| Term | Definition |
|---|
| strong acid | pH<7 an acid that ionizes completely in aqueous solution |
| actual yield | the amount of product actually produced when a chemical reaction is carried out in an experiment. |
| amphoteric | any species that can react as wither an acid or base |
| arrhenius acid/ base | a chemical compund that increases in caoncentration of H+ in an auqeous solution; a substances that increases the concentration of OH- in an aqueous solution |
| strong base | pH>7 is most commonly thought of as an aqueous substance that can accept protons. |
| boiling point | The temperature at which a liquid's vapor pressure is equal to the external or atmospheric pressure. |
| Bronstead Lowry | A model of acids and bases in which an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor. |
| buffers | weak acid and a salt of the acid that causes a solution to resist changes in pH |
| chemical reactions | The process by which the atoms of one or more substances are rearranged to form different substances; occurrence can be indicated by changes in temperature, color, odor, and physical states. |
| colligative properties | A physical property of a solution that depends on the number, but not the identity, of the disswolved solute particles; example properties include vapor pressure lowering, boiling point elevation, osmotic pressure, and frezzing point depression |
| colloids | Heterogeneous mixture containg particles larger than solution particles but smaller than suspension particles that are categorized according to the phases of heir dispersed particles and dispersing mediums. |
| composition reactant | a reaction in which two or more substances combine to form a new compound |
| concentration | solurte/solvent; molartity; is the measure of how much of a given substance there is mixed with another substance. |
| conductivity | ability to conduct electricity |
| conugate acids | The species produced when a base accepts a hydrogen ion from an acid. |
| Dalton's Law | States that the total pressure of a mixture of gasses is equal to the sum of the pressures of all the gases in the mixture. |
| density | A ration that compares the mass of an object to its volume. |
| dilute | to make (a liquid) thinner or weaker by the addition of water or the like. |
| dissociation | the separation of ions that occurs when an ionic compund dissolves |
| effervescence | the rapid escape of a gas from the liquid in which it is dissolved (opening and pouring soda) |
| electrolyte | a subatance that dissolves in water to give a solution that conducts electric current |
| endothermic (and sign) | noting or pertaining to a chemical change that is accompanied by an absorption of heat (delta H) |
| equilibrium | a dynamic condition in which two opposing changes occur at equal rates in a closed system |
| equilibrium constant | the ratio of the mathmetical product of the concentrations of substances formed at equilibrium to the mathematical product of the concentrations of hte reacting substances. Each concentration is raised to a power equal to the soeffienct that substance in the shemical equation. |
| equilibrium vapor pressure | the pressure exterted by vapor in equilibrium with its corresponding liquid at a given temperature |
| evidence of chemical reaction | change in color, smell, fromation of ppt |
| excess reactant | the substance that is not used up completely in a reacition |
| exothermic (and sign) | noting or pertaining to a chemical change that is accompanied by a liberation of heat (delta) |
| gas | the state of matter in which a substance has neither definite volume or shape |
| heterogeneous | not having a uniform composition throughout |
| homogeneous | having a uniform composition throughout |
| IMAFs (3) | .the force of attraction between moecules: London Dispersion Forces, Dipole-Dipole Forces, and Hydrogen bonding |
| ionization | the formation of ions from solute molecules by the action of teh solvent; andy process that results in the formation of an ion |
| kinetic energy | the energy of a body or a system with respect to the motion of the body or of the particles in the system. |
| kinetic molecular theory | .Explains the properties of gases in terms of the energy, size, and motion of their particles. |
| Le Chatelier | when a system at equilibrium is distriubuted by application of a stress, it attains a new euqilibrium poistion that minimizes the stress |
| limiting reactant | the reactant that limits the amounts of the other reactants that can combine- and the amount of product that can form- chemiscal reation |
| liquid | the state of matter in which the substance has definite volume but indefinite shape |
| Molality (m) | the cincentration os solution expressed in moles of solute per kilogram of solvent |
| Molarity (M) | The number of moles of solute dissolved per liter of solution; also known as molar concentration. |
| mole ratio | In a balanced equation, the ratio between the numbers of moles of any two substances. |
| neutral | pH=0 exhibiting neither acid nor alkaline qualities |
| percent yeild | The ratio of actual yield (from an experiment) to theoretical yield (from stichiometric calculations) expressed as a percent. |
| pH | The negative logarithm of the hydrogen ion concentration of a solution; acidic solutions have pH values between 0 and 7, basic solutions have values 7 and 14, and a solution with a pH of 7 is neutral. |
| phase changes | A type of change that alters the physical properties of a substance but does not change its composition. |
| pOH | The negative logarithm of the hydroxide ion concentration of a solution; a solution with a pOH above 7 is acidic, a solution with a pOH below 7 is basic, and a solution with a pOh of 7 is neutral. |
| polarity | attraction toward a particular object orin a specific direction |
| pressure (P) | Force applied per unit area. (atm) |
| salt | an ionic sompund composed of a cation and anion from an acid; an inoic compound composed of a cation from a base and an anion from and acid |
| saturated | a solution that sontians the maximum amount of dissolved solute |
| solid | the state of matter that has definite volume and definite shape |
| solubility | the amount of a substance required to form a saturated solution with a specific amount of solvent at a specified temperature |
| solution | A uniform mixture that may contain solids, liquids, or gasas; also called a homogeneous mixture. |
| spectator ions | ions that don't take part in ta chemical reation and is found in asolution both before and after the reaction. |
| supersaturated | a solution that contains more dissolved solute than saturated solution contians under the same conditions |
| suspension | A type of heterogeneous mixture whose particles settle out over time and can be seperated from the mixture by filtration. |
| temperature | A measure of the average kinetic energy of the particles in a sample of matter. |
| theoretical yeild | In a chemical reaction, the maximum amount of product that can be produced from a given amount of reactant. |
| titration | the controlled addition and measurement of the amount of a solution of known concerntration required to react sompletely with a measured amount of a solution of unknown concentration. |
| Tyndall effect | The scattering of light by colloidal particles. |
| unsaturated | a solution that contians less solute that a saturated solution under the existing conditions |
| conjugate base | The species produced when an acid donates a hydrogen ion to a base. |
| effects of temperature | The chemical effects of greater temperature include changes in the rate of reaction and the position of chemical equilibrium. Almost all reactions proceed more rapidly at higher temperatures because the molecules (in the gas phase) collide more vigorously at higher temperatures. A thermodynamic consequence of changing temperature is that the equilibrium constant of an exothermic reaction decreases as the temperature is raised, so reactants are more favored at low temperatures than at high. This dependence is sometimes referred to as Le Chatelier's principle, but it is better to regard it as a consequence of thermodynamics and in particular of the second law of thermodynamics.The higher the temperature, the greater the proportion of molecules in a state of high energy. High temperature corresponds to a higher average speed of the molecules and a wider range of speeds in the sample. |
| solubility rules | (refer to your chem notes) |
| solubility of gasses | Henry's Law; The solubility of a gas in a liquid depends on temperature, the partial pressure of the gas over the liquid, the nature of the solvent and the nature of the gas. The most common solvent is water. |
| solubility of solids | The solubility of a solid substance usually refers to the concentration of the substance in a liquid that has reached equilibrium with the substance in solid phase. solubility is determined by the combination of substance and liquid |
| nonpolar | a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in abalanced distribution of electrical charge |
| polar | having an uneven distribution of charge |
| precipitate (ppt) | a solid that is produced as a result of chemical reations in a solution and that separates from the solution |
| enthalpy change | the amount of energy absorbed or lost by a system during a process at constant pressure |
| strong electrolyte | any compound of which all or almost all of the dissolved compound exists as ions in aqueous solutions |
| weak electrolyte | a coumpound of which a relatively small amount of the dissolved compound exists as ions in an aqueous solution |
| nonelectrolyte | a substance that dissolves in water to give a solution that does not conduct an electric current |
| weak acid | pH<7 an acid that is weak electrolyte and does not completely ionize |
| weak base | pH>7 is most commonly thought of as an aqueous substance that can accept protons. |
| Concentrated | a solution containing relatively large amounts of solute |
| enthalpy of fusion | Energy required to convert a solid to a liquid. |
| enthalpy of vaporization | the amount of heat energy required to vaporize a metal, a measure of the strength of the bonds that hold it together |
| Enthalpy of solution | the net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent. |
| enthalpy of vaporization | the amount of heat energy required to vaporize a metal, a measure of the strength of the bonds that hold it together |
| Strong Acids | HI, HBr, HCl, HNO3, H2SO4, HClO3, HClO4 (BrICl NO SO) |
| Strong Bases | LiOH, NaOH, KOH, RbOH, Ba(OH)2, Sr(OH)2, Ca(OH)2 (CaSr Na BALiK) |
| common industrial acids | sulfuric, nitric, phosphoric, hydrochloric, acetic |
| Lewis Acid | Electron Acceptor |
| Lewis Base | Electron Donor |
| amphiprotic | can donate or accept proton (ie: H20) |
| BrINClHOF | Bromine, Iodine, Nitrogen, Chlorine, Hydrohen, Oxygen, Fluorine (written with subscript 2 by when by itself) |
| London Dispersion | temporary(spontaneous) dipole- induced dipole attraction. Only possible attractive forces for nonpolar molecules. As the size of the molecule increases, the strength of the forces increase. |
| Dipole-Dipole | attraction between negative and positive ends of POLAR moecules. Stronger than London dispersion forces |
| Hydrogen Bonding | Very strong dipole-dipole attraction, only possible when Hydrogen is bonded with F, O, or N |
| Balancing Chemical Equations | (super obvious, refer to notes if you need help) |
| Soichiometry | the calculation of quantitative (measurable) relationships of the reactants and products in a balanced chemical reaction (refer to notes for set up and practice probs) |
| Percent yeilds | Percent yield= 100x (atual amount/ predicted amount) |
| Solutions | deals with molarity (refer to notes for set up) |
| Limiting reactants | The reactant in a chemical reaction that limits the amount of product that can be formed. The reaction will stop when all of the limiting reactant is consumed. (refer to notes for calculation set up) |
| Boyle's Law | Pressure-Volume Relationship: P1V1=P2V2 "Boyle the Peas and Vegetables" (refer to notes for practice probs) |
| Gay-Lussac's Law | Pressure-Tempurature Relationship: P1/ T1=P2/T2 "Gayle drives a PT cruiser" (refer to notes for practice probs) |
| Avogadro's Law | Equal volumes of gases at the same tempurature and pressure contain equal numbers of molecules. V=kn (constant x given moles) Standard molar volume of gas at STP: k (constant) = 1mol = 22.4L. |
| Combined gas Law | Expresses the relationship between pressure, volume, and tempurature of a fixed amount of gas. P1V1/T1=P2V2/T2 (refer to notes for practice probs) |
| Ideal gas Law | Relationship between pressure, volume tempurature, and number of moles of a gas: PV=nRT; R= 0.08206(ideal gas law contant) (refer to notes for practice probs) |
| Dalton's Law | The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases: Ptot= Pa + Pb + Pc. Appying Dalton's Law-The gas collected by water displacemen(or collected over water): Patm= Pgas + PH2O |
| Graham's Law | States that the rate of effusion of gases at the same tempurature and pressure are inversely proportional to the square root of their molar masses: Rate1 / Rate2 = square root of (Mass2 / Mass 1) [refer to notes for practice probs] |
| Henry's Law | The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid: kC ( constant x concentration) |
| Gas Law constant | k (constant)= R= 0.08206(ideal gas law contant); units(R): L*atm/ mol*K |
| Gas Law units | Pressure (P), Volume (V) , moles(n) , R (constant), Tempurature (T) |
| Gas Law variables | atm (P), L [Liter] (V), mol (n), L*atm/ mol*K (R), K [Kelvin] (T) |
| BCE | A Balanced Chemical Equation has an equal ratio of moles on both sides of the equation, written with phases. |
| TIE | Total Ionic Equation includes every single part of the reaction; all ionized reactants and products. |
| NIE | Net Ionic Equation include only those compoudns and ions that undergo a chemical change in a reaction in an aqueos solution |
| Colligative Properties | property determined by the number of particles present in a system but that is independent of of the properties of the particles themselves. (1) Vapor Pressure Lowering (2) Boiling Point Elevation [delta tb=Kbm] (3) Freezing Point depression [delta tf=Kfm] (4) Osmotic Pressure [external pressure that must be applied to stop osmosis] |
| Equilibrium calculations | K= [C]c [D]d / [A]a [B]b (eqilibrium constant): K, Kc, Keq, Ka, Kb, Kw, Ksp, Kp (refer to notes for set up and practice probs) |
| Rate of dissolution | (rate of solubility) Factors that affect this are increasing the surface area of the solute, agitating a solution, and heating a solvent |
| Types of Chemical reactions | Synthesis, decomposition, single replacement, double replacement, combustion (products= CO2 + H2O), acid-base |
| Titrations | a method used to determine he concentration of a substance in a solution of known volume and concentration until the reaction is completed, which is usually indicated by a change in color. (refer to notes for calculation set up) |
| Standard Tempurature Pressure (STP) | 0 degrees C, one atm (760 mmHg, 760 torr) |
| Charle's Law | Volume- Tempurature Relationship: V1/T1=V2/T2 (refer to notes for practice probs) |
| absolute zero (relating to gas laws) | when determining Kelvin for gas law equations, K= 273.15 + C (degrees celcius in the prob) |
| miscible | two liquids will mix |
| immiscible | liquids won't mix |
| acids | sour taste, change color of acid-base indicator, react w/ active metals and release hydrogen gas, react w/ bases to produce salts and water, conduct electric current |
| bases | bitter taste, change color of acid-base indicator, feel slippery, react w/ acids to produce salts and water, conduct electric current |
| Polyprotic | Monoprotic: HCl Diprotic:H2SO4 Polyprotic: H3PO4 |
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