The magnetic quantum number is denoted by letter "m" ,and for a given value of "1" ,it can have all the values ranging from "-1" to "+1 including zero.For a given "1,m has "21+1" values.For example, if "I=2,m" can have values,i.e.,m=-2,-1,0,+1,+2" .This implies that there are five different orientations of the d- subshell.In other words,"d-]subshell has five d-orbitals How many electrons can fit into the orbitals that comprise the third quantum shell "n=3?

What values of magnetic quantum number, m are permitted for an electron having angular momentum quantum number value, l = 2 ?

If a quantum number l has value of 2, what are the permitted values of quantum number 'm_(1)' ?

How many electrons in a given atom can have the following quantum numbers ? (a) n = 3, l = 1 (b) n = 3, l = 2, m_l = 0 (c ) n = 3, l = 2, m_l = +2, m_s = + 1/2 (d) n = 3 .

An electron in a mercury atoms is in the 3d subshell. Which of the following m_(l) values are possible for it, (a) -3 , (b) -1 , (c ) 0, (d) 1, (e) 2?

Give the possible value for the missing quantum number (s) in each of the following sets. (a) n=3, l=0, m_(l)=? , (b) n=3, l=?, m_(l)=-1 (c) n=?, l=1, m_(l)=+1 , (d) n=?, l=2, m_(l)=? .

What are the possible values of m_(s) when m_(l) have values +1, +2,+3 ?

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 l = 2 , what are the permitted values for m?

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?