The valence shell electron configuration of first excited state of sulphur is $3 \mathrm{s}^{2} 3 \mathrm{p}^{3} 3 \mathrm{d}^{1}$
The valence shell electron configuration of second excited state of sulphur is $3 \mathrm{s}^{1} 3 \mathrm{p}^{2} 3 \mathrm{d}^{2}$.
This is followed by sp ${ }^{3} \mathrm{d}^{2}$ hybridization to form $\mathrm{SF}_{6}$.
Thus $\mathrm{SF}_{6}$ is formed in the second excitation state of sulphur atom.
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Calculate the amount of energy required to convert $110\, mg$ of $'X'$ atom in gaseous state into $X^+$ ion .................... $\mathrm{kJ}$ (Atomic wt. for $X = 7\, g/mol$)
Statement $(I)$ : $\mathrm{SiO}_2$ and $\mathrm{GeO}_2$ are acidic while $\mathrm{SnO}$ and $\mathrm{PbO}$ are amphoteric in nature.
Statement $(II)$ : Allotropic forms of carbon are due to property of catenation and $\mathrm{p} \pi-\mathrm{d} \pi$ bond formation.
In the light of the above statements, choose the most appropriate answer from the options given below: