Identify four sets of quantum numbers for the ff. electrons: 3p5 , 4d4 and 5f13
To identify the quantum numbers for the given electrons (3p5, 4d4, and 5f13), we need to understand the different quantum numbers and how they relate to the electrons' energy levels and spatial orientation.
Quantum numbers are a set of values used to describe the properties and behavior of electrons in an atom. There are four main quantum numbers: principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (ml), and spin quantum number (ms).
1. For the electron 3p5:
- Principal quantum number (n) = 3: The electron is in the third energy level or shell.
- Azimuthal quantum number (l) = 1: The electron is in the p subshell, which corresponds to l = 1 (p subshell has three orbitals).
- Magnetic quantum number (ml) = -1, 0, 1: Since l = 1, there are three possible orientations for the p subshell (-1, 0, 1).
- Spin quantum number (ms) = +1/2 or -1/2: Each orbital can accommodate two electrons with opposite spins. However, since we have only one electron, the spin can be either +1/2 or -1/2.
The four sets of quantum numbers for the electron 3p5 are:
(3, 1, -1, +1/2)
(3, 1, 0, -1/2)
(3, 1, 1, +1/2)
(3, 1, -1, -1/2)
2. For the electron 4d4:
- Principal quantum number (n) = 4: The electron is in the fourth energy level or shell.
- Azimuthal quantum number (l) = 2: The electron is in the d subshell, which corresponds to l = 2 (the d subshell has five orbitals).
- Magnetic quantum number (ml) = -2, -1, 0, 1, 2: Since l = 2, there are five possible orientations for the d subshell (-2, -1, 0, 1, 2).
- Spin quantum number (ms) = +1/2 or -1/2: Each orbital can accommodate two electrons with opposite spins. However, since we have only one electron, the spin can be either +1/2 or -1/2.
The four sets of quantum numbers for the electron 4d4 are:
(4, 2, -2, +1/2)
(4, 2, -1, -1/2)
(4, 2, 0, +1/2)
(4, 2, 1, -1/2)
3. For the electron 5f13:
- Principal quantum number (n) = 5: The electron is in the fifth energy level or shell.
- Azimuthal quantum number (l) = 3: The electron is in the f subshell, which corresponds to l = 3 (the f subshell has seven orbitals).
- Magnetic quantum number (ml) = -3, -2, -1, 0, 1, 2, 3: Since l = 3, there are seven possible orientations for the f subshell (-3, -2, -1, 0, 1, 2, 3).
- Spin quantum number (ms) = +1/2 or -1/2: Each orbital can accommodate two electrons with opposite spins. However, since we have only one electron, the spin can be either +1/2 or -1/2.
The four sets of quantum numbers for the electron 5f13 are:
(5, 3, -3, +1/2)
(5, 3, -2, -1/2)
(5, 3, -1, +1/2)
(5, 3, 0, -1/2)
Remember, quantum numbers describe the properties and behavior of individual electrons within an atom.