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Chemistry - norm > 2 - Chemistry of the Elements > Flashcards

2 - Chemistry of the Elements Flashcards

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1
Q

What are periods?

A
  • Rows across

- Properties change as you go along

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2
Q

What are groups?

A
  • Columns going across
  • Similar chemical properties because of the electrons on the outer shell
  • Gradually change as you go down and the atomic number increases
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3
Q

What are metals in the periodic table?

A

The majority (including aluminium)

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4
Q

What are non-metals in the periodic table?

A

The minority (including oxygen and boron)

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5
Q

Group 0 properties

A
  • Noble gases
  • All inert
  • Full outer shell of electrons
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6
Q

Group 1 properties

A
  • The alkali metals
  • Reactivity increases going down
  • All react similarly with water
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7
Q

How do group 1 react with water?

A

e.g. sodium + water –> sodium hydroxide + hydrogen

solid + liquid –> aqueous + gas

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8
Q

Describe an experiment to show alkali metals reacting with water

A
  • Put a small lump in a beaker with water
  • Universal indicator shows the colour change (green to blue to purple (alkaline))
  • Use a stopwatch to time how long it takes to fizz out
  • As you go down the group it will react more vigorously and quicker
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9
Q

Describe an experiment to show alkali metals reacting with water

A
  • Put a small lump in a beaker with water
  • Universal indicator shows the colour change (green to blue to purple (alkaline))
  • Use a stopwatch to time how long it takes to fizz out
  • As you go down the group it will react more vigorously and quicker
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10
Q

Group 7 properties

A
  • Halogens
  • Colour gets darker as you go down
  • Solidify as you go down
  • boiling point increases
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11
Q

Group 7 properties

A
  • Halogens
  • Colour gets darker as you go down
  • Solidify as you go down
  • boiling point increases
  • Reactivity decreases (shell with missing electron in further away from nucleus)
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12
Q

What happens to hydrogen chloride gases in water?

A
  • It dissociates
  • The ions split into H+ ions and Cl- ions
  • Hydrochloric acid is formed
  • This doesn’t happen in methylbenzene because it isn’t acidic
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13
Q

What are the state symbols in a halogen displacement reaction?

A

All aqueous

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14
Q

What is an oxidising agent?

A

Something in a reaction that accepts electrons and gets reduced (the more reactive element is normally the oxidising agent)

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15
Q

What is a reducing agent?

A

Something that loses electrons and gets oxidised (the less reactive element is normally the reducing agent)

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16
Q

What is a redox reaction?

A

A reaction where reduction and oxidation occur at the same time

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17
Q

What is a redox reaction?

A

A reaction where reduction and oxidation occur at the same time

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18
Q

What happens when chlorine water is added to potassium bromide solution

A
  • Turns from colourless to orange

-

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19
Q

What happens when chlorine water is added to potassium bromide solution

A
  • Turns from colourless to orange
  • Displacement reaction
  • Potassium chloride and bromine is formed
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20
Q

What happens when chlorine water is added to potassium iodide solution?

A
  • Turns from colourless to brown
  • Displacement reaction
  • Potassium chloride and iodine is formed
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21
Q

What happens when bromine water is added to potassium iodide solution?

A
  • Turns from colourless to brown
  • Displacement reaction
  • Potassium bromide and iodide is formed
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22
Q

What does an acid + metal make?

A

Acid + metal –> salt + hydrogen

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23
Q

What does a metal + water make?

A

Metal + water –> metal hydroxide + hydrogen

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24
Q

What is the reactivity series?

A

Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium, Carbon, Zinc, Iron, Hydrogen, Copper, Silver, Gold

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25
Q

What is rust?

A

The corrosion of iron or steel when it meets oxygen (from the air) and water
- It is an oxidation reaction (the iron gains oxygen)

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26
Q

What is the symbol equation for rust?

A

iron + oxygen + water –> hydrated iron(III) oxide

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27
Q

What are ways to prevent rusting?

A
  • Barrier methods

- Sacrificial method

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28
Q

What is the barrier method?

A
  • Coating the iron to prevent oxygen/water reacting with it
  • Plastic/coating with plastic is often used for big and small structures
  • Oiling/greasing is used when moving parts are involved
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29
Q

What is the barrier method?

A
  • Coating the iron to prevent oxygen/water reacting with it
  • Plastic/coating with plastic is often used for big and small structures
  • Oiling/greasing is used when moving parts are involved
30
Q

What is the sacrificial method?

A
  • Using a more reactive metal to corrode instead of iron
  • Zinc is often used
  • Spraying zinc or putting big blocks bolted to it
31
Q

What is galvanising?

A

Spraying zinc in sacrificial method

32
Q

How much nitrogen is in the air?

A

78%

33
Q

How much oxygen is in the atmosphere?

A

21%

34
Q

How much argon is in the atmosphere?

A

1%

35
Q

How much carbon dioxide is in the atmosphere?

A

0.04%

36
Q

What are the main gases in the atmosphere?

A

Nitrogen, oxygen, argon and carbon dioxide

37
Q

Describe an experiment using copper to show there is oxygen in the air

A
  • ## Put excess copper in a tube and pass air over it using two syringes
38
Q

Describe an experiment using copper to show there is oxygen in the air

A
  • Put excess copper in a tube and pass air over it using two syringes
  • Make marks on the syringes so you can see how much O2 is used up
  • Heat the copper in the middle and oxygen will be lost
  • If you start with 100cm3 of air you will end up with about 80cm3 showing 20% of air must be oxygen
39
Q

Describe an experiment to show oxygen in air using iron or phosphorus

A
  • Iron reacts with air to form rust
  • Soak some iron wool with acetic acid (the catalyst) the put the wool in a test tube with your thumb over the end in a beaker of water
  • Over time the water level will rise
  • This is to take up the space left by oxygen reacting
  • To work out the amount lost mark the start and end position of the water
  • About 20% oxygen should be used
40
Q

Describe an experiment to make oxygen in a lab

A
  • Through the decomposition of hydrogen peroxide (H2O2)
  • Decomposes to make oxygen and water
  • Manganese (VI) oxide can be used as a catalyst
  • It can be collected over water or in a gas syringe
41
Q

What colour is the magnesium flame in air?

A
  • Bright white flame
  • White precipitate
  • Will be alkaline when dissolved in water
42
Q

What colour is the carbon flame in air?

A
  • Orangey/yellow flame
  • Produces a carbon dioxide gas
  • Slightly acidic in water
43
Q

What colour is the sulphur flame in air?

A
  • Pale blue flame
  • Produces sulphur dioxide
  • Acidic in water
44
Q

Describe an experiment to make carbon dioxide

A
  • Calcium carbonate (marble chips) put in the bottom of a flask with dilute hydrochloric acid
  • The dilute HCl reacts with the calcium carbonate to produce calcium chloride, water and CO2 gas
  • Can be collected in a gas syringe or a downward delivery
45
Q

When do you use a downward delivery?

A

When the gas is heavier than air (e.g. CO2, Cl2)

46
Q

When do you use an upward delivery?

A

When the gas is lighter than air (e.g. H2)

47
Q

When do you use an upward delivery?

A

When the gas is lighter than air (e.g. H2)

48
Q

Describe an experiment to make carbon dioxide using thermal decomposition

A
  • Heating green copper carbonate

- Black copper oxide and carbon dioxide gas will be collected

49
Q

When is carbon dioxide used?

A
  • In fizzy drinks
  • Reacted with water to make carbonic acid
  • Used in fire extinguishers as it is more dense than air so sinks into the flame and stops oxygen getting to it
  • Used mainly for putting out electrical fires
50
Q

Why is carbon dioxide a greenhouse gas?

A
  • It absorbs most of the heat that is radiated out into space and radiates it back to earth which warms it up
  • Released in deforestation and burning fossil fuels
51
Q

What colour is a lithium flame?

A

Crimson red

52
Q

What colour is a sodium flame?

A

Yellow/orange

53
Q

What colour is a potassium flame?

A

Lilac

54
Q

What colour is a calcium flame?

A

Brick red

55
Q

How do you do a flame test?

A
  • Clean a platinum wire loop by dipping it in dilute HCl

- Hold it to the flame

56
Q

What colour is a copper (II) precipitate?

A
  • Blue

- Cu2+(aq) + 2OH(aq)- –> Cu(OH)2(s)

57
Q

What colour is an iron (II) precipitate?

A
  • Sludgy green

- Fe2+(aq) + 2OH-(aq) –> Fe(OH)2(s)

58
Q

What colour is an iron (III) precipitate?

A
  • Red/brown

- Fe3+(aq) + 3OH-(aq) –> Fe(OH)3(s)

59
Q

What is a test for ammonia?

A
  • Damp red litmus paper will turn blue

- To test for ammonium ions add sodium hydroxide and ammonia gas will be given off

60
Q

What is a test for ammonia?

A
  • Damp red litmus paper will turn blue
  • To test for ammonium ions add sodium hydroxide and ammonia gas will be given off
  • Strong smell
61
Q

How can you test for carbonates?

A
  • Add dilute HCl

- Carbon dioxide will be released

62
Q

How can you test for sulphates?

A
  • Sulphate ions produce a white precipitate
  • Add dilute HCl
  • Add barium chloride solution
  • A white precipitate will form
  • (The HCl removes any carbonate or sulphite ions)
63
Q

How can you test for halides?

A
  • Add nitric acid

- Add silver nitrate solution

64
Q

What colour is a silver chloride precipitate?

A

White

65
Q

What colour is a silver bromide precipitate

A

Cream

66
Q

What colour is a silver iodide precipitate?

A

Yellow

67
Q

How can you test for chlorine gas?

A

Bleaches damp litmus paper

68
Q

How can you test for oxygen?

A

Relights a glowing splint

69
Q

How can you test for carbon dioxide?

A

Turns limewater cloudy

70
Q

How can you test for hydrogen?

A

Makes a ‘squeaky pop’ with a lightened splint

71
Q

How can you test for water chemically?

A
  • Wet copper(II) sulphate is blue
  • If you heat the water off it’ll turn white
  • Add water it will turn blue again
72
Q

How can you test for water physically?

A
  • Boils at 100*C

- Freezes at 0*C

Chemistry - norm (6 decks)

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