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Chemistry > Group 2 And 7 Elements > Flashcards

Group 2 And 7 Elements Flashcards

1
Q

How many electrons on outermost shell of group 2

A

2

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2
Q

what do group 2 metals form

A

ionic compounds where they donate these two outermost electrons (so they act as reducing agents) to become an ion with +2 charge (so they themselves become oxidised)

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3
Q

Going down the group do group 2 elements get more reactive or less

A

more

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4
Q

what does the first ionisation energy do

A

the energy needed to remove the first outer electron of an atom

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5
Q

What happens to the size of the elements down group 2

A

become larger as the outer two electrons occupy a new shell which is further away from the nucleus

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6
Q

What happens to the melting point of the elements down group 2

A

The melting point of the elements decreases going down the group as the outer electrons get further away from the nucleus

This means that the attraction between the nucleus and the bonding electrons decreases causing a decrease in melting point

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7
Q

what happens as you go down the group to the density of the alkali earth metals

A

the density of the alkali earth metals drops till Calcium and then increases

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8
Q

What happens when the group 2 metal oxide reacts with water

A

a group 2 hydroxide is formed

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9
Q

what happens to the solubility of these hydroxides, going down the group

A

increases.
This means that the concentration of OH- ions increases, increasing the pH of the solution

As a result, going down the group, the alkalinity of the solution formed increases when Group 2 oxides react with water

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10
Q

Magnesium (group 2 metal) reacting with water at room temp
Equation and description

A

Mg(s) + 2H2O(l) –> Mg(OH)2(aq) + H2(g)
Very slow reaction with Mg. It will take several hours for bubbles of H2 to start to show.

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11
Q

What is Mg(OH)2 (aq) used for

A

Magnesium Hydroxide can also be called ‘Milk of Magnesia’ and is used as an indigestion remedy to neutralise stomach acid.

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12
Q

Calcium (group 2 metal) reacting with water at room temp
Equation and description

A

Ca(s) + 2H2O(l) –> Ca(OH)2(aq) + H2(g)
More vigorous reaction with Ca. It will bubble at a fast rate and the mixture will heat up.

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13
Q

Magnesium (group 2 metal) reacting with steam
Equation and description

A

Mg(s) + H2O(l) –> MgO(s) + H2(g)
reaction more vigorous with steam than water

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14
Q

How soluble is Mg(OH)2

A

Insoluble

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15
Q

How soluble is Ba(OH)2

A

Completely dissolves

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16
Q

How soluble is MgSO4

A

Completely Dissolved

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17
Q

How soluble is BaSO4

A

Insoluble

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18
Q

What is BaSO4 (Barium Sulfate) used for

A

Barium Sulfate is very good at absorbing X rays. Feed the patient a ‘Barium Meal’.
Barium Sulfate is highly toxic. However it is perfectly safe to feed to patients because it is so insoluble it cannot dissolve and pass through cell membranes into body tissue

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19
Q

How to test for Sulfate Ions (SO4 2-)

A

add a solution of Barium Chloride (BaCl2)
no visible change = NO Sulfate ions present
WHITE PRECIPITATE = Sulfate ions present

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20
Q

Group 7 also known as

A

Halogens

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21
Q

What is the ion of florine called

A

Fluoride (F-)

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22
Q

Physical property of Fluorine

A

very pale yellow gas

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23
Q

Physical property of Chlorine

A

greenish gas.

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24
Q

Physical property of Bromine

A

orange/brown liquid which vaporizes easily into an orange gas.

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25
Q

Physical property of Iodine

A

a black solid which vaporises on heating to a purple gas.

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26
Q

What happens to the size of group 7 going down the group

A

get bigger on descending the group because each additional element has a whole extra electron shell in comparison to the previous element

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27
Q

What are three factors that affect electronegativity

A
  • A greater nuclear charge will withdraw electrons more strongly.
  • A shorter atomic radius will also help withdraw electrons more strongly.
  • The more shielding will however reduce the amount electrons can be withdrawn.
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28
Q

What intermolecular forces exist between halogens

A

As they are non-polar diatomic molecules, they only have Van der Waals forces.

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29
Q

What changes the strength of the van de wall forces in group 7

A

on the size of the molecule

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30
Q

What element in group 7 has the lowest boiling and melting point

A

F2

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31
Q

What state is Fluorine and chlorine at room temperature

A

gas

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32
Q

What state is bromine at room temperature

A

liquid

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33
Q

What state is iodine at room temperature

A

solid

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34
Q

in group 7 which element is the strongest oxidizing element

A

Fluorine as it accepts electrons the easiest

35
Q

During halogen displacement reactions what should the element HIGHEST UP Group 7 form

A

HALIDE ION

36
Q

During halogen displacement reactions what should the halogen LOWEST DOWN Group 7 form

A

HALOGEN MOLECULE

37
Q

Reacting Chlorine with Sodium Bromide
equation and explanation

A

Cl2(aq)+2NaBr(aq) –> Br2(aq) + 2NaCl(aq)

Because Chlorine is higher in Group 7 than Bromine, the Chlorine displaces the Bromide to form Sodium Chloride, and the Bromide is converted to Bromine.

38
Q

Reacting Chlorine with Potassium Fluorine
equation and explanation

A

Cl2(aq) + 2KF(aq) –> No Reaction

Fluorine is higher in Group 7 than Chlorine. This means Fluorine should exist at Fluoride ions, and the Chlorine should exist as a Chlorine molecule. These are already present in the reactants, and so no reaction occurs.

39
Q

What are halogens in form of an ‘agent’

A

OXIDISING AGENT

40
Q

What are halide ions in form of an ‘agent’

A

REDUCING AGENT

41
Q

Equation of Mg with steam

A

Mg (s) + H2O (g) → MgO (s) + H2 (g)

42
Q

Equation of Ca with water

A

Ca (s) + 2H2O (l) → Ca(OH)2 (s) + H2 (g)

43
Q

Equation of Sr with water

A

Sr (s) + 2H2O (l) → Sr(OH)2 (aq) + H2 (g)

44
Q

Equation of Ba with water

A

Ba (s) + 2H2O (l) → Ba(OH)2 (aq) + H2 (g)

45
Q

Equation of Mg with water

A

Mg (s) + 2H2O (l) → Mg(OH)2 (aq) + H2 (g)

46
Q

Equation of Mg with dilute HCL

A

Mg (s) + 2HCl (aq) → MgCl2 (aq) H2 (g)

47
Q

Reaction with Ca with dilute HCL

A

Ca (s) + 2HCl (aq) → CaCl2 (aq) H2 (g)

48
Q

Reaction with Sr with dilute HCL

A

Sr (s) + 2HCl (aq) → SrCl2 (aq) H2 (g)

49
Q

Reaction with Ba with HCL

A

Ba (s) + 2HCl (aq) → BaCl2 (aq) H2 (g)

50
Q

Reaction with Mg with H2SO4

A

Mg (s) + H2SO4 (aq) → MgSO4 (aq) + H2 (g)

51
Q

Reaction with Ca with H2SO4

A

Ca (s) + H2SO4 (aq) → CaSO4 (aq) + H2 (g)

52
Q

Reaction with Sr with H2SO4

A

Sr (s) + H2SO4 (aq) → SrSO4 (s) + H2 (g)

53
Q

Reaction with Ba with H2SO4

A

Ba (s) + H2SO4 (aq) → BaSO4 (s) + H2 (g)

54
Q

oxide + water ->

55
Q

metal oxide + dilute hydrochloric acid ->

A

metal chloride + water

56
Q

Equation of Mg(OH)2 with dilute HCL

A

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

57
Q

Equation of Ca(OH)2 with dilute HCL

A

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

58
Q

Equation of Sr(OH)2 with dilute HCL

A

Sr(OH)2 (s) + 2HCl (aq) → SrCl2 (aq) + 2H2O (l)

59
Q

Equation of Ba(OH)2 with dilute HCL

A

Ba(OH)2 (s) + 2HCl (aq) → BaCl2 (aq) + 2H2O (l)

60
Q

Reaction of Mg(OH)2 with dilute H2SO4

A

Mg(OH)2 (s) + H2SO4 (aq) → MgSO4 (aq) + 2H2O (l)

61
Q

Reaction of Ca(OH)2 with dilute H2SO4

A

Ca(OH)2 (s) + H2SO4 (aq) → CaSO4 (aq) + 2H2O (l)

62
Q

Reaction of Sr(OH)2 with dilute H2SO4

A

Sr(OH)2 (s) + H2SO4 (aq) → SrSO4 (s) + 2H2O (l)

63
Q

Reaction of Ba(OH)2 with dilute H2SO4

A

Ba(OH)2 (s) + H2SO4 (aq) → BaSO4 (s) + 2H2O (l)

64
Q

hydroxide + dilute hydrochloric acid →

A

chloride + water

65
Q

hydroxide + dilute sulfuric acid →

A

sulfate + water

66
Q

Reaction of MgCO3 with dilute HCL

A

MgCO3 (s) + 2HCl (aq) → MgCl2 (aq) + H2O (l) + CO2 (g)

67
Q

Reaction of CaCO3 with dilute HCL

A

CaCO3 (s) + 2HCl (aq) → CaCl2 (aq) + H2O (l) + CO2 (g)

68
Q

Reaction of SrCO3 with dilute HCL

A

SrCO3 (s) + 2HCl (aq) → SrCl2 (aq) + H2O (l) + CO2 (g)

69
Q

Reaction of BaCO3 with dilute HCL

A

BaCO3 (s) + 2HCl (aq) → BaCl2 (aq) + H2O (l) + CO2 (g)

70
Q

Reaction of CaCO3 with dilute H2SO4

A

CaCO3 (s) + H2SO4 (aq) → CaSO4 (aq) + H2O (l) + CO2 (g)

71
Q

Reaction of MgCO3 with dilute H2SO4

A

MgCO3 (s) + H2SO4 (aq) → MgSO4 (aq) + H2O (l) + CO2 (g)

72
Q

Reaction of SrCO3 with dilute H2SO4

A

SrCO3 (s) + H2SO4 (aq) → SrSO4 (s) + H2O (l) + CO2 (g)

73
Q

Reaction of BaCO3 with dilute H2SO4

A

BaCO3 (s) + H2SO4 (aq) → BaSO4 (s) + H2O (l) + CO2 (g)

74
Q

carbonate + dilute hydrochloric acid →

A

chloride + water + carbon dioxide

75
Q

carbonate + dilute sulfuric acid →

A

sulfate + water + carbon dioxide

76
Q

what is impure calcium carbonate used for

77
Q

What is calcium oxide used for

78
Q

what is s calcium hydroxide used for

A

Slaked lime

79
Q

What are limestone, quick lime and Slaked lime used for and why it used

A

used in agriculture to raise the pH of the soil
Calcium carbonate is more commonly used in agricultural lime as it is cheaper and safer to handle

80
Q

Uses of Barium

A

sed in medicine in the form of barium sulfate, BaSO4
Barium absorbs X-rays which means the gut shows up white on the image

Barium is toxic though can be used in this form because
Barium sulfate is insoluble so is not absorbed into the blood

81
Q

Uses of Magnesium

A

‘milk of magnesia’ used to neutralise excess acid in the stomach and treat constipation

82
Q

colour of Silver chloride precipitate

83
Q

colour of Silver bromide precipitate

A

Cream precipitate

84
Q

colour of silver iodide precipitate

A

yellow precipitate

Chemistry (38 decks)

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