Question: Q. 8. The energy levels of a hypothetical atom are given below. Which of the shown transitions will result in the emission of photon of wavelength $275 \mathrm{~nm}$ ?

A] [OD South 2016]

Show Answer

Solution:

Ans. (i) Energy of photon $=\frac{h c}{\lambda}$

$$ \begin{aligned} & =\frac{6.64 \times 10^{-34} \times 3 \times 10^{8}}{275 \times 10^{-9} \times 1.6 \times 10^{-18}} \mathrm{eV} \ & =4.5 \mathrm{eV} \quad 1 / 2+1 / 2 \end{aligned} $$

(ii) The corresponding transition is $B$

[CBSE Marking Scheme 2016]

Detailed Answer :

Energy of a photon corresponding to wavelength $\lambda$,

$$ \begin{aligned} E & =h \frac{c}{\lambda} \ & =\frac{6.6 \times 10^{-34} \times 3 \times 10^{8}}{275 \times 10^{-9}} \mathrm{~J} \quad 1 / 2 \ & =\frac{6.6 \times 10^{-34} \times 3 \times 10^{8}}{275 \times 10^{-9} \times 1.6 \times 10^{-19}} \mathrm{eV} \end{aligned} $$

$$ \begin{align*} & =\frac{6.6 \times 3 \times 10^{2}}{275 \times 1.6} \ & =4.5 \mathrm{eV} \tag{1} \end{align*} $$

(ii) the calculated energy of the photon matches with the transition $B$.



विषयसूची

जेईई के लिए मॉक टेस्ट

एनसीईआरटी अध्याय वीडियो समाधान

दोहरा फलक