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A-Level Chemistry > C7 > Flashcards

C7 Flashcards

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1
Q

Reaction that causes chlorine to oxidise water in sunlight:

A

2Cl2 + 2H2O —-> O2 + 4HCl

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2
Q

Property of an impurity that would cause mass to of (e.g. FeSO4.7H2O) to be different?

A

A version of FeSO4 with less than 7 H2O

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3
Q

What is manufactured directly from SO2?

A

H2SO4 or SO3 or Plaster of Paris

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4
Q

Half equation that forms a yellow precipitate when you add Silver Nitrate to an ion.

A

(e.g. I- ions) Ag+ + I- —> AgI

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5
Q

What happens if you put AgI in concentrated Ammonia solution?

A

Nothing, it is insoluble in all ammonia solutions

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6
Q

What happens if you put AgCl in a Ammonia solution?

A

Dissolves to give a colourless solution

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7
Q

What happens if you put AgBr in a Ammonia solution?

A

Insoluble in dilute Ammonia but soluble in concentrated Ammonia to give a colourless

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8
Q

Why is Silver Nitrate solution acidified and what acid is used?

A

To get rid of carbonate ions, Nitric Acid

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9
Q

Why is Sulfuric Acid or Hydrochloric Acid not used?

A

As they would interfere with the results, giving a precipitate of silver sulphate and silver chloride respectively.

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10
Q

What is the oxidation of oxygen?

A

-2 (OF2 it is +2) (in peroxides it is 2+ e.g. H2O2)

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11
Q

What is the oxidation state of Hydrogen?

A

+1 except in metal hydrides, e.g. NaH

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12
Q

What is the oxidation state of a group 1 metal?

A

Always +1

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13
Q

What is the oxidation state of a group 2 metal?

A

Always +2

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14
Q

What is the oxidation state of Aluminium?

A

Always 3+

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15
Q

What is the oxidation state of Fluorine?

A

Always -1

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16
Q

What is the oxidation state of Chlorine?

A

-1 (except in compounds with F and O where it has positive values)

17
Q

What is a disproportionation reaction?

A

A reaction in which the same specimen is both oxidised and reduced.

18
Q

What is the s block?

A

Groups 1 and 2

19
Q

What is the p block?

A

Group 3, 4, 5, 6 and 7

20
Q

What is the d block?

A

Transition metals

21
Q

What is the f block?

A

Radioactive metals

22
Q

What is the trend of atomic radius in a period?

A

As you go across a period, the atomic radius decreases as each atom has an extra proton and therefore a greater nuclear charge, whilst still having the same amount of inner shells, therefore they all have similar shielding. Consequently as the nuclear charge increases, so does the e.f.a between the positive nucleus and outer shell, meaning the outer electrons can be pulled closer to the nucleus.

A-Level Chemistry (11 decks)

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