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Chem 101

Quiz

TermDefinition
London Dispersion Forces (LDFs) Are attractive forces that are present in all species, mostly with non-polar molecules or with no permanent dipole
Temp. Dipole Electrons are distributed asymmetrically. Result in a weak electrostatic attraction between the species
Induced Dipole The presence of this dipole distorts the electrons of a neighboring atom or molecule. Result in a weak electrostatic attraction between the species.
LDFs Examples F2, CH4 , Ne, C6H12
Dipole-Dipole Attractions The electrostatic forces between the partially positive end of one polar molecule and the partially negative end of another. Both molecules must be polar
Dipole-Dipole Examples H2O, PH3, HCl
Hydrogen Bonding A stronger type of dipole-dipole interaction observed in molecules with F-H, O-H, or N-H bonds. The H bonded to these very electronegative atoms interacts with other highly electronegative atoms (N, O, F) in other molecules
H-Bond Examples H2O, NH3, HF
Ion-Dipole Attractions Are forces that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole (polar).
Ideal Gas Law Relates the pressure, volume, temperature, and number of moles of a gas. PV=nRT
Boyle’s Law Applies at constant temperature; when the volume of a given amount of gas is decreased, the molecules will be exposed to a decreased container wall area and will exert more pressure against the walls of the container. P1V1=P2V2
Charles’s Law Applies at constant pressure; as the temperature of a gas is increased, a constant pressure may be maintained only if the volume occupied by the gas increases. V1/T1=V2/T2
Avogadro’s Law Applies at constant pressure and temperature; when increasing the number of gaseous molecules will require a proportional increase in the container volume. V1/N1=V2/N2.
Created by: user-1864799
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