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10 Cards in this Set
- Front
- Back
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What the equation when a halide ion reacts with sulphuric acid acting as an acid?
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e.g. NaCl + H2SO4 -> HCl + NaHSO4 (same with all halides)
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What would you see when sulphuric acid acts as an oxidising agent with chloride or fluoride ions?
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Steamy fumes
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What would you see when sulphuric acid acts as an oxidising agent with Bromide ions?
What is the ionic equation for this reaction? |
1. Steamy fumes
2. Brown vapour (bromine) 3. Suplphur dioxide (colourless gas) 4H(+) + SO4(2-) + 2Br(-) -> SO2 + 2H2O + BR2 |
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What would you see when sulphuric acid acting as an oxidising agent reacts with iodide ions?
What is the ionic equation for this reaction? |
1. Steamy fumes ( hydrogen iodide)
2. Purple vapour or grey solid (iodine) 3. Yellow solid suplur 4. Rotten egg smell (Hydrogen Sulphide) 5. Colourless gas (sulphur dioxide) 10H(+) + SO4(2-) + 8I(-) -> H2S + 4I2 + 4H2O |
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What happens to the reducing ability of the halides as you go down the group?
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Increases
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What factors increase rate of reaction?
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1. Concentration
2. Temperature 3. Surface Area 4. Catalyst 5. Pressure (gases only) |
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What happens to electronegativity of halogens as you go down the group?
Why? |
Decreases
Shielding increases meaning that outer rlectrons are less attracted to the nucleus |
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What is the trend in boiling points of the halogens as you go down the group?
Why? |
Increases
The size of the van der waal forces increase as atomic radius increases |
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What happens to oxidising ability of halogens as you go down the group?
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Decreases (F2 - STRONG BUT I2 WEAK)
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An oxidising agent is.......?
A reducing agent is.........? |
Reduced
Oxidised |
