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(D) The energy of an electron in the $n^{th}$ orbit of a hydrogen atom is given by $E_n = -\frac{13.6}{n^2} \ eV$.For the ground state,$n = 1$.The sec

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(D) The energy of an electron in the $n^{th}$ orbit of a hydrogen atom is given by $E_n = -\frac{13.6}{n^2} \ eV$.For the ground state,$n = 1$.The second excited state corresponds to $n = 3$.The energy of the electron in the second excited state is $E_3 = -\frac{13.6}{3^2} = -\frac{13.6}{9} \approx -1.51 \ eV$.The energy required to ionize the atom from this state is the energy needed to bring the electron to $n = \infty$,which is $E_{\infty} - E_3 = 0 - (-1.51) = 1.51 \ eV$.

List-$I$ (Spectral Series for Hydrogen)	List-$II$ (Spectral Region)
$A$. Lyman	$I$. Infrared region
$B$. Balmer	$II$. $UV$ region
$C$. Paschen	$III$. Infrared region
$D$. Pfund	$IV$. Visible region

The ionization energy of a hydrogen atom is $13.6 \ eV$. The energy required to ionize a hydrogen atom in its second excited state is ........... $eV$.

Similar Questions

Which of the following is correct regarding Bohr's theory?

Consider an electron moving in the first Bohr orbit of a $He^{+}$ ion with a velocity $v_1$. If it is allowed to move in the third Bohr orbit with a velocity $v_3$, then indicate the correct $v_3: v_1$ ratio.

Rutherford's $\alpha$-particle scattering experiment eventually led to the conclusion that

Match List-$I$ with List-$II$.

List-$I$ (Spectral Series for Hydrogen) List-$II$ (Spectral Region)

$A$. Lyman $I$. Infrared region

$B$. Balmer $II$. $UV$ region

$C$. Paschen $III$. Infrared region

$D$. Pfund $IV$. Visible region

Choose the correct answer from the options given below:

The energy of an electron in the first Bohr orbit of hydrogen atom is $-2.18 \times 10^{-18} \ J$. Its energy in the third Bohr orbit is $........$.

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