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Electronic Structure of the Atom

Electronic Structure of the Atom. Electrons  Bonding  Properties. Bohr ’ s Model. Proposed that electrons in a H-atom could only exist in specific energy states.

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Electronic Structure of the Atom

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  1. Electronic Structure of the Atom Electrons  Bonding  Properties

  2. Bohr’s Model • Proposed that electrons in a H-atom could only exist in specific energy states. • Electrons could move from one orbit to another by absorbing or emitting specific amounts of energy called a “QUANTUM”, corresponding to the energy differences between the orbits.

  3. THEORY OF QUANTUM MECHANICS • Electrons occupy particular regions of space called ORBITALS, in a particular energy level.

  4. Energy Level Diagram for H (Hebden pg 152) • Quantum Number = n

  5. Orbital • For each orbital, the maximum number of electrons you can have is 2!

  6. Analogy • Pauli Exclusion Principle • Bus scenario: You only sit with someone (seats for 2 occupants) when there are no other seats left. • Fill up the same energy level first with 1 electron, before you pair it up with the 2nd electron

  7. Analogy • Analogy: Filling a bottle of jam  Fills up the bottom (representing the lower energy) before moving higher up the bottle (the next higher energy level) • Fill up the lower energy shells first before you move up to the next higher energy level

  8. Definitions • Shell = the set of all orbitals all having the same n-value. Eg. 3rd shell consists of 3s, 3p, 3d orbitals • Subshell = a set of orbitals of the same type Eg. The set of five 3d-orbitals is a subshell

  9. Rules: Types of Orbitals Possible

  10. Rules: Orbitals

  11. Orbital Shapes (Do NOT memorize, this is extra info)

  12. Problem… The energy level diagram Bohr had only worked for H, 1 electron... What about polyelectronic atoms?

  13. Energy Level Diagram for Polyelectronic Atoms (Hebden pg 153)

  14. Electronic Configuration A description of how the electrons of an atom are arranged into orbitals.

  15. Electronic Configuration: 2 Rules You MUST know!! • Electrons are added to the orbitals having the LOWEST energy first. The order in which orbitals are filled is: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p… (Do not memorize these energy levels! Just fill up your subshells by following their orders in the periodic table  Next Slide “Subshells in the Periodic Table”) 2) A maximum of 2 e can be placed in each orbital. This means there can be a maximum of 2e in s-type subshell, 6e in p-type subshell, 10e in d-type subshell, 14e in f-type subshell

  16. Subshells in the Periodic Table (Hebden pg 155)

  17. Practice Problems: Write Electronic Configuration for the following • He • Li • O • Cl

  18. Homework • Hebden Unit VIII: Do Question 26 (a) to (o) (pg 155)

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