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Electron Configurations

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Presentation on theme: "Electron Configurations"— Presentation transcript:

1 Electron Configurations
Section 5.3

2 Electron Configurations
Atom is in the ground state 3 rules or laws Aufbau principle Pauli Exclusion principle Hund’s Law

3 Aufbau Principle Electrons occupy lowest energy orbital available
All orbitals of a sublevel are equal energy Sublevels have different energies s < p < d <f Orbitals within one principal energy level can overlap orbitals of another

4 Electron Filling Order
Which orbital will fill first, 4s or 3d?

5 Periodic Table Helps!

6 Pauli Exclusion Principle
Maximum of 2 electrons in an orbital, but only if they have opposite spin.

7 Hund’s rule Electrons with same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbital.

8 Orbital Filling Order 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

9 Electron Configurations
Three methods 1. Electron Configuration Notation 2. Noble Gas Notation 3. Orbital Diagrams

10 Electron Configuration Notation
Ex: N # of electrons? Start with the lowest energy, fill to capacity, go to next lowest energy, etc. Stop when you run out of electrons. Superscripts = total electrons

11 Electron Configuration Notation
You try … Zinc

12 Electron Configuration Notation
1s2 2s22p6 3s23p6 4s23d10

13 Assignment Write the electron configuration notation for the following elements: Boron (B), Neon (Ne), Sulfur (S), Magnesium (Mg), Vanadium (V), Silver (Ag)

14 Noble Gas Notation Shorthand
Find the noble gas closest to the element (without going over). Ex: For Gold (79): Xenon (54) We write [Xe] and start counting from there The first orbital after xenon is 6s

15 [Xe]6s2 4f14 5d9 Noble Gas Notation
Check: (Xe’s atomic number) = 79 (gold’s Atomic number)!

16 You Try… Silver

17 Assignment P.147 #79

18 Orbital Diagrams Draw a line for each orbital
Designate each electron with an arrow = orbital with 1 electron = orbital with 2 electrons

19 Orbital Diagrams Nitrogen: 1s22s22p3 Write notation of N
Then we fill them with electrons using the Aufbau principle, Pauli exclusion principle, and Hund’s law

20 Orbital Diagrams You try another example: Cu

21 Orbital Diagrams Answer

22 Assignment Draw orbital diagrams for beryllium, aluminum, nitrogen, and sodium, manganese, germanium, and europium.

23 Electron Dot Structures
Valence electrons Electrons in outermost energy level. Responsible for chemical properties

24 Electron Dot Structures
Valence electrons only Place ‘dots’ around element symbol 4 sides of element = orbitals Fill these orbitals one at a time (Hund’s)

25 Electron Dot Structures

26 Assignment P.141 #23(yellow box), 26, 28 P.147 #81


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