Question

the allowable combinations of quantum numbers for each of the electron in 4s, 3p,5d orbitals respectively : ​

Answer 1

Answer:

4s

n=4, l=0    m=-l to +l i.e. 0  s = + or - 1/2

3p

n=3, l=1    m=-l to +l i.e. -1, 0 , 1   s = + or - 1/2

5d

n=5, l=2    m=-l to +l i.e. -2 ,- 1 , 0 , 1, 2   s = + or - 1/2

Explanation:

Answer 2

For 4s n=4,l=0 and m=0

For 3p, n=3,l=1 and m=+1,0,-1

For 5d, n=5,l=2 and m=+2,+1,0,-1,-2.

• n is called the principal quantum number.
• l is called the azimuthal quantum number and for 's' orbital l is 0, for p orbital it is 1 and for d orbital l is 2.
• m is the magnetic quantum number. It has a value from +l to -l.
• Thus, the value of the quantum numbers for each of the electrons in 4s, 3p,5d orbitals respectively-
• For 4s n=4,l=0 and m=0
• For 3p, n=3,l=1 and m=+1,0,-1
• For 5d, n=5,l=2 and m=+2,+1,0,-1,-2.