Question

If energy is absorbed by a hydrogen atom in its ground state, the atom is excited to a higher energy state. For example, the excitation of an electron from the level with $n=1$ to the level with $n=3$ requires radiation with a wavelength of $102.6 \mathrm{nm} .$ Which of the following transitions would require radiation of longer wavelength than this? (a) $n=2$ to $n=4$ (c) $n=1$ to $n=5$ (b) $n=1$ to $n=4$ (d) $n=3$ to $n=5$

          If energy is absorbed by a hydrogen atom in its ground state, the atom is excited to a higher energy state. For example, the excitation of an electron from the level with $n=1$ to the level with $n=3$ requires radiation with a wavelength of $102.6 \mathrm{nm} .$ Which of the following transitions would require radiation of longer wavelength than this?
(a) $n=2$ to $n=4$
(c) $n=1$ to $n=5$
(b) $n=1$ to $n=4$
(d) $n=3$ to $n=5$

Added by Xavier M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

10/24/2022

Step 1

The energy of a photon is given by $E = h \nu = h c/\lambda$, where $h$ is Planck's constant, $\nu$ is the frequency of the radiation, $c$ is the speed of light, and $\lambda$ is the wavelength of the radiation. Show more…

Show all steps

Thanks for your feedback!

If energy is absorbed by a hydrogen atom in its ground state, the atom is excited to a higher energy state. For example, the excitation of an electron from the level with $n=1$ to the level with $n=3$ requires radiation with a wavelength of $102.6 \mathrm{nm} .$ Which of the following transitions would require radiation of longer wavelength than this? (a) $n=2$ to $n=4$ (c) $n=1$ to $n=5$ (b) $n=1$ to $n=4$ (d) $n=3$ to $n=5$