Unit 3

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42 Terms

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elastic deformation

temporary change, returns to normal

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plastic deformation

permanent change, but doesn’t break

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ionic solid

strong inter and intramolecular forces

high melting/boiling point

brittle

not conductive unless dissolved in water

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molecular solid

formed by distinct molecules bonded together

strong intramolecular forces, weak intermolecular forces

low melting/boiling point

cannot conduct electricity

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covalent network solid

formed by atoms bonded covalently in a 3d network

indicated by presence of B/Si/Ge + element, C + metalloid, or just C

high melting point

does not conduct electricity

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metallic solid

sea of electrons keeps metal atoms together

malleable/ductile

good conductors of electricity

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dipole-dipole interactions

between polar + polar, increased polarity strengthens

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dipole-induced dipole

polar + nonpolar, temporary, electronegative atom of polar molecule repels electrons, creating partial positive charge

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London Dispersion Forces

nonpolar + nonpolar, present in all IMFs, stronger with larger molecules b/c more polarizable

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hydrogen bonding

H surrounded by F/O/N, type of dipole-dipole, strong

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ion-dipole

negative from dipole connects with positive ion + vice versa

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stronger IMF effect on boiling point, surface tension, heat of vaporization

boiling point- raised

surface tension- raised

heat of vaporization- raised

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volatility

ease of evaporating, stronger IMF lowers

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viscosity

resistance to flow, stronger IMF increases

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vapor pressure

pressure exerted by a gas when it is at equilibrium with its liquid, stronger IMF lowers b/c liquid doesn’t evaporate as much

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relative strength of intermolecular forces

h bonding > dipole-dipole > LDF (when molecules are similar sized); LDF more important when molecules are larger

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effect of volume on pressure

as volume increases, pressure decreases; inversely proportional

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effect of number of particles on pressure

less particles = less pressure

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effect of temperature on pressure

higher temp = higher pressure

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ideal gas law

(pressure)(volume) = (# moles)(R)(temp in kelvin)

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r

0.08206 atm

8.314 kPa

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partial pressure

pressure that each gas would exert if it was the only gas present in the container (mole fraction x total pressure)

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graph with same temperature but different masses

heavier molecules move slower and have a narrower distribution

<p>heavier molecules move slower and have a narrower distribution</p>
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graph with same gas at different temperatures

higher temp = higher velocity = wider distribution

<p>higher temp = higher velocity = wider distribution</p>
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what makes a gas more ideal

higher temperature, lower pressure, weak IMF’s, smaller molecules (more attraction = less ideal)

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positive pressure deviation

caused by non-negligible particle volumes (big particles = hit wall more often)

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negative pressure deviation cause

stronger interparticle attractions (if they’re attracted to each other, won’t hit wall as often)

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molarity

moles solute / liters solution

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things to consider when drawing molecules

relative size, orientation (Âą), number (read directions)

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distillate

the liquid that is collected after vaporizing a mixture and then condensing the vapor back into a liquid during the process of distillation (lowest boiling point)

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chromatography

substances with similar polarity as mobile phase (liquid) will move further up, substances with different polarity to liquid won’t move as far

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higher solubility

stronger interactions between solute + solvent molecules

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lower Rf value

spot is lower on the plate/didn’t move as far

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gas relationship between temp and solubility

as temp increases, solubility decreases

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solid relationship between temp and solubility

temp increases, solubility increases

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microwave radiation

rotates molecules

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infrared radiation

vibrates molecules (move closer/further from each other)

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ultraviolet/visible light

transitions in energy levels of electrons

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ultraviolet wavelength

1-400 nm

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visible light wavelength

400-750 nm

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infrared wavelength

750 nm- 1 mm

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microwave wavelength

1 mm- 1 m