Reviewormation about an electron's probablebe represented by an electron-densityan orbital. An orbital is characterizedtation in space.Part AWhat is the angular-momentum quantum number (also called the azimuthal quantum number), l, for the orbital shown here?Express your answer numerically as an integer.View Available Hint(s)l=SubmitPart BVCompare the orbital shown in Parts A to the orbital shown here in size, shape, and orientation. Part BCompare the orbital shown in Parts A to the orbital shown here in size, shape, and orientationZхWhich quantum number(s) would be different for these two orbitals?View Available Hint(s)n onlyl onlyme onlyl and meп, е, and me

The azimuthal quantum numbers for different orbitals are given below.s-orbital ------>…

Answered: Review ormation about an electron's…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 135QRT

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How does probability fit into the description of the atom?
The energies of macroscopic objects, as well as those of microscopic objects, are quantized, but the effects of the quantization are not seen because the difference in energy between adjacent states is so small. Apply Bohr’s quantization of angular momentum to the revolution of Earth (mass6.01024kg) , which moves with a speed of 3.0104ms1 in a circular orbit (radius1.51011m) about the sun. The sun can be treated as fixed. Calculate the value of the quantum number n for the present state of the Earthsun system. What would be the effect of an increase in n by 1?
Quantum mechanics predicts that the energy of the ground state of the H atom is 13.6eV . Insight into the magnitude of this quantity is gained by considering several methods by which it can be measured. (a) Calculate the longest wavelength of light that will ionize H atoms in their ground state. (b) Assume the atom is ionized by collision with an electron that transfers all its kinetic energy to the atom in the ionization process. Calculate the speed of the electron before the collision. Express your answer in meters per second (ms1) and miles per hour (milesh1) . (c) Calculate the temperature required to ionize a H atom in its ground state by thermal excitation. (Hint: Recall the criterion for thermal excitation of an oscillator in Planck’s theory of blackbody radiation is that hvkBT .)
Use the mathematical expression for the 2pz wave function of a one-electron atom (see Table 5.2) to show that the probability of finding an electron in that orbital anywhere in the x-y plane is 0. What are the nodal planes for a dxz orbital and for a dx2y2 orbital?
The cesium atom has the lowest ionization energy, 375.7kJmol1 , of all the neutral atoms in the periodic table. What is the longest wavelength of light that could ionize a cesium atom? In which region of the electromagnetic spectrum does this light fall?
6.32 What are the mathematical origins of quantum numbers?
The ionization of the hydrogen atom can be calculated from Bohr's equation for the electron energy. E = (NARhc)(Z2/n2) where NARhc =1312 kJ/mol and Z is the atomic number. Let us use this approach to calculate a possible ionization energy for helium. First, assume the electrons of the He experience the full 2+ nuclear charge. This gives us the upper limit for the ionization energy. Next, assume one electron of He completely screens the nuclear charge from the other electrons, so Z = 1. This gives us a lower limit to the ionization energy. Compare these calculated values for the upper and lower limits to the experimental value of 2372.3 kJ/mol. What does this tell us about the ability of one electron to screen the nuclear charge?
6.106 When Bohr devised his model for the atom, was he using deductive or inductive reasoning? Explain your answer.
Using Fig. 2-30, list the elements (ignore the lanthanides and actinides) that have ground-state electron configurations that differ from those we would expect from their positions in the periodic table.
Use the aufbau procedure to obtain the electron configuration and orbital diagram for atoms of the following elements. (a) Be (b) B (c) Ne (d) Rb
Imagine a world in which the rule for the l quantum number is that values start with 1 and go up to n. The rules for the n and mi quantum numbers are unchanged from those of our world. Write the quantum numbers for the first two shells (i.e., n = 1 and n = 2).

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