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A Level Chemistry > Inorganic chem and periodic table - Topic 4 > Flashcards

Inorganic chem and periodic table - Topic 4 Flashcards

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1
Q

what is thermal decomposition

A

the name of a reaction in which a compound decomposes on heating

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2
Q

what do acids and metals make

A

hydrogen gas and a salt (a metal compound)

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3
Q

what do acids and bases make (neutralisation reaction)

A

salt and water

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4
Q

why do all the reactions between acids and bases make water

A

as the hydrogen ions react with the hydroxide ions to form water
supporting equation
OH-(aq) + H+(aq) ——> H20

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5
Q

what do acids and carbonates make

A

salt water and carbon dioxide

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6
Q

what are ionic precipitation reactions

A

a reaction which produces a solid precipitate on mixing two solutions containing ions

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7
Q

solubility table

A

to revise this better draw a table with one side being what is soluble in water and the other being whats insoluble in water

what are soluble:
- all acids
- calcium, sodium and potassium hydroxide - HOWEVER OTHER METAL OXIDES AND HYDROXIDES ARE INSOLUBLE (NOT SOLUBLE)
- carbonates of sodium and potassium -HOWEVER ALL OTHER CARBONATES ARE INSOLUBLE (NOT SOLUBLE)
- all nitrates
- all chlorides - HOWEVER SILVER CHLORIDE AND LEAD CHLORIDE ARE INSOLUBLE (NOT SOLUBLE)
- all sulfates - HOWEVER BARIUM SULFATE AND LEAD SULFATE ARE INSOLUBLE (NOT SOLUBLE)
- all sodium, potassium and ammonium salts

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8
Q

what does the solubility table explain

A

if the compound is soluble in wate then it is an aqueous but if it isnt then it is a solid

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9
Q

what are the changes to the atoms down the group in alkali metals

A
  • the charge of the nucleus increase
  • the atomic radius increases as there is an increase in the number of shells
  • the force of attraction decreases
  • the nuclear charge stays the same as its always plus 1
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10
Q

What happens in reactions with alkali metals and water

A
  • they all form metal hydroxides and hydrogen
  • lithium gives off steam with bubbles of hydrogen
  • sodium melts to form a shiny bead that skates on the surface of the water
  • potassium catches on fire and burns with a lilac flame
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11
Q

Reactions with metals and chlorines

A

the all form colourless ionic metal chlorides

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12
Q

what is the trend of solubility down metal hydroxides

A

the solubility increases as you go down a group

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13
Q

why are hydroxides strong bases

A

as they are fully ionised in water, giving solutions of hydroxide ions

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14
Q

why do carbonates produce alkaline solutions when dissolved in water

A

as the carbonate ions remove the h+ ions from water molecules to form hydrogencarbonate ions and hydroxide ions, and these hydroxide ions make the solution alkaline

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15
Q

In a chemical test what proves the presence of hydroxides

A

white solids

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16
Q

In a chemical test what would group 1 nitrates look like

A

white crystalline solids

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17
Q

what does the thermal decomposition of group 1 NITRATE form AND whats the exception

A

a NITRITE and oxygen
e.g
2KNO3 —–> 2KNO2(s) + O2 (g)

EXCEPT LITHIUM as it decomposes into the oxide, nitrogen dioxide and oxygen

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18
Q

explain why sodium and potassium are used as chemical reagents

A
  • their ions are inert so act as spectator ions
  • they are the most soluble in water, including their hydroxides and carbonates compared to to other metal hydroxides and carbonates which are insoluble
  • they are colourless in aqueous solutions so do not interfere with other colour changes
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19
Q

flame colours of GROUP 1 METALS

A

lithium - bright red
sodium - bright yellow
potassium - lilac

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20
Q

why does compounds containing sodium not burn during a flame test

A

as the energy from the flame excites the outer electrons of the sodium ions, raising them to higher energy levels, the atom emits the characteristic of a yellow light as as the electrons drop back to lower energy levels

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21
Q

Trend of solubility in group 2

A

Decreases as you go down the group

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22
Q

Why does the reactivity increase as you go down alkaline earth metals (group 2)

A

As the first and second ionisation energy decreases as the atomic radius increases and the number of inner electron shells increase as you go down the group, so there is a weaker attraction between the nucleus and outer electrons as you go down the group so the first and second ionisation energies decrease as less energy is required to remove the outer 2 electrons causing the reactivity to increase

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23
Q

How does Mg, Ca and Ba react with oxygen

A
  • They all form a white ionic oxide (which are solids)
  • Mg burns with oxygen to form a bright white flame and a white solid magnesium oxide
  • calcium burns with a yellow flame and forms a white solid calcium oxide
  • barium burns with a green flame to form a peroxide BaO2 (which is also white)
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24
Q

How do alkaline earth metals (group 2 metals) react with water

A
  • produces the alkaline metal hydroxides and hydrogen gas
  • the rate of reaction increases as you go down the group
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25
Q

How do alkaline earth metals (group 2 metals) react with chlorine

A
  • it forms a metal chloride (and nothing else)
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26
Q

Why does the thermal stability of group 2 carbonates and nitrates increases as you go down the group

A
  • as you go down the group the atomic radius of the metal ion increases, causing the size of the metal ion to increase so it will have a lower charge density, this decreases the polarising power of the metal ion as the low charge density makes it harder for the metal ion to attract the bonding electrons in carbonate/nitrate ion, so the electron cloud is not easily distorted so the bonds require a higher temperature to break so thermal stability increasees.
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27
Q

what is a basic oxide

A

a metal oxide which can react to form salts and water by acting as a base by taking the hydrogen ion from the base

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28
Q

what do group 2 metals and acids form

A

salt and water
as the group 2 metals are basic oxides

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29
Q

What do group 2 metal oxides and water form

A

A metal hydroxide

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30
Q

Explain the reaction of calcium oxide and water

A

the calcium oxide dissolves in the water to form calcium hydroxide solution but as calcium hydroxide is only slightly soluble in water so the solution becomes quickly saturated and as we continue to form calcium hydroxide this no longer dissolved but instead forms solid calcium hydroxide

31
Q

Trend in solubility of group 2 hydroxides

A

Increases as you go down the group

32
Q

How does the trend in solubility in group 2 hydroxides explain why group 2 metal hydroxides become more alkaline as you go down the group

A

As when the metal hydroxide dissolved in water it forms a metal ion and a hydroxide ion. This means that as the solubility increases down the group it will become more alkaline as the metal hydroxides will dissolve in water more easily and hence release more hydroxide ions making it more alkaline

33
Q

Uses of group 2 hydroxides

A
  • neutralisation reactions in agriculture and medicine
  • treat indigestion ( the excess of HCL in the stomach) - such as milk of magnesia which contains Mg(OH)2
34
Q

properties of group 2 sulfates

A
  • similar in that they are all colourless solids with the formula MS04
  • different in that they become less soluble down the group
35
Q

properties of group 2 nitrates

A
  • similar in that they all have the formula M(NO3)2 they are colourless crystalline solids, very soluble solids and decompose to the oxide when heated
  • different in that they become more difficult to decompose down the group
36
Q

general formula for the decomposition of group 2 nitrates

A

XNO3 —-> XO + NO2 + O2

lithium nitrate also follows this general formula

37
Q

general formula for the decomposition of group 1 nitrates

A

2XNO3 —-> 2XNO2 + O2

EXCEPT LITHIUM - DOES NOT FOLLOW TGIS FORMULA

38
Q

properties of group 2 carbonates

A
  • similarities: they all have the formula MCO3, are insoluble in water, react with dilute acids and form an oxide and carbon dioxide during thermal decomposition
  • differences: thermal stability increases down a group (become more difficult to decompose down the group)
39
Q

general formula for the thermal decomposition of group 2 carbonates

A

CaCO3 —-> CaO + CO2

40
Q

flame colours for group 2

A

beryllium - no colour
magnesium - no colour
calcium - brick red
strontium - bright red
barium - pale green

41
Q

Colours of halogens at rtp

A

Florine - pale yellow gas
Chlorine - pale green gas
Bromine - red brown liquid
Iodine - grey black solid

42
Q

Why does the melting point and boiling point increase as you go down group 7

A

As you go down the group the strength of the London forces increase as the number of electrons increase, so more energy is required to overcome the London forces as you go down the group so mp and bp increase down group 7

43
Q

Explain the Trends in Electronegativity in the halogens

A

The Electronegativity decreases as you go down the group as the number of electron shells and atomic radius increases, which reduces the attraction between the bonding electrons and the nucleus causing the Electronegativity to decrease as you go down the group

44
Q

What forms when a halogen reacts with a metal

A

Ionic halides

45
Q

Explain the Trend in strength of oxidising agents in halogens

A

The strength of the oxidising agent decreases as you go down the group as the atomic radius increases as you go down the group and the number I’d shells also increase so the outer electrons become further from the nucleus and the attraction between the outer electrons and the nucleus decreases, making it harder for the halogens to gain an electron and hence act as a less powerful oxidising agent

46
Q

Why can’t iron(111) iodine ions form when reacting iodine with iron

A

As the iodine ions reduce iron (111) to iron (11) ions. So when heating iron with iodine vapour it produces iron (11) iodide

47
Q

test to distinguish halides and the result for the test

A

silver nitrate
add silver nitrate to a solution of halide ions to form a silver halide
- silver chloride - white precipitate, which turns purple grey in sunlight
- silver bromide - creamy coloured precipitate
- silver iodide - yellow precipitate

48
Q

How does chlorine Bromine and Iodine react with hydrogen

A
  • hydrogen Produces the colourless acidic gas, hydrogen chloride, HCL (NOT HYDROCHLORIC ACID only referred to hydrochloric acid when the gas is in a solution of water)
  • bromine forms hydrogen bromide with a pale bluish flame
  • iodine forms hydrogen iodide and unlike the other two it is a reversible reaction
49
Q

Explain the Trend of the strength of reducing agents in halogens

A

The strength of reducing agents of halide ions increase as you go down the group as when you go down the group the atomic radius and the number of inner shields increase so the outer electron is further away frown the group so the attraction between the outer electron and the nucleus decreases making it easier for the halogens to lose an electron causing them to be a stronger reducing agent as you go down the group

50
Q

Products from Reaction between sodium chloride and concentrated sulfuric acid and what type of reaction

A

NaCl (s) + H2SO4 (l) ——> NaHSO4 (s) + HCl (g)

Products: sodium hydrogensulfate (white solid) and hydrogen chloride (not hydrochloricacid) (forms white fumes)

Type of reaction: acid base reaction - as oxidation’s numbers stay the same and chloride ion is a weak reducing agent so cannot reduce the sulfur in the sulfuric acid

51
Q

products formed from Reaction between sodium bromide and concentrated sulfuric acid and type of reaction and observations

A

2Br- + H2SO4(l) + 2H+ —-> SO2(g) + 2H2O(l) + Br2(l)
Products: sulfur dioxide gas, bromine and water
Observation: produces orange vapour (Br2) mixed with colourless acidified gas (SO2)
Type of reaction: redox

52
Q

observation of precipitate formed when dissolving silver halides in aqueous ammonia

A

silver chloride - precipitate dissolves easily in DILUTE ammonia to form a colourless solution
silver bromide - precipitate dissolves n CONCETRATED aqueous ammonia to form colourless solution
silver iodide - precipitate does not dissolve in ammonia solution

53
Q

Reaction between sodium iodide and concentrated sulfuric acid - observations, products and type of reaction

A

Products: iodine, sulfur and hydrogen sulfide
Observations : dark solid which gives of purple vapour (I2), yellow solid (S) and a bad egg smell (H2S)
Type of reaction: redox

54
Q

Properties of hydrogen halide

A
  • colourless gas at room temp which fume in moist air
  • very soluble in water forming acidic solutions which completely ionise in water
  • strong acids so ionise in water
55
Q

Test for hydrogen halides

A

Mixing any hydrogen halide with ammonia will produce a white smoke of ammonium salt

E.g
Nh3 + HCl ——> NH4Cl

56
Q

What happens when chlorine dissolves in water

A

A reversible reaction takes place to produce a mixture of hydrochloric acid and chloric(I) acid (hypochlorous acid)

Cl2 (g) + H2O (l) —-> HClO (aq) + HCl (aq)
<—– (REVERSIBLE REACTION)

57
Q

state an application for the reaction between chlorine and water to make chloric (1) acid

A

To kill bacteria in drinking water

58
Q

State an application for the reaction between sodium hydroxide to make sodium chlorate (same reaction with potassium but with sodium)

A

household bleach

59
Q

what happens when chlorine is added to water in the presence of bright sunlight

A
  • chlorine reacts with oxygen to form hypochlorus acid which further breaks down into hydrogen chloride and oxygen gas by sunlight

2HOCl ——> 2HCl + O2 (in the presence of sunlight)

overall equation: 2H20 + 2Cl2 ——-> 4HCL + O2

60
Q

Trend of solubility in group 2 hydroxides and sulfates

A

Group 2 hydroxides - solubility increases down the group
Group 2 sulfates - solubility decreases down the group

61
Q

Why do we dip the flame test wire into concentrated HCl

A
  • it reacts with the compounds to form volatile chlorides
62
Q

Why do metal ions produce different flame colours

A

As different wavelengths of light are released due to different gaps between energy levels

63
Q

What is the flame test wire made from

A

Nichrome or platinum

64
Q

Test for sulfate ions

A

You first acidify the solution you are testing with dilute hydrochloric acid and then add barium chloride solution.

If you have a sulfate, you will get a white precipitate of insoluble barium sulfate

65
Q

Describe how you would compare the thermal stability of two different group 2 nitrates. You must include one safety precaution

A
  • Record time it takes to produce a brown fume
  • same heat applied
  • same amount if each nitrate I’m seperate test tubes
  • saftey precaution: fume cupboard
66
Q

Explain the origins of flame colours

A

Heat from the flame promotes the electrons to higher energy levels, the electrons then drop back down to lower energy levels causing light to be emitted

67
Q

write the half equation for the oxidation of the chlorine molecules to chlorate ions in the presence of cold hydroxide ions

A

Cl2(g) + 2OH- (aq) —–> ClO- (aq) + Cl- (aq) + H20 (l)

68
Q

The reaction between chlorine and cold dilute sodium hydroxide solution

A

2NaOH + Cl2 ——> NaCl + NaClO + H2O

69
Q

The reaction between chlorine and HOT concentrated sodium hydroxide solution

A

6NaOH + 3Cl2 ——-> 5NaCl + NaClO3 + 3H2O

70
Q

Explain why magnesium nitrate, Mg(NO3)2 decomposes more readily on heating than potassium nitrate, KNO3

A
  • magnesium ion is smaller (than the potassium ion)
  • magnesium ion has a higher charge
  • magnesium ion polarises nitrate ion more
  • so weakening the N−O bonds more
71
Q

A student suggest that the difference in the rates of reaction of strontium and barium with water is due to the difference in the sum of their first and second ionisation energies. Discuss this suggestion.

A
  • The sum of the first two ionisation energies for barium is lower / barium loses (its outer) electrons more easily.
  • Barium is a bigger atom/barium has a larger atomic radii
  • Barium has greater shielding than Sr
  • These outweigh the fact that Barium has more protons.
  • Therefore Barium is more reactive.
72
Q

ionic equation for the reduction of chlorine molecules to chloride ions

A

Cl2 +2e- ——> 2Cl-

73
Q

All sodium halide reactions with concentrated sulfuric acid

A

Sodium chloride + concentrated sulfuric acid
Sodium bromide + concentrated sulfuric acid
Sodium iodide + concentrated sulfuric acid

74
Q

Equation for the disproportionate reaction from chlorate (1) ions to chlorate (v) and chloride ions on heating

A

3ClO- (aq) ——> ClO3- (aq) + 2Cl- (aq)

A Level Chemistry (15 decks)

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