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

Topic 4 Inorganic Chemistry & Periodic Table Flashcards

(106 cards)

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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 solubility of g2 hydroxides? Why?

A

solubility increases down
hydroxIIIIIIIdes
Due to decreasing lattice enthalpies

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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
what are 2 factors affecting thermal stability?
1. charge of cation (eg g2 is 2+) - higher charge = more polarising = more thermal stable 2. ionic radius (smaller=more stable)
26
what is the size of ion's effect on thermal stability?
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
27
trend of thermal stability of g2 carbonates and nitrates down?
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
28
whats the general equation of metal nitrate decomposition? (if no brown fumes are observed)
metal nitrate -> metal nitrite + oxygen MNO3 -> MNO2 + O2
29
whats the general equation of metal nitrate decomposition (if brown fumes are observed)
metal nitrate -> metal oxide + nitrogen dioxide + oxygen
30
how to conduct a flame test?
- use safety apparatus - use concentrated HCl for more accurate results - use clean nichrome/platinum wire - hold above blue bunsen flame
31
why is concentrated HCl used in a flame test? (1 mark)
“To form volatile chlorides”
32
2 problems with flame tests
1. impurities in mixtures, more intense colours could mask another element 2. describe colours w words are subjective
33
whats the colour of lithium in a flame test?
red
34
whats the colour of sodium in a flame test?
yellow
35
whats the colour of potassium in a flame test?
lilac
36
whats the colour of rhubidium in a flame test?
red/purple
37
whats the colour of caesium in a flame test?
blue
38
whats the colour of beryllium in a flame test?
no colour
39
whats the colour of magnesium in a flame test?
no colour
40
whats the colour of calcium in a flame test?
(brick) red
41
whats the colour of strontium in a flame test?
(crimson) red
42
whats the colour of barium in a flame test?
apple green
43
what causes colours in flame tests?
- 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
how to test for ammonium ions?
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
what is the bp and mp trend in G7?
increasing down the group
46
why does mp and bp increase down g7?
London forces increase as number of e-s increase
47
what is the reactivity trend down g7?
reactivity decreases down since electronegativity decreases down (atomic radius gets larger)
48
explain the halide displacement reactions
elements higher up g7 are more reactive and displaces those down the group
49
what state does halide displacement have to take place in?
aqueous
50
what is disproportionation?
a species of an element is both reduced and oxidised in a reaction
51
what is chlorine's reaction to cold, dilute alkali?
Cl2+ 2NaOH -> NaCl + NaClO + H2O produces salts: sodium chloride and sodium chlorate(I) aka sodium hypochlorite
52
what is chlorine's reaction to hot concentrated alkali?
3Cl2 + 6NaOH -> NaClO3 + 5NaCl + 3H2O forms sodium chloride and sodium chlorate (V)
53
what the difference between halogen vs halide
halogen is diatomic eg Cl2 halide is an ion eg Cl-
54
what is the product and physical result of NaCl + H2SO4
misty fumes of hydrogen chloride (chloride ions have low reducing power)
55
what is the product and colour of NaBr + H2SO4
brown fumes of hydrogen bromide
56
what is the product and colour of NaI + H2SO4
purple fumes of hydrogen iodide
57
what is the reaction eq between sodium chloride and concentrated sulfuric acid?
NaCl + H2SO4 -> HCl + NaHSO4
58
what is the reaction eq between sodium bromide and concentrated sulfuric acid? then it further oxidising
NaBr + H2SO4 -> HBr + NaHSO4 2HBr + H2SO4 -> 2H2O + **SO2 + Br2**
59
formation of hydrogen iodide eq NaI + H2SO4 ->
HI + NaHSO4
60
how many redox reactions take place when sodium iodide reacts with conc sulfuric acid
3
61
how to test for halides in solution?
1. add dilute nitric acid (to remove other anions) 2. add silver nitrate solution 3. add dilute ammonia solution and conc
62
what is the reaction of chloride ions to silver nitrate, dilute aqueous ammonia and conc aqueous ammonia?
white precipitate soluble soluble
63
what is the reaction of bromide ions to silver nitrate, dilute aqueous ammonia and conc aqueous ammonia?
cream precipitate insoluble soluble
64
what is the reaction of iodide ions to silver nitrate, dilute aqueous ammonia and conc aqueous ammonia?
yellow precipitate insoluble insoluble
65
what is the general equation of halides' reacting with silver nitrate?
X- (aq)+ Ag+(aq) -> AgX(s) also AgNO3 + NaCl -> AgCl + NaNO3
66
what are hydrogen halides' reaction with water?
forms H3O+ and halide ion eg HCl + H2O -> H3O+ + Cl-
67
what do hydrogen halides (GAS) and ammonia GAS form? +eq
salts HCl(g) + NH3(g) -> NH4Cl (s) WHITE SOLID FORMED
68
NaCl + H2SO4 -> ?
HCl + NaHSO4
69
NaBr + H2SO4 -> ?
HBr + NaHSO4
70
NaI + H2SO4 -> ?
HI + NaHSO4
71
H2SO4 + 2H+ + 2I- -> ?
SO2 + I2 + 2H2O
72
H2SO4 (aq) + 6H+ (aq) + 6I- (s) ->
S (s) + 3 I2 (s) + 4H2O (l)
73
H2SO4 + 8H+ + 8 I- -> ?
H2S + 4 I2 + 4H2O
74
Why does reducing power increase down group 7 halide ions?
Because more shielding so lose electron easiest
75
8H+ + 8I‐ + H2SO4 →
4I2 + H2S + 4H2O
76
What is the thermal decomposition of Lithium nitrate? Give equation (It is different to the usually G1 or G2 metal trend)
4LiNO3 (s) -> 4NO2 + 4Li2O (s) + O2
77
What are the 5 products from reacting NaBr + H2SO4?
H2O SO2 HBr Br2 NaHSO4
78
Why do HCl and HBr reacting seperately with H2SO4 produce different gaseous products?
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
How to test if both chloride and iodide ions are present in a sample? (4 marks)
- 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
What is the thermal decomposition equation for calcium nitrate?
Ca(NO3)2 (s) -> CaO (s) + 2NO2 + 1/2 O2
81
what 2 observations from adding HCl to a tube of solid sodium carbonate?
effervesence white solid turns colourless
82
what does aqueous NaCl look like?
colourless solution bcs its dissolvable in water
83
all chlorides are soluble except..
silver and lead Ag and Pb
84
What is observed when HI reacts with conc NH3?
white smoke
85
What observations made when excess HCl is reacted with malachite?
Effervescence Green solution Solid malachite dissolves
86
MgCO3 + 2HCl ->
MgCl2 + H2O + CO2
87
Is G1 or G2 hydroxides more soluble?
G1 hydroxides are more soluble
88
What is the equation for strongly heating lithium nitrate?
4LiNO3 (s) -> 2 Li2O (s) + 4 NO2 (g) + O2 (g)
89
What is the equation for strongly heating lithium nitrate?
4LiNO3 (s) -> 2 Li2O (s) + 4 NO2 (g) + O2 (g)
90
What is the equation for strongly heating potassium nitrate?
KNO3 (s) -> KNO2 (s) + 1/2 O2 (g) Same for G1 metals except Li !!!
91
What is the equation for strongly heating caesium carbonate?
No decomposition Carbonates become more stable to heat as you go down the group
92
What is the equation for the reaction between chlorine and water?
Cl2 (g) + H2O (l) -> HOCl (aq) + HCl (aq)
93
What is the equation for the reaction between chlorine and water?
Cl2 (g) + H2O (l) -> HOCl (aq) + HCl (aq)
94
Which G1 carbonate is the only G1 cation that can be thermally decomposed?
Li2CO3 It is the only one that can - polarise the CO3 2- enough to weaken the bonds within it
95
Which G1 carbonate is the only G1 cation that can be thermally decomposed? Why?
Li2CO3 It is the only one that can - polarise the CO3 2- enough to weaken the bonds within it
96
What is the colour of flame test on calcium iodide?
(Yellow-) red
97
Why is HOCl + HCl not a good idea?
Produces Cl2 which is a toxic gas and can kill
98
Why is HOCl + HCl not a good idea?
Produces Cl2 which is a toxic gas and can kill
99
Why are there different **colours** in flame tests?
Different energy released in elements / diff energy gaps
100
Why is high decomposition temperature required to decompose CaCO3?
Strong bonds within the carbonate ions
101
Why is high decomposition temperature required to decompose CaCO3?
Strong bonds within the carbonate ions
102
Why is each ionisation energy more difficult than the last?
every time an electron is removed , remaining e-s are pulled closer because of less shielding
103
Why is there a big difference of ionisation energies between shells
Distance in sheiding As e-s are much closer to nucleus So more energy needed to overcome the stronger attraction
104
Calcium nitrate decomposes in a similar way to magnesium nitrate, but requires a higher temp for decomposition. Explain this observation in terms of the charge and size of cations. (3 marks)
Mg 2+ causes more polarisation As it has greater nuclear charge To N-O bonds
105
Explain why HBr, a colourless gas, appears as Misty fumes when it makes contact with moist air. (2 marks)
- HBr dissolves in water in air - forms droplets of hydrobromic acid
106
Explain the trend in reactivity of the primary chloro-, bromo- and iodoalkane with aqueous hydroxide ions. (2 marks)
- reactivity increases down G7 - as C-I enthalpy is the weakest, C-X enthalpy decreases - as it has the biggest atomic radius (polarity matters less)

Chemistry Edexcel A Level (24 decks)

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