What colour is fluorine?
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| Term | Definition |
|---|---|
What colour is fluorine? | Pale yellow |
What colour is chlorine? | green |
What colour is bromine? | red-brown |
What colour is iodine? | grey |
What physical state is fluorine at room temperature? | gas |
What physical state is chlorine at room temperature? | gas |
What physical state is bromine at room temperature? | liquid |
What physical state is iodine at room temperature? | solid |
Boiling points _____ down the group | increase |
Why do boiling points increase down the group? (3) |
Trend is shown in changes of physical state from fluorine (gas) to iodine (solid)) |
Electronegativity _______ down the group | decreases |
Why does electronegativity decrease down the group? (2) |
|
Halogens become _____ oxidising down the group | less |
Why do halogens become less oxidising down the group? | Get less reactive down the group ∵ atoms become larger
Outer shell further away from nucleus ∴ electrons less attracted to it |
How can you see the relative oxidising strengths of halogens? | By displacement reactions with halide ions |
What is the basic rule for halogens in a displacement reaction with halide ions | A halogen will displace a halide from solution if the halide is below it in the periodic table |
What can we use these displacement reactions (halogens and halides) for? | To help identify which halogen (or halide) is present in solution |
Why can’t you investigate fluorine in aqueous solution? | ∵ it reacts with water |
Name 2 uses of chlorine | Used to kill bacteria in water
Mix it with sodium hydroxide to make bleach |
Describe how you get bleach | If you mix chlorine gas with cold, dilute, aqueous sodium hydroxide, you get sodium chlorate(I) solution (NaClO(aq)) = bleach |
Write an equation to show how bleach is made | Cl₂(g) + 2NaOH(aq) → NaCl(aq) + NaOCl(aq) + H₂O(l) |
Write the oxidation states of chlorine in this equation |
|
What do the oxidation states of chlorine in this equation tell us? | Oxidation state of Cl goes up and down, meaning chlorine is both oxidised and reduced. This is called disproportionation. |
Name 3 uses of sodium chlorate(I) solution (bleach) | Water treatment (kills bacteria)
Bleach paper and textiles |
When you mix chlorine with water, what does it undergo? | Disproportionation |
Write an equation to show the reaction of chlorine with water to form chloride ions and chlorate(I) ions. Include the oxidation states for chlorine. | Cl₂(aq) + H₂O(l) → Cl⁻(aq) + ClO⁻(aq) + 2H⁺(aq) Oxidation states of chlorine:
|
In sunlight, what can chlorine do to water & what does this form? | Can decompose water to from chloride ions and oxygen |
Write an equation to show the reaction of chlorine with water to form chloride ions and oxygen | 2Cl₂(aq) + 2H₂O(l) → 4Cl⁻(aq) + O₂(g) + 4H⁺(aq) |
______ ____ kill bacteria | Chlorate(I) ions |
Chlorine is ___ | toxic |
Name 3 advantages of adding chlorine to water supplies | Chlorine is important part of water treatment |
Describe disadvantages of adding chlorine to water supplies (3) | Risks from using chlorine to treat water |
Reducing Power of Halides Down the Group | Increases |
Why does the reducing power of halides increase down the group? | (To reduce something, halide ion needs lose electron from its outer shell) |
Describe the test for halides | Add dilute nitric acid (HNO3) and then silver nitrate solution (AgNO3)
Precipitate is formed (of silver halide) |