Question

Write the four quantum numbers for an electron in a 3p orbital

Answer 1

Answer:

n=3,l=1,ml=0,1,-1ms=1/2

Explanation:

for3p orbital

n=3,l=1,ml=0,1,-1

Answer 2

Answer:

For $3p$ orbital, the four quantum numbers i.e. $n,l,m,s$ are as follows-

$n=3,\\l=1,\\m=-1,0,+1\\s=-\frac{1}{2},+\frac{1}{2}$

Explanation:

• In quantum physics and chemistry, quantum numbers describe the numbers or numerical values of the conserved quantities of a quantum system.

• To specify the energy, size, shape and orientation of an atom in an orbital completely, a set of four quantum numbers are necessary i.e.

$n,l,m,s$  

• The principal quantum number '$n$' identifies the shell, and determines the size, and energy of the orbital.

• Azimuthal quantum number '$l$' or orbital angular momentum. It gives information about the subshell and determines the shape of orbitals, the energy of orbitals in multi-electron atoms with principal quantum numbers with orbital angular orbital i.e. $\sqrt{l(l+1)}\frac{h}{2\pi }$.

• For a given value of $n$, it can have values ranging from 0 to $n-1$ . The total number of subshells in a particular shell is equal to the value of $n$.

• Magnetic quantum number or magnetic orbital quantum number (ml) gives information about the spatial orientation of the orbital to the standard set of co-ordinate axis.

• Electron spin quantum number (s) refers to the orientation, of the spin of the $e^{-}$. this can have 2 values $+\frac{1}{2 }$(clockwise spin) and $-\frac{1}{2}$(anti-clockwise spin).

Hence for $3p$ orbital,

Value of principal quantum number($n$) = $3$

Value of Azimuthal quantum number ($l$) = $1$

Value of magnetic quantum number ($m$)= $-1,0,+1$

Value of spin quantum number ($s$)= $-\frac{1}{2} , +\frac{1}{2}$