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Quantum-Mechanical Model
pg. 294-301
LO: I can write the electron configuration of elements in the PT.
What is the quantum-mechanical model?
A model that explains...The probability of where an electron exists
when orbiting the nucleus.
With a focus on...The energy of the electrons
Bohr Model vs. Quantum-Mechanical Model
Bohr
Orbits—circular path around the nucleus showing the electrons motion.
Differently sized radii
Quantum-Mechanical
Orbitals—probability map showing likelihood of where an electron will be found.
Differently sized shapes
Quantum Numbers
• Used to specify an electron’s “address”• 4 total numbers
1. Energy level “n”2. Sublevel “shape”3. Orientation of sublevel orbitals4. Spin of electrons in sublevel orbitals “ms”
QN1: Energy Levels
1. Energy level “n” n = 1, 2, 3, 4, 5, 6, 7The higher the number, the
farther the e- is from the nucleus.
QN2: Sublevel Shape
2. Sublevel “shape” s = spherical p = lobed d = dumbbell f = “complicated”
There are as many sublevels as the number of the level.
QN3: Orientation
3. Orientation of sublevel s = 1 orientation p = 3 orientations d = 5 orientations f = 7 orientations
QN4: Electron Spin
4. Electron Spin “ms” s = p = d = f =
Hund’s Rule: Electrons occupy sublevels one at a time before filling up with a second electron.
Pos. Spin= Neg. spin=
Electron Configurations (addresses)
Electron Configuration: Tells us the location of an electron in the electron cloud.
Pauli Exclusion Principle: No two electrons have the same configuration (address).
Aufbau Principle: Electrons will occupy the lowest energy position (sublevel) available. (like tennis balls filling a tube)
Aufbau Principle: How orbitals are filled
Complete the half-sheet and insert it into your ISN
Electron Configuration ExamplesProcess
1. Determine the # of electrons
2. Fill up electrons in each energy sublevel
Lowest Highest 3. Don’t forget
Hund’s RuleHW: Worksheet write the first 20 element electron
configurations due (Monday 11/16)