1) Give the four quantum numbers for each of the each of the two electrons in a 6s orbital.

2.     Give the values of the quantum numbers associated with the orbitals in the 3p subshell.

3.     Determine the four quantum numbers of the electrons residing in the 4^th energy level. What is the total number of orbitals associated with the principal quantum number?

4.     Write the four quantum numbers for an electron in a 4d orbital.

5.     Write the electron configuration for aluminum. Draw its orbital diagram.

 

1. n= 6 , l= 0 , m_l= 0 , m_s= +-1/2

2. n= 3 , l= 1 , m_l= -1,0,+1 , m_s= +-1/2

3. No. Of orbitals = n²

= 4²

= 16 orbitals

4. n= 4, l= 2 , m_l= -2,-1,0,+1,+2 , m_s= +-1/2

5. Al= 1s² 2s² 2p⁶ 3s² 3p¹

Complete answer (including orbital diagram) is attached as image.

Step-by-step explanation

Principal Quantum Number (n) represents the energy of an electron and the size of the orbital

n can have any integral value of 1,2,3,---

Azimuthal quantum number (l) represents the shape of an orbital with a particular principal quantum number

l can have any integral value of 0,1,2,---,(n-1)

Values of l for subshell s=0, p=1, d=2, f=3

Magnetic quantum number (m_l) represents the orientation in space of an orbital of a given energy (n) and shape (l)

It can have any integral value ranging -l,---,0,---,+l

Spin quantum number (m_s) represents the orientation of the spin axis of an electron. An electron can spin in only one of two directions sometimes called up and down, often represented as +1/2 or -1/2

Please see the attached file for the complete solution