Chapter 5 Electrons in Atoms

Light and Quantized Energy (5.1) ,[object Object],[object Object],[object Object]

Spectrum Radio waves Microwaves Infrared . Ultra-violet X-Rays Gamma Rays Long Wavelength Short Wavelength Visible Light Low energy High energy Low Frequency High Frequency

Light is a Particle ,[object Object],[object Object]

Atomic Emission Spectrum ,[object Object],[object Object],[object Object]

Prism ,[object Object],[object Object]

If the light is not white ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],[object Object]

An explanation of the Atomic Emission Spectra

Where the electron starts ,[object Object],[object Object]

[object Object],Changing the energy

[object Object],[object Object],Changing the energy

The Bohr Ring Atom n = 3 n = 4 n = 2 n = 1

[object Object],Ultraviolet Visible Infrared

Light is also a wave ,[object Object],[object Object],[object Object]

Heisenberg Uncertainty Principle ,[object Object]

Quantum Theory and the Atom (5.2) ,[object Object],[object Object],[object Object]

Bohr’s Model ,[object Object],[object Object],[object Object],[object Object]

Bohr’s Model Nucleus Electron Orbit Energy Levels

Bohr’s Model ,[object Object],[object Object],Increasing energy Nucleus First Second Third Fourth Fifth }

The Quantum Mechanical Model ,[object Object],[object Object],[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],The Quantum Mechanical Model

Atomic Orbitals ,[object Object],[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],“ S” orbitals

“ P” orbitals ,[object Object],[object Object],[object Object]

“ P” Orbitals (aligned on the x,y,z axis)

“ D” orbitals ,[object Object],[object Object],[object Object]

“ F” orbitals ,[object Object],[object Object],[object Object]

Summary 1 2 3 4 s 1 2 S P d S P D f Energy Level (n) S P Sublevels (S, p, d, f) Number of orbitals (Odd 1,3,5,7) 1 3 2 6 1 3 5 2 6 10 1 3 5 7 2 6 10 14 Maximum Number of Electrons (orbital x 2)

By Energy Level ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Filling order ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Increasing energy 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 7p 3d 4d 5d 6d 4f 5f

Increasing energy 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 3d 4d 5d 7p 6d 4f 5f

Electron Configurations (5.3) ,[object Object],[object Object],[object Object],[object Object]

Electron Configuration ,[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],Increasing energy 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 3d 4d 5d 7p 6d 4f 5f

[object Object],[object Object],Increasing energy 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 3d 4d 5d 7p 6d 4f 5f

[object Object],[object Object],[object Object],[object Object],Increasing energy 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 3d 4d 5d 7p 6d 4f 5f

Easy way to remember - Fill from the bottom up, following the arrows ,[object Object],[object Object],1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f

Rewrite when done ,[object Object],[object Object],[object Object]

Exceptions to Electron Configuration (optional)

Orbitals fill in order ,[object Object],[object Object],[object Object],[object Object],[object Object]

Write these electron configurations ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Chromium is actually ,[object Object],[object Object],[object Object]

Chromium is actually ,[object Object],[object Object],[object Object],[object Object],[object Object]

Copper’s electron configuration ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

In each energy level ,[object Object],[object Object],[object Object],[object Object],[object Object]

Chapter 5 Electrons in Atoms

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Chapter 5 Electrons in Atoms