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A Chem Finale pt 2. > Unit 3.3 Chemistry of the p-block > Flashcards

Unit 3.3 Chemistry of the p-block Flashcards

1
Q

Define amphoteric behaviour

A

Can react with both acid and alkalis

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2
Q

What are 2 p-block elements to our concern?

A
  • Aluminium (Al)
  • Lead (Pb)
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3
Q

2 things about an Al+3 ion?
(Connectable)

A
  • Small and highly charged…
  • extensively hydrated solution (aqueous)
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4
Q

What is the aqueous form of Al+3?
(We may or may not stick with this)

A

[Al(H2O)6]+3

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5
Q

Eqn representation of sodium hydroxide to aqueous Al+3 ions?

A

Al3+ + 3OH- ⇌ Al(OH)3 (s) + 3H2O

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6
Q

“Product” (observation) formed for eqn representation of sodium hydroxide to aqueous Al+3 ions?

A

White + colourless ppt

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7
Q

If more OH- ions added to Al+3, what is created?

A

Aluminate ion

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8
Q

Eqn of creation of aluminate ion from adding more OH-

A

[Al(H2O)3(OH)3] + OH- ⇌ [Al(H2O)2(OH)4]-

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9
Q

How to reverse the reaction of the creation of aluminate ion?

A

Additions of acid

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10
Q

So which aluminium is the amphoteric?

A

Al(OH3) = Aluminium hydroxide

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11
Q

How to show the amphoteric behaviour of aluminium?
(2 ways)

A
  1. Al2O3 reacting w/ 3H2SO4
  2. Al2O3 reacting w/ 2NaOH + 3H2O
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12
Q

Amphoteric behaviour of aluminium w/ 3H2SO4 eqn?

A

Al2O3 + 3H2SO4 -> Al2(SO4)3 + 3H2O

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13
Q

Amphoteric behaviour of aluminium w/ 2NaOH + 3H2O eqn?

A

Al2O3 + 2NaOH + 3H2O -> 2NaAl(OH)4

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14
Q

2 things about Pb (lead)?

A
  • Pb2+ is derived
  • from PbNO3
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15
Q

Write eqn of Pb2+ w/ sodium hydroxide

A

Pb2+(aq) + 2OH-(aq) -> Pb(OH)2(s)

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16
Q

“Product” (observation) formed when lead(II) ion react w/ sodium hydroxide?

A

White ppt

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17
Q

But for excess sodium hydroxide, write the eqn of that for if it was Pb2+

A

Pb(OH)2 + 2OH-(aq) -> [Pb(OH)4]2-(aq)

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18
Q

Therefore, how do reverse reaction from plumbate ion?

A

Addition of acid (so similar wow)

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19
Q

The other iteration of Pb2+?

A

Pb(H2O)2

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20
Q

How to show amphoteric behaviour of lead (II)?

A
  1. PbO react w/ 2HCl
  2. PbO react w/ 2NaOH + H2O
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21
Q

Amphoteric behaviour of lead (II) w/ 2HCl eqn?

A

PbO + 2HCl -> PbCl2 + H2O

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22
Q

Amphoteric behaviour of lead (II) w/ 2NaOH + H2O eqn?

A

PbO + 2NaOH + H2O -> Na2[Pb(OH)4]

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23
Q

Define “Inert pair effect”?
(2-way)

A
  • Tendency of heavier elements
  • to form lower oxidation states
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24
Q

What causes the inert pair effect?
(2-way)

A
  • When s2 (2 inner electrons)
  • of e- not becoming involved
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25
Q

In which groups may u see the “inert pair effect”?

A

3 4 5

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26
Q

Show me inert pair effect in group 3
(Bold = favoured oxidation state)
(About 5 elements… use ur intuition to overcome this one)

A

B = 3
Al = 3
Ga = 1, 3
In = 1, 3
Ti = 1, 3

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27
Q

Show me inert pair effect in group 4
(Bold = favoured oxidation state)

A

C = 2, 4
Si = 4
Ge = 2, 4
Sn = 2, 4
Pb = 2, 4

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28
Q

Show me inert pair effect in group 5
(Bold = favoured oxidation state)

A

N = 3, 5
P = 3, 5
As = 3, 5
Sb = 3, 5
Bi = 3, 5

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29
Q

What does it mean for an atom to have a “full octet”?

A

Has all 8 electrons on outer shell

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30
Q

Tell me about “breaking the octet rule”?
(3-way)

A
  • Atoms w/ atomic no < 20
  • tend to combine so valence shells have
  • 8 electrons
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31
Q

What are the 3 exceptions to breaking the octet rule?
(() for 2 3)

A
  1. Molecules have odd no of e-
  2. Molecules have more than 8 e-
    (group 5 6 7)
  3. Molecules have less then 8 e-
    (> group 3)
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32
Q

What are also 2 things that u must know for breaking the octet rule from AS?

A
  • VSEPR
  • Shapes, degrees, BP LP , ye those shenanigans
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33
Q

In what scenario causes the coordinate bond?
(2 things)

A
  • Central atom has > 8 electrons
  • bonds with a “spare lone pair”
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34
Q

What is a dimer and its significance?

A
  • Structure containing 2 identical compounds
    (Al2Cl6)
  • Has coordinate bonds
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35
Q

Remember carbon? What other element is analogous towards that one?

A

Boron Nitride (BN)

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36
Q

3 types of Boron Nitrides?

A
  • “Graphite”
  • “Diamond”
  • “Graphene”
    … idk the terminologies they kinda just showed it?
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37
Q

Properties of “Graphite”?
(4 (“” thing) things)

A
  • Doesn’t conduct electricity (No delocalised electrons)
  • “Sheets stacked on top of each other”
  • ^ Slippery, layers slide over each other (weak vdw between)
  • High mp & bp (layers of strong covalent bonds)
  • Has sp3 hybridisation insteada sp2
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38
Q

Properties of “Diamond”?
(5 things)

A
  • Tetrahedral shapes (109.5°)
  • Hard (strong covalent bonds in all directions)
  • High mp & bp (strong covalent bonds)
  • No conduction electricity (no free e-)
  • Lattice like structures
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39
Q

Properties of “Graphene”?
(6 things)

A
  • Trigonal planar (120°)
  • Hexagonal layers (like “graphite”)
  • Flexible (folded into tube-like structure)
  • Strong covalent bond
  • Low density
  • No conduction electricity
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40
Q

When going down group 4 elements, tell me about their oxidation state preferences?
(3 things)

A
  • From carbon downwards, +4 is preferable
  • Reaching tin it prefers +2 & +4
  • Lead prefers +2 due to how delicate it feels
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41
Q

Explain carbon’s oxidation state preference?
Fe2O3 + 3CO -> 2Fe + 3CO2
(3-way)

A
  • C = +2 -> +4 as shown clearly
  • Hence oxidised (OIL)
  • CO = [H]
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42
Q

Explain lead’s oxidation state preference?
PbO2 + 4HCl -> PbCl2 + Cl2 + 2H2O

A
  • Pb = +4 -> +2 as shown clearly
  • Hence reduced (RIG)
  • PbO2 = [O]
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43
Q

How come lead (Pb) is the unique one in oxidation?
(5 way)

A
  • Pb real group is 28
  • Periodic table isn’t including lanthanide elements
  • Pb smaller than expected
  • ∴ S2 e-s are inert (6s2 not involved)
  • INERT PAIR EFFECT
44
Q

CO2 “common” origins?

A

Gas sublimes from solid form (-78°C)

45
Q

Nature of CO2?
(2 things)

A
  • Acidic base
  • Dissolves in H2O to form acid
46
Q

Eqn of CO2 in water?
+ an additional significance?

A

CO2 + H2O ⇌ H+ + HCO3- (aq)
- CO2 can neutralise a base

47
Q

How to determine the base with CO2 rxns with such?

A

It’s never CO2 and H2O

48
Q

CO2 reacting with NaOH solution eqn?
- Guess the base

A

CO2 + 2NaOH -> Na2CO3 + H2O

49
Q

CO2 reacting with NaOH solution eqn?
(In excess)
- Guess the base too

A

CO2 + NaOH -> NaHCO3

50
Q

CO2 reacting with limewater eqn?

A

Ca(OH)2 + CO2 -> CaCO3 + H2O

51
Q

Observation of CO2 reacting with limewater?

52
Q

Excess CO2 reacting with limewater eqn?
(“2-part”)
- Name the category of the product

A

CaCO3 + CO2 + H2O -> Ca(HCO3)2 (aq)

Salt.

53
Q

Explain excess CO2 rxn w/ limewater?
(2-way)

A
  • Re-dissolves ppt to form solution
  • containing calcium & hydrogencarbonate ions
54
Q

Why can’t we extract Ca(HCO3)2 through evaporation?
(2-way-1 thing)

A
  • Only gain CaCO3
  • due to temporary hardness of H2O
  • Ca(HCO3)2 thermally decomposes
55
Q

With CO2 in mind, what about Lead(II) oxide (PbO)?

A

It’s amphoteric.

56
Q

Amphoteric nature of PbO eqn (w/ acid)?
- Point out the acid and the base

A

PbO + 2HNO3 -> Pb(NO3)2 + H2O
Acid = 2nd, Base = 4th

57
Q

Amphoteric nature of PbO eqn (w/ base)?
- Point out the acid and the base

A

PbO + 2NaOH + H2O -> [Na2Pb(OH)4]
Base = 2nd, Acid = 4th

58
Q

Define hybridisation?
(2-way)

A
  • Process of combining atomic orbitals
  • to create new hybrid orbitals
59
Q

Which of the group 4 elements use sp3 hybridisation?

A

Carbon (C) and silicon (Si)

60
Q

Show hybridisation of the 2 particular elements using sp3 hybridisation?

A

2s2 2p2 -> 2s1 2p4
(Ye not best visualisation)
(Draw it urself, from 2s^2 to 2s^1, separation)

61
Q

Significance of C & Si using sp3 hybridisation?
(2 things)

A
  • Can maximise distance apart
  • Can form sigma bonds with 4 cl atoms
62
Q

Try draw 4 sp3 hybridised orbitals
+ sigma-covalent bond version
(Of important however, state the shape + degrees)

A

Mleh
- Tetrahedral, 109.5°

63
Q

Why can’t CCl4 react with water?
(2 things)

A
  • No d-orbitals
  • forms 2 immiscible layers
64
Q

But what about SiCl4 rxn w/ water?
(3 things)

A
  • Violent in a hydrolysis reaction
  • Produces colourless solid
  • & misty fumes
65
Q

Eqn of SiCl4 rxn w/ water?
State colourless and misty ones.

A

SiCl4(l) + 2H2O(l) -> SiO2(s) + 4HCl(g)
Colourless solid = 3rd, Misty fumes = 4th

66
Q

However, difference for silicon?
Hence, rewritten rxn of SiCl4 w/ water?

A
  • Can have 3d subshells/orbitals
    SiCl4 + 4H2O -> Si(OH)4 + 4HCl
67
Q

Why can’t carbon be like silicon?
(“2-way”)

A
  • Carbon no access to 2d & 3d subshell
  • Too high in energy
68
Q

Ond, what about PbCl2 rxn w/ water?
(3 things)

A
  • Largely ionic character = fairly insoluble in cold water
  • Dissolves in hot water
69
Q

Tho eqn of creation of PbCl2?
State “category name” of product and a meticulous awareness?

A

Pb2+(aq) + Cl-(aq) -> PbCl2(s)
- Solid ppt, dropwise Cl-

70
Q

However, creation of PbCl2 in excess Cl- eqn?
State product name

A

PbCl2(s) + Cl-(aq) -> [Pb(Cl)4]2-(aq)
- Tetrachlorolead(II)

71
Q

Pb2+ + OH- dropwise observation?

72
Q

Pb2+ + excess OH- observation?

A

Ppt dissolves (colourless)

73
Q

Pb2+ + Cl- dropwise observation?

74
Q

Pb2+ + excess Cl- observation?

A

Ppt dissolves (colourless)

75
Q

Pb2+ + I- dropwise observation?

A

bright Yellow ppt

76
Q

Pb2+ + OH- dropwise compound formed?

A

Pb(OH)2(s)

77
Q

Pb2+ + excess OH- compound formed?

A

[Pb(OH)4]2-(aq)

78
Q

Pb2+ + Cl- dropwise compound formed?

79
Q

Pb2+ + excess Cl- compound formed?

A

[PbCl4]2-(aq)

80
Q

Pb2+ + I- dropwise compound formed?

81
Q

What are disproportionation reactions?

A

Goes under oxidation & reduction

82
Q

How can chlorine have disproportionation reactions w/ what?

A
  • Based on the conditions
  • With NaOH
83
Q

The equation for Cl with cold, dilute sodium hydroxide?

A

2NaOH + Cl2 -> NaCl + NaClO + H2

84
Q

Name of 2nd product from eqn of Cl w/ cold, dilute sodium hydroxide?

A

Sodium Chlorate (I)

85
Q

The equation for Cl with warm, concentrated sodium hydroxide?

A

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

86
Q

Name of 2nd product from eqn of Cl w/ warm, concentration sodium hydroxide?

A

Sodium chlorate (V)

87
Q

But what’s so special about Cl2?
(3 things)

A
  • Strong oxidising power
  • Even the chlorate ion (ClO-)
  • Used in bleaching
88
Q

Why is Cl2/ClO- used in bleaching?

A

Has an antibacterial effect

89
Q

Eqn of ClO- being reduced?

A

ClO- + 2H+ + 2e- -> Cl-(aq) + H2O

90
Q

When u add any sodium halide to a conc. H2SO4, what u get?

A

Hydrogen halide formed as a steamy gas

91
Q

NaCl rxn w/ conc. H2SO4 eqn?

A

NaCl + H2SO4 -> HCl(g) + NaHSO4

92
Q

NaCl rxn w/ conc. H2SO4 eqn….
State observation and from which product?

A
  • HCl
  • Steamy fumes (colourless)
93
Q

NaBr rxn w/ conc. H2SO4 eqn?

A

NaBr + H2SO4 -> HBr(g) + NaHSO4

94
Q

NaBr rxn w/ conc. H2SO4 eqn…
State observation and from which product?

A
  • HBr
  • Misty fumes
95
Q

Further reaction of NaBr rxn w/ conc. H2SO4 eqn?

A

2HBr + H2SO4 -> Br2(g) + SO2(g) + 2H2O

96
Q

Further reaction of NaBr rxn w/ conc. H2SO4 eqn…
State observation(s) and from which product(s)?
(3.)

A
  • Br2 + 2H2O = orange solxns
  • Br2 = brown fumes
  • SO2 = colourless fumes
97
Q

NaI rxn w/ conc. H2SO4 eqn?

A

NaI + H2SO4 -> HI + NaHSO4

98
Q

NaI rxn w/ conc. H2SO4 eqn…
State observation and from which product?

A
  • Misty fumes
  • HI
99
Q

Further reaction of NaI rxn w/ conc. H2SO4 eqn?

A

8HI + H2SO4 -> 4I2 + H2S + H2O

100
Q

Further reaction of NaI rxn w/ conc. H2SO4 eqn…
State observation(s) and from which product(s)?
(3.)

A
  • 4I2 = purple fumes
  • H2S = rotten egg smell
  • Yellow solid
101
Q

Put the 3 hydrogen halides in order of reducing ability?

A

I- > Br- > Cl-

102
Q

Explain HCl reducing ability?

A

Difficult to oxidise

103
Q

Explain HBr reducing ability?

A

Slightly easier to oxidise than HCl

104
Q

Explain HI reducing ability?

A

Least ε° value, hence best reducing agent

105
Q

Wordy but, we continue to experiment and I believe foundation is much imp together w/ understanding

A Chem Finale pt 2. (10 decks)

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