BIG AP Chem Review
About this set
Created by:
JoelCastillo on April 9, 2012
Subjects:
Description:
Preparation for AP Chem Test
Log in to favorite or report as inappropriate.
Order by
130 terms
Terms | Definitions |
|---|---|
 Scientific Method | a method of investigation involving observation and theory to test scientific hypotheses |
| Law of Conservation of Mass | matter can't be created nor destroyed |
| Mass | a measure of resistance of an object to a change in its state of motion |
| Weight | amount of gravitational force exerted on an object |
| Celsius to Kelvin | Tk=Tc+273 |
| Matter | anything occupying space and with mass |
| Law of Definite Proportion | a given compound always has exactly the same proportion of elements by mass |
| Law of Multiple Proportions | when two elements form a series of compounds, the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers |
| Radioactivity | Spontaneous emission of radiation |
| Types of Radiation | Alpha Particles- 2+ charge Beta Particles- high-speed electrons Gamma Ray- high-energy light |
| Isotopes | atoms with the same number of protons but a different number of neutrons |
| Chemical Bonds | Force that holds atoms together |
| Naming Binary Ionic Compounds | 1.Cation first, anion second 2.A monoatomic cation takes name from its element 3.A monoatomic anion is named by taking its root and adding "-ide" 4.If needed, indicate charge of metal(cation) by a Roman Numeral 5.In covalent bonds, the 1st element is full element name and the 2nd is named like an anion 6.In covalent bonds, prefixes are used to tell amount of atoms present 7.In acid without O2, acid starts in hydro- and ends in -ic 8. In acid with O2, -ate is -ic, and -ite is -ous |
| Naming Polyatomic Ions | 1.The ion with the smaller number of O2 ends in -ite 2.The one with the larger number of O2 ends in -ate 3.If there is more than two oxyanions, then hypo is for fewest O2 ion and per- is used for most O2 ion |
| Finding Empirical Formulas | 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary, multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula |
| Percent Yield | Actual Yield/Theoretical Yield*100% |
| Net Ionic Equation | only contains ions that change in reaction |
| Acids | substances that form H+ when dissolved in water; proton donors |
| Bases | Substances that form OH- when dissolved in water; proton acceptors |
| Molarity | moles of solute/volume of soln(L) |
| 1atm=?mmHg/Torr | 760mmHg/Torr |
| 1atm=?Pa | 101,325 Pa |
| Ideal Gas Law | PV=nRT P=atm V=L n=mol R=.0826Latm/Kmol T=K |
| STP | 0°C and 1 atm |
| Dalton's Law of Partial Pressures | Ptotal=P1+P2+P3+... |
| Kinetic Molecular Theory | -FOR IDEAL GASES!!! 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion, which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K) |
| Decrease Volume and Increase Temperature | Increase Pressure |
| Increase Temperature | Increase Volume |
| Root Mean Square Velocity | u(rms)=(3RT/M)^1/2 R=8.31J/Kmol |
| Joule | SI unit of energy; Kg*m^2/s^2 |
| Molality | mol of solute/kg of solvent |
| Normality | (N) number of equivalents per liter of solution -for acid-base rxn, equivalent is the mass of acid/base that makes 1 mole of protons -for redox rxn, equivalent is amount of red/oxi agent that can take or make 1 mole of electrons |
| Enthalpy of Solution | ▲Hsoln=▲H1+▲H2+▲H3+... |
| Molal BP Elevation Constant | ▲T=k*m(solute) ▲T=BP elevation k=constant characteristic of solvent m(solute)=molality of solute |
| Molal FP Depression Constant | ▲T=k*m(solute) ▲T=FPsolvent-FPsolution k=constant of solvent |
| Osmotic Pressure | Osmotic pressure=MRT M=molarity of solution R=.0821Latm/Kmol T=K |
| van't Hoff Factor | i=moles of particles/moles of solute dissolved |
| Chemical Kinetics | studies the rate at which a chemical process occurs and sheds light on its reaction mechanism |
| Zero-Order Rate Law | r=k |
| First-Order Rate Law | r=k[A] |
| Second-Order Rate Law | r=k[A]^2 |
| Zero-Order Half Life | [A]0/2k |
| First-Order Half Life | .69/k |
| Second-Order Half Life | 1/([A]0*k) |
| Integrated Rate Law | expresses how the concentrations depend on time |
| Overall Reaction Order | n+m (these are orders of reactants) |
| Integrated First-Order Rate Law | ln[A]=-kt + ln[A]0 -linear form |
| Integrated Second-Order Rate Law | 1/[A]=kt + 1/[A]0 |
| Integrated Zero-Order Rate Law | [A]=-kt + [A]0 |
| c= | λv |
| Speed of light | c=2.9979*10^8 m/s |
| Theory of Relativity | E=mc^2 |
| Quantum Model | electrons in a hydrogen atom move around the nucleus only in circular orbits |
| Quantum Mechanical Model | involves quantum numbers |
| Quantum Numbers | describe various properties of one orbital |
| Principal Quantum Number | (n) has values 1,2,3,...; tells energy levels |
| Angular Momentum Quantum Number | (ℓ), has values from 0 to (n-1); tells shape of atomic orbitals |
| ℓ=0 | s orbital |
| ℓ=1 | p orbital |
| ℓ=2 | d orbital |
| ℓ=3 | f orbital |
| ℓ=4 | g orbital |
| Magnetic Quantum Number | (mℓ) has values from -ℓ to ℓ, including zero; tells orientation of the orbital relative to other orbitals |
| Nodes | where there are no electrons |
| Electron Spin Quantum Number | (msubs) can only be +1/2 or -1/2 |
| Pauli Exclusion Principle | in a given atom no two electrons can have the same set of four quantum numbers |
| Aufbau Principle | as protons are added to the nucleus, electrons are similarly added |
| Hund's Rule | the lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals |
| Equilibrium Expression | K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count |
| Equilibrium constant | K |
| Reaction Quotient | (Q) does the same as equilibrium expression, except it uses initial concentrations |
| Q=K | at equilibrium (Q?K) |
| Q>K | shift to left (Q?K) |
| Q<K | shift to right (Q?K) |
| Le Chatelier's Principle | if a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change |
| Acid Dissociation Constant | Ka=[products]^m/[reactants]^n |
| pH= | =log[H+] |
| Buffered Solution | a solution that resists a change in its pH |
| Solubility Product | (Ksp) an equilibrium expression |
| Law of Conservation of Energy | energy can't be created nor destroyed |
| Heat | the transfer of energy between two objects due to temperature difference |
| Work | force acting over distance |
| ▲E | q+w |
| Specific Heat Capacity | J/°Cg or J/Kg |
| Molar Heat Capacity | J/°Cmol or J/Kmol |
| Hess's Law | in going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps |
| ▲H°reaction | Σn▲H°(products)-Σn▲H°(reactants) |
| Entropy | (S) the driving force for a spontaneous is an increase in entropy of the universe |
| ▲Suniv | ▲Ssys+▲Ssurr |
| ▲Ssurr | -▲H/T |
| ▲G | ▲H-T▲S |
| ▲G° | ▲H°-T▲S° |
| G | G°+RTln(Q) R=8.31 |
| w(max) | =▲G (work) |
| Galvanic Cell | a device in which chemical energy is changed to electrical energy |
| Anode | where oxidation occurs |
| Cathode | where reduction occurs |
| Cell Potential | (Ecell) driving force of the electrons |
| Volt | unit of electrical potential; J/C |
| Faraday | 96,485 C/mol e- |
| ▲G | -nFE E=cell potential |
| Ampere | (A), C/s |
| Bond Energy | energy required to break a bond |
| Polar Covalent Bond | bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs |
| Electronegativity | ability of an atom in a molecule to attract shared electrons to itself |
| Dipole Moment | a molecule having a center of positive charge and a center of negative charge |
| ▲H | Σ(bonds broken)-Σ(bonds formed) |
| LE Model | assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms |
| Lone Pair | pairs of electrons localized on an atom |
| Bonding Pairs | electron pairs found in the space between the atoms |
| 3 Parts of the LE Model | 1. Describe the valence e- arrangement using Lewis structures 2. Predict the shape of the molecule using VSEPR 3. Describe the type of atomic orbitals used by the atoms |
| Resonance | when more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows |
| Formal Charge | (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule) |
| Valence Electrons(assigned) | (# of lone pair e-)+1/2(# of shared e-) |
| Steps to VSEPR Model | 1. Draw the Lewis Structure 2. Count the e- pairs and arrange as far apart as possible 3. Determine positions of atoms from way e- pairs are shared 4. Determine name of molecular structure from positions of atoms |
| Linear | 180°, sp |
| Trigonal Planar | 120°, sp^2 |
| Tetrahedral | 109.5°, sp^3 |
| Trigonal Bipyramidal | 90°&120°, dsp^3 |
| Octahedral | 90°, d^2sp^3 |
| Hybridization | the mixing of native atomic orbitals to form special orbitals for bonding |
| Sigma Bond | the line running between the atoms |
| Pi Bond | occupies the space above and below a sigma bond |
| Molecular Orbitals (MOs) | similar to atomic orbitals, except between molecules |
| Antibonding Molecular Orbital | higher in energy than the atomic orbitals of which it is composed |
| Bond Order | # bonding e- - # antibonding e-/2 |
| Coordination Compound | consists of a complex ion, a transition metal with attached ligands, and counterions |
| Counterions | anions or cations as needed to produce a compound with non net charge |
| Ligand | a neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion |
| London Dispersion Forces | the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles |
First Time Here?
Welcome to Quizlet, a fun, free place to study. Try these flashcards, find others to study, or make your own.