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A LEVEL CHEM > Topic 4-Inorganic Chemistry And The Periodic Table > Flashcards

Topic 4-Inorganic Chemistry And The Periodic Table Flashcards

1
Q

What is the test for ammonium compounds?

A

Gas turns damp red litmus paper blue.

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2
Q

Name the 2 problems with the flame test

A

Sodium compounds (as impurities) can mask other colours

Subjective —> people have different levels of vision so a word description maybe mean different colours to different people.

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3
Q

What causes the colours in the flame tests?

A

Electrons can absorb energy and move to higher energy levels.

Instantly returns to ground state which releases energy and sometimes this energy is within the radiation of the visible light spectrum which makes a colour appear.

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4
Q

Define electronegativity.

A

The ability of an atom to draw a pair of bonding electrons from a covalent bond.

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5
Q

Describe the trends of reactions of group 7 with chlorine.

A

More vigorous down the group.

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6
Q

Describe the trend in reactions of group 7 with oxygen

A

More vigorous down the group

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7
Q

How do group 2 elements generally react with water?

What is an exception?

A

M + H2O —> M(OH)2 + H2
metal + water –>metal hydroxide + hydrogen

Magnesium and steam (reacts slowly) is an exception as it forms Magnesium Oxide and hydrogen

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8
Q

What group 2 oxide doesn’t react with water?

A

Beryllium

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9
Q

What could Mg(OH)2 be used for and why?

A

Indigestion tablets as Magnesium Hydroxide is very insoluble so won’t react/dissolve into the body.

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10
Q

What is BaSO4 used for and why?

A

Barium meal for patients about to have an x-ray as it absorbs the x-rays so can be traced but is insoluble so the toxicity won’t affect the body.

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11
Q

What is the interaction between the nucleus and outer electrons called?

A

Electrostatic attraction

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12
Q

How does group 2 react with oxygen?

A

Group 2 metals will BURN in oxygen to form solid white oxides.

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13
Q

How does group 2 react with chlorine?

A

Group 2 metals form white chlorides when reacting with chlorine.

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14
Q

The oxides form more strongly alkaline solutions a you go ….. the group?

A

Down the group

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15
Q

Oxides and hydroxides are examples of what?

A

Bases.

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16
Q

What makes metal hydroxides in solutions strongly alkaline?

A

The hydroxide ions (OH-).

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17
Q

What will bases do to dilute acids?

A

Neutralise them.

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18
Q

Name the flame colour of Li, Na,K,Rb,Cs (Group1 )

A 
Li=red
Na=yellow
K=lilac
Rb=red
Cs=blue
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19
Q

Name the flame colour of Ca,Sr,and Ba (Group 2)

What are the colours of the other Group 2 elements?

A 
Ca=brick red
Sr=crimson
Ba=Green
No colour (radiation beyond the visible light spectrum)
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20
Q

Name the risks of adding Chlorine to water?

A

Chlorine gas is toxic

Liquid chlorine burns the eyes and skin

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21
Q

What does adding to water and Chlorine do? (in absence of sunlight)

A

Cl2 + H2O –> HCl + HClO

which ionises to make CLO- which kills bacteria to clean water!

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22
Q

Name some benefits of water treatment

A

Kills harmful bacteria

prevents deaths

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23
Q

What do Group 1 carbonates decompose to?

A

They don’t decompose (thermally stable)

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24
Q

What do Group 2 carbonates decompose to?

A

Oxides and carbon dioxide.

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25
Q

What do Group 2 Nitrates decompose to?

A

Oxygen, oxide, nitrogen dioxide

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26
Q

What do group 1 Nitrates decompose to?

A

Nitrite, oxygen.

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27
Q

Halogens undergo what kind of reaction with COLD ALKALIS?

A

Disproportionation

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28
Q

Halogens + hot alklais undergo a ……… reaction

A

disproportionation

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29
Q

Define the general trend of reactivity of Group 7

A

Less reactive down the group

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30
Q

What trend do melting and boiling points have down Group 7?

A

Increase down the group

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31
Q

Which species is displaced: halogens/halides

A

Halogens displace less reactive halides e.g. Cl2 displaces Br- and I-

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32
Q

What colours are Cl2, Br2 and I2 in water?

A 
Cl2= colourless
Br2= yellow
I2= brown
33
Q

What colours are Cl2, Br2 and I2 in hexane?

A

Cl2= colourless
Br2=orange
I2= pink

34
Q

What colours are Fluorine, Chlorine, Bromine and Iodine at room temperature?

A 
Fluorine = pale yellow
Chlorine= green
Bromine= red-brown
Iodine= grey
35
Q

What two substances form bleach?

A

Chlorine + Sodium hydroxide

36
Q

How can you test the thermal stability of Nitrates?

A

How long it takes for an amount of NO2 (brown gas) to be produced- toxic
OR
How long it takes for a certain amount of oxygen to be produced? (i.e enough to relight a glowing splint)

37
Q

How can you test the thermal stability of carbonates?

A

How long it takes for lime water to turn cloudy.

38
Q

What is the trend in thermal stability down Group 2?

A

Increases down group 2 (large cations cause less distortion)

39
Q

If something is thermally stable, what does this mean in regard to decomposition?

A

More energy will be needed to decompose something thermally stable.

40
Q

What do Group 1 and 2 carbonates decompose to?

A

Group 1 don’t decompose as they’re thermally stable.

Group 2 decompose into Oxides and carbon dioxide.

41
Q

What do group 1 and 2 Nitrates decompose to?

A

Group 1 = Nitrite and oxygen

Group 2 = Nitrogen dioxide, oxygen, and oxide.

42
Q

What ion kills bacteria?

A

Chlorate (I) ions.

43
Q

The reducing power of halides …… down the group

A

The reducing power of halides increases down the group.

44
Q

Describe the trends in melting points in group two?

A

Melting point Decreases down the table.

45
Q

The hydrogen halides react with ammonia to give…

A

White fumes

46
Q

What group 2 oxide reacts with water VERY slowly?

A

Magnesium

47
Q

Oxides are more strongly alkaline … the group?

A

Oxides are more strongly alkaline down the group

48
Q

Which key trends of Group 2 INCREASE DOWN the group?

A 
Reactivity with water
Reactivity
Solubility with Hydroxides
How strongly alkaline 
Thermal stability
49
Q

Which key trends of Group 2 decrease down the group/increase up?

A

Solubility with sulfates

Melting points

50
Q

Describe why the trend in Group 2 melting points happens?

A

Group 2 elements decrease in melting point due to the ion cores having LARGER radii therefore electrons experience less attraction to the nuclei making bonding weaker.

51
Q

Why does reactivity of water ….. down the group?

A

Reactivity of water increases down the group because they have low ionisation energies so will easily lose their outer electrons.

52
Q

Ground 2 compounds are …… thermally stable than Group 1 compounds, WHY?

A

Group 2 compounds are less thermally stable than Group 1 compounds because the greater the charge on the cation, the greater the distortion and the less stable the carbonate/nitrate is.

53
Q

The reducing power of halides ……. down the group

A

The reducing power of halides increases down the group.

54
Q

How do the different halide ions react with silver nitrate

A 
F- = no precipitate
Cl- = white precipitate
Br- = cream precipitate
I- = yellow precipitate
55
Q

When reacting halide ions with silver nitrate, what do you add before and why?

A

Add dilute nitric acid to remove ions which may interfere with the reaction.

56
Q

How will Fluorides and Chlorides react with sulfuric acid?

A

(could be any gr1 metal)
KF+ H2SO4 –> HF + KHSO4
Chloride is the same

57
Q

How will Bromides react with sulfuric acid?

A

KBr + H2SO4 –> HBR + KHSO4

2HBr + H2SO4 –> Br2 + SO2 + 2H2O

58
Q

How will Iodides react with sulfuric acid?

A

KI + H2SO4 –> HI + KHSO4
2HI + H2SO4 –> I2 + SO2 + 2H2O
6HI + SO2 –> 3I2 + H2S + 2H2O

59
Q

What will the observation of AgCl, AgBr and AgI be with ammonia?

A 
AgCl = Dissolve, and form a colourless solution
AgBr = Won't dissolve unless ammonia is very concentrated
AgI = Won't dissolve even if ammonia is very concentrated.
60
Q

Why do we further test the halide with silver nitrate solution with ammonia?

A

As the colours with just silver nitrate can look quite similar. Ammonia helps us be sure which halide we have.

61
Q

Give two reasons why a bromide ion is a more powerful reducing agent than a chloride ion?

A

Because the attraction between the nucleus is weaker (due to shielding and the size of the ion increasing)

62
Q

What would you see if you mixed hydrogen iodide with ammonia?

A

White fumes

63
Q

If Bromide is displaced and bromine is formed what colour will the mixture turn?

A

Orange

64
Q

If iodide is displaced and iodine is formed what colour will the mixture turn?

A

Brown

65
Q

How can you test for sulfates?

A

Adding Hcl and Barium chloride solution, makes a white precipitate if barium sulfate forms.

The Hcl removes traces of carbonates which would also form a white precip

66
Q

How can you detect carbonates?

A

Hydrochloric acid makes carbonates fizz as they give off CO2

67
Q

How do you properly test for ammonium ions?

A

Add sodium hydroxide to substance and gently heat it. if this the turns damp red litmus paper blue ammonia is present.

68
Q

Why does litmus paper need to be damp?

A

So the gas can dissolve and make the colour change.

69
Q

What produces orange-brown fumes?

A

NO2 or Br

70
Q

What forms steamy fumes in moist air?

A

Hydrogen halides can dissolve in water and moisture in air to produce musty fumes of acidic gas.

71
Q

HCl + NH3 would produce what observation?

A

White smoke

72
Q

What anion after heating gives a brown gas?

A

NO3-

73
Q

How can you describe the “reducing power” of something?

A

The ability for a substance to REDUCE something else (give an electron to something else)

74
Q

Going down Group 7 from chlorine to iodine the …….. power of the halide ion increases

A

the reducing power of the halide ion increases.

75
Q

When iodide ions are added to a solution of chlorine a …… colour appears/disappears?

A

brown APPEARS

76
Q

Halide ions act as …….. agents by ……. an electron. Therefore the best halide ion for this is

A

Halide ions act as REDUCING AGENTS by LOSING an electron

Iodide as attraction=weaker down group so electron lost more easily

77
Q

Give an equation for hot alkalis reacting with a halogen

A

3Cl2 + 6NaOH –> NaClO3 + 5NaCl + 3H2O

78
Q

Give an equation for cold alkalis reacting with a halogen.

A

Br2 + 2NaOH —> NaOBr + NaBr + H2O

79
Q

Show Chlorine and Sodium Hydroxide reacting to form bleach.

A

Cl2 + 2NaOH –> NaClO + NaCl + H2O

Cold dilute NaOH

A LEVEL CHEM (34 decks)

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