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Chemistry Year 1 > Topic 4 Periodic table > Flashcards

Topic 4 Periodic table Flashcards

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1
Q

what do water and group 2 metal react to form

A

metal hydroxides

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2
Q

What is the reaction between magnesuim & water like

A

reacts very slowly + bubbles of hydrogen gas form

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3
Q

what can be seen in the reaction of G2 metal with water

A
  • As you go down the group the level of bubbling, effervecence & vigour increase
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4
Q

what is the model reaction of G2 metals with water

A

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

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5
Q

what does calcuim form in the reaction with water

A

white precipitate

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6
Q

what does Sr form in the reaction with water

A

Colourless solution

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7
Q

what does Ba form in the reaction with water

A

Colourless solution

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8
Q

what do G2 metals form when they react with oxygen

A

metal oxides

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9
Q

what is the model equation of the reaction of G2 metal with oxygen

A

2M + O2 = 2MO

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10
Q

what is formed when G2 metal react with chlorine

A

Metal Chlorides

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11
Q

what is the model equation for the reaction of G2 metals with chlorine

A

M + Cl2 = MCl2

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12
Q

what is the observation in the reaction between G2 metals and chlorine

A

a yellow glow can be seen

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13
Q

what happens in the reaction between magnesuim & steam

A

Reacts very vigourously

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14
Q

what is formed with magnesuim is reacted with steam

A

Magnesuim Oxide

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15
Q

What is formed when G2 oxides react with water

A

Metal Hydroxides

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16
Q

What happens to the alkalinity of the G2 hydroxides as you go down the group

A

Become more alkaline as there is more OH being dissolved

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17
Q

what are formed when G2 oxides are reacted with acids

A

Salt (either sulphate or chloride)
Water

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18
Q

what happens when G2 hydroxides are reacted with acids

A

forms colourless solution of metal salts

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19
Q

what happens to the solubility of G2 hydroxides as you go down the group

A

increase

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20
Q

what happens to the solubility of G2 sulphates as you go down the group

A

decrease

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21
Q

what can be used as test for sulpahtes

A

adding HCL & baruim chloride to form baruim sulphate which is a white precipitate

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22
Q

what is thermal decomposition

A

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

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23
Q

what is formed in the TD of G2 carbonates

A

Group 2 Carbonates breakdown via thermal decomposition to form metal oxides and carbon dioxide.

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24
Q

what happens to G2 carbonates as you go down the group and what is required

A

Going down the group, the carbonates become more stable, and more heat is needed to break them.

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25
Q

what is formed in the TD of G2 nitrates

A

Group 2 nitrates undergo thermal decomposition to form metal oxide, nitrogen dioxide and oxygen.

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26
Q

how does each of the products of the TD of G2 nitrates look like

A

The group 2 nitrates are white solids, the metal oxide is also a white solid. Nitrogen dioxide is a brown gas

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27
Q

what is one precaution that must be taken in the TD of G2 nitrates

A

Since nitrogen dioxide is toxic, the thermal decomposition of nitrates take place in a fume cupboard.

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28
Q

what happens to G2 nitrates as you go down the group and what is required

A

The nitrates become more stable down the group and so require more heat.

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29
Q

what happen during thermal stability reaction

A

when carbonate/nitrate ion is placed near positive G2 ion the G2 ion attracts the delocalised electrons towards itself. The carbonate/nitrate ion becomes polarized which then weakens the C-O bond. If this is heated then the CO2 breaks free and forms a metal oxide

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30
Q

how the reaction between carbonate ion & G2 cation change as you go down the group

A
  • As you go down the group the size of ion increases which decreases the charge density.
  • The ability to polarize the carbonate ion decreases
  • The C-O bond in the carbonate ion is weakened less
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31
Q

what does TD of G1 nitrate form

A
  • Metal Nitrate
  • Oxygen
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32
Q

what happens in the TD of G1 carbonate

A
  • Decomposition won’t take place as they require high temperaturs
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33
Q

which element is an exception for the pattern of the TD of G1 nitrates and what does it form

A
  • Lithuim
  • Forms Metal Nitrate, Nitrogen dioxide and oxygen
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34
Q

what are the 3 steps to flame test

A
  1. Clean platinuim/nichrome wire by dipping in concentrated HCL
  2. Dip into the sample
  3. Place the loop into Blue bunsen burner
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35
Q

why do we get different colours in the flame test

A

Electrons in the shells move to higher energy levels as they absorb energy from the flame. When they drop back down to lower energy level, they release energy in the form of light. The colour depends on the wavelength of light energy transmitted.

36
Q

why do some ions not have a colour

A

When some electrons drop back down to lower orbitals, the energy emitted may not have a wavelength in the visible light part of the electromagnetic spectrum, which explains why not all atoms and ions produce a colour in the flame test.

37
Q

what colour does lithuim form

A

crimson

38
Q

what colour does soduim form

A

yellow-orange

39
Q

what colour does pottasuim form

A

Lilac

40
Q

what colour does Rubiduim form

A

Red

41
Q

What colour does Caesuim form

A

Blue

42
Q

what colour does Berylluim form

A

No colour

43
Q

what colour does magnesuim form

A

No colour

44
Q

what colour does calcuim form

A

Brick Red

45
Q

what colour does Strontuim form

A

Red

46
Q

what colour does Baruim form

A

green

47
Q

characteristics of Fluorine

A
  • Yellow Gas
  • Toxic
  • Extremely Reactive
48
Q

Characteristics of Chlorine

A
  • Green Gas
  • Very Reactive
  • Toxic
49
Q

Characteristics of Bromine

A
  • Orange Liquid
  • Very Reactive
  • Toxic
50
Q

Characteristic of Iodine

A
  • Grey Crystal
  • Reactive
  • Toxic
  • Can easily turn into purple vapour upon heating
51
Q

what happens to MP/BP as you go down the group & why for G7

A
  • Increase as you go down the group
  • As you go down the group the number of electrons increase
  • Also the molecule gets larger as you go down the group
  • Due to these 2 factors there is a greater instantaneous dipole induced dipole force
  • Therefore it will have stronger London Forces
52
Q

what happens to electronegativity as you go down the group and why for G7

A
  • The electronegativity decreases
  • This is due to an increase in atomic radii which means that the outer electrons are further from nucleus
  • This means that the incoming electron will experience more shielding.
53
Q

what happens to reactivity as you go down the group and why for G7

A
  • The reactivity decreases as you go down the group
  • As you go down the group the atoms become larger so outer electron are further away and therefore more shielding for incoming electrons
54
Q

what is the solubility of G7 in water like

A
  • Since water is polar & G7 aren’t they aren’t able to dissolve fully
  • Fluorine reacts violently
  • The other halogens dissolve in water to some extent
55
Q

what do the solutions of halogens dissolved in water look like

A
  • Cl : pale green at top & clear aqueous layer at bottom
  • Br: Orange at top and clear aqueous layer at bottom
  • I : Brown at top & clear aqueous layer at bottom
56
Q

what is the solubility of halogens in cyclohexane like

A
  • They are both polar and so they dissolve due to london forces being attracted to each other
57
Q

what do the solutions of halogen being dissolved in cyclohexane look like

A
  1. CL: Pale green at top and clear aqueous layer at bottom
  2. Br: Orange at top & clear aqueous layer at bottom
  3. I: Purple at top & cleat aqueous layer at bottom
58
Q

what can displacement reaction of halogens indicate

A

Their reactivity

59
Q

when NaBr is added to the cyclohexane & chlorine solution what is the colour change

A

Pale green to orange

60
Q

when NaI is added to cylohexane solution containing chlorine what is the colour change

A

Pale green to purple

61
Q

when NaI is added to cyclohexane and Bromine solution what are the colour changes

A

Brown to purple

62
Q

what happens during the reaction between G1 + G7

A

the group 1 become oxidised as it goes from 0 to +1

63
Q

what happens during the reaction between G2 + G7

A

the group 2 becomes oxidised as it goes from 0 to +2

64
Q

what is a disproportionation reaction

A

reaction where the same species is oxidised & reduced

65
Q

when can this be seen specifically

A

reaction of Chlorine with:
1. water
2. Cold alkali
3. Hot alkali

66
Q

what is the equation of the reaction of Chlorine with water

A

Cl2(g) + H2O(l) ⇌ HCl(aq) + HClO (aq)

67
Q

what is the equation of chlorine with cold alkali (15 degrees)

A

Cl2(g) + 2NaOH(aq) → NaCl(aq) + NaClO (aq) + H2O(l)

68
Q

what is the equation of chlorine with hot alkali (70 degrees)

A

5Cl2(g) + 6NaOH(aq) → 5NaCl(aq) + NaClO (aq) + 3H2O(l)

69
Q

what happens to oxidising power of halogens as you go down group & why

A
  • Decrease
  • This is due to the larger radii as you go down the group which causes sheilding and further distance from nucleus means it can’t attract an incoming electron
  • They are known as oxidising agents
70
Q

what happens to reduction ability of halides as you go down the group and why

A
  • Increases
  • This is because it gets easier to donate an electron due to weak force of attraction between positive nucleus & negative electron
71
Q

what is the equation between sulphuric acid & chloride ions and what is the observation

A
  • NaCl + H2SO4 = NaHSO4 + HCl
  • The HCL can be seen as a misty white fume
72
Q

what are the 2 reactions of bromine with sulphuric acid, and why it happens as well as the observation made

A
  1. H2SO4 + NaBr = HBr + NaHSO4
  2. 2HBr + H2SO4 = SO2 + Br2 + 2H2O
  • The bromine in HBr is sufficiently strong reducing agent to reduce sulphuric acid into sulphur dioxide while being oxidised itself into Bromine gas
  • The bromine gas can be seen as a redish-brown gas
73
Q

what is the first reaction of iodide with sulphuric acid,

A
  1. H2SO4 + NaI = HI + NaHSO4
74
Q

what is the second reaction of iodide with sulphuric acid, why it happens and the observation

A
  1. 2HI + H2SO4 = I2 + SO2 + H2O
    - Formed due to the concentrated sulphuric acid oxidising the HI into Iodine and reducing itself to sulphur dioxide
    - The iodine can be seen as a purple vapour
75
Q

what is the third reaction of iodide with sulphuric acid, why it happens and the observation

A
  1. 6HI + H2SO4 = S + 3I2 + 4H2O
    - The concentrated sulphuric acid oxides the HI to iodine and is reduced to to sulphur
    - This can be seen as a yellow sold
76
Q

what is the fourth reaction of iodide with sulphuric acid, why it happens and what is the observation

A
  1. 8HI + H2SO4 = H2S + 4I2 + 4H2O
    - The concentrated sulphuric acid is reduced to hydrogen sulphide
77
Q

what is formed when hydrogen halides are ionised in water

A

form acidic solution

78
Q

what is the general equation for hydrogen halide with water

A

HX + H20 = H3O+ + X-

79
Q

what is the test for halide

A
  1. dissolve in nitric acid
  2. add silver nitrate to form precipitate
80
Q

what is the general equation for halide with silver nitrate

A

AgNO3 + NaX = AgX + NaNO3

81
Q

what colours precipitates to halides form

A

chlorine = white
bromine = cream
iodine = yellow

82
Q

what is another test for halides

A

AgCl: precipitate dissolves to give a colourless solution
AgBr: precipitate is almost unchanged using dilute ammonia solution, but dissolves in concentrated ammonia solution to give a colourless solution
AgI: precipitate is insoluble in ammonia solution of any concentration

83
Q

what is the general equation of the ammonia test with halides

A

AgX + 2NH3 = Ag(NH3)2 + X-

84
Q

what is ammonia test

A
  • Add NaOH and gently warm
  • Test the gas produced by holding near damp litmus paper
  • turns blue
  • smells like bleach
85
Q

test for sulphates

A
  • add HCL
  • Add baruim chloride
  • form white precipitate
86
Q

test for carbonate ions

A
  • Add HCL
  • Causes fizzing and forms CO2
  • gas is collected and bubbled through lime water
  • Turns cloudy / white precipitate
87
Q

test for nitrate ions

A

A
- Add HCL
- Causes fizzing and forms CO2
- gas is collected and bubbled through lime water
- Turns cloudy / white precipitate

Chemistry Year 1 (11 decks)

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