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105 Cards in this Set

  • Front
  • Back
Characteristics of gases
1. Compressible
2. No fixed volume OR shape
3. No intermolecular forces (IMF)
Characteristics of solids
1. Non-compressible "condensed phases"
2. Fixed volume AND shape
3. Physical properties controlled by IMF
Characteristics of liquids
1. Non-compressible "condensed phases"
2. Fixed volume
3. NO fixed shape
4. Physical properties controlled by IMF
Two ideas behind the Kinetic - Molecular Theory
1. Particles are in constant motion
2. Vibrational Motion stops at 0 Kelvin - kinetic energy = 0
List the different intermolecular forces
1. Dipole-Dipole
2. London Disperson
3. Ion Dipole
4. Hydrogen Bonding
Rank the IMF in terms of strength (lowest to highest)
Lowest: Disperson
- Dipole-Dipole
- Hydrogen Bonding
Highest: Ion-Dipole
What is a solid turning into a liquid called in scientific terms?
1. Fusion
Liquid to gas is called... Gas to liquid is called...
1. Vaporization
2. Condensation - gas to liquid
Dispersion has a _____________ dipole
1. Temporary - induced
How does dispersion occur?
1. Electrons may move towards one atom causing a temporary negative dipole on that atom and a positive dipole on the opposite atom.
2. If another molecule were to come close, a dipole would also be induced on that molecule due to the attraction/repulsion forces of + or - charges.
What molecules have dispersion forces?
1. ALL MOLECULES HAVE DISPERSION FORCES!
Let's say you have CH4 and C8H18... which has a larger dipole moment and why?
1. C8H18 because the size is larger meaning there is more space and potential for the electrons to move towards one side or the other without causing "conflict" with one another.
2. In a small molecule - moving electrons even the slightest bit towards eachother will cause conflict and repulsion, but not so in a larger molecule.
Larger molecules have _______________ dispersion forces.
1. Stronger
The size of the induced dipole depends upon two things...
1. Polarizability - size/weight of atom - bigger atoms have larger orbitals to move electrons around in and create dipole.
2. Shape (molecules) linear means larger dipole because more surface area to interact with other dipole.
In order to move something into a gas phase, what needs to be done?
1. IMF have to be broken.
Bigger Dipole means _________ boiling point.
Bigger interaction area means ___________ dispersion force
1. Bigger
2. Bigger
If you increase weight of a molecule, you will ____________________ the polarizability.
1. Increase
Dipole - Dipole Interactions
1. One must have molecules with permanent dipole - must be polar.
2. MOST important in small molecules.
Four most electronegative elements
F, O, N, Cl
Higher dipole (more polar) size means __________________ boiling point at the same molar mass.
1. Higher
Explain the concept of Hydrogen Bonding
1. Strong dipole-dipole interaction
2. H-F, H-O, H-N (H needs to be bound to F, O, N
3. Bonds can only be formed with other molecules including hydrogen and F, O, N, Cl.
Why are H20, HF and NH3 outliers on the graph showing increasing boiling point with increasing size?
1. Because these three have hydrogen bonding forces in them, so they are stronger, means higher boiling point.
Why is H20 above HF on the graph showing boiling point increases?
1. Because it has two potential bonding hydrogen instead of just one on the HF.
Ion-Dipole Attraction
1. Polar Molecules --> polar solvents
2. Permanent charge and permanent dipole
Do liquids have IMF, if so what do they do?
1. Yes
2. They have enough net attraction force to have a fixed volume, but not fixed shape.
Surface Tension - explain
1. Property of a liquid to minimize surface area
2. Wants fewest molecules on surface
3. Tries to get towards middle to make more interactions - with more interactions means lower PE - interior molecule has more attractive options.
Factors affecting surface tension...
1. IMF - stronger IMF - stronger surface tension.
2. Temperature - put in more KE, your PE will go down and more bonds broken. Higher temps means less surface tension.
What is viscosity?
1. resistance to flow
What happens to dispersion forces when the chain of molecules gets longer?
1. Stronger IMF when change gets longer - stronger dispersion forces.
As viscosity increases, IMF __________________.
1. Increases
2. Higher viscosity = harder to flow - stuck together more
Higher temp means what for viscosity?
1. Higher temp means more kinetic energy which means fewer total IMF attractions and VISCOSITY decreases.
2. Hot = low visc
3. Cold = high visc
Capillary action - define adhesion and cohesion
1. Rise of liquid of a small bore tube against gravity
2. Adhesion: attraction to container
3. Cohesion: attraction to itself
Why is water attracted to glass?
1. There are OH bonds on the surface of the SiO2 glass and therefore the hydrogen bonding occurs between OH and H20.
In mercury what occurs between adhesion or cohesion forces?
1. Adhesion forces - weak
2. Cohesion forces - strong
3. Miniscus UPWARDS
If cohesion is weak, what will the miniscus look like?
1. FLAT
Vaporization and Condensation are both ______________ events.
1. Surface
2. Molecules will only leave at the surface
Elaborate on vaporization and temperature...
1. As the temp increases the curve of avg kinetic energy shifts to the right and so you get more molecules that can evaporate at the minimum KE point, than if temp was lower.
How does condensation work?
1. Gas to liquid
2. Surface event
3. Some gas molecules will hit surface of liquid and if they don't have enough KE, they will get sucked/attracted into liquid form again.
What is dynamic equilibrium in terms of condensation and evaporation?
1. Rate going into gas phase = rate going into liquid phase.
Vapor pressure
1. Gas pressure of compound in gas phase over liquid.
2. Reach equilibrium in a closed system when rate into gas equals rate into liquid.
What changes the Vapor Pressure?
1. IMF - stronger IMF = LOWER VP - less evaporates because forces holding together stronger.
2. Temperature - More KE put into system, more molecules can vaporize, meaning HIGHER VP.
What doesn't change Vapor Pressure?
1. Volume Above Liquid - may temporarily decrease but it will reach equilibrium and be same as before.
2. Volume of Liquid in a Flask
3. Surface area of liquid - may change how fast gets to equilibrium, but doesn't change VP
What happens to the vapor pressure if you make the volume above a liquid larger?
1. Rate of condensation goes down because less chance for molecules to hit surface and get sucked in.
2. However, it hasn't reached equilibrium at this point, so eventually vapor pressure will be same no matter what the volume.
What is NORMAL boiling point? What is boiling point?
1. NORMAL: The temperature at which a liquid's vapor pressure equals one atm.
2. Boiling: temp at which vapor pressure equals atmospheric pressure.
Heat of Vaporization is a ___________________ process.
1. ENDOthermic.
A polar molecule will be miscible with a _______________ molecule.
1. Polar
Why does the heating curve of a liquid level off during the boiling phase even though you're adding more heat?
1. Any heat added during boiling will go directly to vaporizing the liquid to a gas.
2. Once all the liquid has evaporated, the heat will go up as the gas is heated.
What things should you remember to do using the Clausius-Clapeyron Equation for vaporization and temps?
1. UNITS IN KELVIN
2. Convert everything to Joules
3. R = 8.134
How does temperature change vapor pressure?
1. As it gets colder, there aren't as many molecules with enough KE to escape, so the VP goes down.
What is a supercritical fluid?
1. Fluid in which densities of both liquid and gas are the same - so it looks as though the substance is the same throughout.
2. Reaches a certain temp where density of liquid starts to drop, so then the liquid density becomes same as gas - looks uniform.
What is sublimation?
1. Solid to Gas
When doing heat calculations - remember slope = _____________ and plateau = ________________.
1. Slope = specific heat
2. Plateau = Delta H
Why is Delta H Vaporization so much higher than Delta H of Fusion?
1. Delta H Fusion only requires the breaking of SOME IMF in order to allow for movement of molecules.
2. Delta H Vaporization requires ALL IMF to be broken in order to get the molecule to move around, therefore the energy need is much higher.
What should you remember when doing heat calculations with specific heat and delta H equations?
1. Put all segments in kJ when you are finished, so that you can add them together.
2. Also, remember to check your delta T. If you stop at 30 degrees, don't do the ENTIRE slope, be careful!!!!!
What is a phase diagram?
1. Map of the phases of a compound as a function of pressure and temperature.
What do the lines mean on a phase diagram?
1. A line represents that both phases are in equilibrium.
The line between gas and solid on phase diagram means?
1. Sublimation curve
The line between solid and liquid on a phase diagram means?
1. Fusion curve
The line between liquid and gas on a phase diagram means?
1. Vaporization curve
When all three phases are in equilibrium at the same time = _________________.
1. Triple Point
What does the negative slope on the fusion curve show for water?
1. It shows that the solid phase is less dense than the liquid phase.
If the slope of the fusion curve on a phase diagram was straight up or slightly positive, it would mean....
1. Solid phase would be MORE dense than the liquid phase - if positive slope.
Crystal Lattice
1. Regular repeating array of points
2. Positionally fixed
What are the two things Unit Cells must do?
1. Must map ALL latice points
2. Must map all the space
What things can make up a lattice point?
1. Atoms
2. Ions
3. Molecules
What are some things to remember with unit cells?
1. Pick unit cell that looks similar to what looks like under microscope.
2. Map ANION to ANION, not other way otherwise when you translate there will be two cations touching = bad!
3. The unit cells will always have the correct ratio of atoms/ions/molecules as formula.
In molecular solids, what are the lattice points?
1. MOLECULES
How do molecules pack in molecular solids?
1. Pack to MAXIMIZE strongest IMF forces (usually dispersion).
What is the melting point like in molecular solids and why?
1. Low melting point in molecular solids
2. Due to only IMF forces holding together, no bonds - easier to break.
What are the attractive forces in ionic solids?
1. Electrostatic forces between anions/cations.
Properties of Ionic Solids...
1. High melting point - due to strong attractive forces
2. Brittle - if shift too far, repulsive forces between cations break crystal.
3. Insulators as solids - Conductors as liquids/aq
How is packing done in ionic solids?
1. Packing is controlled by maximizing cation-anion and minimizing anion-anion/cation-cation.
What is electrostatic interaction dependent upon?
1. The charges of each object and the distance between them.
2. You obviously want a positive and negative with short distance to be strongest.
Nonbonding atomic solids - properties, what are they, etc.
1. Noble Gases
2. ONLY DISPERSION FORCES hold together
3. Very Low Melting Point
Think of packing marbles into box - maximize dispersion forces
Metallic Atomic Solids - properties, what are they...
1. Electron sharing in "metallic" bonds.
2. Valence electrons shared by all atoms in solid *** (delocalized electrons)
3. Lower melting point
4. Shiny, malleable, ductile
5. Amount of electrons available in sea of electrons determines conductivity.
6. Good conductors of both thermal and electric due to mobility of delocalized electrons.
Network Covalent Solids - properties, what are they...
1. Solids held together by sharing electrons in covalent bonds.
2. Very high melting points - have to break covalent bonds.
3. Semiconductors or insulators - electrons LOCALIZED not free to move.
Properties of diamond
1. Very high melting point
2. Very rigid
3. Very hard
4. Electric insulator
5. Thermal conductor
Properties of graphite
1. Very high melting
2. Slippery feel
3. Electrical conductor
4. Thermal insulator
NOTE: no covalent bonds BETWEEN layers - only dispersion between layers
What is a solution and what are the major and minor components called?
1. Solution - homogeneous mixture
2. Major component - Solvent
3. Minor component - Solute
Define solubility...
1. Maximum solute that can be dissolved in a fixed amount of solvent.
Why are gases all soluble in each other?
1. They have no IMF - so they have no attraction and can disperse however they please within eachother.
With a solid solute, the solubility _________________ as temperature ___________________.
With a gas solute, the solubility ___________________ as temperature ___________________.
1. Solubility increases as temperature increases - solid
2. Solubility decreases as temperature increases - gas
What is entropy?
1. System will move to have more random distribution of particles.
What is the process of making a solution in terms of IMF and solvent solute interactions?
1. Starts with solvent-solvent and solute-solute interactions.
2. Have to input energy in order to break IMF holding those together and get single solute and solvent molecules.
3. Once you break apart, the solute and solvent can have a net attraction to one another and you end up getting energy out at this point.
Explain the energetics of delta H of solution - use the delta H of solvent-solvent, etc to explain.
1. Delta H solution = delta H solvent-solvent + delta H solute-solute + delta H solvent-solute.
2. The only one of these who gets energy out is solvent-solute. The others require energy in to break IMF bonds.
If solution forms when there is a greater attraction between solute-solute and solvent-solvent, then the ________________ must be the largest player. If a solution doesn't form, what does that mean?
1. Entropy largest player if it ends up forming.
2. If doesn't form, IMF not compatible or entropy not enough.
What does hydration mean?
1. Surrounding compound with water.
2. In case of NaCl - Na + ions surrounded by water.
3. Delta H hydration gives you the amount of energy you get when surround Na+ with water.
What is solution equilibrium?
1. Occurs when you reach saturation
2. Rate of dissolution = rate of deposition
If amount solute dissolved is equal to solubility limit - called ____________________.
If amount solute dissolved is greater than solubility limit - called ___________________.
1. Saturated solution
2. Super saturated solution
How you can you make a solution SUPER saturated? How does it differ between solid and gas solutes?
1. Solid solute - add solute to saturated solution with HIGHER temperature.
2. Gas solute - add solute to saturated solution in closed system with HIGH pressure of gas over liquid.
What is Henry's Law?
1. Solubility of gas (concentration) is directly proportional to its partial pressure.

Sgas=(kH) * (Pgas)

2. PRESSURE NEEDS TO BE ATM
Define colligative properties
1. Physical properties of a solution that depends ONLY on concentration of solute particles.
*be aware if solute will break into ions or not
How is vapor pressure different between pure solvents and solvents in solution?
1. VP of solvent in solution will be LOWER than vapor pressure of pure solvent.
2. In pure solvent - every molecule has a chance to escape into vapor if enough KE.
3. In solvent solution - there are decreased number of solvent molecules at surface due to competition with solute particles - less solvent molecules chance to escape.
What is Raoult's Law?
1. Pressure of solution (nonvolatile) = Pressure pure solvent * mole fraction of solvent
How do you calculate mole fraction?
1. Moles solvent / total moles of ALL compound in solution (solvent moles + solute moles)
What is the density of water?
1 g/mL
How does the change in VP when adding a solute into solution affect boiling and freezing point?
1. Boiling point goes UP - when add solute, VP goes down and so you have to add heat to get back up to atmospheric pressure for boiling to occur.
2. Freezing point goes DOWN -
What do you have to remember when dealing with electrolyte or non-electrolyte solutions?
1. Find how many particles of solute - for the mole fractions make sure to use (i) to multiply the mole amount of solute by particle amounts.
Why are measured i values less than expected i values when talking about particles solutes?
1. The clusters of ions may "hang out" near each other and act as one particle, however, we know that some split into 2, 3 or 4 particles!
How do you calculate freezing point depression or boiling point elevation?
1. Delta Tf = i*Kf*molality

2. Molality = moles solute/kg of solvent
What is Osmosis?
1. Process of Solvent passing through semi-permeable membrane.
2. Solvent goes to solution with higher solute concentration to try and dilute it.
What is the difference between hyperosmotic and hyposmotic solutions?
1. Hyperosmotic - water rushes out of cell because solution concentration is high (cell shrivels)
2. Hyposmotic - water rushes INTO cell because solution concentration low (cell swells)
How do you calculate the pressure of a solution with a volatile solute?
Psolution = (Pa * Xa) + (Pb * Xb)
What is the difference between ideal and nonideal solutions?
1. Ideal: obeys Rault's Law
2. Ideal: IMF between solvent and solute are nearly identical to the solvent-solvent and solute-solute interactions.
What is a positive versus negative deviation?
1. Positive: VP higher than expected - interactions solvent-solute are less favorable.
2. Negative: VP lower than expected - interactions solvent-solute more than favorable. H < 0