ie exam qs Flashcards
State and explain the trend in the first ionisation energies of the elements in Group
2 from magnesium to barium.
decreases, ions get bigger, weaker attraction of ion to lost electron
State the element in Period 3 that has the highest first ionisation energy.
Explain your answer
Argon, largest number of protons same amount of shielding
Give one reason why the second ionisation energy of silicon is lower than the
second ionisation energy of aluminium.
Electron in Si (removed from) (3)p orbital
Explain why the ionisation energy of every element is endothermic.
Heat or energy needed to overcome the attraction between the negative electron and the positive nucleus
Explain why the value of the first ionisation energy of sulfur is less than the value of
the first ionisation energy of phosphorus.
Paired electrons in (3)p orbital
repel
Explain why the second ionisation energy of magnesium is greater than the
first ionisation energy of magnesium.
electron being removed is closer to the nucleus
Explain why the first ionisation energy of sulphur is lower than would be
predicted from the general trend.
e–pair in the 3p sub-level
repulsion between the e–
in this e–pair
Explain why the value of the first ionisation energy of magnesium is higher than that
of sodium.
more protons, same shielding
How the values deviate from the trend
Explanation for Al
Explanation for S
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–
Explain why chromium is placed in the d block in the Periodic Table.
Highest energy e
Explain the general increase in the values of the first ionisation energies of the
elements Na–Ar
increased nuclear charge, same shielding, Stronger attraction between nucleus and outer electrons
for describing electron spray ionisation
say particle gains a proton
Give the formula of the ion that reaches the detector first in the TOF mass
spectrometer.
C3H6O2N+
cm to m
/100
Explain why the first ionisation energy of the Group 2 elements decreases down the
group
the atoms get larger
There is a weaker attraction between the nucleus and the outer
electron