1.19 Sodium vapor lamps, used for public lighting, emit yellow light of wavelength 589 nm. How much energy is emitted by (a) an excited sodium atom when it generates a photon; (b) 5.00 mg of sodium atoms emitting light at this wavelength; (c) 1.00 mol of sodium atoms emitting light at this wavelength? 1.20 When an electron beam strikes a block of copper, x-rays with a frequency of 1.2 x 1017 Hz are emitted. How much energy is emitted at this wavelength by (a) an excited copper atom when it generates an x-ray photon; (b) 2.00 mol of excited copper atoms (c) 2.00 g of copper atoms? 1.23 The velocity of an electron that is emitted from a metallic surface by a photon is 3.6 X 103 km-s1 (a) What is the wavelength of the ejected electron? (b) No electrons are emitted from the surface of the metal until the frequency of the radiation reaches 2.50 x 1016 Hz. How much energy is required to remove the electron from the metal surface? (c) What is the wavelength of the radiation that caused photoejection of the electron? (d) What kind of electromagnetic radiation was used?

1.19 Sodium vapor lamps, used for public lighting, emit yellow light of wavelength 589 nm. How much energy is emitted by (a) an excited sodium atom when it generates a photon; (b) 5.00 mg of sodium atoms emitting light at this wavelength; (c) 1.00 mol of sodium atoms emitting light at this wavelength? 1.20 When an electron beam strikes a block of copper, x-rays with a frequency of 1.2 x 1017 Hz are emitted. How much energy is emitted at this wavelength by (a) an excited copper atom when it generates an x-ray photon; (b) 2.00 mol of excited copper atoms (c) 2.00 g of copper atoms? 1.23 The velocity of an electron that is emitted from a metallic surface by a photon is 3.6 X 103 km-s1 (a) What is the wavelength of the ejected electron? (b) No electrons are emitted from the surface of the metal until the frequency of the radiation reaches 2.50 x 1016 Hz. How much energy is required to remove the electron from the metal surface? (c) What is the wavelength of the radiation that caused photoejection of the electron? (d) What kind of electromagnetic radiation was used?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes a transition from level n= 6 to n= 1? What is the wavelength of light emitted when the electron in a hydrogen atom undergoes a transition from level n= 6 to n= 1? (c=3.00×108 m/s, h=6.63×10−34 J⋅s, RH=2.179×10−18 J)(c=3.00×108 m/s, h=6.63×10−34 J·s, RH=2.179×10−18 J) Select one: a. 144.8 nm b. 982 nm c. 93.7 nm d. 239 nm
In Einstein's photoelectric experiment, the kinetic energy of an electron displaced from a metal by a photon was the difference between the energy of a photon and a threshold energy value for the metal. If you were to perform a similar experiment with cobalt, which has a threshold energy of 8.01 × 10⁻¹⁹ J, and ultraviolet light of wavelength 29.5 nm, what would be the kinetic energy (in J) of the electron displaced?
A certain shade of blue has a frequency of 7.28×1014 Hz.7.28×1014 Hz. What is the energy of exactly one photon of this light? Planck's constant is ℎ=6.626×10−34 J⋅s.
For photons with the following energies, calculate the wavelength and identify the region of the spectrum they are from: (a) 3.5 x 10−20 J, (b) 8.7 x 10−26 J, (c) 7.1 x 10−17 J, (d) 5.5 x 10−27 J
2. A laser pointer used in the classroom emits light at 6550 A, at a power of 4.00 mW. (One watt is the SI unit of power, the measure of energy per unit of time. 1 W = 1 J/s). How many photons are emitted from the pointer in 115 seconds?
The scattering of sunlight by the mixture of gas molecules in air results in the blue color of the sky. Calculate the energy (in Joules) of a single photon of blue light with a frequency of 7.50 × 1014 Hz. (h = 6.626 x 10-34 J•s) |x 10 49 J 2 3 4 5 C 7 8. +/- х 100
3. (i) Define the term photon. Then, (ii) state whether a photon of blue light or red light has higher energy and (iii) explain how you made your determination. Be sure to (iv) include an equation that can justify your answer.
Microwave ovens heat food by the energy given off by microwaves. These microwaves have a wavelength of 5.00 3 106 nm. (a) How much energy in kilojoules per mole is given off by a microwave oven? (b) Compare the energy obtained in (a) with that given off by the ultraviolet rays (l <100 nm) of the Sun that you absorb when you try to get a tan.
The scattering of sunlight by the mixture of gas molecules in air results in the blue color of the sky. Calculate the energy (in Joules) of a single photon of blue light with a frequency of 6.30 × 10¹⁴ Hz. (h = 6.626 × 10⁻³⁴ J • s)
The scattering of sunlight by the mixture of gas molecules in air results in the blue color of the sky. Calculate the energy (in Joules) of a single photon of blue light with a frequency of 7.20 × 10¹⁴ Hz. (h = 6.626 × 10⁻³⁴ J • s)
The scattering of sunlight by the mixture of gas molecules in air results in the blue color of the sky. Calculate the energy (in Joules) of a single photon of blue light with a frequency of 6.70 × 1014 Hz. (h = 6.626 × 1034 J•s)
5. The human eye can detect as little as 2.5*10-¹6 joules of light. How many photons of green (510nm) light can your eye detect? How many photons of red (620nm) light can your eye detect? 6. An unknown metal sample is interrogated using a beam of X-rays to liberate electrons which are then caught by a detector that determines their kinetic energy. A beam of X-rays with wavelength 9.54nm irradiate the surface of this metal, and the detector observes electrons with kinetic energies equal to 7.3716*10 J. What is the binding energy of this unknown metal sample.