SCIENCE 9 #2 QUANTUM MECHANCAL MODEL.pptx

SCIENCE 9 QUARTER 2 Quantum mechanical model.

1. SCIENCE 9 QUARTER 2 Quantum Mechanical Model

2. Quantum There are clouds called orbits where electrons exist Electrons do not orbit in a predetermined path around the nucleus Erwin Schrodinger 1926

3. QUANTUM MECHANICAL MODEL the modern framework scientists use to understand how electrons behave inside atoms.

4. Pauli’s Exclusion Principle: No two electrons can have the same four quantum numbers.

5. Hund’s Rule: Electrons fill degenerate orbitals singly first, with parallel spins, before pairing.

6. Aufbau Principle Fill lower-energy orbitals first.

7. Activity

8. 1. Al = 2. Sc = 3. Ni = 4. Ne= 5. Ba = Write the electron configuration of the following elements 1s 2 2s 2 2p 6 3s 2 3p 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 8 1s 2 2s 2 2p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2

9. 1. Al = Arrange the electrons into orbitals. 1s 2 2s 2 2p 6 3s 2 3p 1

10. 1. Sc = Arrange the electrons into orbitals. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1

11. 1. Al = 2. Sc = 3. Ni = 4. Ne= 5. Ba = Arrange the electrons into orbitals. 1s 2 2s 2 2p 6 3s 2 3p 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 8 1s 2 2s 2 2p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2

12. Quantum numbers

13. QUANTUM NUMBERS They help us locate electrons. They explain element properties. Schrodinger 1803

14. Energy level (1, 2, 3.....) Represents size and energy of the orbital. Higher n → electron farther from nucleus. Principal Quantum Number n

15. He 1s 2 n= 1 Principal Quantum Number n

16. Sublevel/shape (s, p, d, f) Determines shape of orbital. ℓ ≤ n-1 (s=0, p=1, d=2, f=3) Angular Momentum Quantum Number ℓ

17. Angular Momentum Quantum Number

18. He 1s 2 n= 1 ℓ= 0 Angular Momentum Quantum Number ℓ

19. Orbital orientation mₗ = integer values from –ℓ to +ℓ. Describes orbital’s orientation in space. Magnetic Quantum Number mₗ

20. Magnetic Quantum Number mₗ

21. He 1s 2 n= 1 ℓ= 0 mₗ = 0 Magnetic Quantum Number mₗ

22. Spin direction (+½ or −½) mₛ = +½ or −½. Two electrons can occupy the same orbital only if spins are opposite. Spin Quantum Number mₛ

23. He 1s 2 n= 1 ℓ= 0 mₗ = 0 mₛ = +½ or −½. Spin Quantum Number mₛ

24. "What are the quantum numbers for the last electron of Nitrogen (1s² 2s² 2p³)?"

25. "What are the quantum numbers for the last electron of Nitrogen (1s² 2s² 2p³)?" 2p³ n = 2 ℓ = 1 m l = -1, 0, 1 mₛ = -½ or ½

26. Activity Quantum Numbers

27. "What are the quantum numbers for the last electron of the ff. elements? Carbon Silicon Boron Gold HELIUM n = ℓ = m l = mₛ =