AS periodicity + structure Flashcards

1
Q

How is the periodic table arranged?

A

In atomic numbers , groups and periods

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

3 factors affecting ionisation energies

A
  1. Nuclear charge - ↑ proton = ↑ attraction
  2. Atomic radius - ↑ dist. = ↓ attraction
  3. Shielding - ↑ shells = ↑ repulsion
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What stays relatively constant throughout the period

A

Atomic radius and shielding

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

3 exceptions to the steady ↑ in
ionisation energy across period

A
  1. group 2 -> 3
  2. group 5 -> 6
  3. increase in period
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Why is their a dip in ionisation energy between
group 2 -> 3 ?

(3 points)

A

electron removed is going from 2s -> 2p
↑ in atomic radius = ↓ attraction

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

Why is their a dip in ionisation energy between group 5 -> 6 ?

A

Group 5 has 3 electrons in 2p orbital
Group 6 has 4 electrons in 2p orbital
↑ repulsion at Group 6 as electron shares orbital

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

Why is there a dip in ionisation energy when going from down period?

A
  1. ↑ atomic radius
  2. ↑ shielding
  3. both factors outwiegh ↑ nuclear charge
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the pattern in ionisation energies down the group + WHY?

A

↓ down the group
1. gain a shell
2. shielding increases
3. atomic radius increases
4. both factors outweigh increased nuclear charge

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

How to predict group through successive ionisation energies ?

A

A peak in ionisation energies = no. of electron in outershell = group no.

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

Definition of ionisation energy

A

Energy required to remove 1 mol of electrons from 1 mol of gaseous atoms to form 1 mol of gaseous 1+ ions

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

Define Metallic bonding

A

The electrostatic attraction between metal cation and sea of delocalised electron

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

What is the structure of all metal ?

A

A gaint metallic lattice structure

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

4 Properties of metallic srtucture

A
  1. ↑ MP and BP
  2. ↑ electrical conductivity
  3. Insoluble
  4. malleable
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Define gaint covalent structure

A

A network of atoms bonded by strong covalent bond

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

Properties of gaint covalent structure

A
  1. high M.P. and B.P.
  2. Insoluble
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

electrical conductivity of graphite and diamond

A

Graphite - conducts
[only 3 covalent bond/carbon,1 mobile]
Diamond - Doesn’t
[ 4 covalent bonds, no mobile electron]

17
Q

describle the trend of B.P. across period

A

Group 1-4 = gradual increase [gaint structure]
Group 4-5 = sudden drop
group 5-8 = neglictible difference [simple molecular]

19
Q

Reactivity of group 2 down the group

A

INCREASES
1. ↑atomic radius
2. ↑shielding
3. ↓energy required to remove an electron

20
Q

What happens when group 2 reacts

A

oxidised to form 2+ ions

21
Q

What do Group 2 form when reacted to water

A

metal hydroxide and hydrogen

22
Q

how does solubility changes down the group 2 ? and WHY?

A

INCREASES solubility and pH
1. As they are more reactive down the group
2. particles are more likely to be attracted to polared molecules
3. hence more soluble

23
Q

how does pH changes down the group 2 ? and WHY?

A

INCREASES1. as they are mroe soluble down the group 2. more group 2 oxides reacts and form more OH ions 3. hence conc of OH increases

24
Q

What is the action of water on group 2 oxides

A

metal oxides + water -> metal 2+ + 2 OH -

25
2 uses of group 2 compounds
1. milk of magnesia (Mg(oH)2) - neutralise stomach acid 2. Calcium hydroxide neturalise acidic soil
26
What do all pure halogens exists in?
diatomic molecules
27
Trend of BP down the group 7?
Increases down the group 1. ↑ no. of electrons 2. ↑ London forces 3. ↑ electrons = ↑ london forces
28
Color of halogens in water
Cl - pale green Br - orange I - brown
29
which halogen have a different colour in organic solvent and what colour ?
In cyclohexane : Iodine - violet
30
Reactivity of Halogens down the group
Decreases 1. ↑ atomic radius' 2. ↑ shielding 3. ↓ nuclear attraction to GAIN ELECTRON
31
Rule for halogen displacement
More reactive displaces less reactive
32
formulae for Bleach
NaClO
33
formula for choric acid
HClO
34
Pros and cons of use of Chlorine in water treatment
Pros * kills bacteria (e.g. Cholera) Cons * irritant in small amount * fatal in large amounts * chlorinated hydrocarbon may form
35
How does atomic radius increases
down and left
36
How does 1st ionisation increases **across** period? | + explain (4)
1. ↑ nuclear charge 2. dist. from nucleus = k 3. shielding = k 4. ↓ atomic radius ↑ attraction so ↑
37
Colour of iodine in solution
Yellow - orange
38
Colour of bromine in solution
Orange
39
Colour of chlorine in solution
Pale green