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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

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

A

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

used to remove SO2 from factory chimneys

24
Q

Explain the use of magnesium in the extraction of titanium from TiCl4

A

The Mg reduces the TiCl4 to Ti by the reaction TiCl4 + 2Mg –> Ti + 2MgCl2

reducing agent

25
Q

By what name are the elements F2, Cl2, Br2 and I2 collectively known?

A

halogens

26
Q

By what name are the ions F-, Cl-, Br- and I- collectively known?

A

halides

27
Q

State and explain the trend in electronegativity of the Group 7 elements

A

decreases down group
more shells
bonding electrons more shielded from nucleus
atom less able to attract bonding electrons to itself

28
Q

State and explain the trend in boiling point of the Group 7 elements

A

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
Q

Explain why the halogens are all oxidizing agents and state and explain the trend in oxidizing ability of the halogens

A

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
Q

Explain why the halides are all reducing agents and state and explain the trend in reducing ability of the halides

A

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
Q

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

A

no change

stays brown

32
Q

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

A

brown solution

Cl2(aq) + 2I-(aq) –> 2Cl-(aq) + I2(aq)

33
Q

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

A

no change; stays brown

34
Q

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

A

brown solution

Br2(aq) + 2I-(aq) –> 2Br-(aq) + I2(aq)

35
Q

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

A

no change; stays orange

36
Q

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

A

yellow/orange solution;

Cl2(aq) + 2Br-(aq) –> 2Cl-(aq) + Br2(aq)

37
Q

write a half equation for this reaction:

I- to I2

A

2I- –> I2 + 2e

38
Q

write a half equation for this reaction:

Br- to Br2

A

2Br- –> Br2 + 2e

39
Q

write a half equation for this reaction:

H2SO4 to SO2

A

H2SO4 + 2H+ + 2e –> SO2 + 2H2O

40
Q

write a half equation for this reaction:

H2SO4 to H2S

A

H2SO4 + 8H+ + 8e –> H2S + 4H2O

41
Q

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

A

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
Q

Write an equation to show the reaction between Iodide ions and concentrated sulphuric acid

A

H2SO4 + 2H+ + 2Br- –> SO2 + Br2 + 2H2O

43
Q

Write an equation to show the reaction between Bromide ions and concentrated sulphuric acid

A

H2SO4 + 8H+ + 8I- –> H2S + 4I2 + 4H2O

44
Q

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

A

H2SO4 + Cl- –> HSO4- + HCl

The oxidation number of S is +6 in both reactant and product

45
Q

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

A

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
Q

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

A

2Cl2 + 2H2O –> 4HCl + O2

Cl is reduced (from 0 to -1) and O is oxidized (from -2 to 0)

47
Q

Explain why chlorine is added to the water supply

A

Chlorine is added to the water supply to kill harmful bacteria (ie to sterilize the water)

48
Q

State one advantage and one disadvantage of adding chemicals to the water supply

A

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
Q

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

A

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
Q

what is the test for OH-

A

NH4CL and warm

produces pungent smell

51
Q

what is the test for Mg2+

A

aq NaOH

thick white ppt formed

52
Q

what is the test for Ca2+

A

aq NaOH

faint white ppt formed

53
Q

what is the test for Sr2+

A

H2SO4

faint white ppt formed

54
Q

what is the test for Ba2+

A

H2SO4

thick white ppt

55
Q

what is the test for NH4+

A

NaOH and warm

produced pungent smell

56
Q

Test for H+

A

Na2CO3

effervescence

CHEMISTRY (8 decks)

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