Quantum Electron Configurations

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Presentation transcript:

Quantum Electron Configurations

Erwin Schrödinger 1887 - 1961

The Schrödinger Equation

Werner Heisenberg 1901 – 1976

Bohr Theory The electron is a particle that must be in orbital in the atom. Quantum Theory The electron is like a cloud of negative energy or a wave. Orbitals are areas in 3D space where the electrons most probably are. The energy of the electron is in its vibrational modes- like notes on a guitar string. Photons are produced when high energy modes change to lower energy modes

S orbitals Each orbital holds 2 electrons

S orbitals S

Animation P orbitals There are 3 suborbitals Each contains 2 electrons Total electrons = 6 Animation

P Orbitals

P Orbitals

D orbitals There are 5 suborbitals Each contains 2 electrons Total electrons = 10

D orbitals

F orbitals There are 7 suborbitals Each contains 2 electrons Total electrons = 14

F orbitals

Quantum Periodic Table 1s2 F 2s2 2p5 Count the electrons in each different orbital type until you get to Fluorine. Put in order of lowest to highest energy level.

1. F The Electron Configuration 1s22s22p5 Principle Quantum Number Number of Electrons in the Orbital Orbital Type- s, p, d, or f

Quantum Periodic Table 1s2 2s2 2p6 3p6 3s2 Ca 4s2

2. Ca 1s22s22p63s23p64s2 1s2 2s22p6 3s23p6 4s2 2 8 8 2 Simplify to a Bohr electron configuration

Quantum Periodic Table 1s2 2s2 2p6 3p6 3s2 Cu 3d9 4s2

3. Cu 1s22s22p63s23p63d94s2 Simplify to a Bohr electron configuration 1s2 2s22p6 3s23p63d9 4s2 2 8 17 2

Quantum Periodic Table 1s2 2s2 2p6 3p6 3s2 4p6 Kr 3d10 4s2 Count the electrons in each different orbital type until you get to Kr. Put in order of lowest to highest energy level.

4. Kr 1s22s22p63s23p63d104s24p6 Simplify to a Bohr electron configuration 1s2 2s22p6 3s23p63d10 4s24p6 2 8 18 8

Quantum Periodic Table 1s2 2s2 2p6 3p6 3s2 4p6 3d10 4s2 5s2 4d4 Mo

4. Mo 1s22s22p63s23p63d104s24p64d45s2

Quantum Periodic Table 1s2 2s2 2p6 3p6 3s2 4p6 3d10 4s2 5s2 4d10 5p5 I

5. I 1s22s22p63s23p63d104s24p64d105s25p5 Simplify to a Bohr electron configuration 1s2 2s22p6 3s23p63d10 4s24p64d10 5s25p5 2 8 18 18 7

Why does the 4s fill before the 3d? 4p 3d 4s 3p 3s

Quantum Periodic Table 1s2 2s2 2p6 3p6 3s2 4p6 4s2 3d10 5s2 4d10 5p6 Ba2+

6. Ba2+ 1s22s22p63s23p63d104s24p64d105s25p6 Xe I- The above chemical species are isoelectronic- same electron configuration

Ishihara Test for Colour Blindness – if you can read all of the numbers you have good colour vision Atomic Theory Song

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