(a) A molecule decreases its vibrational energy by 0.250 eV by giving up a photon of light. What

Name: Problem 20, Chapter 29: College Physics
Uploaded: 2019-12-19T02:11:00-08:00
Duration: 1 min 19 s
Channel: Kai Chen

step 1 is this question. We have C energy of the hydrogen corpulent bound to be deductive four point fo

Question

(a) A molecule decreases its vibrational energy by $0.250 \mathrm{eV}$ by giving up a photon of light. What wavelength of light does it give up during this process, and in what part of the electromagnetic spectrum does that wavelength of light lie? (b) An atom decreases its energy by $8.50 \mathrm{eV}$ by giving up a photon of light. What wavelength of light does it give up during this process, and in what part of the electromagnetic spectrum does that wavelength of light lie? (c) A molecule decreases its rotational energy by $3.20 \times 10^{-3} \mathrm{eV}$ by giving up a photon of light. What wavelength of light does it give up during this process, and in what part of the electromagnetic spectrum does that wavelength of light lie?

   (a) A molecule decreases its vibrational energy by $0.250 \mathrm{eV}$ by giving up a photon of light. What wavelength of light does it give up during this process, and in what part of the electromagnetic spectrum does that wavelength of light lie? (b) An atom decreases its energy by $8.50 \mathrm{eV}$ by giving up a photon of light. What wavelength of light does it give up during this process, and in what part of the electromagnetic spectrum does that wavelength of light lie? (c) A molecule decreases its rotational energy by $3.20 \times 10^{-3} \mathrm{eV}$ by giving up a photon of light. What wavelength of light does it give up during this process, and in what part of the electromagnetic spectrum does that wavelength of light lie?

College Physics

Hugh D. Young Philip… 11th Edition

Chapter 29, Problem 20

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Solved by Expert Kai Chen

12/19/2019

Step 1

We know that 1 eV = 1.6 x 10^(-19) J. (a) The energy of the photon is E = 0.250 eV = 0.250 * 1.6 x 10^(-19) J = 4.0 x 10^(-20) J. We can use the energy-wavelength relationship for a photon: E = hc/λ, where h is the Planck's constant (6.63 x 10^(-34) Js), c is Show more…

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(a) A molecule decreases its vibrational energy by $0.250 \mathrm{eV}$ by giving up a photon of light. What wavelength of light does it give up during this process, and in what part of the electromagnetic spectrum does that wavelength of light lie? (b) An atom decreases its energy by $8.50 \mathrm{eV}$ by giving up a photon of light. What wavelength of light does it give up during this process, and in what part of the electromagnetic spectrum does that wavelength of light lie? (c) A molecule decreases its rotational energy by $3.20 \times 10^{-3} \mathrm{eV}$ by giving up a photon of light. What wavelength of light does it give up during this process, and in what part of the electromagnetic spectrum does that wavelength of light lie?

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Key Concepts

Bond Dissociation Energy

This concept represents the energy required to break a specific chemical bond, such as a covalent bond between two atoms. It quantifies the bond’s strength and defines the minimum energy needed to overcome the attractive forces holding the atoms together.

Photon Energy and Wavelength Relationship

This principle, defined by Planck’s equation (E = hc/?), states that the energy of a photon is inversely proportional to its wavelength. It explains that to supply a specific amount of energy, one can determine the required wavelength of light, with higher energy corresponding to shorter wavelengths.

Electromagnetic Spectrum

The electromagnetic spectrum includes all types of electromagnetic radiation, categorized by their wavelengths and frequencies. Understanding which part of the spectrum, such as the ultraviolet region, can provide photons with sufficient energy is key when considering processes like photodissociation of molecules.

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