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(D) The thermal decomposition of $AgNO_3$ is given by the reaction: $2AgNO_3(s) \rightarrow 2Ag(s) + 2NO_2(g) + O_2(g)$.The two paramagnetic gases pro

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$6$

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(D) The thermal decomposition of $AgNO_3$ is given by the reaction: $2AgNO_3(s) \rightarrow 2Ag(s) + 2NO_2(g) + O_2(g)$.The two paramagnetic gases produced are $NO_2$ and $O_2$.$NO_2$ is an odd-electron molecule with $1$ unpaired electron.$O_2$ has $2$ unpaired electrons in its antibonding $\pi^*2p_y$ and $\pi^*2p_z$ orbitals.Since $O_2$ has a higher number of unpaired electrons $(2 > 1)$,we consider the antibonding molecular orbitals of $O_2$.The molecular orbital configuration of $O_2$ ($16$ electrons) is: $\sigma1s^2, \sigma^*1s^2, \sigma2s^2, \sigma^*2s^2, \sigma2p_x^2, \pi2p_y^2 = \pi2p_z^2, \pi^*2p_y^1 = \pi^*2p_z^1$.The antibonding molecular orbitals are $\sigma^*1s$,$\sigma^*2s$,and $\pi^*2p_y, \pi^*2p_z$.The number of electrons in these orbitals are $2 + 2 + 1 + 1 = 6$.

Thermal decomposition of $AgNO_3$ produces two paramagnetic gases. The total number of electrons present in the antibonding molecular orbitals of the gas that has the higher number of unpaired electrons is. . . . .

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