all revision

7/30/2019 All Revision

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RATES OF REACTIONThe rate of a chemical reaction is determined by HOW FASTa reaction occurs (this is the rate of

reaction):

TYPES OF REACTION :VERY FAST an explosion e.g. dynamite

FAST group 1 metals + water

SLOW zinc + acidVERY SLOW rusting

FACTORS AFFECTING RATE :TEMPERATURE: each atom will then have a higher kinetic energy, which increases the number of collisions(as the particles are moving faster and crazier), and bigger and faster collisions

CONCENTRATION: a higher concentration means more atoms and molecules which will then increase theprobability of collision, which increases the efficiency of a reaction

SURFACE AREA: the larger the surface area, the more reactions can take place on that certain substance,which increases the efficiency of the reaction

CATALYST: lowers the ACTIVATION ENERGY allowing the substance to react at a lower temperature, whichdecreases the amount of energy needed, allowing it to react faster

PRESSURE: the increase in pressure for gases is the same as increasing concentration for liquids; it meansthat there are more of that certain atom, which therefore increases the likelihood of collision

CATALYSTSThey are mainly used in industrial processes, as they manage to speed up the rate of reaction. They do this

by lowering the activation energy, which means that they can use less energy to complete the reaction. This

reduces costs, and is therefore very useful to the companies.

ENZYMESEnzymes are complex molecules which act as a biological catalyst in leaving systems, such as humans

(amylase, protease etc.). They are very sensitive to temperature and pH.


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Catalysts Enzymes

Manganese Dioxide Making O2 from hydrogen

peroxideAmylase

Platinum, Rhodium & Palladium used in car

exhaust pipesProtease

Nickel - making margarine Lipase

ATOMIC STRUCTURE &

CHEMICAL BONDING

Electrons:

relative charge: -1

relative mass: 11836

Protons

relative charge: +1 relative mass: 1

Neutrons

relative charge: 0 relative mass: 1

Electrons found in a shell

around the nucleus

Nucleus has protons andneutrons


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POTASSIUMS ELECTRONIC STRUCTURE

Atoms transfer electrons in chemical bonds to try and achieve a full outer shell as it is MORE STABLE.

IONSIons are electrically atoms or groups of atoms. They are formed by the loss or gain of electrons

Type of Ion Charge

Metal Atoms&Ions Positively Charged (+)

Non-Metal Ion Negatively Charged (-)

COMMON IONS

SODIUM:Na+ MAGNESIUM:Mg

2+

AMMONIUM:NH4 + OXIDE:O2- CHLORIDE:Cl-

IONIC BONDINGIonic bonding includes the gain or loss of one or more electrons from an atom

-to obtain a FULL OUTER SHELL

Ionic Bonding only occurs between: METALSANDNON-METALS (1metal+1non-metal)

K2,8,8,1


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EXAMPLES:

ClNa

Na Cl

NaCl

OMg

Mg O

MgO


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LATTICE STRUCTUREA way of displaying regular patterns within atoms of oppositely charged ions is used a lattice structure:

IONIC SUBSTANCES THEY HAVE HIGH METING POINTS: strong electrostatic bonds between each ion (and these have to

break)o The greater the charge on the ions the higher the melting and boiling point.

COVALENT BONDINGDEFINITION :Covalent bonding is the sharing of a pair of electrons between two atoms. Covalent bonds are only

formed between NON-METALS + NON-METALS.

FAl

Al F

AlF3

Lattice of NaCl+

++

++ +

++ --

--

-

--


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FORMATION

METALLIC BONDING

DEFINITIONA metallic bond is a giant structure of positive (metal) ions, surrounded by a sea of delocalised (free)electrons.

Cl ClH H H Cl

O O

H

O

H H

C

H

H

N

H

H

O O O

Positive metal ions

Sea of negative ions

+

+ ++ +

+

+

+


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STRUCTURECARBON DIOXIDE :

Double bonds Structured in a line It is stable (has a full outer shell)

DIAMOND

Single covalent Bonds All bonds are strong No weak Bonds Tetrahedron of Carbon atoms

GRAPHITE Hexagonal shape of c atoms Only 3 covalent bonds It is formed in layers Weak bonds between layers

C O C

C

C

C C

C

C


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THE STRUCTURE DIAGRAM

SIMPLE MOLECULAR SUBSTANCESThey normally have low boiling and melting points because the forces of attraction are typically

weaker, and therefore they are easier to break.

They dont conduct electricity, because they are all COVALENT bonds, and therefore share electrons which

UTILISES all of them, which means there are no free electrons.

DIAMOND and GRAPHITE have many strong covalent bonds making their melting and boiling points veryhigh.

HOWEVER

DIAMOND has no free electrons within its structure which means that it cannot conduct electricity.

GRAPHITEdoes have free electrons between layers of carbon atoms, and can therefore conductelectricity. It also has layers of carbon atoms connected by weak bonds making them slippery.

Giant Structure Molecular Structure

Substances made up ofhuge numbersof atoms, or

ions

Substances that are made up of a mixed number of

atoms shown by the molecular formula (eg. H2O or

C6H12O6

The number of particles is not fixed, but are usually

arranged in a regular pattern(lattice)

Generally the atoms are joined by covalent bonds.

The molecules are usually very small but can be

large in some cases

Includes:

Giant Metallic - all metals and alloys Giant ionic all ionic substances

Giant Covalent in diamond, graphite andsilicon

Includes Simple Structures:

Monatomic like He, Ne, Ar etc. Simple Molecules like H2, H2O, CO2

Structure

Sim leGiant

Gra hiteDiamond

Silicon

Carbon

All

Metals

Anything

Ionic Almost all

covalent

substances


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MACROMOLECULEA macromolecule is an extremely large molecule containing a very large number of atoms.

REACTIVITY SERIES

DISPLACEMENTExample:

OXIDE:The removal of electrons from a substance, or the addition of oxygen

REDUCTION:The addition of electrons from a substance, or the removal of oxygen

REDOX:a reaction in which reduction and oxidation is both occurring

OXIDISING AGENT:A substance that is capable of oxidising another substance

REDUCING AGENT:A substance that is capable of reducing another substance

Element Cold water/steam Dilute Acid

Potassium

React very vigorously with cold water

to form a solution of the metalhydroxide + hydrogen

Reacts vigorously to form a

metal salt + hydrogenSodium

Lithium

Calcium

Decreasing vigour as scaledecreases (forms metal salt +

hydrogen)

Magnesium Reacts very slowly with cold water, but

burns with steam MgO + H2

Aluminium Does not react with cold waterhowever reacts with steam without

burning, to form metal oxide +hydrogen

Zinc

Iron

Tin

Does not react with steam or water

Lead

Copper

Does not reactSilver

Gold

Platinum

More Take Salt


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EXAMPLES2Na+O Na2O

Mg + OMgO

2K + 2H2O H2+2KOH

Ca + 2H2O Ca(OH)2 + H2

3AgNO3 + Fe 3Ag + Fe(NO3)3

MgSO4 + Cu CuSO4 + Mg

RUSTINGFe2 + 3O2 Fe2O3

A REDOX reaction will occur and the iron will be oxidised. Rusting normally occurs in moisture-prone areas.

EXTRACTION &USES OF METALSMost metals found recently are higher up in the reactivity series. This is because as technology progresses

we are able to find more reactive substances, which could not have been found previously, and so are now

founded.

As the reactivity series increases the extraction methods become more extravagant and expensive.

If the substance is low down it is safer and can therefore be used in consumer products.

QUALITATIVE ANALYSISQualitative: what is present?

Quantative: how much?

IONSAn ion is a charged atom or molecule: Cations are POSITIVE: Li+, Na+, K+, and NH4

Anions are NEGATIVE: F-, Cl-, Br-, and OH-

Ions can have more than one chargehowever.

Group 1 2 3 4 5 6 7

Charge +1 +2 +3 -3 -2 -1


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Positive Ions Negative Ions

Hydrogen ion H+ Magnesium Mg2+ Aluminium Al3+ Chloride Cl- Oxide O2-

Lithium Li+ Calcium Ca2+ Iron(III) Fe3+ Bromide Br- Co32-

Sodium Na+ Barium Ba2+ Iodide I- Sulfate SO42-

Potassium K+ Manganese (II) Mn2+ Hydroxide OH-

Ammonium NH4+ Iron (II) Fe2+ Nitrate NO3-

Copper (II) Cu2+

Zinc Zn2+

TESTING FOR CATIONS1. Flame test: some metals burn with a distinctive colour2. Dissolve the unknown substance in concentrated Hydrochloric Acid (HCl)3. Dip this solution on a piece of sterile wire4. Hold in a hot flame

Metal Ion Flame Colour

Li+ (Lithium) Red scarlet

Na+ (Sodium) Orange yellow

K+ (Potassium) Lilac

Ca2+ (Calcium) Brick-red

Ba2+ (Barium) Apple-Green

Or

1. Sodium Hydroxide test: adding sodium hydroxide to Cations produces a precipitate2. Aqueous metal salt + aqueous sodium hydroxide precipitate

Metal Ion Precipitate

Al3+, Mg2+, Ca2+ White precipitate

Al(OH)3Re-dissolves sodium

hydroxide

Cu2+ Pale blue

Fe2+ Dirty green

Fe3+ Rusty brown

SYMBOLEQUATION: CaCl2 (aq)+2NaOH(aq)Ca(OH)2 (s)+2NaCl(aq)

IONICEQUATION: Ca2+(aq) + 2OH-(aq) Ca(OH)2 (s)


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TESTING FOR IONSThe anions are only the halides (group 7 metals Cl, Br, I), the sulphates, carbonates, and nitrates.

HALIDES:You can test for them using DILUTE NITRIC ACID AND SILVER NITRATE forms an insoluble silver iodide

precipitate.

1. Make a solution of suspected halide2. Add enough nitric acid to make it acidic3. Then add some silver nitrate solution (AgNO3(aq))

White precipitate: AgCl

Pale Green: AgBr

Yellow: AgI

Equations

Ag

+

(aq) + X

-

(aq) AgX (s)Ag+(aq) + Cl

-(aq) AgCl (s)

AgNO3(aq) + NaBr(aq) AgBr NaNO3 (s)As the precipitates are similar colours you can do a further test to make sure that you know what is what.

The test is the SOLUBILITY IN AMMONIA SOLUTION.

Halide Solubility in Dilute Ammonia In Concentrated Ammonia

Silver Chloride Silver Bromide Silver Iodide

FURTHER ATOMIC STRUCTURE

A Single

Atom

2 Separate

Atoms

2 Chemically

Joined Atoms


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GENERAL STRUCTURE

Isotope: atoms with different numbers of neutrons however, are the same element.

Relative atomic mass: the weighted average mass of the isotopes of an element relative to an atom of

Carbon-12

We use the weighted average mass because there ARENT EQUAL AMOUNTS OF ISOTOPES of eachelement.

To find out the Relative Formula Mass (Mr) of Chlorines isotopes, we need to know its isotopes and their

relative atomic mass:

Eg1. The isotopes of chlorine are: 75% 35Cl, and 25% 37Cl.

When we add these two together, we get 35.5, this means the RFM (Mr) is 35.5 (35.5Cl)

Relative Formula Mass: the relative formula mass of a compound is the sum of relative atomic masses (Ar)

of the atoms in the numbers shown in the formula.

Eg2. MgCO3= 1Mg 1C 3O

( )

23

11 Na

Mass Number protons and

neutrons

Atomic Number Protons (and

neutrons if it isnt an isoto e


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Mass

MrMole

THE MOLEThe mole is a measurement of a substance, a mole of carbon; a mole of water.

For example: Ar of C=12 . . . So 1 mole of C is 12g

Mr of H2O is 18, so 1 mole of H2O is 18g

The molar mass = mass of 1 mole

= same as Mr

QUESTIONS

Whats the mass of 1 mole of Mg?

Ar=24.3, 1 mole=24.3g

What is the mass of 1 mole of NaOH?

Mr=40, 1 mole=40g

What is the mass of 0.2 moles of CaCO3?

Mr=100, 0.2x100=20g

How many Moles in 54g of H2O?

Mr=18,

18 moles

AVOGADROS NUMBER One mole of something always contains the same number of molecules (or atoms if its an element) That number is 3 So 1 mole of carbon has a mass of 12g and contains 3 atoms of Carbon-12 But 1 mole of water has a mass of 18g and also contains 3 of water molecules

KEY CONCEPTSRadicals Formula Valency

Ammonium NH4- 1

Hydroxide OH-

1Nitrate NO3

- 1

Carbonate CO32- 2

Sulfate SO42- 2


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The reaction ratio is called the STOICHIOMETRY

GENERAL FORMULAS

CALCULATIONSWHAT MASS OF MGO IS FORMED WHEN 4.8G OF MG IS OXIDISED?

1. Balance Equation:

2. Stoichiometry:

3. Work something out:

4. Mr of MgO = 40

PERCENTAGE YIELD

EMPIRICAL FORMULA1. Calculate moles of each element2. Divide by smallest = ratio

Eg1. Mg O Eg2. H O

=0.1

1

1

8

16

0.1

MgO H2O


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AVOGADROS LAW That 1 mole of any gas will OCCUPY 24DM3 1Litre = 1dm3 = 1000cm3 1 Mole of Ammonium will occupy 24000cm3

CALCULATING THE VOLUME OF GASCALCULATE THE VOLUME OF 0.01G OF HYDROGEN:

3

CALCULATE THE VOLUME OF CARBON DIOXIDE PRODUCED AT ROOM TEMPERATURE WHEN DILUTE

HCL IS ADDED TO 1.00G OF CACO3

3

CALCULATING THE CONCENTRATIONThis is the number of moles in a litre (of water or another solvent)

1mole in litre has a concentration of 1mol/dm3 (1moldm-3)

Also 1M = 1 molar solution

Volume in dm3

3

3

CRITICAL EQUATIONS:


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CHEMISTRY OF THE ELEMENTSIMPORTANT GROUPS:

Group 1LITHIUM, SODIUM, POTASSIUM Group 7CHLORINE, BROMINE, IODINE Group 0 noble gases; HELIUM, NEON, ARGON (full outer shell)

GROUP 1In group 1, the elements get INCREASINGLY REACTIVE due to the distance between the first shell and last

shell, in order for a reaction to take place, these shells must be broken, and so the more that need to be

broken, the more reactive they are.

GROUP 7Chlorine a yellow/green GAS at room temperature

Bromine a brown LIQUID at room temperature

Iodine a black SOLID at room temperature

ORGANIC CHEMISTRYTerm Definition

Homologous seriesA series of organic compounds that have the same general formula,similar chemical reactions and where each member differs from the

next by a Ch2- group

Hydrocarbon A compound only containing the elements hydrogen and carbon

Saturated An organic compound in which all bonds are single bonds

Unsaturated An organic compound that contains carbon-carbon double bonds

General FormulaA formula that states the ratio of atoms of each element in the

formula of every compound in a particular homologous series

IsomerismCompounds that have the same molecular formula but differentdisplayed formulae are said to exhibit isomerism; the different

compounds are called isomers


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ALKANES

This is a homologous series that has the general formula:CnH2n+2. these are the first five terms in theseries:

Molecular Formula Name

CH4 Methane

C2H6 Ethane

C3H8 Propane

C4H10 Butane

C5H12 Pentane

Displayed Formula

ReactionsCombustion: the alkanes burn when heated in air or oxygen. If there is a plentiful supply of air/oxygen the

products are carbon dioxide and water.

() () () ()

38 () () () ()

Methane Ethane Propane Butane

DimethylpropaneMethylbutaneMethylpropanePentane

Both butane and pentane have isomers: Methylpropane is an

isomer of butane; and Methylbutane and Dimethylpropane

are isomers of pentane


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If there is insufficient oxygen:

() () () ()

With Bromine: Methane and bromine react together in the presence of UV radiation to form

bromomethane.

() () 3() ()

ALKENES

This is a homologous series that has the general formula:CnH2n. these are the first five terms in the series:

Molecular Formula Name

C2H4 Ethene

C3H6 Propene

C4H8 Butene

C5H10 Pentene

Reactions of the AlkenesAlkenes undergo addition reactions with halogens. For example, a bromine molecule will add across the

double bond of ethene to form 1,2-dibromoethane:

1,2-dibromoethane is colourless, so when

bromine or bromine water is shaken with ethene

the BROMINE WILL DECOLOURISE. All alkenes will

decolourise bromine. This is the TEST FOR

UNSATURATION (c=c double bonds).

Ethene Propene But-1-ene

Meth l ro eneMethane Ethane Propane Butane

But-2-aneMethane Ethane Propane Butane


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ETHANOLEthanol is manufactured by two different processes: fermentation and direct hydration of ethane.

Fermentation Dissolve sugar or starch in water and add yeast Leave the mixture to ferment at 25-40C for several days in the absence of air Filter off the excess yeast to obtain a dilute solution of ethanol

If the ethanol content in the mixture rises to around 15%, the yeast is now killed. If a moreconcentrated solution of ethanol is required, the mixture is fractionally distilled.

Whatever the starting point, sugar or starch, the enzymes in the yeast produce glucose, C6H12O6. Theenzymes in yeast then convert the glucose into ethanol:

616() () ()

Direct Hydration of Ethane A mixture of ethene and steam is passed over a phosphoric acid catalyst at a temperature of 300C

and 60-70 atmosphere pressure:

() () () The ethanol is condensed as a liquid The ethene required for this reaction is obtained from crude oil

Comparing the Two Methods

EXTRACTION OF ALUMINIUMThe method of extraction of metals relates to their reactivity, the higher the reactivity, the more difficult the

extraction process.

Fermentation Hydration

Raw materials USE RENEWABLE SOURCESUses NON-RENEWABLE resources

once all the crude oil is used up

there will not be any more

Type of process BATCH process CONTINUOUS process

Rate of reaction Very SLOW, several days FAST

Quality of product

Produces a DILUTE solution of

ethanol that needs further

processing if pure ethanol is

required

Produces PURE ETHANOL

Reaction conditions LOWTEMPERATURES requiredHigh temperature and pressures

required, increasing the COSTS


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ELECTROLYSIS

The positive and negative electrodes are made of graphite (Carbon). The electrolyte is a solution of aluminium oxide dissolved in molten cryolite. The main ore of aluminium is bauxite. The bauxite is first purified to produce aluminium oxide, Al2O3 Aluminium oxide has a very high melting point and hence it is dissolved in cryolite to make the

electrolyte. This mixture has a much lower melting point and is also a much better conductor ofelectricity than molten aluminium oxide.

At the negative electrode:3

The aluminium melts and collects at the bottom of the cell and is then tapped off.

At the positive electrode:

Some of the oxygen produced at the positive electrode then reacts with

graphite to produce carbon dioxide gas:

() () ()

This means that the positive electrode slowly burns away and needs to be regularly replaced.

+

-

Positive electrode

Negative

electrode

Insulation

Electrolyte

Tapping hole


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EXTRACTION OF IRONBLAST FURNACE

The raw materials are iron ore (haematite), coke (carbon), limestone (calcium carbonate) and air Iron ore, coke and limestone are mixed up together and fed into the top of the blast furnace Hot air is blasted into the bottom of the furnace

Iron ore mixed with

limestone and coke

Waste

gases

Waste

gases

Blast of

hot air

Molten slag

Molten iron


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THE REACTIONS

Oxygen in the air reacts with the coke to form CARBON DIOXIDE:() ()

Carbon dioxide reacts with coke to form CARBON MONOXIDE:() () ()

Carbon monoxide REDUCES IRON (III) OXIDE in the iron ore:3() ()

The iron melts and collects at the bottom of the furnace, where it is tapped off The calcium carbonate in the limestone decomposes to form CALCIUM OXIDE:

3() () ()

The calcium core reacts with silicon dioxide, which is an impurity in the iron ore, to form CALCIUM

SILICATE:

() () 3()

The calcium silicate melts and collects as a molten slag on top of the molten iron, which is thentapped off separately

USES OF ALUMINIUM AND IRON

Aluminium

Iron

Use Most important property

Aeroplane body high strength-to-weight ratio

Overhead power cable Good conductor of electricity

Saucepans Good Conductor of heat

Food cans Non-toxic

Window frames Resists corrosion

Use Most important property

Car Bodies Strong (withstand collisions)

Iron Nails Strong

Ships, Girders & Bridges Strong


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CRUDE OILWHAT IS IT?Crude oil is a thick, sticky, black liquid that is found under the ground and under the sea in certain

parts of the world such as the Middle East and Texas (USA). It is a mixture of hydrocarbons, MOSTLY

ALKANES.

REFINING CRUDE OILCrude oil, as such, has no direct use. It has to BE REFINED before it is of any use. The first step in the

refining of crude oil is FRACTIONAL DISTILLATION.

Fractional distillation is carried out in fractioning columns. The column is hot at the bottom and gradually

becomes cooler towards the top.

The crude oil is split into various fractions

as described below. A fraction is a mixture

of hydrocarbons with very similar boiling

points.

Crude oil is heated to convert it intoVAPOUR and is then fed into the

bottom of the column

The hydrocarbons with very highboiling points (fuel oil and bitumen)IMMEDIATELY TURN INTO LIQUIDS

and are tapped off at the bottom ofthe column

The hydrocarbons that have boilingpoints lower than 400oC remain as

gases and RISE UP THE COLUMN,AS THEY DO THEY COOL DOWN.

The different fractions willcondense at different heights

according to their different boilingpoints. When they condense theyare tapped off as liquids

The fraction with the lowest boilingpoint (refinery gas) REMAINS AS AGAS and comes out the top.

Refinery

Gasoline (petrol)

Kerosene

Diesel Gas (gas oil)

Fuel Oil

Bitumen

Crude Oil

40oC

400oC

Fractioning

Column


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PROPERTIES

USES

HOW DOES CRACKING WORK?Alkane is a long-chain hydrocarbon, and these molecules are passed over a catalyst (silica or aluminium

oxide) and heated to about 600oC. They then start to break down into a short-chained alkane, and at least

one alkene.

Eg. Cracking of Decane (C10H22) to produce octane (C8H18) and ethene (C2H4).

1() 818() ()

INCOMPLETE COMBUSTION can create carbon monoxide, which reduces the bloods ability to carryoxygen.

Fraction

Number of

Carbon AtomsBoiling Point Thickness

Refinery Gases

INCREASES INCREASES INCREASES

Gasoline

Kerosene

Diesel Oil

Fuel Oil

Bitumen

Fraction Uses

Refinery Gases Bottled Gas For Camping

Gasoline Petrol for Cars

Kerosene Fuel for planes; oil for central heating; paraffin for small heaters

Diesel Oil Diesel fuel for buses, lorries, trains and cars

Fuel Oil Fuel for ships and for industrial heating

Bitumen Road surfaces and covering flat roofs of buildings


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OXYGEN AND OXIDESCOMPOSITION OF GASES IN CLEAN UNPOLLUTED AIR :

HOW TO SHOW THAT AIR CONTAINS1

OF OXYGEN:H

Using Copper

This apparatus can be used to find the percentage of oxygen in air:

Set up the apparatus with 100cm3 of air in one gas syringe Heat the copper at one end of the silica tube using a blue Bunsen burner Pass the air backwards and forwards over the copper As the volume of gas decreases, move the Bunsen flame along the tube so it heats fresh copper Stop heating when the volume of gas has stopped decreasing The copper has reacted with the oxygen to form black copper oxide:

() () ()

The final volume will be around 78-79cm3 which shows that 21cm3 has reacted with the copper sothat says that 21% of oxygen is in the air.

Gas Percentage in Air

Nitrogen 78

Oxygen 21

Argon 0.9

Carbon dioxide 0.04

Originally 100cm3 of airSilica tube packed with copper

Gas syringeHeat


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Using IronPlace wet iron filings in the end of a burette and set up the apparatus as shown in the diagram.

Over several days the water will rise up the burette and reach a constant level. This is because

the iron reacts with the oxygen in the air. Take the initial and final readings of the water level

in the burette.

( )

( )

( )

LABORATORY PREPARATION OF OXYGENHydrogen peroxide (H2O2), decomposes slowly to form water and oxygen. The speed of decomposition is

increased by adding a catalyst: MnO2, manganese dioxide. The oxygen can be collected over water. Since

oxygen is not very soluble in water, very little is lost. An aqueous solution of hydrogen peroxide is used.

() () ()

Manganese (IV) Oxide

Oxygen

Hydrogen Peroxide


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REACTIONS OF OXYGEN

Magnesium oxide is a basic oxide, and is very slightly soluble in water and when saturated will have a pH of

about 10. It reacts with water to form magnesium hydroxide:

() () ()()

CARBON DIOXIDELAB PREPARATION: 3

The reaction between any metal carbonate and an acid will produce carbon dioxide. Calcium carbonate is

the most commonly used carbonate in the laboratory preparation of carbon dioxide. The most convenient

form of calcium is in marble chips. They are very easy to handle and the reaction is not too fast so the

Element Observations Equation

MagnesiumBurns with bright, white flame to

form a white powder

Carbon

Burns with a yellow-orange flame

to form a colourless gas

SulphurBurns with a blue flame to form a

colourless gas

Calcium carbonate

Carbon Dioxide

Dilute Hydrochloric acid

Water

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