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Chemistry > Inorganic Chemistry And Periodic Table > Flashcards

Inorganic Chemistry And Periodic Table Flashcards

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1
Q

trend in ionisation in group 2

A

decrease down the group
outer electron distance from the nucleus increases
shielding also increases
attraction to the nucleus decreases

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2
Q

trend in reactivity in group 2

A

as you go down, increases
can lose electron easier
as increased shielding
increase atomic radii

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3
Q

reaction of group 2 with oxygen

A

2M + O2 → 2MO
except barium forms a peroxide
Ba + O2 → 2BaO2

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4
Q

flame colour of Mg

A

bright white

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5
Q

flame colour of Ca

A

brick red

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6
Q

flame colour of Sr

A

crimson

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7
Q

flame colour of Ba

A

apple green

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8
Q

reaction of group 2 with water

A

less reactive than group 1
Ca + 2H2O → Ca(OH)2 + H2
steam Mg + H2O → MgO + H2

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9
Q

reaction of group 2 with chlorine

A

when heated

Mg + Cl2 → MgCl2

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10
Q

reaction of group 2 oxides with water

A

CaO + H2O → Ca(OH)2

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11
Q

reaction of group 2 oxides with dilute acid

A

MgO + H2SO4 → MgSO4 + H2O
CaO + 2HNO3 → Ca(NO3)2 + H2O
BaO + 2HCl → BaCl2 + H2O

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12
Q

reaction of group 2 hydroxides with dilute acid

A

Ca(OH)2 + 2HNO3 → Ca(NO3)2 + 2H2O

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13
Q

trend in the solubilities of group 2 sulphates

A

decreases down the group
Ba2+(aq) + SO42-(aq) → BaSO4(s)
ca=slightly soluble
Sr+Ba=insoluble

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14
Q

trend in the solubilities of group 2 hydroxides

A

increases down the group

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15
Q

trend in thermal decomposition of group 1 carbonates

A

Li2CO3 Li2O + CO2
more thermally stable down the group
atomic radius increases
decreased charged density
decreased polarising power
aren’t able to distort the carbonate as much
Bonds in the carbonate aren’t weakened as much

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16
Q

trend in thermal decomposition of group 2 carbonates

A 
MgCO3 MgO + CO2
less thermally stable than group 1
higher charge density
more thermally stable down the group
raduis incr, less charge dense
decreased polarising power
Bonds in the carbonate aren’t weakened as much
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17
Q

trend in thermal decomposition of group 1+2 nitrates

A 
Li+G2 less thermally stable
2M(NO3)2 → 2MO + 4NO2 + O2
4LiNO3 → 2Li2O + 4NO2 + O2
G1 more stable break apart less
NaNO3 → 2NaNO2 + O2
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18
Q

reasons for flame tests colours

A

placed in a flame, their electrons are pushed to a higher energy level
electrons drop back to a lower level again, give out energy in the form of light
The light is characteristic of each particular metal and gives the flame a certain colour

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19
Q

flame test for Li

A

red

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20
Q

flame test for Na

A

yellow

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21
Q

flame test for K

A

lilac

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22
Q

states and colours of chlorine

A

Room temp= green gas
Aq=pale green
hydrocarbon solution=pale green

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23
Q

states and colours of Bromine

A

Room temp=red/brown liquid
Aq=orange/yellow
hydrocarbon=red

24
Q

states and colours of iodine

A

room temp=grey/black solid
Aq=brown
hydrocarbon=violet

25
Q

trend in bp+mp of group 7

A

increases down the group
have more electrons
stronger london forces
more energy need to overcome intermolecular forces

26
Q

electronegativity of group 7

A

decreases down the group
larger atomic radius
shared bonding pair of e- is further from nucleus
increased shielding

27
Q

trend in reactivity of group 7

A 
decreases down the group
increased shielding 
increased atomic radius
decreased attraction to the nucleus
harder to gain electrons
28
Q

example of halogen displacement reaction

A

Cl2 + 2KBr → Br2 + 2KCl

29
Q

when an organic solvent is added to displacement reactions

A

forms two layers

eg cyclohexane on the top layer

30
Q

colours of the two layers of bromine water in displacement

A

dissolves more easily in organic so dark orange top layer light less concentrated bottom layer

31
Q

colours of the two layers of iodine water in displacement

A

purple top layer pale green bottom layer

32
Q

halogen oxidizing power

A 
decreases down the group
increasing shielding
increasing atomic radius
decreasing attraction to the nucleus
electron gained less easily
33
Q

oxidation reactions of group 1+2 metals

A

2Na + Cl2 → 2NaCl

Mg + Br2 → MgBr2

34
Q

disproportionation reaction of chlorine with water

A

Cl2 + H2O ⇌ HOCl + HCl

35
Q

use of chlorine in water treatment

A

chloric(I) acid, HOCl, contains the chlorate(I) ion which has a strong anti-bacterial action, so sterilises the water

36
Q

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

A

Cl2 + NaOH → NaOCl + NaCl + H2O

produces a much higher concentration of chlorate(I)

37
Q

the disproportionation reaction of chlorine with hot alkali

A

3Cl2 + 6NaOH → NaClO3 + 5NaCl +3H2O

38
Q

halide reducing power

A

increases down the group
ion increases in size
more able to lose an electron and return to the Halogen. halide ion transfers its electron to another substance
substance is reduced

39
Q

Concentrated sulfuric acid with chloride

A

KCl + H2SO4 → KHSO4 + HCl

white steamy fumes produced

40
Q

Concentrated sulfuric acid with bromide

A

2HBr + H2SO4 → Br2 + 2H2O + SO2

orange-brown steamy fumes

41
Q

Concentrated sulfuric acid with iodide

A

2HI + H2SO4 → I2 + 2H2O + SO2

42
Q

halide test

A

Ag+(aq) + X-(aq) → AgX(s)
dissolved in water, acidified with dilute nitric acid
silver nitrate solution is added.
A precipitate of silver halide forms

43
Q

halide test to further determine

A

add dilute ammonia solution
concentrated ammonia solution
or
sunlight

44
Q

order of halide test with the colour gradient

A

CBI

45
Q

test for chloride

A

White precipitate
purple/grey in sunlight
dissolves in dilute ammonia

46
Q

test for bromide

A

cream precipitate
green/yellow is sunlight
partially dissolves in dilute fully dissolves in conc

47
Q

test for iodide

A

yellow precipitate
no effect in sunlight
doesn’t dissolve

48
Q

hydrogen halides with water

A

HX(aq) → H+(aq) + X-(aq)

soluble in water, and when dissolved in they split up (dissociate) into ions forming an acidic solution

49
Q

hydrogen halides with ammonia

A

HX(g) + NH3(g) → NH4X(s)

gaseous hydrogen halides come into contact with gaseous ammonia, dense white smoke of ammonium halide is produced

50
Q

assumptions of fluorine properties (too reactive to test)

A

strongest oxidising agent in the group, but fluoride ions would be the weakest reducing agent

51
Q

assumptions of astatine properties (too radioactive, has a short half-life)

A

weakest oxidising agent in the group, but astatide ions would be the strongest reducing agent

52
Q

test for Carbonate, hydrogencarbonate

A

CO32-(aq) + 2H+(aq) → H2O(l) + CO2(g)
HCO3-(aq) + H+(aq) → H2O(l) + CO2(g)
Add dilute HCl test gas given off with limewater

53
Q

test for Sulfate

A

Ba2+(aq) + SO42-(aq) → BaSO4(s)

Add dilute hydrochloric acid to a solution of X, followed by barium chloride solution, White precipitate forms

54
Q

test for Ammonium

A

NH4+(aq) + OH-(aq) → H2O(l) + NH3(g)

Warm X with sodium hydroxide solution, Hold damp red litmus to the mouth of the tube, Red litmus goes blue

55
Q

limewater test

A

Ca(OH)2(aq) + CO2(g) → CaCO3(s) + H2O(l)

colourless to cloudy

Chemistry (19 decks)

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