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37 Cards in this Set
- Front
- Back
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Electron pair geometry |
You simply count the number of outer atoms and decide from there the shape. Each lone pair will take the shape up another step... |
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Linear |
Two outer atoms. |
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Triginal planer |
3 outer atoms. Or 2 outer atoms and one lone pair on the central atom! |
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Tetrahedral |
4 outer atoms. Or 3 outer atoms + 1 lone pair Or 2 outer atoms + 2 lone pairs |
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Trigonal bipyramidal |
5 outer atoms Or 4 outer atoms + 1 lone pair Or etc......... |
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Polar |
The atom is assametric Ex: H------N:--------H | H |
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Non polar |
The atom is symetric, no electrons on the central atom. |
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Hydrogen bonding |
H is attached to N, O, or F |
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Ionic bonding |
It's an ionic molecule |
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Dipole-Dipole |
Polar Assymetric |
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Dispersion/London/Van Der Waals |
Weakest Non-polar Symetric |
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Covalent |
Two non-metals |
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Ionic |
Metal + non-metal. |
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Boiling point |
Bigger molecule = Higher BP = Higher IMF |
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Intermolecular Forces |
- Forces between molecules (Two or more molecules interact) - Deals with physical properties |
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Intramolecular Forces |
Forces between atoms in a molecule (Atoms doing stuff in a single molecule) |
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High IMF |
High BP High viscosity (thickness) High Surface Tension High Melting Point (Hard to seperate the molecules) |
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Low IMF |
High Vapor Pressure (Can be separated easily) |
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Bond Order |
Sigma bonds happen first and then Pi bonds happen. |
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Electronegativity |
Decreases from right to left Decreases from top to bottom |
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Surface tension |
the tendency of a liquid to possess elasticity at its surface |
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Capillary action |
movement of a liquid through a narrow tube because of attractive forces between the liquid and the container |
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Cohesion |
The attractive forces between a single type of molecule (Intermolecular forces, Dispersion forces, Hydrogen bonding) |
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Adhesion |
the attractive forces between two different types of molecules |
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Meniscus |
curvature at the liquid-container interface |
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Paramagnetic |
One electron is unpaired it has a weird net spin |
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Diamagnetic |
All electrons are paired |
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Polar Covalent |
Moderate Electronegativity difference. Electrons unequally shared. |
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Pure Covalent |
Little-to-no Electronegativity difference. Electrons shared equally. |
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Electron vs molecular geometry |
Molecular geometry only pays attetion to bonds, not lone pairs |
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Types of bonding |
Non-polar Covalent Polar Covalent Ionic Hydrogen Dipole-Dipole Dispersion |
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Hybrid Orbitals |
sp, sp^2, sp^3, sp^3d, sp^3d^2 This is talking about electron geometry, so focus on how many areas of high density it has. Doesn't matter for this if they're lone pairs or not. (INCLUDE LONE PAIRS THOUGH) |
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Types of solids |
Covalent/Network Solids Ionic Solids Metallic Solids Molecular Solids |
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Covalent/Network Solids |
Strongest Covalent bonding |
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Ionic Solids |
Second strongest Ionic bonding |
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Metallic Solids |
Third strongest Mostly pure metal, but can be mixed. |
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Molecular Solids |
Weakest Held together by IMF basically two molecules held together. |
