Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Group 1 and 2 > Flashcards

Group 1 and 2 Flashcards

1
Q

What are group 2 metals also known as?

A

Alkali earth metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What do group 2 metals act as?

A

reducing agents as they give 2 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Do the metals in group 2 get more reactive going down the group?

A

Yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is the trend in ionisation energies down the group for group 1 and 2?

A

They decrease so becomes easier to remove the 2 outer electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the general equation of group 2 metals with oxygen?

A

2M +O2 = 2MO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What do Sr and Ba also form when reacted with oxygen?

A

Peroxides - MO2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the general equation for all group 2 metals with water?

A

M + 2H2O = M(OH)2 + H2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Which group 2 metal does not react with water?

A

Be

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Which group 2 metal reacts extremely slowly with cold water?

A

Mg

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What kind of solution is formed when Mg reacts with water and why?

A

It is weakly alkaline (pH 9) as magnesium hydroxide is only slightly soluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What happens when Mg is heated with steam?

A

It reacts vigorously to make MgO and H2
Mg + H2O = MgO + H2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What happens when group 2 metals react with chlorine gas?

A

They form a metal chloride

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are all group 2 oxides?

A

Basic - except for BeO which is amphoteric (can act as both an acid and a base)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is formed when group 2 oxides react with water?

A

Alkaline solutions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is observed when MgO reacts with water?

A

MgO is only slightly soluble in water, so weakly alkaline solution (pH 10) formed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is observed when CaO reacts with water?

A

Vigorous reaction which releases a lot of energy, causing some water to boil off as solid lump seems to expand and open (pH 11)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the general equation for group 2 oxides and water?

A

Oxide + water = hydroxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is calcium hydroxide known as when in solution?

A

Limewater

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is formed when a group 2 oxide react with sulphuric acid?

A

Group 2 sulphate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What happens when group 2 oxides react with sulphuric acid in terms of the actual reaction?

A

The insoluble sulphate forms at the surface of the oxide, so the solid oxide beneath it can’t react with acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

How can this (The insoluble sulphate forms at the surface of the oxide, so the solid oxide beneath it can’t react with acid) be prevented?

A

By using the oxide in powder form and stirring in which case neutralisation can’t take place

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is the general equation for group 2 oxides and HCl?

A

Oxide + dilute HCl = chloride + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the general equation for group 2 oxides and H2SO4?

A

Oxide + dilute H2SO4 = sulfate + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What do group 2 metal hydroxides form when reacted with a dilute acid?

A

Colourless solutions of metal salts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

How do the solubility of the sulphates change going down the group?

A

They decrease (barium sulphate is an insoluble white precipitate)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What is the general equation for group 2 hydroxides and HCl?

A

Hydroxide + dilute HCl = chloride + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What is the general equation for group 2 hydroxides and H2SO4?

A

Hydroxide + dilute H2SO4 = sulphate + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Going down the group, how does the alkalinity of the solutions formed from oxides with water change?

A

It becomes more alkaline

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What is the ionic reaction when oxides dissolve in water?

A

O2- + H2O = 2OH-

30
Q

What happens when we have a high concentration of OH- ions?

A

The more alkaline the solution

31
Q

What is equation for the hydroxides dissolving in water?

A

X(OH)2 = X + 2OH-

32
Q

How does the solubility of the hydroxides change going down the group?

A

It increases so the concentration of OH- ions increases, increasing the pH of the solution

33
Q

What is the connection between solubility and alkalinity for hydroxides?

A

As solubility increases, alkalinity increases

34
Q

What is the solubility like for group 2 sulphates?

A

Decreases down the group

35
Q

What is thermal decomposition?

A

The breakdown of a compound into 2 or more different substances using heat

36
Q

What happens when group 2 carbonates break down when heated?

A

They form the metal oxide and CO2

37
Q

What is the general equation when group 2 carbonates decompose?

A

XCO3 = XO + CO2

38
Q

What happens when group 2 nitrates decompose when heated?

A

They form the metal oxide, oxygen gas and nitrogen dioxide gas

39
Q

What is the general equation when group 2 nitrates decompose?

A

X(NO3)2 = XO +0.5O2 + 2NO2

40
Q

Why does the breakdown of group 2 nitrates need to happen in a fume cupboard?

A

Nitrogen dioxide gas it toxic

41
Q

What is needed more to breakdown the nitrates and carbonates of group 1 and 2 as you go down the groups?

A

Heat

42
Q

How does the thermal stability of group 1 and 2 change going down the group?

A

It increases

43
Q

Why will the smaller positive ions at the top of the groups polarise the anions more than the larger ions at the bottom of the group?

A
  • The small positive ion attracts the delocalised electrons in the carbonate ions towards itself
  • The higher the charge and the smaller the ion the higher the polarising power
44
Q

What happens as a result of group 1 and 2 carbonates and nitrates being more polarised?

A

The more likely they are to thermally decompose as the bonds in the carbonate and nitrate ions become weaker

45
Q

What will lithium carbonate produce when heated?

A

Lithium oxide and Carbon dioxide

46
Q

Apart from lithium, do the other group 1 carbonates decompose at bunsen temperatures?

A

No

47
Q

What is the only group 1 nitrate that will decompose completely and what does it produce?

A

Lithium - produces lithium oxide, nitrogen dioxide and oxygen

48
Q

What is nitrogen dioxide?

A

A brown, toxic gas

49
Q

What do the rest of the group 1 nitrates, apart from lithium, produce when decomposed?

A

The metal nitrite (NO2-) and oxygen
e.g.
2XNO3 = 2XNO2 + O2

50
Q

Why do we need higher temperature for decomposition as you go down group 1?

A

It gets more difficult

51
Q

What happens when metal ions are heated strongly?

A

They produce a colour

52
Q

Why can flame tests be used to identify metal ions?

A

Different metal ions produce different colours when heated

53
Q

What do we have to do first before we carry out a flame test?

A

Dip the loop of an un reactive metal (nichrome, platinum) in concentrated acid and hold it in the blue flame of a bunsen until there is no colour change

54
Q

Why do we have to clean the metal loop before we carry out a flame test?

A

To avoid contamination
- Test will only work if there is 1 type of ion present
- 2 or more ions means colours will mix, making identification erroneous

55
Q

How do we carry out the flame test?

A

Dip the clean loop into the solid sample and place it in the edge of the blue Bunsen flame

56
Q

What should we avoid during a flame test?

A

Letting the wire get so hot it glows red as this can be confused with a flame colour

57
Q

What does the heat of the flame test cause the electron in the metal ion to do?

A

Move to a higher energy level

58
Q

After the electron moves to the higher energy level in a flame test, why does it not stay there?

A

It is unstable at this energy level so it falls back down

59
Q

What creates the colour from the metal ion in a flame test?

A

As the electron drops back down from the higher energy level, energy is emitted in the form of visible light energy with the wavelength of the observed light

60
Q

What colour does Li+ produce?

A

Scarlet red

61
Q

What colour does Na+ produce?

A

Yellow

62
Q

What colour does K+ produce?

A

Lilac

63
Q

What colour does Rb+ produce?

A

Red

64
Q

What colour does Cs+ produce?

A

Blue

65
Q

What colour does Mg2+ produce?

A

No flame colour

66
Q

What colour does Ca2+ produce?

A

Brick red

67
Q

What colour does Sr2+ produce?

A

Red

68
Q

What colour does Ba2+ produce?

A

Apple green

69
Q

Why does Mg 2+ not have an observed flame colour?

A

The energy emitted is outside the visible spectrum

70
Q

What is the bonding like in metal oxides? What is the exception?

A

Ionic - except for BeO which has covalent character

Chemistry (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions