ErwinSchrödingerSolution of the Schrödinger wave equation for the hydrogen atom results in a set of functions (orbitals) thatdescribe the behavior of the electron.Each function is characterized by 3 quantum numbers: n, I, and m,n is known as theI is known as them, is known as then specifies / specifies my specifies0quantum number.quantum number.quantum number.A.The subshell-orbital shape.B.The energy and average distance from the nucleus.C.The orbital orientation.

The quantum numbers are the set of four numbers that describe the position and energy of electrons…

Erwin Schrödinger Solution of the Schrödinger wave equation for the hydrogen atom results in a set of functions (orbitals) that describe the behavior of the electron. Each function is characterized by 3 quantum numbers: n, I, and m, In is known as the I is known as the m, is known as the n specifies / specifies m/ specifies quantum number. quantum number. quantum number. A.The subshell-orbital shape. B.The energy and average distance from the nucleus. C.The orbital orientation.

Erwin Schrödinger Solution of the Schrödinger wave equation for the hydrogen atom results in a set of functions (orbitals) that describe the behavior of the electron. Each function is characterized by 3 quantum numbers: n, I, and m, In is known as the I is known as the m, is known as the n specifies / specifies m/ specifies quantum number. quantum number. quantum number. A.The subshell-orbital shape. B.The energy and average distance from the nucleus. C.The orbital orientation.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter9: Pre-quantum Mechanics

Section: Chapter Questions

Problem 9.16E: Some scientists study Rydberg atoms, atoms whose electron has a large value of the n quantum number....

See similar textbooks

Similar questions

In the Stern-Gerlach experiment, silver atoms were used. This was a good choice, as it turned out. Using the electron configuration of silver atoms, explain why silver was a good candidate for being able to observe the intrinsic angular momentum of the electron. Hint: Dont use the aufbau principle to determine the electron configuration of Ag, because its one of the exceptions. Look up the exact electron configuration in a table.
What is the probability of finding an electron in the 1s orbital within 0.1A of an Ne9+ nucleus? Compare your answer to the answer to exercise 11.77 and justify the difference.
A 25-kg child is on a merry-go-round/calliope, going around and around in a large circle that has a radius of 8meters. The child has an angular momentum of 600kgm2/s. a From these facts, estimate the approximate quantum number for the angular momentum the child has. b Estimate the quantized amount of energy the child has in this situation. How does this compare to the childs classical energy? What principle does this illustrate?
Consider a one-dimensional particle-in-a-box and a three-dimensional particle-in-a-box that have the same dimensions. a What is the ratio of the energies of a particle having the lowest possible quantum numbers in both boxes? b Does this ratio stay the same if the quantum numbers are not the lowest possible values?
a For a pendulum having classical frequency of 1.00s1, what is the energy difference in J between quantized energy levels? b Calculate the wavelength of light that must be absorbed in order for the pendulum to go from one level to another. c Can you determine in what region of the electromagnetic spectrum such a wavelength belongs? d Comment on your results for parts a and b based on your knowledge of the state of science in early twentieth century. Why wasnt the quantum mechanical behavior of nature noticed?
For the Li atom, the energy difference between the ground state and the first excited state, in which the outermost electron is in a 2p orbital, is 2.961019J . In the Li2+ ion, the energy difference between the 2s and 2p levels is less than 0.00002 of this value. Explain this observation.
In exercise 11.57 regarding C60, what are the numerical values of the total angular momenta of the electron for each state having quantum number l? What are the z components of the angular momentum for each state?
The helium ion He+ is a one-electron system whose wave functions and energy levels are obtained from those for H by changing the atomic number to Z=2 . Calculate the average distance of the electron from the nucleus in the 2s orbital and in the 2p orbital. Compare your results with those in Problem 11 and explain the difference.
Using Table 5.2, write down the mathematical expression for the 2px wave function for an electronically excited H atom. Estimate the probability of finding the 2px electron if you look in a cubical box of volume of 0.8(pm)3 centered at a distance of 0.5001010m in the =/2 , =0 direction. Does this probability change as you change ? At what angles is the probability of finding the electron smallest and at what angles is the probability the largest? (Note that =2 is the same location as =0 , so don’t double count.)
Why does the wavefunction 4,4,0 not exist? Similarly, why does a 3f subshell not exist? See exercise 11.73 for notation definition.
What are the values of E, L, and Lz for an F8+ atom whose electron has the following wavefunctions, listed as n,l,ml? a 1,0,0 b 3,2,2c 2,1,1d 9,6,3.
Is the spin orbital 1s for the H atom still spherically symmetric? Explain your answer.