10/17, 202A

Front 1

Radial Distribution function?

Back 1

describes probabilyt of finding an electron at a given radius (in all directions)

Front 2

Slaters rule?

Back 2

For electron in shell n, s = 0.35

For electron in shell n-1, s = 0.85

For electron in shell <n-1, s = 1

Where s = shielding effect.

S =∑s

Front 3

Effective nuclear charge?

Back 3

Zeff = Z-S

where Z = nuclear charge

S= shielding constant

Front 4

Trends in Effective nuclear charge?

Back 4

across row: Zeff increases - additional protons, poorly shielding additional electrons s = 0.35

down group, Zeff increases for first few elements then remains constant.

Front 5

Trends in orbital energies?

Back 5

-Down group energies become less negative, n-increases, Zeff-same

-across row enegies become more negative Zeff-increases, n-constant

Front 6

Atomic Radii trends?

Back 6

Down group radii increase (radial distribution function)

across row radii decreases - Zeff increases, valence electrons more attracted to nucleus.

Front 7

Atomic radii exceptions?

Back 7

Al -> Ga,

Ga - 10 extra protons, 10 extra non-fully shielding electrons therefore Zeff increases therefore smaller radius

Front 8

Ionisation energy (definition)

Back 8

The energy required to remove an electron from a gas-phase atom

Front 9

Ionisation energy trends?

Back 9

Down group, IE decreases- radius increases, Zeff constant.

across Row IE (generally) increases- Zeff increases,

Front 10

Ionisation energy exceptions

Back 10

Front 11

Electronegativity definition?

Back 11

The tendency of an atom, in a molecuse to attract a pair of electrons to itself.

Front 12

Electronegativity trends?

Back 12

Increases across a period - Zeff increases,

Decreases down a group,

Front 13

Metallic element characteristics?

Back 13

Low electronegativity

Readily give up electrons (low ionisation energy)

Metallic bonding

Delocalised electrons

Conduct heat and electricity

Front 14

Non-metallic elements characteristics?

Back 14

High electronegativity

High electron affinity

Covalent bonding

insulators

Low melting and boiling points

Front 15

Metalloid elements characteristics?

Back 15

intermediate electronegativity

Characteristics of bot hmetals and non-metals

Front 16

ionisation (eq)

Back 16

M(g) -> M(g)⁺ + e⁻

Front 17

Standard reduction potential E₀ (eq)

Back 17

∆G = -nFE₀

n = number of electrons

F = faraday constant

∆G = gibbs free energy (wants to be negative for a reaction to go forward rather than back.

therefore negative E₀ is a disfavoured process

Front 18

What sort of compounds do group 1 halides form

Back 18

ionic compounds

Front 19

What causes ionic compounds to form?

Back 19

Large electronegativity differences between atoms

Front 20

trends in ∆H of formation for group 1 halides.

Back 20

Front 21

Born Haber Cycle

Back 21

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