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77 Cards in this Set
- Front
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Nomenclature |
Binary, Polyatomic, Stock System |
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Binary Ionic Compounds |
Metal + Non-metal Cation first, followed by anionMetal cations are name of elementNon-metal anions names are changed to "...ide" |
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Binary Covalent Compounds |
Non-metal + Non-Metal* Add "...ide" to the root of the least metallic element.* use numeric prefixesEx) NO2 = nitrogen dioxide |
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polyatomic ions |
acetate, ammonium, carbonate, chlorate, chlorite, chromate, cyanide, dichromate, bicarbonate, bisulfate, bisulfite, hydroxide, hypochlorite, nitrate, nitrite, oxalate, perchlorate, permanganate, phosphate, sulfate, sulfite |
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stoichiometry |
Convert beginning measurement into moles of that elementMultiply moles of what you have by what you needTurn moles of what you need into ending measurement |
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balancing equations |
1. Never touch subscripts2. Treat polyatomic as one unit3. Balance Metals4. Balance non-metalsSave hydrogen and oxygen for lastMake sure coefficients are at their lowest ratio |
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percent yield equation |
Percent Yield= (Actual Yield / Theoretical Yield) x 100% |
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Ideal gas law |
PV=NRT |
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Boyles Law |
P1V1=P2V2 |
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Charles Law |
V1/T1 = V2/T2 |
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Combined Gas Law |
P1V1/T1 = P2V2/T2 |
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Hess' Law of constant heat summation |
Regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes. |
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Specific Heat |
The heat required to raise the temperature of the unit mass of a given substance by a given amount (usually one degree) |
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Enthalpy of a reaction |
Enthalpy of a reaction or energy change of a reaction DH, is the amount of energy or heat absorbed in a reaction. If the energy is required, DH is positive, and if energy is released, the DH, is negative. |
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Heat of Formation |
Hreaction = SUM (Hproducts) - SUM (Hreactants)or if you prefer using symbolsHreaction = SHproducts - SHreactants |
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Isotope |
Two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei |
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# sigma and pi bonds in a compound |
Sigma bonds are the first bonds, pi bonds are the second and third bonds. They are made from leftover p orbitals. |
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Formal charge |
The charge assigned to an atom in a molecule, assuming that electrons in all chemical bonds are shared equally between atoms regardless of electronegativity. |
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Hydrogen bond |
A weak bond between two molecules resulting from an electrostatic attraction between a proton in one molecule and an electronegative atom in the other. |
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Absolute zero |
The temperature at which all substances have no thermal energy; 0 Kelvin or -273.15 Celsius |
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Absorption series |
The series of discrete lines at characteristic frequencies representing the energy required to excite an electron from the ground state. |
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Acid |
A species that donates hydrogen ions or accepts electrons--Lewis Acid. |
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Acid Dissociation Constant (Ka) |
The equilibrium constant that measures the degree of dissociation of an acid under specific conditions. |
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Acidic solution |
An aqueous solution that contains more H+ ions than OH- ions; pH<7 under standard conditions. |
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Adiabatic Process |
A process that occurs without the transfer of heat into or out of the system. |
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Alkali Metals |
Elements found in Group IA of the periodic table; highly reactive, readily losing one valence electron to form ionic compounds with nonmetals. |
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Amphoteric Species |
A species capable of reacting as either as an acid or base, depending on the nature of the reactants. |
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Amphiprotic Species |
A species that may either gain or lose a proton. |
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Anion |
Negatively charged ion |
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Anode |
The electrode at which oxidation occurs. |
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Antibonding Orbital |
A molecular orbital formed by the overlap of two or more atomic orbitals; energy is greater than the energy of the combining atomic orbitals. |
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Arrhenius Base |
A species that donates hydroxide ions (OH-) in aqueous solution. |
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Arrhenius Acid |
A species that donates protons (H+) in an aqueous solution. |
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Arrhenius Equation |
A chemical kinetics equation that relates the rate constant (k) of a reaction with the frequency factor (A), the activation energy (Ea), the ideal gas constant (R), and temperature (T) in kelvin. |
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Atomic Mass Unit |
A unit of mass defined as 1/12 the mass of a carbon-12 atom; approximately equal to the mass of one proton or one neutron. |
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Atomic Orbital |
Describes the region of space where there is a high probability of finding an electron. |
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Atomic Radius |
The average distance between a nucleus and its outermost electron; usually measured as one-half the distance between two nuclei of an element in its elemental form. |
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Aufbau Principle |
The concept that electrons fill energy levels in order of increasing energy, completely filling one sublevel before beginning to fill the next. |
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Autonization |
The process by which a molecule (usually water) spontaneously dissociates into cations and anions. |
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Bohr Model |
The model of the hydrogen atom in which electrons assume certain circular orbits around a positive nucleus. |
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Boiling point elevation |
The amount by which a given quantity of solute raises the boiling point of a liquid; a colligative property. ΔT = i Kb mi=Van't Hoff Factor (degree of dissociation for the solute) for substances that ionize in water (ie separate into ions). Substances which do not ionize have a Van't Hoff Factor of 1. Kb=molal boiling point elevation constant (ebullioscopic constant)m=molality of the solution. |
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bond length |
The average distance between two nuclei in a bond; as the number of shared electron pairs increases, the bond length decreases. (so single bond>double bond>triple bond in terms of increasing to decreasing bond length). |
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bond order |
The number of shared electron pairs between two atoms; a single bond has a bond order of 1, a double bond has a bond order of 2, and a triple bond has a bonder order of 3. |
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bonding orbital |
A molecular orbital formed by the overlap of two or more atomic orbitals; energy is less than that of the combining orbitals. |
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Boyle's Law |
The law stating that at constant temperature, the volume of a gaseous sample is inversely proportional to it's pressure. |
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Buffer |
A solution containing a weak acid and its salt (or a weak base and its salt) that tends to resist changes in pH. |
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Cathode |
The electrode at which reduction takes place. |
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Cation |
Positively charged ion |
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Charle's Law |
The law stating that the volume of a gas at constant pressure is directly proportional to its absolute (kelvin) temperature. |
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Common Ion Effect |
A shift in the equilibrium of a solution due to the addition of ions of a species already present in the reaction mixture. |
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Conjugate Acid-Base Pair |
The relationship between a Bronsted-Lowry acid and its deprotonated form, or a Bronsted-Lowry base and its protonated form. |
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Diffusion |
The random motion of gas or solute particles across a concentration gradient, leading to uniform distribution of the gas or solute throughout the container. |
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Dipole-Dipole Interactions |
The attractive forces between two dipoles; magnitude is dependent on both the dipole moments and the distance between the two species. |
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Dipole |
A species containing bonds between elements of different electronegativities, resulting in an unequal distribution of charge. |
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Dipole Moment |
A vector quantity with a magnitude that is dependent on the product of the charges and the distance between them; oriented from the positive to the negative pole. |
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Dissociation |
The separation of a single species into two separate species; usually used in reference to salts or weak acids or bases. |
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Double-Displacement Reaction |
A reaction in which ions from two different compounds swap their associated counterions; typically, one of the products of this type of reaction is insoluble in solution and will precipitate. |
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Electrolysis |
The process in which an electrical current is used to power an otherwise nonspontaneous decomposition reaction. |
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Electronegativity |
A measure of the ability of an atom to attract the electrons in a bond; commonly measured with the Pauling scale. |
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Empirical Formula |
The simplest whole-number ratio of the different elements in a compound. |
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Enthalpy |
The heat content of a system at constant pressure; the change in enthalpy (delta H) in the course of a reaction is the difference between the enthalpies of the products and the reactants. |
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Entropy |
A property related to dispersion of energy through a system or degree of disorder in that system; the change in entropy (delta S) in the course of a reaction is the difference between the entropies of the products and the reactants. |
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Equilibrium |
The state of balance in which the forward and reverse reaction rates of a reversible reaction are equal; the concentrations of all species will remain constant over time unless there is a change in the reaction conditions. |
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Exothermic Reaction |
A reaction that gives off heat to the surroundings (negative delta H, delta H<0) as the reaction proceeds. |
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First order reaction |
A reaction in which the rate is directly proportional to the concentration of only one reactant. |
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Gibbs Free Energy |
The energy of a system available to do work. The change in Gibbs free energy, delta G, can be determined for a given reaction equation from the enthalpy change, temperature, and entropy change; a negative delta G denotes a spontaneous reaction, while a positive delta G denotes a nonspontaneous reaction. |
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Metalloids |
-also called semimetals-EN and ionization energy inbetween metals and nonmetals |
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IMF and relative strength |
Weakest: dispersal or London or Van der Waals forces-temporary dipoles (the reason noble gases can liquify)Intermediate: dipole-dipole interactions-more permanent dipoles (not relevant with gases)Strongest: hydrogen bonding (10% of covalent bond) |
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zero order reaction |
temp matters, concentration doesnt matter A (T) vs Time |
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1st order reation |
rate is proportional to reactant changes with concentration Concentration VS Time |
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2nd order reaction |
depends on collision between two reactant molecules 1/A VS Time |
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Hess' Law |
enthalpy changes of a reaction are additive |
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Solubility |
Ksp The solubility of non-gaseous solvents increases with temp, while that of gaseous temps decreases with increased temp |
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latent heat |
heat absorbed or radiated during a change of phase at a constant temperature and pressure |
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conduction |
Heat transfer by direct contact. Requires things to touch |
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convection |
Heat transfer by flowing current. Need the physical flow of matter |
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radiation |
Heat transfer by electromagnetic radiation. Does not need the physical flow of matter, can occur through vacuum |