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Chemistry > Section 2: Chemistry of the Elements > Flashcards

Section 2: Chemistry of the Elements Flashcards

1
Q

Do metals create acidic or basic oxides?

A

Basic

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2
Q

Do non-metals create acidic or basic oxides?

A

Acidic

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3
Q

What are group 1 elements called?

A

The alkali metals

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4
Q

What happens in terms of properties as you go down the group 1 metals?

A

1) melting point decreases

2) reactivity increases

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5
Q

Why does reactivity increase down the group 1 metals?

A

1) more shells
2) electron in outer shell is further away from the pull of the nucleus
3) easier to lose the electron

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6
Q

Describe the reaction of lithium with water

A

1) floats
2) doesn’t melt
3) doesn’t catch fire
4) creates basic solution (lithium hydroxide)

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7
Q

Describe the reaction of sodium with water

A

1) floats
2) melts
3) doesn’t catch fire
4) makes basic solution (sodium hydroxide)

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8
Q

what observations can be made during the reaction of potassium and water?

A

1) effervescence/fizzing/bubbles
2) potassium moves/darts/floats
3) potassium leaves white trail
4) potassium forms into a ball
5) potassium becomes smaller/disappears
6) (lilac) flame

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9
Q

What is chlorine like at room temperature?

A

A pale green gas

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10
Q

What is bromine like at room temperature?

A

Orange liquid

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11
Q

What is iodine like at room temperature?

A

Dark grey solid

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12
Q

What is the trend in physical properties down group 7?

A

1) melting point increases

2) reactivity decreases

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13
Q

What colour is chlorine when dissolved in water and in hexane?

A

Water: colourless
Hexane: pale green

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14
Q

What colour is bromine when dissolved in water and in hexane?

A

Water: orange
Hexane: orange

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15
Q

What colour is iodine when dissolved in water and in hexane?

A

Water: orange
Hexane: purple

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16
Q

What is the difference between hydrogen chloride gas and hydrochloric acid?

A

Hydrogen chloride gas is a covalently bonded. When it is dissolved in water it becomes hydrochloric acid and splits into H+ ions and Cl- ions (the H+ ions make it acidic)

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17
Q

Why is hydrogen chloride gas acidic in water but not in methyl benzene?

A

When hydrogen chloride dissolved in methyl benzene it doesn’t disassociate (split up) so since there are no H+ ions the solution is neutral

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18
Q

What is the trend in reactivity of halogens as the number of shells increases?

A

Distance between outer shell and nucleus increases
Electrostatic attraction if nucleus and electron it wants to gain is weaker
Harder to gain electrons
Reactivity decreases

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19
Q

If chlorine is added to sodium bromide, will a reaction occur?

A

Yes, as chlorine is more reactive it will displace the bromide ion

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20
Q

What type of reaction are halogen displacement reactions?

A

redox reactions

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21
Q

What percentage of air is nitrogen?

A

78%

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22
Q

What percentage of air is oxygen?

A

21%

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23
Q

What percentage of air is Argon?

A

0.9%

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24
Q

What percentage of air is carbon dioxide?

A

0.04%

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25
Q

How do you prepare oxygen in a lab?

A

Hydrogen peroxide (+manganese dioxide) —> water + oxygen

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26
Q

What is the chemical equation for the preparation of oxygen in a lab?

A

2H2O2 —> 2H2O + O2

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27
Q

How do you prepare carbon dioxide in a lab?

A

Calcium carbonate + hydrochloric acid —> calcium chloride + carbon dioxide + water

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28
Q

what is the reaction of magnesium with oxygen in air?

A

Oxygen + Magnesium —> Magnesium Oxide (white solid)

29
Q

what is the reaction of carbon with oxygen in air?

A

Oxygen + Carbon —> Carbon Dioxide

30
Q

what is the reaction of sulfur with oxygen in air?

A

Oxygen + Sulphur —> Sulphur Dioxide

31
Q

What can you heat to to give carbon dioxide and a metal oxide?

A

Metal carbonates break down into carbon dioxide and metal oxide in thermal decomposition

32
Q

Why is carbon dioxide used in carbonating drinks?

A

Carbon dioxide is soluble in water

33
Q

Why is carbon dioxide used in fire extinguishers?

A

Because it is more dense than air so it sinks below lighter gases such as oxygen, covering a fire and keeping oxygen out

34
Q

What are the products of sulphuric acid and metals reacting?

A

Metal sulphate and hydrogen gas

35
Q

What are the products of metal and hydrochloric acid reacting?

A

Metal chloride and hydrogen gas

36
Q

How do you test for the presence of water?

A

Use anhydrous copper sulphate which turns from white to blue in the presence of water

37
Q

what is the order of metals in the reactivity series?

A 
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
(carbon)
Zinc
Iron
(hydrogen)
Copper
Silver
Gold
38
Q

Which is the least reactive metal to react with water?

39
Q

Which is the least reactive metal to react with steam?

40
Q

What is the least reactive metal to react with hydrochloric acid or sulphuric acid?

41
Q

what is an oxdising agent?

A

a substance which oxidises something else (provides the oxygen)

42
Q

what is a reducing agent?

A

a substance which reduces something else (takes the oxygen)

43
Q

what is rust?

A

Hydrated iron (III) oxide

44
Q

What is the colour of flame in flame test for Li+?

45
Q

What is the colour of flame in flame test for Na+?

46
Q

What is the colour of flame in flame test for K+?

47
Q

What is the colour of flame in flame test for Ca 2+?

48
Q

What type of flame is used during flame tests?

A

Blue/roaring flame so doesn’t interfere with colour reading

49
Q

How do you test for ammonia?

A

Add sodium hydroxide solution and warm. It will turn damp red litmus paper blue and smell of ammonia

50
Q

How do you test for Cu2+ ions?

A

1) Add sodium hydroxide solution.

2) Forms blue precipitate (copper hydroxide)

51
Q

How do you test for Fe2+ ions?

A

1) add sodium hydroxide solution

2) Forms green precipitate

52
Q

How do you test for Fe3+ ions?

A

1) add sodium hydroxide solution

2) Forms red/brown precipitate

53
Q

How do you test for Cl- ions?

A

Add dilute nitric acid and then silver nitrate solution and then a white precipitate will form (silver chloride)

54
Q

How do you test for Br- ions?

A

Add dilute nitric acid and then silver nitrate solution and then a cream precipitate will form

55
Q

How do you test for I- ions?

A

Add dilute nitric acid and then silver nitrate solution and then a yellow precipitate will form

56
Q

How do you test for sulphate ions?

A

Add dilute hydrochloric acid and then barium chloride and a white precipitate forms (barium sulphate)

57
Q

How do you test for carbonate ions?

A

Add dilute acid and then bubbles of carbon dioxide will be produced

58
Q

How do you test for hydrogen?

A

Lit splint burns with a squeaky pop

59
Q

How do you test for oxygen?

A

Relights a glowing splint

60
Q

How do you test for carbon dioxide?

A

Bubble through line water and it will turn milky

61
Q

How do you test for ammonia gas?

A

Turns damp red litmus paper blue

62
Q

How do you test for chlorine gas?

A

bleaches damp litmus white

63
Q

What colour would you predict astatine to be?

64
Q

What colour is fluorine gas?

A

Pale yellow

65
Q

what are the conditions required for rusting to occur?

A

1) oxygen

2) water

66
Q

what speeds up the process of rusting?

67
Q

how does a coat of zinc protect iron from rusting?

A

1) zinc corrodes/oxidises/reacts in preference to
iron
2) because zinc is more reactive than iron

68
Q

how can carbon dioxide be collected?

A

1) over water
2) downward delivery in air
3) in a gas syringe

69
Q

why is potassium more reactive than lithium?

A

1) potassium loses its outer electron more easily
2) because it is further from the attraction of the nucleus
3) and therefore less strongly attracted
to the nucleus

Chemistry (5 decks)

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