Question

Xenon has closed shell configuration but is known to give compounds with fluorine because:
A. Xe atom has large size and lower ionization potential as compared to other noble gases
B. Xe has unpaired electrons which can form covalent bonds
C. Xe has highest boiling point hence it can form compounds with fluorine
D. Fluorine is the smallest element hence it can react with all noble gas

Answer 1

Hint: It is given that xenon has filled electronic configuration even though it forms a compound so we have to determine the reason for the formation of xenon compounds with fluorine. The reactivity of an element to form compounds depends upon the electronic configuration, size, ionization potential, etc.

Complete step-by-step answer:
Xenon is a group-$18$element. The atomic number of xenon is $54$. The electronic configuration of xenon is as follows:
${\text{[Kr]4}}{{\text{d}}^{{\text{10}}}}{\text{5}}{{\text{s}}^{\text{2}}}{\text{5}}{{\text{p}}^{\text{6}}}$ .
The outermost shell is ${\text{5s}}$ and ${\text{5p}}$ which are completely filled, so the xenon should be unreactive.

Down in a group, the electrons get added in the next higher shell, so the distance between the nucleus and outermost shell electron increases, so the size of the atom increases down in the group. Xenon comes in the sixth period, so its size is very large.

Due to the large distance between the nucleus and outermost shell electron, the outermost shell electrons are not tightly bound, so it is easy to remove an electron from xenon outermost shell. So, xenon can react easily. So, Xenon has closed shell configuration but is known to give compounds with fluorine because xenon atoms have large size and lower ionization potential as compared to other noble gases.

Therefore, option (A) xenon atom has large size and lower ionization potential as compared to other noble gases, is correct.

Note: Left to right in a period size decreases and down in a group size increases. The energy required to remove an electron from an isolated gaseous atom is known as ionization energy. Left to right in the periodic table ionization energy increases. Down in a group, the ionization energy decreases so, reactivity increases down in the group.