tests Flashcards
conditions needed for reaction of hydration of cyclohexane
high temperature and a nickle or platinum catalyst
condition for Benzene and chlorine addition reaction
bright sunlight to be effective
what does benzene and chlorine give
hexachlorocyclohexand C6H6Cl6
copper (II) [Cu(H2O)6]2+ and HCl colour change
from light blue to green
copper (II) [Cu(H2O)6]2+ and ammonia colour change
from light blue to dark blue
iron is used as a catalyst in what reaction
in the harbour process, to produce ammonia from hydrogen and nitrogen
Nickle is used as a catalyst in what reaction
in the hydration of vegetable iols to form margarine
Platinum is used as a catalysts in what reaction
The oxidation of ammonia to form nitric acid
Vanadium Oxide , V2O5 is used as a catalyst in what reaction
The contact process for he production of sulfuric acid
Manganeses dioxde MnO2 is used as a catalysts for what reaction
The catalytic decompostion of hyrgoen peroxide
What is seen in the decomposition of hydrogen peroxide
white fumes
what is formed when weak basic ammonia gas mixes with strong acidic HCl gas
Acidic salt of ammonia chloride is formed and blue fumes released
How to make Fehlings reagent
Mixing together copper(II) sulfate and potassium sodium tartate and then make the solution alkali with sodium hydroxide
what is the test that usees Fehling’s reagent
Reagent is deep blue, if aldehyde is added and warmed colour changes to orange-red
how to make Brady’s reagent
dissolving 2,4,dinitrophenyhydrazaine in acid
Test that uses Brady’s reagent
test for aldehydes and ketones
Mixing Brady’s reagent with a aldehyde or ketone produces an orange-red solid
indentification of methyl carbonyl group (CH3C=O) or CH3CH(OH) in a molecule
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
Formation of carboxylic acids by oxidation of alcohold and aldehydes
colour change and oxidising agent
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
testing phenol using aquous bromine
add bromine drop by drop to phenol solution
Bromine is decolorised then with more bromine added a white precipitate is formed
reaction of phenol with bromine
formes 2,4,6,tribromophenol and HBr
white precipitate of 2,4,6,tribromophenol
Bromine is decoorised
Its the main test for phenol
Phenol and Iron(III)Chloride
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
Iron(III) chloride and carboxylic acid
Red/Brown colour or precipitate formed
How to make Tollen’s reagent
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
Test using Tollen’s reagent
Positive rest (that it is a aldyhyde) a silver mirror will coat the inside of the tube, ketone will not react this way
name two ways to form alcohols
- Halogenoalkalnes by a substitution reaction
- By reducing aldehydes, ketones or carboxlyic acids
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
conditions for the reaction of alcohols with HBr
Br displaceses the OH and water s also formed
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
alcohol and ehtanol together make…
and what will be seen
ester
misty fumes will be seen
alcohol and a carboxylic acid make
ester and water
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
formation of nitrobenzen using sulfuric acid of nitric acid
Nitrobenzen is a yello liquid redced to phenylamine, C6H5NH2 by using tin metal and HCl
Benzene and bromine
Need Iron filings asa catalyst in order to react
Chlorination of Benzene
Anyhdrous aluminium chloride (AlCl3) or iron(III) chlorides used as catalyst
Excess Cl2 produces both products
Chloroalkane and sodium hydroxide
React on heating under reflux
zin placed into sopper sulfate solution
zinc rapidly changes from silvery sulfate to brwon as copper metal covers the zinc
(titrattion) acidified potassium manganate(VII) ions with iron(II) ions.
colour change to pale pink
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
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)
SIlicon chloride (SiCl4) and water
reacts very quickly, produces fumes of HCl gas and SiO2 as a solid precipitate
lead compounds(II) in water (solubility)
most which are insoluble in cold water can be dissolved in hot water
REAction of solutions of Pb2+ ions in water
most insoluble ini water , other than Pb(NO3)2 and Pb(CH3COOH)
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
reaction of Pb2+ ions with HCl
A dense white precipitate of lead chloride PbCl2 is formed
reaction of Pb2+ ions with KI
A dense bright yellow precipitate of lead ioidie PBI2 is formed,
Key observation for Pb2+ ions
Bubble chlorine gas in solution contatining bromine ions
Solution turns orange (formation of Br2)
Addition of sulfuric acid to sodium chloride
Steady fumes of HCl observed
addition of sulfuric acid to sodium bromide
steady fumes of HBr
HBr oxidises —> brwon fumes of Br2 and So2 gas
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
colour of [Fe(H2O)6]2+ Complex
pale green
colour of [Fe(H2O)6]3+ complex
yellow
colour of [Cu(H2O)6]3+ complex
blue
colour of [Cr(H2O)6]3+ Complex
Dark green
coloud of [Co(H2O)6]2+ complex
pink
colour of [CuCl4]2- compllex
yellow or green
colour of [COCl4]2- complex
blue
colour of CO2+ in absence of water
blue
colour of MnO4-
dark purple
Colour of Cr2O7 2-
orange
colour of CrO4 2-
yellow
copper (II) ions reacting with concentrated HCl
pale blue to yellow/green
addition of ammonia turns solution royal blue
cobalt(II) ions reacting with concentrated HCl
pink to blue
addition of MnO2 to hydrogen peroxide
catalyst for decomposition, white fumes/gas seen
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-
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
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
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
Magnesium ribbon burnt in air
bright flame and some white ash
zinc powder added to copper(II)sulfate
red-brown deposit is formed on the zinc
solution of sodium hydroxide added toa solution of magnesium chloride
white precipitate formed of magnesium hydroxide
solution of sodium sulfate is added to a solution of barium chloride
white precipitate formed of barium sulfate
group 1 /2 salts in water
no precipitate, all salt of group 1 and group 2 are soluble
gropu1 metals reacting in water
all react vigorosly, reactivity increases down the group
group1/2 elements with acid
forms salt (react vigorously)
s block elements reacting with oxygen
all react + brun in air, caesium inflames spontaneously
lithium flame test
red
sodium flame test
strong orange
potassium flame test
lilac(pink)
rubidium flame test
red(redish-violet)
Caesium flame test
blue-violet
Calcium flmae test
orange-red
Strontium flame test
red
Barium flame test
pale green
copper flame test
blue-green(often with white flashes)
lead flame test
greyish-white
reaction of iodine wiht potassium bromide
no reaction
chlorine and aquoes sodium bromide reaction
brimide is liberated
Test for sulfate ions
Barium chloride and sulfate ions in water
Barium sulfate insoluble in water and will be seen as a white precpitate
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
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
copper(II) oxide added to dilute sulfuric acid
solution turns blue (might need heating to t react)
copper(II) carbonate added to dilute sulfuric acid
fizzing seen (carbon dioxide being released)
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
addition of concentrated HCl to solution of Dissolved hydrated copper(II) sulfate crytals in water
solution turnes from pale blue to yellow-green
increased pressure of NO2 gas
increases N2O4 turning gas from brown to colourless
acid and base/alkalie makes
salt and water
acid and a carbonate makes
salt, water, and carbon dioxide
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
rate of reaction colud prac
thiosulfate inos in acid solution forms sulfur making solution cloudy
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
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
test for primary and secoundary alcohols
addition of potassium dichromate
if primay or secoundary alcohol present, colour change form orange to green
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
carboxylic acid and alcohol
produces ester which has a sweet smell
