Cupric compounds are more stable than their c | vedclass

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(D) The electronic configurations of cuprous $(Cu^{+})$ and cupric $(Cu^{2+})$ ions are as follows:$Cu^{+} = [Ar] 3d^{10} 4s^{0}$$Cu^{2+} = [Ar] 3d^{9

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the lattice energy released for cupric compounds is much higher than for cuprous compounds

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(D) The electronic configurations of cuprous $(Cu^{+})$ and cupric $(Cu^{2+})$ ions are as follows:$Cu^{+} = [Ar] 3d^{10} 4s^{0}$$Cu^{2+} = [Ar] 3d^{9} 4s^{0}$Although $Cu^{+}$ has a more stable electronic configuration, $Cu^{2+}$ compounds are more stable in the solid state.This is primarily because the $2^{nd}$ ionization potential $(IP)$ of $Cu$ is not sufficiently high to prevent the formation of $Cu^{2+}$, and the higher charge density of $Cu^{2+}$ leads to a significantly higher lattice energy in ionic compounds compared to $Cu^{+}$ compounds.This large release of lattice energy compensates for the energy required to remove the second electron.

Cupric compounds are more stable than their cuprous counterparts in the solid state. This is because

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