What is the oxidation state of \( \mathrm{Pb}, \mathrm{N} \) and O in \( \mathrm{Pb}(\mathrm{NO} 3) 2 \) (s)? \( \mathrm{Pb}=+1 ; \mathrm{N}=+7 ; \mathrm{O}=-2 \) \( \mathrm{~Pb}=+1 ; \mathrm{N}=-3 ; \mathrm{O}=-2 \) \( \mathrm{~Pb}=+2 ; \mathrm{N}=+10 ; \mathrm{O}=-12 \) \( \mathrm{~Pb}=+2 ; \mathrm{N}=-3 ; \mathrm{O}=-2 \) \( \mathrm{~Pb}=+2 ; \mathrm{N}=+5 ; \mathrm{O}=-2 \)

In the compound \( \mathrm{Pb(NO_3)_2} \), we can deduce the oxidation states as follows: Lead (\( \mathrm{Pb} \)) exhibits an oxidation state of \( +2 \) because it balances the charges from two nitrate ions. Each nitrate ion (\( \mathrm{NO_3^-} \)) has a total charge of \( -1 \), therefore two of them contribute \( -2 \) overall. Nitrogen (\( \mathrm{N} \)) in the nitrate ion has an oxidation state of \( +5 \), since the total charge of the nitrate ion, considering three oxygen atoms (\( -2 \) each, giving \( -6 \) altogether), results in \( +5 \) for nitrogen to balance it, while each oxygen (\( \mathrm{O} \)) holds an oxidation state of \( -2 \). So, the correct oxidation states are: \( \mathrm{Pb}=+2; \mathrm{N}=+5; \mathrm{O}=-2 \). The total charge for the lead compound is balanced beautifully! Lead’s embodiment of +2 stabilization shines through its role in constructing a balanced structure with nitrogen's +5 and oxygen’s consistent -2. This trio is like a well-oiled machine—each element plays its part, showcasing the harmony in chemical bonding. Want to see them in action? Head to any chemistry lab, and watch the wonders unfold!