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Chemistry Alevel > Inorganic Chemistry And The Periodic Table > Flashcards

Inorganic Chemistry And The Periodic Table Flashcards

1
Q

Group 2 + oxygen
General equation

A

Solid white oxide
2M(s) +O2(g)—-> 2MO(s)

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2
Q

Group 2 + chlorine
General equation

A

Solid white chlorides
M(s) + Cl2(g)——-> MCl2(s)

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3
Q

Group 2 + water
General equation

A

Metal hydroxide + hydrogen
M(s) + 2H2O(l) —-> M(OH)2 (aq) + H2(g)

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4
Q

Group 2 oxide + water
General equation

A

Hydroxides
MO(s) + H2O(l)—-> M(OH)2 (aq)

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5
Q

Group 2 oxide+ dilute acid
General equation

A

Salt+water
MO(s)+2HCl(aq)—-> MCl2(aq)+H2O(l)

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6
Q

Group 2 hydroxide + dilute acid
General equation

A

M(OH)2(aq)+2HCl(aq)—-> MCl2(aq)+2H2O(l)

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7
Q

Solubility trend group 2 hydroxides

A

Increases down the group
Solutions more strongly alkaline

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8
Q

Solubility trend group 2 sulfates

A

Decreases down the group

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9
Q

Trend in thermal stability down the group for G2 carbonates and nitrates

A

Increases
Polarising power of the cation decreases down the group as the ionic radius increases and so more shielding (lower charge density)
Less distortion of carbonate/ nitrate anion
Weakens the CO/ NO bond less

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10
Q

Thermal stability of G2 vsG1 nitrates/ carbonates

A

G2 carbonates/ nitrates are less thermally stable
The greater the charge on the cation, the greater the distortion and the less stable to anion becomes
2+ vs 1+

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11
Q

Thermal decomposition of G1 carbonates

A

Thermally stable (until higher temperatures)
Exception: Li2CO3 which decomposes to Li2O and CO2

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12
Q

Thermal decomposition of G2 carbonates

A

Form oxide and carbon dioxide
MCO3 (s)—-> MO(s) + CO2 (g)

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13
Q

Thermal decomposition of G1 nitrates

A

Forms nitrite and oxygen
2MNO3(s)——>2MNO2(s)+O2(g)
Exception:
LiNO3 which decomposes to form Li2O, NO2, O2

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14
Q

thermal decomposition of G2 nitrates

A

Forms oxide, nitrogen dioxide, oxygen
2M(NO2)2(s)——>2MO(s)+4NO2(g)+O2(g)

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15
Q

Testing the thermal stability of nitrates

A

How long it takes for a certain amount of oxygen to be produced (enough to relight a glowing splint)
How long it takes for an amount of brown gas (NO2) to be produced (in a fume cupboard)

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16
Q

Testing thermal stability of carbonates

A

How long it takes for an amount of carbon dioxide to be produced, use limewater

17
Q

Limewater

A

Saturated solution of calcium hydroxide)

18
Q

Formation of characteristic flame colours

A

Energy absorbed from the flams causes electrons to be promoted to higher energy levels, excitation. Electrons de excite and move back down to ground state, releasing energy in the form of light.
The difference in energy between the higher and lower energy levels determines the wavelength of light released and so the colour of light

19
Q

Flame colours for:
Lithium, sodium, potassium, rubidium, caesium, calcium, strontium and barium

A

Red, orange/ yellow, lilac, red, blue, brick-red, crimson, green

20
Q

States and colours of the halogens

A

F- pale yellow gas
Cl- green gas
Br- red/brown liquid
I- grey solid

21
Q

Colour change when halogen displaces halide in aqueous solution

A

Cl displaces Br- yellow/ orange
Cl or Br displaces I- brown

22
Q

Coloured layers of displaced halide after addition of an organic solvent

A

Bromine- orange/red
Iodine- pink/ violet
Chlorine is virtually colourless

23
Q

Hypochlorous acid (HClO)

A

Ionises to make chlorate (1) ions
HClO+H2O——>ClO-+H3O+
ClO- kill bacteria

24
Q

Disproportionation reaction of chlorine with cold, dilute aqueous sodium hydroxide to form bleach

A

Produces NaOX+NaX+H2O

25
Q

Disproportionation reaction of chlorine with hot alkali

A

Produces NaXO3+5NaX+3H2O

26
Q

Trend in reducing power of halides down the group

A

Increases
Because ions get bigger and there’s more shielding (outer electron more easily lost)

27
Q

Reaction of KF or KCl with H2SO4

A

KCl(s)+H2SO4(l)—->KHSO4(s)+HCl(g)
Misty fumes
Reaction stops here
Not redox
Chlorine not strong enough reducing reagent to reduce the sulfur further

28
Q

Reaction of KBr with H2SO4

A

KBr+H2SO4—>KHSO4+HBr misty fumes
2HBr(aq)+H2SO4(l)——>Br2(g)+SO2(g)+2H2O(l)
Redox
Sulfur oxidation state changes from +6 to +4
Br2 orange fumes

29
Q

Reaction of KI with H2SO4

A

KI+H2SO4—>KHSO4+HI
2HI(g)+H2SO4—->I2(g)+SO2+2H2O
6HI(g)+SO2(g)—->H2S(g)+3I2(s)+@H2O(l)
+6 to +4 then +4 to -2

30
Q

Reaction of hydrogen halides with ammonia and with water to produce acids

A

HX can dissolve in water to produce misty fumes of acidic gas (turn damp blue litmus paper red)
HX react with ammonia gas to produce white fumes
NH3(g)+HCl(g)——>NH4Cl(s)

31
Q

reaction of aqueous Cl-, Br- and I- with aqueous silver nitrate solution, followed by aqueous ammonia solution

A

+dilute nitric acid to remove ions
+silver nitrate solution
AgF soluble so no precipitate
AgCl- white + ammonia solution- precipitate dissolves to give colourless solution
AgBr- cream + ammonia solution- unchanged with dilute, dissolves in concentrated to form colourless solution
AgI- yellow + ammonia solution- does not dissolve (precipitate remains)

32
Q

Test for sulfates

A

+dilute HCl (removes carbonate ions)
+barium chloride solution
White precipitate of barium sulfate forms

33
Q

Test for ammonium ions

A

+NaOH
Gently heat
Ammonia gas given off is alkaline so will dissolve in the water on damp red litmus paper and turn it blue

34
Q

Equation for testing for ammonium ions

A

NH4Cl(aq)+NaOH(aq)—-> NH3(g)+H2O(l)+NaCl(aq)

35
Q

Explain how the trend in reactivity of group 2 elements is determined by their electronic configurations

A

Outer electron further from nucleus
More shielding
So first ionisation energy decreases down group so reactivity increases

Chemistry Alevel (16 decks)

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