Group 7 Flashcards
Reducing ability of halides
Increases down the group, ionic radius increases, weaker attraction between outer electrons and nucleus.
Halide reactions
H2SO4 + (Br- or I-) –> SO2 (acidic gas)
H2SO4 + I- –> S yellow solid
HzSO4 + I- —> H2S - bad egg smell
halide half equations
2I- –> I2 + 2e- (appears as a black solid)
2Br- –> Br2+ 2e- (appears as brown fumes)
Reduction half equations
2e- +2H+ +H2SO4 –> SO2 +2H2O
6e- +6H+ +H2SO4 –> S +4H2O
8e- +8H+ +H2SO4 –> H2S + 4H2O
Flouride and Chloride are too weak as reducing agents to reduce H2SO4 sp they undergo basic acid reactions
F- + H+–> HF (observation= misty fumes of HF gas)
Cl- + H+ –> HCl (misty fumes of HCl gas)
Solid reaction: 2NaCl +H2SO4 –> Na2SO4 + 2HCl
Forms white solid
Halide tests
- dissolve sample in water if not already aqueous
- Add HNO3 (to remove any possible CO£2- imurities)
- Add AgNO3
F- no precipitate
Cl-= White precipitate
Br-= Cream precipitate
I-= yellow precopitate - Add dilute NH3
Cl- white precipitate dissolves
Br-= Cream precipiate insoluble
I-= yellow precipitate insoluble - Add concentrated NH3
Br-= cream precipitate dissolves
I-= yellow precipitate insoluble.
Ionic equations for halide tests
Precipitates:
Ag+(aq) +F-(aq)–> AgF
Ag+(aq) +Cl- (aq)–> AgCl
Ag+(aq) + Br- (aq) –> AgBr
Ag+(aq) +I- (aq)–> AgI
NH3:
AgCl +2NH3 –> Ag(NH3)2+ + Cl-
AgBr +2NH3 –> Ag(NH3)2+ + Br-
Halogen displacement reactions
trend in oxidising ability- Decreases down group, larger radius, weaker attraction between nucleus and incoming electron.
Displacement reaction examples
Chlorine + sodium bromide –> Bromine + sodium chloride
Cl2 +2Br- –> 2Cl- + Br2
Chlorine + sodium Iodide –>Iodine + sodium chloride
Cl2 +2I- –> 2Cl- + I2
Br- and Cl2
B2 formed- solution turns brown
CL2 AND I-
I2 formed- black solid
Br2 and I-
I2 formed- black solid.
Chlorine
Sterilises water by klling bacteria. used because benefits outweigh risks, used in small concentrations so not toxic
Chlorine and water: Cl2 + H2O ⇌ HClO + HCl
This is a disproportionation, the same element gets reduced and oxidised