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Quantum numbers:
Each electron has a set of four numbers, called quantum numbers
Pauli Exclusion Principle
Principal quantum number (house) sublevel (floor of room) orbital (your room) electron spin (you in your room)
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Principle Quantum Number (n)
Corresponds to energy level
Describes the size of the electron cloud
As you move farther from the nucleus, energy increases.
Energy levels are not evenly spaced out. The higher the energy level, the farther it’s spaced out
To determine maximum number of electrons in an energy level, where n = energy level, 2n2
Each energy level contains sublevels
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Sublevel (l)
n = 1 | 1 sublevel | s |
---|---|---|
n = 2 | 2 sublevels | s, p |
n = 3 | 3 sublevels | s, p, d |
n = 4 | 4 sublevels | s, p, d, f |
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Letter | Shape | # orientations | Max electrons |
---|---|---|---|
S | spherical | 1 | 2 |
P | dumbell | 3 | 6 |
D | double dumbbell (cloverleaf) | 5 | 10 |
F | too complex | 7 | 14 |
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Every orientation has a maximum of 2 electrons. (# orientations * 2 = max electrons)
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Orbital (ml)
Letter | # orbitals | # electrons |
---|---|---|
S | 1 | 2 |
P | 3 | 6 |
D | 5 | 10 |
F | 7 | 14 |
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Electron Spin (ms)
Describes the spin of an electron
Tells exact location
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Properties of Electrons:
Letter | Energy levels they can exist at | # orbitals | # electrons |
---|---|---|---|
S | 1st and higher | 1 | 2 |
P | 2nd and higher | 3 | 6 |
D | 3rd and higher | 5 | 10 |
F | 4th and higher | 7 | 14 |
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Rules for filling orbitals:
Aufbau Principle: Electrons always fill the lowest energy levels first.
Pauli Exclusion Principle: No two electrons with the same energy characteristics can occupy an orbital at the same time
Hund’s Rule: When filling multiple orbitals of the same sublevel (P, D, F) electrons half-fill the sublevel first before pairing electrons
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Directions:
read the periodic table LEFT to RIGHT
stop once you get to the element
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Ions:
Cations - lose electrons
Anions - gain electrons
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Electrons configuration:
metals go BACK to the LAST noble gas. non-metals go FORWARD to the NEXT noble gas
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Lewis Dot Diagrams (non-hybridized)
ONLY Valence electrons (s & p)
Write the abbreviated configuration
Fill in (s) first
Draw in the (p) dots until you have a total of the # of valence electrons (left to right) OR you run out of (p)s
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Orbital Filling Diagrams
Use a square, underscore, or circle. This represents an orbital
Fill orbitals one at a time (like the Lewis Dot Diagram)
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