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physical chemistry > 3.1.1.3 Electron configuration- First ionisation energy > Flashcards

3.1.1.3 Electron configuration- First ionisation energy Flashcards

1
Q

why the first ionisation energy of rubidium is less than the first ionisation energy of krypton

A 
outer electron in Rb is in 5th shell (or additional shell) 
further away (or more shielded) from nucleus
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2
Q

Chemical equation for the enthalpy change: the first molar ionisation energy of silicon

A

Si(g) → Si+ (g) + e–

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3
Q

Chemical equation for the enthalpy change: the second molar ionisation energy of silicon

A

Si+ (g) → Si2+(g) + e–

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4
Q

reasons why the first ionisation energy of neon is lower than the third ionisation energy of magnesium

A

Mg2+ ion smaller than Ne atom / Mg2+ e – closer to nucleus

Mg2+ has more protons than Ne / higher nuclear charge

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5
Q

The general trend in the first ionisation energies of the Period 3 elements, Na – Ar

A

trend: increases
more protons / increased proton number / increased nuclear charge
same shell / same shielding / smaller size

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6
Q

why the first ionisation energy of sulphur is lower than would be predicted from the general trend of period 3 elements

A

e- pair in the 3p sub-level

repulsion between the e– in this e– pair

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7
Q

Definition: first ionisation energy

A

Energy to remove 1 electron

from a gaseous atom

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8
Q

why boron has a lower first ionisation energy than beryllium

A

Be’s outer electron is in an s (2s) orbital
B’s outer electron is in a p (2p) orbital
B’s outer electron is higher in energy

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9
Q

why the first ionisation energy of helium is very large

A

Electron is not shielded from nucleus

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10
Q

the general trend in the first ionisation energy of the Period 3 elements from Na to Ar

A

Increases

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11
Q

how, and explain why, the first ionisation energy of aluminium does not follow this general trend

A

lower than expected / lower than Mg / 1 less energy needed to ionise; e– removed from (3)p sub-level;
of higher energy / further away from nucleus / shielded by 3s e – s;

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12
Q

an equation, including state symbols, to represent the process for which the energy change is the first ionisation energy of Na

A

Na(g) → Na+ (g) + e–

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13
Q

the general trend in the values of the first ionisation energies of the elements Na to Ar

A 
Trend : Increases
Explanation : Increased nuclear charge or proton number
Stronger attraction (between nucleus and (outer) e– )
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14
Q

how, and explain why, the values of the first ionisation energies of the elements Al and S deviate from the general trend

A

How values deviate from trend: (both values) too low
Explanation for Al: e– removed from 3p
e – or orbital is higher in energy level or better shielded than (3)s
or p electron is shielded by 3s electrons
Explanation for S: e– removed from (3)p electron pair (1) repulsion between paired e– (reduces energy required)

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15
Q

Definition: first ionisation energy

A

Heat / enthalpy / energy for removal of one electron (1) from a gaseous atom

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16
Q

Why the first ionisation energy of neon is higher than sodium

A

Neon’s electron is in a lower (2p) shell

attracted more strongly to (or less shielded from) the nucleus

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17
Q

Why the first ionisation energy of magnesium is higher than sodium

A

more protons
electrons in same shell
similar shielding

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18
Q

why the first ionisation energy of aluminium is lower than that of magnesium

A

Als outer electron is in a 3p sub-shell

higher in energy than 3s in Magnesium

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19
Q

the variation in first ionisation energy of the elements across Period 3 from sodium to argon

A

general increase across period
because number of protons (or nuclear charge) increases
but electrons in same shell (or similar shielding)
fall from Mg to Al
Al’s outer electron is in a p orbital
higher in energy than s electron in Mg
fall from P to S
two of the p electrons in S are paired (or in same orbital)

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20
Q

the trend in the first ionisation energies of the elements in Group 2 from magnesium to barium

A

Decrease
Ions get bigger / more (energy) shells
Weaker attraction of ion to lost electron

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21
Q

the element in Period 3 that has the highest first ionisation energy

A

Argon / Ar
Large(st) number of protons / large(st) nuclear charge
Same amount of shielding / same number of shells / same number of energy levels

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22
Q

an equation, including state symbols, to show the process that occurs when the first ionisation energy of rubidium is measured

A 
Rb(g) → Rb+ (g) + e(–) 
OR Rb(g) + e(–) → Rb+ (g) + 2e(–) 
OR Rb(g) - e(–) → Rb+ (g)
23
Q

why the first ionisation energy of rubidium is lower than the first ionisation energy of sodium

A

Rb is a bigger (atom) / e further from nucleus / electron lost from a higher energy level/ More shielding in Rb / less attraction of nucleus in Rb for outer electron / more shells

24
Q

why the value of the first ionisation energy of sulfur is less than the value of the first ionisation energy of phosphorus

A

Paired electrons in (3)p orbital

repel

25
the element in Period 2 that has the highest first ionisation energy
Neon/Ne
26
an equation, including state symbols, to show the reaction that occurs when the first ionisation energy of lithium is measured.
Li(g) → Li+ (g) + e- (g) Li(g) - e- (g) → Li+ (g) Li(g) + e- (g) → Li+ (g) + 2e
27
the general trend in first ionisation energies for the Period 3 elements aluminium to argon
Increases Increasing nuclear charge / increasing no of protons Same or similar shielding / same no of shells / electron (taken) from same (sub)shell / electron closer to the nucleus / smaller atomic radius
28
how selenium deviates from this general trend in first ionisation energies for the Period 4 elements gallium to krypton
Lower Paired electrons in a (4) p orbital (Paired electrons) repel
29
why the first ionisation energy of krypton is lower than the first ionisation energy of argon
Kr is a bigger atom / has more shells / more shielding in Kr / electron removed further from nucleus/ electron removed from a higher (principal or main) energy level
30
Definition: first ionisation energy
Energy/enthalpy (needed) to remove one mole of electrons from one mole of atoms/compounds/molecules/elements 1 OR Energy to form one mole of positive ions from one mole of atoms OR Energy/enthalpy to remove one electron from one atom In the gaseous state (to form 1 mol of gaseous ions)
31
the general trend in the first ionisation energies of the Period 3 elements sodium to chlorine
Increase Bigger nuclear charge (from Na to Cl)/more protons electron (taken) from same (sub)shell/similar or same shielding/ electron closer to the nucleus/smaller atomic radius
32
How and why the element sulfur deviates from the general trend in first ionisation energies across Period 3
Lower Two/pair of electrons in (3)p orbital repel (each other)
33
one element which deviates from the general trend in the first ionisation energies of the Period 2 elements lithium to fluorine
Boron/B or oxygen/O/O2
34
Definition: first ionisation energy of an atom
enthalpy/energy change/required when an electron is removed/ knocked out / displaced/ to form a uni-positive ion from a gaseous atom
35
The Ne atom and the Mg2+ ion have the same number of electrons reasons why the first ionisation energy of neon is lower than the third ionisation energy of magnesium
Mg2+ ion smaller than Ne atom / Mg2+ e– closer to nucleus | Mg2+ has more protons than Ne / higher nuclear charge or e – is removed from a charged Mg2+ion / neutral neon atom
36
The general trend in the first ionisation energies of the Period 3 elements, Na – Ar
trend: increases more protons / increased proton number / increased nuclear charge same shell / same shielding / smaller size
37
why the first ionisation energy of sulphur is lower than would be predicted from the general trend
the e– pair in the 3p sub-level | repulsion between the e– in this e–pair
38
the general trend in the first ionisation energy of the Period 3 elements from Na to Ar
trend: increases
39
How and why the first ionisation energy of aluminium does not follow this general trend
``` lower than expected / lower than Mg / less energy needed to ionise; e– removed from (3)p sub-level; (‘e– removed’ may be implied) o f higher energy / further away from nucleus / shielded by 3s e–s ```
40
Definition: first ionisation of an atom
Enthalpy change/required when an electron is removed/knocked out/displaced From a gaseous atom
41
why the value of the first ionisation energy of magnesium is higher than that of sodium
Increased/stronger nuclear charge or more protons | Smaller atom or electrons enter the same shell or same/similar shielding
42
why the value of the first ionisation energy of neon is higher than that of sodium
Electron removed from a shell of lower energy or smaller atom or e– nearer nucleus or e– removed from 2p rather than from 3s Less shielding
43
Definition: first ionisation energy
Heat / enthalpy / energy for removal of one electron | from a gaseous atom
44
an equation, including state symbols, to represent the process for which the energy change is the first ionisation energy of Na
``` Na(g) → Na+ (g) + e– OR Na(g) + e– → Na+ (g) + 2e– ```
45
the general trend in the values of the first ionisation energies of the elements Na to A
``` Trend : Increases Explanation : Increased nuclear charge or proton number Stronger attraction (between nucleus and (outer) e– ) ```
46
how and why the values of the first ionisation energy of the element Al deviates from the general trend
too low e– removed from (3) p e – or orbital is higher in energy or better shielded than (3)s or p electron is shielded by 3s electrons
47
how and why the values of the first ionisation energy of the element S deviates from the general trend
too low e– removed from (3)p electron pair repulsion between paired e– (reduces energy required)
48
Why the first ionisation energy of krypton is greater than that of bromine
Krypton has more protons than bromine | But its outer electrons are in the same shell (or have similar shielding)
49
why the value of the first ionisation energy of magnesium is higher than that of sodium
Increased/stronger nuclear charge or more protons | Smaller atom or electrons enter the same shell or same/similar shielding
50
Explain why the value of the first ionisation energy of neon is higher than that of sodium
Electron removed from a shell of lower energy or smaller atom or e– nearer nucleus or e– removed from 2p rather than from 3s Less shielding
51
Explain why helium has a much higher first ionisation energy than lithium
He’s electron in 1s | closer to nucleus (or no shielding)
52
why beryllium has a higher first ionisation energy than boron
Be’s outer electron in 2s | lower in energy than 2p
53
why the first ionisation energy of krypton is greater than the first ionisation energy of bromine
more protons or increased nuclear charge attracting electrons in the same {shell/orbital/sub–shell/energy level or similar shielding

physical chemistry (18 decks)

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