/
Revision for C1 Revision for C1

Revision for C1 - PowerPoint Presentation

cheryl-pisano
cheryl-pisano . @cheryl-pisano
Follow
379 views
Uploaded On 2017-12-05

Revision for C1 - PPT Presentation

C1 1 Fundamental ideas C1 2 Rocks and building materials C1 3 Metals and their uses C1 4 Crude oil and fuels C1 5 Products from oil C1 6 Plant oils C1 7 Our changing planet C1 11 12 and 13 ID: 612670

water carbon dioxide oil carbon water oil dioxide iron electrons copper atmosphere food limestone calcium vegetable years oxygen land

Share:

Link:

Embed:

Download Presentation from below link

Download Presentation The PPT/PDF document "Revision for C1" is the property of its rightful owner. Permission is granted to download and print the materials on this web site for personal, non-commercial use only, and to display it on your personal computer provided you do not modify the materials and that you retain all copyright notices contained in the materials. By downloading content from our website, you accept the terms of this agreement.


Presentation Transcript

Slide1

Revision for C1

C1 1 Fundamental ideasC1 2 Rocks and building materialsC1 3 Metals and their usesC1 4 Crude oil and fuelsC1 5 Products from oilC1 6 Plant oilsC1 7 Our changing planetSlide2

C1 1.1, 1.2 and 1.3

Atoms are made up of protons, neutrons and electrons.

Particle

Charge

Mass

Proton

+1

1

Neutron

0

1

Electron-10

Nucleus

Electrons are arranged in energy levels (shells).

The first shell can hold 2 electrons.

The second shell can hold 8 electrons.

The third shell can hold 8 electrons.

The fourth shell can hold 18 electrons (but you don’t need to go that far).

All atoms want a full outer shell of electrons, and they will do that by gaining electrons, losing electrons or sharing electrons.

Electron configurations can be written 2,8,8,18.Slide3

C1 1.4 Forming bonds

Group

1

2

3

4

5

6

7

8

Outer shell electrons

123

45

678

Electrons gained/lostLoses 1

Loses

2Loses 3N/A

Gains 3Gains 2

Gains 1N/AIon charge

+2+

3+N/A3-

2--N/A

Na

+

Cl

-

We draw the electrons as different shapes to show which atom they came from (dot and cross diagrams)

A metal atom gives electrons to a non-metal atom, so that both of them have full outer shells.

When drawing the electron configuration for an ion, we draw square brackets around it, and put the charge on the outside.

Charges on ions from different groups

Electron configurations can be written Na [2,8]

+

and Cl

[

2,8,8]

-

Slide4

Mg

+

2

F

-

F

-

If the positive and negative ions have different charges, then you will need different numbers of ions to balance out the charge e.g. MgF

2

.

Remember: Swap n’ drop

Mg

2+

F

-

MgF

2

Swap the ion charge numbers, and drop them down to the bottom right of the element symbol. Get rid of the charge.

These ions are on your data sheet, so you don’t need to remember them.

Compound ions

If your compound has a compound ion (OH

-

, NO

3

-

, SO

4

2-

, CO

3

2-

, NH

4

+) and there is more than one of them, you need to put it in brackets.E.G Mg(NO3)2, or (NH4)2O, or Al2(SO4)3

C1 1.4 Forming bondsSlide5

Covalent bonding is a shared pair of electrons.

F

F

covalent bond

solid

line (one line = 1 pair)

F

F

F

F

F

simplified

dot and cross diagram

F

Covalent bonding occurs between non metals.

Group 4 elements share 4 electrons.

Group 5 elements share 3 electrons.

Group 6 elements share 2 electrons.

Group 7 elements and hydrogen share 1 electron.

H

H

O

H

H

H

N

H

Cl

O

O

C

C1 1.4 Forming bondsSlide6

Balancing equations

+

+

CH

4

+ 2O

2

 CO

2

+ 2H

2

OThere are 4 hydrogens here, bonded together.There are 4 hydrogens here. You multiply the big number by the little number.There are 2 molecules of oxygen not bonded together.

You can only change the BIG numbers in equations – we cannot change the small numbers or add or take away any reactants or products.Slide7

C1 2.1 Limestone and its uses

Methane is fuel for the fire to heat limestone.

Carbon dioxide is formed from thermal decomposition of limestone and from burning methane.

Argon and nitrogen come from the air.

CaCO

3

CaO

+ CO

2

Reaction of thermal decomposition limestone.CalciumcarbonateCalciumoxideCarbon dioxideSlide8

CaCO

3(s)  CaO(s) + CO2(g)

CaO(s)

+ H2O

(l)  Ca(OH)2(s)

Ca(OH)

2(s)  Ca(OH)

2(aq)

Ca(OH)

2(

aq

) + CO2(g)  CaCO3(s) + H2O(l) C1 2.2 Reactions of carbonatesLimestone is heated and breaks down (thermal decomposition) into calcium oxide (quicklime) and carbon dioxide.Calcium oxide (quicklime) is added to water to make solid calcium hydroxide (slaked lime).Solid calcium hydroxide (slaked lime) is dissolved in water to make aqueous calcium hydroxide (lime water).Aqueous calcium hydroxide (lime water) is added to carbon dioxide which makes calcium carbonate and water.Slide9

CaO

Water

Sand

Ca(OH)

2

Gravel

Limestone

CaCO

3

Calcium Carbonate

CO

2

+

+

+ Water

HEAT

Calcium Oxide

Carbon Dioxide

Calcium Hydroxide

+ Clay

Cement

+

+

+

Concrete

Sand

Water

+

Mortar

Limewater

C1 2.3 Limestone reaction cycle and C1 2.4 cement and concreteSlide10

C1 2.5 Limestone issues

Limestone quarrying has many advantages and disadvantages:AdvantagesIt creates jobsIt provides building materials nearby

DisadvantagesPollutionNoise pollutionIt ruins the landscapeSlide11

Extracted using electrolysis.

Extracted using reduction by carbon.

Found as elements (native).

Reduction is a reaction that removes oxygen from the metal oxide.

C1 3.1 Extraction of metalsSlide12

Carbon + oxygen

 Carbon dioxide C + O2  CO2

Carbon dioxide + carbon  Carbon monoxide CO

2 + C  2CO

Iron oxide + carbon monoxide  Iron + carbon dioxide Fe2

O3 + 3CO  2Fe + 3CO

2

Iron oxide + carbon  Iron + carbon dioxide 2Fe

2

O

3

+ 3C  4Fe + 3CO2The iron produced in the blast furnace is 4% carbon. This is called pig iron. Pig iron is very brittle because the atoms are not in layers due to the carbon atoms disrupting the layers.Pure iron is arranged in layers . When an atom is struck, the whole layer moves. Pure iron is malleable.C1 3.2 Extraction of ironSlide13

Steel

Composition

Uses

Low carbon steel

Iron, carbon (0.1%)

Cars, buildings and bridges

High carbon steel

Iron, carbon (1.5%)

Tools, knives and swords

Low alloy steels

Iron, carbon, manganese, nickel

Cars, trucks, bridgesHigh alloy steels

Iron, carbon, chromiumTools, armour

Stainless steelsIron, carbon, nickel, chromiumCutlery, saucepans, medical instruments.

Tungsten steelIron, carbon, tungsten

Drill bits

Steels are mixtures of iron, carbon and possibly other metals. Steels are alloys. Alloys are stronger than pure metals because they disrupt the layers of the metals and stop them sliding over each other.The layers of alloys are disrupted, so they stop the layers of metal atoms sliding over each other.

Pure iron is arranged in layers . When an atom is struck, the whole layer moves. Pure iron is malleable.C1 3.2 SteelsSlide14

Aluminium is too reactive to extract from its ore using carbon, so it is extracted using electrolysis. Aluminium is light and strong. It is used for aircraft, foil, drinks cans, saucepans and bicycles.

Titanium is not reactive, but if carbon is used to displace it, it will form brittle titanium carbide. Instead, titanium oxide is reacted with chlorine to make titanium chloride. It is then reacted with sodium to make titanium. This is expensive as the sodium needs to be extracted using electrolysis.

C1 3.3

Aluminium and titaniumSlide15

Copper sulphide + oxygen

 Copper + sulphur dioxideThis is called smelting. Sulphur dioxide causes acid rain.The copper then undergoes electrolysis in order to purify it.

Copper can also be extracted by

phytomining. Plants take up copper from the soil. The plants are then burnt and the ashes are put in sulphuric acid. Scrap iron is added to the copper sulphate to displace it.

Iron + copper sulphate  Copper + iron sulphate

Copper can also be extracted by bioleaching. Bacteria feed on copper ores to get copper solutions.

These solutions are also reacted with iron to extract the copper. Iron + copper sulphate  Copper + iron

sulphate

C1 3.4

Extraction of

copper and C1 3.6 metallic issues.Slide16

C1 chapter 3.5 Useful metals and C1 3.6 metallic issues.

They have the following properties:ShinyMalleableHardStrongHigh melting pointSonorousConducts electricityConducts heat

It is good to recycle metals because it saves energy from extracting them. It reduces pollution as the vehicles are no longer needed to excavate them and it means that less ore is used up. Slide17

C1 chapter

4.1 Crude oilCrude oil is a mixture of lots of different chemicals called alkanes.

Alkanes only contain hydrogen and carbon (hydrocarbons) an they have all single bonds (they are saturated) and have a general formula of C

nH2n+2.Slide18

C1 4.1 Alkanes

Longer chain alkanes have:

Higher boiling points.High viscosity.

Less flammability.Shorter chain alkanes have:

Lower boiling points.Low viscosity.High flammability.Slide19

In fractional distillation, crude oil is heated up. Smaller alkanes have lower boiling points and they go to the top.

Larger alkanes have larger boiling points and they stay at the bottom. The crude oil is split into fractions. Each fraction has a use.C1 4.2

Fractional distillation Slide20

C1 4.3 and C1 4.4 Burning fuels and Cleaner fuels.Slide21

Biodiesel

Biodiesel is fuel from plant or animal products, such as vegetable oils or animal waste.AdvantagesIt burns cleanly.It is carbon neutral.It is less harmful to plants and animals.DisadvantagesIt needs land that should be used for food.It destroys habitats.

C1 4.5 Alternative fuels

Ethanol

Made by fermenting sugar from plants.

Advantages

It burns cleanly.

It is carbon neutral.

Disadvantages

It needs land that should be used for food.

It destroys habitats.

HydrogenMade from electrolysis of water.AdvantagesIt burns cleanly.Obtained from water

DisadvantagesRequires electricity.Explosive.Needs larger volume to store.Slide22

C1 5.1 Cracking hydrocarbons

Cracking – this is when a large alkane is turned into a smaller alkane and an alkene.Alkenes – Alkenes are hydrocarbons (made up of carbon and hydrogen) with a carbon-carbon double bond (C=C). They have the general formula CnH2n (2 hydrogens for every carbon).

You can use bromine water to work out if you have an alkene. Bromine water is brown. Alkenes make it colourless. Alkanes do not change the colour (it stays brown).Slide23

C1

5.2 Making polymers from alkenesIf alkenes are put under a high temperature and pressure, then they all link up to form a long chain called a polymer.

An individual alkene is called a monomer (mono = one, mer = part). When they are joined together, they become a polymer (poly = many)

n

= a big number

An individual unit is in square brackets.

The lines show that it is bonded to monomers outside the brackets.Slide24

C1

5.3 New and useful polymers

Stitches can be made from shape memory polymers which tighten to just the right tightness to close a wound. Eventually, when the wound is healed, they dissolve away.

Hydrogels are polymers that can trap water inside them. They can be used as contact lenses or dressings for burns.

Plasters can be made from light sensitive polymers that lose their stickiness when exposed to light. Instead of ripping the plaster off, you can just rip the cover off which makes the plaster fall away.Slide25

C1

5.4 Plastic waste 

Landfill

Incineration

Recycling

Biodegradable plastics

Advantages

Easy

Relatively cheap

Quick

Quick

The plastics can be used as fuel.Saves energy and resources.Saves landfill space.Preserves crude oil supplies.Tropical forests are destroyed to create farm land.Disadvantages

Uses up landThe plastics stay for centuriesCauses pollutionTakes time and fuel (to transport and sort).Recycled plastic is never as strong as original plastic.

Needs land space to grow crops (reduces land space to grow food)Slide26

C1

5.5 EthanolEthene + steam EthanolC2

H4 + H2O

C2

H5OH

Phosphoric acid catalyst

Sugar (glucose)

Ethanol + carbon dioxide

C

6

H

12O6 2C2H5OH + 2 CO2yeastEthanol can be made by fermentationEthanol can also be made by hydration (Adding water to) ethene.Ethanol can be used as a fuel or a solvent.Ethene is from crude oil, so this method is non renewable. It does produce pure ethanol, however.Sugar is a renewable resource, but it needs land to grow, which would take away land needed to grow food.Slide27

C1

6.1 Extracting vegatable oilCarbon dioxide + water

Glucose + oxygen

Chlorophyll

Sunlight

6CO

2 + 6H2O

C

6

H

12

O6 + 6O2Animal fatVegetable oilAnimal fatVegetable oilPlants use energy from the sun to make glucose. They then turn this glucose into other chemicals, such as vegetable oil.Vegatable oils are unsaturated (they have carbon-carbon double bonds). Animal fats are saturated (they have no double bonds). Vegatable oils are liquids at room temperature. Animal fats are solids at room temperature.Slide28

C1

6.2 Cooking with vegetable oilsC

C

H

H

C

C

H

H

H

H

Nickel60oCHH+

Unsaturated vegetable oilHardened vegetable oilCooking things in oil (compared to cooking things in water) cooks them more quickly (because oil has a higher boiling point), makes the outside of the food change colour and crispier, and makes the inside softer.Foods cooked in oil have more energy than foods cooked in water.

vsCooking in water.Cooking in oil.Hydrogenation of vegetable oilsSlide29

C1

6.3 Everyday emulsions

Water

Oil

When water and oil mix, little droplets of oil form in the water. This mixture is called an emulsion.

However, water and oil do not mix easily (they are immiscible), so they end up like this.

We use emulsifiers to help oil and water mix. Emulsifiers have two parts –a head that mixes with water (hydrophilic) and a tail that mixes with oil (hydrophobic).

This is how emulsifiers help oil and water mix.

Emulsifiers can be used to help make mayonnaise and detergents to help wash up oily pans.Slide30

C1

6.4 Food issuesA food additive is a substance that is added to a food to improve its taste, preserve it or change its colour. All food additives in our food have an E number to prove that they have passed a safety standard. Emulsifiers have an E number that begins with 4.Emulsifers stop oil and water based substances from separating. Emulsifiers are needed in chocolate, mayonaise and ice cream. So emulsifers make foods with lots of energy easier to eat and so it is tempting to eat more fatty food.

Vegetable oils are healthier than animal fats. They contain vitamin E and

t

hey are better for the heart than animal fats.

vsSlide31

C1

7.1 Structure of the Earth

Atmosphere

Crust

Mantle

Core

About 100km from the surface to the top.

5 – 70km thick

3000km thick

3500km in diameter

Made of 78% nitrogen, 21% oxygen, 1% argon and 0.04% carbon dioxide

. We collect the gases from the atmosphere to use.Made of rock. We get minerals from the crust and the oceans.Semi liquid. It can flow very slowly. The crust floats on top of it.

Made of iron and nickel. The outer part is liquid due to the high temperature and the inner part is solid due to the high pressure.We know what the inside of the earth is like from earthquake data. The way the earthquake waves bend tell us the density of the substances below the surface.Slide32

C1

7.2 The restless EarthThe Earth’s crust is split into sections called plates. The plate boundaries are where we find earthquakes, volcanoes and mountains.

Mountains form when two plates move together. Earthquakes occur when two plates rub side by side.

Plates move because they are floating on top of the semi-liquid mantle. Radioactive processes in the mantle release heat which make convection currents which make the plates move.

Alfred Wegener came up with the theory of plate tectonics. His evidence was that fossils and rocks on different continents were similar, indicating that they were once joined. However, this was also supported by the idea of a land bridge which connected South America and Africa. His theories were not accepted until 50 years later when scientists discovered something called seafloor spreading. Slide33

C1

7.3 The Earth’s atmosphere in the past4 Billion years agoEarth’s atmosphere was mainly carbon dioxide, with methane, water vapour, nitrogen and ammonia

.

4 billion years ago The oceans are formed when water vapour condensed.

3.4 Billion years ago Life was formed. It was bacteria that used undersea volcanoes as a source of food

.

2.5 Billion years ago Algae evolved which could use photosynthesis to make food from gases in the atmosphere.

2.5 Billion years ago 

The oxygen in the atmosphere reacts with the methane and the ammonia in the atmosphere.

600 million years

ago

Animals evolved which could use the oxygen for respiration.200 million years ago The Earth’s atmosphere is the same as what it is today.Slide34

C1

7.4 Life on EarthThe Miller-Urey experiment took place in 1953. The scientists took the substances that were in the atmosphere billions years ago. They used water, methane, ammonia and hydrogen and passed an electric spark through them. They got 11 amino acids.Slide35

C1

7.5 Gases in the atmosphereCarbon dioxide has been ‘locked into’ rocks such as limestone.

CH

4 + 2O2

 CO2 + 2H

2O4NH

3 + 3O2

 2N2 + 6H

2

O

Ammonia and methane in the atmosphere reacted with oxygen to form carbon dioxide, water and nitrogen.

The gases in the atmosphere can be removed by fractional distillation. The gases are cooled to a temperature below -200oC and gradually heated up. Nitrogen boils off first at -196oC.Slide36

C1

7.6 Carbon dioxide in the atmosphere

Respiration

hotosynthesis

espiration

issolves

alcium

arbonate

imestone

Sedimentation

Sedimentation

lants

nimals

The carbon cycle

Since the 1960s, the amount of carbon dioxide in the atmosphere has increased. This may be due to burning fossil fuels. Some of the carbon dioxide is absorbed into the oceans. This makes them more acidic, which reacts with coral reefs.