Question

In a hydrogen atom, the electron jumps from 3 to 2 energy level, the energy released is:

• A. $3.03\times {10}^{-19}Jato{m}^{-1}$
• B. $1.03\times {10}^{-19}Jato{m}^{-1}$
• C. $3.03\times {10}^{-18}Jato{m}^{-1}$
• D. $6.06\times {10}^{-19}Jato{m}^{-1}$

Answer 1

The correct option is A $3.03\times {10}^{-19}Jato{m}^{-1}$

Energy of electron in $1^{st}$ orbit $=-13.6ev$

$Energy\propto \frac{Z^2}{n^2}$

Energy in the $2^{nd}$ orbit $=\frac{-13.6}{4}ev$

Energy in the $3^{rd}$ orbit $=\frac{-13.6}{9}ev$

$\Delta E=-13.6\times (\frac{1}{9}-\frac{1}{4})\times 1.6\times {10}^{-19}$

$\Delta E=3.022\times {10}^{-19}Jato{m}^{-1}$

Hence, option A is correct.