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A-level Chemistry > A2 Inorganic > Flashcards

A2 Inorganic Flashcards

1
Q

Reaction of sodium and water

A

2Na + 2H2O –> 2NaOH +H2

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2
Q

Product of magnesiums reaction with water at room temperature

A

Magnesium hydroxide

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3
Q

Product of heated magnesium and steam reaction

A

Magnesium oxide

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4
Q

two allotropes of phosphorus, and define allotrope

A

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

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5
Q

two products of the reaction of sulfur and oxygen

A

sulfur dioxide, trioxide

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6
Q

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

A

aluminium oxide

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7
Q

product of the reaction of sodium oxide and water

A

sodium hydroxide

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8
Q

product of the reaction of magnesium oxide and water

A

magnesium hydroxide

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9
Q

the two period 3 elements that do not react with water

A

aluminium oxide, silicon dioxide

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10
Q

product of reaction of phosphorus with water

A

phosphoric acid, H3PO4

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11
Q

product of reaction of sulfur dioxide with water

A

sulfurous acid, H2SO3

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12
Q

product of reaction of sulfur trioxide with water

A

sulfuric acid, H2SO4

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13
Q

which period three oxide is amphoteric

A

aluminium oxide

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14
Q

reaction of sodium oxide and sulfuric acid

A

Na2O + H2SO4 –> Na2SO4 +H2O

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15
Q

Product of the reaction of silicon dioxide and sodium hydroxide

A

sodium silicate, Na2SiO3

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16
Q

product of Reaction of phosphoric acid and sodium hydroxide

A

Sodium phosphate, Na3PO4

17
Q

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

A

Chromium and copper

18
Q

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

A

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

19
Q

What are the four properties of transition metals

A

variable oxidation states
colour
catalysis
complex ion formation

20
Q

How are complex ions formed?

A

ligands form coordinate bonds with transition metals

21
Q

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

A

aqua ions

22
Q

two examples of bidentate ligands

A

ethane - 1,2 - diamine, ethanedioate

23
Q

the name given to complex ions with polydentate ligands

A

chelates

24
Q

Describe the chelate effect

A

mulitdentate ligands replace monodentate ligands due to the increase in entropy

25
Q

the two types of isomerism seen in complex ions

A

cis-trans (or E-Z), optical

26
Q

Why are transition metals coloured?

A

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.

27
Q

what are the equations for the contact process

A

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

28
Q

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

A

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

29
Q

Explain autocatalysis

A

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

30
Q

Why are more charged ions more acidic when dissolved in water

A

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

31
Q

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

A

[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.

32
Q

What metal aqua ion is amphoteric

A

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

33
Q

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

A

ligand substitution reaction, NH3 ligand replaces H2O

34
Q

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

A

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

35
Q

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

A

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]

36
Q

Give the reaction of metal aqua ions that produces fizzing

A

carbonate with metal 3+ aqua ion

37
Q
A

A-level Chemistry (6 decks)

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