The orbital with `n=3` and `l=2` is

Quantum Numbers The whereabouts and characteristics of an electron in an atom can be known by a set of four quantum numbers, which describe the electron's distance from nucleus, shape of the orbital, its orientation, and spin. Principal quantum number (n): The principal quantum number (n) is a positive integer (n = 1, 2, 3, 4, ...) on which the size and energy level of the orbital primarily depends. Its value gives us the 'shell in which the electron is present. It also gives us an idea of the average energy possessed by an electron and the average distance from the nucleus where it is likely to be found. Azimuthal quantum number (l) : The azimuthal quantum number defines the three-dimensional shape of the orbital (subshell) in which the electron is present. Its value ranges from 0 to n-1 for a given value of n, for example, if n = 2, possible values of l are 0 and 1. The azimuthal quantum number is also known as the angular momentum quantum number, and it gives an idea about the absolute value of energy possessed by the electron. For example, an orbital with n= 3 and l = 2 in the 3d orbital, n = 3 represents the 3rd shell and l = 2 represents the d subshell (if l = 0, 1, 2, and 3, the orbital is s, p, d, and f, respectively). Magnetic quantum number (m): The magnetic quantum number defines the spatial orientation of the orbital with respect to a standard set of coordinate axes. For an orbital whose angular momentum quantum number is l , the magnetic quantum number m can have values ranging from -l to +l , including 0. Thus, within each subshell (orbitals with the same value of l ) there are 2l+1 different spatial orientations for those orbitals. For example, if l = 0 , then m= 0. If l = 1 , then m = -1, 0, or +1. If l = 2 , then m= -2,-1, 0, +1, or +2 . If l = 3 , then m=-3, -2, -1, 0, +1, +2, or +3 ... and so forth. Spin quantum number(s): The spin quantum number exemplifies the spin of an electron around its imaginary axis. For each value of magnetic quantum number, only two values of the spin quantum number are permitted, that is, +(1)/(2) or -(1)/(2), s = +(1)/(2) denotes a clockwise spin and -(1)/(2) denotes anticlockwise spin. A maximum of only 2 electrons can be accommodated in each of the spatial orientations represented by m. Based on the provided information, answer the following questions: If the principal quantum number is 3, what possible values can azimuthal quantum number have?

Quantum Numbers The whereabouts and characteristics of an electron in an atom can be known by a set of four quantum numbers, which describe the electron's distance from nucleus, shape of the orbital, its orientation, and spin. Principal quantum number (n): The principal quantum number (n) is a positive integer (n = 1, 2, 3, 4, ...) on which the size and energy level of the orbital primarily depends. Its value gives us the 'shell in which the electron is present. It also gives us an idea of the average energy possessed by an electron and the average distance from the nucleus where it is likely to be found. Azimuthal quantum number (l) : The azimuthal quantum number defines the three-dimensional shape of the orbital (subshell) in which the electron is present. Its value ranges from 0 to n-1 for a given value of n, for example, if n = 2, possible values of l are 0 and 1. The azimuthal quantum number is also known as the angular momentum quantum number, and it gives an idea about the absolute value of energy possessed by the electron. For example, an orbital with n= 3 and l = 2 in the 3d orbital, n = 3 represents the 3rd shell and l = 2 represents the d subshell (if l = 0, 1, 2, and 3, the orbital is s, p, d, and f, respectively). Magnetic quantum number (m): The magnetic quantum number defines the spatial orientation of the orbital with respect to a standard set of coordinate axes. For an orbital whose angular momentum quantum number is l , the magnetic quantum number m can have values ranging from -l to +l , including 0. Thus, within each subshell (orbitals with the same value of l ) there are 2l+1 different spatial orientations for those orbitals. For example, if l = 0 , then m= 0. If l = 1 , then m = -1, 0, or +1. If l = 2 , then m= -2,-1, 0, +1, or +2 . If l = 3 , then m=-3, -2, -1, 0, +1, +2, or +3 ... and so forth. Spin quantum number(s): The spin quantum number exemplifies the spin of an electron around its imaginary axis. For each value of magnetic quantum number, only two values of the spin quantum number are permitted, that is, +(1)/(2) or -(1)/(2), s = +(1)/(2) denotes a clockwise spin and -(1)/(2) denotes anticlockwise spin. A maximum of only 2 electrons can be accommodated in each of the spatial orientations represented by m. Based on the provided information, answer the following questions: Which of the following sets of quantum numbers are not permitted? Why?

Quantum Numbers The whereabouts and characteristics of an electron in an atom can be known by a set of four quantum numbers, which describe the electron's distance from nucleus, shape of the orbital, its orientation, and spin. Principal quantum number (n): The principal quantum number (n) is a positive integer (n = 1, 2, 3, 4, ...) on which the size and energy level of the orbital primarily depends. Its value gives us the 'shell in which the electron is present. It also gives us an idea of the average energy possessed by an electron and the average distance from the nucleus where it is likely to be found. Azimuthal quantum number (l) : The azimuthal quantum number defines the three-dimensional shape of the orbital (subshell) in which the electron is present. Its value ranges from 0 to n-1 for a given value of n, for example, if n = 2, possible values of l are 0 and 1. The azimuthal quantum number is also known as the angular momentum quantum number, and it gives an idea about the absolute value of energy possessed by the electron. For example, an orbital with n= 3 and l = 2 in the 3d orbital, n = 3 represents the 3rd shell and l = 2 represents the d subshell (if l = 0, 1, 2, and 3, the orbital is s, p, d, and f, respectively). Magnetic quantum number (m): The magnetic quantum number defines the spatial orientation of the orbital with respect to a standard set of coordinate axes. For an orbital whose angular momentum quantum number is l , the magnetic quantum number m can have values ranging from -l to +l , including 0. Thus, within each subshell (orbitals with the same value of l ) there are 2l+1 different spatial orientations for those orbitals. For example, if l = 0 , then m= 0. If l = 1 , then m = -1, 0, or +1. If l = 2 , then m= -2,-1, 0, +1, or +2 . If l = 3 , then m=-3, -2, -1, 0, +1, +2, or +3 ... and so forth. Spin quantum number(s): The spin quantum number exemplifies the spin of an electron around its imaginary axis. For each value of magnetic quantum number, only two values of the spin quantum number are permitted, that is, +(1)/(2) or -(1)/(2), s = +(1)/(2) denotes a clockwise spin and -(1)/(2) denotes anticlockwise spin. A maximum of only 2 electrons can be accommodated in each of the spatial orientations represented by m. Based on the provided information, answer the following questions: Write down the values of n and l for an electron having the highest energy in a sodium atom.

What designations are given to orbitals with n = 4, l = 1 and n = 4, l =3 ?

What is the designation of an orbital having n = 4 and l = 2 ?

Maximum number of electrons in an orbital having n = 4 and l = 2 are :

The orbital with `n=3` and `l=2` is

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