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Edexcel A-Level Chemistry > Topic 4 - INORGANICS > Flashcards

Topic 4 - INORGANICS Flashcards

1
Q

Why does ionisation energy decrease down group 2?

A
  • Outer electron is in a successively higher energy level
  • Distance and shielding both increase
  • (Even though nuclear charge increases)
  • Attraction between outer electron and nucleus is weaker
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2
Q

What is the trend in reactivity down group 2?

A

‘Reducing strength’ increases down group 2
- The sum of 1st and 2nd ionisation energies decreases
- The strength of metallic bonding decreases

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3
Q

What is the trend in hydroxide solubility down group 2?

A

Group 2 hydroxides become more soluble down the group

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4
Q

What is the trend in sulphate solubility down group 2?

A

Group 2 sulphates become less soluble down the group

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5
Q

Group 2 metal + oxygen –> ?

A

Group 2 metal oxide

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6
Q

Are group 2 elements oxidised or reduced when reacted with something?

A

Always oxidised
- They gain a 2+ charge

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7
Q

What are the properties of a group 2 metal oxide?

A
  • Ionic compound
  • White solid
  • High melting point
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8
Q

Group 2 metal + chlorine –> ?

A

Group 2 metal chloride

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9
Q

What are the properties of a group 2 metal chloride?

A
  • Ionic compound
  • White solid
  • High melting point
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10
Q

Group 2 metal + water –> ?

A

Group 2 metal hydroxide + hydrogen

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11
Q

What are the observations of a reaction between a group 2 metal and water?

A
  • Effervescence
  • Metal disappears
  • Delayed white precipitate with Ca(OH)2
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12
Q

Group 2 metal oxide + water –> ?

A

Group 2 metal hydroxide

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13
Q

What are the observations of a reaction between a group 2 metal oxide and water?

A

White precipitate formed with Mg(OH)2 and Ca(OH)2

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14
Q

Group 2 metal oxide + acid –> ?

A

Salt + water

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15
Q

Why does CaCO3 thermally decompose?

A
  • Ca2+ ion polarises the CO3 2- ion
  • The lower electron density at the other end of the CO3 2- ion weakens a C-O bond
  • When provided with heat, the bond breaks
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16
Q

Why do nitrates thermally decompose?

A
  • The cation polarises the NO3- ion
  • The lower electron density at the other end of the NO3- ion weakens an N-O bond
  • When provided with heat the bond breaks
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17
Q

Are group 1/2 carbonates/nitrates more or less thermally stable down the group?

A

More stable

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18
Q

Why are group 1/2 carbonates + nitrates more thermally stable down the group?

A
  • Cation radius increases
  • Cation polarises CO3 2-/NO3- less
  • C-O/N-O bonds are weakened less
  • Either they break more slowly, or they need a higher temperature to break
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19
Q

What are the observations of group 1/2 carbonate decomposition?

A
  • Limewater turns cloudy
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20
Q

What are the observations of group 1/2 nitrate decomposition?

A
  • Glowing splint relights
  • Brown fumes
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21
Q

What is the trend of melting/boiling point down group 7?

A

Melting/boiling point increases down the group

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22
Q

Why does melting/boiling point increase down group 7?

A
  • More electrons per halogen molecule
  • Stronger London forces between molecules
  • More energy required to overcome IMFs
23
Q

How does state of matter vary down group 7?

A
  • Fluorine: Gas
  • Chlorine: Gas
  • Bromine: Liquid
  • Iodine: Solid
24
Q

How does colour change down group 7?

A

Colour becomes darker down the group
Pale yellow->grey

25
Q

Why do halogens dissolve poorly in water?

A
  • London forces are broken in ‘X2’
  • Hydrogen bonds are broken in H2O
  • Only London forces are formed between X2 and H2O
  • IMFs broken are stronger than IMFs formed
26
Q

Why do halogens dissolve well in hydrocarbon solvents?

A
  • London forces are broken in ‘X2’
  • London forces are broken in HC
  • London forces are also formed between X2 and HC
  • IMFs broken are similar to IMFs formed
27
Q

What is the trend in electronegativity down group 7?

A

Electronegativity decreases down group 7

28
Q

Why does electronegativity decrease down group 7?

A

The bonding electron pair is:
- Further from the nucleus
- Better shielded from the nucleus

Hence the attraction between the nucleus and bonding electron pair is weaker

29
Q

Are group 7 elements oxidised or reduced when reacted with something?

A

Reduced
- Gain a 1- charge

30
Q

What is the trend with reactivity of group 7 elements down the group?

A

Oxidising strength increases up the group
This is because the incoming electron is:
- Closer to the nucleus
- Less shielded from the nucleus

31
Q

What is a halogen displacement reaction?

A

When a more strongly oxidising halogen can oxidise the halide ions of less strongly oxidising halogens

32
Q

What colours are Cl2, Br2 and I2 in organic solutions?

A
  • CL2: pale green
  • Br2: red
  • I2: Purple
33
Q

What colours are Cl2, Br2 and I2 in aqueous solutions?

A
  • Cl2: pale green
  • Br2: yellow/orange
  • I2: brown
34
Q

What are the products of a chlorine disproportionation in water?
Cl2 + H2O –> ?

A

HCl + HClO

35
Q

What are the products of a chlorine disproportionation in cold, dilute alkali (NaOH)?
Cl2 + 2NaOH –> ?

A

NaCl + NaClO + H2O

36
Q

What are the products of a chlorine disproportionation in hot, concentrated alkali (NaOH)?
3Cl2 + 6NaOH –> ?

A

5NaCl + NaClO3 + 3H2O

37
Q

What state are hydrogen halides at room temp and pressure?

A

Gases

38
Q

Observations of the reaction between hydrogen halides + air + ammonia?

A
  • Steamy white fumes
  • Damp blue litmus paper turns red

+ Ammonia
- Dense white smoke

39
Q

What is the trend in reactivity in halide ions?

A

Reducing strength increases down the group

40
Q

Why does reducing strength increase down the group of halide ions?

A

Outer electron is:
- Further from nucleus
- Better shielded from nucleus
- Less strongly attracted by nucleus

41
Q

NaCl + H2SO4 –> ?
What are the observations?

A

NaHSO4 + HCl
- Effervescence
- Steamy white fumes
- White solid
- Damp blue litmus paper turns red

HCl cannot reduce NaHSO4 any further

42
Q

2HBr + H2SO4 –> ?
What are the observations?

A

Br2 + SO2 + 2H2O
- Brown liquid
- Orange fumes

43
Q

NaI + H2SO4 –?
What are the observations?

A

HI + NaHSO4
- Effervescence
- Steamy white fumes
- White solid
- Damp blue litmus paper turns red

HI is a strong enough reducing further to then reduce NaHSO4

44
Q

8HI + H2SO4 –> ?
What are the observations?

A

4I2 + H2S + 4H2O
- Grey solid
- Purple fumes

45
Q

What is the chemical test for the presence of halide ions?

A
  • Add dilute nitric acid
  • Then add silver nitrate
46
Q

What are the observations of the chemical test for the presence of halide ions?

A
  • Cl2: white precipitate
  • Br2: cream precipitate
  • I2: yellow precipitate
47
Q

What chemical is added to distinguish between halide precipitates, and what are the observations?

A

Ammonia solution
- AgCl: ppt disappears
- AgBr: ppt disappears in concentrated ammonia
- AgI: no change

48
Q

What colours are the flames according to group 1/2 cations?

A

Li+: Red
Na+: Yellow
K+: Lilac
Ca2+: Brick red
Sr2+: Red
Ba2+: Green

49
Q

What is the chemical test for chlorine?

A

Damp blue litmus paper turns white

50
Q

What is the chemical test for carbonates?

A
  • Add HCl
  • Bubble through limewater; if limewater turns cloudy, carbonates are present
51
Q

What is the chemical test for sulphates?

A

Chemical test for carbonates, then:
- Add barium chloride
- If sulphates are present, white ppt formed

52
Q

What is the chemical test for ammonium?

A
  • Add dilute sodium hydroxide
  • Damp blue litmus paper turns red
53
Q

What is the theory behind flame tests?

A
  • Electron absorbs heat energy and is promoted to a higher energy level
  • The electron is unstable in the higher energy level
  • The electron drops back to a more stable energy level by emitting a photon
54
Q

What are the disadvantages of using chlorine to sterilise water?

A
  • Toxic in excess
  • Can react with hydrocarbons to produce carcinogens

Edexcel A-Level Chemistry (16 decks)

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