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Alevel > topic 4 > Flashcards

topic 4 Flashcards

1
Q

flame test procedure

A

place nichrome wire in conc HCL
place wire in roaring bunsen flame
place wire in sample then back into flame
observe colour

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2
Q

Li+

A

bright red

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3
Q

Na +

A

bright yellow

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4
Q

k+

A

lilac

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5
Q

Be 2+

A

no colour

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6
Q

mg2+

A

colourless

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7
Q

ca 2+

A

brick red

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8
Q

sr 2+

A

bright red

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9
Q

ba 2+

A

pale green

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10
Q

what could cause yello contamination

A

Na + presence

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11
Q

what causes colour

A

e excited to higher energy level

e relaxes back to lower energy level, emitting photon of light whose energy is equal to the energy difference between the shells e has moved from

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12
Q

thermal decomposition

A

breaking down using heat = lot of energy required to break strong bond between atoms

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13
Q

group 1 hydroxide solubility

A

soluble

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14
Q

group 1 sulfate solubility

A

soluble

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15
Q

group 1 nitrate solubility

A

soluble

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16
Q

group 1 carbonate solubility

A

soluble

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17
Q

group 2 hydroxide solubility

A

solubility increases down group

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18
Q

group 2 sulfate solubility

A

solubility decreases down group

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19
Q

group 2 nitrate solubility

A

soluble

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20
Q

group 2 carbonate solubility

A

insoluble

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21
Q

which chloride aren’t soluble

A

silver and lead chloride

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22
Q

which sulfates arent soluble

A

barium and lead sulfates

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23
Q

reactivity trend in group 2

A

reactivity increases down group

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24
Q

barium plus water observation

A

lots of bubbles

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25
Q

Mg plus water observation

A

nothing much occurs

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26
Q

calcium oxide plus water

A

CaO plus H2O —–> Ca(OH)2

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27
Q

why dont BeO and MgO react with water well

A

BeO is insoluble and

MgO isnt very soluble

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28
Q

Group 1 nitrates decomposition

A

partially decompose to form metal nitrate plus oxygen

exception lithium undergoes complete decomposition to form lithium oxide (white solid), NO2 (red brown gas) and oxygen

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29
Q

group1 carbonates decomposition

A

do not decompose

except lithium carbonate to give lithium oxide plus CO2

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30
Q

group 2 nitrates

A

all nitrates fully decompose to form metal oxide, NO2 and oxygen

becomes harder to decompose down group = more thermally stable

31
Q

group 2 carbonates

A

decompose to form metal oxide and CO2

32
Q

measuring rates of decomposition

A

change in mass

colorimetry

gas formation

33
Q

positives and negatives of change in mass

A

+ = accuate measurements, mass balance to 2 d.p

  • = non continuous measurement and toxic no2 produced, skin eye burns, fatal if inhaled
34
Q

positives and negatives of colorimetry

A

+ = continous monitoring

  • = product is involved in furhter reaction (2NO2 —-> N2O4)
35
Q

positives and negatives of gas formation

A

+ = continous monitoring, toxic No2 captured

  • = potential for NaOH solution to be drawn back into test tube after heating = pressure difference so glass could break
36
Q

comparing MgCO3 and SrCO3 decomposition

A

Mg 2+ has higher charge density than sr2+

Mg 2+ strongly polarises the carbonate ion more than the sr2+

so the Mg- O bond is strengthened results in the C- O bond weakening

less energy required to break C- O bond so less energy to decompose MgCO3

37
Q

group 7 MP trend and why

A

increases down group due to increased london forces as the molecules get larger

38
Q

group 7 electronegativity trend and why

A

decrease as you go down the group due to increased shielding and atomic radius so weaker attraction to bonded electrons

39
Q

Fluorine

A

pale yellow gas

40
Q

chlorine

A

pale green gas

41
Q

bromine

A

brown/red liquid

42
Q

iodine

A

grey solid

violet vapour

43
Q

astatine

A

black solid

44
Q

colour of chlorine dissolved in water

A

pale green

45
Q

colour of bromine dissolved in water

A

orange

46
Q

colour of iodine dissolved in water

A

brown

47
Q

colour of chlorine dissolved in organic solvent

A

pale green

48
Q

colour of bromine dissolved in organic solvent

A

orange

49
Q

colour of iodine dissolved in organic solvent

A

purple

50
Q

Cl2 plus Br- —->? colour change

A

orange solution produced

51
Q

Cl2 plus I- —->?

colour change

A

brown solution produced

52
Q

Br2 plus I- ——>?

colour change

A

brown solution produced

53
Q

oxidising agent strength trend group 7

A

decreases down group

chlorine strongest oxidising agent as it has smallest atomic radius and less shielding so able to attract incoming e more easily

54
Q

reducing agent strength (donates e) trend

A

reducing agent strength increases down group as atomic radius get larger and increased shielding means there’s less attraction between valence e and nucleus so electrons lost more easily

55
Q

test for halides procedure and results

A

dissolve sample
add nitric acid to remove carbonates
add silver nitrate (silver complex ions)

cl- white ppt
br- cream ppt
I- yellow ppt

56
Q

how to test ppt from above

A

AgCl dissolves in dilute and conc NH3

AgBr dissolves in conc NH3 but not in Dilute NH3

AgI doesn’t dissolve in either dilute or conc NH3

57
Q

chlorine plus water

A

Cl2 (g) + H2O —-> HClO (aq) + HCl (aq)

58
Q

chlorine plus cold KOH

A

Cl2 (g) + 2KOH (aq) ——> KClO (aq) + KCl (aq) +H2O

59
Q

chlorine plus hot KOH

A

3Cl2 (g) + 6KOH (aq) ——> KClO3 (aq) + 5KCl +5H20

60
Q

HBr + NH3 —–>

A

HBr + NH3 —–> NH4Br

61
Q

HBr +H20 —–>

A

HBr +H20 —–> H3O+ + Br-

62
Q

metal plus halogen procedure

A

in fume hood so cl2 doesnt escape
iron is in wool not in blocks to increase surface area
iron heated to increase rate of reaction
halogen vapour is dry otherwise cl2 reacts with H20 to form acidic gas
excess gas allowed to escape so no pressure build up

63
Q

does iodine with fe2+ ion

A

no bc iodine isnt strong enough oxidisng agent

64
Q

Cl2 + H2 —–>

A

Cl2 + H2 —–> 2HCl violent reaction

65
Q

Br2 plus H2

A

creates HBr react with calm pale blue flame

66
Q

iodine plus hydrogen

A

produces HI and reaction is reversible

67
Q

H2SO4 + NaBr —–>

A

H2SO4 + NaBr —–> Br2 (g) + SO2 (g) + H2O (g)

br2 is orange and so2 is acidic choking

68
Q

H2SO4 + NaI —->

A

H2SO4 + 6NaI —-> 3 I2(s) + 2 H2O (s) + H2S(g) +NaHSO4

i2 is grey solid
s is yellow solid and H2s has egg smell

69
Q

H2SO4 + NaCl —->

A

H2SO4 + NaCl —-> HCl + NaHSO4

70
Q

test for carbonate ions

A

disslove carbonate
add hcl to solution
bubble gas through limewater
if carbonate present - limewater turns cloudy

71
Q

equation for test carbonate

A

CO3- + H+ ——-> H20 + C02

72
Q

test for sulphate ions

A

disslove compound and add dilute HCl to remove carbonate ions
add few drops of barium chloride
if sulphate ion present - white ppt of barium sulfate forms

73
Q

equation for testing of sulphate ions

A

SO42- + Ba2+ —-> BaSO4(s)

74
Q

testing for NH4+ ions

A

dissolve NH4+
add dilute NaOH
heat gently
IF ion present damp red litmus paper turns blue

Alevel (30 decks)

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