a) Write an acceptable value for the missing quantum numbers in the following set and identify the corresponding atomic orbital n= ?, e 3, me ?, m, = ½ b) How many different orbitals in an atom can have the principal quantum number n = 4? List the names of corresponding subshells. c) What is the maximum number of electrons that can have the following set of quantum numbers? Explain your reasoning. n= 3, e 1, m,- -½ d) Provide a set of 4 quantum numbers for an unpaired electron in a ground state rhenium (Re) atom. Identify the atomic orbital

a) Write an acceptable value for the missing quantum numbers in the following set and identify the corresponding atomic orbital n= ?, e 3, me ?, m, = ½ b) How many different orbitals in an atom can have the principal quantum number n = 4? List the names of corresponding subshells. c) What is the maximum number of electrons that can have the following set of quantum numbers? Explain your reasoning. n= 3, e 1, m,- -½ d) Provide a set of 4 quantum numbers for an unpaired electron in a ground state rhenium (Re) atom. Identify the atomic orbital

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

See similar textbooks

Similar questions

State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f, 4f, and 5s. Briefly explain your answers.
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?
Write a complete set of quantum numbers (n, , m) that quantum theory allows for each of the following orbitals: (a) 2p, (b) 3d, and (c) 4f.
What experimental evidence supports the quantum theory of light? Explain the wave-particle duality of all matter .. For what size particles must one consider both the wave and the particle properties?
What are quantum numbers? What information do we get from the quantum numbers n, l, and ml? We define a spin quantum number (ms), but do we know that an electron literally spins?
6.96 When a helium atom absorbs light at 58.44 nm, an electron is promoted from the 1s orbital to a 2p orbital. Given that the ionization energy of (ground state) helium is 2372 kJ/ mol, find the longest wavelength of light that could eject an electron from the excited state helium atom.
Which of the following sets of quantum numbers correctly represents a 4p orbital? (a) n = 4, = 0, m = 1 (b) n = 4, = 1, m = 0 (c) n = 4, = 2, m = 1 (d) n = 4, = 1, m =2
What is the maximum number of orbitals that can be identified by each of the following sets of quantum numbers? When none is the correct answer, explain your reasoning. (a) n = 3, = 0, m = +1 (b) n = 5, = 1, (c) n = 7, = 5, (d) n = 4, = 2, m = 2
What is the maximum number of electrons that can occupy a f subshell (l = 3)?
Answer the following questions. (a) What characteristic of an atomic orbital does the quantum number ms describe? (b) Does a photon with a frequency of 35.8 Hz have more or less energy than one with a frequency of 125 Hz? (c) How many orbitals can be associated with the following set of quantum numbers:n=3, l=2? (d) Is a sample of ZnCl2 containing the Zn2+ ion diamagnetic?
How do 2p orbitals differ from each other? How do 2p and 3p orbitals differ from each other? What is a nodal surface in an atomic orbital? What is wrong with lp, ld, 2d, lf, 2f, and 3f orbitals? Explain what we mean when we say that a 4s electron is more penetrating than a 3d electron.
The most prominent line in the emission spectrum of aluminum is at 396.15nm. What is the frequency of this line? What is the energy of one photon with this wavelength? Of 1.00 mol of these photons?