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Chemistry > 3.2 Inorganic Chemistry > Flashcards

3.2 Inorganic Chemistry Flashcards

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1
Q

What happens to atomic radius down the group?

A

It increases down the group as extra electron shells are added.

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2
Q

What is the trend in first ionisation energies going down group 2?

A

It decreases. Each element has one more shell so, shielding increases. So, outer electrons are further away from the nucleus and attraction is reduced. So, it’s easier to remove the outer electron.

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3
Q

What is the trend in reactivity down group 2?

A

It increases. When group 2 atoms react, they lose electrons and form positive ions. Down the group first ionisation energy decreases so, it’s easier to lose their electron so, they become more reactive.

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4
Q

What happens to the melting point of group 2 elements down the group?

A

Group 2 elements have metallic structure, with positive ions in a crystal structure surrounded by delocalised electrons. Down the group, metal ions get bigger. The electrons are farther away from the nucleus and feel less attraction. So, it takes less energy to break the bonds.

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5
Q

What reaction does beryllium undergo with water?

A

It doesn’t react with water.

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6
Q

How does magnesium react with water?

A

It reacts slowly to produce magnesium hydroxide. It reacts with steam vigorously.

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7
Q

What happens to the solubility of group 2 hydroxides down the group?

A

Solubility increases
Mg(OH)2- sparingly
Ca(OH)2- slightly
Sr, Ba- fully

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8
Q

What happens to the solubility of group 2 sulphates down the group?

A

It decreases.
BaSO4 is insoluble.

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9
Q

What is the use of acidified BaCl2?

A

The test for sulphates.
Add barium chloride and acidified hydrochloric acid and a white precipitate of barium sulphate will form.

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10
Q

Why can barium be dangerous?

A

It is toxic so soluble forms are very dangerous as they can be absorbed by the digestive system.

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11
Q

What is BaSO4 used for?

A

It is used as a contrast medium for x-rays. It’s safe as it is insoluble and cannot be absorbed by the bloodstream.

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12
Q

What are some of the other uses for group 2 compounds?

A

Mg(OH)2, CaCO3- used as an indigestion remedy.
Ca(OH)2, CaCO3- neutralises acidic soil.
CaO- used in flue gas desulfurisation. Removes SO2 from combustion waste.
Mg- used to extract titanium from the metal ore rutile.

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13
Q

Why is barium chloride acidified when used as a test for sulphate ions?

A

The addition of acid removes carbonate ions as carbon dioxide. Barium carbonate is also a white insoluble solid which would be indistinguishable from barium sulfate.

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14
Q

What happens to electronegativity going down group 7?

A

It decreases. Down the group, the shared pair of electrons gets further away from the nucleus as atomic radius increases. So shielding increases due to more inner electron shells.

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15
Q

What happens to melting and boiling point down group 7?

A

They increase. Larger atoms have more electrons so Van der Waals intermolecular forces become stronger.

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16
Q

Are halogens oxidising or reducing agents?

A

oxidising agents

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17
Q

What happens to the oxidising ability of the halogens down group 7?

A

It decreases. Down the group there is more shielding of the outermost electron. So, the attraction of the electrons to the nucleus becomes weaker and heavier atom is less likely to accept electrons.

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18
Q

What happens in the displacement reaction of a halogen?

A

In an aqueous solution, halogens react with halides to displace the least reactive one.

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19
Q

Are halides oxidising or reducing agents?

A

They’re reducing agents.

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20
Q

What happens to the reducing ability of the halides down the group?

A

It increases. Down the group, there is more shielding of the outermost electrons. The attraction of the electrons to the nucleus becomes weaker and the atom is more likely to lose electrons.

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21
Q

What is test 1 for the halide ions?

A

Add acidified AgNO3 and add dilute HNO3 to acidify the solution.

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22
Q

What would you observe when acidified AgNO3 is added to Cl- ions?

A

White precipitate
d.NH3- the precipitate redissolves
c.NH3- the precipitate redissolves

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23
Q

What would you observe when acidified AgNO3 is added to Br- ions?

A

Cream precipitate
d.NH3- no change
c.NH3- the precipitate redissolves

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24
Q

What would you observe when acidified AgNO3 is added to I- ions?

A

Pale yellow precipitate
d.NH3- no change
c.NH3- no change

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25
Q

What is the trend in solubility of the halide salts?

A

All halide salts are soluble except for silver halides. Which is why silver nitrate is used to test for halide ions.

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26
Q

What is test 2 for the halide ions?

A

Add concentrated sulfuric acid.

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27
Q

What would you observe when H2SO4 is added to Cl- ions?

A

The sulfuric acid isn’t reduced.
HCl (steamy white fumes), HNaSO4/Na2SO4
The hydrogen halide gas turns damp blue litmus paper red.

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28
Q

What would you observe when H2SO4 is added to Br- ions?

A

The H2SO4 is reduced
When reduced: Br2 (orange solution), SO2 (choking fumes)
When not reduced: HBr (brown fumes) , HNaSO4 / Na2SO4
The hydrogen halide gas turns damp blue litmus paper red

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29
Q

What would you observe when H2SO4 is added to I- ions?

A

The H2SO4 is reduced
When reduced: I2 (purple vapour), SO2 (choking fumes), S (yellow solid), H2S (rotten egg smell)
When not reduced: HI (steamy fumes) , HNaSO4 / Na2SO4
The hydrogen halide gas turns damp blue litmus paper red

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30
Q

Why is the silver nitrate acidified before testing for halide ions?

A

It gets rid of any soluble carbonate or hydroxide impurities.

31
Q

Why is dilute and concentrated ammonia added after silver nitrate?

A

the colours of silver bromide and silver iodide precipitate are similar.

32
Q

Why do we use chlorine in swimming pools even though it’s toxic?

A

The benefits to our health of water treatment by chlorine outweigh its toxic effects.

33
Q

What is the use of chlorine in water treatment?

A

It is used to kill bacteria in swimming pools and drinking water, to prevent life-threatening diseases. The chloric acid formed in the reaction between chlorine and water is an oxidising agent and kills bacteria through oxidation and it’s also a bleach.

34
Q

What happens when chlorine and water react in sunlight? What is the solution to this problem?

A

Hydrochloric acid is formed and and chlorine is rapidly lost from the pool. So, shallow pools need a frequent addition of chlorine. Instead, solid sodium chlorate is added.

35
Q

What are the conditions for the reaction between sodium chlorate and water?

A

Swimming pool need to be kept slightly acidic as in an alkaline solution, the equilibrium of the reaction moves to the left and the HClO is removed as ClO- ions.

36
Q

How is bleach formed?

A

Chlorine reacts with cold, dilute sodium hydroxide to from NaClO. This is also a disproportionation reaction.

37
Q

What is the test for Mg2+ ions?

A

Add sodium hydroxide
Colourless solution to white precipitate

38
Q

What is the test for Ba2+ ions?

A

Add sulfuric acid
Colourless solution to white precipitate

39
Q

What is the test for NH4 + ions?

A

Add sodium hydroxide
Warm in a water bath
Turns damp red litmus paper blue

40
Q

What is the test for OH- ions?

A

Add magnesium chloride
Colourless solution to white precipitate

41
Q

What is the test for CO3 - ions?

A

Add nitric acid
Effervescence

42
Q

What does fluorine look like in pure form?

A

Pale yellow gas

43
Q

What does chlorine look like in pure form?

A

Pale green gas

44
Q

What does bromine look like in pure form?

A

Dark red liquid

45
Q

What does iodine look like in pure form?

A

Grey solid

46
Q

What does fluorine look like in non-polar solvents?

A

N/a ( it reacts with solvents)

47
Q

What does chlorine look like in non-polar solvents?

A

Pale green solution

48
Q

What does bromine look like in non-polar solvents?

A

Orange solution

49
Q

What does iodine look like in non-polar solvents?

A

Purple solution

50
Q

What does fluorine look like in an aqueous solution?

A

N/a it reacts with water

51
Q

What does chlorine look like in an aqueous solution?

A

Pale green solution

52
Q

What does bromine look like in an aqueous solution?

A

Yellow/ orange solution

53
Q

What does iodine look like in an aqueous solution?

A

Brown solution with grey solid

54
Q

What is periodicity?

A

The repeating patterns of trends across and between periods.

55
Q

Describe the reaction between sodium and water.

A

Sodium will react vigorously with cold water, forming a molten ball on the surface, fizzing and producing H2 gas. This reaction produces NaOH which is a strong alkaline solution.

56
Q

Describe the reaction between magnesium and water.

A

It reacts very slowly with cold water and forms a weak alkaline solution. A thin coating of magnesium hydroxide coats the metal. Magnesium hydroxide isn’t very soluble so less OH- ions are released, making the solution weak. But, magnesium reacts much faster with steam.

57
Q

What are the observations for the reaction between O2 and Na?

A

Yellow flame
White smoke/ solid

58
Q

What are the observations for the reaction between O2 and Mg?

A

White flame
White smoke/ solid

59
Q

What are the observations for the reaction between O2 and Al?

A

Bright white flame
White smoke/ solid

60
Q

What are the observations for the reaction between O2 and Si?

A

White flame
White smoke/ solid

61
Q

What are the observations for the reaction between O2 and P?

A

Burns spontaneously with a bright white flame and smoke.

62
Q

What are the observations for the reaction between O2 and S?

A

Burns with a blue flame

63
Q

What happens when chlorine is added to water?

A

It dissolves to form chlorine water.

64
Q

What Ions are formed after the reaction between water and Na2O? What is the pH of the solution formed?

A

Na+, OH-
Strongly alkaline
13-14

65
Q

What Ions are formed after the reaction between water and MgO? What is the pH of the solution formed?

A

Mg2+, OH-
Moderately alkaline
10

66
Q

What Ions are formed after the reaction between water and Al2O3? What is the pH of the solution formed?

A

There’s so reaction, it’s insoluble.

67
Q

What Ions are formed after the reaction between water and SiO2? What is the pH of the solution formed?

A

There’s no reaction, it’s insoluble.

68
Q

What Ions are formed after the reaction between water and P4O10? What is the pH of the solution formed?

A

H3PO4: H+, PO4 ^3-
Strongly acidic
0-1

69
Q

What Ions are formed after the reaction between water and SO2? What is the pH of the solution formed?

A

H2SO3: H+, SO3 ^2-
Weakly acidic
2-3

70
Q

What Ions are formed after the reaction between water and SO3? What is the pH of the solution formed?

A

H2SO4: H+, SO4 ^2-
Strongly acidic
0-1

71
Q

Why is the solution of Mg(OH)2 less alkaline than NaOH?

A

Mg(OH)2 is less soluble.

72
Q

Why are sodium oxides and magnesium oxides bases?

A

They contain an O 2- ion which is a very strong base as it reacts with water to produce OH- and a strongly alkaline solution.

73
Q

Why is sulfuric acid a stronger acid than sulfurous acid?

A

It fully dissociates in water.

74
Q

What anion does SiO2 form?

A

SiO3 ^2-
(Silicate)

Chemistry (14 decks)

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