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N Chemistry A Level > Topic 4 Inorganic Chemistry & Periodic Table > Flashcards

Topic 4 Inorganic Chemistry & Periodic Table Flashcards

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1
Q

What is the first ionisation energy?

A

energy required to remove an electron from each atom in one mole in a gaseous state

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2
Q

What is the definition of second ionisation energy?

A

energy required to remove an electron from an atom with 1+ charge in one mole in gaseous state

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3
Q

What is the first ionisation trend in group 2?

A

ionisation energy decreases down

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4
Q

why does ionisation energy decrease down group 2?

A

number of shielding increases
more quantum shells down group 2
therefore less energy is required to overcome less electrostatic attraction between the nucleus and the outermost shell e-s

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5
Q

What is the trend of reactivity down group 2? Why?

A

increases down bcs it is easier to remove the 2 outermost shell e-s

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6
Q

what is the first ionisation energy equation?

A

X(g)-> X+(g) + e-

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7
Q

Why is beryllium less reactive than barium?

A

There are more numbers of shielding in barium than beryllium, so the electrostatic attraction between the protons in the nucleus and o.s.e is less, so less energy is needed to ionise and overcome

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8
Q

where is barium stored?

A

in oil so it doesn’t react with oxygen and water vapour in air

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9
Q

what is the reaction when Mg is burnt in air?

A

bright flame and formation of white solid

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10
Q

what is the general equation of G2 metals and oxygen? (equation)

A

2M(s) + O2(g) -> 2MO(s)

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11
Q

What is the reaction between G2 metals and chlorine? (equation)

A

M(s) + Cl2(g) -> MCl2 (s)

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12
Q

what is the trend of physical reaction of G2 metals with water?

A

Increasing effervescence down the group

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13
Q

what is the general eq of G2 Metals and water?

A

M(s) + 2H2O(l) -> M(OH)2(aq) + H2(g)

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14
Q

what is the general eq of calcium and water?

A

Ca(s) + 2H2O(l) -> Ca(OH)2(s!) + H2(g)

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15
Q

What is the reacion between Mg and steam? (eq)

A

Mg(s) + H2O(l) -> MgO(s) + H2 (g)

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16
Q

what are G2 oxides’ reactions with water? (Physical property)

A

form colourless solutions

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17
Q

what is the general equation for g2 oxides and water?

A

MO (s) + H2O(l) -> M(OH)2 (aq)
can be simplified to
O2- + H2O -> OH-
alkali solutions formed

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18
Q

trends in solubillity of g2 hydroxides?

A

solubility increases down
hydroxIIIIIIIdes

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19
Q

what is the test for CO2?

A

limwater aka Calcium hydroxide Ca(OH)2 from clear to cloudy as CaCO3 formed

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20
Q

what are the reactions of G2 metal oxides / hydroxides with acid?

A

neutralisation reactions
salt and water produced

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21
Q

How is g2 oxides and hydroxides used in agriculture?

A

using Lime Ca(OH)2 to neutralise acidity in soil

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22
Q

what is the trend of solubility of g2 sulfates and carbonate?

A

solubility decreases down the group
suLLLLLphateSSSS
LESS
carbonate Sulfate Same

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23
Q

what are the solubility of g2 nitrates and chlorides?

A

ALL are SOLUBLE

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24
Q

how are sulfates tested?

A
  1. Add dilute nitric acid (prevent carbonates forming)
  2. using solution w barium ions (eg Barium nitrate)
    white precipitate of BaSO4 formed
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25
Q

what are 2 factors affecting thermal stability?

A
  1. charge of cation (eg g2 is 2+) - higher charge = more polarising = more thermal stable
  2. ionic radius (smaller=more stable)
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26
Q

what is the size of ion’s effect on thermal stability?

A

smaller = higher charge density = more polarising = less energy needed to break the bonds = less stable
attraction between nucleus and carbonate ion increases down , so more energy needed to break

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27
Q

trend of thermal stability of g2 carbonates and nitrates down?

A

increasing down
T.S. becomes more stable down, more heat is needed down for decomposition to occur
Bcs atom sizes increases, and becomes less polarising

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28
Q

whats the general equation of metal nitrate decomposition? (if no brown fumes are observed)

A

metal nitrate -> metal nitrite + oxygen
MNO3 -> MNO2 + O2

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29
Q

whats the general equation of metal nitrate decomposition (if brown fumes are observed)

A

metal nitrate -> metal oxide + nitrogen dioxide + oxygen

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30
Q

how to conduct a flame test?

A
  • use safety apparatus
  • use concentrated HCl for more accurate results
  • use clean nichrome/platinum wire
  • hold above blue bunsen flame
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31
Q

why is concentrated HCl used in a flame test?

A

to convert metal compounds to a chloride, chlorides are more volatile so results are more accurate

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32
Q

2 problems with flame tests

A
  1. impurities in mixtures, more intense colours could mask another element
  2. describe colours w words are subjective
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33
Q

whats the colour of lithium in a flame test?

A

red

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34
Q

whats the colour of sodium in a flame test?

A

yellow

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35
Q

whats the colour of potassium in a flame test?

A

lilac

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36
Q

whats the colour of rhubidium in a flame test?

A

red/purple

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37
Q

whats the colour of caesium in a flame test?

A

blue

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38
Q

whats the colour of beryllium in a flame test?

A

no colour

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39
Q

whats the colour of magnesium in a flame test?

A

no colour

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40
Q

whats the colour of calcium in a flame test?

A

(brick) red

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41
Q

whats the colour of strontium in a flame test?

A

(crimson) red

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42
Q

whats the colour of barium in a flame test?

A

apple green

43
Q

what causes colours in flame tests?

A
  • electrons absorb energy from heat and move to higher energy levels
  • bcs they become excited
  • it is unstable
  • e-s return to ground state, energy released as radiation that could be a visible colour
44
Q

how to test for ammonium ions?

A
  1. add sodium hydroxide solution (OH- to test for NH3+) + heat
  2. use damp red litmus paper on the gaseous state, turns blue if positive

NH4+ + NaOH -> NH3 + H2O

45
Q

what is the bp and mp trend in G7?

A

increasing down the group

46
Q

why does mp and bp increase down g7?

A

London forces increase as number of e-s increase

47
Q

what is the reactivity trend down g7?

A

reactivity decreases down
since electronegativity decreases down (atomic radius gets larger)

48
Q

explain the halide displacement reactions

A

elements higher up g7 are more reactive and displaces those down the group

49
Q

what state does halide displacement have to take place in?

A

aqueous

50
Q

what is disproportionation?

A

a species of an element is both reduced and oxidised in a reaction

51
Q

what is chlorine’s reaction to cold, dilute alkali?

A

Cl2+ 2NaOH -> NaCl + NaClO + H2O
produces salts: sodium chloride and sodium chlorate(I) aka sodium hypochlorite

52
Q

what is chlorine’s reaction to hot concentrated alkali?

A

3Cl2 + 3NaOH -> NaClO3 + 5NaCl + H2O
forms sodium chloride and sodium chlorate (V)

53
Q

what the difference between halogen vs halide

A

halogen is diatomic eg Cl2
halide is an ion eg Cl-

54
Q

what is the product and physical result of NaCl + H2SO4

A

misty fumes of hydrogen chloride
(chloride ions have low reducing power)

55
Q

what is the product and colour of NaBr + H2SO4

A

brown fumes of hydrogen bromide

56
Q

what is the product and colour of NaI + H2SO4

A

purple fumes of hydrogen iodide

57
Q

what is the reaction eq between sodium chloride and concentrated sulfuric acid?

A

NaCl + H2SO4 -> HCl + NaHSO4

58
Q

what is the reaction eq between sodium bromide and concentrated sulfuric acid?
then it further oxidising

A

NaBr + H2SO4 -> HBr + NaHBr

2HBr + H2SO4 -> H2O + SO2 + Br2

59
Q

formation of hydrogen iodide eq
NaI + H2SO4 ->

A

HI + NaHSO4

60
Q

how many redox reactions take place when sodium iodide reacts with conc sulfuric acid

A

3

61
Q

how to test for halides in solution?

A
  1. add dilute nitric acid (to remove other anions)
  2. add silver nitrate solution
  3. add dilute ammonia solution and conc
62
Q

what is the reaction of chloride ions to silver nitrate, dilute aqueous ammonia and conc aqueous ammonia?

A

white precipitate
soluble
soluble

63
Q

what is the reaction of bromide ions to silver nitrate, dilute aqueous ammonia and conc aqueous ammonia?

A

cream precipitate
insoluble
soluble

64
Q

what is the reaction of iodide ions to silver nitrate, dilute aqueous ammonia and conc aqueous ammonia?

A

yellow precipitate
insoluble
insoluble

65
Q

what is the general equation of halides’ reacting with silver nitrate?

A

X- (aq)+ Ag+(aq) -> AgX(s)
also
AgNO3 + NaCl -> AgCl + NaNO3

66
Q

what are hydrogen halides’ reaction with water?

A

forms H3O+ and halide ion
eg
HCl + H2O -> H3O+ + Cl-

67
Q

what do hydrogen halides (GAS) and ammonia GAS form? +eq

A

salts
HCl(g) + NH3(g) -> NH4Cl (s)
WHITE SOLID FORMED

68
Q

NaCl + H2SO4 -> ?

A

HCl + NaHSO4

69
Q

NaBr + H2SO4 -> ?

A

HBr + NaHSO4

70
Q

NaI + H2SO4 -> ?

A

HI + NaHSO4

71
Q

H2SO4 + 2H+ + 2I- -> ?

A

SO2 + I2 + 2H2O

72
Q

H2SO4 (aq) + 6H+ (aq) + 6I- (s) ->

A

S (s) + 3 I2 (s) + 4H2O (l)

73
Q

H2SO4 + 8H+ + 8 I- -> ?

A

SO2 + 4 I2 + 4H2O

74
Q

Why does reducing power increase down group 7 halide ions?

A

Because more shielding so lose electron easiest

75
Q

8H+ + 8I‐ + H2SO4 →

A

4I2 + H2S + H2O

76
Q

What is the thermal decomposition of Lithium nitrate? Give equation (It is different to the usually G1 or G2 metal trend)

A

4LiNO3 (s) -> 4NO2 + 4Li2O (s) + O2

77
Q

What are the 5 products from reacting NaBr + H2SO4?

A

H2O
SO2
HBr
Br2
NaHSO4

78
Q

Why do HCl and HBr reacting seperately with H2SO4 produce different gaseous products?

A

HBr is a stronger reducing agent than HCl (releases H+ ions easier due to larger bond length)
, so reduces sulfur further
HBr can reduce H2SO4 but HCl cannot
So more reduction reactions take place to produce more products

79
Q

How to test if both chloride and iodide ions are present in a sample? (4 marks)

A
  • dilute nitric acid and silver nitrate
  • filter paper filter ppt
  • add dilute ammonia solution
  • add dilute nitric acid to filtrate, if white ppt forms, proves chloride presence
  • add conc ammonia solution to filtrate, if stays white, iodide present
80
Q

What is the thermal decomposition equation for calcium nitrate?

A

Ca(NO3)2 (s) -> CaO (s) + 2NO2 + 1/2 O2

81
Q

what 2 observations from adding HCl to a tube of solid sodium carbonate?

A

effervesence
white solid turns colourless

82
Q

what does aqueous NaCl look like?

A

colourless solution bcs its dissolvable in water

83
Q

all chlorides are soluble except..

A

silver and lead
Ag and Pb

84
Q

What is observed when HI reacts with conc NH3?

A

white smoke

85
Q

What observations made when excess HCl is reacted with malachite?

A

Effervescence
Green solution
Solid malachite dissolves

86
Q

MgCO3 + 2HCl ->

A

MgCl2 + H2O + CO2

87
Q

Is G1 or G2 hydroxides more soluble?

A

G1 hydroxides are more soluble

88
Q

What is the equation for strongly heating lithium nitrate?

A

4LiNO3 (s) -> 2 Li2O (s) + 4 NO2 (g) + O2 (g)

89
Q

What is the equation for strongly heating lithium nitrate?

A

4LiNO3 (s) -> 2 Li2O (s) + 4 NO2 (g) + O2 (g)

90
Q

What is the equation for strongly heating potassium nitrate?

A

KNO3 (s) -> KNO2 (s) + 1/2 O2 (g)
Same for G1 metals except Li !!!

91
Q

What is the equation for strongly heating caesium carbonate?

A

No decomposition
Carbonates become more stable to heat as you go down the group

92
Q

What is the equation for the reaction between chlorine and water?

A

Cl2 (g) + H2O (l) -> HOCl (aq) + HCl (aq)

93
Q

What is the equation for the reaction between chlorine and water?

A

Cl2 (g) + H2O (l) -> HOCl (aq) + HCl (aq)

94
Q

Which G1 carbonate is the only G1 cation that can be thermally decomposed?

A

Li2CO3
It is the only one that can
- polarise the CO3 2- enough to weaken the bonds within it

95
Q

Which G1 carbonate is the only G1 cation that can be thermally decomposed?

A

Li2CO3
It is the only one that can
- polarise the CO3 2- enough to weaken the bonds within it

96
Q

What is the colour of flame test on calcium iodide?

A

(Yellow-) red

97
Q

Why is HOCl + HCl not a good idea?

A

Produces Cl2 which is a toxic gas and can kill

98
Q

Why is HOCl + HCl not a good idea?

A

Produces Cl2 which is a toxic gas and can kill

99
Q

Why are there different colours in flame tests?

A

Different energy released in elements / diff energy gaps

100
Q

Why is high decomposition temperature required to decompose CaCO3?

A

Strong bonds within the carbonate ions

101
Q

Why is high decomposition temperature required to decompose CaCO3?

A

Strong bonds within the carbonate ions

102
Q

Why does each ionisation energy more difficult than the last?

A

every time an electron is removed , remaining e-s are pulled closer because of less shielding

103
Q

Why is there a big difference of ionisation energies between shells

A

Distance in sheiding
As e-s are much closer to nucleus
So more energy needed to overcome the stronger attraction

N Chemistry A Level (19 decks)

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