Question

how many orbitals can have the following set of quantum numbers n=3,l=1, m1=0?
a)3
b)1
c)4
d)2​

Answer 1

Therefore the correct option is (b) 1

we have to find the number of orbitals in the set of quantum numbers n = 3, l = 1 and m₁ = 0

solution : we know, there are four quantum numbers to identify the position of electron in an atom.

principal quantum number = n

azimuthal quantum number = l

magnetic quantum number = m

spin quantum number = s

here n = 3 and l = 1

shows the orbitals of $3p_x, 3p_y, 3p_z$ [ p subshell has only three orbitals i.e., px , py and pz ]

but m₁ = 0, shows any one of three orbitals.

[ other two magnetic quantum numbers are m₂ = 1 , m₃ = -1 ]

let m₁ = 0 shows $3p_z$

Therefore n = 3, l = 1 and m₁ = 0 shows only one orbital i.e., $3p_z$

Therefore the correct option is (b) 1

Answer 2

Answer:

Therefore the correct option is (b) 1

we have to find the number of orbitals in the set of quantum numbers n = 3, l = 1 and m₁ = 0

Explanation:

solution : we know, there are four quantum numbers to identify the position of electron in an atom.

principal quantum number = n

azimuthal quantum number = l

magnetic quantum number = m

spin quantum number = s

here n = 3 and l = 1

shows the orbitals of  [ p subshell has only three orbitals i.e., px , py and pz ]

but m₁ = 0, shows any one of three orbitals.

[ other two magnetic quantum numbers are m₂ = 1 , m₃ = -1 ]

let m₁ = 0 shows  

Therefore n = 3, l = 1 and m₁ = 0 shows only one orbital i.e.,

Therefore the correct option is (b) 1

if it helps u keep this as brainlist answer