Term
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Definition
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Term
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Definition
| forces that cause the aggregation of the components of a substance to form a liquid or a solid. (Does not include covalent or ionic bonding) |
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Definition
| molecules with dipole moments can attract each other electrostatically by lining up so the positive and negative ends are close to each other |
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Term
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Definition
dipole-dipole attractions between H and N, O, or F
because H is so small, they can get close and N, O, F are highly electronegative |
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| London dispersion forces (LDF) |
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Definition
| Forces between noble gases and nonpolar molecules because of an instantaneous dipole moment. Significant for big molecules. |
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Definition
| electrons move around and the nonsymmetrical electron distribution can affect the electron distribution of a close atom. |
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Definition
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Definition
| low compressibility, lack of rigidity, high density, |
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| Why liquid droplet is a sphere? |
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Definition
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Definition
| Resistance of a liquid to an increase in its surface area |
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Definition
| spontaneous rising of a POLAR liquid in a narrow tube |
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Definition
| Forces between molecules of the liquid. Surface tension and capillary action. |
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Definition
| forces between liquid molecules and their container |
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Term
| why water creeps up sides of glass tube? |
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Definition
| because its adhesive forces are stronger than its cohesive forces, forming a concave shape of the meniscus |
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Term
| what raises boiling points? |
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Definition
H bonds, ionic forces, LDF (larger molecule has more), dipole-dipole forces.
Basically, all the forces |
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Term
| the forces that occur between two polar molecules |
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Definition
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Term
| the force between a noble gas and a nonpolar molecule |
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Definition
| London Dispersion Forces (LDF) |
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Term
| bonding between N, O, or F and H |
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Definition
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Term
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Definition
| atoms, molecules, or ions occupy the lattice positions |
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Term
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Definition
| molecules occupy the lattice points |
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Definition
| ions occupy the lattice points |
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Term
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Definition
| atoms occupy the lattice points |
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