Inorganic Chemistry

Question 1

How do you test for carbonate ions in a solution?

Answer 1

Add acid, carbon dioxide will be produced if it’s a positive test, you can see if carbon dioxide is produced by bubbling the gas produced through lime water, which will go cloudy if positive.

Question 2

What are the trends for group 2?

Answer 2

Get more reactive going down⬇️
Atomic radius increases going down the group due to increased energy levels ⬇️
First ionisation energy increases going up ⬆️
So atomic radius is a larger factor.

Question 3

What are the trends in melting point for group 2?

Answer 3

Radius of metal ions increases going down ⬇️
Charge density increases going up ⬆️
Force of attraction between metal ions and delocalised electrons increases going up ⬆️
(reduces strength of metallic bonding)

Question 4

Why is magnesium anomalous in the group 2 melting trend?

Answer 4

It has a different metallic structure to beryllium.

Question 5

What happens when Beryllium is heated in the presence of water?

Answer 5

Nothing, beryllium doesn’t react with water. 😕

Question 6

What is produced when magnesium reacts with water?

Answer 6

Magnesium hydroxide and hydrogen

Question 7

Describe the reaction of magnesium with water.

Answer 7

Very slow

Magnesium hydroxide isn’t very soluble so leaves ppt

Question 8

Describe the reaction and the products produced when calcium reacts with water.

Answer 8

Steady reaction with water
Ca(OH)2 and H2 produced
Ca(OH)2 is slightly soluble leaving cloudy alkaline solution

Question 9

Describe the reaction between Strontium and water.

Answer 9

Quick

Exothermic

Question 10

Describe the products of strontiums reaction with water.

Answer 10

Sr(OH)2 soluble forming cloudy alkaline solution

Stored in oil to prevent reinformation

Question 11

Explain the reaction between barium and water.

Answer 11

Same as strontium and water but quicker and better…

Question 12

Explain the trend in solubility for alkaline metal hydroxides.

Answer 12

Increases going down the group ⬇️

Question 13

Explain the trend in alkaline metal sulphates.

Add application

Answer 13

Becomes more soluble going up ⬆️

Barium is good at absorbing x-Rays so can be used to outline the gut

Question 14

Considering the trend with ionisation energies with group 2, how does this affect the shielding ability of the shells?

Answer 14

It means that the inner shells are more effective at shielding the nucleus.

Question 15

What happens to group2 in redox reactions?

Answer 15

They’re oxidised

Question 16

Where is the name of alkaline metals derived?

Answer 16

Their oxides and hydroxides are alkaline.

Question 17

Most metals found in the earth are oxides, how are they extracted?

Answer 17

They are extracted in a displacement reaction with carbon.

This produces the metal and carbon dioxide.

Question 18

Why can Titanium not be displaced from titanium oxide using carbon?

Answer 18

Titanium carbide would be produced with is a very brittle metal.

Question 19

How is titanium removed from titanium oxide?

Answer 19

First it reacts with chlorine and carbon to make TiCl4 and CO.
Next TiCl4 is reduced to titanium by reacting it with magnesium making 2MgCl2 and Ti!

Question 20

How do the trends with hydroxides and sulphates work for solubility in group 2?

Answer 20

Hydroxides - solubility increases going down.

Sulphates - solubility increases going up.

Question 21

How can barium sulphate be used to detect sulphate ions?

Answer 21

1) Solution acidified with nitric acid.
2) Barium chloride solution is added to the solution
3) If a sulphate ion is present a white precipitate is formed
- You can add acid to remove the carbonate ions

Question 22

How do you test for chloride, bromide and iodide ions?

Answer 22

1) Add dilute nitric acid and silver nitrate solution to your solution.
2) If chlorine ions are present, a white ppt is formed
If bromine ions are present, a cream ppt is formed
If iodide ions are present, a yellowish ppt is formed

Question 23

How can you distinguish between silver bromide ions and silver chloride ions?

Answer 23

1) Add an excess of dilute aqueous ammonia solution, if chloride ions are present, the ppt will redissolve.
2) Add an excess of concentrated ammonia solution, if bromide ions are present, the ppt will redissolve.

Question 24

Explain a trend in appearance for the halogens.

Answer 24

They become darker and denser going down the group.

Question 25

What is the trend in Electronegativity for the halogens?

Answer 25

Decrease going down.

Question 26

What is the trend in atomic radius for the halogens?

Answer 26

Increase going down.

Question 27

What is the trend in mp and bp for the halogens?

Answer 27

Increase going down

Question 28

What causes fluorine to have generally untypical properties?

Answer 28

Very weak bond.

Question 29

What is a structural isomer?

Answer 29

Same molecular formula, but different structural formula.

Question 30

What is a position isomer?

Answer 30

The functional group is attached to the main chain at different points.

Question 31

What is a functional group isomer?

Answer 31

There are different functional groups.
E.g. CH3CH2OH - Ethanol
CH3OCH3 - Methyloxymethane

Question 32

What is a chain isomer?

Answer 32

Hydrocarbon is arranged differently.
E.g. CH3CH2CH2CH2OH - butan-1-ol
CH3CH(CH3)CH2OH - 2-methylpropan-1-ol