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Chemistry - inorganic > 2.3 halogens > Flashcards

2.3 halogens Flashcards

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1
Q

physical properties of the first 4 halogens

A

fluorine: pale yellow gas
chlorine: green gas
bromine: red-brown liquid
iodine: grey solid

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2
Q

trend of boiling point down group 7

A

increases down the group.
molecules get larger as you go down the group so they will have stronger van der waal forces.
which need more energy to break

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3
Q

trend in electronegativity down group 7

A

decreases down the group.
atomic radius increases down the group due to increase number of shells.
the nucleus therefore is less able to attract the bonding pair of electrons

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4
Q

trend of reactivity down group 7

A

decreases down the group.
atomic radius increases in size due to more shells.
electrons are further from the nucleus.
there is a weaker electrostatic force of attraction between the electron + nucleus.
so it is harder for larger halogens to attract electrons and form a full outer shell

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5
Q

trend of oxidising power down group 7

A

decreases down the group.
as it is harder for larger halogens to attract electrons their ability to be oxidising agents decreases

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6
Q

reaction between chlorine + bromide/iodide

A

chlorine will displace both halogens as it is the strongest oxidising agent

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7
Q

equation + observation between chlorine + bromide/iodide

A

Cl2+ 2Br- ➔ 2Cl-+ Br2
yellow solution
Cl2 + 2I- ➔ 2Cl- + I2
brown solution

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8
Q

reaction between bromine + chloride/iodie

A

bromine will displace iodide as it is a stronger oxidising power, but will not displace chloride

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9
Q

equation and observation between bromine + iodide

A

Br2 + 2I- ➔ 2Br- + I2
brown solution

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10
Q

ionic oxidation equation for bromide

A

2Br- ➔ Br2 + 2e-

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11
Q

ionic reduction equation for chlorine

A

Cl2 + 2e- ➔ 2Cl-

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12
Q

trend of reducing agent down group 7

A

increases down the group.
more electron shells, larger atomic radius, outer electrons further away from the nucleus, weaker electrostatic force of attraction, easier for larger halide ions to lose electrons

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13
Q

test for halide ions

A

1.adding nitric acid (HNO3) to sample - to remove any carbonates.
2. add silver nitrate (AgNO3) to form a halide precipitate

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14
Q

observation of each halide precipitate

A

Cl- = white precipitate
Br- = cream precipitate
I- = yellow precipitate

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15
Q

further steps to identify AgCl

A

add dilute ammonia to AgCl
forms a complex ion and a colourless solution

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16
Q

equation when dilute NH3 is added to AgCl

A

AgCl (aq) + 2NH3 (aq) ➔ [Ag(NH3)2]+ (aq) + Cl- (aq)

17
Q

further steps to identify AgBr

A

add conc ammonia to AgBr
forms a complex ion and a colourless solution

18
Q

equation when conc NH3 is added to AgBr

A

AgBr (aq) + 2NH3 (aq) ➔ [Ag(NH3)2]+ (aq) + Br- (aq)

19
Q

why does adding dilute NH3 to AgBr + AgI and conc NH3 to AgI have no reaction

A

they remain insoluble

20
Q

observation when H2SO4 is added to NaF or NaCl + what type of reaction is it

A

white steamy fumes or HF or HCl
acid-base reaction

21
Q

equations for the reaction between NaF/NaCl + H2SO4

A

NaF(s) + H2SO4 (l) -> NaHSO4 (s) + HF(g)
NaCl(s) + H2SO4 (l) -> NaHSO4 (s) + HCl(g)

22
Q

observation when H2SO4 is added to NaBr (acid-base)

A

white steamy fumes of HBr

23
Q

equations for the reaction between NaBr + H2SO4

A

NaBr(s) + H2SO4 (l) ->NaHSO4 (s) + HBr(g)

24
Q

observation between HBr + H2SO4 (redox)

A

orange fumes of bromine + colourless gas SO2

25
Q

equation for the reaction between HBr + H2SO4

A

2 H+ + 2 Br - + H2SO4 -> Br2(g) + SO2 (g) +2H2O(l)

26
Q

observation between NaI + H2SO4

A

white steamy fumes of HI
black solid and purple fume of iodine
colourless gas - SO2
yellow solid - sulfur
gas with a bad egg smell - H2S

27
Q

what is disproportiation

A

where one element is both oxidised and reduced

28
Q

reaction of chlorine with water

A

Cl2(g) + H2O (l) ⇌ HClO (aq) + HCl (aq)

29
Q

use of chlorine

A

used as a water treatment to kill bacteria

30
Q

reaction of chlorine with water in the sunlight

A

2Cl2 + 2H2O -> 4H+ + 4Cl- + O2

31
Q

equation for the production of bleach

A

Cl2(aq) + 2 NaOH (aq) -> NaCl (aq) + NaClO (aq) +

Chemistry - inorganic (4 decks)

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