Which of the following orders regarding ionisation energy is correct?
N > O > F
N < O < F
N > O < F
N < O < F
C.
N > O < F
Ionisation energy is the energy required to remove an electron from outer shell of an atom. Since, on moving from left to right in a period, size decreases, thus, larger amount of energy is required to remove an electron, i.e. ionisation energy increases.
The size of Oxygen atom is smaller as compared to Nitrogen but the ionisation energy of Nitrogen is higher. This is mainly because in Nitrogen, the electron is to be removed from half-filled 2p3 orbital.
Thus, the correct order of ionisation energy is O < N < F.
The electronic configuration 1s2, 2s22p6, 3s23p63d9 represents a
metal atom
non metal atom
non-metallic anion
metallic cation
In a given shell the order of screening effect is
s > p > d > f
s > p > f > d
f > d > p > s
s < p < d < f
The ionisation energy of hydrogen atom is 13.6eV. What will be the ionisation energy of He+?
13.6 eV
54.4 eV
122.4 eV
Zero