What is the energy (in J atom\(^{-1}\)) required for the following process?}
\[
Li^{2+}(g) \rightarrow Li^{3+}(g) + e^{-}
\]
(Take the ionization energy for the H atom in the ground state as \(2.18 \times 10^{-18}\) J atom\(^{-1}\)).
- \(8.72 \times 10^{-18}\)
- \(1.962 \times 10^{-18}\)
- \(1.962 \times 10^{-17}\)
- \(6.54 \times 10^{-17}\)
The Correct Option is C
Solution and Explanation
Step 1:Calculate ionization energy} \[ E = 2.18 \times 10^{-18} \times 3^2 \] \[ E = 2.18 \times 10^{-18} \times 9 \] \[ E = 19.62 \times 10^{-18} \] \[ E = 1.962 \times 10^{-17} \] Thus \[ \boxed{1.962 \times 10^{-17}} \]
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