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Electron Configurations Objective: express the arrangement of electrons in atoms through electron configurations and Lewis valance electron dot structures. Electron Locations • According to the Heisenberg Uncertainty Principle we can not know the exact position and motion of electrons with complete certainty. • We can only describe the probable locations of electrons. • We will describe the location of electrons when the atom is at its lowest energy . • These are called “ground state” configurations. • If electrons move to higher energy states this is called “excited.” Quantum Numbers • There are four quantum numbers that describe the location of all electrons in an atom. • No two electrons in the same atom can have the same set of four quantum numbers that describe their location. • This is called the Pauli Exclusion Principle. Quantum Numbers • Erwin Schrodinger produced mathematical equations to describe the wave like behavior of the electron. Principle Quantum Number called Energy Level • Represented by letter “n” • From 1 to 7 for present elements. • Represents the average distance of the electron from the nucleus. • Also represents the amount of energy the electron contains. • 2n2 represents the maximum number of electron per energy level. Angular Momentum Quantum Number Called Sublevel The secondary quantum number “L” gives the shape of the orbital. L=1 is a “s” sublevel L=2 is a “p” sublevel L=3 is a “d” sublevel L= 4 is a “f” sublevel “s” sublevels are the simplest and require the least amount of energy for electrons to occupy. s→p→d→f Electrons will occupy which every energy level and sublevel that takes the least amount of energy. Sublevels • • • • • • • Energy Level 1 2 3 4 5 6 Possible Sublevels s s and p s, p, and d s, p, d, and f s, p, d, f, and g (no g at present) s, p, d, f, g, and h (no g or h) Magnetic Quantum Number Called Orbital • mL has to do with the orientation of an orbital in a magnetic field. Think of this as orientation around the x-y-z axis in 3-dimensional space. • Equal to ( –L to + L) • Sublevel Orbitals Electrons • s 1 2 • p 3 6 • d 5 10 • f 7 14 Spin Quantum Number Called Spin • The final quantum number is the spin quantum number, it describes the spin orientation of an electron. • Two electrons can occupy the same orbital, but they must have different spins. • One positive and one negative. Rules to arrange by. • Heisenberg uncertainty principle. • Pauli exclusion principle. • Hunds Rule: The most stable arrangement is the one with the maximum number of unpaired electrons. • Aufbau: Electrons are “lazy” and will go to the lowest energy level and sublevel combination. Electron Configurations • Electron configuration, orbital notations, and Lewis electron dot diagrams use the quantum numbers to give the locations of electrons in atoms. • No two atoms will have the same electron configuration. • This is why all atoms have a different bright line spectrum.