Given below are two statements : Statement I : The correct order of first ionization enthalpy values of Li, Na, F and Cl is Na < Li < Cl < F.…

It is noticed that $\mathrm{Pb}^{2+}$ is more stable than $\mathrm{Pb}^{4+}$ but $\mathrm{Sn}^{2+}$ is less stable than $\mathrm{Sn}^{4+}$. Observe the following reactions. $\mathrm{PbO}_{2}+\mathrm{Pb} \rightarrow 2 \mathrm{PbO} ; \Delta_{\mathrm{r}} \mathrm{G}^{\circ}(1)$ $\mathrm{SnO}_{2}+\mathrm{Sn} \rightarrow 2 \mathrm{SnO} ; \Delta_{\mathrm{r}} \mathrm{G}^{\circ}(2)$ Identify the correct set from the following

An excess of AgNO$_3$ is added to $100$ mL of a $0.05$ M solution of tetraaquadichloridochromium (III) chloride. The number of moles of AgCl precipitated will be __________ $\times 10^{-3}$. (Nearest integer)

Which of the following elements has the highest electronegativity?

First and second ionization enthalpies of lithium are $520$ kJ mol$^{-1}$ and $7297$ kJ mol$^{-1}$ respectively. Energy required to convert $3.5$ mg lithium (g) into $\text{Li}^{2+}$(g) $[\text{Li(g)} \rightarrow \text{Li}^{2+}\text{(g)}]$ is _______ kJ mol$^{-1}$. (nearest integer) [Molar mass of Li $= 7$ g mol$^{-1}$]

Identify the molecule $(X)$ with maximum number of lone pairs of electrons (obtained using Lewis dot structure) among $\mathrm{HNO}_{3}, \mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{NF}_{3}$ and $\mathrm{O}_{3}$. Choose the correct bond angle made by the central atom of the molecule $(\mathrm{X})$.