My notes and thoughts from Biology 111, for Wednesday, August 27, 2008. The entire series can be found here.
Wednesday’s lecture began with a review of atomic structure, including a reminder that our e– * diagrams are 2D representations of 3D space.
Then we moved on to some more basic chemistry.
We focused mostly on electrons, and will continue to, as electrons are what determines reactivity of an atom, and reactivity is what’s really vital to biology.
e– orbits are called e– shells or energy levels. Each e– orbital can hold up to 2 e–.
The first energy level has one orbital, because it’s so small, and electrons, having all the same negative electrical charge, repel each other.
The second and third energy levels each contain 4 orbitals, each energy level then is capable of holding 8 e– (2 e– in each orbital).
Then doc talked about how electrons fill from the innermost energy level, out.
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