2.3 Group 7 Flashcards

1
Q

What is the trend in bpt down group 7? Why?

A

Increases down the group.
Because: size of atom increases as more occupied electron shells —> stronger Van de Waals forces of attraction between molecules, take more energy to break

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2
Q

What is the trend in electronegativity down Group 7? Why?

A

Decreases
Because: more occupied electron shells —> greater atomic radius and outer electrons are further from the positive charge of the nucleus —> lower force of attraction between the nucleus and electron pair in the covalent bond

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3
Q

What do you use to test for halide ions

A

Acidified AgNO3

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4
Q

Why do you add HNO3 ? Why not HCl?

A

To remove CO3 2-
Adding HCl would add Cl- ions creating a false positive

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5
Q

Result and equation for Cl- test?

A

Ag+ + Cl- —> AgCl (s)

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6
Q

What is the result and equation for the test for Br

A

Cream ppt
Ag+ + Br- —> AgBr (s)

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7
Q

What is the result and equation for the test for I-

A

Yellow ppt
Ag+ + I- —> AgI (s)

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8
Q

What happens (+ equations) to each of the silver halide precipitates when dilute/conc ammonia are added ?

A

AgCl (s) - dissolves in both conc and dilute ammonia
AgCl (s) + 2NH3 —> [Ag(NH3)2]+ (aq) + Cl-
AgBr (s) - dissolves in conc ammonia
AgBr (s) + 2NH3 —> [Ag(NH3)2]+ (aq) + Br-
AgI (s) will not dissolve in either

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9
Q

What is the trend in oxidising ability down Group 7? Why?

A

Decreases down the group (Cl best, I worst)
Because: Cl has fewest occupied electron shells, greatest force of attraction between outer electrons and nucleus, easiest to gain electrons and be reduced —> best oxidising agent

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10
Q

Write the equation for Cl2 oxidising 2I-

A

Cl2 + 2I- —> 2Cl- + I2

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11
Q

What is the trend in reducing ability down Group 7?

A

Increases down the group (Cl worst, I best)
Because: I- has the most occupied electron shells, so outer electrons are further from the nucleus, weakest force of attraction between positive charge of nucleus and outer electrons —> easiest to be oxidised and lose electrons —> best reducing agent

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12
Q

What products are formed when I reacts with H2SO4? [4]

A

H2SO4 + 2I- —> SO4 2- + 2HI
H2SO4 + 2H+ + 2I- —> SO2 + I2 + 2H2O (SO2 is a choking gas with a pungent smell)
H2SO4 + 6H+ + 6I- —> S + 3I2 + 4H2O (S is a yellow solid)
H2SO4 + 8H+ 8I- —> H2S + 4I2 + 4H2O (H2S smells of rotten eggs)

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13
Q

What are the products of Br + H2SO4?

A

HBr and SO2

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14
Q

Does Cl- reduce H2SO4?

A

No, not a powerful enough reducing agent, only HCl is formed

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15
Q

Why is Chlorine added to drinking water? Why is it safe?

A

Forms ClO- ions which kill all microorganisms in the water.
Once it has done it’s job, little remains, and the health benefits outweigh the risks of using it

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16
Q

What are the potential risks of adding chlorine to water

A

Chlorine is toxic and damages the respiratory system in large enough quantities; can form carcinogens with hydrocarbons

17
Q

Why is Ozone not used to purify water in the UK?

A

More expensive than Chlorine, evaporates from water more quickly

18
Q

What is the reaction of Cl2 with water?

A

Cl2 (g) + H2O (l) —> HClO (aq) + HCl (aq)

19
Q

What type of reaction is Chlorine with water?

A

Disproportionation; Chlorine is both oxidised and reduced

20
Q

What are the two forms of the Chlorate ion?

A

ClO- is Chlorate (I)
[ClO3]- is Chlorate (V)

21
Q

What is the equation for making bleach?

A

Cl2 + 2NaOH —> NaCl + NaClO + H2O

22
Q

Give the equation for the reaction of chlorine and water in the presence of sunlight

A

2Cl2 + 2H2O —> 4HCl + O2

23
Q

What is desalination?

A

Converts saltwater into clean, potable water
Either by reverse osmosis (using a smart membrane) or by vacuum distillation at low temperature and low pressure

24
Q

What are the advantages and disadvantages of desalination?

A

Advantages - Safe, clean, drinkable water produced in places where it might not otherwise be available
Disadvantages - uses lots of energy, reverse osmosis has low efficiency, can disturb marine ecosystems