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Chemistry
| Question | Answer |
|---|---|
| Four variables used to describe an ideal gas | Pressure, Volume, Moles, Temperature |
| Law that states that pressure and volume are inversely proportional at a constant temperature | Boyle's Law |
| Law that states that volume and temperature are directly proportional at a constant pressure | Charles's Law |
| Law that states that pressure and temperature are directly proportional at a constant volume | Gay-Lussac's Law |
| Combined gas law | (P1V1)/T1 = (P2V2)/T2 |
| Ideal gas law | PV = nRT |
| Ideal gas constant | 8.31 |
| SI unit for amount of substance | Moles |
| Avogadro's number | 6.022 * 10^23 |
| Mass of one mole of substance | Molar Mass |
| Molar mass units | g/mol |
| Reactant that is completely used up in a chemical reaction | Limiting Reagent |
| Reactant that has some left over after a chemical reaction is completely finished | Excess Reagent |
| Amount of product that can be made by the limiting reagent | Theoretical Yield |
| Acids that produce hydrogen ions when dissolved | Arrhenius Acids |
| Bases that produce hydroxide ions when dissolved | Arrhenius Bases |
| Acids that are proton donors | Brønsted-Lowry Acids |
| Bases that are proton acceptors | Brønsted-Lowry Bases |
| Acids that accept electron pairs | Lewis Acids |
| Bases that donate electron pairs | Lewis Bases |
| Log scale that determines acidity or basicity of an aqueous solution | pH Scale |
| pH equation | pH = -log[H+] |
| Solution with a pH below 7 | Acid |
| Solution with a pH above 7 | Base |
| Acids and bases that completely dissolve in water | Strong Acids and Bases |
| Acids and bases that only partially dissolve in water | Weak Acids and Bases |
| Constant that determines the strength of weak acids and bases | Dissociation Constant (Ka) |
| Solutions that resist a pH change | Buffers |
| Composition of buffer solutions | Weak Acid and Conjugate Base (or Weak Base and Conjugate Acid) |
| pH of human blood | 7.4 |
| Study of heat energy associated with chemical reactions | Thermochemistry |
| Measure of total heat content | Enthalpy |
| Reactions that release heat into their surroundings | Exothermic |
| Reactions with a negative change in enthalpy | Exothermic |
| Reactions that absorb heat from their surroundings | Endothermic |
| Reactions with a positive change in enthalpy | Endothermic |
| Change in enthalpy during the formation of 1 mole of a substance from its constituent elements in their standard forms | Standard Enthalpy of Formation |
| Standard temperature and pressure | 25 degrees Celsius, 1 atmosphere |
| Standard enthalpy of formation for any element in its standard state | 0 |
| Enthalpy is this kind of function, where the path it takes doesn't matter | State Function |
| Law that states that, for a reaction carried out as steps, the enthalpy for the total reaction is equal to the sum of the changes in enthalpy for the products at each step, minus the sum of the change in enthalpy for the reactants in each step | Hess's Law |
| Hess's Law | ΔH°_reaction = Σ ΔH°f(products) - Σ ΔH°f(reactants) |
| Study of the relationship between chemical reactions and electrical energy | Electrochemistry |
| Type of reaction where there is a change in oxidation number | Redox (Oxidation/Reduction) Reaction |
| Type of reaction where there is a loss of electrons | Oxidation Reaction |
| Type of reaction where there is a gain of electrons | Reduction Reaction |
| Agent that gets oxidized | Reduction Agent |
| Agent that gets reduced | Oxidation Agent |
| Charge on an atom if all bonds on it were 100% ionic | Oxidation State |
| Increase in oxidation state | Oxidation |
| Decrease in oxidation state | Reduction |
| Devices that can generate electrical energy from a chemical reaction or use electrical energy to cause a chemical reaction | Electrochemical Cells |
| Electrochemical cell that uses spontaneous redox reactions to generate electrical current | Galvanic (Voltaic) Cell |
| Batteries are this type of cell | Galvanic (Voltaic) Cell |
| Electrochemical cell that uses external electrical energy to cause non-spontaneous redox reactions | Electrolytic Cell |
| Electrochemical cell used for electrolysis and electroplanting | Electrolytic Cell |
| Electrode where oxidation occurs | Anode |
| Electrode where reduction occurs | Cathode |
| Device that connects two half-cells | Salt Bridge |
| Electrons flow from anode to cathode through this | External Wire |
| Functional group with a hydroxyl | Alcohol |
| Functional group with a terminal carbonyl | Aldehyde |
| Functional group with a carbonyl in the middle of the carbon chain | Ketone |
| Functional group with a bonded carbonyl and hydroxyl | Carboxylic Acid |
| Functional group that smells fruity | Ester |
| Functional group with a carbon double bonded to an oxygen and single bonded to a second oxygen | Ester |
| Functional group with a nitrogen and carbon bonded together | Amine |
| Basic functional group | Amine |
| Functional group with an oxygen bridge in the middle of the carbon chain | Ether |
| Molecules with the same molecular formula but a different arrangement of atoms | Isomers |
| Isomers where the atoms are connected in a different order | Structural Isomers |
| Isomers with the same order of atoms but different spatial arrangements | Stereoisomers |
| Isomers with high-priority groups on specific sides of a double bond | Geometric (Cis-Trans) Isomers |
| Geometric isomers where both groups are on the same side of the double bond | Cis |
| Geometric isomers where the groups are on opposite sides | Trans |
| Isomers that are non-superimposable mirror images of each other | Enantiomers |
| Structure that is necessary for enantiomers | Chiral Center |
| Weak attractive forces that hold different molecules together | Intermolecular Forces |
| Three types of intermolecular forces | London Dispersion Forces, Dipole-Dipole Forces, Hydrogen Bonds |
| Intermolecular force that is present in all atoms and molecules | London Dispersion Forces |
| Partial charge caused by the random motion of electrons | Spontaneous Dipole |
| Partial charges caused by spontaneous dipoles coming near other atoms or molecules | Induced Dipoles |
| Intermolecular force only present in polar molecules | Dipole-Dipole Forces |
| Intermolecular force only present in molecules where hydrogen is bonded to either oxygen, nitrogen, or fluorine | Hydrogen Bonds |
| Three elements that hydrogen can bond with for hydrogen bonding to be possible | Oxygen, Nitrogen, Fluorine |
| Strongest type of intermolecular force | Hydrogen Bonds |
| Study of the rate of chemical reactions | Chemical Kinetics |
| Change in concentration of reactants or products over time, in M/s | Reaction Rate |
| Theory that explains the kinetics of chemical reactions | Collision Theory |
| Minimum kinetic energy needed in a collision for particles to bond | Activation Energy |
| Law that relates the rate of a reaction to the concentration of the reactants | Rate Law |
| General rate law | rate = k([A]^x)([B]^y) |
| Describes how changing the concentration of a reactant changes the reaction rate | Reaction Order |
| Laboratory technique that is used to determine an unknown concentration by reacting it with a substance of known concentration, using an indicator to signal the end of the reaction | Titration |
| Substance of unknown concentration in a titration | Analyte |
| Substance of known concentration in a titration | Titrant |
| Device used to slowly add titrant to the analyte in a titration | Buret |
| Formed when an acid donates a proton | Conjugate Base |
| Formed when a base accepts a proton | Conjugate Acid |
| Point in titration where the titrant and analyte concentrations are equal | Equivalence Point |
| Equivalence point for strong acid-base titration | 7 |
| When the indicator changes color in a titration | Endpoint |
| Equation that relates the pH of a buffer solution to the pKa of the weak acid and the ratio of the concentrations of the conjugate base and acid | Henderson-Hassalbach Equation |
| pKa equation | pKa = -log(Ka) |
| Henderson-Hassalbach Equation | pH = pKa + log([A-]/[HA]) |
| Study of reactions involving atomic nuclei | Nuclear Chemistry |
| Spontaneous emission of particles from an atomic nucleus | Radioactive Decay |
| Emission of a helium nucleus | Alpha Decay |
| What is an alpha particle | Helium Nucleus |
| Emission of a high-energy electron from the nucleus | Beta Decay |
| What is a beta particle | Electron |
| Change in atomic number after beta decay | +1 |
| Emission of a high-energy photon from the nucleus | Gamma Decay |
| What is a gamma particle | Photon |
| Time for half of a radioactive sample to decay | Half-Life |
| Splitting of a large nucleus to create smaller ones | Nuclear Fission |
| Type of nuclear reaction that fuels nuclear power plants | Nuclear Fission |
| Combining of smaller nuclei to create a larger one | Nuclear Fusion |
| Type of nuclear reaction that fuels the sun | Nuclear Fusion |
| Type of reaction where two molecules combine to form a larger one by breaking pi bonds | Addition Reaction |
| Type of reaction where one molecule splits into two smaller ones by adding pi bonds | Elimination Reaction |
| Type of reaction where an atom or group of atoms is replaced by a different atom or group of atoms | Substitution Reaction |
| Reactant that is electron rich, having a lone pair or pi bond that is attracted to positive charges | Nucleophile |
| Type of acid or base that nucleophiles are | Lewis Bases |
| Reactant that is electron poor because it is positively polarized or has an empty orbital | Electrophile |
| Type of acid or base that electrophiles are | Lewis Acid |
| Substitution reaction where the rate determining step is bimolecular | SN2 Reaction |
| What SN2 stands for | Substitution Nucleophilic Bimolecular |
| Study of interactions between matter and electromagnetic radiation | Spectroscopy |
| Type of spectroscopy that relies on the ability of bonds to vibrate | Infrared Spectroscopy |
| Information given by infrared spectroscopy | Functional Groups |
| Broad dip at 3300 inverse cm in an IR spectrum | Alcohol (O-H Bond) |
| Sharp peak at 1700 inverse cm in an IR spectrum | C=O Bond |
| Type of spectroscopy that bombards a sample with electrons to form a positive ion | Mass Spectrometry |
| Determines how much ions are deflected in mass spec | Mass-to-Charge Ratio |
| Plotted on an IR spectrum | Transmittance vs. Wave Number |
| Plotted on a mass spectrum | Relative Abundance vs. m/z |
| Information given by mass spectrometry | Molar Mass |
| Ion that is formed in mass spec | Molecular Ion |
| Peaks in mass spec act like this for molecular structure | Fingerprints |
| Farthest right peak in mass spec | Molecular Ion Peak |
| Type of spectroscopy that relies on spin | NMR Spectroscopy |
| Information given by NMR spec | Carbon-Hydrogen Framework |
| Chemical environment is given by this on an NMR spectrum | Chemical Shift |
| VSEPR | Valence Shell Electron Pair Repulsion |
| 3D arrangement of electron pairs around a central atom | Electron Geometry |
| 3D arrangement of all atoms in the molecule connected to the central atom | Molecular Geometry |
| Amount of bonds and lone pairs around a central atom | Steric Number |
| Electron geometry with a steric number of 2 | Linear |
| Electron geometry with a steric number of 3 | Trigonal Planar |
| Electron geometry with a steric number of 4 | Tetrahedral |
| Electron geometry with a steric number of 5 | Trigonal Bipyramidal |
| Electron geometry with a steric number of 6 | Octahedral |
| Molecular geometry with a steric number of 4 and 1 lone pair | Trigonal Pyramidal |
| Molecular geometry with a steric number of 3 and 1 lone pair | Bent |
| Molecular geometry with a steric number of 5 and 1 lone pair | Seesaw |
| Molecular geometry with a steric number of 5 and 2 lone pairs | T-Shaped |
| Molecular geometry with a steric number of 6 and 1 lone pair | Square Pyramidal |
| Molecular geometry with a steric number of 6 and 2 lone pairs | Square Planar |
| Homogeneous mixtures of two or more substances | Solution |
| Substance that does the dissolving in a solution | Solvent |
| Substance that is dissolved in a solution | Solute |
| Measure of solute in a given amount of solvent or in a given amount of solution | Concentration |
| Units of concentration | Molarity |
| Process of decreasing concentration by adding solvent | Diluting |
| Dilution equation | M1V1 = M2V2 |
| Solutions that have not yet been diluted | Stock Solution |
| State where the forward and reverse reactions in a reversible chemical reactions are equal | Chemical Equilibrium |
| Value that expresses the relationship between the concentration of reactants and products at equilibrium | Equilibrium Constant (Keq) |
| Standard Keq expression | Keq = (([C]^c)([D]^d))/(([A]^a)([B]^b)) |
| Direction of equilibrium if Keq is greater than 1 | Right |
| Direction of equilibrium if Keq is lower than 1 | Left |
| Value that expresses the relationship between the concentration of reactants and products at any point | Reaction Quotient (Q) |
| Direction that the reaction will shift if Q is less than Keq | Right |
| Direction that the reaction will shift if Q is greater than Keq | Left |
| Study of compounds with complex ions | Coordination Chemistry |
| Ions with a central metal cation bonded to one or more ligands | Complex Ions |
| Ions or molecules with lone pairs that become bonded to the central ion in a complex ion | Ligands |
| Number of ligands directly bonded to the central ion in a complex ion | Coordinate Number |
| Type of bond formed between the central metal ion and ligands in a complex ion | Coordinate Covalent Bond |
| Ligands that donate only one electron pair to the central metal | Monodentate Ligands |
| Ligands that donate two electrons pairs from two different atoms to the central metal | Bidentate Ligands |
| Ligands that can form two or more bonds to the central metal | Polydentate Ligands |
| Polydentate ligands are these agents | Chelating Agents |
| Section of the periodic table with transition metals | d-block |
| Study of chemical and biochemical phenomena that occur in natural places | Environmental Chemistry |
| Precipitation with a pH under 5.6 | Acid Rain |
| Acid rain is caused by the emission of these two types of compounds | Sulfur Oxides, Nitrogen Oxides |
| Atoms or molecules with an unpaired electron | Free Radicals |
| Atom that catalyzes ozone depletion | Chlorine Radical |
| Step of water treatment that causes small particles to clump together | Coagulation and Flocculation |
| Larger clumps formed by the coagulation of tiny dirt particles during water treatment | Floc |
| Step of water treatment where floc particles settle to the bottom of the tank | Sedimentation |
| Step of water treatment where water is passed through porous barriers to remove dissolved particles | Filtration |
| Step of water treatment where chlorine is added to kill any remaining bacteria or viruses | Disinfection |
| Steps of water treatment | Coagulation and Flocculation, Sedimentation, Filtration, Disinfection |
Created by:
KatieThiel