1. Aim: How are an atom’s electrons configured?
Electromagnetic Spectrum -the total range of light including gamma rays, x-rays, ultraviolet, visible, infrared, microwaves, and radio waves.
Orbital- region where electron can most likely be found.
Ground state- when electron is in a state of lowest possible energy
Excited state- when electron acquires additional energy. An electron can only absorb a discrete, or fixed amount of energy that would allow it to move to a higher energy level.

2. Aim: How are an atom’s electrons configured?
Emission Spectrum- visible light produced by electrons. Each atom has its own distinct pattern of emission lines (or bright line spectrum), and these spectra are used to identify elements.
Electron configuration-distribution of electrons

3. Aim: How are an atom’s electrons configured?
Essential Questions:
Explain how the wavelengths of light emitted by an atom provide information about electron energy levels.
How did Bohr explain the presence of line-emission spectra?
Compare the quantum models of Rutherford an Bohr.