Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Chapter 15, Problem 15.21E
Interpretation Introduction
Interpretation:
The term symbol of the
Concept introduction:
A term symbol describes the orbital, spin, and total angular momenta of an electronic state. The symbol
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Chapter 15 Solutions
Physical Chemistry
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- Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a length near 1.34 Å. The motion of an electron in such a bond can be treated crudely as motion in a one-dimensional box. Calculate the energy of an electron in each of its three lowest allowed states if it is confined to move in a one-dimensional box of length 1.34 Å. Calculate the wavelength of light necessary to excite the electron from its ground state to the first excited state.arrow_forwardA hydrogen atom is immersed in a magnetic field so that its energy levels split according to the Zeeman effect. Neglecting any effects due to electron spin, how many unique energy levels are available to an electron in the 5f subshell?arrow_forwardThe nucleus of a boron-11 atom has a spin (s) quantum number of 3/2. Calculate the magnitude of the spin vector as well as the possible values it can take for the z-component of the spin vector? Is boron-11 a boson or fermion?arrow_forward
- Three of the term symbols that correspond to a nd3 electron configuration are 2P, 2F, and 4P. Rank these in terms of increasing energy.arrow_forward3- Consider the atom having the electron configuration 1s 2s2 2p 3s 3p. Assume that the z components of both the orbital and spin angular momenta of the electron in the 3p subshell are positive. What are the quantum numbers that describe the state of this electron? On=3,1= 1, m = 1, s = 1/2 n = 3,1 = 2, m = 1, s = 1/2 On= 3,1= 2, m 2, s =-1/2 On=3,13D 1, m = 2, s = 1/2 On=3,1 1, m = -1, s = 1/2 %3Darrow_forwardIndicate which of the given electronic configurations are true ground state configurations for the respective atoms and which are false. (Take care! There are some exceptions to the simple rules.) Hg [Xe]4f145d106s2 Ca 1s22s22p63s23p64s1 Cr [Ar]3d54s1 Te 1s22s22p63s23p64s23d104p64d105s25p3 Ra [Xe]4f145d106s26p6arrow_forward
- Describe the orbital approximation for the wavefunction of a many-electron atom. What are the limitations of the approximation?arrow_forwardFor a He atom in the excited state with atomic electronic configuration 1s1 2s1: write out the symmetric and antisymmetric spatial wavefunctions. These two are linear combination of ψ1s and ψ2s each with an electron in them. combine each spatial wavefunction with the appropriate spin wavefunctions for two electrons (there are four of them) such that the total wavefunction is antisymmetric.arrow_forwardSketch the boundary surface of a dx2 −y2 and a py orbital. Be sure to show and label the axes.arrow_forward
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