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States of Matter
• Kinetic Molecular Theory: the idea that particles of matter are always in motion; this applies to all states of matter
• Used to explain properties of matter in terms of energy
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Ideal Gas= hypothetical gas that perfectly fits all 5 assumptions of
the Kinetic Molecular Theory:
1) Gases consist of a large # of particles that occupy a larger space with respect to their relative sizes
thus gases can be easily compressed
2) Collisions b/t particles and walls are perfectly elastic ( = no loss of KE)
3) Gas particles are in rapid, random, constant motion4) There are no forces of attraction b/t gas particles5) Temperature of a gas depends on the average
KE of the particles; directly proportional
A gas that is always a gas - Doesn’t exist!
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Characteristics of Gases
• Expansion: no definite shape or volume; fill any container, regardless of shape
• Fluidity: particles slide easily over one another; act like liquids, thus they are both fluids
• Low Density and Compressibility: volume can be decreased greatly
• Diffusion: since gases are always randomly moving, freely mix together with other gases
• Effusion: process by which gases move out of a small opening; molecules with low mass effuse more quickly than those with larger masses
KE= ½ mv2
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Liquids
• Least common state of matter in universe; not so on Earth
• Operate at slim range of temps/pressures
• Volume, shape, density?• Particles in constant
motion, and closer than those of a gas (intermolecular forces)
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Other Characteristics of liquids:• Have a very high density when compared to
gases; depends on temperature lower temp…except for water
• Not easily compressed
• Easily diffuse in other liquids it can dissolve in d/t… much slower than it is in gases
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Surface Tension
• All liquids exhibit surface tension = a force that tends to pull adjacent particles at a liquids surface together, decreasing its surface area to the smallest possible size; meniscus
• Results from… water shows high surface tension
• Capillary action = attraction of a liquid to a solid; rises in a small tube against gravity
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Surface TensionLook at the picture below. The milk forms small droplets that
resemble a crown. But why does this happen?
Because of the surface tension of water, which keeps the
droplets spherical.
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Some terms:
solid liquid gasMELTING BOILING
FREEZING CONDENSATION
0ºC 100ºC
melting/freezing point boiling/condensation point
(ice) (steam)(water)
SUBLIMATION
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More info on Liquids• Vaporization – liquid to
gas• Evaporation – escape
from a non-boiling liquid at its surface
• Boiling – vaporization through the entire liquid
• Freezing – physical change from liquid to solid through the loss of HEAT. Evaporation- a beautiful process.
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Solids
• Particles in a solid are tightly-packed together due to attractive forces. Highly-ordered.
• Atomic/molecular motion is restricted, but it occurs.
• 2 types:1) Crystalline: consists of crystals
(orderly, geometric, repeating pattern)
2) Amorphous: particles are randomly arranged
Sodium Chloride crystals
Amorphous solid
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Properties of solids• Definite shape and volume
• Definite melting point (d/t addition of heat)
• High density and incompressible
• Low rates of diffusion
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Crystals• Arranged in a lattice structure
• Smallest unit of a crystal that shows the 3-D pattern of the lattice = UNIT CELL
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Changes of State
• Phase = any part of a system that has a uniform composition and properties
• Condensation = process by which a gas turns into a liquid
• Vapor = a gas in contact with its liquid or solid phase
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Vapor Pressure
• The pressure exerted by a vapor that is in equilibrium with its corresponding liquid
• Develops in a closed system
• Increase AKE, increase particles leaving liquid, increased pressure
• Volatile liquids evaporate
easily d/t weak IMF
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Vapor Pressure
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Notes on Boiling Point• BP = when vapor pressure
equals atmospheric pressure• Increase pressure, increase
BP = pressure cooker• Molar Enthalpy of
Vaporization = amount of heat needed to vaporize 1 mole of a liquid at the liquid’s BP at a constant pressure; the stronger the attraction….
• Vapor pressure is directly proportional to temperature
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Freezing and Melting• Definitions?
• What is the difference b/t freezing water and ice? Boiling water and steam?
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Do Now• Explain the importance and significance of
this graph…
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More Vocab
• Molar Enthalpy of Fusion = the amount of heat required to melt one mole of a solid
(40.79 kJ/mol for water)
• Sublimation vs. deposition
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Phase Diagrams graph of pressure vs. temperature that shows the conditions
under which the phases of a substance would exist
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Water• Most abundant liquid
on Earth; essential to life; most reactions take place in it IMPORTANT!!!
• Review its structure and properties…
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Water