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76 Cards in this Set
- Front
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energy |
the capacity to do work measured in Joules (J). Never created or destroyed. |
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evaporation |
the change of a substance from a liquid to a gas |
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endothermic |
describes the process in which heat is absorbed from the environment |
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exothermic |
describes the process in which a system releases heat into the environment |
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law of conservation of energy |
the law that states that energy cannot be created or destroyed but can be changed from one form to another |
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heat |
the energy transferred between objects that are at different temperatures |
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kinetic energy |
the energy of an object that is due to the object’s motion |
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temperature |
a measure of how hot or cold something is; specifically, a measure of the average kinetic energy of the particles in an object. |
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specific heat |
the quantity of heat required to raise a unit mass of homogeneous material 1 K or 1°C in a specified way given constant pressure and volume |
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enthalpy |
the sum of the internal energy of a system plus the product of the system’s volume multiplied by the pressure that the system exerts on its surroundings. |
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thermodynamics |
the branch of science concerned with the energy changes that accompany chemical and physical changes. |
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calorimetry |
the measurement of heat-related constants, such as specific heat or latent heat. |
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calorimeter |
a device used to measure the heat absorbed or released in a chemical or physical change. |
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Hess's law |
the law that states that the amount of heat released or absorbed in a chemical reaction does not depend on the number of steps in the reaction. |
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evaporation |
the change of a substance from a liquid to a gas |
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boiling point |
the temperature and pressure at which a liquid and a gas are in equilibrium |
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condensation |
the change of state from a gas to a liquid |
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melting |
the change of state in which a solid becomes a liquid by adding heat or changing pressure |
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melting point |
the temperature and pressure at which a solid becomes a liquid |
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freezing |
the change of state in which a liquid becomes a solid as heat is removed |
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freezing point |
the temperature at which a solid and liquid are in equilibrium at 1 atm pressure; the temperature at which a liquid substance freezes |
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sublimation |
the process in which a solid changes directly into a gas (The term is sometimes also used for the reverse process.) |
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heat of fusion |
The enthalpy of fusion also known as (latent)heat of fusion is the change in enthalpy resulting from heating a given quantity of a substance to change its state from a solid to a liquid. The temperature at which this occurs is the melting point. |
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heat of evaporation |
The Heat (or Enthalpy) of Vaporization is the quantity of heat that must be absorbed if a certain quantity of liquid is vaporized at a constant temperature. In a solution with both a vaporized and liquidized states, the kinetic energy of the vapor is higher than the kinetic energy of the liquid. |
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entropy |
a measure of the randomness or disorder of a system. A thermodynamic property which has unit - s J/K |
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Gibbs energy |
the energy in a system that is available for work represented by G (G = H - TS). Also called free energy. |
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molar heat capacity |
(of a pure substance) is the energy as heat needed to increase the temperature of 1 mol of a substance by 1 K. |
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ppm |
One unit of concentration used in pollution measurements that involve very low concentrations. Parts per million is the number of grams of solute in 1 million grams of solution. g solute 1000 000 g solution m |
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molarity |
a concentration unit of a solution expressed as moles of solute dissolved per liter of solution. |
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concentration |
the amount of a particular substance in a given quantity of a mixture, solution, or ore |
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solute |
in a solution, the substance that dissolves in the solvent |
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solvent |
in a solution, the substance in which the solute dissolves |
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chemical equilibrium |
a state of balance in which the rate of a forward reaction equals the rate of the reverse reaction and the concentrations of products and reactants remain unchanged |
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Keq |
a number that relates the concentrations of starting materials and products of a reversible chemical reaction to one another at a given temperature |
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Ksp |
the equilibrium constant for a solid that is in equilibrium with the solid’s dissolved ions |
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Le Chatelier’s principle |
the principle that states that a system in equilibrium will oppose a change in a way that helps eliminate the change |
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strong acid |
an acid that ionizes completely in a solvent (e.g., Nitric acid, HNO3) |
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weak acid |
an acid that releases few hydrogen ions in aqueous solution (e.g., Hypochlorous acid, HOCl) |
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strong base |
a base that ionizes completely in a solvent (e.g., sodium hydroxide, NaOH) |
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weak base |
a base that releases few hydroxide ions in aqueous solution (e.g., Ammonia, NH3) |
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Bronsted-Lowry acid |
a substance that donates a proton to another substance |
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Bronsted-Lowry base |
a substance that donates a proton to another substance |
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conjugate acid |
an acid that forms when a base gains a proton |
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conjugate base |
a base that forms when an acid loses a proton |
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amphoteric |
describes a substance, such as water, that has the properties of an acid and the properties of a base |
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pH |
a value used to express the acidity or alkalinity of a solution; it is defined as the logarithm of the reciprocal of the concentration of hydronium ions; a pH of 7 is neutral, a pH of less than 7 is acidic, and a pH of greater than 7 is basic |
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pOH |
a measure of hydroxide ion (OH-) concentration. It is is a measure of the alkalinity of a solution. |
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Self-ionization constant of water, Kw |
the product of the concentrations of the two ions that are in equilibrium with water; [H3O+ ][OH− ] |
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neutral |
describes an aqueous solution that contains equal concentrations of hydronium ions and hydroxide ions |
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indicator |
a compound that can reversibly change color depending on the pH of the solution or other chemical change |
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neutralization reaction |
the reaction of the ions that characterize acids (hydronium ions) and the ions that characterize bases (hydroxide ions) to form water molecules and a salt |
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titration |
a method to determine the concentration of a substance in solution by adding a solution of known volume and concentration until the reaction is completed, which is usually indicated by a change in color |
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buffer solution |
a solution made from a weak acid and its conjugate base that neutralizes small amounts of acids or bases added to it. |
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reaction rates |
the rate at which a chemical reaction takes place; measured by the rate of formation of the product or the rate of disappearance of the reactants |
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rate law |
he expression that shows how the rate of formation of product depends on the concentration of all species other than the solvent that take part in a reactionrate = k[reactant]n |
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reaction mechanism |
the way in which a chemical reaction takes place; expressed in a series of chemical equations |
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order |
in chemistry, a classification of chemical reactions that depends on the number of molecules that appear to enter into the reaction |
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rate-determining step |
in a multistep chemical reaction, the step that has the lowest velocity, which determines the rate of the overall reaction |
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activation energy |
the minimum energy required to start a chemical reaction and is represented by the symbol Ea. No reaction is possible if the colliding pair has less energy than Ea. |
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activated complex |
a molecule in an unstable state intermediate to the reactants and the products in the chemical reaction. Also called transition state. |
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catalyst |
a substance that changes the rate of a chemical reaction without being consumed or changed significantly |
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enzyme |
a type of protein that speeds up metabolic reactions in plants and animals without being permanently changed or destroyed |
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nucleons |
a proton and a neutron |
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isotope |
One of two or more atoms that have the same atomic number (the same number of protons) but a different number of neutrons. Carbon 12, the most common form of carbon, has six protons and six neutrons, whereas carbon 14 has six protons and eight neutrons. Isotopes of a given element typically behave alike chemically. |
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nuclide |
an atom that is identified by the number of protons and neutrons in its nucleusquarks |
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strong force |
the interaction that binds nucleons together in a nucleus |
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radioactivity |
the process by which an unstable nucleus emits one or more particles or energy in the form of electromagnetic radiation |
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beta particle |
a charged electron emitted during a certain type of radioactive decay, such as beta decay |
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gamma ray |
the high-energy photon emitted by a nucleus during fisson and radioactive decay |
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nuclear fission |
the splitting of the nucleus of a large atom into two or more fragments, a process that produces additional neutrons and a lot of energy |
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chain reaction |
a reaction in which a change in a single molecule makes many molecules change until a stable compound forms |
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critical mass |
the minimum mass of a fissionable isotope that provides the number of neutrons needed to sustain a chain reaction |
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nuclear fusion |
the combination of the nuclei of small atoms to form a larger nucleus, a process that releases energy |
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half-life |
the time required for half of a sample of a radioactive substance to disintegrate by radioactive decay or natural processes |
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fusion |
fusion is the combining of nuclei to form a bigger and heavier nucleus |
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fission |
is the splitting of a heavy nucleus into lighter nuclei |
