orbitals - orbitals o o o o o o o s orbital - lowest energy...

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orbitals    s orbital - lowest energy orbital, has spherical symmetry o ψ 2 approaches 0 as it gets farther apart from nucleus o nodes - regions where ψ 2 goes to 0 o orbital size increases as n increases p orbital - has dumbbell shaped orbital w/ 2 lobes o shape shows average distribution of electrons, not its path o every shell beyond the 1st has 3 p orbitals, each w/ different spatial orientation d orbital - occur beyond 1st 2 shells o 5 different d orbitals f orbital - occur beyond 1st 3 shells o 7 different f orbitals in atoms w/ multiple electrons, repulsions cause different subshells to be at different energies degenerate orbitals - orbitals w/ same energy Pauli exlusion principle  - no 2 electrons can have same set of quantum numbers (n, l, m l , m s )   electron spin - property of electrons where each electron spins on an axis spin generates magnetic field m s = +1/2 or -1/2, spin magnetic quantum number each orbital can hold 2 electrons, as long as they spin in opposite directions
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orbitals - orbitals o o o o o o o s orbital - lowest energy...

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