General Chemistry 4th EditionMcQuarrie Rock GalloglyWrite the ground state electron configuration of B using the noble-gas shorthand notation.electron configuration:ANOVUniversity Science Bocpresented by Macmillan LearQuestion Source: McQuarrie, Rock, And Gallogly 4e-General ChemistryZAtv NallHePublisher: UniversWD C

Answered: Image /qna-images/answer/69206a0b-3fd7-4a94-88dd-77b08484d9aa.jpg

General Chemistry 4th Edition McQuarrie Rock Gallogly Write the ground state electron configuration of B using the noble-gas shorthand notation. electron configuration: C NOV University Science Boc presented by Macmillan Lear Question Source: McQuarrie, Rock, And Gallogly 4e-General Chemistry tv Nall He Publisher: Univers WD C

General Chemistry 4th Edition McQuarrie Rock Gallogly Write the ground state electron configuration of B using the noble-gas shorthand notation. electron configuration: C NOV University Science Boc presented by Macmillan Lear Question Source: McQuarrie, Rock, And Gallogly 4e-General Chemistry tv Nall He Publisher: Univers WD C

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 139QRT

See similar textbooks

Similar questions

Section 11.6 uses a "firefly" analogy to illustrate how the wave mechanical modal for the atom differs from Bohr’s. model. Explain this analogy.
Construct an energy level diagram showing all orbitals for the hydrogen atom up to n=5, labeling each orbital with its appropriate quantum numbers. How many different orbitals are in each shell?
Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital (as described by the more modern, wave mechanical picture of the atom).
Atoms of which group in the periodic table have a valence shell electron configuration of ns2?
Photoelectron spectroscopy studies have determined the orbital energies for fluorine atoms to be 1s689eV2s34eV2p12eV Estimate the value of Zeff for F in each of these orbitals.
What does wave-particle duality mean? What are its implications in our modem view of atomic structure?
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 .)
The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.
When metallic sodium is dissolved in liquid sodium chloride, electrons are released into the liquid. These dissolved electrons absorb light with a wavelength near 800 nm. Suppose we treat the positive ions surrounding an electron crudely as defining a three-dimensional cubic box of edge L, and we assume that the absorbed light excites the electron from its ground state to the first excited state. Calculate the edge length L in this simple model.
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.
Both the electron affinity and the ionization energy of chlorine are higher than the corresponding quantities for sulfur. Explain why in terms of the electronic structure of the atoms.
Until recently, it was thought that Ca was unstable, and that the Ca atom therefore had a negative electron affinity. Some new experiments have now measured an electron affinity of +2.0kJmol1 for calcium. What is the longest wavelength of light that could remove an electron from Ca ? In which region of the electromagnetic spectrum does this light fall?