Physics, Books a la Carte Edition (5th Edition)
5th Edition
ISBN: 9780134020853
Author: James S. Walker
Publisher: PEARSON
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Chapter 31, Problem 13PCE
To determine
The order of increasing energy for given substances.
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Consider the Bohr model as applied to the following threeatoms: (A) neutral hydrogen in the state n = 2; (B) singly ionizedhelium in the state n = 1; (C) doubly ionized lithium in the staten = 3. Rank these three atoms in order of increasing Bohr radius.Indicate ties where appropriate.
Consider the Bohr model as applied to the following
three atoms:
(A) neutral hydrogen in the state n = 2;
(B) singly ionized helium in the state n = 1;
(C) doubly ionized lithium in the state n = 3.
Part A
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Rank these three atoms in order of decreasing orbital radius.
Rank atoms from largest to smallest Bohr radius. To rank items as equivalent, overlap
them.
Largest
P Pearson
atom A
atom B
atom C
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Smallest
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An electron in the hydrogen atom is in the 4s state.
(a) Find the orbital angular momentum of the electron (in units of h).
(b) Find the energy of the electron (in eV).
(c) Ignoring electron spin, find the total number of quantum states that have this same
energy.
(d) Make a table listing the uantum numbers n, I, and ms of each of the degenerate states.
Indicate the spectroscopic label (e.g. 1s, 2s, etc) that would apply to each state.
Chapter 31 Solutions
Physics, Books a la Carte Edition (5th Edition)
Ch. 31.1 - Prob. 1EYUCh. 31.2 - Prob. 2EYUCh. 31.3 - Prob. 3EYUCh. 31.4 - Prob. 4EYUCh. 31.5 - Prob. 5EYUCh. 31.6 - Prob. 6EYUCh. 31.7 - Prob. 7EYUCh. 31 - Prob. 1CQCh. 31 - Prob. 2CQCh. 31 - Prob. 3CQ
Ch. 31 - Prob. 4CQCh. 31 - Prob. 5CQCh. 31 - Prob. 6CQCh. 31 - Prob. 7CQCh. 31 - Prob. 8CQCh. 31 - Prob. 9CQCh. 31 - Prob. 1PCECh. 31 - Prob. 2PCECh. 31 - Prob. 3PCECh. 31 - Prob. 4PCECh. 31 - Prob. 5PCECh. 31 - Prob. 6PCECh. 31 - Prob. 7PCECh. 31 - Prob. 8PCECh. 31 - Prob. 9PCECh. 31 - Prob. 10PCECh. 31 - Prob. 11PCECh. 31 - Prob. 12PCECh. 31 - Prob. 13PCECh. 31 - Prob. 14PCECh. 31 - Prob. 15PCECh. 31 - Prob. 16PCECh. 31 - Prob. 17PCECh. 31 - Prob. 18PCECh. 31 - Prob. 19PCECh. 31 - Prob. 20PCECh. 31 - Prob. 21PCECh. 31 - Prob. 22PCECh. 31 - Prob. 23PCECh. 31 - Prob. 24PCECh. 31 - Prob. 25PCECh. 31 - Prob. 26PCECh. 31 - Prob. 27PCECh. 31 - Prob. 28PCECh. 31 - Prob. 29PCECh. 31 - Prob. 30PCECh. 31 - Prob. 31PCECh. 31 - Prob. 32PCECh. 31 - Prob. 33PCECh. 31 - Prob. 34PCECh. 31 - Prob. 35PCECh. 31 - Prob. 36PCECh. 31 - Prob. 37PCECh. 31 - Prob. 38PCECh. 31 - Prob. 39PCECh. 31 - Prob. 40PCECh. 31 - Prob. 41PCECh. 31 - Prob. 42PCECh. 31 - Prob. 43PCECh. 31 - Prob. 44PCECh. 31 - Prob. 45PCECh. 31 - Prob. 46PCECh. 31 - Prob. 47PCECh. 31 - Prob. 48PCECh. 31 - Prob. 49PCECh. 31 - Prob. 50PCECh. 31 - Prob. 51PCECh. 31 - Prob. 52PCECh. 31 - Give the electronic configuration for the ground...Ch. 31 - Prob. 54PCECh. 31 - Prob. 55PCECh. 31 - Prob. 56PCECh. 31 - The configuration of the outer electrons in Ni is...Ch. 31 - Prob. 58PCECh. 31 - Prob. 59PCECh. 31 - Prob. 60PCECh. 31 - Prob. 61PCECh. 31 - Prob. 62PCECh. 31 - Prob. 63PCECh. 31 - Prob. 64PCECh. 31 - Prob. 65PCECh. 31 - Prob. 66PCECh. 31 - Prob. 67PCECh. 31 - Prob. 68GPCh. 31 - Prob. 69GPCh. 31 - Prob. 70GPCh. 31 - Prob. 71GPCh. 31 - Prob. 72GPCh. 31 - Prob. 73GPCh. 31 - Prob. 74GPCh. 31 - Prob. 75GPCh. 31 - Prob. 76GPCh. 31 - Prob. 77GPCh. 31 - Prob. 78GPCh. 31 - Prob. 79GPCh. 31 - Prob. 80GPCh. 31 - Prob. 81GPCh. 31 - Prob. 82GPCh. 31 - Prob. 83GPCh. 31 - Prob. 84PPCh. 31 - Prob. 85PPCh. 31 - Prob. 86PPCh. 31 - Prob. 87PPCh. 31 - Prob. 88PPCh. 31 - Prob. 89PP
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- (a.) The figure below representing the lowest energy levels of the electron in the hydrogen atom, gives the principal quantum number n associated with each, and the corresponding value of the energy, measured in joules. (i.) Calculate the wavelength of the lines arising from the transitions márk A, B, C, D on the figure.(ii.) Show that the other transitions that can occur give rise to lines which are in either the ultraviolet or the infrared regions of the spectrum.(iii.) The level n = 1 is the ground state of the excited hydrogen atom. Explain why hydrogen in its ground state is quite transparent to light emitted by the transition A, B, C, D and also what happens when 21.7 × 10-19 J of energy is supplied to a hydrogen atom in its ground state.arrow_forwardThe energy E of the electron in a hydrogen atom can be calculated from the Bohr formula: R 23 n² E In this equation R, stands for the Rydberg energy, and 12 stands for the principal quantum number of the orbital that holds the electron. (You can find the value of the Rydberg energy using the Data button on the ALEKS toolbar.). Calculate the wavelength of the line in the absorption line spectrum of hydrogen caused by the transition of the electron from an orbital with n=5 to an orbital with n=9. Round your answer to 3 significant digits. 0 Line X Sarrow_forwardPlease only type answerarrow_forward
- Answer of the question immediately pleasearrow_forwardPlease answer (i), (v), and (vi). Thank you! (i) Using Bohr model for atomic hydrogen, obtain energy levels for the 2s, 3s and 3p states in the actual number with the unit of [eV]. We consider a transition that electron in the 3p state emits a photon and make a transition to the 2s state. What is the frequency v of this photon ? (ii) Now we do not include electron spin angular momentum, and just estimate an effect of a magnetic field B on this transition (Normal Zeeman effect) with orbital angular momentum. How many lines of optical transition do we expect ? What is the interval of the frequency in the field B = 0.1 Tesla ? (iii) In this situation, we do not expect transition from 3s to 2s state if the electron is initially in the 3s state, Explain the reason. (iv) We now consider an effect of magnetic field B to a free electron spin (not in Hydrogen, but a free electron). The magnetic field of B = 1.0 Tesla will split the energy level into two (Zeeman) levels. Obtain the level…arrow_forwardThe following image is an energy level diagram for a simple atom, where E1 0.00 ev, E2 = 1.34 ev, and E3 3.95 ev. %3D n=3 E3=? n=2 E,=? n=1 - Ez=? What wavelengths appear in the atom's emission spectrum? (Enter your wavelengths in the order of smallest to largest.) 3.14x10-7 m 4.75×10-7 m 9.25x10-7 m You are correct. Your receipt no. is 162-5156 ? Previous Tries What wavelengths appear in the atom's absorption spectrum? (Enter your wavelengths in the order of smallest to largest.)arrow_forward
- Consider a hydrogen atom in its 1s state (ground state) and assume (for simplicity) that the electron and the proton are separated by a constant distance a, = 5.292 × 10–1'm (called the Bohr radius). (a) Calculate the gravitational force between these two charges. (use: Fg = G"m2) (b) Calculate the electric force between these two charges. (use: Fe = k«l&i[IQzl) (c) Calculate the ratio of these two forces to appreciate the strength of the electric force in comparison to the gravitational force.arrow_forwardConsider the Bohr model of the atom. Suppose an electron in a hydrogen atom transitions from the n=3 level to the n=5 level. 1) CALCULATE the energy (ΔE) for this transition. 2) Does this transition involve the absorption or emission of a photon of light? How do you know?arrow_forwardAn electron is in the nth Bohr orbit of the hydrogen atom. (a) Show that the period of the electron is T = n3t0 and determine the numerical value of t0. (b) On average, an electron remains in the n = 2 orbit for approximately 10 ms before it jumps down to the n = 1 (ground-state) orbit. How many revolutions does the electron make in the excited state? (c) Define the period of one revolution as an electron year, analogous to an Earth year being the period of the Earth’s motion around the Sun. Explain whether we should think of the electron in the n = 2 orbit as “living for a long time.”arrow_forward
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