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Remember me chemistry!!

Name ............................................... class....................teacher................date ..............

1) Catalyst and applications

Applications Catalysts and other conditions 1 Haber Process iron2 Contact Process Vanadium(V) oxide3 Ostwald Process platinum4 Decomposition of hydrogen peroxide Manganese(IV) oxide5 Zinc reacts with sulphuric acid Copper(II) sulphate solution6 Hydrogenation process ( alkene to alkane) Nickel/platinum temp 180 oC7 Esterification Concentrated sulphuric acid8 Addition of hydroxyl group( ethene to

ethandiol)No catalyst . Add Acidified KMnO4

9 Dehydration of ethanol Porcelain chips/alumina10 Hydration of ethene to ethanol Phosphoric acid temp: 300 oC, 60 atm

2) Colour of substances

Salts Oxide metals Metals

All salts are white in colour excepta) Copper(II) sulphate, copper(II)

nitrate, copper(II) chloride – blueb) Copper(II) carbonate – greenc) All iron (II) salts are greend) All iron(III) salts are browne) Lead(II) iodide – yellow precipitatef) Lead(II) chromate- yellow

precipitate g) Potassium chromate- yellow

solution

All oxide metals are white excepta) Copper(II) oxide- blackb) Zinc oxide – yellow (hot) ,

white(cold)c) Lead(II) oxide- brown(hot)

–yellow(cold)d) Iron(II) oxide-greene) Iron(III) oxide- brown

All metals are grey except a) Copper- brownb) Silver- shiny white

3) Solubility of salts

Soluble insoluble

Chlorides All PAH ( Lead(II) chloride, silver chloride, mercury chloride)

Sulphate All PCB ( Lead(II) sulphate, Calcium sulphate, barium sulphate)

carbonates KAN ( Potassium carbonate, ammonium carbonate, sodium carbonate )

ALL

Tests for Anions ( remember method and observation)

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Chloride ion Sulphate ion Nitrate ion Carbonate ion

Tests Add nitric acid , Add silver nitrate solutionWhite precipitate formed

Add nitric acid , Add barium nitrate solutionWhite precipitate formedOR Add hydrochloric acid , Add barium chloride solutionWhite precipitate formed

Add sulphuric acid , Add iron(II) sulphate solutionCarefully add conc sulphuric acid Brown ring formed

Add any dilute acid , Bubbles of gas that turn lime water milky

4) Tests for cations in solutions- ( remember method and observation)

Cations Add sodium hydroxide solution in excess

Add ammonia solution in excess

Confirmatory tests

NH4+

Na+

K+

-No change , but when heated gas turned damp red litmus to red-no change -no change

-no change -no change- no change

-Nessler’s reagent turned to brown precipitate

Ca2+

Mg2+

-white precipitate -white precipitate

-no change -white precipitate

Zn2+

Al3+

Pb2+

-white precipitate soluble in excess- white precipitate soluble in excess- white precipitate soluble in excess

- white precipitate soluble in excess-white precipitate-white precipitate

How to differentiate between aluminium ion and lead(II) ions?Add HCl dilute or add H2SO4 dilute, white precipitate shows Pb2+. No change with Al3+

OR Add KI solution, yellow precipitate soluble in hot solution shows Pb2+ ion, no change with Al3+ ion

Fe2+

Fe3+

Cu2+

-green precipitate -brown precipitate-blue precipitate

-green precipitate -brown precipitate-blue precipitate soluble in excess to form dark blue solution

-Add potassium hexacyanoferrate (III)solution , dark blue solution formed ( to test Fe2+ formed during rusting only)- Add potassium hexacyanoferrate (II)solution , dark blue solution formed - Add potassium thiocyanatesolution , blood red colouration formed

5) Test for gases ( remember method and observation)

Oxygen gas Place a glowing wooden splinter near the gas, glowing splinter relights

Hydrogen gas Place a lighted wooden splinter near the gas, ‘pop’ sound is

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produced

Carbon dioxide gas Bubble the gas through lime water, lime water turns chalky

6) Tests for halogens (remember method and observation)

Chlorine gas, Cl2 Add tetrachlormethane to the solution, shake well, lower layer is pale yellow in colour

OR – place a damp blue litmus paper to the gas (if gas, and not chlorine water!) damp blue litmus paper change to red, then is bleached

Bromine gas gas,Br2

Add tetrachlormethane to the solution, shake well, lower layer is brown in colour

Iodine gas , I2 Add tetrachlormethane to the solution, shake well, lower layer is purple yellow in colour

OR, add starch to iodine , blue black colour is formed.

7) Types of glass

Type of glass properties uses composition

Soda lime glass Cheap, breakable, low melting point, easy to shape

Glass containers, window panes, cheap glassware

Silica and calcium carbonate

Borosilicate glass Expensive, not easy to break, resistant to high heat and chemical reaction

Cooking utensils, laboratory apparatus

Silica and boron oxide and aluminium oxide

Fused glass Expensive, not easy to break, resistant to high heat and chemical reaction

Optical lenses, telescope lenses

Silica and boron oxide

Crystal lead glass

High density and refractive index,

Crystal glass ware, lenses, prisms

Silica and lead oxide

8) Composite materials

Composite material components uses

Reinforced concrete Concrete and steel rods Construct framework for buildings, highways, bridges

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Fibre glass Glass and polyester plastic Racquets, boat, car body

Superconductor Copper oxide, yttrium oxide and barium oxide

Stronger and lighter magnets, computers

Photochromic glass Glass and silver chloride Lenses that go dark in light and becomes clear in dark

Optical fibre Glass of low refractive index and glass of high refractive index

Transmit data in telecommunications

9) Food additives

Types of functions examples

preservatives Slow down growth of microorganisms

Salt, sugar, vinegar( pickled food)

Sodium nitrite/nitrate(burger /sausage)

Sodium benzoate/acid benzoic(tomato sauce, chilli sauce,)

antioxidants To prevent oxidation that cause fruit browning and oil or fat to go rancid

Ascorbic acid/ vitamin c ( fruit juice)

Vitamin E/ BHA/BHT( oils and margarine)

Stabilisers Pevent emulsion from separated Lecithin (chocolate), ice cream, butter

Thickening agents To thicken food Acacia gum ( jelly)

Gelatine, pectin, starch and gum

Dyes To add or restore colour Azo compounds, tartrazine

flavourings To improve taste of food MSG, Aspartarme

10) Traditional medicine

example Aloe vera Mint ginseng ginger garlic

uses Burns,intestinal disorder

Cough, aids in digestion

Anti-stress, boost immune system

Indigestion, morning sickness

Lower cholesterol, lower blood pressure

Types Examples uses Side effects

Analgesics

(reduce pain or fever)

aspirin Reduce oain and fever- prevents blood clot

Stomach ulcer

paracetamol Reduce oain and fever- Damage liver

codeine Reduce oain and fever – reduce cough

addiction

Antibiotics

( reduce bacteria infection)

penicillin Treat bacteria infection - gonorrhoea

Allergic reaction

streptomycin Treat bacteria infection - Tuberculosis

Allergic reaction

Psychotherapeutic Stimulant (caffeine) Stimulate brain Sleep disorder

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drug

(treat mental illness)

Antidepressant

(tranquilisers and barbiturate)

Relieves anxiety drowziness

Antipsychotic ( clozapine and haloperidol)

Treat schizophrenia addiction

REDOX

Oxidising agent Colour change Reducing agent Colour change

Acidified potassium manganate(VII) Purple solution to colourless

Iodide ion

(potassium iodide)

Bromide ion

( potassium bromide)

Colourless to brown solution ( purple in CCl4)

Colourless to brown solution (brown in CCl4)

Acidified potassium dichromate(VI) Orange solution to green Iron(II) ion Green solution to brown

chlorine Pale yellow to colourless

bromine Brown to colourless

Iron (III) ion Brown to green solution

Any substance that gain electron Any substance that lose electron

Carbon compound

Homologous series

General formula Functional group

example Physical properties

Alkane CnH2n+2 none ethane Gas, colourless, not soluble in water, less dense than water, does not conduct electricity

Alkene CnH2n C=C ethene Gas, colourless, not soluble in water, less dense than water, does not conduct electricity

Alcohol CnH2n+1OH -OH ethanol liquid, colourless, soluble in water, does not conduct electricity

Carboxylic acid CnH2n+1COOH -COOH Ethanoic acid liquid, colourless, soluble in water, conduct electricity

ester CnH2n+1COO CmH2m+1

-COO ethylethanoate

liquid, colourless, insoluble in water, does not conduct electricity, floats on water, sweet smelling

Products of Electrolysis

electrolyte electrode Products at cathode and factor Product at anode and factor

Hydrochloric acid, sodium chloride solution

( 0.01 moldm-3 or less)

Carbon Hydrogen

(Position of ion in ECS)

Oxygen

(Position of ion in ECS)

Hydrochloric acid, sodium Carbon Hydrogen Chlorine

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chloride solution

(more than 0.01 moldm-3 )

(Position of ion in ECS) (concentration of ion)

Sulphuric acid or sodium sulphate solution

carbon Hydrogen

(Position of ion in ECS)

Oxygen

(Position of ion in ECS)

Copper(II) sulphate solution Carbon Copper

(Position of ion in ECS)

Oxygen

(Position of ion in ECS)

Copper(II) sulphate solution copper Copper

(Position of ion in ECS)

Copper ion

( type of electrodes)

Silver nitrate solution Carbon Silver

(Position of ion in ECS)

Oxygen

(Position of ion in ECS)

Silver nitrate solution silver Silver

(Position of ion in ECS)

Silver ion

( type of electrode)

Contact Process

Step 1 : S + O2 SO2 Step 2:2 SO2 + O2 2 SO3

Temp: 450 oC -550oC

Pressure – 1 atm

Catalyst- vanadium(V) oxide

Step 3: SO3 +conc H2SO4 H2S2O7

H2S2O7 + H2O 2H2SO4

Haber Process

3H2 + N2 2NH3 Temp: 450 oC -550oC Pressure –200-400 atm Catalyst- iron

Good luck! Man jadda wajada,waman zar’a hasoda........