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Intermolecular force
part 1
| Question | Answer |
|---|---|
| what does covalent bonds determine? | molecular shape, bond energies, chemical properties |
| Intermolecular forces (non-covalent bonds) influences what? | physical properties of liquids and solids |
| the lack of significant attractive force between gas molecules, allow a gas to do what? | to fill its container |
| What if the attractive forces of gas molecules become significant? (like under high pressure) | the gases exhibit non-ideal behavior |
| why can liquid assume the shape of their containers? | because the attractive forces are not strong enough to keep neighboring molecules in a fixed position and molecules are free to move past or slide over one another |
| crystalline | the molecules in a solid adopt a packing arrangement |
| Why are solid rigid? | because of the strong intermolecular forces between neighboring molecules |
| kinetic energy | keeps molecules apart and moving around |
| intermolecular forces try to do what? | draw particles together |
| what 2 things can change the state of a substance | temperature and pressure |
| heating and cooling can change the (blank) of particles in a substance | kinetic energy |
| how does increasing the P increase the strength of intermolecular forces? | by forcing the molecules closer together |
| what if you increase the pressure on a liquid? | it may change to a solid |
| What if you decrease T and increase P? | the molecules are closer (tighter) together |
| what if you increase T and decrease P? | the molecules are farther from each other |
| is intermolecular force weaker or stronger than covalent bonds? | weaker |
| How does a molecular substance states while the atoms within the molecule are unchange? | because intermolecular bonds are much weaker than covalent bonds. |
| the temperature at which liquid boils reflects what? | the kinetic energy needed to overcome the attractive intermolecular force |
| the strength of the intermolecular forces determines what? | the physical properties of the substance |
| Name the attractive forces between neutral molecules | dipole-dipole, London dispersion, hydrogen bonding |
| van der Waals forces | dipole-dipole and dispersion forces |
| name the force between neutral and charged (ionic) molecules | ion-dipole forces |
| Ion dipole force | charged ion and polar molecule interaction; cations are attracted to the neg. end of the dipole and anion to the pos. end; |
| dipole-dipole forces | between neutral polar molecules; weaker than ion-dipole forces; |
| for substances with similar molecular mass, how do you increase its boiling point? | by increasing dipole moment |
| London dispersion force are only significant when atoms are | close together |
| polarizability means what? | how easy it is for an electric field to induce a dipole with a molecule |
| dispersion forces increase with what? | with increasing molecular mass |
| hydrogen bonding | a hydrogen atom experience an attractive force with a neighboring electronegative molecule/ion which has an unshared pair of electrons |
| Are hydrogen bonds weak or strong? | weaker than typical covalent bonds, but stronger than dipole-dipole and/or dispersion forces |
| dispersion force increase in strength with what? | increasing molecular weight |
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