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A Level Chemistry > Inorganic Chemistry > Flashcards

Inorganic Chemistry Flashcards

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1
Q

Down group 2 IE does what and explain why relating to how reactions occur in metals

A

Shielding increases
Nuclear charge increases but is outweighed
Nuclear attraction decreases
Atomic radi increases
Reactivity increases as they react by losing electrons.

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2
Q

Group 2 metal + 1/2O2(g)->

Also give state symbol

A

MO(s)

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3
Q

Group 2 M (s) + Cl2 (g) ->

Add state symbol

A

MCl2 (s)

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4
Q

Group 2 metal + 2H2O (l) ->

Add state symbols

A

M(OH)2 (aq) + H2 (g)

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5
Q

Reactions of group 2 metal with oxides:
MO (s) + H20 (l) ->
MO (s) + 2HCl (aq) ->

Add state symbols

A

M(OH)W (aq)

MCl2 (aq) + H20 (l)

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6
Q

Group 2 metal with hydroxide/ base:
M(OH)2 (s) + 2HCl (aq) ->

Add state symbols

A

MCl2 (aq) + 2H2O (l)

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7
Q

Solubility trends group 2 metals acronym, explain, examples

A

HIS DOG
hydroxides increase, sulfatos decrease, down group

Ba(OH)2 is soluble
BaSO4 is insoluble

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8
Q

Explain the Thermal decomposition trend down group two

A

Gets harder to decompose down the group hence more thermal energy is needed, the cation gets larger hence is less polarising hence less weakening in the bonds of an anion.

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9
Q

Li and group 2 nitrates thermal decomposition reactions examples :
2LiNO3 (s) -> (heat on top of arrow)
Ca(NO3)2 (s) -> (heat on top of arrow)

Add state symbols

A

Li2O (s) + 2NO2 (g) + 1/2 O2 (g)
CaO + 2NO2 (g) + 1/2O2(g)

NO2 (g) = brown fumes

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10
Q

Feast of group one nitrate thermal decomposition reactions:
MNO3 (s) -> (heat on top of arrow)

Add state symbols

A

MNO2 s) + 1/2O2 (g)

Metal NO2 is not brown fumes

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11
Q

Li and group 2 carbonates thermal decomposition reactions:
Li2CO3 (s) -> (heat on top of arrow)
CaCO3 (s) -> (heat on top of arrow)

Add state symbols
How do we test for CO2?

A

Li2O (s) + CO2 (g)
CaO (s) + CO2 (g)

Limewater turns milky

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12
Q

Reactions of group one carbonates thermal decomposition reactions? And explain why?

A

Do not undergo because the cations are too lowly charges/ have too large a radius to polarise the anion as much as lithium or calcium ions

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13
Q

Flame test procedure

A

Clean a nichrome/ platinum wire loop by dipping in HCl
Put in fire to sterilise
Dip in sample
Put in flame and observe colour change

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14
Q 
Flame test colours of:
Li + 
Ma+
K+
Rb+
Cs+
A 
Red 
Yellow 
Lilac 
Red/purple
Blue/violet
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15
Q 
Flame test colours of:
Be2+ 
Msg 2+ 
Ca2+
Sr2+
Ba2+
A 
No colour 
No colour 
Brick red 
Crimson red 
Apple green
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16
Q

Explanation for why colours are seen when reacting group one and two metals in flame tests. Also relate to Be2+ and Mg2+.

A

The electrons absorb energy and exalted from their ground state level to a higher energy state and when they fall back down again, energy of a specific frequency is releases which is observed as a colour.

Be2+ and Mg2+ release a wave of frequency not in visible light spectrum.

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17
Q

Trend in melting point down group seven halogens?

A

Decreases down the group

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18
Q

Cl2 Br2 I2 - state trend and link to number of electrons

A

Gas liquid solid

More electrons more strong because London forces so higher melting and boiling point

19
Q

Reasons why electronegativity decreases

A

More shielding
Outweighs increased charge
Decreased attraction on outermost electrons
Larger atomic radius

20
Q

Trend in reactivity down group seven and reasons

A

Decreases
More shielding which outweighs increased nuclear charge so decreased attraction on bonding electrons hence larger atomic radi so harder to gain electrons

21
Q

How can we show reactivity decreases down group seven?

A

Displacement reactions ass NaBr for example for a solution

22
Q

Cl2 Br2 I2 colour as an element

A

Green gas
Red liquid
Grey solid

23
Q

Cl2 Br2 I2 colour in an aqueous solution

A

Pale green
Orange
Brown

24
Q

Cl2 Br2 I2 colour in a cyclohexane (organic)

A

Pale green
Orange
Purple

25
Q

Group one and two metals reaction with group seven halogens is

A

Redox

Metal is oxidised and halogen is reduced

26
Q

What is disproportionation

A

When an element in a single species is both oxidised and reduces in a reaction

27
Q

Water treatment example of disproportionation with group seven halogen chemical equation
And state what products are reduced and oxidised

A

Cl2 + H2O -> HCl + HOCL

HCl is reduced HOCL is oxidised

28
Q

Bleach formation disproportionation reaction (halogen) chemical equation and state which product is oxidised and reduced

A

Cl2 + 2NaOH (cold, dilute) -> NaOCl + NaCl + H29

NaOCl is oxidised and NaCl is reduced

29
Q

Disproportionation reaction example with hot alkali chemical equation and state which of the products is reduced and oxidised

A

3Cl2 + 6NaOH -> NaClO3 + 5NaCl + 3H2O

NaClO3 is oxidised and 5NaCl is reduced

30
Q

Reducing ability of halides trend and explanation

A

Increases down group seven as electrons are not held on as strongly as because of a larger radius and lower nuclear attraction

31
Q

How can we see the reducing ability of halides increases?

A

When a halide like NaBr (aq) is reacted with H2SP4

32
Q

Observations, and products formed when NaCl is reacted with H2SO4?

A

Misty fumes (HCl) and NaHSO4 are seen

33
Q

Observations and products formed when NaBr (aq) is reacted with H2SO4?

A

Misty fumes (HBr)
Brown fumes (Br2)
Colourless gas/choking smell (SO2)
NaHSO4

34
Q

Observations and products formed when NaI (aq) is reacted with H2SO4?

A 
Misty fumes (HI)
Purple fumes or black solid (I2)
Colourless gas or choking smell (SO2) 
Yellow solid (S)
Rotten egg smell from colourless gas (H2S)
NaHSO4
35
Q

Precipitation test for halides process and results for Cl,Br,I

A

Dissolve in add silver nitrite solution to halide ion to form for example AgCl (white) AgBr (cream) and AgI (yellow)
AgCl will dissolve in dilute NH3
AgBr will dissolve in concentrated NH3

36
Q

Hydrogen halide reaction with ammonia with state symbols for example

NH3 (g) + HCl (g) ->

Also comment on products

A

NH4Cl (s)

Smoke

37
Q

Hydrogen halide reaction with water with state symbols:
HCl (g) + H2O (l) ->

Also comment on product

A

H3O+ (aq) + Cl- (aq)

H3O+ is an acidic sol

38
Q

Inorganic analysis order to prevent false positives

A 
Test for chlorides ions
Test for sulfato ions
Using silver nitrite solution test for halide ions and then dissolve in dilute and concentrated ammonia 
Use cyclohexane 
Flame tests on group one and two
39
Q

HCL dissolves in water. Why is the solution formed acidic?

A

Dissociates into H+ ions, hence solution is acidic

40
Q

How to test for chlorine (NOT IONS)

A

Litmus paper bleaches

41
Q

Carbonate ion test

A

Add HCL and bubble gas through limewater if turns cloudy CO2 produced and carbonate present

42
Q

Sulfate ion testa

A

Add a few drops of HCL to remove carbonate ions
Add barium chloride
If sulfate present white pot of barium sulfate visible

43
Q

NH4+ ammonium ion test

A

Warm with NaOH to form ammonia

Ammonia gas will turn damp red litmus paper blue

A Level Chemistry (8 decks)

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