3. Which scientist is responsible for the rule that says one electron must be loaded into each degenerate orbital before they can be paired up? a. Bohr b. Aufbau c. Pauli d. Hund 4. An electron orbital can best be defined as: a. A ring around which an electron circles the nucleus, much like a planet orbiting the sun. b. The outermost boundary within which you can find an electron. c. A space where the exact location and speed of an electron can be determined. d. The region of 3-dimensional space where the probability of locating an electron is high.

3. Which scientist is responsible for the rule that says one electron must be loaded into each degenerate orbital before they can be paired up? a. Bohr b. Aufbau c. Pauli d. Hund 4. An electron orbital can best be defined as: a. A ring around which an electron circles the nucleus, much like a planet orbiting the sun. b. The outermost boundary within which you can find an electron. c. A space where the exact location and speed of an electron can be determined. d. The region of 3-dimensional space where the probability of locating an electron is high.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter7: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 29Q: The Bohr model works for only one electron species. Why do we discuss it in this text (what's good...

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Similar questions

The Bohr model works for only one electron species. Why do we discuss it in this text (what's good about it)?
Why was Bohr's theory for the hydrogen atom initially accepted, and why was it ultimately discarded?
Your text describes the probability map for an s orbital using an analogy to the earth’s atmosphere. Explain this analogy.
Which statement is true of the quantum mechanical model, but not of the Bohr model? a. Electrons orbit the nucleus in simple circular orbits, just like planets orbit the Sun. b. The exact path that an electron follows within an atom cannot be specified. c. The electron is attracted to the nucleus of the atom.
The Energy levels of hydrogen (and other atoms) are , which means that only certain values of energy are allowed.
Consider the orbitals shown here in outline. (a) What is the maximum number of electrons contained in an orbital of type (x)? Of type (y)? Of type (z)? (b) How many orbitals of type (x) are found in a shell with n=2? How many of type (y)? How many of type (z)? (c) Write a set of quantum numbers for an electron in an orbital of type (x) in a shell with n=4, of an orbital of type (y) in a shell with n=2. Of an orbital of type (z) in a shell with n=3. (d) What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z)? (e) What are the possible I and ml values for an orbital of type (x)? Of type (y)? Of type (z)?
Defend and criticize Bohrs model. Why was it reasonable that such a model was proposed, and what evidence was there that it "works"? Why do we no longer "believe" in it?
• rank various orbitals in terms of size and energy.
Suppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?
Which orbital is the first be filled in any atom? Why?
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.
How does the 3dxy orbital of an electron in O7+ resemble the 3dxy orbital of an electron in a hydrogen atom? How does it differ?