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"Shut up," said Chemistry absently > 4: Inorganic Chemistry > Flashcards

4: Inorganic Chemistry Flashcards

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1
Q

Trend in ionisation energies down group 2

A

Ionisation energies decrease

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2
Q

Reason for group 2 trend in ionisation energies

A

The atomic radius increases and the shielding increases

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3
Q

Trend in reactivity down group 2

A

Metals become more reactive down group 2

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4
Q

Combustion of group 2 metals (excluding barium)

A

2M + O2 → 2MO

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5
Q

Combustion of barium

A

Ba + O2 → BaO2

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6
Q

Reaction of group 2 metals with water (except magnesium and beryllium)

A

M + 2 H2O → M(OH)2 + H2

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7
Q

Reaction of magnesium and steam

A

Mg + H2O → MgO + H2

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8
Q

Reaction of metals and chlorine

A

M + Cl2 → MCl2

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9
Q

Reaction of group 2 metal oxides with water (excluding beryllium oxide)

A

MO + H20 → M(OH)2

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10
Q

General reaction of acid and base

A

Acid + Base → Salt + Water

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11
Q

Trend in solubility of group 2 sulphates

A

Solubility decreases down the group

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12
Q

Group 2 sulphates with their solubility

A

Magnesium - Soluble
Calcium - Slightly soluble
Strontium - Insoluble
Barium - Insoluble

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13
Q

Trend in solubility of group 2 hydroxides

A

Solubility increases down the group

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14
Q

Group 2 hydroxides with their solubility

A

Magnesium - Insoluble
Calcium - Soluble
Strontium - Soluble
Barium - Soluble

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15
Q

Trend in thermal stability of carbonates

A

Thermal stability increases down the groups

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16
Q

Reason for trend in thermal stability of carbonates

A
  • As the cations become larger, the charge density becomes less, so they distort the anion less
  • This distortion weakens the C-O bond
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17
Q

Reason for group 1 carbonates being more stable than group 2

A

The charge on the cation is less

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18
Q

Nitrate thermal stability

A

-All nitrates thermally decompose

19
Q

Group 1 nitrates thermal decomposition (excluding lithium nitrate)

A

2 MNO3 → 2 MNO2 + O2

20
Q

Group 2 nitrates thermal decomposition

A

2 M(NO3)2 → 2 MO + 4 NO2 + O2

21
Q

Lithium nitrate thermal decomposition

A

4 LiNO3 → 2 Li2O + 4NO2 + O2

22
Q

Explanation of flame colours in flame tests

A
  • When group 1 or 2 metals or their compounds are placed in a flame, the electrons are pushed to a higher energy level
  • As the electrons drop back down they give out energy as light
23
Q

How to show the trend of thermal decomposition in carbonates

A
  • Pass the gas produced through limewater

- Record how long it takes to turn cloudy

24
Q

Appearance of Fluorine

A

RTP - yellow gas

25
Q

Appearance of Chlorine

A

RTP - pale green gas
Aq - colourless
Org - colourless

26
Q

Appearance of Bromine

A

RTP - brown liquid
Aq - yellow/orange
Org - orange

27
Q

Appearance of Iodine

A

RTP - grey solid
Aq - brown
Org - Purple

28
Q

Trend in MP/BP of halogens

A

MP/BP increase down the group as there are more electrons, and therefore stronger London forces

29
Q

Trend in electronegativity of halogens

A

Electronegativity decreases down the group and atomic radius increases and more shielding

30
Q

Trend in reactivity of halogens

A

Reactivity decreases down the group as the attraction of the nucleus decreases as there is more shielding

31
Q

How to show trend in reactivity in halogens

A

Can be shown by the displacement in the reaction of a halogen with a Group 1 metal halide (e.g Cl2 + 2KBr → Br2 + 2KCl)

32
Q

Reaction of a halogen with a metal

A

2 M + X2 → 2 MX

33
Q

Chlorine reaction with water

A

Cl2 + H20 ⇌ HCl + HClO

34
Q

Use of reacting chlorine with water

A

HClO sterilises water, and is in small quantities as the reaction is reversible

35
Q

Chlorine reaction with cold NaOH

A

Cl2 + NaOH → NaClO + NaCl

36
Q

Chlorine reaction with hot NaOH

A

3 Cl2 + 6 NaOH → NaClO3 + 5 NaCl

37
Q

Formula of bleach

A

NaClO

38
Q

Reaction of Fe(II) with halides

A

Fluorine, Chlorine and Bromine are strong enough to oxidise F2 + 2 Fe(II) → 2 F- + 2 Fe(III)

39
Q

Reaction of Group 1 halides with concentrated sulphuric acid

A

MX + H2SO4 → MHSO4 + HX

40
Q

Addition reaction following Group 1 halides reaction with conc. H2SO4

A

Only with bromide/iodide: 2 HX + H2SO4 → X2 + 2 H20 + SO2

41
Q

Trend in strength as reducing agent in halides

A

As the halide ions become bigger they become more able to lose an electron and therefore become stronger

42
Q

Dissolving and dissociation of hydrogen halides in water

A

HX → H+ + X-

43
Q

Reaction of hydrogen halides and gaseous ammonia

A

HX + NH3 → NH4X

44
Q

Observation in reaction of hydrogen halides and gaseous ammonia

A

Dense white smoke produced

"Shut up," said Chemistry absently (9 decks)

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