# he energy of the hydrogen atom in its nth orbit is En = $-\frac{13.6}{n^2} ev$. The energy required for sending electron from 1st orbit to the 2nd o

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he energy of the hydrogen atom in its nth orbit is En$-\frac{13.6}{n^2} ev$. The energy required for sending electron from 1st orbit to the 2nd orbit will be:

1. 10.2eV
2. 12.1 eV
3. 13.6 eV
4. 3.4 eV

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Correct Answer - Option 1 : 10.2eV

CONCEPT:

• The energy of electrons in any orbit is given by:

$E_n = -13.6 \frac{Z^2}{n^2} \,eV$

Where n = principal quantum number and Z = atomic number

CALCULATION:

Given - n = 2 and For hydrogen (Z) = 1

• The energy of electrons in 2nd is given by:

$⇒ E_2 = \frac{-13.6}{4} \,eV=-3.4 \,eV$

• The energy of electrons in 1st is given by:

$⇒ E_1 = \frac{-13.6}{1} \,eV=-13.6 \,eV$

• The energy required for sending electron from 1st orbit to the 2nd orbit will be:

⇒ ΔE = E2 - E1

⇒ ΔE = -3.4eV + 13.6eV = 10.2 eV