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chemistry > Inorganic > Flashcards

Inorganic Flashcards

1
Q

Salt flame test colour
Lithium chloride

A

Red

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2
Q

Salt flame test colour
Sodium chloride

A

Yellow

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3
Q

Salt flame test colour
Potassium chloride

A

Lilac

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4
Q

Salt flame test colour
Barium Chloride

A

Green

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5
Q

Salt flame test colour
Calcium chloride

A

Orange red

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6
Q

Salt flame test colour
Strontium chloride

A

red

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7
Q

Salt flame test colour
Magnesium chloride

A

no colour

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8
Q

Salt flame test colour
Copper chloride

A

Blue-green

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9
Q

Salt flame test colour
Zinc chloride

A

Colourless

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10
Q

G2M reaction with oxygen

A

Burn in oxygen to form simple metal oxides
2X(s) + O2(g)—> 2XO(s)

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11
Q

G2M reaction with chlorine

A

Burn in chlorine gas to form solid metal chlorides
X(s) + Cl2(g) —> XCl2(s)

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12
Q

G2M reaction with water

A

Beryllium= no reaction due to thick oxide layer
Magnesium= slight reaction to cold water
Mg(s) + 2H2O(l) —> Mg(OH)2 (s) + H2 (g)
Reaction soon stops because magnesium hydroxide is almost insoluble in water and forms a barrier
Magnesium will react with steam to form metal hydroxide and hydrogen
Mg(s) + H2O(l)—>MgO(aq) + H2(g)
Other G2M react with cold water with increasing vigour to give metal hydroxide and hydrogen
Ca(s) + 2H2O(l)—>Ca(OH)2 (aq) + H2(g)

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13
Q

Oxides of G2M with water

A

MgO reacts slightly with water
CaO fizzes to form calcium hydroxide
Solubility of oxides in water increases down a group

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14
Q

Trend in solubility of G2M oxides down a group

A

Increases

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15
Q

Reaction of oxides of G2M with acids

A

React with dilute HCl to form chloride salt and water
React with dilute nitric acid to form nitrate salt and water
XO(s) + 2HNO3 (aq)—> X(NO3)2 (aq)

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16
Q

Reaction of G2M hydroxides with HCl and HNO3

A

React similarly to G2M oxides
X(OH)2 + 2HCl (aq) —> XCl2(aq) + 2H2O

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17
Q

Solubility of G2M hydroxides

A

Increases down group
Ionic radius increases so metal ions get larger so charge density decreases
Get a lower attraction between OH- and 2+ ions
Ions more easily split apart
Greater conc of OH- ions in water

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18
Q

Solubility of G2M sulfates

A

Decrease down group
Mg and Ca =soluble

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19
Q

Test for sulfate

A

Soluble Ba salt
Ba2+(aq) + (SO4)2 2- —> BaSO4 (s) white precip

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20
Q

General formula of G2M carbonates

A

MCO3

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21
Q

G2M carbonates solubility

A

Insoluble in water

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22
Q

Thermal decomposition of G2M carbonates

A

MCO3 (s) —> MO + CO2

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23
Q

Trend in thermal decomposition down G2M carbonates

A

increase down group, Harder down group= more thermally stable

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24
Q

General formula of G2M nitrates

A

M(NO3)2

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25
Q

G2M nitrates solubility in water

A

Soluble

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26
Q

Thermal decomposition of G2M nitrates

A

2M(NO3)2(s) —> 2MO(s) + 4NO2(g) + O2

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27
Q

Trend in thermal decomposition if G2M nitrates down group

A

increase down group, Becomes harder=more thermally stable

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28
Q

Thermal stability

A

Indicator of the ease with which compounds decompose on heating

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29
Q

factors deciding thermal stability of G2M carbonates and nitrates

A

-charge on metal ion
-size of metal ion

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30
Q

generally what is more stable G2M carbonates/nitrates, or G1M carbonates/nitrates

A

G1M compounds

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31
Q

effect of charge of metal ion on thermal stability

A

larger charge on metal ion=smaller ion=less stable

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32
Q

effect of size of metal ion on thermal stability

A

smaller ion=less stable

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33
Q

polarising power

A

the extent at which the positive ion can distort neighboring electron cloud

34
Q

halide ions …. electrons and become ……. molecules. …… ions lose electrons more ……

A

lose
halogen
larger
easily

35
Q

trend in reducing agent going down halide group

A

become better reducing agents as you go down

36
Q

general half equation formula of oxidation of halides

A

2X- →X2 + 2e-

37
Q

list the halides in order of worst to best reducing agent

A

Cl-
Br-
I-

38
Q

reaction of halide
Cl- (chloride) salt with conc sulfuric acid H2SO4

A

white effervesence

39
Q

which halide reaction involving chloride observes white effervescence

A

reaction of chloride salt and H2SO4 sulfuric acid

40
Q

reaction of halide
Cl- (chloride) with indicator paper

A

orange=acidic

41
Q

reaction of halide
Cl- (chloride) with conc ammonia

A

white fumes
Cl- dissolves dilute and conc ammonia

42
Q

reaction of halide
Cl- (chloride) with lead acetate paper

A

no change, remains white because Cl- cannot reduce H2SO4 (OS sulfur=+6) to H2S (OS sulfur=-2)

43
Q

reaction of halide
Cl- (chloride) with acidified dichromate solution

A

no change, remains yellow
Cl- cannot reduce H2SO4 (OS sulfur=+6) to SO2 (OS sulfur=+4)

44
Q

write the equation for sodium chloride salt with sulfuric acid

A

NaCl + H2SO4 → NaHSO4 + HCl

OS of sulfur remains at +6
not a redox reaction

45
Q

reaction of halide
Br- (Bromide) salt with conc sulfuric acid H2SO4

A

yellow/orange effervescence

46
Q

reaction of halide
Br- (Bromide) salt with indictor paper

A

red=acidic

47
Q

reaction of halide
Br- (Bromide) salt with conc ammonia

A

white fumes, Br- dissolves CONC ammonia not dilute ammonia

48
Q

reaction of halide
Br- (Bromide) salt with conc ammonia

A

white fumes, Br- dissolves CONC ammonia not dilute ammonia

49
Q

reaction of halide
Br- (Bromide) salt with lead acetate paper

A

no change (white)
Br- is not a strong enough reducing agent to reduce H2SO4 (OS sulfur=+6) to H2S (OS sulfur=-2)

50
Q

reaction of halide
Br- (Bromide) salt with acidified dichromate solution

A

yellow to white
Br- is a strong enough reducing agent to reduce H2SO4 (OS sulfur=+6) to SO2 (OS sulfur=+4)

51
Q

write 2 reactions, starting with sodium bromide with H2SO4 and then the redox. and the changes in OS of both bromine and sulfur

A

NaBR + H2SO4→NaHSO4 + HBr
2HBr + H2SO4→SO2 +2H2O + Br2

Bromine = -1→0
sulfur= +6→+4

52
Q

reaction of halide
I- (iodide) salt with conc sulfuric acid H2SO4

A

brown/black/red effervescence

53
Q

reaction of halide
I- (iodide) with indicator paper

A

red=acidic

54
Q

reaction of halide
I- (iodide) with concentrated ammonia

A

no reaction

55
Q

reaction of halide
I- (iodide) with lead acetate paper

A

white→brown
I- is a strong enough reducing agent to reduce H2SO4 (OS sulfur=+6) to H2S (OS sulfur=-2)

56
Q

reaction of halide
I- (iodide) with acidified dichromate

A

yellow → white
I- is a strong enough reducing agent to reduce H2SO4 (OS sulfur=+6) to SO2 (OS sulfur=+4)

57
Q

write the 3 reactions iodide has to reduce the sulfur. initially start with NaI and H2SO4

A

NaI + H2SO4→ NaHSO4 + HI
2HI + H2SO4→SO2 + 2H2O + I2
6HI + SO2→H2S + 2H2O + 3I2

58
Q

change in OS of sulfur when reacted with each halide salt

A

Cl- doesn’t reduce H2SO4
Br- reduces H2SO4 to SO2 (+6→+4)
I- reduces H2SO4 to SO2 and then to H2S (+6→+4→-2)

59
Q

describe the test for halide ions

A

add sample to a test tube, add 3 drops dilute nitric acid, add 3 drops silver nitrate (get rid of carbonates) let mixture stand, should see an initial colour change.
Cl-=white
Br-=cream
I-=yellow
to help distinguish between these colours add ammonia
Cl-= dissolves dilute and conc
Br-=dissolves conc
I-=no reaction

60
Q

testing for halogens
reaction of chlorine with bromide

A

cream

61
Q

testing for halogens
reaction of chlorine with iodide

A

yellow/gold

62
Q

testing for halogens
reaction of chlorine with hexane

A

colourless

63
Q

testing for halogens
reaction of bromine with chloride

A

no change

64
Q

testing for halogens
reaction of bromine with iodide

A

red

65
Q

testing for halogens
reaction of bromine with hexane

A

orange

66
Q

testing for halogens
reaction of iodine with chloride

A

no change

67
Q

testing for halogens
reaction of iodine with bromide

A

no change

68
Q

testing for halogens
reaction of iodine with hexane

A

brown with a purple layer

69
Q

disproportionation definition

A

same element/species is reduced and oxidised at the same time

70
Q

chlorine reaction with cold and dilute NaOH produces

A

sodium chlorate NaClO
sodium chloride
water

71
Q

balanced equation of chlorine with cold and dilute NaOH

A

Cl2 (aq) + 2NaOH (aq) → NaClO (aq) + NaCl (aq) + H2O(l)

72
Q

what is the change in oxidation state of chlorine in the reaction with cold and dilute NaOH
Cl2 (aq) + 2NaOH (aq) → NaClO (aq) + NaCl (aq) + H2O(l)

A

0 in Cl2
+1 in NaClO
-1 in NaCl

73
Q

which product of chlorine with cold and dilute NaOH is an oxidising agent

A

sodium chlorate (i)

74
Q

chlorine reaction with hot and dilute NaOH equation

A

3Cl2(g) + 6NaOH(aq)→ NaClO3(aq) + 5NaCl(aq) + 3H2O (l)

75
Q

what are the products from the reaction of chlorine with hot and dilute NaOH

A

sodium chlorate (v)
sodium chloride
water

76
Q

what reaction is this:
3Cl2(g) + 6NaOH(aq)→ NaClO3(aq) + 5NaCl(aq) + 3H2O (l)

A

reaction of chlorine with hot and dilute NaOH to produce sodium chlorate (v) and sodium chloride and water

77
Q

write the equation of the reaction between chlorine and sunlight/water

A

2Cl2(g) + 2H2O(l)→4HCl(aq)+O2(g)

78
Q

what reaction is this:
2Cl2(g) + 2H2O(l)→4HCl(aq)+O2(g)

A

reaction between chlorine and sunlight/water

79
Q

ionic equation for reaction of chlorine (chloric acid) with water

A

HClO(aq)+H2O(l) ⇌ H+(aq) + ClO- (aq)

80
Q

what happens during the reaction of chlorine (chloric acid) and water

A

chloric acid dissociates H+ and ClO-

81
Q

what product of chlorin (chloric acid) with water is a strong reducing ion

A

ClO (kills algae and bacteria)

chemistry (7 decks)

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