2.3 Group 7 the halogens Flashcards

1
Q

Describe the trend in atomic radius down the group

A

Atomic radius increases down the group.

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2
Q

Why does atomic radius increase down the group

A

The atoms increase in size due to additional electron shells.

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3
Q

Describe the trend in reactivity down the group

A

Reactivity decreases.

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4
Q

Why does reactivity decrease down the group

A
  • Group 7 elements need to gain an electron
  • Weaker attraction between nucleus and outer shell due to greater atomic radius and increased shielding
  • Harder to attract an electron, so reactivity decreases
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5
Q

Describe the trend in first ionisation energy down the group

A

Decreases down the group.

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6
Q

Why does first ionisation energy decrease down the group

A
  • Weaker attraction between nucleus and electron being removed due to a greater atomic radius and increased shielding
  • Less energy required to remove the electron
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7
Q

Describe the trend in boiling point down the group

A

Boiling point increases down the group

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8
Q

Explain why boiling point increases down the group

A
  • Group 7 elements are simple covalent molecules held together by van der waals forces
  • Down the group, the Ar increases/more electrons
  • Causes van der waals forces to be stronger, so more energy required to overcome them
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9
Q

Describe the trend in oxidising power down the group

A

Oxidising power decreases down the group

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10
Q

Why does oxidising power decrease down the group

A
  • Weaker attraction between nucleus and outer shell
  • Atoms less able to attract an electron (harder to be reduced)
  • Causes oxidising power to decrease
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11
Q

Describe and explain the trend in reducing power down the group

A
  • Reducing power increases down the group
  • Atomic radius increases, so outer electron more easily lost as there is a weaker attraction between the nucleus and outer shell
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12
Q

What is the equation for the reaction between fluoride ions and sulfuric acid

A

NaF + H2SO4 => NaHSO4 + HF

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13
Q

What is the equation for the reaction between chloride ions and sulfuric acid

A

NaCl + H2SO4 => NaHSO4 + HCl

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14
Q

What are the equations for the 2 reactions between bromide ions and sulfuric acid

A

NaBr + H2SO4 => NaHSO4 + HBr

2HBr + H2SO4 => Br2 + SO2 + 2H2O

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15
Q

What are the equations for the 3 reactions between iodide ions and sulfuric acid

A

NaI + H2SO4 => NaHSO4 + HI

2HI + H2SO4 => I2 + SO2 + 2H2O

6HI + SO2 => H2S + 3I2 + 2H20

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16
Q

What is the relationship between reducing power and length of reaction

A

The greater the reducing power, the longer the reaction as the halide is powerful enough to reduce more species.

17
Q

What is used to test for halide ions

A

Acidified silver nitrate and ammonia.

18
Q

What happens when silver nitrate is added to chloride ions

A

A white precipitate forms (AgCl).

19
Q

What happens when silver nitrate is added to bromide ions

A

A cream precipitate forms (AgBr).

20
Q

What happens when silver nitrate is added to iodide ions

A

A yellow precipitate forms (AgI).

21
Q

What happens when dilute ammonia (NH3) is added to chloride ions

A

The precipitate dissolves.

22
Q

What happens when dilute ammonia (NH3) is added to iodide ions

A

No change.

22
Q

What happens when dilute ammonia (NH3) is added to bromide ions

A

No change.

23
Q

What happens when concentrated ammonia (NH3) is added to chloride ions

A

The precipitate dissolves.

24
Q

What happens when concentrated ammonia (NH3) is added to bromide ions

A

The precipitate dissolves.

25
Q

What happens when concentrated ammonia (NH3) is added to iodide ions

A

No change.

26
Q

What is a disproportionation reaction

A

A reaction in which the same species is both oxidised and reduced.

27
Q

What is the equation for the reaction between chlorine and cold alkali

A

Cl2(aq) + 2NaOH(aq) => NaCl(aq) + NaClO(aq) + H2O(l)

28
Q

What is the equation for the reaction between chlorine and water

A

Cl2(aq) + H2O(l) => HCl(aq) + HClO(aq)

29
Q

What is the equation for the reaction between chlorine and sunlight (UV light)

A

2Cl2 + 2H2O => 4HCl + O2

30
Q

How do you test for sulfate ions (SO4^2-)

A

Adding BaCl2, reacts to form a while precipitate.

31
Q

How do you test for hydroxide ions (OH-)

A

Use red litmus paper which will turn blue.

32
Q

How do you test for carbonate ions (CO3^2-)

A
  • When you add an acid (e.g. HCl), the substance containing the carbonate ions will fizz and CO2 is given off
  • This can be collected and bubbled through limewater which will turn cloudy