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A Level Chemistry > Module 3 - Halogens > Flashcards

Module 3 - Halogens Flashcards

1
Q

describe fluorine

A

-very pale yellow gas
-highly reactive

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2
Q

describe chlorine

A

-greenish, reactive gas
-poisonous in high concentrations
-used in sterilisation

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3
Q

describe bromine

A

-red liquid
-gives off dense brown/orange poisonous fumes

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4
Q

describe iodine

A

-shiny grey solid
–red/brown liquid
-purple vapour

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5
Q

describe the trend in melting and boiling point in halogens

A

-increase down the group

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6
Q

explain the trend in melting and boiling point in halogens

A

-more electrons
-stronger London forces
-more energy is needed to break these forces

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7
Q

describe the trend in reactivity of halogens

A

-decreases down the group

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8
Q

explain the trend in reactivity of halogens

A

-more shielding
-increase in nuclear charge
-decrease in nuclear attraction
-larger atomic radius
-more difficult to gain an electron

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9
Q

describe the trend in electronegativity of halogens

A

-decreases down the group

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10
Q

explain the trend in electronegativity of halogens

A

-as atomic radius increases
-more electron shells
-more shielding
-so attract electron density in a covalent bond less strongly

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11
Q

describe the electron configuration of halogens

A

-7 electrons in their outer shell
-found in p block

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12
Q

how can halogens be recognised

A

-halogens form solutions with different colours
-a colour change shows if a reaction has taken place
-if you shake the reaction mixture with an organic solvent eg cyclohexane, it can help distinguish between halogens that have reacted

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13
Q

colour of Cl2 in water

A

pale-green

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14
Q

colour of Cl2 in a cyclohexane

A

pale-green

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15
Q

colour of Br2 in water

A

orange

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16
Q

colour of Br2 in a cyclohexane

A

orange

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17
Q

colour of I2 in water

A

brown

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18
Q

colour of I2 in a cyclohexane

A

violet

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19
Q

define a displacement reaction

A

-when a more reactive halogen displaces a less reactive halogen from its compound

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20
Q

name the three halogen displacement reactions

A
  1. add Cl2 water to individual test tubes of NaCl, NaBr, NaI
  2. add Br2 water to individual test tubes of NaCl, NaBr, NaI
  3. add I2 water to individual test tubes of NaCl, NaBr, NaI
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21
Q

describe the reaction between NaCl and Cl2 water

A

-no reaction

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22
Q

describe the observation for the reaction between NaCl and Cl2 water

A

-stays pale green in water and organic solvent

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23
Q

describe the reaction between NaBr and Cl2 water

A

-displacement reaction so ionic equation must be written

24
Q

describe the observation for the reaction between NaBr and Cl2 water

A

-orange in water and organic solvent

25
Q

describe the reaction between NaI and Cl2 water

A

-displacement reaction so ionic equation must be written

26
Q

describe the observation for the reaction between NaI and Cl2 water

A

-in organic solvent = purple
-in water = brown

27
Q

describe the reaction between NaCl and Br2 water

A

-no reaction

28
Q

describe the observation for the reaction between NaCl and Br2 water

A

-stays orange in water and organic solvent

29
Q

describe the reaction between NaBr and Br2 water

A

-no reaction

30
Q

describe the observation for the reaction between NaBr and Br2 water

A

-stays orange in water and organic solvent

31
Q

describe the reaction between NaI and Br2 water

A

-displacement reaction so ionic equation must be written

32
Q

describe the observation for the reaction between NaI and Br2 water

A

-brown in water
-purple/violet in organic solvent

33
Q

describe the reaction between NaCl and I2 water

A

-no reaction

34
Q

describe the observation for the reaction between NaCl and I2 water

A

-stays brown in water
-stays violet in organic solvent

35
Q

describe the reaction between NaBr and I2 water

A

-no reaction

36
Q

describe the observation for the reaction between NaBr and I2 water

A

-stays brown in water
-stays violet in organic solvent

37
Q

describe the reaction between NaI and I2 water

A

-no reaction

38
Q

describe the observation for the reaction between NaI and I2 water

A

-stays brown in water
-stays violet in organic solvent

39
Q

name the type of reaction a halogen displacement reaction is

A

redox reaction

40
Q

define an oxidising agent

A

-element that gains the electrons

41
Q

define a reducing agent

A

-element that loses the electrons

42
Q

describe the trend in oxidising ability of halogens

A

-ability of the halogen as an oxidising agent decreases down the group

43
Q

explain the trend in oxidising ability of halogens

A

-more shielding
-increased nuclear charge
-decreased nuclear attraction
-more difficult to accept electrons

44
Q

describe the trend in reducing ability of halide ions

A

-ability of halides as a reducing agent increases down the group

45
Q

explain the trend in oxidising ability of halogens

A

-more shielding
-increased nuclear charge
-decreased nuclear attraction
-easier to lose/donate electrons

46
Q

why is chlorine reacted with water

A

-used to purify water supplies as it is toxic to bacteria which can cause disease

47
Q

disadvantages of chlorine

A

toxic to humans
-risks with gas leaks during chlorination process
-risks of formation of chlorinated hydrocarbons which are also toxic
chlorination of drinking water raises questions about individual freedom as individuals cannot opt out

48
Q

describe the process of the reaction of chlorine with water

A

-small amounts of chlorine are added to water

49
Q

describe the products of the reaction of chlorine with water

A

-hydrochloric acid (HCl)
-chloric (I) acid (HClO)

50
Q

describe the types of reaction chlorine with water is

A

disproportionation
- as chlorine is oxidised and reduced
limited reaction

51
Q

describe household bleach

A

-commonly contains the chlorate (I) ion (ClO-) in the form of sodium chlorate (I) (NaOCl)
-the bacteria are killed by the chloric ion and chloric acid

52
Q

describe the solubility of the reaction of chlorine with water

A

-low solubility of chlorine in water
-if water contains some dissolved sodium hydroxide ions, more chlorine dissolves

53
Q

describe the type of reaction that chlorine with sodium hydroxide is

A

-disproportionation
-chlorine is oxidised and reduced

54
Q

describe the conditions for reacting chlorine with sodium hydroxide

A

-cold
-aqueous
-NaOH

55
Q

equation for reacting chlorine with sodium hydroxide

A

Cl2 + 2NaOH -> NaClO + NaCl + H2O

56
Q

equation for reacting chlorine with water

A

Cl2 + 2H2O -> HClO + HCl

A Level Chemistry (12 decks)

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