What to know for the test:
4.1
1. Define electromagnetic spectrum, electromagnetic wave, wavelength, frequency, photon, ground state, excited state, s orbital, p orbital, d orbital, f orbital, electron configuration, noble gas electron configuration
2. know that when electrons are excited they absorb energy and move from a lower to higher energy level which initiates a tug of war between the energy added to the atom and the pull of the nucleus. The vibration of the electron between energy levels causes the (emission) release of photons and a steady stream of photons creates a wave.
4.2
3. In chemistry, the part of quantum numbers that is significant to us is that in the ground state, energy levels 1, 2, 3, 4, 5, 6, 7 are the only ones needed to accommodate the electrons of all of the atoms on the periodic table. Electrons will take one of four shape orbits about the nucleus, they are s, p, d & f's. There is only one way to do an s at each energy level and two electrons can fit in that orbit. There are 3 ways to do a p at energy levels 2 and up. The p orbitals can accommodate 6 electrons at each energy level. There are 5 ways to do a d at energy level 3 and up and 10 electrons can be accommodated at each of those levels. Finally there are 7 ways to do an f orbit at energy levels 4 and up, with 14 electrons accommodated.
4. In each orbital one electron spins clockwise and the other counter clockwise causing the repulsive electrons to attract magnetically.
4.3
5. Be able to write long hand and noble gas electron configurations with or without electron boards.
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