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Ch.6 - Electronic Structure of Atoms
All textbooksBrown 14th EditionCh.6 - Electronic Structure of AtomsProblem 25b
Chapter 6, Problem 25b

(b) Calculate the energy of a photon of radiation whose wavelength is 413 nm.

Verified step by step guidance
1
Convert the wavelength from nanometers to meters by using the conversion factor: 1 nm = 1 x 10^{-9} m.
Use the speed of light equation: c = \lambda \nu, where c is the speed of light (3.00 x 10^8 m/s), \lambda is the wavelength in meters, and \nu is the frequency in s^{-1}. Rearrange the equation to solve for frequency: \nu = \frac{c}{\lambda}.
Substitute the wavelength in meters into the equation to calculate the frequency.
Use Planck's equation to find the energy of the photon: E = h\nu, where E is the energy in joules, h is Planck's constant (6.626 x 10^{-34} J·s), and \nu is the frequency calculated in the previous step.
Substitute the frequency and Planck's constant into the equation to calculate the energy of the photon.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Photon Energy

The energy of a photon is directly related to its frequency and inversely related to its wavelength. It can be calculated using the equation E = hν, where E is energy, h is Planck's constant (6.626 x 10^-34 J·s), and ν (nu) is the frequency of the radiation. The frequency can be derived from the wavelength using the speed of light equation, c = λν.
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Wavelength and Frequency Relationship

Wavelength (λ) and frequency (ν) are inversely related through the speed of light (c), which is approximately 3.00 x 10^8 m/s. The relationship is expressed as c = λν, meaning that as the wavelength increases, the frequency decreases, and vice versa. This relationship is crucial for converting wavelength measurements into frequency for energy calculations.
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Planck's Constant

Planck's constant is a fundamental constant in quantum mechanics that relates the energy of a photon to its frequency. It has a value of approximately 6.626 x 10^-34 J·s. This constant is essential for calculating photon energy and highlights the quantized nature of electromagnetic radiation, where energy is emitted or absorbed in discrete packets called quanta.
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Related Practice
Textbook Question

If human height were quantized in 1-cm increments, what would happen to the height of a child as she grows up: (i) the child's height would never change, (ii) the child's height would continuously increase, (iii) the child's height would increase in jumps of 6 cm, or (iv) the child's height would increase in 'jumps' of 1 cm at a time?

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Textbook Question
Einstein's 1905 paper on the photoelectric effect was thefirst important application of Planck's quantum hypothesis.Describe Planck's original hypothesis, and explain howEinstein made use of it in his theory of the photoelectriceffect.
Textbook Question

(a) Calculate the energy of a photon of electromagnetic radiation whose frequency is 2.94 × 1014 s-1.

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Textbook Question

(c) What wavelength of radiation has photons of energy 6.06 × 10-19 J?

Textbook Question

(a) A green laser pointer emits light with a wavelength of 532 nm. What is the frequency of this light?

Textbook Question

(b) What is the energy of one of these photons?

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