3.2.3.1 Trends in properties Flashcards

1
Q

How can you identify halide ions?

A

All metal halides, except fluorides, react with silver ions in aqueous solution.
Solution is first acidified by adding dilute nitric acid. The nitric acid reacts with and removes impurities which would of produced a confusing precipitate
Add a few drops of silver nitrate solution
The colour of the precipitate indicates the halide ion

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2
Q

Why does bromine dissolve into hexane rather than water?

A

Strength of the bonding between solvent molecules is similar to the strength of bonding between simple covalent molecules and the solvent
Strength of bonds between water and bromine isn’t sufficient to overcome the hydrogen bonding

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3
Q

What are the properties of hydrogen halides?

A

All have the formula HX
All dissolve in water
All form acidic solutions due to formation of H+ ions
Are all gases

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4
Q

What are the colours and natural states of the halogens?

A
Fluorine = pale yellow gas
Chlorine = green gas
Bromine = red - brown liquid
Iodine = black solid
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5
Q

What is the trend for bond energies of the halogens in their natural state?

A

Decreases down the group

However F - F is weaker than chlorine and bromine

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6
Q

What is the trend in electronegativities of the halogens?

A

Decreases in electronegativity down the group

This is because the shared pair of electrons becomes further from the nucleus the further down the group you get

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7
Q

What is the trend in melting and boiling points of the halogens?

A

Increase going down the group
This is due to increased size which increases the van der Waals forces
Additionally they become more volatile up the group

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8
Q

What is the trend in oxidising ability of halogens?

A

Oxidising ability increases going up the group

Fluorine = one of the most powerful oxidising agent one

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9
Q

What happens in a halogen displacement reaction?

A

A more reactive halogen displacing a halide in a compound
This is a redox reaction
A halogen will displace the ion of a halogen below it in the periodic table

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10
Q

What happens to halide ions in reactions?

A

They act as reducing agents

They lose electrons to become halogen molecules

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11
Q

What is the trend in reducing ability of halide ions?

A

Increasing reducing power down the group

This is because the ions are larger so are further from the nucleus and loses the electron more easily

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12
Q

How does sodium chloride react with concentrated sulfuric acid?

A

NaCl + H2SO4 = NaHSO4 + HCl
Chloride is a weak reducing agent
Similar reaction happens with sodium fluoride to produce hydrogen fluoride

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13
Q

How does sodium bromide react with concentrated sulfuric acid?

A
Two reactions occur:
NaBr + H2SO4 = NaHSO4 + HBr
2H+ ➕ 2Br- ➕ H2SO4 = SO2 ➕ 2H2O ➕ Br2
Bromide are strong reducing agents to reduce sulfuric acid
Redox reaction
Exothermic
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14
Q

How does sodium iodide react with concentrated sulfuric acid?

A

NaI + H2SO4 = NaHSO4 + HI
Iodide is a stronger reducing agent so it reduces sulfuric acid even further
8H+ ➕ 8I- ➕ H2SO4 = H2S ➕ 4H2O ➕ 4I2

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15
Q

What happens when you add a metal halide (except fluorides) to silver ions in solution?

A

A precipitate of an insoluble silver halide is formed
Dilute nitric acid is first added to the halide solution to remove any carbonate or hydroxide ions which would confuse the result

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16
Q

What are the results of the halide ion test?

A

Silver fluoride: soluble in water
Silver chloride: white precipitate, dissolves in dilute ammonia
Silver bromide: cream precipitate, dissolves in concentrated ammonia
Silver iodide: pale yellow precipitate, insoluble in concentrated ammonia

17
Q

How does chlorine react with water?

A

Reversible reaction
Cl2 + H2O = HClO + HCl
Disproportionation reaction

18
Q

How does chlorine react with water in sunlight?

A

2Cl2 + 2H2O = 4HCl + O2

19
Q

What is an alternative to the direct chlorination of swimming pools?

A

Add solid sodium or calcium chlorate
NaClO ➕ H2O = Na+ ➕ OH- ➕ HClO
Reversible reaction

20
Q

How does chlorine react with dilute sodium hydroxide?

A

Cl2 + 2NaOH = NaClO + NaCl + H2O

Other halogens behave similarly