Section 5 3
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Section 5.3. Electron Configurations. Electron Configurations. Atom is in the ground state 3 rules or laws Aufbau principle Pauli Exclusion principle Hund’s Law. Aufbau Principle. Electrons occupy lowest energy orbital available All orbitals of a sublevel are equal energy

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Section 5.3

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Section 5 3

Section 5.3

Electron Configurations


Electron configurations

Electron Configurations

  • Atom is in the ground state

  • 3 rules or laws

    • Aufbau principle

    • Pauli Exclusion principle

    • Hund’s Law


Aufbau principle

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


Electron filling order

Electron Filling Order

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


Periodic table helps

Periodic Table Helps!


Pauli exclusion principle

Pauli Exclusion Principle

  • Maximum of 2 electrons in an orbital, but only if they have opposite spin.


Hund s rule

Hund’s rule

  • Electrons with same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbital.


Orbital filling order

Orbital Filling Order

1s 2s 2p 3s 3p 4s

3d 4p 5s 4d 5p 6s

4f 5d 6p 7s 5f 6d 7p


Electron configurations1

Electron Configurations

  • Three methods

    1. Electron Configuration Notation

    2. Noble Gas Notation

    3. Orbital Diagrams


Electron configuration not ation

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


Electron configuration notation

Electron Configuration Notation

  • You try … Zinc


Electron configuration notation1

Electron Configuration Notation

1s2 2s22p6 3s23p6 4s23d10


Assignment

Assignment

  • Write the electron configuration notation for the following elements:

    • Boron (B), Neon (Ne), Sulfur (S), Magnesium (Mg), Vanadium (V), Silver (Ag)


Noble gas notation

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


Noble gas notation1

Noble Gas Notation

  • [Xe]6s2 4f14 5d9

  • Check: (Xe’s atomic number) 54 + 2 + 14 + 9 = 79 (gold’s Atomic number)!


You try

You Try…

  • Silver


Assignment1

Assignment

  • P.147 #79


Orbital diagrams

Orbital Diagrams

  • Draw a line for each orbital

  • Designate each electron with an arrow

    • = orbital with 1 electron

    • = orbital with 2 electrons


Orbital diagrams1

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


Orbital diagrams2

Orbital Diagrams

  • You try another example: Cu


Orbital diagrams3

Orbital Diagrams

  • Answer


Assignment2

Assignment

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


Electron dot structures

Electron Dot Structures

  • Valence electrons

    • Electrons in outermost energy level.

    • Responsible for chemical properties


Electron dot structures1

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)


Electron dot structures2

Electron Dot Structures


Assignment3

Assignment

  • P.141 #23(yellow box), 26, 28

  • P.147 #81


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