JEE CHEMISTRY MCQ: STRUCTURE OF ATOM

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Application +4 | -1

Based on the equation

\Delta E=-2.0 \times 10^{-18} \mathrm{~J}\left(\frac{1}{n_2^2}-\frac{1}{n_1^2}\right)

the wavelength of the light that must be absorbed to excite hydrogen electron from level

n=1

to level

n=2

will be

\left(h=6.625 \times 10^{-34} \mathrm{~J} \mathrm{~s}, c=3 \times 10^8 \mathrm{~m} \mathrm{~s}^{-1}\right)

View answer and explanation

Correct option: A

1.325 \times 10^{-7} \mathrm{~m}

Option A (

1.325 \times 10^{-7} \mathrm{~m}

) is correct because it is the calculated wavelength of light absorbed during the electron transition from n=1 to n=2 in a hydrogen atom, using the provided energy equation.

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