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Year 9 EOY Revision > Chemistry Revision > Flashcards

Chemistry Revision Flashcards

1
Q

What is air made from?

A

Air is made from a mixture of gases; nitrogen, oxygen, carbon dioxide and water vapour.

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2
Q

Where is infrared radiation produced and where does it go?

A

Infrared radiation is produced by the earth. Heat travels through the atmosphere and escapes into outer space.

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3
Q

What absorbs the infrared heat?

A

Greenhouse gases absorb the heat and reflects it back to the earth, causing the average earth’s temperature to increase.

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4
Q

Why are more greenhouse gases in the atmosphere bad?

A

Increased levels of greenhouse gases in the atmosphere trap more of the emitted heat. This leads to a greater increase in the Earth’s temperatures.

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5
Q

How was the earth formed?

A

No life on earth. The surface cools and forms a solid crust. Volcanoes are produced due to tectonic plate movement. Volcanoes produce 4 gases(Carbon Dioxide, Methane, Water-vapour and Ammonia). The earth cools even more and the water-vapour condenses to form oceans. Tress and animals evolve. Trees photosynthesise and take in CO2. Animals respire and take in O2.

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6
Q

How does population effect the greenhouse effect?

A

As the population rises and plant numbers are cut, CO2 remains in the atmosphere.

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6
Q

What is global warming?

A

Global warming is the excessive build up of heat in the earth’s atmosphere.

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7
Q

Why are polar ice caps a problem?

A

As the temperature rises, the ice will melt releasing lots of methane (greenhouse gas). Polar ice caps are the biggest supplier of means in the world.

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8
Q

Why is the ozone so important?

A

Ozone (O3) protects the earth from UV rays produced by the sun. This protects us humans from skin cancer etc.

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9
Q

What destroys the ozone layer?

A

Chlorofluorocarbons (CFCs).

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10
Q

What are Chlorofluorocarbons?

A

Chlorofluorocarbons are chemicals containing Chlorine, Fluorine and Carbon. They are used in aerosol sprays and foam packaging.

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11
Q

Why is the greenhouse effect good for the earth?

A

The greenhouse effect keeps the earth warm at and average temperature of 14 degrees centigrade

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12
Q

What happens if the concentration of greenhouse effect increases?

A

It causes the earth to heat up as more heat radiation is absorbed by the earth and less is re-emitted back into space.

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13
Q

What causes climate change?

A

Increase in greenhouse gases

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14
Q

How can we slow down climate change?

A

We need to cut down on fossil fuels as they release greenhouse gases which contribute to global warming. Be more energy efficient with out life’s and use less carbon dioxide.

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15
Q

How was nitrogen put into the atmosphere?

A

Oxygen reacted with ammonia to from nitrogen and it was released by denitrifying bacteria.

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16
Q

How to test if a gas is oxygen?

A

Place a glowing splint in the gas and if it is oxygen, the splint will re-light.

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17
Q

What are atoms made up of?

A

Atoms are made up of 3 subatomic particles: Protons, Neutrons and Electrons.

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18
Q

Give some properties of Protons

A

Protons are heavy and POSITIVELY CHARGED (+1)

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19
Q

Give some properties of Neutrons

A

Neutrons are heavy and NEUTRAL (0)

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20
Q

Give some properties of Electrons

A

Electrons have hardly any mass and are NEGATIVELY CHARGED (-1)

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21
Q

Describe the nucleus of an atom.

A

It is in the middle of an atoms and contains protons and neutrons. It has a positive charge because of the protons and the whole mass of the atoms is in the nucleus, it is tiny compared to the whole atom.

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22
Q

Describe the electrons within an atom.

A

Electrons move around the nucleus in electron shells. They are tiny but their shells cover a lot of space.

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23
Q

What charge are atoms?

A

All atoms are NEUTRAL and have no charge (unlike ions) - this is because atoms have the same number of protons as electrons.

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24
Q

How does the atomic number and mass number describe an atom?

A

The atomic number (bottom right) tells you how many protons/ Electrons an atom has.
To calculate the neutrons, you subtract the atomic number from the mass number as the mass number says how many protons and neutrons an atom has.

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25
Q

What are electron shell rules?

A

Electrons always occupy shells
The lowest energy levels are always filled first
Only a certain number of electrons are allowed in each cell: 2,8,8.

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27
Q

How does population effect the greenhouse effect?

A

As the population rises and plant numbers are cut, CO2 remains in the atmosphere.

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28
Q

What is global warming?

A

Global warming is the excessive build up of heat in the earth’s atmosphere.

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29
Q

Why are polar ice caps a problem?

A

As the temperature rises, the ice will melt releasing lots of methane (greenhouse gas). Polar ice caps are the biggest supplier of means in the world.

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30
Q

Why is the ozone so important?

A

Ozone (O3) protects the earth from UV rays produced by the sun. This protects us humans from skin cancer etc.

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31
Q

What destroys the ozone layer?

A

Chlorofluorocarbons (CFCs).

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32
Q

What are Chlorofluorocarbons?

A

Chlorofluorocarbons are chemicals containing Chlorine, Fluorine and Carbon. They are used in aerosol sprays and foam packaging.

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33
Q

How to work out electron configurations?

A

You take the atomic number (e.g. 7) and you fill in the shell layers starting with the 1st then 2nd (2,5).

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34
Q

What are ions?

A

Ions are charged particles - they can be single atoms or groups of atoms.

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35
Q

Why do atoms loose or gain electrons?

A

They loose or gain electrons to try and get a full outer shell.

36
Q

When do positive and negative ions occur?

A

Negative ions form when atoms gain electrons (as electrons are negatively charged and there are more electrons than protons).

Positive ions form when atoms loose electrons (as electrons are negatively charges and there more protons than electrons).

37
Q

Which groups on the periodic table are most likely to form ions?

A

1 & 2 are most likely to form positive ions.

6 &7 are most likely to form negative ions.

38
Q

What is ionic bonding?

A

Ionic bonding is when a metal and non-metal react together, the metal atom loosing electrons to form a positive atom and the non-metal atom gaining electron to form a negative atom.

39
Q

Give an example of ionic bonding.

A

Sodium Chloride (NaCl)

The sodium (2,8,1) atom gives up its outer electron, becoming and Na+ ion. The chlorine atom picks up the electron becoming a Cl- ion.

40
Q

Give some rules for drawing dot and cross diagrams for ionic bonding.

A

To represent an ion you must put it within square brackets [ ] and show the charge (by how many electrons) in the top right corner.

41
Q

What is covalent bonding?

A

Covalent bonding is where a bond is formed between two non-metal atoms share a pair of electrons to form a full outer shell.

42
Q

Name a different between ionic bonding and covalent bonding.

A

In covalent bonding atoms share electrons to form a full outer shell, rather than donate like ionic bonding. In covalent bonding, there is no charge involved.

43
Q

Give an example of covalent bonding.

A

Water (H2O)

Oxygen has 6 electrons on its outer shell and Hydrogen only 1. When water is formed, the 2 hydrogen atoms shares its one electron with the oxygen vice versa. This completes a full outer shell of 8 for oxygen and 2 for hydrogen.

44
Q

What is oxidation?

A

Oxidation is when something reacts with or gaining of oxygen because of the loss of electrons.

45
Q

What is reduction?

A

Reduction is the removal of oxygen because of the gain of electrons

46
Q

What is combustion?

A

Combustion is an exothermic reaction (doesn’t require energy) by which something is burned using oxygen.

47
Q

What is the reactivity series?

A

The reactivity series is a table that lists metals in order of their reactivity.

48
Q

Why is carbon in the reactivity series?

A

A metals position in the reactivity series compared to carbon dictates how it is extracted: either using electrolysis or reduction using carbon.

49
Q

Why is hydrogen in the reactivity series?

A

Hydrogen is included in the reactivity series as it shows the reactivity of metals with dilute acids.

50
Q

What are the metals at the top of the series prone to?

A

The metals at the top are more likely to loose their electrons to form positive ions. They also will oxidise quickly.

51
Q

How does acid tell you about metals reactivity?

A

When you place a small amount of a certain metal in an acid (hydrochloric acid), the more reactive the metal the louder the pop when it reacts.

52
Q

What is the equation when a metal reacts with water?

A

Metal + Water –> Metal hydroxide + Hydrogen

Or: Less reactive metal + Steam –> Metal oxide + Hydrogen

53
Q

Which metals react vigorously with water?

A

Potassium, Sodium, Lithium and Calcium

54
Q

Which metals react with steam?

A

Magnesium, Zinc and Iron

55
Q

What type of reaction is a displacement reaction?

A

A redox reaction

56
Q

What is a redox reaction?

A

A redox reaction is where oxidation and reduction happen simultaneously in a reaction - in the case of a displacement reaction, the more reactive metal is oxidised and the less reactive metal is reduced.

57
Q

What is a displacement reaction?

A

A displacement reaction is where a more reactive metal displaces a less reactive metal.

58
Q

What will happen if you put a less reactive metal into a solution of a more reactive metal salt?

A

Nothing will happen

59
Q

What is a metal ore?

A

A metal ore is a rock which contains enough metal to make it economically worthwhile to extract.

60
Q

Give an example of an ore.

A

Aluminium ore is known as bauxite (aluminium oxide)

61
Q

What are metal ores combined with?

A

Oxygen

62
Q

How does extracting metals using carbon work?

A

Metal can be extracted from an ore by reduction using carbon. The carbon bonds with the oxygen (making the metal an oxide) and forms carbon dioxide. This is a by product of the reaction, leaving pure metal.

63
Q

Finish the sentence: When an ore is reduced, …

A

…oxygen is removed from it.

64
Q

Where is carbon extraction took place.

A

In a blast furnace.

65
Q

What are the two methods of purifying a metal?

A

Carbon reduction and Electrolysis.

66
Q

Why are metals below CARBON in the reactivity series extracted using carbon reduction?

A

Because carbon is more reactive, it takes the oxygen away from the metallic ore (displacement reaction).

67
Q

Why are metals above CARBON in the reactivity series extracted using electrolysis?

A

Because the carbon will not be able to displace the oxygen as the other metal is more reactive and carbon isn’t reactive enough.

68
Q

What is electrolysis?

A

Electrolysis is the separation of metals using electricity.

69
Q

Explain the stages of electrolysis.

A

Molten metal ore (melted) is put into a steal case with a NEGATIVE CATHODE and POSITIVE ANODE. The metal and oxygen are no longer bonded just in contact with each other. The metal ion (positive ion) is attracted to the negative cathode. The oxygen ion (negative ion) is attracted to the positive anode. They are separated and pure metals are formed.

70
Q

Pros of using carbon reduction over electrolysis.

A

Electrolysis requires a lot of electricity in order for it to be successful and is therefore very expensive to do.

71
Q

Cons of using carbon reduction over electrolysis.

A

Electrolysis is a lot easier and more successful.

72
Q

Why does extracting raw materials use large amounts of energy?

A

Because fossil fuels are burnt in order to power it.

73
Q

Why is it important to conserve fossil fuels?

A

Because they are a non-renewable source and are running out.

74
Q

Why are metals similar to fossil fuels?

A

Because they are both a non-renewable sources.

75
Q

Where are transition metals found in the periodic table?

A

They sit in the middle section and do not have a group.

76
Q

Give some properties of transition metals.

A

Hard, strong, shiny, conductor of heat and electricity, have high melting points and high densities.

77
Q

Give an example of a transition metal and what it is used for.

A

Iron is used as a catalyst in the Haber process for making ammonia.

78
Q

What are alloys?

A

An alloy is a metal made by combining two or more metallic elements to change its properties; either making it stronger, more resistant to corrosion, more conductive of electricity etc.

79
Q

Why are alloys stronger than pure metals?

A

Pure metals only contain one type of atom. These layers of ions can slide over each other making it weak. When another compound is added in, it slots between the layers and stops the sliding (bending) of the metal.

80
Q

What does the alloy steel compose of?

A

Steel is iron atoms with carbon atoms in between. The formula is Fe.

81
Q

How does carbon also help iron?

A

A small amount of carbon in iron means that it becomes much more resistant to corrosion.

82
Q

What type of reaction is rusting?

A

A redox reaction.

83
Q

What is corrosion?

A

Corrosion is when oxygen and water react with a metal to form its metal oxide.

84
Q

What is rusting?

A

The corrosion of iron.

85
Q

Give one way of preventing rusting.

A

Galvanising is an example of sacrificial protection - it involves placing a more reactive metal with the iron.

Year 9 EOY Revision (5 decks)

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