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Chem > Topic 4- Inorganic Chemistry and the periodic table > Flashcards

Topic 4- Inorganic Chemistry and the periodic table Flashcards

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1
Q

What is a common name
given to group 2 metals?

A

Alkaline Earth Metals

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2
Q

What is the most reactive Metal of group 2

A

Barium

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3
Q

3 Physical Properties of G2 metals

A

High melting and boiling points
● Low density metals
● Form colourless (white) compounds

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4
Q

The highest energy electrons
of group 2 metals are in which
subshell

A

S

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5
Q

Does reactivity increase or
decrease down group 2?
Why

A

Increases
● Electrons are lost more easily because larger
atomic radius and more shielding

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6
Q

What happens to the first
ionisation energy as you go
down group 2? Why?

A

Decreases because:
-Number of filled electron shells increases down the group →
increased shielding
- Increased atomic radius → weaker force between outer - -
-Electron and nucleus → less energy needed to remove
electron

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7
Q

What type of reaction is the
reaction between group 2
elements and oxygen?

A

Redox

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8
Q

What are the products when
group 2 elements react with
water?

A

Hydroxide and hydrogen gas

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9
Q

Exception of G2 metals with Water?

A

Magnesium and Steam -> MgO + H2

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10
Q

Which group 2 element
doesn’t react with water?

A

Beryllium

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11
Q

Which group 2 element reacts
very slowly with water?

A

Magnesium

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12
Q

What type of reaction is the
reaction between group 2
metal and water?

A

Redox

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13
Q

Write an equation for the
reaction of barium and
water

A

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

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14
Q

What is oxidised and what is
reduced in a reaction between
group 2 metal and water

A

Metal → oxidised
One hydrogen atom from each water →
reduced

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15
Q

What are the products when a
group 2 oxide reacts with an
dilute acid?

A

Salt + Water

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16
Q

What is formed when group 2
oxides react with water?

A

Metal hydroxide

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17
Q

Write an equation for the
reaction between a group 2
oxide and water

A

MO(s) + H2O -> M(OH)2 (aq)

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18
Q

What group 2 metal oxide is
insoluble in water

A

Beryllium oxide

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19
Q

Write an equation for the
reaction between Mg(OH) 2
and nitric acid

A

2HNO 3 (aq) + Mg(OH) 2 (aq) Mg(NO 3 ) 2
(aq) + 2H2O (l)

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20
Q

What is the trend in hydroxide
solubility down group 2?

A

Increases down the group
Mg(OH)₂ is slightly soluble
Ba(OH)₂ creates a strong alkaline solution

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21
Q

What is the trend in sulphate
solubility down group 2?

A

Group 2 sulphates become less soluble
down the group with BaSO4 being the
least soluble

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22
Q

Explain the reasons for the
trend of thermal stability in
group 2 carbonates

A

More Stable down the group
Cation Gets bigger so have less of a polarising effect distorting the carbonate ion less

C-O bond is not weakened as much it harder to break down

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23
Q

Explains the reasons for the trend of the thermal stability of G1 carbonates

A

Do not decompose except from Li
DOnt have big enough Charge densuty to polarise the carbonate ion as they only form 1+ ions
Lithium ion is small enough to have a polarising effect

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24
Q

Explain the reasons for the
trend of thermal stability in
group 2 nitrates

A

More stable down grou
Down the group ions get larger and therefore has less charge densitry = less polaristaion of nitrate anion and less weakening of the N-O bond

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25
Explain the reasons for the trend of thermal stability in group 1 nitrates
Do not decompose apart from Lithium nitrate Lithium ion is small enough to charge polarisation of the nitrate ion therefore weakening N-O bond
26
Lithium flame test
Scarlet Red
27
Sodium flame test
Yellow
28
Potassium flame test
lilac
29
Rubidium flame test
red
30
Caesium flame test
Blue
31
Magnesium flame test
No flame colour (ENergy emitted is outside visible spectrum)
32
Calcium flame test
brick red
33
Strontium flame test
red
34
Barium flame test
Apple green
35
How do you carry out flame test
Use a nichrome wire Sterilise wire by dipping in concentrated HCl then heating in flame Make sure sample grounded/grinded Dip wire in solid and put in flame
36
How are the colours from the flame test formed
Heat causes electron to get excited Moves to a higher energy level but at this higher level is unstable so then moves back down As it moves from a higher to lower energy level energy is emitted in the form of visible light energy (Colour seen)
37
2 properties of halogens
Low melting and boiling points Diatomic molecules
38
What is the trend in boiling point down group 7? Why
Increases down the group because: -size of atom increases as more occupied electron shells → stronger London forces of attraction between molecules, take more energy to break
39
What is the trend in reactivity down group 7? Why?
Reactivity decreases because: ● Atomic radius increases ● Electron shielding increases ● Ability to gain an electron and form 1- ions decreases
40
Explain the trend of electronegativity down group 7
Decreases Atomic Radii increases due to no. shells Reduced nuclear attraction between outermost electrion and nucleus
41
What is the trend in oxidising ability down the group? Why?
Decreases down group This is because top elements have the fewest occupied electron shells, greatest force of attraction between outer electrons and nucleus and thus is the easiest to gain electrons and be reduced → best oxidising agent React by gaining electrons tho so good oxidising agents.
42
What is the trend in reducing ability of the halides down the group? Why HALIDE - ION
Increases down the group This is because BOTTOM OF GROUP has the most occupied electron shell so outer electrons are further from the nucleus, weakest force of attraction between outer electrons and positive charge of nucleus and thus is the easiest to be oxidised and lose electrons → best reducing agent
43
When a more reactive halogen displaces a less reactive halide, what is the reaction called?
Displacement
44
What is the colour of chlorine in water?
Pale green
45
What is the colour of Bromine in water?
Orange
46
What is the colour of iodine in water?
Brown
47
What is the colour of chlorine in cyclohexane?
pale green/barely visible
48
What is the colour of bromine in cyclohexane?
Orange
49
What is the colour of iodine in cyclohexane?
Violet
50
Out of the 3 halides Cl - , Br - & I - , which one of these can be oxidised by chlorine
Br - & I - ions
51
Define disproportionation
The oxidation and reduction of the same element in a redox reaction
52
What is the equation for the reaction of Cl 2 with water
Cl₂ (g) + H₂O (l) → HClO (aq) + HCl (aq)
53
What type of reaction is the reaction of chlorine with water?
Disproportionation; chlorine is both oxidised and reduced
54
Why is chlorine added to drinking wate
It kills the bacteria in the water and makes it safer to drink
55
What are the two forms of the chlorate ion
ClO- is chlorate (I) ClO₃- is chlorate (V)
56
What is the equation for forming bleach and conditions
Cold dilute alkali Cl₂ (aq) + 2NaOH (aq) → NaCl (aq) + NaClO (aq) + H₂O (l) NaClO is bleach
57
What is bleach
NaClO
58
What do you use to test for halide ions?
Acidified AgNO3
59
Why do you add HNO 3 ? Why not HCl?
To remove CO₃2- Adding HCl would add Cl- ions, giving a false positive resul
60
Result and equation for Cl- test?
Ag + + Cl - → AgCl (s) White precipitate
61
What is the result and equation for the test for Br
Cream ppt Ag + + Br - → AgBr (s)
62
What is the result and equation for the test for I-
Yellow ppt Ag + + I - → AgI (s)
63
What happens (+ equations) to each of the silver halide precipitates when dilute/conc NH 3 are added
AgCl- dissolves in both dilute and conc AgCl (s) + 2NH₃ (aq) → [Ag(NH₃)₂] + (aq) + Cl - AgBr- only dissolves in conc AgBr (s) + 2NH₃ (aq) → [Ag(NH₃)₂] + (aq) + Br - AgI- will not dissolve in either
64
What products are formed when I - reduces H 2 SO 4
2HI SO2 + I2 + 2H2O S + 3I2 + 4H2O H2S + 4I2 + 4H2O
65
What is SO2
Choking gas with pungent odour
66
What is S
Yellow solid
67
What is H2S
Smells of rotten eggs
68
Does Cl- reduce H2SO4
No; not a powerful reducing agent; Only HCl is formed
69
What are the broducts of Br- + H2SO4?
HBr and SO2
70
How do you test for carbonate ions
Add strong acid to the sample Collect the gas produced Pass through lime water
71
What is the positive test result for Carbonate ion tests
Fizzing Limewater turns cloudy
72
Eqn for carbonate ion tests
CO 3 2- (aq) + 2H + (aq) → H 2 O (aq) + CO 2 (g
73
How can you test for sulfate ions, SO 4 2- ?
Dilute HCl Barium Sulphate
74
positive test result for sulphate test?
White precipitate of barium sulphate formed
75
Write an equation for the sulfate ion test
Ba 2+ (aq) + SO 42- (aq) → BaSO 4 (s)
76
When testing for carbonate, sulfate and halide ions, in which order should the tests be carried out and why?
1. Carbonate test 2. Sulfate test 3. Halide test Because barium ions forms insoluble precipitate of BaCO 3 and silver ions form insolube precipitate of Ag2 SO 4
77
How can you test for ammonium ions, NH 4 + ?
Add sodium hydroxide to the sample and warm it Test the gas produced with red litmus paper
78
What are the observations for positive ammonium ions test
● Red litmus paper turns blue ● Ammonia has a pungent smell
79
Write the equation for ammonium ions test
NH4 + (aq) + OH - (aq) → NH 3 (aq) + H 2 O (aq)
80
Explain trends in bond enthalpy of G7
F-F so small lone pairs repel eacth other Down the group atomic radii increases; distance of bonding pair to nuclei increases so attraction decreases
81

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