part 1
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| what does covalent bonds determine? | molecular shape, bond energies, chemical properties
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| Intermolecular forces (non-covalent bonds) influences what? | physical properties of liquids and solids
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| the lack of significant attractive force between gas molecules, allow a gas to do what? | to fill its container
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| What if the attractive forces of gas molecules become significant? (like under high pressure) | the gases exhibit non-ideal behavior
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| 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
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| crystalline | the molecules in a solid adopt a packing arrangement
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| Why are solid rigid? | because of the strong intermolecular forces between neighboring molecules
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| kinetic energy | keeps molecules apart and moving around
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| intermolecular forces try to do what? | draw particles together
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| what 2 things can change the state of a substance | temperature and pressure
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| heating and cooling can change the (blank) of particles in a substance | kinetic energy
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| how does increasing the P increase the strength of intermolecular forces? | by forcing the molecules closer together
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| what if you increase the pressure on a liquid? | it may change to a solid
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| What if you decrease T and increase P? | the molecules are closer (tighter) together
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| what if you increase T and decrease P? | the molecules are farther from each other
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| is intermolecular force weaker or stronger than covalent bonds? | weaker
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| How does a molecular substance states while the atoms within the molecule are unchange? | because intermolecular bonds are much weaker than covalent bonds.
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| the temperature at which liquid boils reflects what? | the kinetic energy needed to overcome the attractive intermolecular force
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| the strength of the intermolecular forces determines what? | the physical properties of the substance
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| Name the attractive forces between neutral molecules | dipole-dipole, London dispersion, hydrogen bonding
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| van der Waals forces | dipole-dipole and dispersion forces
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| name the force between neutral and charged (ionic) molecules | ion-dipole forces
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| 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;
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| dipole-dipole forces | between neutral polar molecules; weaker than ion-dipole forces;
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| for substances with similar molecular mass, how do you increase its boiling point? | by increasing dipole moment
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| London dispersion force are only significant when atoms are | close together
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| polarizability means what? | how easy it is for an electric field to induce a dipole with a molecule
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| dispersion forces increase with what? | with increasing molecular mass
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| hydrogen bonding | a hydrogen atom experience an attractive force with a neighboring electronegative molecule/ion which has an unshared pair of electrons
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| Are hydrogen bonds weak or strong? | weaker than typical covalent bonds, but stronger than dipole-dipole and/or dispersion forces
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| dispersion force increase in strength with what? | increasing molecular weight
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To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
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