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1. Quantum numbers

2. • 1- principal quantum number (n)
• Identify
• The main energy levels . So
• n= 1,2,3,4,………………..
• The maximum no. of electrons in the first
fourth energy levels by 2n2

3. • Ex n=1
• The maximum electron no. = 2 e
• n=2
• No.of e = 8
• n= 3
• No. of e = 18
• n= 4
• No . Of e =32

4. • 2- Subsidiary ( azimuthal ) qu. No. (l )
• Identify
• The sublevels in each main energy level .
• S , p , d , f .
• l= ( 0 , 1 , 2 , 3 ) by l = ( 0 , n-1 )

5. • 3- the magnetic qu. No. (ml)
• Identify
• The orbitals and there orientation
• 4- the spin qu. No.
• Identify
• The motion of electron ( + 1/2 or - 1 /2 )

6. • Distribution of electron
• Auf – bau principle
• Filling electrons in sublevels begin by low
energy then high one
• Follow that diagram

7. 1S
2S 2P
3S 3P
4S 3d 4P
5S 4d 5P
6S 4f 5d 6P
7S 5f 6d 7P

8. • S = 1 orbital field by 2 electrons
• P = 3 orbital 6
• d= 5 orbital 10
• f = 7 14

9. • Ex write the electronic configuration of the
following elements then calculate the four
quantum no. of the last electron
• Na =11
• S = 16
• Cr = 24
• Cu = 29
• Ce = 58