Term
| Assumptions for "Ideal Gases" |
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Definition
High Temperature with Low Pressure
No intermolecular forces
Elastic Collisions
Molecules have no mass or volume |
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Term
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Definition
| Weak forces between nonpolar or polar molecules. |
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Term
Van der Waals:
Dipole-Dipole |
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Definition
Between 2 polar molecules.
A negative to positive attraction. |
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Term
Van der Waals:
Dipole-Induced Dipole |
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Definition
| A nonpolar molecule is affected by the polarity of another molecule. A dipole is created int he nonpolar molecule. |
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Term
Van der Waals:
London Dispersion |
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Definition
The electron cloud is stretched: (-) electrons are attracted to the (+) nuclei of a neighboring molecule.
Occurs in nonpolar molecules.
Effect increases with greater mass/electrons/protons. With more electrons, outer electrons are held loosely. |
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Term
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Definition
Between an ion and polar molecule. An attraction of charge.
Ex: salt dissolving in water.
Cations have stronger attraction than anions. Smaller cations have stronger attraction that larger ones (fewer (-) electrons) |
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Term
| Ionic vs. Molecular forces |
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Definition
| Ionic forces are always stronger than molecular ones. |
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Term
Hydrogen Bonding
(Van der Walls) |
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Definition
Lone pairs of electrons are attracted to neighboring hydrogen.
Special, strong Van der Walls.
Occurs with large electronegative atoms: F, O, N |
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Term
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Definition
Usually a gas, but at low temperatures, solid.
Becomes a solid when IMFs increase.
Has dispersion, dipole and/or hydrogen bonds. |
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Term
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Definition
Sea of electrons--electrons are freely shared. Delocalized bonding.
Causes metallic flexibility. |
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Term
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Definition
An array of covalent bonds.
Material comes off in sheets like mica. |
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Term
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Definition
| Cations and anions are held together by charge (electrostatic) attraction. Lattice pattern with alternating + and - ions. |
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