H spectra 656 nm 486 nm 434 nm 410 nm

Ne spectra 540.1green 585.2yellow 588.2yellow 603.0orange 607.4orange 616.4orange 621.7red-orange 626.6red-orange 633.4red 638.3red 640.2red 650.6red 659.9red 692.9red 703.2red

Energy levels and H bright line spectrum Energy sp d f energy IR teal UV “ground state” “excited state” n animation: orbital shapes and spectra

Energy levels and H bright line spectrum Energy sp d f energy V teal UV “ground state” “excited state” n animation: orbital shapes and spectra energy

Ne spectra 540.1green 585.2yellow 588.2yellow 603.0orange 607.4orange 616.4orange 621.7red-orange 626.6red-orange 633.4red 638.3red 640.2red 650.6red 659.9red 692.9red 703.2red

Neon bright line spectrum Energy sp d f Joules Neon: 10 electrons Ne: 1s 2 2s 2 2p 6

Neon bright line spectrum Energy sp d f Joules Neon: 10 electrons “Ground state” Ne: 1s 2 2s 2 2p 6 energy an “excited state” Ne: 1s 1 2s 1 2p 3 3p 1 4p 1 5s 1 5f 1 6p 1

Why do we get only distinct lines in the atomic emission spectrum? Make a concept map: –Ground state –Excited state –Energy level –Electron –Energy –Frequency –Wavelength –light: visible, UV, IR –orbital

Bright line (emission) spectra hydrogen mercury

Energy levels and H bright line spectrum Energy sp d f energy V teal UV “ground state” “excited state” n animation: orbital shapes and spectra Dr. Quantum double slit electrons as waves...Quantum Mechanics!! energy

Neon bright line spectrum Energy sp d f Joules Neon: 10 electrons Ne: 1s 2 2s 2 2p 6

Neon bright line spectrum Energy sp d f Joules Neon: 10 electrons “Ground state” Ne: 1s 2 2s 2 2p 6 energy an “excited state” Ne: 1s 1 2s 1 2p 3 3p 1 4p 1 5s 1 5f 1 6p 1

Energy sp d f Neon: 10 electrons Ne: 1s 2 2s 2 2p 6 Energy sp d f Mercury: 80 electrons Different atoms have different “empty” energy level diagrams

Hg spectra nm (blue), nm (green), and a pair at nm and nm (yellow- orange). There are two other blue lines at nm and nm and a weak line at nm.