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1
Q

conditions needed for reaction of hydration of cyclohexane

A

high temperature and a nickle or platinum catalyst

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2
Q

condition for Benzene and chlorine addition reaction

A

bright sunlight to be effective

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3
Q

what does benzene and chlorine give

A

hexachlorocyclohexand C6H6Cl6

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4
Q

copper (II) [Cu(H2O)6]2+ and HCl colour change

A

from light blue to green

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5
Q

copper (II) [Cu(H2O)6]2+ and ammonia colour change

A

from light blue to dark blue

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6
Q

iron is used as a catalyst in what reaction

A

in the harbour process, to produce ammonia from hydrogen and nitrogen

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7
Q

Nickle is used as a catalyst in what reaction

A

in the hydration of vegetable iols to form margarine

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8
Q

Platinum is used as a catalysts in what reaction

A

The oxidation of ammonia to form nitric acid

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9
Q

Vanadium Oxide , V2O5 is used as a catalyst in what reaction

A

The contact process for he production of sulfuric acid

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10
Q

Manganeses dioxde MnO2 is used as a catalysts for what reaction

A

The catalytic decompostion of hyrgoen peroxide

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11
Q

What is seen in the decomposition of hydrogen peroxide

A

white fumes

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12
Q

what is formed when weak basic ammonia gas mixes with strong acidic HCl gas

A

Acidic salt of ammonia chloride is formed and blue fumes released

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13
Q

How to make Fehlings reagent

A

Mixing together copper(II) sulfate and potassium sodium tartate and then make the solution alkali with sodium hydroxide

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14
Q

what is the test that usees Fehling’s reagent

A

Reagent is deep blue, if aldehyde is added and warmed colour changes to orange-red

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15
Q

how to make Brady’s reagent

A

dissolving 2,4,dinitrophenyhydrazaine in acid

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16
Q

Test that uses Brady’s reagent

A

test for aldehydes and ketones

Mixing Brady’s reagent with a aldehyde or ketone produces an orange-red solid

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17
Q

indentification of methyl carbonyl group (CH3C=O) or CH3CH(OH) in a molecule

A

organic compound is warmed wth a colourless solution of iodine in NaOH or potassium iodidde and NaOCl
[(I2/NaOH) or (I-/OCl-)]
Triidomethane (iodoform) , CHI3 is formed, yellow solid

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18
Q

Formation of carboxylic acids by oxidation of alcohold and aldehydes
colour change and oxidising agent

A

Acidified potassium dichromate can be used as the oxidising agengent;
orange Cr2O7 2- —> green Cr3+

Or

Alkaline potassium dichromate can be used
purple MnO4 - —> black/brown sludge of manganate (IV) oxide

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19
Q

testing phenol using aquous bromine

A

add bromine drop by drop to phenol solution

Bromine is decolorised then with more bromine added a white precipitate is formed

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20
Q

reaction of phenol with bromine

A

formes 2,4,6,tribromophenol and HBr
white precipitate of 2,4,6,tribromophenol
Bromine is decoorised

Its the main test for phenol

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21
Q

Phenol and Iron(III)Chloride

A

purple colour in aquous solution
any ocmpound with -OH bonded directly to a benzene ring will give a brightly coloured complex generally purple,green or blue

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22
Q

Iron(III) chloride and carboxylic acid

A

Red/Brown colour or precipitate formed

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23
Q

How to make Tollen’s reagent

A

Adding aquous NaOH to silver nitrate solution untill a brown precipitate of silver(I)oxide just redissolves. ALdyhyde’s then added and then is gentally warmed

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24
Q

Test using Tollen’s reagent

A

Positive rest (that it is a aldyhyde) a silver mirror will coat the inside of the tube, ketone will not react this way

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25
Q

name two ways to form alcohols

A
  • Halogenoalkalnes by a substitution reaction

- By reducing aldehydes, ketones or carboxlyic acids

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26
Q

conditions for the reaction of alcohols with hydrogen chloride

A

Chlorination–> pass HCl gas into the alcohol in present of a zinc chloride as a catalyst

Heat

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27
Q

conditions for the reaction of alcohols with HBr

A

Br displaceses the OH and water s also formed

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28
Q

conditions fo the reaction of alcohol with HI

A

warm damp red phospharus and iodine together to form PI3 then the reaction below;

3CH3CH2OH + PI3 –> 3CH3CH2I + H3PO3

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29
Q

alcohol and ehtanol together make…

and what will be seen

A

ester

misty fumes will be seen

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30
Q

alcohol and a carboxylic acid make

A

ester and water

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31
Q

test to distinguish between simple aliphatic acids (e.g.ethanoic acid) and phenol

A

addition of sodium carbonate solutio. Ethanoic acid will react to give bubbles of carbon dioxide but phenol will not

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32
Q

formation of nitrobenzen using sulfuric acid of nitric acid

A

Nitrobenzen is a yello liquid redced to phenylamine, C6H5NH2 by using tin metal and HCl

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33
Q

Benzene and bromine

A

Need Iron filings asa catalyst in order to react

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34
Q

Chlorination of Benzene

A

Anyhdrous aluminium chloride (AlCl3) or iron(III) chlorides used as catalyst

Excess Cl2 produces both products

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35
Q

Chloroalkane and sodium hydroxide

A

React on heating under reflux

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36
Q

zin placed into sopper sulfate solution

A

zinc rapidly changes from silvery sulfate to brwon as copper metal covers the zinc

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37
Q

(titrattion) acidified potassium manganate(VII) ions with iron(II) ions.

A

colour change to pale pink

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38
Q

potassium dichromate(VII) in acid solution

A

will oxideise Fe2+ and Fe3+
colour change from dark orange to green
Cr2O72- + 14H+ +6e- –> 2Cr3+ + 7H2O
orange ——————> green

CrO72- +H2O 2CrO4 2- + 2H+
DArk orange ———yellow

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39
Q

addition of colourless solution containg iodine ions to a blue solution contatining copper (II)

A

Fomration of a cloudy brown solution, addition of starch indicator (flesh coloured mixture)

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40
Q

SIlicon chloride (SiCl4) and water

A

reacts very quickly, produces fumes of HCl gas and SiO2 as a solid precipitate

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41
Q

lead compounds(II) in water (solubility)

A

most which are insoluble in cold water can be dissolved in hot water

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42
Q

REAction of solutions of Pb2+ ions in water

A

most insoluble ini water , other than Pb(NO3)2 and Pb(CH3COOH)

43
Q

Pb2+ ions with NaOH reactions

A

anitial white precipitate of Pb(OH)2 is formed

excess -OH = the white precipitate redissolves in excess OH- ions to form the tetrahydroxoplumbate(II) ion

44
Q

reaction of Pb2+ ions with HCl

A

A dense white precipitate of lead chloride PbCl2 is formed

45
Q

reaction of Pb2+ ions with KI

A

A dense bright yellow precipitate of lead ioidie PBI2 is formed,
Key observation for Pb2+ ions

46
Q

Bubble chlorine gas in solution contatining bromine ions

A

Solution turns orange (formation of Br2)

47
Q

Addition of sulfuric acid to sodium chloride

A

Steady fumes of HCl observed

48
Q

addition of sulfuric acid to sodium bromide

A

steady fumes of HBr

HBr oxidises —> brwon fumes of Br2 and So2 gas

49
Q

Addition of sulfuric acid to sodium iodine

A

intially produces HI gas

sulfurica acid oxidises HI

Steamy fumes of HI, purple fumes of I2 or black solid/Brown solution
smell of rotten eggs(H2S), yellow solid

50
Q

colour of [Fe(H2O)6]2+ Complex

A

pale green

51
Q

colour of [Fe(H2O)6]3+ complex

A

yellow

52
Q

colour of [Cu(H2O)6]3+ complex

A

blue

53
Q

colour of [Cr(H2O)6]3+ Complex

A

Dark green

54
Q

coloud of [Co(H2O)6]2+ complex

A

pink

55
Q

colour of [CuCl4]2- compllex

A

yellow or green

56
Q

colour of [COCl4]2- complex

A

blue

57
Q

colour of CO2+ in absence of water

A

blue

58
Q

colour of MnO4-

A

dark purple

59
Q

Colour of Cr2O7 2-

A

orange

60
Q

colour of CrO4 2-

A

yellow

61
Q

copper (II) ions reacting with concentrated HCl

A

pale blue to yellow/green

addition of ammonia turns solution royal blue

62
Q

cobalt(II) ions reacting with concentrated HCl

A

pink to blue

63
Q

addition of MnO2 to hydrogen peroxide

A

catalyst for decomposition, white fumes/gas seen

64
Q

ADdition of sodium hydroxide to solution contatining a [Cr(H2O)6]3+ complex

A

with some OH- ions; grey-green precipitate of [Cr(H2O)3(OH3)]
with excess OH-ions ; precipitate dissolves giving a deep green solution of [Cr(OH)6]3-

65
Q

ADdition of sodium hydroxide to solution contatining a [Fe(H2O)6]2+ complex

A

some OH; dark green precipitate of [Fe(H2O)4(OH)2]

excess OH; no further reaction for bulk, some red-brown colour seen at the suraface due to oxidation by the air

66
Q

ADdition of sodium hydroxide to solution contatining a [Fe(H2O)6]3+ complex

A

some OH; red-brown precipiatate of [Fe(H2O)3(OH)3]

excess OH; no further reaction

67
Q

ADdition of sodium hydroxide to solution contatining a [Cu(H2O)6]2+ complex

A

some OH; pale blue precipitate of [Cu(H2O)4(OH)2]

excess OH; no further reaction

68
Q

Magnesium ribbon burnt in air

A

bright flame and some white ash

69
Q

zinc powder added to copper(II)sulfate

A

red-brown deposit is formed on the zinc

70
Q

solution of sodium hydroxide added toa solution of magnesium chloride

A

white precipitate formed of magnesium hydroxide

71
Q

solution of sodium sulfate is added to a solution of barium chloride

A

white precipitate formed of barium sulfate

72
Q

group 1 /2 salts in water

A

no precipitate, all salt of group 1 and group 2 are soluble

73
Q

gropu1 metals reacting in water

A

all react vigorosly, reactivity increases down the group

74
Q

group1/2 elements with acid

A

forms salt (react vigorously)

75
Q

s block elements reacting with oxygen

A

all react + brun in air, caesium inflames spontaneously

76
Q

lithium flame test

A

red

77
Q

sodium flame test

A

strong orange

78
Q

potassium flame test

A

lilac(pink)

79
Q

rubidium flame test

A

red(redish-violet)

80
Q

Caesium flame test

A

blue-violet

81
Q

Calcium flmae test

A

orange-red

82
Q

Strontium flame test

A

red

83
Q

Barium flame test

A

pale green

84
Q

copper flame test

A

blue-green(often with white flashes)

85
Q

lead flame test

A

greyish-white

86
Q

reaction of iodine wiht potassium bromide

A

no reaction

87
Q

chlorine and aquoes sodium bromide reaction

A

brimide is liberated

88
Q

Test for sulfate ions

A

Barium chloride and sulfate ions in water

Barium sulfate insoluble in water and will be seen as a white precpitate

89
Q

test for halide ions

A

silver nitrate solution added to water with halide ions, silver halde precipitated.

silver chloride- white precipitate(dissolves in dilute ammonia)
silver bromide - cream precipitate (dissolves in concentrated ammonia)
silver iodide - pale yellow precipiatate

90
Q

TEsting for carbonate ions

A

acid is added to the testes compound if carbonate ions are present then carbon dioxide gas bubbles off, if this is passed through lime water it turns the lime water from clear to cloude

91
Q

copper(II) oxide added to dilute sulfuric acid

A

solution turns blue (might need heating to t react)

92
Q

copper(II) carbonate added to dilute sulfuric acid

A

fizzing seen (carbon dioxide being released)

93
Q

heating of copper(II) sulfate

A

water of crystallisation is given off as steam, leaving a white powder called anyhydrous copper(II) sulfate

addition of water and the powder gets hot and turns blue

94
Q

addition of concentrated HCl to solution of Dissolved hydrated copper(II) sulfate crytals in water

A

solution turnes from pale blue to yellow-green

95
Q

increased pressure of NO2 gas

A

increases N2O4 turning gas from brown to colourless

96
Q

acid and base/alkalie makes

A

salt and water

97
Q

acid and a carbonate makes

A

salt, water, and carbon dioxide

98
Q

iodine clock

A

idodine and starch gives a strong coloured blue complex. addition of thiosulfate ions( which rapidly react with iodine) no blue colour will appear

99
Q

rate of reaction colud prac

A

thiosulfate inos in acid solution forms sulfur making solution cloudy

100
Q

test for alkene

A

addition of bromine to unkonwn solution

decolorisation of Brommine water (brown) if alkene is present
only works on a alkane in the present of UV light

decolorisation of purple acidified potassium manganate(VII) can also be sed as a test for alkene

101
Q

test for halogenoalkanes

A

aquoues silver nitrate added and then sodium hydroxidde )in excess) and then neutralised with dilute nitric acid

presence of halide ions shown by silver nitrate in the usual way

if nitric acid is not added before silver nitrate, silver hydroxide as a brown precipipiatet will be formed

102
Q

test for primary and secoundary alcohols

A

addition of potassium dichromate

if primay or secoundary alcohol present, colour change form orange to green

103
Q

reaction of copper(II) oxide and methanoic acid

A

when warmed, black solid of opper(II) oxide dissolvs to form a blue solution of the salt

104
Q

carboxylic acid and alcohol

A

produces ester which has a sweet smell

chemistry tests and indicators (2 decks)

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