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Answer: Consider the following energy levels of a

Chapter 7, Problem 29P

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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.

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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,  

   

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