IMF & Phases of Matter

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Solid

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FIXED shape and volume

  • vibrates around a fixed location

Does NOT compress or expand at all

  • too dense

Can be crystalline: a regular, repeating pattern

  • or noncrystalline (amorphous)

slightly higher D than liquids

  • exception: ice = 0.917 g/mL

Does NOT mix by diffusion

  • cannot mix uniformly this way

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Liquid

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VARIABLE shape, FIXED volume

does not compress or expand significantly

usually flow readily (viscosity)

Higher D than gases (due to IMF)

  • water = 1.0 g/mL

If soluble, they mix homogeneously

  • diffuse more slowly than gases

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34 Terms

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Solid

FIXED shape and volume

  • vibrates around a fixed location

Does NOT compress or expand at all

  • too dense

Can be crystalline: a regular, repeating pattern

  • or noncrystalline (amorphous)

slightly higher D than liquids

  • exception: ice = 0.917 g/mL

Does NOT mix by diffusion

  • cannot mix uniformly this way

2
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Liquid

VARIABLE shape, FIXED volume

does not compress or expand significantly

usually flow readily (viscosity)

Higher D than gases (due to IMF)

  • water = 1.0 g/mL

If soluble, they mix homogeneously

  • diffuse more slowly than gases

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Gas

INDEFINITE shape and volume

Can expand a lot!

  • V increases as V of container increases

Can compress a lot!

  • if compressed enough, it will liquify and D increases

have low D

  • due to the space between the particles

  • air = 0.001 g/mL (at sea level)

mix completely with other gases in a container

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Boiling Point

the temp at which a liquid will vaporize into a gas

atmospheric pressure equal to vapor pressure

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freezing point

temperature at which a substance transitions from a liquid state to a solid state

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melting

solid to liquid

T increases

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freezing

liquid to solid

T decreases

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sublimination

solid to gas

P decreases

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deposition

gas to solid

P increases

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evaporation

liquid to gas

P decrease

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condensation

gas to liquid

P increases

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kinetic energy

the energy an object has due to its motion

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potential energy

the stored or pent-up energy of an object

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temperature

a measure of the AVERAGE KINETIC ENERGY of a sample

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pressure

a measure of the COLLISION OF PARTICLES

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normal boiling point

the temperature at which the vapour pressure is equal to the standard sea-level atmospheric pressure (1 atm)

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vaporization

conversion of a substance from the liquid or solid phase into the gaseous (vapour) phase

Evaporation and boiling

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vapor pressure

the pressure exerted by vapor just above the surface of a liquid that is at its boiling point

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atmospheric pressure

the force per unit area exerted by an atmospheric column above a specified area

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critical point

the temp above which the gas cannot be liquified no matter how much pressure is applied

(the kinetic energy simply is too great for attractive forces to overcome)

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triple point

the condition of temperature and pressure where ALL THREE phases exist in equilibrium

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viscosity

the resistance of a liquid to flow

more viscous = stronger IMF

ex. honey

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surface tension

energy required to increase the surface area of a liquid by a given amount

inward pull by particles in the interior of a liquid

stronger IMF = greater surface tension

drops on a penny

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DIPOLE-DIPOLE

polar covalent molecule

result from the attraction of the + and - ends

‘DI’pole = 2 poles

  • opposite poles align to maximize attraction and minimize repulsion

  • unequal distribution of electron density within the molecule

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london dispersion forces

exist between ALL atoms and molecules

  • if a molecule has electrons, it has LDFs

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nonpolar molecule

ONLY has LDFs

an instantaneous/temporary dipole results from an unequal sharing of electrons.

  • one particle with an instantaneous (or temporary) dipole will affect other particles adjacent to it producing a short-range attractive interaction

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what makes LDFs stronger

LARGER MOLAR MASS

larger particles

more electrons present

more polarizable electron clouds

stronger the force of attraction

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what makes dipole-dipole stronger

larger dipole

stronger the force of attraction between the 2 molecules

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hydrogen bonding (BINDING)

includes F, N, O

FORCE, not a bond!

when H atoms that are already covalently bonded to highly EN atoms (F,N,O) are also attracted to the - end of a dipole formed by the EN atom in a DIFFERENT molecule

  • or a different part of the same molecule

* INTERNAL OH TO ANOTHER OH

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order of strength for intermolecular forces

LDF → dipole-dipole → H-bonding → ion-dipole

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volatility

How readily a substance vaporizes.

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intramolecular forces

exist within a molecule

is a BOND (ionic, PC, NPC)

stronger than intermolecular forces

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intermolecular forces

exist between 2+ molecules

is a FORCE

the specific structure and size of the particles involved can play an important part in determining the overall strength of particular IMFs

weaker than intramolecular forces

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