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Chemistry > AS periodicity + structure > Flashcards

AS periodicity + structure Flashcards

1
Q

How is the periodic table arranged?

A

In atomic numbers , groups and periods

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2
Q

3 factors affecting ionisation energies

A
  1. Nuclear charge - ↑ proton = ↑ attraction
  2. Atomic radius - ↑ dist. = ↓ attraction
  3. Shielding - ↑ shells = ↑ repulsion
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3
Q

What stays relatively constant throughout the period

A

Atomic radius and shielding

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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
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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

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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

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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
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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

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9
Q

How to predict group through successive ionisation energies ?

A

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

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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

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11
Q

Define Metallic bonding

A

The electrostatic attraction between metal cation and sea of delocalised electron

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12
Q

What is the structure of all metal ?

A

A gaint metallic lattice structure

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13
Q

4 Properties of metallic srtucture

A
  1. ↑ MP and BP
  2. ↑ electrical conductivity
  3. Insoluble
  4. malleable
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14
Q

Define gaint covalent structure

A

A network of atoms bonded by strong covalent bond

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15
Q

Properties of gaint covalent structure

A
  1. high M.P. and B.P.
  2. Insoluble
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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]

18
Q
A
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
Q

2 uses of group 2 compounds

A
  1. milk of magnesia (Mg(oH)2) - neutralise stomach acid
  2. Calcium hydroxide neturalise acidic soil
26
Q

What do all pure halogens exists in?

A

diatomic molecules

27
Q

Trend of BP down the group 7?

A

Increases down the group
1. ↑ no. of electrons
2. ↑ London forces
3. ↑ electrons = ↑ london forces

28
Q

Color of halogens in water

A

Cl - pale green
Br - orange
I - brown

29
Q

which halogen have a different colour in organic solvent and what colour ?

A

In cyclohexane : Iodine - violet

30
Q

Reactivity of Halogens down the group

A

Decreases
1. ↑ atomic radius’
2. ↑ shielding
3. ↓ nuclear attraction to GAIN ELECTRON

31
Q

Rule for halogen displacement

A

More reactive displaces less reactive

32
Q

formulae for Bleach

A

NaClO

33
Q

formula for choric acid

A

HClO

34
Q

Pros and cons of use of Chlorine in water treatment

A

Pros
* kills bacteria (e.g. Cholera)

Cons
* irritant in small amount
* fatal in large amounts
* chlorinated hydrocarbon may form

35
Q

How does atomic radius increases

A

down and left

36
Q

How does 1st ionisation increases across period?

+ explain (4)

A
  1. ↑ nuclear charge
  2. dist. from nucleus = k
  3. shielding = k
  4. ↓ atomic radius

↑ attraction so ↑

37
Q

Colour of iodine in solution

A

Yellow - orange

38
Q

Colour of bromine in solution

A

Orange

39
Q

Colour of chlorine in solution

A

Pale green

Chemistry (6 decks)

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