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Paper 1 CHEM MMS EXAM > ✅4 - Inorganic Chemistry and the Period Table > Flashcards

✅4 - Inorganic Chemistry and the Period Table Flashcards

1
Q

How does ionisation energy change down group 2?

A

It decreases

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2
Q

Why does ionisation energy decrease down Group 2?

A

The extra inner shells shield electrons

Nucleus is further away from outer electrons due to more shells

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3
Q

How does reactivity change down group 2?

A

Reactivity increases

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4
Q

Why does reactivity increase down group 2?

A

It becomes easier for the outer electrons to be lost, as they have lower ionisation energies

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5
Q

What do group 2 elements react with?

A

Water, oxygen and chlorine

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6
Q

What are the group 2 elements?

A

Beryllium, Magnesium, Calcium, Strontium, Barium (Radium)

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7
Q

What do group 2 elements produce when they react with water?

A

Hydroxides and hydrogen

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8
Q

Which group 2 elements react with water?

A

All except Be, Mg reacts very slowly

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9
Q

What do group 2 elements produce when they react with oxygen?

A

Oxides

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10
Q

What colour are group 2 oxides?

A

White

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11
Q

What do group 2 elements produce when they react with chlorine?

A

Chlorides

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12
Q

What colour are group 2 chlorides?

A

White

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13
Q

Oxides and hydroxides are…

A

…bases

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14
Q

What happens when group 2 oxides dissolve in water?

A

They form a strongly alkaline solution due to OH-

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15
Q

What happens when beryllium oxide is added to water?

A

It doesn’t dissolve, it is insoluble

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16
Q

What happens when magnesium oxide is added to water?

A

It reacts slowly and isn’t very soluble

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17
Q

When oxides and hydroxides are added to acid, what do they form?

A

They neutralise the acid to form salts

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18
Q

What is the equation for the reaction between MgO and H2O?

A

MgO + H2O —-> Mg(OH)2

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19
Q

What is the equation for the reaction between MgO and HCl?

A

MgO + 2HCl —-> MgCl2 + H2O

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20
Q

Solubility trends of group 2 depend on…

A

…the anion

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21
Q

If a group 2 compound has a singly charged anion (OH-) how does the solubility change down the group?

A

It increases

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22
Q

If a group 2 compound has a doubly charged anion (SO4 2-) how does the solubility change down the group?

A

It decreases

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23
Q

Which group 2 sulfate is insoluble?

A

Barium Sulfate

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24
Q

How does thermal stability change down group 1 and 2 carbonates and nitrates?

A

It increases

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25
Why do carbonates and nitrates become more stable down the group?
Large ions have less polarising power so distort the electron cloud less and have a lower charge density. Therefore, they distort the carbonate or nitrate less
26
Which of group 1 and group two compounds are more thermally stable?
Group 1
27
Why are Group 1 compounds more stable than group 2?
They have a lower charge, so a lower charge density and therefore less polarising power
28
What do group 2 carbonates decompose to form?
An oxide and carbon dioxide
29
What is the equation for thermal decomposition of CaCO3?
CaCO3 ----> CaO + CO2
30
Do group 1 carbonates decompose?
No
31
What do group 1 nitrates decompose to form?
The Nitrite (NO2) and oxygen
32
What is the equation for decomposition of Potassium nitrate?
2KNO3 ----> 2KNO2 + O2
33
What is the exception to the group 1 nitrate decomposition?
Lithium
34
What does lithium nitrate decompose to form?
LiO2, NO2 and O2
35
What doe group 2 nitrates decompose to form?
The oxide, nitrogen dioxide and oxygen
36
What is the equation for the decomposition of Ca(NO3)2?
2Ca(NO3)2 ----> 2CaO + 4NO2 + O2
37
How can the thermal stability of nitrates be tested?
Measuring how long it takes for a certain amount of oxygen to be produced OR How long it takes for brown gas (NO2) to be produced
38
How can the thermal stability of carbonates be tested?
Measuring how long it takes for a certain amount of CO2 to be produced using lime water
39
What is the flame colour for Lithium?
Red
40
What is the flame colour for Sodium?
Orange/Yellow
41
What is the flame colour for Potassium?
Lilac
42
What is the flame colour for Rubidium?
Red
43
What is the flame colour for Caesium?
Blue
44
What is the flame colour for Calcium?
Brick red
45
What is the flame colour for Strontium?
Crimson
46
What is the flame colour for Barium?
Apple green
47
Why is a colour produced during a flame test?
The electrons are excited to a higher energy level and then as they drop back down, they release the energy in the form of light.
48
What determines the wavelength of light produced in a flame test?
The difference between the higher and lower energy levels
49
What is the solubility of halogens?
Low, as they are non polar
50
What do halogens dissolve easily in?
Cyclohexane
51
How can halogens be identified when dissolved in organic compounds?
They have distinctive colours
52
What colour is bromine in hexane?
Orange/Red
53
What colour is iodine in hexane?
Purple
54
How does the reactivity of halogens change down the group?
It decreases
55
How do the melting and boiling points of halogens change down the group?
They increase
56
Why do melting and boiling points increase down group 7?
There are more electron shells, so greater London forces
57
What can chlorine displace?
Br- and I-
58
What can bromine displace?
I-
59
What redox property do halogens have?
They are reducing agents
60
How do halogens react with group 1 metals?
They produce halide salts, so the metal is reduced and the halogen oxidised
61
What is the equation for the reaction between Li and F?
2Li + F2 ----> 2LiF
62
How do halogens react with group 2 metals?
They form halide salts, where the metal is reduced and the halogen oxidised
63
What type of reaction occurs between halogens and cold alkalis?
Disproportionation
64
What is the equation for the reaction between I2 and NaOH?
I2 + 2NaOH ----> NaOI + NaI + H2O
65
What type of reaction do halogens undergo with hot alkali?
Disproportionation
66
What compound is used to kill bacteria?
Chlorate (I) - ClO-
67
How does the reducing power of halides change down the group?
It increases
68
What is the equation for the reaction between KCl and H2SO4?
KCl + H2SO4 ----> KHSO4 + HCl
69
What happens during the reaction between KCl and H2SO4?
HCl gas is given off as misty fumes Cl- aren't strong enough reducing agents to reduce sulfuric acid, so reaction stops there Not a redox reaction
70
What are the equations for the reaction between KBr and H2SO4?
KBr + H2SO4 ----> KHSO4 + HBr | 2HBr + H2SO4 ----> Br2 + SO2 + 2H2O
71
What happens during the reaction between KBr and H2SO4?
The first reaction gives misty fumes of HBr Br- are stronger reducing agents so react with H2SO4 in a redox reaction The reaction produces fumes of sulfur dioxide and orange fumes of Br2
72
What are the equations for the reactions between Kl and H2SO4?
KI + H2SO4 ----> KHSO4 + HI 2HI + H2SO4 ----> I2 + SO2 + 2H2O 6HI + SO2 ----> H2S + 3I2 + 2H2O
73
What happens during the reactions between Kl and H2SO4?
HI gas is produced in the initial reaction Iodide ions then reduce H2SO4 as before I- is a strong reducing agent and reduced the SO2 to H2S
74
What are hydrogen halides?
Acidic gases
75
How do hydrogen halides behave in water?
The dissolve
76
How do hydrogen halides react with ammonia?
They give off white fumes of ammonium halides
77
What colour precipitate does Chlorine give with Silver Nitrate?
White
78
What colour precipitate does Bromine give with Silver Nitrate?
Cream
79
What colour precipitate does Iodine give with Silver Nitrate?
Yellow
80
How does AgCl behave with ammonia?
The precipitate dissolves to give a colourless solution
81
How does AgBr behave with ammonia?
The precipitate remains unchanged in dilute, but will dissolve in conc ammonia
82
How does AgI behave with ammonia?
The precipitate will not dissolve, even in conc ammonia
83
What is the test for carbonates?
Add dilute hydrochloric acid and use lime water to test for any CO2 given off
84
What is the test for Sulfates?
Add dilute HCl and BaCl2. If a white precipitate forms, a sulfate is present The hydrochloric acid is needed to react with carbonate impurities that are often found in salts which would form a white Barium carbonate precipitate and so give a false result. You could not used sulphuric acid because it contains sulphate ions and so would give a false positive result.
85
How is ammonia tested for?
It is alkaline, so damp red litmus paper can be used. If ammonia gas is present, the paper will turn blue
86
How are ammonium ions tested for?
Add sodium hydroxide and gently heat the mixture. If ammonia is given off, ammonium ions were present

Paper 1 CHEM MMS EXAM (12 decks)

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