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chemistry > inorganic chemistry > Flashcards

inorganic chemistry Flashcards

1
Q

potassium chloride flame test colour

A

lilac

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2
Q

copper chloride flame test colour

A

bluey greeny

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3
Q

calcium chloride flame test colour

A

orange red

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4
Q

lithium chloride flame test colour

A

red/pink

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5
Q

sodium chloride flame test colour

A

yellow

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6
Q

with what and why do we clean the wire?

A
  • clean with hydrochloric acid (HCl)
  • cleans the wire to remove any impurities. also allows the ions to stick onto the wire
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7
Q

soluble or insoluble - all nitrates

A

soluble

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8
Q

soluble or insoluble - most common chlorides

A

soluble

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9
Q

soluble or insoluble - most common sulphates

A

soluble

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10
Q

soluble or insoluble - lead + silver chloride

A

insoluble

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11
Q

soluble or insoluble - sodium, potassium, ammonium, sometimes calcium hydroxide

A

soluble

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12
Q

soluble or insoluble - most metal hydroxides

A

insoluble (sometimes almost)

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13
Q

soluble or insoluble - sodium potassium and ammonium compounds

A

soluble

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14
Q

soluble or insoluble - lead sulphate, barium, silver and calcium

A

insoluble

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15
Q

soluble or insoluble - sodium, potassium, ammonium carbonates

A

soluble

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16
Q

hydrogen gas test

A

put a lit splint near the test tube
if hydrogen is present, a squeaky pop should occur

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17
Q

oxygen gas test

A

glowing (not lit) splint put near the test tube
if oxygen is present, the splint should be set alight

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18
Q

carbon dioxide gas test

A

bubble the gas through and aqueous solution of calcium hydroxide (aka limewater)
if carbon dioxide is present, limewater should turn milky

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19
Q

chlorine gas test

A

damp litmus paper over test tube
if chlorine gas is present, the litmus paper bleaches and turns white

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20
Q

ammonia gas test

A

damp red litmus paper/universal indicator over test tube
if ammonia gas is present, the red litmus paper turns blue

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21
Q

water physical test

A

boil/freeze it at 100°C
its water if it freezes/boils

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22
Q

water chemical test

A

add anhydrous copper to water
if water is present it turns blue

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23
Q

blue litmus paper in acid

A

red

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24
Q

blue litmus paper in alkali

A

blue

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25
Q

red litmus paper in acid

A

red

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26
Q

red litmus paper in alkali

A

blue

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27
Q

universal indicator in acid

A

red-yellow

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28
Q

universal indicator in alkali

A

blue-purple

29
Q

phenolphthalein in acid

A

no colour

30
Q

phenolphthalein in alkali

A

pink

31
Q

methyl orange in acid

A

red

32
Q

methyl orange in alkali

A

yellow

33
Q

general ionic equation

A

Mx+ + XOH -> M(OH)

34
Q

precipitation reaction?

A

soluble + soluble -> insoluble salt

35
Q

acid and a metal oxide reaction?

A

acid + metal oxides -> salt + water

36
Q

what are alkalis (in terms of bases)

A

bases that dissolve in water

37
Q

chlorine colour

A

yellow-green

38
Q

bromine colour

A

red-brown

39
Q

iodine colour

A

purple

40
Q

trends in group 7

A

gas -> liquid -> solid as you go down
increasing melting + boiling point
less reactive as you go down

41
Q

why do halogens become less reactive the more you go down

A

since the halogens react by gaining an electron on the outer shell:

  • outer shell becomes further from the nucleus
  • electron shielding increases
  • attraction decreases between nucleus and outer electrons
  • electrons are gained less easily
  • halogens become less reactive
42
Q

approximate percentages of gases abundant (theres four of them)

A

78% nitrogen
21% oxygen
0.9% argon
0.04% carbon dioxide

43
Q

what conditions are needed for rusting

A

air and water

44
Q

ways to prevent rusting

A

barrier, sacrificial protection, galvanising

45
Q

galvanising

A

applying a protective zinc coat onto iron which stops the air and water from rusting it since zinc is more susceptible to ionise.

46
Q

reactivity series

A

potassium
sodium
lithium
calcium
magnesium
aluminium
carbon
zinc
iron
lead
hydrogen
copper
silver
gold
platinum

47
Q

metal and acid form

A

metal + acid -> salt + hydrogen

48
Q

oxidation

A

gain of oxygen/loss of electron

49
Q

reduction

A

gain of electron/loss of oxygen

50
Q

redox

A

where both oxidation and reduction occur

51
Q

oxidising agent

A

causes another reactant to be oxidised and is reduced itself

52
Q

reducing agent

A

causes another reactant to be reduced and is oxidised itself

53
Q

metal + oxygen

A

metal + oxygen -> metal oxide

54
Q

sacrificial protection

A

attaches a more reactive metal (like a magnesium ribbon) to the iron as it will oxidise more easily, preventing the iron from rusting

55
Q

barrier method

A

coating with paint, grease or oil and grease

56
Q

what ions do metal atoms form

A

positive

57
Q

test for halide ions

A

add dilute nitric acid followed by silver nitrate solution

58
Q

chloride precipitate colour

A

white

59
Q

bromide precipitate colour

A

cream

60
Q

iodide precipitate colour

A

yellow

61
Q

copper (II) precipitate colour

A

blue

62
Q

iron (II) precipitate colour

A

green

63
Q

iron (III) precipitate colour

A

brown

64
Q

sulfate ions test

A

add dilute hydrochloric acid followed by barium chloride solution
a white precipitate will form if sulfate ions are present

65
Q

carbonate ions test

A

carbonates react with dilute acid to create carbon dioxide
gas is bubbled through limewater. if the limewater is cloudy co2 is present

66
Q

acids and bases in terms of proton transfer

A

acids transfer protons
bases accept protons

67
Q

acid + metal carbonate

A

acid + metal carbonate -> salt + water + carbon dioxide

68
Q

how to draw out ammonium gas from random powder

A

chemistry (4 decks)

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