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CHEMISTRY > Group 2 / Group 7 > Flashcards

Group 2 / Group 7 Flashcards

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1
Q

By what name are the group II metals also known?

A

alkali earth metals

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2
Q

State and explain the trend in atomic radius down group 2

A

Size increases down the group
Shielding increases
So the outer shell electrons are further from the nucleus

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2
Q

State and explain the trend in first ionization energy down group 2

A

On descending the group
Shielding increases
Attraction between the nucleus and outer electrons decreases

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3
Q

State and explain the trend in melting point down group 2

A

The size of the cations increases down the group
Attraction between cations and delocalised electrons decreases
So the metallic bonding gets weaker

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4
Q

State and explain how the reactivity of the group II elements to water changes down the group

A

On descending the group
Shielding increases
Attraction between nucleus and outer electrons decreases
Outer electrons are more easily lost

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5
Q

write an equation for the reaction of magnesium with steam

A

Mg(s) + H2O(g) –> MgO(s) + H2(g)

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6
Q

write an equation for the reaction of calcium with water

A

Ca(s) + 2H2O(l) –> Ca(OH)2(s) + H2(g)

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7
Q

write an equation for the reaction of barium with water

A

Ba(s) + 2H2O(l) –> Ba(OH)2(s) + H2(g)

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8
Q

State two differences you would observe in the reactions of calcium and barium with water

A

the reaction with calcium would be slower and the solution would go cloudy

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9
Q

State the trend in the solubility of the Group II sulphates

A

decreases down group

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10
Q

State the trend in the solubility of the Group II hyrdoxides

A

increases down group

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11
Q

State what you would observe when barium chloride and sulphuric acid are mixed, and write ionic equations for any reactions you observe

A

white precipitate
Ba2+(aq) + SO42-(aq) –> BaSO4(s)

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12
Q

State what you would observe when barium chloride and sodium hydroxide are mixed, and write ionic equations for any reactions you observe

A

no reaction

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13
Q

State what you would observe when magnesium chloride and sodium hydroxide are mixed, and write ionic equations for any reactions you observe

A

white precipitate: Mg2+(aq) + 2OH-(aq) –> Mg(OH)2(s)

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14
Q

State what you would observe when calcium chloride and sodium hydroxide are mixed, and write ionic equations for any reactions you observe

A

faint white precipitate: Ca2+(aq) + 2OH-(aq) –> Ca(OH)2(s)

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15
Q

State what you would observe when calcium chloride and sulphuric acid are mixed, and write ionic equations for any reactions you observe

A

faint white precipitate: Ca2+(aq) + SO42-(aq) –> CaSO4(s)

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16
Q

State what you would observe when magnesium chloride and sulphuric acid are mixed, and write ionic equations for any reactions you observe

A

no reaction

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17
Q

Describe a suitable test for sulphate ions in solution

A

Add dilute hydrochloric acid followed by barium chloride solution
A white precipitate will be observed

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18
Q

Explain how BaSO4 is used in medicine

A

BaSO4 is consumed in a “barium meal”; it absorbs X-rays and so its path through the digestive system can be tracked using X-rays

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19
Q

Explain how MgSO4 is used in medicine

A

MgSO4 is consumed in order to treat Mg deficiency

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20
Q

Write an equation for the reaction between magnesium hydroxide and hydrochloric acid

explain a useful application of this reaction

A

Mg(OH)2(s) + 2HCl(aq) –> MgCl2(aq) + 2H2O(l)

used to treat indigestion caused by excess stomach acid

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21
Q

Write an equation for the reaction between calcium hydroxide and hydrochloric acid

explain a useful application of this reaction

A

Ca(OH)2(s) + 2HCl(aq) –> CaCl2(aq) + 2H2O(l)

used to neutralize acidic soils

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22
Q

Write an equation for the reaction between calcium oxide and sulphur dioxide

explain a useful application of this reaction

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A

CaO(s) + SO2(g) –> CaSO3(s)

used to remove SO2 from factory chimneys

23
Q

Write an equation for the reaction between calcium carbonate with sulphur dioxide

explain a useful application of this reaction

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A

CaCO3(s) + SO2(g) –> CaSO3(s) + CO2(g)

used to remove SO2 from factory chimneys

24
Explain the use of magnesium in the extraction of titanium from TiCl4
The Mg reduces the TiCl4 to Ti by the reaction TiCl4 + 2Mg --> Ti + 2MgCl2 reducing agent
25
By what name are the elements F2, Cl2, Br2 and I2 collectively known?
halogens
26
By what name are the ions F-, Cl-, Br- and I- collectively known?
halides
27
State and explain the trend in electronegativity of the Group 7 elements
decreases down group more shells bonding electrons more shielded from nucleus atom less able to attract bonding electrons to itself
28
State and explain the trend in boiling point of the Group 7 elements
increases down group molecules have more electrons/larger surface area so stronger Van der Waal’s forces so more energy required to separate the molecules
29
Explain why the halogens are all oxidizing agents and state and explain the trend in oxidizing ability of the halogens
they have only seven electrons in the outer shell so can act as electron acceptors and become halides Oxidising ability decreases down group more shielding So the incoming electron is less strongly attracted to the nucleus
30
Explain why the halides are all reducing agents and state and explain the trend in reducing ability of the halides
they can lose electrons to become halogens reducing ability increases down group more shells means more shielding So electrons can be more easily lost from the outer shell
31
Predict whether or not a reaction would take place between SODIUM CHLORIDE AND IODINE. If a reaction does take place, state what you would observe and write an ionic equation for the reaction taking place
no change stays brown
32
Predict whether or not a reaction would take place between SODIUM IODIDE AND CHLORINE. If a reaction does take place, state what you would observe and write an ionic equation for the reaction taking place
brown solution Cl2(aq) + 2I-(aq) --> 2Cl-(aq) + I2(aq)
33
Predict whether or not a reaction would take place between SODIUM BROMIDE AND IODINE. If a reaction does take place, state what you would observe and write an ionic equation for the reaction taking place
no change; stays brown
34
Predict whether or not a reaction would take place between SODIUM IODIDE AND BROMINE. If a reaction does take place, state what you would observe and write an ionic equation for the reaction taking place
brown solution Br2(aq) + 2I-(aq) --> 2Br-(aq) + I2(aq)
35
Predict whether or not a reaction would take place between POTASSIUM CHLORIDE AND BROMINE. If a reaction does take place, state what you would observe and write an ionic equation for the reaction taking place
no change; stays orange
36
Predict whether or not a reaction would take place between POTASSIUM BROMIDE AND CHLORINE. If a reaction does take place, state what you would observe and write an ionic equation for the reaction taking place
yellow/orange solution; Cl2(aq) + 2Br-(aq) --> 2Cl-(aq) + Br2(aq)
37
write a half equation for this reaction: I- to I2
2I- --> I2 + 2e
38
write a half equation for this reaction: Br- to Br2
2Br- --> Br2 + 2e
39
write a half equation for this reaction: H2SO4 to SO2
H2SO4 + 2H+ + 2e --> SO2 + 2H2O
40
write a half equation for this reaction: H2SO4 to H2S
H2SO4 + 8H+ + 8e --> H2S + 4H2O
41
Chloride ions cannot reduce concentrated sulphuric acid. Bromide ions reduce concentrated sulphuric acid to sulphur dioxide. Iodide ions reduce concentrated sulphuric acid to hydrogen sulphide. Explain these observations in terms of the relative reducing ability of the halides
Cl- is the weakest reducing agent and I- is the strongest reducing agent Reducing power increases down the group; more shells and more shielding mean that the attraction between the outermost electrons and the nucleus is weaker and the species is a better electron donor Cl- cannot reduce H2SO4 Br- reduces S in H2SO4 from +6 to +4 I- reduces S in H2SO4 from +6 to -2:
42
Write an equation to show the reaction between Iodide ions and concentrated sulphuric acid
H2SO4 + 2H+ + 2Br- --> SO2 + Br2 + 2H2O
43
Write an equation to show the reaction between Bromide ions and concentrated sulphuric acid
H2SO4 + 8H+ + 8I- --> H2S + 4I2 + 4H2O
44
10) Chloride ions react with concentrated sulphuric acid to give hydrogen chloride gas. Write an equation for this reaction and show that it is not a redox reaction
H2SO4 + Cl- --> HSO4- + HCl The oxidation number of S is +6 in both reactant and product
45
Write an equation to show the reaction between chlorine and water to make chloric (I) acid State what is oxidized and what is reduced in this reaction State an application of this reaction
Cl2 + H2O == HCl(aq) + HClO(aq) Cl is both oxidised (from 0 to +1) and reduced (from 0 to -1) this is used to sterilise water; HClO is a sterilising agent
46
State what happens when chlorine is added to water in the presence of bright sunlight State what is oxidized and what is reduced in this reaction
2Cl2 + 2H2O --> 4HCl + O2 Cl is reduced (from 0 to -1) and O is oxidized (from -2 to 0)
47
Explain why chlorine is added to the water supply
Chlorine is added to the water supply to kill harmful bacteria (ie to sterilize the water)
48
State one advantage and one disadvantage of adding chemicals to the water supply
Adding chemicals to the water supply can have health benefits by killing harmful toxins or providing important nutrients. The chemicals added to the water supply can themselves be toxic to some people and they take away the right of the individual to choose whether to add chemicals to their water
49
Write an equation to show the reaction between chlorine and sodium hydroxide to make sodium chlorate (I) State what is oxidized and what is reduced in this reaction State an application of this reaction
Cl2 + NaOH --> NaCl(aq) + NaClO(aq) + H2O Cl is both oxidised (from 0 to +1) and reduced (from 0 to -1) this is used to make bleach
50
what is the test for OH-
NH4CL and warm produces pungent smell
51
what is the test for Mg2+
aq NaOH thick white ppt formed
52
what is the test for Ca2+
aq NaOH faint white ppt formed
53
what is the test for Sr2+
H2SO4 faint white ppt formed
54
what is the test for Ba2+
H2SO4 thick white ppt
55
what is the test for NH4+
NaOH and warm produced pungent smell
56
Test for H+
Na2CO3 effervescence

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