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Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. On= 4, 1= 2, m₁=+4 O n= 3, 1= 2, m₁=-3 O n= 4, 1= 3, m₁=-2 O n= 2, 1= 2, m₁=0 O n=2, 1= 2, m₁=-1 Next

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. On= 4, 1= 2, m₁=+4 O n= 3, 1= 2, m₁=-3 O n= 4, 1= 3, m₁=-2 O n= 2, 1= 2, m₁=0 O n=2, 1= 2, m₁=-1 Next

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Quantum Numbers Exercise **Question:** Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. **Options:** - O n= 4, l= 2, mₗ=+4 - O n= 3, l= 2, mₗ=-3 - O n= 4, l= 3, mₗ=-2 - O n= 2, l= 2, mₗ=0 - O n= 2, l= 2, mₗ=-1 ### Explanation: Quantum numbers are used to describe the properties of atomic orbitals and the properties of electrons in orbitals. The four quantum numbers are: 1. **Principal Quantum Number (n)**: Indicates the main energy level or shell of the electron. It can be any positive integer (n=1, 2, 3, ...). 2. **Angular Momentum Quantum Number (l)**: Indicates the shape of the orbital. It can be any integer from 0 to n-1. For example, if n=3, then l can be 0, 1, or 2. 3. **Magnetic Quantum Number (mₗ)**: Indicates the orientation of the orbital in space. It can be any integer from -l to +l, including zero. For example, if l=2, then mₗ can be -2, -1, 0, +1, or +2. 4. **Spin Quantum Number (mₛ)**: Indicates the spin of the electron in the orbital, either +1/2 or -1/2. This quantum number is not used in this particular problem. Using these rules, we can determine the correct set of quantum numbers: - **n= 4, l= 2, mₗ=+4**: This is incorrect because the value of mₗ should range from -l to +l. Here it incorrectly goes beyond this range. - **n= 3, l= 2, mₗ=-3**: This is incorrect because the value of mₗ should range from -l to +l. Here it incorrectly goes beyond this range. - **n= 4, l= 3, mₗ=-2**: This is correct. l=
Transcribed Image Text:### Quantum Numbers Exercise **Question:** Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. **Options:** - O n= 4, l= 2, mₗ=+4 - O n= 3, l= 2, mₗ=-3 - O n= 4, l= 3, mₗ=-2 - O n= 2, l= 2, mₗ=0 - O n= 2, l= 2, mₗ=-1 ### Explanation: Quantum numbers are used to describe the properties of atomic orbitals and the properties of electrons in orbitals. The four quantum numbers are: 1. **Principal Quantum Number (n)**: Indicates the main energy level or shell of the electron. It can be any positive integer (n=1, 2, 3, ...). 2. **Angular Momentum Quantum Number (l)**: Indicates the shape of the orbital. It can be any integer from 0 to n-1. For example, if n=3, then l can be 0, 1, or 2. 3. **Magnetic Quantum Number (mₗ)**: Indicates the orientation of the orbital in space. It can be any integer from -l to +l, including zero. For example, if l=2, then mₗ can be -2, -1, 0, +1, or +2. 4. **Spin Quantum Number (mₛ)**: Indicates the spin of the electron in the orbital, either +1/2 or -1/2. This quantum number is not used in this particular problem. Using these rules, we can determine the correct set of quantum numbers: - **n= 4, l= 2, mₗ=+4**: This is incorrect because the value of mₗ should range from -l to +l. Here it incorrectly goes beyond this range. - **n= 3, l= 2, mₗ=-3**: This is incorrect because the value of mₗ should range from -l to +l. Here it incorrectly goes beyond this range. - **n= 4, l= 3, mₗ=-2**: This is correct. l=
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