QTipp MCAT Chemistry EK
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80 terms
Terms | Definitions |
|---|---|
 First two groups/families on Periodic Table | IA = Alkali metals IIA = Alkaline Earth Metals |
| Last two groups/families in Periodic Table | VIIA = Halogens VIIIA = Noble Gases |
| Periodic Trends for: Energy of Ionization Electron Affinity Electronegativity | Increase up and right |
| Periodic trends for: Atomic Radius Metallic Character | Increase down and left |
| meaning of pico and femto | pico = 10e-12 Femto = 10e-15 |
| Molecular vs Empirical formula for glucose (C6H12O6) | Molecular = C6H12O6 Empirical = CH2O |
| Reaction Types: A+B -> C | Combination |
| Reaction Type: C-> A+B | Decomposition |
| Reaction Type: A+BC -> B + AC | Single Displacement |
| AB+CD -> AD + CB | Double Displacement |
| Azimuthal quantum number (l) | subshell = s,p,d,f orbital shape |
| Describe each of 4 quantum numbers | 1st = shell, corresponds to energy level 2nd = subshell, corresponds to shape 3rd = orbital withn subshell 4th = e- spin, distinguishes between two electrons |
| Planck's quantum theory formula | ΔE= hf where h= Planck's constant deltaE=hf |
| Photoelectric Effect | The quantization of photon energy levels as demonstrated by Einstein. Electrons hit by a photon will only move to the next energy level if the photon is of sufficient energy. If not the photon is reflected. |
| Define STP | Standard Temperature and Pressure 0 degrees Celsius and 1 Atmosphere (atm) |
| Ideal gas law | PV=nRT Assumes 1) molecules have 0 volume 2) molecules exert no forces other than collisions 3) elastic collisions 4) avg KE of gas is proportional to Temp. |
| Standard Molar Volume | 22.4 Liters Know this. |
| Partial Pressure of A | Partial Pressue of A = (Molar Fraction of A) * (Total Pressure) |
| Effusion | The spreading of a gas from high pressure to very low pressure through a 'pinhole' |
| Diffusion | The spreading of one gas into another gas or into empty space |
| Conditions where real gases deviate from Ideal Gases | High Pressure and Low Temperatures |
| Compare pressue and Volume between real and ideal gases | Real gases have greater volume Reals gases have lower pressure |
| Elementary Reaction | Reaction that occurs in single step Reaction coefficients tell you how many molecules participate in a reaction producing collision. |
| Chemical Equilibrium | When the Forward reaction rate equals the Reverse Reaction Rate. |
| Predict Direction of reaction: Q = k Q > k Q < k | Q=k --> Equilibrium Q>k --> reverse reaction Q<k --> forward reaction |
| Reaction Quotient "Q" | Q= (Products^Coeff)/(Reactants^Coeff) |
| Equilibrium Constant "K" | K== (Products^Coeff)/(Reactants^Coeff) |
| Definition of heat and work | heat = energy transfer from warm body to cool body work = energy transfer due to force (w=Fd & w=PΔV). Any energy transfer not heat |
| Three types of Heat | Conduction = Molecular Collisions Convection = Fluid movements Radiation = Electromagnetic waves |
| 1st law of Thermodynamics | ΔE = q + w q = heat flow into system w = work done on system |
| 2nd law of Thermodynamics | Heat cannot be changed completely into work in a cyclical process. The entropy of an isolated system will never DECREASE ΔSsystem + ΔSsurroundings = ΔSuniverse >= 0 |
| Define Pressure | Pressure is the random translational kinetic energy per volume |
| Enthalpy (H) formula | ΔH = ΔU + PΔV (constant pressure) ΔH = q (constant pressure, closed system at rest, PV work only) |
| 25 degrees Celsius = ? Kelvin | 298 degrees Kelvin 25 + 273 |
| Transition state vs Intermediate | Transition Sate = Bump on energy diagram Intermediate = Valley between bumps on energy diagram |
| Gibbs free energy G | ΔG = ΔH - TΔS When ΔG = 0 equilibrium is reached |
| Define spontaneity | When ΔG is negative |
| London dispersion forces | forces that hold non-polar molecular molecules together by weak intermolecular bonds |
| Electrolyte | Compound that forms ions in aqueous solution |
| Molarity (M) | =moles of solute / volume of solution |
| Molality (m) | = moles of solute / kilogram of solvent |
| Mole Fraction(Χ) | =moles of solute / total moles of all solutes and solvent |
| mass % | = mass of solute/total mass of solution x 100 |
| ppm | = mass of solute / total mass of solution x 10^6 |
| Equivalent of Acid/Base | Mass of acid or base that can furnish or accept one mole of protons |
| When does boiling occur? | When the vapor pressure equals local atmospheric pressure |
| When does melting occur? | When vapor pressure of solid is equal to the vapor pressure of the liquid |
| Vapor Pressure of Solution | Proportional to mole fraction of liquid (a) and the vapor pressure of liquid Pa. Psol. = ΧliqPliq |
| Saturated Solution | when rate of dissolution and precipitation are equal the solution is saturated |
| Heat Capacity (C) = | C= q/ΔT Amount of energy a substance can absorb per unit Temp. |
| Specific Heat Capacity | q=mcΔT (looks like MCAT) c=q/mΔT m is mass |
| What do flat line segments on a heat curve represent? | Phase change. At this point the heat capacity is infinite. |
| 6 types of Phase Changes | melting - freezing vaporization - condensation sublimation - deposition |
| Sublimation | solid to gas |
| Deposition | gas to solid |
| critical temperature | the temperature above which a substance cannot exist in the liquid state |
| critical pressure | the lowest pressure at which a substance can exist as a liquid at the critical temperature |
| Colligative properties | depend on the number of particles irrespective of the type of particle. |
| 4 Colligative properties in Chem | vapor pressure, boiling point, freezing point, osmotic pressure. Depend on the number of particles irrespective of the type of particle. |
| Osmotic Pressure eqn (Π) | Π=iMRT M=molarity i=Vant't Hoff factor (number of particles into which a single solute particle will dissociate when added to solution) |
| Osmotic pressure | Measure of the tendency of water (or other solvent) to move into a solution via osmosis |
| Arrhenius acid/base | acid produces hydrogen ions in aqueous solution base produces hydroxide ions in aqueous solution |
| Bronsted Lowry acid/base | acid donates a proton base accepts a proton |
| Lewis acid/base | acid accepts a pair of electrons base donates a pair of electrons |
| Acid vs Conjugate base Strength | The stronger the acid the weaker the conjugate. The weaker the acid the stronger the conjugate. |
| value of Kw (autoionization of water) at 25 degrees celsius | 10e-14 |
| pH +pOH = | pH+pOH = pKw = 14 |
| Almost Vertical line in a titration curve | Equivalence point Stoichiometric point Point at where there is an equal equivalent of acid and base in solution |
| Where is equivalence point of titration of a Weak Acid with strong base? | Above pH of 7 |
| Where is equivalence point of titration of a Strong Acid with a weak base? | Below pH of 7 |
| Half equivalence point | Point where exactly one half of the acid has been neutralized by the base. Concentration of acid is equal to concentration of CONJUGATE base. This is a buffered solution. |
| How to make a buffer solution? | Put copious amounts of a weak acid and its conjugate base. |
| Oxidation state of Florine | -1 |
| Oxidation state of Hydrogen | 1 (exept when bonded to a metal:then -1) |
| Oxidation state of Oxygen | -2 (except when it is in a peroxide like H2O2) |
| Reduction potential of 2H+ + 2e- -> H2 | Eo=0.00V |
| Direction of e- flow in Galvanic Cell | From anode to the cathode |
| Is a positive cell potential spontaneous or non-spontaneous? | spontaneous ΔG=-nFE where F= Faraday's constant; n=#of moles; E = voltage |
| Concentration cell | Reduction half reaction taking place in one half cell and the reverse of the same reaction taking place in the other half of the cell. The halves differ in concentration. |
| An electrolytic cell | Contains a power source instead of a resistor. Electrons flow in opposite direction. Anode and Cathode reverse sign but still RED CAT AN OX |
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