larger radius
Lower ionisation energy

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

How does the Nuclear charge affect the ionisation energy?

A

Higher charge
Higher ionisation energy

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

How does the Shielding effect, affect the ionisation energy?

A

More sheilding
Lower ionisation energy

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

What happens to the ionisation across a period?

A

Ionisation energy increases as atoms are smaller and hold electrons tightly

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

What happens to the ionisation down a group?

A

Ionisation energy decreases as atoms are larger with more electron shielding

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

What happens to the atomic radius in the periodic table?

A

Decreases across a period
Increases down a group

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

What happens to the electronegativity in the periodic table?

A

Increases across a period
Decreases down a group

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

What happens to the melting and boiling points in the periodic table?

A

Increase from group 1 to group 4
Decrease from group 5 and stay relatively low to group 8

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

What is Polarity?

A

Distribution of electrical charge over atoms in a molecule

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

Describe metals

A

Conductive
Malleable
Lose electrons

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

Describe non-metals

A

Poor conductors
Brittle
Gain electrons

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

Describe Alkali metals

A

Group 1
Very reactive
Soft metals
Low melting point
Increases down the group

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

Describe Alkaline earth metals

A

Group 2
Reactive
Harder than alkali metals
Increases down the group
Found in Compounds like calcium

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

What is the reactivity of alkaline earth metals?

A

Increases as you move down the group du8e to decrease ionisation energy

17
Q

What is a redox reaction?

A

A reaction involving the transfer of electrons

18
Q

What is an oxidation reaction?

A

Loss of electrons

19
Q

What is a reduction reaction?

A

Gaining of electrons

20
Q

Where are transition metals found?

A

In the d-block of the period table

21
Q

What are the properties of a transition metal?

A

Form coloured compounds
Variable oxidation states
Good conductors

22
Q

What are transition metals used for?

A

Catalysts
Structural materials
Coins

23
Q

What are the characteristics of redox reactions of transition metals?

A

Transition metals often act as catalysts in redox reactions

24
Q

What is the variable oxidation sate of redox reactions of transition metals?

A

Change to oxidation state to facilitate redox reactions