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Science Revision—C1

Topic: Structure of an atom


Science Revision—C1 Science Revision—C1

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Topic: Mass Numbers and Atomic Numbers

Topic: Electronic Structure Topic: Noble Gases

Draw and label the structure of an atom.

Use this to explain what an element is.

Draw a table to show the mass and charge of the particles that make

up an atom.

Use this to explain why atoms have no overall charge.

For each of the atoms below give the mass number, atomic number

and work out the number of protons, neutrons and electrons.

Extension:

Use the chlorine atoms to explain what “isotopes” are

C 12

6 Na

23

11 P

31

15 Cl

37

17 Cl

35

17 U

238

92

Draw the electronic structures of the atoms below:

Why do elements in the same group have similar chemical properties?

What is the link between the group number and the electronic struc-

ture of each atom?

C 12

6 Na

23

11 P

31

15 Cl

37

17

Where do we get Noble gases from?

How do we separate Noble Gases from the oxygen and nitrogen?

Why are Noble gases unreactive?

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Element is a substance containing only one

type of atom.

Particle Charge Mass

Proton +1 1

Neutron 0 1

Electron -1 0

The number of protons and

electrons must be equal so

the atom is neutral.

C 12

6

Na 23

11

P 31

15

Cl 37

17

Cl 35

17

U 238

92

Atomic Mass Number Protons Neutons Electrons

6 12 6 6 6

11 23 11 12 11

15 31 15 16 15

17 37 17 20 17

17 35 17 18 17

92 238 92 146 92

Isotopes: Same number of protons, different number of neutrons

Noble gases are found in the air.

You can isolate them using fractional distillation:

Step 1: cool the air down until it is a liquid

Step 2: Let it warm up—the gases boil off pure, one by one.

Noble Gases are unreactive because the all have a full outer shell.

Elements in same group have same number of electrons in outer shell, so

have similar chemical properties.

Group number equals number of electrons in outer shell


Topic: Bonding



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Topic: Theories of where life came from

Topic: Ionic and Covalent Bonding Topic: Balancing Equation and Conservation of Mass

Use diagrams to help explain the different types of bonding in sodium

chloride (an ionic compound) and chlorine (a covalent molecule), and

how they occur.

Detail the following theories developed to explain where life came from:

Miller-Urey experiment

Primordial Soup theory.

Where did Earth’s early atmosphere come from?

List the gases it contained.

Where did Earth’s oceans come from?

Where did all the CO2 end up?

Where did all the oxygen come from?

Balance the following equations and for each work out the mass of the

missing product:

Fe2O3 + CO —> Fe + CO2

160g 84g …………... 132g

C5H12 + O2 —> CO2 + H2O

72g 256g 220g ……….



Volcanic eruptions produced the gases in the early atmosphere.

The main gases were CO2, H2O, N2, CH4, NH3

The water cooled to form the oceans.

Some of the CO2 dissolved in the oceans.

The rest of the CO2 was absorbed by plants, eaten by living things and over

time turned into fossil fuels or the shells are compressed into rocks like lime-

stone.

Miller-Urey experiment: Gases

in the air react to form amino

acids when lightning occurs.

Primordial Soup: Chemical from

atmosphere dissolved in oceans,

reacted there and formed the

Sodium Chloride—Ionic Bonding—Metal + Non-metal

Electrons are given and taken

Chlorine—Covalent Bonding—Non-metal and Non-metal

Electrons are shared

Balance the following equations and for each work out the mass of the

missing product:

Mass must be conserved—mass or reactants = mass of products

Fe2O3 + 3 CO —> 2 Fe + 3 CO2

160g 84g 112g 132g

C5H12 + 8 O2 —> 5 CO2 + 6 H2O

72g 256g 220g 108g


Topic: Limestone



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Topic: The Limestone Cycle

Topic: Reaction of metal carbonates and acids Topic: Chemical Formulae

What is the chemical formula for limestone?

Give some advantages and disadvantages of mining limestone.

Describe how the following materials are made from limestone

mortar

cement

concrete

Write a word and symbol equations for the reaction of limestone with

hydrochloric acid.

Describe a test to identify the gas produced in this reaction.

Identify how many atoms are in each of the following compounds:

NaCl

NaOH

C4H10

Ca(OH)2

Na2SO4

Al2(SO4)3

Mg(NO3)2

Draw a diagram to show the limestone cycle.

Write balanced chemical equations for:

the thermal decomposition of limestone

the reaction of calcium oxide with water

Which other metal carbonates undergo thermal decomposition and

which don’t.



Identify how many atoms are in each of the following compounds:

NaCl 2

NaOH 3

C4H10 14

Ca(OH)2 5

Na2SO4 7

Al2(SO4)3 17

Mg(NO3)2 9

Calcium Carbonate + Hydrochloric Acid

—> Calcium Chloride + Water + Carbon Dioxide

CaCO3 + 2HCl —> CaCl2 + H2O + CO2

All metal carbonates react with acids to form salts.

Carbon dioxide test:

Bubble gases through limewater and if gas is CO2, limewater goes cloudy.

Limestone is CaCO3

Limestone decomposes when heated to give carbon dioxide and calci-

um oxide.

Cement—calcium oxide + clay

Mortar — calcium oxide + clay + sand

Concrete—calcium oxide + clay + sand + gravel

Advantages of mining limestone: versatile building material: creates

jobs; better transport link built as a result.

Disadvantages of mining limestone: noise; dust; increased traffic; quar-

ries look bad; bad for tourism. Sodium and potassium carbonate DO not decompose when heated; all

other do.


Topic: Extracting Iron



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Topic: Extracting Copper

Topic: Aluminium, Titanium, Gold Topic: Alloys

Explain how copper is extracted by:

smelting

electrolysis

phytomining

bioleaching

displacement with scrap iron

Explain why the copper extracted by electrolysis is much higher value

than that extracted by smelting.

Why are bioleaching and phytomining important new methods of ex-

traction?

What is an ore?

How is aluminium extracted from its ore?

Why can’t it be extracted by reduction with carbon?

What is it used for? Why?

How is titanium extracted from its ore?

Why can’t it be extracted by reduction with carbon?

What is it used for? Why?

Why don’t we need to extract gold from an ore?

Draw diagrams to show a pure metal and an alloy.

Use the diagrams to explain why:

pure metals are soft

alloys are hard

Give properties of:

low carbon steels

high carbon steels

stainless steel

Explain how iron is extracted in a Blast Furnace by smelting

Describe the make-up of the iron produced and why this is a problem.

Why is it important to recycle iron (and other metals)?



Carbon is put in furnace with iron

oxide. Burning it gives the high tem-

peratures necessary. It also takes the

oxygen off the iron to form more

CO2.

The iron produced is 96% Fe and 4%

C. This makes it brittle and of limited

use.

Recycling is important as it saves on

resources, minimises waste going to

landfill and saves on energy costs.

Smelting— copper oxide reacts with carbon to give copper metal

Electrolysis—use electricity to purify impure copper metal.

Electrolysis copper is much purer, so can be drawn into wires and

madesinto pipes that can bend. Smelting iron is brittle due to carbon.

Phytomining—copper absorbed from low grade ores by plants, then burn

plants to get metal.

Bioleaching—copper absorbed from solutions by bacteria, then collect

bacteria and burn them to get metal.

Recycled iron—drop it into solutions containing copper ions and the iron

displace the copper so copper metal can be lifted out.

These three allow copper to be extracted from ores with low concentra-

tions, where smelting or electrolysis would not give profit.

Ore: Rock with enough metal in to make it financially viable to extract it.

Aluminium—extract by electrolysis because it is more reactive than carbon (smelting will not work). Uses: cans, foil, takeaway trays, in alloy wheels.

Resistant to corrosion; common, easily shaped, excellent electrical conductor.

Titanium—extract by electrolysis because if you use carbon, it stays in metal making it brittle and useless. Uses: artificial hips, fighter jets.

Resistant to corrosion, lightweight, very strong.

Gold is found as the element in the ground as it is unreactive, not in an ore, so no need to extract.

Pure metal

Atoms arranged in layers.

Layers can slide so metal is soft.

Alloy

Some atoms of different sizes means no layers.

Layers can slide so metal is hard.

High Carbon Steel No layers, so brittle, hard and strong. Retains its shape.

Low Carbon Steel Softer metal so layers can slide; good for steel wires

Stainless Steel Chromium added to stop it rusting.


Topic: Separating Crude Oil



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Topic: Alkanes

Topic: Combustion Topic: Air Pollution

For each of the following pollutants, describe how they are formed and what their effect is on the environment:

carbon dioxide

carbon (particulate)

sulphur dioxide

nitrogen oxides

For sulphur, explain how sulphur is removed from fuels (to minimise sulphur dioxide emissions).

Describe how crude oil is separated into fractions.

Explain the meaning of fraction.

Explain how the following factors changes for the fractions as you

move down the column:

length of carbon chain

boiling point

Flammability

viscosity

Describe the products of complete and incomplete combustion and

balance equations for the complete combustion of:

C5H12 C8H18

Draw diagrams and name the first four alkanes.

Deduce the molecular formula of these alkanes.

Deduce the general formula of alkanes.

Explain the meaning of the word hydrocarbon.

Explain the meaning of the word saturated.



CH4

C2H6

C3H8

C4H10

General formula: CnH2n+2

A hydrocarbon contains

carbon and hydrogen

only

Saturated molecules

contain no carbon-

carbon double bonds.

A fraction is a

mixture of

alkanes with

similar boil-

ing points.

Carbon dioxide — formed whenever fossil fuels are burnt

Environmental Problem: Global Warming

Carbon — formed from incomplete combustion of alkanes

Environmental Problem: Global Dimming

Nitrogen Oxides —formed whenever fuels are burnt at very high temp.

Environmental Problem: Acid Rain

Sulphur dioxide—formed whenever fossil fuels are burnt as they contain small amounts of sulphure

Environmental Problem: Acid Rain

Sulphur removed from petrol before it is burnt

Sulphur removed from coal after is is burnt using filters in the chimneys.

C5H12 + 8 O2 —> 5 CO2 + 6 H2O

C8H18 + 12.5 O2 —> 8 CO2 + 9 H2O

Complete combustion forms carbon dioxide and water.

Incomplete combustion forms water and either carbon monoxide or

carbon.


Topic: Cracking



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Topic: Alkenes

Topic: Polymers Topic: Ethanol

Describe the process of cracking

Explain why cracking is important.

Describe a test that can be used to prove one of the prod-

ucts is an alkene.

Explain why the other alkane products are also desirable.

Draw diagrams and name the first three alkenes.

Deduce the molecular formula of these alkenes.

Deduce the general formula of alkenes.

Explain the meaning of the word hydrocarbon.

Explain the meaning of the word unsaturated.

Draw the structures of ethene and poly(ethene).

Draw the repeating unit of polyethene.

Explain different ways to change the properties of a polymer.

What are polymers used for?

Why are biodegradable polymers important for the environment?

What are the two methods of producing ethanol?

Write the word equations for each method.

What are the advantages and disadvantages of each method?

List some uses of ethanol.



Hydrocarbons—molecules that contain carbon and hydrogen only.

Unsaturated—contains a carbon-carbon double bond

Cracking splits large alkanes into smaller alkanes

(better for fuels) and alkenes (good for making pol-

ymers and alcohols).

The products of crack-

ing are more useful

than the things they

are made from. They

are therefore worth

more.

Test for alkenes using bromine water

With alkanes it stays orange.

With alkenes it turns colourless. polymers and alcohols).

To change the properties of a polymer:

use a different monomer

Change the temperature or pressure

it is made at.

Polymers

used as

plastics

Polymers like poly

(ethene) sit in land-

fill for thousands of

years. New biode-

gradable polymers

developed that will

pollute less in land-

Fermentation Hydration

Equation Sugar —> Ethanol + Carbon Dioxide

37°C/yeast catalyst

Ethene + Steam —> Ethanol

High pressure/

temperature

Advantages Cheap method, Uses little en-

ergy; Uses renewable feed-

stock

Product 95% pure; contin-

uous process; quick

Disadvantages Slow; Product only 14% pure;

Batch process

Uses non-renewable

feedstock

Uses lots of energy

Ethanol used as a solvent and to make alcoholic drinks!!


Topic: Extracting Plant Oils



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Topic: Emulsions

Topic: The Structure of the Earth Topic: Wegener

Detail the two methods commonly used to extract plant oils.

Why are vegetable oils important foods?

List oils and fats that are healthy and unhealthy and identify which are

likely to be saturated and unsaturated.

How does hardening make unsaturated oils more saturated.

Explain what an emulsion is and how they are made.

Give some common examples of emulsions.

What are the advantages of using emulsions.

With the use of a diagram, explain how an emulsifier works.

Describe Wegener’s theory of Continental Drift.

What evidence did Wegener collect to support this?

How did Wegener explain Continental drift occurring?

Draw and label a diagram to show the structure of the Earth.

Describe what happens at tectonic plate boundaries.

Explain why these events are hard to predict.



Plant Oils made by:

cold pressing (squashing seeds until the oil comes out) or

distillation (boiling with water, evaporating the oil then cooling it down)

Oils give us energy.

Cooking with oils gives food more flavour and better texture.

Healthy oils contain carbon-carbon double bonds (they are unsaturated)

Examples: Olive oil, Sunflower oil—liquid fats

Unhealthy oils have few/no carbon-carbon double bonds (they are saturated)

Examples: Butter/Lard—solid fats

Hardening:

Emulsions

Examples—

mayonnaise, paint,

milk, margarine

They have a creamy

texture and nice

appearance com-

pared to what they

are made from.

Emulsifier

added—the

oil and water

stay com-

bined as a

mixture.

No emulsifier

added—the oil

and water sep-

arate to form

two layers.

Emulsifiers have one

end that love oil

(hydrophobic) and

another that loves

water (hydrophilic)

The crust is split into tectonic plates that can move.

At the boundaries, you are likely to experience earth-

quakes, volcanic eruptions and this is where moun-

tains develop as the plates move past each other.

Earthquakes are caused by a

build up of pressure deep

underground. Difficult to pre-

dict because we can’t see the

boundaries, nor predict when

the pressure will be released.

Previous theory—the Earth’s crust formed, then cooled over millions of years. As it cooled

it wrinkled (like custard skin!!) forming mountains.

Wegener— the crust was split into tectonic plates that can move:

radioactive processes in the core produce heat

this heat causes convection currents of molten rock n the Mantle

the movement of the mantle causes the plates to move as well

Evidence

Jigsaw puzzle approach predicts some continents fit together and were once connected.

Wegener found identical rock samples and fossils on different continents where the conti-

nents would have fitted together.

Previous explanation of these places being connected by a land bridge did not make sense.

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