Which element of the following pairs of elements has higher ionisation energy? Justify your answer
a) K or Ca
b) Be or B
c) I or Ba
d) F or Cl
e) N or O
Answers
Across the Periods, Ionization energy increases due to the increase in the nuclear charge and decrease in the atomic size.
In the Group, from top to the bottom, Ionization energy decreases due to the increases in the Atomic size and decrease in the nuclear charge.
(a). In K and Ca, Ca has the high Ionization energy.
Reason ⇒ K and Ca lies in the Fourth Periods, in which K lies at first and Ca lies after than.
(b). In Be and B,Be have the high Ionization energy.
Reason ⇒ Although, Boron lies after the Be in the Second Period, but The ionization energy of Boron is less than that of Beryllium because in Boron there is a complete 2s orbital. The increased shielding of the 2s orbital reduces the ionization energy of the Boron. Hence, the Be have the high Ionization energy.
(c). Iodine (or I) have the more Ionization energy than the Ba, because Iodine lies at the last of the Period 5 where the Ionization energy is high, and Ba lies in the starting of the Periods 6, when the Ionization energy is least.
(d). In Florine and Chlorine, Florine have the high ionization energy than than the Chlorine because Chlorine lies below the Florine in the Halogen Group.
(e). Oxygen have the high Ionization energy because it lies after the Nitrogen in the Periods.
Hope it helps.
Answer:
Ionization energy is the amount of the energy released while converting the neutral isolated gaseous atom into the positively charged ions.
Across the Periods, Ionization energy increases due to the increase in the nuclear charge and decrease in the atomic size.
In the Group, from top to the bottom, Ionization energy decreases due to the increases in the Atomic size and decrease in the nuclear charge.
(a). In K and Ca, Ca has the high Ionization energy.
Reason ⇒ K and Ca lies in the Fourth Periods, in which K lies at first and Ca lies after than.
(b). In Be and B,Be have the high Ionization energy.
Reason ⇒ Although, Boron lies after the Be in the Second Period, but The ionization energy of Boron is less than that of Beryllium because in Boron there is a complete 2s orbital. The increased shielding of the 2s orbital reduces the ionization energy of the Boron. Hence, the Be have the high Ionization energy.
(c). Iodine (or I) have the more Ionization energy than the Ba, because Iodine lies at the last of the Period 5 where the Ionization energy is high, and Ba lies in the starting of the Periods 6, when the Ionization energy is least.
(d). In Florine and Chlorine, Florine have the high ionization energy than than the Chlorine because Chlorine lies below the Florine in the Halogen Group.