Answer
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Work Step by Step
For the ground state of an atom, the possible set of values for the four quantum numbers are as follows:
1. Principal quantum number (n): It represents the energy level of the electron and can take positive integer values (1, 2, 3, ...).
2. Azimuthal quantum number (l): It represents the shape of the orbital and can take values from 0 to (n-1).
3. Magnetic quantum number (m_l): It represents the orientation of the orbital and can take values from -l to +l.
4. Spin quantum number (m_s): It represents the spin of the electron and can take values of +1/2 or -1/2.
For a boron atom, the ground state electron configuration is 1s² 2s² 2p¹. Therefore, the possible set of quantum numbers for the electron in the 2p orbital of boron are:
- n = 2
- l = 1
- m_l = -1, 0, 1
- m_s = +1/2 or -1/2
For a nitrogen atom, the ground state electron configuration is 1s² 2s² 2p³. Therefore, the possible set of quantum numbers for one of the electrons in the 2p orbital of nitrogen are:
- n = 2
- l = 1
- m_l = -1, 0, 1
- m_s = +1/2 or -1/2
These sets of quantum numbers satisfy the Pauli exclusion principle and describe the ground state electron configurations for boron and nitrogen atoms.
