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Chemistry > Topic 4 -Inorganic Chemistry > Flashcards

Topic 4 -Inorganic Chemistry Flashcards

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1
Q

Describe and explain the trend in atomic radius down group 2

A

Atomic radius down group 2 increases because as you go down the group the atoms have more electron shells making the atom bigger.

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2
Q

Decribe and explain the trend in melting points down group 2

A

They decrease because atomic size increases meaning there is a larger distance between positive ions and delocalised electrons. Therefore there is a weaker eletrostatic force of attraction and less energy needed to overcome this attraction.

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3
Q

Describe the trend in 1st ionisation energy down group 2

A

It decreases down the group because the outermost electrons are held futher from the nucleus. Inner shell electrons also provide a shielding effect

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4
Q

Explain and decribe the trend in reactivity down group 2

A

Reactivity increases as atomic radii increases so there is more shielding. The nuclear attraction decreases making it easier to remove outer shell electons, so cations form more easily

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5
Q

What needs to be done to magnesium ribbon before testing reaction rates as why?

A

Cleaned off with emery paper because and uncleaned ribbon will give false results because both Mg and MgO formed on ribbon from reaction with air will react at different rates

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6
Q

What is produced when magnesium reacts in steam?

A

Magnesium oxide and hydrogen

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7
Q

What will the other group 2 metals react with cold water to form?

A

Metal hydroxide and hydrogen

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8
Q

What would one observe when group 2 hydroxides produce the water alkaline?

A

Fizzing- that gets more vigorous down the group
The metal dissolving -Faster down the group
Solution heats up- more down the group
With calcium, a white precipitate appears

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9
Q

What do ionic oxides react with water to form?

A

Hydroxides

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10
Q

Describe the trend in solubility of group 2 hydroxides down the group

A

Solubility increases down the group but Mg(OH)2 is insoluble and Ca(OH)2 is reasonably soluble

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11
Q

Which group 2 hydroxide is classed as insoluble in water ?

A

Magnesium hydroxide

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12
Q

How and why is magnesium hydroxide used in medicine

A

To neutralise excess acid in the stomach to treat constipation. It is safe to use as it is wealky alkaline n wont produce CO2

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13
Q

What is an aqueous solution of calcium carbonate called?

A

limewater

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14
Q

Which metal hydroxide is used in agriculture and what for?

A

Calcium hydroxide is used to neutralise acidic soils

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15
Q

Describe the trend of solubility of group 2 sulfates down the group

A

Group 2 sulfates become less soluble down the group

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16
Q

Explain rate at which barium metal reacts with sulfuric acid

A

It reacts slowly because insoluble barium sulfate produced covers the surface of the metal preventing futher attack.

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17
Q

What happens to group 2 metals when heated?

A

They decompose to produce group 2 oxides and carbon CO2

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18
Q

Describe and explain the trend in thermal stability of group II carbonates

A

They become more thermally stable going down the group because their cations get bigger and have less of a polarising effect and distort the carbonate ions less. The C-O bond is weakened less so it less easily breaks down.

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19
Q

Describe and explain thermal decomposition of group 1 carbonates

A

They do not decompose with the exception of lithium. This is because they only have 1+ chages which is not a big enough charge density to polarise the carbon ion. Lithium is an exception as its ion is small enoughnto have a polarising effect.

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20
Q

Descibe an experiment that can be conducted to done to investigate ease of decomposition of the carbonates

A

Heat a know mass of carbonate in a side arm boiling tube, pass the gas through limewater, time for the first cloudiness to appear. repeat for different moles of the carbomnates.

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21
Q

What do group II nitrates decompose to form?

A

Group II oxides
Oxygen
Nitrogen dioxide gas

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22
Q

What will be observed when a group 2 nitrate decomposes?

A

Brown gas (NO2)
A white nitrate solid melting into a colurless solution solution then re-solidify

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23
Q

Explain why magnesium nitrate decomposes the easiest?

A

The Mg 2+ ion is the smallest and has the greater charge density, this causes more polarisation of the nitrate anion weaking the N-O bond.

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24
Q

How do group 1 nitrates with the exception of lithium decompose to form?

A

They give a nitrate (III) salt and oxygen

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25
Q

Give the colour of lithium in a flame test

A

Scarlett red

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26
Q

Give the colour of sodium in a flame test

A

Yellow

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27
Q

Give the colour of potassium in a flame test

A

Lilac

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28
Q

Give the colour of rubidium in a flame test

A

Red

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29
Q

Descibe the method of conducting a flame test

A

Use a nichrome wire and clean it by dipping in conc HCL and heating in bunden flame until no orange flame showed. Dip wire in powdered solid and observe colour.

30
Q

Explain how a flame test causes colour to show.

A

When heating, the heat causes an electron to move to a higher energy level. The electron is unstable at this higher energy level and so drops back down. As it drops backl down to ,lower energy level, energy is emitted in the form of visible light, the wavelength of the light determins the colour.

31
Q

Give the colour of caesium in a flame test

A

Blue

32
Q

Give the colour of magnesium in a flame test

A

No flame colour as wavelength outside of visible spectrum.

33
Q

Give the colour of calcium in a flame test

A

Brick red

34
Q

Give the colour of strontium in a flame test

A

Red

35
Q

Give the colour of barium in a flame test

A

green

36
Q

Describe and explain the trend in melting and boiling points of halogens down the group

A

Increases as the molecules become larger, there are therefore larger london forces between the molecules. Intermolecular forces are larger so there is more energy required to break the forces. Increasing mp and bp

37
Q

Describe the trend in electronegativity down group 7

A

Decreases due to increasing number of shells. The nucleus is therefore less able to attract the bonding pair of electrons

38
Q

Describe and explain the reactivity of halogens down the group.

A

Decreases as atoms get bigger with more shielding so they less easily attract and accept electrons. They therefore form 1- ions less easily down the group

39
Q

What are oxidising agents

A

Electron acceptors

40
Q

What is disproportionation?

A

A reaction where an elemt simultaneously oxidises and reduces.

41
Q

What does chlorine produce when reacted with water and how is this an example of a disproportionation reaction?

A

Cl2(g) + H2O(l) –> HClO(aq) + HCl (aq)
Chlorine is both simultaneously reducing and oxidising changing its oxidation number from 0 to -1 and 0 to +1

42
Q

Why is chlorine used as treatment for water despite some toxic effects?

A

benefits outweigh the toxic effects

43
Q

Chlorine bromina and iodine in aqueous solutions will react with cold sodium hydroxide. How will the colour of the solution change?

A

It will change to be colourless

44
Q

How is disproportionation with hot alkalis different than cold with halogens?

A

The halogens go to a higher oxidation state however, NaClO+NaCL+H20 is still produced and used as bleach

45
Q

What does a reducing agent do?

A

Donates electrons

46
Q

Explain in terms of reactivity why chlorine can displace iodine and bromine but iodine cannot displace bromine or chlorine?

A

A more reactive halogen with displace a less reactive halogen in a solution. Down the group, reactivity of group 7 elements decrease, Cl2 therefore will displace Br2 and I2 in a redox reaction

47
Q

Write an example of a word redox reaction between group 7 showing displacement

A

Potassium bromide(aq) + Chlorine(aq) —–> Potassium Chloride(aq) + Bromine (aq)

48
Q

What colour is the solution when chlorine displaces bromine in a redox reaction?

A

Yellow solution

49
Q

What colour is the solution when Iodine is displaced by a halogen?

A

Brown solution

50
Q

Give an example of an organic solvent used in a redox reaction for halogens

A

cyclohexane

51
Q

Why would an organic solvent be added to the redox reaction between halide ions and halogens?

A

The changes are easier to see as the halogen present will dissolve in the organic solvent, which settles out as a distinct layer above the aqueous solution.

52
Q

What colour is shown by chlorine bromine and iodine when an organic solvent is added to a displacement reaction>

A

Chlorine- Colourless
Bromine- Yellow
Iodine- Purple

53
Q

How ca the increasing power of halides as reducing agents ben shown through the reactions of solid halides with H2SO4?

A

Br- ions are stronger reducing agents the Cl- and F- and after the initial acid base reaction, reduce sulphur H2SO4 from +6 to +4 in SO2 and I- ions are the strongest and they reduce sulphur in H2SO4 +6 to +4 in SO2 and 0 in s to -2 in H2S

54
Q

Write a symbol equation for the reaction of sulfuric acid with solid chlorine or fluoride ions. Also write what is observed when reaction takes place?

A

NaF(s) + H2SO4(l) —–>NaHSO4(s) + HF(g)- Steamy white fumes of HF
NaCl(s) + H2SO4(l) ——> NaHSO4(s) + HCl(g)- Steamy white fumes of HCL

55
Q

What is the role of nitric acid in the reaction between halide ions and silver nitrate?

A

The role of nitric acid is to react with any carbonates present to prevent formation of the precipitate Ag2CO3 .This would mask the desired observations

56
Q

What colour precipitates do Chlorides, bromides and iodides produce when reacted with silver nitrate?

A

Chlorides- White
Bromides- Cream
Iodides- Pale yellow

57
Q

What is the effect of light on silver halides formed (except AgI)

A

It darkens in sunlight to form silver.

58
Q

What can be added to the silver halides to differentiate them if they look too similar and how does this help differntiate?

A

Ammonia solution helps differentiate them as AgCl dissoves in dilute ammonia whereas and Agbr dissolves in conc ammonia to form complex ions whereas AgI does not react with ammonia

59
Q

Why does AgI not react with ammonia?

A

It is too insoluble

60
Q

How are hydrogen halides(only no other products) made?

A

Reaction of solid sodium halide salts with phosphoric acid.

61
Q

Why is phosphoric acid more suitable for making hydrogen halides than concentrated sulfuric acid to make Hcl, Hbr ad HI?

A

There are no extra redox reactions taking place and no other products formed. Phosphoric acid is not an oxidising agent

62
Q

What are the observations of the reaction used to form only hydrogen halides?

A

White steamy fumes of the hydrogen halides are evolved.

63
Q

Describe what hydrogen hallides dissolve in water to form

A

They all dissolve in water to form acidic solutions

64
Q

What is used to test for sulfate ions and what is observed?

A

Barium chloride is added and a white precipitate is formed

65
Q

Describe the test for halide ions with silver nitrate

A

This reaction is used as a test to identify which halide ion is present. The test solution is made acidic with nitric acid, and then silver nitrate solution is added dropwise.

66
Q

Why can HCL not be used to acidify test solution for halide ions?

A

Hydrochloric acid cannot be used to
acidify the mixture because it contains
chloride ions which would form a
precipitate

67
Q

Give two ways ammonia gas can be identified

A

Ammonia gas can be identified by its
pungent smell or by turning damp red
litmus paper blue

68
Q

Describe the test for ammonium ion

A

NH4+ reacted with with warn NaOH to form NH3

69
Q
A
70
Q

What is observed when hydrogen bromide gas reacts with ammonia gas?

A

White smoke

Chemistry (7 decks)

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