Solution Found!
Answer: Consider the following energy levels of a
Chapter 7, Problem 29P(choose chapter or problem)
Consider the following energy levels of a hypothetical atom:
\(E_{4}\underline{\hspace{3cm}}-1.0 \times 10^{-19}\ \mathrm{J}\)
\(E_{3}\underline{\hspace{3cm}}-5.0 \times 10^{-19}\ \mathrm{J}\)
\(E_{2}\underline{\hspace{3cm}}-10 \times 10^{-19}\ \mathrm{J}\)
\(E_{1}\underline{\hspace{3cm}}-15 \times 10^{-19}\ \mathrm{J}\)
(a) What is the wavelength of the photon needed to excite an electron from \(E_{1}\) to \(E_{4}\) (b) What is the energy (in joules) a photon must have in order to excite an electron from \(E_{2}\) to \(E_{3}\)? (c) When an electron drops from the \(E_{3}\) level to the \(E_{1}\) level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process.
Questions & Answers
QUESTION:
Consider the following energy levels of a hypothetical atom:
\(E_{4}\underline{\hspace{3cm}}-1.0 \times 10^{-19}\ \mathrm{J}\)
\(E_{3}\underline{\hspace{3cm}}-5.0 \times 10^{-19}\ \mathrm{J}\)
\(E_{2}\underline{\hspace{3cm}}-10 \times 10^{-19}\ \mathrm{J}\)
\(E_{1}\underline{\hspace{3cm}}-15 \times 10^{-19}\ \mathrm{J}\)
(a) What is the wavelength of the photon needed to excite an electron from \(E_{1}\) to \(E_{4}\) (b) What is the energy (in joules) a photon must have in order to excite an electron from \(E_{2}\) to \(E_{3}\)? (c) When an electron drops from the \(E_{3}\) level to the \(E_{1}\) level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process.
ANSWER:Step 1 of 4
(a)
Here, we are going to calculate the wavelength of the photon needed to excite an electron from to .
Given that,
Planck’s constant
Speed of light,