A2 Inorganic

Question 1

Reaction of sodium and water

Answer 1

2Na + 2H2O –> 2NaOH +H2

Question 2

Product of magnesiums reaction with water at room temperature

Answer 2

Magnesium hydroxide

Question 3

Product of heated magnesium and steam reaction

Answer 3

Magnesium oxide

Question 4

two allotropes of phosphorus, and define allotrope

Answer 4

red and white, the same element with the atoms arranged differently

Question 5

two products of the reaction of sulfur and oxygen

Answer 5

sulfur dioxide, trioxide

Question 6

Which period 3 metal oxide has a polarised bond, partly covalent

Answer 6

aluminium oxide

Question 7

product of the reaction of sodium oxide and water

Answer 7

sodium hydroxide

Question 8

product of the reaction of magnesium oxide and water

Answer 8

magnesium hydroxide

Question 9

the two period 3 elements that do not react with water

Answer 9

aluminium oxide, silicon dioxide

Question 10

product of reaction of phosphorus with water

Answer 10

phosphoric acid, H3PO4

Question 11

product of reaction of sulfur dioxide with water

Answer 11

sulfurous acid, H2SO3

Question 12

product of reaction of sulfur trioxide with water

Answer 12

sulfuric acid, H2SO4

Question 13

which period three oxide is amphoteric

Answer 13

aluminium oxide

Question 14

reaction of sodium oxide and sulfuric acid

Answer 14

Na2O + H2SO4 –> Na2SO4 +H2O

Question 15

Product of the reaction of silicon dioxide and sodium hydroxide

Answer 15

sodium silicate, Na2SiO3

Question 16

product of Reaction of phosphoric acid and sodium hydroxide

Answer 16

Sodium phosphate, Na3PO4

Question 17

The two transition metals that do not have full 4S orbitals

Answer 17

Chromium and copper

Question 18

Which two d-block metals are not technically transition metals and why

Answer 18

scandium and zinc. They form Sc3+ and Zn2+. Neither of these have “part full” D-orbitals. Sc3+ has 3d0, Zn2+ has 3d10

Question 19

What are the four properties of transition metals

Answer 19

variable oxidation states
colour
catalysis
complex ion formation

Question 20

How are complex ions formed?

Answer 20

ligands form coordinate bonds with transition metals

Question 21

Complex ions that are formed from dissolving a salt of a transition metal in water

Answer 21

aqua ions

Question 22

two examples of bidentate ligands

Answer 22

ethane - 1,2 - diamine, ethanedioate

Question 23

the name given to complex ions with polydentate ligands

Answer 23

chelates

Question 24

Describe the chelate effect

Answer 24

mulitdentate ligands replace monodentate ligands due to the increase in entropy

Question 25

the two types of isomerism seen in complex ions

Answer 25

cis-trans (or E-Z), optical

Question 26

Why are transition metals coloured?

Answer 26

Transition metals have electrons in d- orbitals. The d- orbitals split when ligands attach. When electrons move from one orbital to the next, they absorb energy from a particular wavelength of light. The colour is missing from the spectrum, so we see the colours that are not absorbed.

Question 27

what are the equations for the contact process

Answer 27

SO2 + V2O5 --> SO3 + V2O4 2V2O4 + O2 --> 2V2O5

Question 28

Why is the reaction between S2O8- and I- so slow without a catalyst?

Answer 28

Both ions are negative, so they repel each other. This causes a high activation energy

Question 29

Explain autocatalysis

Answer 29

one of the products of the reaction is the catalyst for the reaction

Question 30

Why are more charged ions more acidic when dissolved in water

Answer 30

The higher positive charge causes electrons to be pulled closer to the nucleus as they are more polarising. As this happens to the oxygen atoms, there is less attraction for the hydrogen atoms, so they dissociate more easily

Question 31

explain how adding a base to a metal aqua ion solution eventually causes the formation of an insoluble precipitate

Answer 31

[M(H20)6]3+ +H2O ⇌ [M(H2O)5(OH)]2+ +H3O+ Adding a base shifts the equilibrium of this reaction to the right, as the base reacts with the H3O+ ions, taking them out of solution. Therefore, the reaction attaches more OH- ligands to the aqua ion, reducing the aqua ions charge. Eventually the aqua ion has neutral charge, so becomes insoluble.

Question 32

What metal aqua ion is amphoteric

Answer 32

aluminium hydroxide [Al(H2O)3(OH)3]

Question 33

What happens when you add excess ammonia to a metal aqua ion

Answer 33

ligand substitution reaction, NH3 ligand replaces H2O

Question 34

What happens when you add carbonate ions to an M2+ metal aqua ion?

Answer 34

carbonate displaces the ligand, so a metal carbonate is formed with 6 H2O

Question 35

What happens when you add carbonate ions to an M3+ metal aqua ion?

Answer 35

M3+ is more acidic, so the carbonate ions react with the extra H3O+ ions, shifting the equilibrium to the right, until an insoluble precipitate is formed - [M(H2O)3(OH)3]

Question 36

Give the reaction of metal aqua ions that produces fizzing

Answer 36

carbonate with metal 3+ aqua ion