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Chapter 6: Q35 E (page 277)

Identify the subshell in which electrons with the following quantum numbers are found:

(a)n= 2,l= 1

(b)n= 4,l= 2

(c)n= 6,l= 0

Short Answer

Expert verified

(a) 2p

(b) 4d

(c) 6s

Step by step solution

01

describing how to identify a subshell

N represents the first value of the subshell. Quantum number l represents the shape of orbitals.

l = 0 represents s-shaped orbital

l = 1 represents p shaped orbital

l = 2 represents d shaped orbital

l = 3 represents f shaped orbitals

02

determining the subshells in which electrons with the following quantum numbers are found

  1. For n = 2, l = 1

L =1 corresponds to p shaped orbital. hence, subshell = 2p

  1. For n = 4, l = 2

L = 2 corresponds to d shaped orbital. Hence, subshell = 4d

  1. For n = 6, l = 0

L = 0 corresponds to s-shaped orbital. Hence, subshell = 6s

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Most popular questions from this chapter

Question:Cobalt鈥�60 and iodine鈥�131 are radioactive isotopes commonly used in nuclear medicine. How many protons,neutrons, and electrons are in atoms of these isotopes? Write the complete electron configuration for each isotope.

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Question:Which of the subshells described in the previous question contain degenerate orbitals? How many degenerateorbitals are in each?

Question:Use an orbital diagram to describe the electron configuration of the valence shell of each of the following

atoms:

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