If the electron in a hydrogen atom were in the energy level with $n = 3$ , how much energy in joule would be required to ionise the atom? (Ionisation energy of $H -$ atom is $2.18 \times 10^{- 18} J$ ):

6.54 \times 10^{- 19}

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1.43 \times 10^{- 19}

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2.42 \times 10^{- 19}

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3.14 \times 10^{- 20}

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Solution

The correct option is C $2.42 \times 10^{- 19}$
Energy of $e^{-}$ in $n^{t h}$ shell $= - 13.6 \frac{τ^{2}}{n^{2}}$
For $H -$ atom with $n = 3 \to E = - 13.6 \times \frac{1}{9}$
$\Rightarrow E = \frac{1}{9}$ (Energy of $e^{-}$ in first shell)
$\Rightarrow E = \frac{1}{9} \times 2.18 \times 10^{- 18}$
$\Rightarrow E = 2.42 \times 10^{- 19} J$ (Ionisation Energy $=$ Energy of $e^{-}$ in first shell)

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If the electron in a hydrogen atom were in the energy level with n=3, how much energy in joule would be required to ionise the atom? (Ionisation energy of H−atom is 2.18×10−18J):

The correct option is C 2.42×10−19Energy of e− in nth shell =−13.6τ2n2For H−atom with n=3→E=−13.6×19⇒E=19 (Energy of e− in first shell)⇒E=19×2.18×10−18⇒E=2.42×10−19J(Ionisation Energy= Energy of e− in first shell)

If the electron in a hydrogen atom were in the energy level with $n = 3$ , how much energy in joule would be required to ionise the atom? (Ionisation energy of $H -$ atom is $2.18 \times 10^{- 18} J$ ):