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Chapter 3 - Intermolecular Forces
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33 Terms
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1
Intermolecular Forces
Forces of attraction between molecules.
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2
Intramolecular Force
Within a molecule, holds atoms together.
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3
Ionic Bonds
Bonds formed by the electrostatic attraction between oppositely charged ions.
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4
Covalent Bonds
Bonds formed by the sharing of electrons between atoms.
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5
Non-polar covalent
Electrons are equally shared between atoms.
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6
Polar covalent
Electrons are unequally shared between atoms.
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7
Dipole-Dipole Forces (DDF)
Attractive forces between polar molecules due to positive and negative dipoles.
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8
Hydrogen Bonding (H-bond)
A stronger type of dipole-dipole interaction involving H bonded to N, O, or F.
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9
London Dispersion Forces (LDF)
Weak attractive forces present in all molecules due to temporary dipoles.
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10
Polarity
A molecule's property that determines how it interacts with other substances.
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11
Hydrogen chloride
Chemical compound with the formula HCl; a polar molecule.
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12
Gecko feet
Utilize a large amount of London dispersion forces for adhesion.
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13
Density of water
Solid form of water is less dense than its liquid form due to hydrogen bonding.
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14
Solubility
Ability of a substance to dissolve in a solvent; 'like dissolves like' principle.
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15
Melting point
The temperature at which a solid becomes a liquid.
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16
Boiling point
The temperature at which a liquid becomes a gas.
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17
Electronegativity
A measure of an atom's ability to attract electrons in a bond.
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18
Surface tension
The tension of the surface film of a liquid caused by intermolecular forces.
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19
Viscosity
A measure of a fluid's resistance to flow.
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20
Partial charges
Uneven distribution of electron density resulting in regions of slight positive and negative charge.
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21
Open lattice structure
Arrangement of molecules in solid form that can trap air, making it less dense.
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22
Fluctuating dipole
Temporary charge imbalance in a molecule that induces dipoles in neighboring molecules.
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23
Polar solvents
Solvents that can dissolve polar solutes.
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24
Non-polar solvents
Solvents that can dissolve non-polar solutes.
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25
Strength of LDF
Increases with the size of the molecule; larger molecules have more electrons.
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Important unique properties of water
High melting and boiling points due to hydrogen bonding.
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27
Behaviors of hydrocarbons
Hydrocarbons are generally non-polar and experience London dispersion forces.
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28
Group 14 Hydrides
Compounds with a hydrogen bond with elements from group 14, often non-polar.
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29
Physical properties dictated by IMF
Include state of matter, melting/boiling point, hardness, and solubility.
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30
Homework assignments
Specific problems assigned from textbook pages for practice.
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31
Anomaly in boiling point trend
Unexpected results regarding boiling points as size increases by group.
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32
Observations in molecular interactions
The study of how molecules influence one another based on their structure.
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33
Effective molecular interactions
Affects the solubility, viscosity, and boiling/melting points of substances.
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