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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
name two ways to form alcohols
- Halogenoalkalnes by a substitution reaction | - By reducing aldehydes, ketones or carboxlyic acids
26
conditions for the reaction of alcohols with hydrogen chloride
Chlorination--> pass HCl gas into the alcohol in present of a zinc chloride as a catalyst Heat
27
conditions for the reaction of alcohols with HBr
Br displaceses the OH and water s also formed
28
conditions fo the reaction of alcohol with HI
warm damp red phospharus and iodine together to form PI3 then the reaction below; 3CH3CH2OH + PI3 --> 3CH3CH2I + H3PO3
29
alcohol and ehtanol together make... and what will be seen
ester misty fumes will be seen
30
alcohol and a carboxylic acid make
ester and water
31
test to distinguish between simple aliphatic acids (e.g.ethanoic acid) and phenol
addition of sodium carbonate solutio. Ethanoic acid will react to give bubbles of carbon dioxide but phenol will not
32
formation of nitrobenzen using sulfuric acid of nitric acid
Nitrobenzen is a yello liquid redced to phenylamine, C6H5NH2 by using tin metal and HCl
33
Benzene and bromine
Need Iron filings asa catalyst in order to react
34
Chlorination of Benzene
Anyhdrous aluminium chloride (AlCl3) or iron(III) chlorides used as catalyst Excess Cl2 produces both products
35
Chloroalkane and sodium hydroxide
React on heating under reflux
36
zin placed into sopper sulfate solution
zinc rapidly changes from silvery sulfate to brwon as copper metal covers the zinc
37
(titrattion) acidified potassium manganate(VII) ions with iron(II) ions.
colour change to pale pink
38
potassium dichromate(VII) in acid solution
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
39
addition of colourless solution containg iodine ions to a blue solution contatining copper (II)
Fomration of a cloudy brown solution, addition of starch indicator (flesh coloured mixture)
40
SIlicon chloride (SiCl4) and water
reacts very quickly, produces fumes of HCl gas and SiO2 as a solid precipitate
41
lead compounds(II) in water (solubility)
most which are insoluble in cold water can be dissolved in hot water
42
REAction of solutions of Pb2+ ions in water
most insoluble ini water , other than Pb(NO3)2 and Pb(CH3COOH)
43
Pb2+ ions with NaOH reactions
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
reaction of Pb2+ ions with HCl
A dense white precipitate of lead chloride PbCl2 is formed
45
reaction of Pb2+ ions with KI
A dense bright yellow precipitate of lead ioidie PBI2 is formed, Key observation for Pb2+ ions
46
Bubble chlorine gas in solution contatining bromine ions
Solution turns orange (formation of Br2)
47
Addition of sulfuric acid to sodium chloride
Steady fumes of HCl observed
48
addition of sulfuric acid to sodium bromide
steady fumes of HBr | HBr oxidises ---> brwon fumes of Br2 and So2 gas
49
Addition of sulfuric acid to sodium iodine
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
colour of [Fe(H2O)6]2+ Complex
pale green
51
colour of [Fe(H2O)6]3+ complex
yellow
52
colour of [Cu(H2O)6]3+ complex
blue
53
colour of [Cr(H2O)6]3+ Complex
Dark green
54
coloud of [Co(H2O)6]2+ complex
pink
55
colour of [CuCl4]2- compllex
yellow or green
56
colour of [COCl4]2- complex
blue
57
colour of CO2+ in absence of water
blue
58
colour of MnO4-
dark purple
59
Colour of Cr2O7 2-
orange
60
colour of CrO4 2-
yellow
61
copper (II) ions reacting with concentrated HCl
pale blue to yellow/green addition of ammonia turns solution royal blue
62
cobalt(II) ions reacting with concentrated HCl
pink to blue
63
addition of MnO2 to hydrogen peroxide
catalyst for decomposition, white fumes/gas seen
64
ADdition of sodium hydroxide to solution contatining a [Cr(H2O)6]3+ complex
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
ADdition of sodium hydroxide to solution contatining a [Fe(H2O)6]2+ complex
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
ADdition of sodium hydroxide to solution contatining a [Fe(H2O)6]3+ complex
some OH; red-brown precipiatate of [Fe(H2O)3(OH)3] | excess OH; no further reaction
67
ADdition of sodium hydroxide to solution contatining a [Cu(H2O)6]2+ complex
some OH; pale blue precipitate of [Cu(H2O)4(OH)2] | excess OH; no further reaction
68
Magnesium ribbon burnt in air
bright flame and some white ash
69
zinc powder added to copper(II)sulfate
red-brown deposit is formed on the zinc
70
solution of sodium hydroxide added toa solution of magnesium chloride
white precipitate formed of magnesium hydroxide
71
solution of sodium sulfate is added to a solution of barium chloride
white precipitate formed of barium sulfate
72
group 1 /2 salts in water
no precipitate, all salt of group 1 and group 2 are soluble
73
gropu1 metals reacting in water
all react vigorosly, reactivity increases down the group
74
group1/2 elements with acid
forms salt (react vigorously)
75
s block elements reacting with oxygen
all react + brun in air, caesium inflames spontaneously
76
lithium flame test
red
77
sodium flame test
strong orange
78
potassium flame test
lilac(pink)
79
rubidium flame test
red(redish-violet)
80
Caesium flame test
blue-violet
81
Calcium flmae test
orange-red
82
Strontium flame test
red
83
Barium flame test
pale green
84
copper flame test
blue-green(often with white flashes)
85
lead flame test
greyish-white
86
reaction of iodine wiht potassium bromide
no reaction
87
chlorine and aquoes sodium bromide reaction
brimide is liberated
88
Test for sulfate ions
Barium chloride and sulfate ions in water Barium sulfate insoluble in water and will be seen as a white precpitate
89
test for halide ions
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
TEsting for carbonate ions
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
copper(II) oxide added to dilute sulfuric acid
solution turns blue (might need heating to t react)
92
copper(II) carbonate added to dilute sulfuric acid
fizzing seen (carbon dioxide being released)
93
heating of copper(II) sulfate
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
addition of concentrated HCl to solution of Dissolved hydrated copper(II) sulfate crytals in water
solution turnes from pale blue to yellow-green
95
increased pressure of NO2 gas
increases N2O4 turning gas from brown to colourless
96
acid and base/alkalie makes
salt and water
97
acid and a carbonate makes
salt, water, and carbon dioxide
98
iodine clock
idodine and starch gives a strong coloured blue complex. addition of thiosulfate ions( which rapidly react with iodine) no blue colour will appear
99
rate of reaction colud prac
thiosulfate inos in acid solution forms sulfur making solution cloudy
100
test for alkene
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
test for halogenoalkanes
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
test for primary and secoundary alcohols
addition of potassium dichromate if primay or secoundary alcohol present, colour change form orange to green
103
reaction of copper(II) oxide and methanoic acid
when warmed, black solid of opper(II) oxide dissolvs to form a blue solution of the salt
104
carboxylic acid and alcohol
produces ester which has a sweet smell

chemistry tests and indicators (2 decks)

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