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Chemistry > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

What happens to ionisation energy as you go down the group?

A

It decreases

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2
Q

Why does the ionisation energy decrease as you go down the group?

A
  • Each element has an extra electron shell
  • Extra shells shield attraction from the nucleus
  • Outer electrons are further away from the nucleus
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3
Q

As ionisation energy decreases down the group, why does this mean that the reactivity in group 1 increases as you go down the group?

A

It is easier for the elements to lose their outer electron when they react and form a +1 ion.

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4
Q

What ions do group 2 elements form?

A

+2 ions

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5
Q

When group 2 elements react with water, what do they form?

A

Metal hydroxide + hydrogen

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6
Q

What is the chemical formula of calcium hydroxide?

A

Ca(OH)2

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7
Q

When group 2 elements burn in oxygen, what is the only product formed?

A

Solid white oxides

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8
Q

What is the chemical formula of calcium oxide??

A

CO

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9
Q

When group 2 elements react with chlorine, what do they form?

A

Chlorides

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10
Q

What is the chemical formula of calcium chloride?

A

CaCl2

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11
Q

Why are metal hydroxides strongly alkaline?

A

Because of the OH- ions

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12
Q

Are the oxides of he group 2 elements soluble?

A

Yes, and it increases as you go down group 2

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13
Q

Why do the group 2 oxides form more strongly alkaline solutions as you go down the group?

A

Because the hydroxides get more soluble

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14
Q

As they are bases, what are the oxides and hydroxides of group 2 metals able to do?

A

Neutralise dilute acids, and form salts

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15
Q

When metal hydroxides react with water, what do they form?

A

Metal hydroxides

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16
Q

When metal oxides react with dilute HCl, what do they form?

A

Metal chlorides and water

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17
Q

When metal hydroxides react with HCl, what do they form?

A

Metal chlorides and water

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18
Q

What happens to the solubility of group 2 hydroxides as you go down the group?

A

The solubility increases

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19
Q

What is a sulfate ion?

A

SO4 2-

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20
Q

What happens to the solubility of group 2 sulfates as you go down the group?

A

The solubility decreases

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21
Q

What is thermal decomposition?

A

When a substance breaks down (decomposes) when heated.

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22
Q

What is the relationship between how thermally stable a compound is and how much heat is required to break it down?

A

The more thermally stable a compound is, the more heat is required to break it down

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23
Q

What are anions?

A

Negative ions

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24
Q

What happens to large negative ions when in the presence of a cation?

A

They can be made unstable, distorting the anion

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25
Q

What is the relationship between the amount of distortion and the stability of the compound?

A

The greater the distortion, the less stable the compound

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26
Q

Why do large cations cause less distortion than small cations?

A

Because large cations have lower charge density

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27
Q

Why do carbonate/nitrate compounds become more stable as you go down the group?

A

Because the larger the cation, the lower the charge density, so the less distortion

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28
Q

What is a carbonate ion?

A

CO3 2-

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29
Q

What is a nitrate ion?

A

NO3 2-

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30
Q

Are group 1 carbonates thermally stable?

A

Yes, you can’t decompose them with a bunsen burner

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31
Q

What do group 1 nitrates decompose to form?

A

The metal nitrite and oxygen

32
Q

What is the chemical formula of magnesium nitrite?

A

MNO2

33
Q

What do group 2 carbonates decompose to form?

A

Metal oxides and carbon dioxide

34
Q

What do group 2 nitrates decompose to form?

A

Metal oxide, nitrogen dioxide, and oxygen

35
Q

How do you test the thermal stability of nitrates?

A
  • How long it takes for an amount of oxygen to be produced

- How long it takes for NO2 to be produced (brown gas)

36
Q

How do you test the thermal stability of carbonates?

A

-How long it takes for carbon dioxide to be produced

37
Q

What is the flame colour of lithium?

A

Red

38
Q

What is the flame colour of sodium?

A

Orange/yellow

39
Q

What is the flame colour of potassium?

A

Lilac

40
Q

What is the flame colour of rubidum?

A

Red

41
Q

What is the flame colour of caesium?

A

Blue

42
Q

What is the flame colour of calcium?

A

Brick-red

43
Q

What is the flame colour of strontium?

A

Crimson

44
Q

What is the flame colour of barium?

A

Green

45
Q

How do you do a flame test?

A
  • Mix with HCl

- Heat with a piece of platinum or nichrome wire

46
Q

What happens to the electronegativity values as you go up group 2?

A

They increase

47
Q

What colour is bromine in water?

A

Yellow/orange

48
Q

What colour is iodine in water?

A

Brown

49
Q

What colour is bromine in hexane?

A

Orange/red

50
Q

What colour is iodine in hexane?

A

Pink/violet

51
Q

What happens to the reactivity of halogens as you go down the group?

A

They decrease in reactivity

52
Q

Why do halogens decrease in reactivity as you go down the group?

A
  • They react by gaining an electron
  • Their radius and number of shells gets bigger as you go down the group, so it is harder for larger atoms to attract an electron
53
Q

What happens to the melting and boiling points of halogens as you go down the group?

A

Increase as the London forces between the molecules get stronger as you go down the group

54
Q

If bromide is displaced and bromine is formed, what colour will the mixture turn?

A

Orange

55
Q

If iodide is displaced and iodine is formed, what colour will the mixture turn?

A

Brown

56
Q

When halogens react with group 1 and 2 metals, what is produced?

A

A salt, e.g. LiF and MgCl2

57
Q

How do you make bleach?

A

2NaOH + Cl2 —> NaClO +NaCl +H20

58
Q

When you mix chlorine with water, what is produced?

A

A hypochlorous acid HClO

59
Q

What does Hypochlorous acid ionise to make?

A

Chlorate ions which kill bacteria

60
Q

What happens to the reducing power of halides as you go down the group?

A

The reducing power increases as it is easier for them to lose their outer electron

61
Q

When a potassium halide reacts with sulfuric acid, what is produced?

A

Hydrohalide + KHSO4

62
Q

What happens when KBr reacts with sulfuric acid?

A

KHSO4 + HBr

63
Q

What happens when potassium iodide reacts with sulfuric acid?

A

KHSO4 + hydrogen iodide

64
Q

What is KHSO4?

A

Potassium bisulfate

65
Q

What are the main properties of hydrogen halides?

A
  • Acidic gases

- Can dissolve in water to produce misty fumes of acidic gases

66
Q

How do you test for halides?

A
  • Add dilute nitric acid to remove ions that interfere with the reaction
  • Add silver nitrate solution and a precipitate of the silver halide is formed
67
Q

What colour is the precipitate of AgCl?

A

White

68
Q

What colour is the precipitate of AgBr?

A

Cream precipitate

69
Q

What colour is the precipitate of AgI?

A

Yellow

70
Q

What happens when AgCl is added to ammonia?

A

A colourless solution is formed

71
Q

What happens when AgBr is added to ammonia?

A

Dissolves in concentrated ammonia to give a colourless solution

72
Q

What happens when AgI is added to ammonia?

A

Precipitate does not dissolve

73
Q

How do you test for carbonates?

A

-With dilute hydrochloric acid, carbonates will fizz because they give off carbon dioxide

74
Q

How do you test for carbon dioxide?

A

Calcium dioxide turns limewater cloudy

75
Q

How do you test for sulfates?

A
  • Add dilute HCl followed by barium chloride solution.

- If a white precipitate of barium sulfate is formed, the original compound contained a sulfate

76
Q

How do you test for ammonium compounds?

A

It turns red litmus paper blue

Add sodium hydroxide to the substance X and gently heat the mixture. If ammonia is given off there is ammonia present

Chemistry (25 decks)

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