Atomic Spectra Ground vs Excited state Do Now

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Atomic Spectra Ground vs. Excited state Do Now: For the element Bromine, write the:

Atomic Spectra Ground vs. Excited state Do Now: For the element Bromine, write the: a) Electron configuration (Bohr configuration) b) Electron configuration with orbitals (quantum mechanical configuration) c) Orbital notation d) Ionic charge e) Lewis dot diagram for the atom f) Lewis dot diagram for the ion

Energy levels • Electrons in the “ground state” are at the lowest possible energy

Energy levels • Electrons in the “ground state” are at the lowest possible energy • Electrons in the “excited state” are NOT at lowest possible energy • Electrons absorb energy to get from ground to excited state • Electrons release energy in the form of light “spectra” when they return to the ground state from the excited state. • Each element has its own characteristic spectra.

Absorb Energy Ground State Excited State Release Energy

Absorb Energy Ground State Excited State Release Energy

Example • The electron configuration for Chlorine in the ground state is 2 -8

Example • The electron configuration for Chlorine in the ground state is 2 -8 -7 or 1 s 22 p 63 s 23 p 5. • A possible excited state configuration is 2 -7 -8 or 1 s 22 p 53 s 23 p 6. • What is another possible excited state configuration? • Why is 1 -9 -7 not a possible configuration?

• What is the ground state electron configuration for carbon? • What is

• What is the ground state electron configuration for carbon? • What is a possible excited state electron configuration for carbon? v. Remember…. v. The excited state should have the SAME number of electrons are the ground state v. Each energy level has a maximum number of electron…don’t exceed the max!