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Video: https://youtu.be/GAj3mE8YK10

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https://docs.google.com/document/d/1eYjW5JEWvNHZtaPk1Kh6AHWn346Teht9iBaQTuaWLow/edit?usp=sharing

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https://docs.google.com/document/d/16vs5L0DhJVa5sxIzc0WqlccW6itbRJ_n0iKjggx94j0/edit?usp=sharing

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-Colligative Properties: properties of a solution that depend on the number of solute molecules (solute concentration) but not the identity

Vapor Pressure Lowering: Introducing nonvolatile solutes results in a decrease in vapor pressure. Solutes take up space at surface, shifting equilibrium

Boiling Point Elevation: Adding nonvolatile solutes increases the boiling point temperature

Freezing Point Depression: Adding nonvolatile solutes lowers the freezing point (Ex. Salting the roads, antifreeze)

Osmotic Pressure: : opposing pressure required to prevent bulk transfer of solvent molecules through a semipermeable membrane

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-Molarity: M = mol solute/L solution

-Mole Fraction: X = mol A/total moles

-Molality: m = mol solute/kg solvent

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-Crystalline Solids: atoms, ions, or molecules are arranged in a definite repeating pattern

1. Ionic Solids: composed of positive and negative ions held together by electrostatic attractions. Can identify them by high melting points, being hard and brittle, they shatter rather than bend, they do not conduct electricity as a solid, but do as an aqueous solutions

2. Metallic Solids: formed by metal atoms. Described as a uniform distribution of atomic nuclei with a ”sea” of delocalized electrons. They have high electrical and thermal conductivity and are malleable

3. Covalent Network Solids: atoms are held together by a network of covalent bonds (ex- Diamond, silicon dioxide (sand)). They are hard and Strong (Graphite is an exception) and have very high melting points - covalent bonds must be broken

4. Molecular Solids: composed of neutral molecules. Strengths of attractive forces vary widely depending on size and polarity

-Amorphous Solids: (noncrystalline solids) atoms, ions, or molecules are in random order. Occurs when a liquid freezes before its molecules become arranged

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-Triple Point: all three phases coexist. At pressures lower than the triple point substance cannot exist as a liquid, regardless of temp

Critical Point: any temperature past the critical point the substance is always a gas, regardless of pressure

Supercritical Fluid: intermediate between liquid and gas

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-Vaporization: liquid to gas transition

△Hvap: enthalpy of vaporization, endothermic process

-Condensation: gas to liquid transition

When rate of vaporization = rate of condensation then vapor and liquid are in dynamic equilibrium

- Vapor Pressure: pressure exerted by the vapor in equilibrium with a liquid in a closed container at a given temperature

Stronger IMFs will impede vaporization and favor condensation resulting in lower vapor pressure, and vice versa

- Boiling Point: (of a liquid) the temperature at which its equilibrium vapor pressure is equal to the pressure exerted on the liquid by its gaseous surroundings (In an open container that pressure is atmospheric pressure)

Normal Boiling Point: boiling point at 1 atm

-Melting: solid to liquid transition

△Hfus: enthalpy of fusion, endothermic process

-Freezing: liquid to sold transition

Melting/Freezing Point: temperature at which the solid and liquid phases of a given substance are in equilibrium

-Sublimation: solid to gas transition (skips the liquid state)

Ex. Dry Ice (Solid CO2)

△Hsub: Enthalpy of sublimation

-Deposition: gas to sold transition (skips the liquid state)

Ex. Frost

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https://docs.google.com/document/d/1aG_H3PjhWLIAgbI2QtTnTi7Y16w0ux6KjlgFYNyeMR4/edit?usp=sharing

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Just some Crash Course videos to help review:
Ideal Gas Law: https://www.youtube.com/watch?v=BxUS1K7xu30&index=12&list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr
Real Gases: https://www.youtube.com/watch?v=GIPrsWuSkQc&index=14&list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr
Effusion, Diffusion and the Velocity of a Gas: https://www.youtube.com/watch?v=TLRZAFU_9Kg&list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr&index=16
Solutions: https://www.youtube.com/watch?v=9h2f1Bjr0p4&index=27&list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr
Doing Solids: https://www.youtube.com/watch?v=bzr-byiSXlA&index=33&list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr

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-Viscosity: measure of a liquids resistance to flow

-Cohesive Forces: attractions between identical molecules; causes liquids to form drops

-Surface Tension: the energy required to increase the surface area of a liquid

-Adhesive Forces: IMFs of attraction between two different molecules

-Capillary Action: adhesion to surface is greater than cohesion within the liquid (ex. Porous materials, small tubes)

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Some of terms are explained more throughout the padlet

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Main Concept: Intermolecular and Intramolecular forces

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Main Concept: Intermolecular and Intramolecular forces

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- Intermolecular forces (IMF) exist between atoms and molecules of a substances, while intramolecular are those within a molecule

Dispersion Forces (aka London Dispersion Forces): Results from instantaneous dipoles and induced dipoles (temporary dipole moment due to momentary asymmetrical distribution of electrons); the weakest IMF, experienced by nonpolar molecules, so affected by size of molecules and shape.

Dipole – Dipole Forces: Attraction between the partial positive and partial negative sides of polar molecules

Hydrogen Bonding: A strong dipole-dipole interaction between molecules that contain an H-F, H-O, or H-N bond; the Strongest IMF

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- Kinetic Molecular Theory:

Molecules are point masses (they have no volume)

Gas molecules exert no force on each other unless they collide

Collisions of molecules with each other or the walls of the container do not decrease the energy of the system

The molecules of a gas are in constant and random motion

the energy of an ideal gas is entirely kinetic.

https://www.khanacademy.org/test-prep/mcat/physical-processes/kinetic-molecular-theory-of-gas/v/kinetic-molecular-theory-of-gases

- Pressure and temperature, as well as volume and temperature, are directly proportional
- volume and pressure are inversely proportional
- conditions for ideal gases are high temperatures and low pressures
-Gas can be collected by displacement of water. When levels are equal the pressure of the trapped gas mixture equals atmospheric pressure

remember that there is a mixture of gas due to the water vapor

-  Effusion and Diffusion both depend on the molar mass of the gas involved, but their rates are not equal. The ratios of their rates, however, are the same
- the rate of diffusion depends on the concentration gradient, the amount of surface area available for diffusion, and the distance the gas particles must travel
- All gases with the same temperature have the same KEavg. The difference comes from molar mass.

As the temperature increases, so does the velocity, and as the mass of an atom/molecule increases the velocity decreases

***Make sure to look at the key terms-- some of the main concepts are in the key terms quizlet