Chemistry
Chemistry
4th Edition
ISBN: 9780393919370
Author: Thomas R. Gilbert
Publisher: NORTON
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Chapter 7, Problem 7.88QP

(a)

Interpretation Introduction

Interpretation: The set of orbitals corresponds to each of the given sets of quantum numbers are to be stated. Also, the number of electrons occupied by these orbitals is to be stated.

Concept introduction: There are four quantum numbers that indicates the size, energy and shape of an atomic orbital. The quantum number n is the principal quantum number that indicates the energy level and size of the orbital and l is the azimuthal quantum number that determines the shape and angular momentum of an orbital. The magnetic quantum number is an integer that takes the values from (l to +l) .

To determine: The set of orbitals correspond to the given set of quantum numbers and the number of electrons occupied by these orbitals.

(a)

Expert Solution
Check Mark

Answer to Problem 7.88QP

Solution

The given set of quantum number, n=2 and l=1 represents 2p orbital and the number of electrons in 2p orbital is 6_ .

Explanation of Solution

Explanation

The given principal quantum number (n) is 2 that represents the energy level and angular momentum quantum number (l) is 1 that represents the shape of an orbital. Therefore, n=2 and l=1 represents 2p sub shell.

The sub shell 2p contains three orbitals (2px,2py,2pz) . Each orbital contains two electrons Therefore; the maximum number of electrons accommodated in p sub shell is six. Hence, the given set of quantum number, n=2 and l=1 represents 2p orbital with six electrons.

(b)

Interpretation Introduction

Interpretation: The set of orbitals corresponds to each of the given sets of quantum numbers are to be stated. Also, the number of electrons occupied by these orbitals is to be stated.

Concept introduction: There are four quantum numbers that indicates the size, energy and shape of an atomic orbital. The quantum number n is the principal quantum number that indicates the energy level and size of the orbital and l is the azimuthal quantum number that determines the shape and angular momentum of an orbital. The magnetic quantum number is an integer that takes the values from (l to +l) .

To determine: The set of orbitals correspond to the given set of quantum numbers and the number of electrons occupied by these orbitals.

(b)

Expert Solution
Check Mark

Answer to Problem 7.88QP

Solution

The given set of quantum number, n=5 and l=3 represents 5f orbital and the number of electrons in 5f orbital is 14_ .

Explanation of Solution

Explanation

The given principal quantum number (n) is 5 and angular momentum quantum number (l) is 3 that represents f sub shell. Therefore, n=5 and l=3 represents 5f sub shell.

The electrons occupied by f orbital are 14 . Hence, the given set of quantum number, n=5 and l=3 represents 5f orbital with 14 electrons.

(c)

Interpretation Introduction

Interpretation: The set of orbitals corresponds to each of the given sets of quantum numbers are to be stated. Also, the number of electrons occupied by these orbitals is to be stated.

Concept introduction: There are four quantum numbers that indicates the size, energy and shape of an atomic orbital. The quantum number n is the principal quantum number that indicates the energy level and size of the orbital and l is the azimuthal quantum number that determines the shape and angular momentum of an orbital. The magnetic quantum number is an integer that takes the values from (l to +l) .

To determine: The set of orbitals correspond to the given set of quantum numbers and the number of electrons occupied by these orbitals.

(c)

Expert Solution
Check Mark

Answer to Problem 7.88QP

Solution

The given set of quantum number, n=3 and l=2 represents 3d orbital and the number of electrons in 3d orbital is 10_ .

Explanation of Solution

Explanation

The given principal quantum number (n) is 3 and angular momentum quantum number (l) is 2 that represents d sub shell. Therefore, n=3 and l=2 represents 3d sub shell.

The sub shell 3d contains five orbitals (3dx,3dy,3dz,3dx2-y2,3dz2) . Each orbital contains two electrons Therefore; the maximum number of electrons accommodated in d sub shell is ten. Hence, the given set of quantum number, n=3 and l=2 represents 3d orbital with ten electrons.

(d)

Interpretation Introduction

Interpretation: The set of orbitals corresponds to each of the given sets of quantum numbers are to be stated. Also, the number of electrons occupied by these orbitals is to be stated.

Concept introduction: There are four quantum numbers that indicates the size, energy and shape of an atomic orbital. The quantum number n is the principal quantum number that indicates the energy level and size of the orbital and l is the azimuthal quantum number that determines the shape and angular momentum of an orbital. The magnetic quantum number is an integer that takes the values from (l to +l) .

To determine: The set of orbitals correspond to the given set of quantum numbers and the number of electrons occupied by these orbitals.

(d)

Expert Solution
Check Mark

Answer to Problem 7.88QP

Solution

The given set of quantum number, n=4 and l=3 represents 4f orbital and the number of electrons in 4f orbital is 14_ .

Explanation of Solution

Explanation

The given principal quantum number (n) is 4 and angular momentum quantum number (l) is 3 that represents f orbital. Therefore, n=4 and l=3 represents 4f sub shell.

The electrons occupied by f orbital are 14 . Hence, the given set of quantum number, n=4 and l=3 represents 4f orbital with 14 electrons.

Conclusion

  1. a. The set of quantum number, n=2 and l=1 represents 2p orbital and the number of electrons in 2p orbital is 6_ .
  2. b. The set of quantum number, n=5 and l=3 represents 5f orbital and the number of electrons in 5f orbital is 14_ .
  3. c. The set of quantum number, n=3 and l=2 represents 3d orbital and the number of electrons in 3d orbital is 10_ .
  4. d. The set of quantum number, n=4 and l=3 represents 4f orbital and the number of electrons in 4f orbital is 14_ .

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Chapter 7 Solutions

Chemistry

Ch. 7.8 - Prob. 11PECh. 7.9 - Prob. 12PECh. 7.9 - Prob. 13PECh. 7.10 - Prob. 14PECh. 7 - Prob. 7.1VPCh. 7 - Prob. 7.2VPCh. 7 - Prob. 7.3VPCh. 7 - Prob. 7.4VPCh. 7 - Prob. 7.5VPCh. 7 - Prob. 7.6VPCh. 7 - Prob. 7.7VPCh. 7 - Prob. 7.8VPCh. 7 - Prob. 7.9VPCh. 7 - Prob. 7.10VPCh. 7 - Prob. 7.11VPCh. 7 - Prob. 7.12VPCh. 7 - Prob. 7.13VPCh. 7 - Prob. 7.14VPCh. 7 - Prob. 7.15VPCh. 7 - Prob. 7.16VPCh. 7 - Prob. 7.17VPCh. 7 - Prob. 7.18VPCh. 7 - Prob. 7.19VPCh. 7 - Prob. 7.20VPCh. 7 - Prob. 7.21QPCh. 7 - Prob. 7.22QPCh. 7 - Prob. 7.23QPCh. 7 - Prob. 7.24QPCh. 7 - Prob. 7.25QPCh. 7 - Prob. 7.26QPCh. 7 - Prob. 7.27QPCh. 7 - Prob. 7.28QPCh. 7 - Prob. 7.29QPCh. 7 - Prob. 7.30QPCh. 7 - Prob. 7.31QPCh. 7 - Prob. 7.32QPCh. 7 - Prob. 7.33QPCh. 7 - Prob. 7.34QPCh. 7 - Prob. 7.35QPCh. 7 - Prob. 7.36QPCh. 7 - Prob. 7.37QPCh. 7 - Prob. 7.38QPCh. 7 - Prob. 7.39QPCh. 7 - Prob. 7.40QPCh. 7 - Prob. 7.41QPCh. 7 - Prob. 7.42QPCh. 7 - Prob. 7.43QPCh. 7 - Prob. 7.44QPCh. 7 - Prob. 7.45QPCh. 7 - Prob. 7.46QPCh. 7 - Prob. 7.47QPCh. 7 - Prob. 7.48QPCh. 7 - Prob. 7.49QPCh. 7 - Prob. 7.50QPCh. 7 - Prob. 7.51QPCh. 7 - Prob. 7.52QPCh. 7 - Prob. 7.53QPCh. 7 - Prob. 7.54QPCh. 7 - Prob. 7.55QPCh. 7 - Prob. 7.56QPCh. 7 - Prob. 7.57QPCh. 7 - Prob. 7.58QPCh. 7 - Prob. 7.59QPCh. 7 - Prob. 7.60QPCh. 7 - Prob. 7.61QPCh. 7 - Prob. 7.62QPCh. 7 - Prob. 7.63QPCh. 7 - Prob. 7.64QPCh. 7 - Prob. 7.65QPCh. 7 - Prob. 7.66QPCh. 7 - Prob. 7.67QPCh. 7 - Prob. 7.68QPCh. 7 - Prob. 7.69QPCh. 7 - Prob. 7.70QPCh. 7 - Prob. 7.71QPCh. 7 - Prob. 7.72QPCh. 7 - Prob. 7.73QPCh. 7 - Prob. 7.74QPCh. 7 - Prob. 7.75QPCh. 7 - Prob. 7.76QPCh. 7 - Prob. 7.77QPCh. 7 - Prob. 7.78QPCh. 7 - Prob. 7.79QPCh. 7 - Prob. 7.80QPCh. 7 - Prob. 7.81QPCh. 7 - Prob. 7.82QPCh. 7 - Prob. 7.83QPCh. 7 - Prob. 7.84QPCh. 7 - Prob. 7.85QPCh. 7 - Prob. 7.86QPCh. 7 - Prob. 7.87QPCh. 7 - Prob. 7.88QPCh. 7 - Prob. 7.89QPCh. 7 - Prob. 7.90QPCh. 7 - Prob. 7.91QPCh. 7 - Prob. 7.92QPCh. 7 - Prob. 7.93QPCh. 7 - Prob. 7.94QPCh. 7 - Prob. 7.95QPCh. 7 - Prob. 7.96QPCh. 7 - Prob. 7.97QPCh. 7 - Prob. 7.98QPCh. 7 - Prob. 7.99QPCh. 7 - Prob. 7.100QPCh. 7 - Prob. 7.101QPCh. 7 - Prob. 7.102QPCh. 7 - Prob. 7.103QPCh. 7 - Prob. 7.104QPCh. 7 - Prob. 7.105QPCh. 7 - Prob. 7.106QPCh. 7 - Prob. 7.107QPCh. 7 - Prob. 7.108QPCh. 7 - Prob. 7.109QPCh. 7 - Prob. 7.110QPCh. 7 - Prob. 7.111QPCh. 7 - Prob. 7.112QPCh. 7 - Prob. 7.113QPCh. 7 - Prob. 7.114QPCh. 7 - Prob. 7.115QPCh. 7 - Prob. 7.116QPCh. 7 - Prob. 7.117QPCh. 7 - Prob. 7.118QPCh. 7 - Prob. 7.119QPCh. 7 - Prob. 7.120QPCh. 7 - Prob. 7.121QPCh. 7 - Prob. 7.122QPCh. 7 - Prob. 7.123QPCh. 7 - Prob. 7.124QPCh. 7 - Prob. 7.125QPCh. 7 - Prob. 7.126QPCh. 7 - Prob. 7.127QPCh. 7 - Prob. 7.128QPCh. 7 - Prob. 7.129APCh. 7 - Prob. 7.130APCh. 7 - Prob. 7.131APCh. 7 - Prob. 7.132APCh. 7 - Prob. 7.133APCh. 7 - Prob. 7.134APCh. 7 - Prob. 7.135APCh. 7 - Prob. 7.136APCh. 7 - Prob. 7.137APCh. 7 - Prob. 7.138APCh. 7 - Prob. 7.139APCh. 7 - Prob. 7.140APCh. 7 - Prob. 7.141APCh. 7 - Prob. 7.142APCh. 7 - Prob. 7.143APCh. 7 - Prob. 7.144APCh. 7 - Prob. 7.145APCh. 7 - Prob. 7.146APCh. 7 - Prob. 7.147APCh. 7 - Prob. 7.148AP
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