Ch 1

• Ground state is the lowest possible energy state of an atom
• Excited state is an atom that has more energy than the ground state
• The Bohr radius is the radius of the atom in the ground state.
• Wave equations use quantum numbers: principal, azimuthal, magnetic, spin
• Principal energy levels are represented by the principal quantum number
• Sublevels are represented by the azimuthal quantum number
• Sublevel equation: n-1
• l=0 is sublevel s
• l=1 is sublevel p
• l=2 is sublevel d
• l=3 is sublevel f
• An orbital contains a maximum of two electrons
• The number of orbitals is determined by the equation 2l+1
• Each orbital is given a number, called the magnetic quantum number
• The possible values of the magnetic quantum number range from -l to +l
• In total, the f sublevel has orbitals of -3 to +3, therefore holds 14 total electrons
• In total, the d sublevel has orbitals of -2 to +2, therefore can hold 10 electrons
• In total, the p sublevel has orbitals of -1 to +1, therefore can hold 6 electrons
• The azimuthal quantum number provides the shape of the orbital
• The s sublevel is spherical shaped
• The p sublevel is dumbbell shaped
• The aufbau ordering fills sublevels based on lowest energy level
• Electronic configurations include complete and abbreviated
• The spin quantum number is either -1/2 or +1/2
• The principal quantum number represents the average distance of the electron to the nucleus, or the size of the principal energy level
• The magnetic quantum number represents the orientation of each orbital in space
• From left to right, the order of periodic table is s, f, d, p
• Lyman series= UV light
• Balmer series= visible light
• Paschen series= infrared light