The amount of energy required to remove the electron from a $L i^{2 +}$ ion in its ground state is how many times greater than the amount of energy required to remove the electron from an $H - a t o m$ in its ground state?

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Solution

The energy of transition is given by,

$E = - 13.6 Z^{2} (\frac{1}{n_{t}^{2}} - \frac{1}{n_{i}^{2}})$

$∵$ Both $n$ values for transition in the question are same

The ratio of the energies determined only by the ratio of the $Z^{2}$ or $1^{2} / 3^{2}$ or $1 / 9$ .

Thus, the energy required to remove an $e^{-}$ from $L i^{2 +}$ is $9$ times more than Hydrogen.

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The amount of energy required to remove the electron from a Li2+ ion in its ground state is how many times greater than the amount of energy required to remove the electron from an H−atom in its ground state?

The energy of transition is given by,E=−13.6Z2(1n2t−1n2i)∵ Both n values for transition in the question are sameThe ratio of the energies determined only by the ratio of the Z2 or 12/32 or 1/9. Thus, the energy required to remove an e− from Li2+ is 9 times more than Hydrogen.

The amount of energy required to remove the electron from a $L i^{2 +}$ ion in its ground state is how many times greater than the amount of energy required to remove the electron from an $H - a t o m$ in its ground state?