ie exam qs Flashcards

1
Q

State and explain the trend in the first ionisation energies of the elements in Group
2 from magnesium to barium.

A

decreases, ions get bigger, weaker attraction of ion to lost electron

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2
Q

State the element in Period 3 that has the highest first ionisation energy.
Explain your answer

A

Argon, largest number of protons same amount of shielding

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3
Q

Give one reason why the second ionisation energy of silicon is lower than the
second ionisation energy of aluminium.

A

Electron in Si (removed from) (3)p orbital

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4
Q

Explain why the ionisation energy of every element is endothermic.

A

Heat or energy needed to overcome the attraction between the negative electron and the positive nucleus

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5
Q

Explain 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

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6
Q

Explain why the second ionisation energy of magnesium is greater than the
first ionisation energy of magnesium.

A

electron being removed is closer to the nucleus

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7
Q

Explain why the first ionisation energy of sulphur is lower than would be
predicted from the general trend.

A

e–pair in the 3p sub-level
repulsion between the e–
in this e–pair

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8
Q

Explain why the value of the first ionisation energy of magnesium is higher than that
of sodium.

A

more protons, same shielding

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9
Q

How the values deviate from the trend
Explanation for Al
Explanation for S

A

How values deviate from trend: (both values) too low
Explanation for Al: e– removed from (3) p
Explanation for S: e– removed from (3)p electron pair repulsion between paired e–

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10
Q

Explain why chromium is placed in the d block in the Periodic Table.

A

Highest energy e

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11
Q

Explain the general increase in the values of the first ionisation energies of the
elements Na–Ar

A

increased nuclear charge, same shielding, Stronger attraction between nucleus and outer electrons

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12
Q

for describing electron spray ionisation

A

say particle gains a proton

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13
Q

Give the formula of the ion that reaches the detector first in the TOF mass
spectrometer.

A

C3H6O2N+

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14
Q

cm to m

A

/100

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15
Q

Explain why the first ionisation energy of the Group 2 elements decreases down the
group

A

the atoms get larger
There is a weaker attraction between the nucleus and the outer
electron

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