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CHEM1040
General Chemistry I
| Term | Definition |
|---|---|
| Principle Quantum Number (n) | the main energy level of atom's electrons |
| Orbital Angular Momentum (l) | the shape of the electron orbital |
| Magnetic Quantum Number (ml) | permitted orbitals in any group |
| Spin Quantum Number (ms) | electron spin |
| Pauli's Exclusion Principle | no two electrons can have the same set of quantum numbers, 2 electrons per orbital, same orbital = paired spin |
| Hund's Rule | orbitals with the same momentum number fill from lowest to highest, "all have one before any have two" |
| Diamagnetic | all spins are paired |
| Paramagnetic | at least one unpaired e- |
| Aufbau Rule | electrons are added one by one, orbitals are ordered by increasing energy, all electron orbitals have identical energies |
| Effective Nuclear Charge (Zeff) | increases ↗ |
| Atomic Size | increases ↙ |
| Ionization Energy | increases ↗ |
| Electron Affinity | increases → (generally) |
| Bond Order | indicates the degree of bonding between two atoms, higher bond order = stronger and shorter bond |
| Resonance Structures | different representation of the same bonding |
| AB2 | Linear, 180° |
| AB3 | Trigonal Planar, 120° |
| AB2E | Bent, 120° |
| AB4 | Tetrahedral, 109.5° |
| AB3E | Trigonal Pyrimidal, 109.5° |
| AB2E2 | Bent, 109.5° |
| AB5 | Trigonal Bipyrimidal, 90°, 120°, 180° |
| AB4E | Seesaw, 90°, 120°, 180° |
| AB3E2 | T-Shaped, 90°, 180° |
| AB2E2 | Linear, 180° |
| Diatomic Molecule | non-polar if items are identical, polar otherwise |
| Triatomic Molecule | non-polar if linear with identical atoms, polar otherwise |
| Empirical Formula | defines the mole ratio of the elements simplified to the LCD |
| Molecular Formula | the number of each type of atom in a molecule |
| Molecular Equation | reactants and products are written as molecular substances |
| Complete Ionic Equation | strong electrolytes are written as separate ions in a solution |
| Net Ionic Equation | spectator ions are cancelled out |
| Arrhenius Acid | produces H+ ions |
| Arrhenius Base | produces OH- ions |
| Bronsted-Lowry Acid | proton donor |
| Bronsted-Lowry Base | proton acceptor |
| K<1 | favours reactants |
| K>1 | favours products |
| K=1 | equilibrium |
| Q<K | too few products (shifts right) |
| Q>K | too few reactants (shifts left) |
| Q=K | at equilibrium |
| Le Châtelier's Principle | if a dynamic equilibrium is disturbed, the reaction proceeds to counteract the change and re-establish equilibrium |
| Concentration | +R = shift right, -R = shift left -P = shift right, +P = shift left |
| Partial Pressure | +V = shift to more moles, -V = shift to less moles -P = shift more moles, +P = shift less moles |
| Temperature | Heat as R -> +H = shift right, -H = shift left Heat as P -> -H = shift right, +H = shift left |
| Lewis Acid | electron pair acceptor |
| Lewis Base | electron pair donor |
| Acidic Cations | conjugate acids of weak bases, small, high charge metal ions |
| Neutral Cations | group 1 and 2 cations, +1 charged metals |
| Acidic Anions | HSO4-, H2PO4- |
| Neutral Anions | conjugate bases of strong acids |
| Basic Anions | conjugate bases of weak acids |
| Common Ion Effect | the shift of an ionic equilibrium due to an addition of solute containing ions in the equilibrium |
| Buffer | a solution that resists change in pH, amount between 0.1 - 10 |
| Effective Buffer | pKa +- 1 |
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