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A Level Chemistry > Module 3 - Halogens > Flashcards

Module 3 - Halogens Flashcards

(59 cards)

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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

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24
Q

describe the observation for the reaction between NaBr and Cl2 water

Study These Flashcards
A

-orange in water and organic solvent

25
describe the reaction between NaI and Cl2 water
-displacement reaction so ionic equation must be written
26
describe the observation for the reaction between NaI and Cl2 water
-in organic solvent = purple -in water = brown
27
describe the reaction between NaCl and Br2 water
-no reaction
28
describe the observation for the reaction between NaCl and Br2 water
-stays orange in water and organic solvent
29
describe the reaction between NaBr and Br2 water
-no reaction
30
describe the observation for the reaction between NaBr and Br2 water
-stays orange in water and organic solvent
31
describe the reaction between NaI and Br2 water
-displacement reaction so ionic equation must be written
32
describe the observation for the reaction between NaI and Br2 water
-brown in water -purple/violet in organic solvent
33
describe the reaction between NaCl and I2 water
-no reaction
34
describe the observation for the reaction between NaCl and I2 water
-stays brown in water -stays violet in organic solvent
35
describe the reaction between NaBr and I2 water
-no reaction
36
describe the observation for the reaction between NaBr and I2 water
-stays brown in water -stays violet in organic solvent
37
describe the reaction between NaI and I2 water
-no reaction
38
describe the observation for the reaction between NaI and I2 water
-stays brown in water -stays violet in organic solvent
39
name the type of reaction a halogen displacement reaction is
redox reaction
40
define an oxidising agent
-element that gains the electrons
41
define a reducing agent
-element that loses the electrons
42
describe the trend in oxidising ability of halogens
-ability of the halogen as an oxidising agent decreases down the group
43
explain the trend in oxidising ability of halogens
-more shielding -increased nuclear charge -decreased nuclear attraction -more difficult to accept electrons
44
describe the trend in reducing ability of halide ions
-ability of halides as a reducing agent increases down the group
45
explain the trend in reducing ability of halogens
-more shielding -increased nuclear charge -decreased nuclear attraction -easier to lose/donate electrons
46
why is chlorine reacted with water
-used to purify water supplies as it is toxic to bacteria which can cause disease
47
disadvantages of chlorine
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
describe the process of the reaction of chlorine with water
-small amounts of chlorine are added to water
49
describe the products of the reaction of chlorine with water
-hydrochloric acid (HCl) -chloric (I) acid (HClO)
50
describe the types of reaction chlorine with water is
disproportionation - as chlorine is oxidised and reduced limited reaction
51
describe household bleach
-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
describe the solubility of the reaction of chlorine with water
-low solubility of chlorine in water -if water contains some dissolved sodium hydroxide ions, more chlorine dissolves
53
describe the type of reaction that chlorine with sodium hydroxide is
-disproportionation -chlorine is oxidised and reduced
54
describe the conditions for reacting chlorine with sodium hydroxide
-cold -aqueous -NaOH
55
equation for reacting chlorine with sodium hydroxide
Cl2 + 2NaOH -> NaClO + NaCl + H2O
56
equation for reacting chlorine with water
Cl2 + 2H2O -> HClO + HCl
57
ionic equation for displacement reaction between chlorine water and compound of bromine
2Br- (aq) + Cl2 (aq) -> 2Cl- (aq) + Br2 (aq)
58
ionic equation for displacement reaction between chlorine water and compound of iodine
2I- (aq) + Cl2 (aq) -> 2Cl- (aq) + I2 (aq)
59
ionic equation for displacement reaction between bromine water and compound of iodine
2I- (aq) + Br2 (aq) -> 2Br- (aq) + I2 (aq)

A Level Chemistry (16 decks)

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