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A-LEVEL CHEMISTRY > B2 Redox + Periodicity > Flashcards

B2 Redox + Periodicity Flashcards

1
Q

Oxidation number of element

A

0

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2
Q

Oxidation number of group 1

A

1+

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3
Q

Oxidation number of group 2

A

2+

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4
Q

Oxidation number of flourine

A

1-

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5
Q

Oxidation number of oxygen in H2O2

A

1-

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6
Q

Oxidation number of hydrogen in H2O2

A

1+

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7
Q

What substance gets the negative oxidation number in a compound

A

The most electronegative

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8
Q

Sum of oxidation numbers in a compound

A

0

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9
Q

Sum of oxidation numbers in an ion

A

Charge of ion

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10
Q

What happens to oxidation number when a substance is reduced

A

Decreases

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11
Q

What happens to oxidation number when a substance is oxidised

A

Increases

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12
Q

When writing systamatic names, when does the Roman numeral oxidation number come

A
  • In brackets after the element
  • e.g Titanium (IV) Oxide
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13
Q

In metal and acid reactions, what is reduced and what is oxidised

A
  • Metal oxidised
  • Hydrogen reduced
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14
Q

Meaning of oxidation

A
  • Loss of electrons
  • Increase in oxidation number
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15
Q

Meaning of reduction

A
  • Gain of electrons
  • Decrease in oxidation number
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16
Q

Define Disproportionation

A

Reduction and oxidation of the same element in the same reaction

17
Q

Define Oxidising Agent

A

Takes electrons from the species being oxidised

18
Q

Define Reducing Agent

A

Adds electrons to the species being reduced

19
Q

How to write elemental half-equations

A
  • Calculate overall charge on each side
  • Add electrons to more positive side
  • Ensure fully balanced
20
Q

How is the periodic table arranged

A

Increasing atomic number

21
Q

How to write half-equations for acidic conditions

A
  • Balance the element changing oxidation state
  • For every oxygen, add an H2O to the other side
  • For every hydrogen, add an H+ to the other side
  • Use electrons to ensure both sides have the same charge
22
Q

What do elements in periods in the periodic table have

A

Repeating trends in physical and chemical properties

23
Q

What do elements in groups of the periodic table have

A

Similar chemical properties

24
Q

Define Periodicity

A

The repeating trends in physical and chemical properties across a period

25
Q

How to explain why an element is in the s/d/p block

A

It’s highest energy electron is in the s/d/p subshell

26
Q

Define First Ionisation Energy

A

The energy required to remove 1mol of electrons from 1mol of gaseous atoms

27
Q

How to explain differences in ionisation energies

A
  • Electron shells
  • Atomic radius
  • Sheilding
  • Nuclear charge
  • Sheilding + atomic radius outweigh nuclear charge
  • Nuclear attraction
28
Q

What must always be stated when describing changes in ionisation energies

A

Sheilding - even if has no effect

29
Q

When given an ionisation energy graph for an element, how can you tell what group that element is in

A
  • Greatest jump in ionisation energies
  • Jump 4 - 5
  • In group 4
30
Q

General equation for first ionisation energy

A
31
Q

General equation for second ionisation energy

A
32
Q

Draw a graph for ionisation energies across period 2

A
33
Q

What element has highest first ionisation energy

A

Helium

34
Q

On first ionisation energy graphs, there is a general increase - what are the exceptions

A
  • New shell - decrease
  • p subshell - decrease
  • group 6 - decrease (new electron in singular paired orbital so more repulsion)

A-LEVEL CHEMISTRY (6 decks)

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