1. Quantum Model of the Atom
Ch. 4 - Electrons in Atoms
Quantum Model of the Atom

2. A. Electrons as Waves Louis de Broglie (1924)
Applied wave-particle theory to e-
e- exhibit wave properties
QUANTIZED WAVELENGTHS

3. A. Electrons as Waves
QUANTIZED WAVELENGTHS

4. A. Electrons as Waves EVIDENCE: DIFFRACTION PATTERNS VISIBLE LIGHT

5. B. Quantum Mechanics Heisenberg Uncertainty Principle
Impossible to know both the velocity and position of an electron at the same time

6. B. Quantum Mechanics Schrödinger Wave Equation (1926)
finite # of solutions  quantized energy levels
defines probability of finding an e-

7. Radial Distribution Curve
B. Quantum Mechanics
Orbital (“electron cloud”)
Region in space where there is 90% probability of finding an e-
Orbital
Radial Distribution Curve

8. B. Quantum Mechanics
Four Types of Orbitals: f d s p

9. C. Quantum Numbers 2s 2px 2py 2pz
Orbitals combine to form a spherical shape. 2s
2pz
2py
2px

10. Electron Configuration
Ch. 5 - Electrons in Atoms
Electron Configuration

11. Heisenberg Uncertainty Principle
Both the position and the velocity of an electron cannot be determined at the same time.

12. A. General Rules Pauli Exclusion Principle
Each orbital can hold TWO electrons with opposite spins.

13. A. General Rules Aufbau Principle
Electrons fill the lowest energy orbitals first.
“Lazy Tenant Rule”

14. A. General Rules WRONG RIGHT Hund’s Rule
Within a sublevel, place one e- per orbital before pairing them.
“Empty Bus Seat Rule”
WRONG
RIGHT

15. B. Periodic Patterns s p d (n-1) f (n-2) 1 2 3 4 5 6 7 6 7
© 1998 by Harcourt Brace & Company

16. B. Periodic Patterns p s d (n-1) f (n-2) Atomic #
Total # of e- in the atom
Period #
energy level (subtract for d & f) s
d (n-1)
f (n-2) p

17. B. Periodic Patterns A/B Group # total # of valence e-
Valence e- are the electrons in the outermost energy level
Core e- are all of the electrons in inner energy levels

18. 1s2 2s2 2p4 O C. Notation 1s 2s 2p 8e- Orbital Diagram
Electron Configuration
1s2 2s2 2p4

19. S 16e- 1s2 2s2 2p6 3s2 3p4 S 16e- [Ne] 3s2 3p4 C. Notation
Longhand Configuration
S 16e-
1s2
2s2
2p6
3s2
3p4
Core Electrons
Valence Electrons
Shorthand Configuration
S 16e- [Ne] 3s2 3p4

20. C. Periodic Patterns p s d (n-1) f (n-2) Shorthand Configuration
Core e-: Go up one row and over to the Noble Gas.
Valence e-: On the next row, fill in the # of e- in each sublevel. s
d (n-1)
f (n-2) p

21. C. Periodic Patterns
Example - Germanium
[Ar]
4s2
3d10
4p2

22. D. Stability Full energy level Full sublevel (s, p, d, f)
Half-full sublevel

23. D. Stability Electron Configuration Exceptions Copper
EXPECT: [Ar] 4s2 3d9
ACTUALLY: [Ar] 4s1 3d10
Copper gains stability with a full d-sublevel.

24. D. Stability Electron Configuration Exceptions Chromium
EXPECT: [Ar] 4s2 3d4
ACTUALLY: [Ar] 4s1 3d5
Chromium gains stability with a half-full d-sublevel.

25. D. Stability 1+ 2+ 3+ NA 3- 2- 1- Ion Formation
Atoms gain or lose electrons to become more stable.
Isoelectronic with the Noble Gases. 1+ 2+ 3+ NA 3- 2- 1-

26. O2- 10e- [He] 2s2 2p6 D. Stability Ion Electron Configuration
Write the e- config for the closest Noble Gas
EX: Oxygen ion  O2-  Ne
O e [He] 2s2 2p6

27. 4 quantum numbers