PRE-LABORATORY ASSIGNMENTThe pre-laboratory assignment must be completed before beginning the laboratory experiment.1.Wave, light, and energy emission in atoms:Given the speed of sound as 343.2 m/s, calculate the frequency of a sound wave of wavelength 15 m.a.b.The wavelength of emission from a sodium atom is 589.3 nm. What flame color would you expectfor sodium? Explain.c. Mercury has an emission wavelength of 454 nm from the relaxation of an excited state to a lowerenergy state. Predict the color of this emission.

The question is based on the concept of atomic spectra. we have been given speed of light and…

PRE-LABORATORY ASSIGNMENT The pre-laboratory assignment must be completed before beginning the laboratory experiment. 1. Wave, light, and energy emission in atoms: a. Given the speed of sound as 343.2 m/s, calculate the frequency of a sound wave of wavelength 15 m. b. The wavelength of emission from a sodium atom is 589.3 nm. What flame color would you expect for sodium? Explain. c. Mercury has an emission wavelength of 454 nm from the relaxation of an excited state to a lower energy state. Predict the color of this emission.

PRE-LABORATORY ASSIGNMENT The pre-laboratory assignment must be completed before beginning the laboratory experiment. 1. Wave, light, and energy emission in atoms: a. Given the speed of sound as 343.2 m/s, calculate the frequency of a sound wave of wavelength 15 m. b. The wavelength of emission from a sodium atom is 589.3 nm. What flame color would you expect for sodium? Explain. c. Mercury has an emission wavelength of 454 nm from the relaxation of an excited state to a lower energy state. Predict the color of this emission.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 21ALQ

See similar textbooks

Similar questions

Explain the hydrogen emission spectrum. Why is it significant that the calm emitted is not while? How does the emission spectrum support the idea of quantized energy levels?
What evidence do we have that energy levels in an atom are quantized? State and explain the evidence.
Scientists use emission spectra to confirm the presence of an element in materials of unknown composition. Why is this possible?
(a) Give the complete electron configuration (1s22s22p) of aluminum in the ground state. (b) The wavelength of the radiation emitted when the outermost electron of aluminum falls from the 4s state to the ground state is about 395 nm. Calculate the energy separation (in joules) between these two states in the Al atom. (c) When the outermost electron in aluminum falls from the 3d state to the ground state, the radiation emitted has a wavelength of about 310 nm. Draw an energylevel diagram of the states and transitions discussed here and in (b). Calculate the separation (in joules) between the 3d and 4s states in aluminum. Indicate clearly which has higher energy.
A photon with a wavelength of 93.8 nm strikes a hydrogen atom, and light is emitted by the atom. How many emission lines would be observed? At what wavelengths? Explain briefly (see Figure 6.10).
Consider the orbitals shown here in outline. (a) What is the maximum number of electrons contained in an orbital of type (x)? Of type (y)? Of type (z)? (b) How many orbitals of type (x) are found in a shell with n=2? How many of type (y)? How many of type (z)? (c) Write a set of quantum numbers for an electron in an orbital of type (x) in a shell with n=4, of an orbital of type (y) in a shell with n=2. Of an orbital of type (z) in a shell with n=3. (d) What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z)? (e) What are the possible I and ml values for an orbital of type (x)? Of type (y)? Of type (z)?
Consider the transition from the energy levels n=2 to n=5. (a) What is the wavelength associated with this transition? (b) In what spectral region does the transition occur? (c) Is energy absorbed?
Give a brief wave description of light. What are two characteristics of light waves?
In the photoelectric effect, electrons are ejected from a metal surface when light strikes it. A certain minimum energy, Emin, is required to eject an electron. Any energy absorbed beyond that minimum gives kinetic energy to the electron. It is found that when light at a wavelength of 540 nm falls on a cesium surface, an electron is ejected with a kinetic energy of 2.601020J. When the wavelength is 400 nm, the kinetic energy is 1.541019J. (a) Calculate Emin for cesium in joules. (b) Calculate the longest wavelength, in nanometers, that will eject electrons from cesium.
When a tube containing hydrogen atoms is energized by passing several thousand volts of electricity into the tube, the hydrogen emits light than when passed through a prism, resolves into the "bright line" spectrum shown in Fig. 11.10. Why do hydrogen atoms emit bright lines of specific wavelengths rather than a continuous spectrum?
Answer the following questions: (a) Without using quantum numbers, describe the differences between the shells, subshells, and orbitals of an atom. (b) How do the quantum numbers of the shells, subshells, and orbitals of an atom differ?
Explain electron from a quantum mechanical perspective, including a discussion of atomic radii, probabilities, and orbitals.