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A-level chemistry > Group 7 > Flashcards

Group 7 Flashcards

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1
Q

describe the trend in atomic radius

A
  • atomic radius increases down the group
  • due to additional electron shells
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2
Q

describe the trend in oxidising power

A
  • oxidising power decreases down the group
  • increase in shielding + atomic radius makes it harder to attract electrons
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3
Q

describe the trend in boiling and melting temperature

A
  • melting and boiling temperature increases down the group
  • due to increase in relative atomic mass, increasing strength of London forces in the simple covalent molecule so more energy is required to overcome them
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4
Q

describe the trend in reactivity

A
  • reactivity decreases down the group
  • due to increase in atomic radius
  • due to additional electron shells the positive attraction of the nucleus decreases
  • harder to attract an electron
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5
Q

describe the trend in electronegativity

A
  • electronegativity decreases down the group
  • atomic radius + electron shielding increase
  • electrons are more easily removed due to less strong attraction to the nucleus
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6
Q

describe the trend in reducing power

A
  • reducing power increases down the group
  • electrons are easier to lose from larger ions
  • due to increased shielding and atomic radius
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7
Q

what is involved in a redox reaction

A

halide + sulfuric acid

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8
Q

NaF + H2SO4 –>

A

NaHSO4 + HF

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9
Q

NaCl + H2SO4 –>

A

NaHSO4 + HCl

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10
Q

what are HCl, HF, HI and HBr

A

misty fumes

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11
Q

why is there only one reaction with HF and HCl when reacting with H2SO4

A

because they aren’t strong enough to reduce the H2SO4 any further so there are no further reactions

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12
Q

all reactions of NaBr + H2SO4

A

NaBr + H2SO4 –> NaHSO4 + HBr
2HBr + H2SO4 –> Br2 + SO2 + 2H2O

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13
Q

What is Br2

A

orange fumes

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14
Q

what is SO2

A

choking fumes

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15
Q

describe the reaction between HBr and H2SO4

A

HBr reduces HsSO4

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16
Q

all reactions of NaI + H2SO4

A

NaI + H2SO4 –> NaHSO4 + HI
2HI + H2SO4 –> I2 + SO2 + 2H20
6I2 + SO2 –> H2S + 3I2 + 2H2O

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17
Q

what is H2S

A

toxic gas

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18
Q

describe what happens in the reaction between NaI + h2SO4

A
  • HI reduces H2SO4
  • HI further reduces the SO2
19
Q

What reaction is chlorine with water

A

disproportionation

20
Q

Cl2 + H2O (with oxidation numbers)

A

Cl2 + H2O –> ClO- + Cl- + 2H+
(0)—————–(+1)—-(-1)——–

21
Q

write the reaction involved in the formation of bleach (sodium chlorate (I))

A

2NaOH + Cl2 –> NaClO + NaCl + H2O
—————(0)———(+1)——-(-1)——-

22
Q

write the reaction between chlorine and hot, concentrated sodium hydroxide

A

3Cl2 + 6NaOH –> NaClO3 + 5NaCl + 3H2O
-(0)————————–(+5)———(-1)————-

23
Q

what forms when you react Chloride ion with AgNO3

A

white precipitate (AgCl)

24
Q

what forms when you react bromide ion with AgNO3

A

cream precipitate (AgBr)

25
Q

what forms when you react iodide ion with AgNO3

A

yellow precipitate (AgI)

26
Q

what happens when you react AgCl with dilute NH3

A

precipitate dissolves

27
Q

what happens when you react AgI and AgBr with dilute NH3

A

nothing happens

28
Q

what happens when you react concentrated NH3 with Br- ion and Cl- ion

A

precipitate formed from AgNO3 dissolves

29
Q

what happens when you react concentrated NH3 with I- ion

A

nothing happens

30
Q

what do hydrogen halides react with ammonia gas to form

A

ammonium salts

31
Q

HCl + NH3 –>

A

NH4Cl

32
Q

what is NH4Cl

A

a strong acid in solution

33
Q

what forms when you react hydrogen halides with water

A

dilute acids which disassociate to release halide and hydrogen ions

34
Q

what do hydrogen ions form with water

A

hydroxonium ions, creating an acidic solution

35
Q

HCl + H2O –>

A

Cl- + H30+

36
Q

What colour and state is fluorine at Room Temperature

A
  • yellow
  • gas
37
Q

What colour and state is chlorine at room temperature

A
  • green
  • gas
38
Q

What colour and state is bromine at room temperature

A
  • brown
  • liquid
39
Q

What colour and state is iodine at room temperature

A
  • dark grey
  • solid
40
Q

What electron configurations do halogens all have

A

S2P5 outer shell configurations

41
Q

What type of covalent molecules are halogens

A

Diatomic covalent (two halogen atoms share a pair of electrons)

42
Q

Describe halogens in terms of displacement

A

A more reactive halogen will displace a less reactive halogen from its halide salt

43
Q
A

A-level chemistry (21 decks)

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