List the four possible subshells in the quantum-mechanical model.

CHEM& 140 – Checkpoint 8 – Show It HW Name ________________________________ Section ___

The notation at the beginning of each problem refers to the location of the problem in the textbook (6th edition of Introductory Chemistry by Tro). Most odd-numbered problems have answers in the back of the book.

1. (CH9 #15) Explain the difference between a Bohr orbit and a quantum-mechanical orbital.

2. (CH9 #18) Why do quantum-mechanical orbitals have “fuzzy” boundaries?

3. Describe/summarize/show how the pattern of the Periodic Table can be used to figure out the order that the atomic orbitals get filled instead of having to memorize the order.

4. What do the terms shell and subshell refer to and how are they related?

5. (CH9 #19) For the four possible subshells in the quantum-mechanical model, list the number of orbitals in each subshell, and the maximum number of electrons that can be contained in each subshell.

6. (CH9 #44) Sketch the shapes of the 3d orbitals. How do the 4d orbitals differ from the 3d orbitals?

7. Do page 128 in the Workbook. Insert a photo of your answer for Fe (or draw it here). Circle the unpaired electrons in the orbital diagram for Fe and state the total number of unpaired electrons in a Fe atom.

Box and whisker chart Description automatically generated

8. For Se (element #34):

· Draw an orbital energy diagram for Se (element #34).

(In an orbital energy diagram, you draw the orbitals vertically in order of increasing E.)

· In your diagram above, circle the orbitals that contain the valence electrons. (Recall that the outermost electrons are found in the highest shell, n.) How many valence electrons does an atom of Se have?

· How many electrons would need to be added to a Se atom to fill these orbitals in the valence shell? (How many more electrons to fill the orbitals in the 4p subshell?)

9. Review page 129 of the Workbook. From page 130 of the Workbook:

· Write full electron configurations for barium (#56) and for lead (#82).

· Write abbreviated electron configurations for barium (#56) and lead (#82) using a noble gas core. (Use the symbol of the previous noble gas in brackets, then continue the electron configuration from that point on.)

10. Do page 131 of the Workbook. Insert your work for #4. If an electron configuration is not valid for an element, fix the error(s) while keeping the total number of electrons the same.

Table Description automatically generated

Applied Sciences

Architecture and Design

Biology

Business & Finance

Chemistry

Computer Science

Geography

Geology

Education

Engineering

English

Environmental science

Spanish

Government

History

Human Resource Management

Information Systems

Law

Literature

Mathematics

Nursing

Physics

Political Science

Psychology

Reading

Science

Social Science

Home

Blog

Archive

Contact

google+twitterfacebook

Copyright © 2019 HomeworkMarket.com