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a level chemistry ocr a > Periodicity > Flashcards

Periodicity Flashcards

Ionisation energy

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1
Q

Periodicity

A

Repeating pattern of properties shown across different periods within their position in the periodic table

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2
Q

Group 1

A

Alkalis, less dense than water, fizzing, floats, dissolve

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3
Q

Why do atoms of elements in a group have similar properties

A

Same number of outer shell electrons, same electron configuration

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4
Q

Group 1 reactivity

A

Reactivity increases as you go down the group due to more shells,

easier to lose electrons,

weaker attraction to nucleus, less atomic radius

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5
Q

Ionisation energy

A

Energy required to remove one electron from each atom in a mole of gaseous atoms

Endothermic

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6
Q

1,2,3 Ionisation energy for sodium

A

Na (g) > Na+ (g) + e-

Na+ (g) > Na2+ (g) + e-

Na2+ (g) > Na+ (g) + e-

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7
Q

Oxygen ionisation energy

A

O (g) > O+ (g) + e-

Atoms are singular so not O2

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8
Q

Successive ionisation energy

A

Measure of energy required to remove each electron in turn

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9
Q

Using graph

A

Electrons in outer shell = lowest group of crosses

Period number = number of groups

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10
Q

Recognising group number with no graph

A

Big jump between ionisation energies

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11
Q

Factors that affect ionisation energy

A

Atomic radius
Electron shielding
Nuclear charge

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12
Q

Atomic radius

A

Distance from nucleus to outer electron shell

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13
Q

Electron shielding

A

Amount of shells

Shells lessen electron repulsion

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14
Q

Nuclear charge

A

Charge of nucleus (protons in nucleus)

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15
Q

Atomic radius across period

A

Decreases

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16
Q

Atomic radius down a group

A

Increases

17
Q

Why does first ionisation energy decrease down a group

A

Number of shells increases

Shielding increases

Atomic radius increases

18
Q

Why does first ionisation energy increase across a group

A

Number of protons increases

Increased nuclear attraction

Atomic radius decreases

Similar shielding

19
Q

Nuclear attraction

A

Atomic radius

Nuclear charge

Electron shielding

20
Q

Boron dip

A

Bosons outer electron is in a 2p orbital rather than a 2s

2p electron is slightly more distant from the nucleus than the 2s

Also, it is partially shielded by the 2s electrons as well as the inner electrons

Both of these factors offset the effect of the extra proton

21
Q

Oxygen dip

A

Despite the extra proton in the oxygen nucleus

Shielding is identical in nitrogen and oxygen and the electron is being removed from an identical orbital

Difference is that in oxygen, the electron being removed is one of the 3px2 pair

Repulsion between the 2 electrons in the same orbital means that the electron is easier to remove than it would otherwise be

22
Q

Graphite

A

3BP 1LP

Layers slide easily due to weak forces between layers

Lots of strong covalent bonds so high MP

Delocalised electrons between layers allow graphite to conduct electricity

Layers far apart so low density

Insoluble as covalent bonds too strong strong to break

23
Q

Diamond

A

Tetrahedral

Conduct well due to tightly packed rigid arrangement

V high MP due to many strong covalent bonds, v hard

Doesn’t conduct electricity due to no delocalised electrons

Insoluble as covalent bonds too strong

24
Q

Silicon

A

Same as diamond

25
Q

Graphene

A

1 layer of graphite- 1 atom thick and hexagonal carbon rings

Delocalised free moving electrons make it great conductor of electricity as they can carry a charge

Delocalised electrons strengthen covalent bonds, giving graphine high strength property

1 cell thick lightweight & transparent

Uses in smart phone screens n aircraft shells

26
Q

Simple molecular

A

Diatomic, nh3, h2o

Low mbp breaking weak london forces

27
Q

Giant covalent

A

Graphite diamond sio2

High m&bp strong covalent bonds

28
Q

Giant ionic

A

High mbp strong electrostatic forces of attraction

Metal non metal

29
Q

Metallic

A

Metal

High mbp string electrostatic forces of attraction

30
Q

Giant ionic solubility

A

As liquid, free ions allow electrical conduction

a level chemistry ocr a (26 decks)

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