Barron's AP Chemistry 7th Edition - Vocabulary

The uncertainty of +_1 in the last digit of a measurement. If this uncertainty is different from +_1, it is written as part of the number; e.g 23.45+_0.05 indicates an uncertainty of +_5 in the last digit.

The lowest possible temperature, 0.0 K or -273.16 degree Celsius

A measure of the amount of light absorbed by a chemical

A constant the value of which depends on the sample and the wavelength at which the measurement is made in spectroscopy

The degree of closeness between a measured value and the true value

Any substance that donates protons, or as Lewis acids are electron - pair acceptors

The oxide of a nonmetal that forms an acid when dissolved in water

The value of the equilibrium expression for the dissociation of a weak acid

The structure of colliding molecules at the moment of collision, generally thought to be intermediate between the structures of the products and of the reactants.

The increase in potential energy, due to a molecular collision, necessary to convert a reactant into a product.

A listing of elemental substances in the order of their ability to be oxidized or reduced. This listing makes it possible to predict whether an element will cause the oxidation or the reduction of an ion of another element

The reaction in which a double bond opens to form two additional single bonds.

The attractive force between two dissimilar substances

An organic compound with an -OH group

An organic compound with a terminal -CHO group

The extremely reactive elements in the first group (column) of the periodic table. They all have ns1 electrons as valence electrons.

The very reactive elements in the second group (column) of the periodic table. They all have ns2 electrons as valence electrons.

Organic compounds with the general formula CnH2n+2

Organic compounds with double bonds in their structures

A functional group that is Alkane in nature

Organic compounds with triple bonds in their structures

One or more distinct forms of an element; classification as an allotrope is based on structure and physical properties, e.g diamond and graphite are two allotropes of carbon

A helium nucleus

Compounds, related to ammonia, in which one or more of the hydrogen atoms in ammonia have been replaces by organic functional groups

An organic acid that contains both an amine and an acid functional group on adjacent carbon atoms

A term meaning without structure

A term describing a substance that can donate a proton and accept a proton

A term describing a substance that can act as an acid or as a base

The oxide of a metal or nonmetal that reacts with water to form a acid or a base, respectively

An ion with a negative charge

A term designating a system that involves water or a chemical mixture or solution having water as the solvent

The equation that relates temperature to rate constant. K=Ae_Ea/RT.

The theory that an acid increases hydrogen ion concentration when dissolved and that a base increase hydroxide ion concentration when dissolved

A functional group that is aromatic in nature

A fundamental particle of chemistry. At present, 109 atoms are known and are arranged in an orderly manner in the periodic table.

The relative mass of an element as compared to the mass of the isotope C-12, which is defined as exactly 12

The number of an element in the periodic table; also, a number representing the number of protons in the nucleus of an atom.

The orbital structure of an element; also, an orbital within an element.

A one or two letter abbreviation of an elements name. Some symbols (Pb for lead) are derived from Latin names of the elements.

The value of the equilibrium expression for the dissociation of water into H+ and OH_

A quantity equal to 6.022 X 10^23

A statement of the direct relationship between the moles of a gas and the volume of that gas.

A term used to describe the position of an atom in a covalent molecule of the AX5 or AX6 basic structure. The axial atom are on the vertical axis of the molecule in positions similar to the Earth's North and South Poles.

The quantum number that specifies the sublevel in which an electron is located; l may be any number from zero up to n_1

A chemical equation that has the smallest whole number coefficients for the reactions and products so that there is the same number of atoms of each element on both sides of the arrow.

A closed end manometer used for measuring atomsphere pressure

Any compound that increases the hydroxide concentration of a solution or is a proton acceptor. Lewis bases are electron pair donors.

The value of the equilibrium expression for the dissociation of a weak base.

One of five basic geometries linear, triangular planar, tetrahedral, trigonal planar, or octahedral that a molecule may take.

The oxide of a metal that forms a base when dissolved in water.

A galvanic cell used to produce electricity for consumer items such as flashlights, portable radios, and heart pacemakers.

The statements that the absorbance of a sample is the product of the absorptivity, optical path length, and sample concentration; A=abc.

An electron

A Lewis base that donates two pairs of electrons.

An acid that contains hydrogen and one other element in its formula.

A cubic structure in which one atom is at each of the eight corners and one atom is in the center of the unit cell.

The model of the atom developed by Niels Bohr. This model views electrons as circling the nucleus like a miniature solar system.

The temperature at which the vapor pressure of a liquid is equal to 760 millimeters of mercury (1.00 atmospheres): also, the temperature at which a gas condenses, also called condensation point.

The temperature increase of the boiling point per molal noun of solute particles.

A pair of electrons that participate in a covalent bond.

The average number of bonds per atom covalently bonded to a central atom.

The law that expresses the inverse relationship between the volume and the pressure of a gas; PV = constant.

The equation that relates the atomic dimensions in a crystal to the angles at which monochromatic X-Rays will undergo constructive reinforcement

The theory that acids are proton donors and bases are proton acceptors.

The allotrope of carbon that has the formula C60.

The moles of strong acid or stronge base required to change the pH of a liter of buffer by 1 pH unit.

An aqueous solution containing a conjugate acid and its conjugate base a molar ratio greater than 0.1 and less than 10.0.

The violent boiling that occurs when a solution becomes superheated.

A tube approximately 1 centimeter in diameter that is used for measuring liquid volumes of 10-100 milliliters

An instrument used to determine heat energy

A substance that speeds up the rate of a chemical reaction by providing an alternative reaction pathway with a lower activation energy

An ion with a positive charge.

The voltage of a galvanic cell under nonstandard state conditions.

The process of separating a solid from a liquid by spinning it rapidly to artificially increase the gravitational force.

A nuclear reaction that produces more neutrons than were needed to initiate it, therefore causing more reactions than occurred in the preceding step.

The law that expresses the direct relationship between the temperature and volume of a gas: P/V = constant

A Lewis base that usually has more than one pair of electrons to donate.

An isomer with substituents on the same side of the double bond.

A system in which mass cannot be lost to or gained from the surroundings.

A number placed in front of a chemical formula to represent the number of molecules of that substance that are included in the equation. This number multiplies the number of atoms in the formula unit.

The sum of all the attractive forces in a pure substance

Any one of several physical properties of a solution that change depending on the amount of solute particles present in the solution.

The theory of kinetics, which relates reaction rates to the frequency, energy and orientation of molecules in collisions.

A reaction between a Lewis acid and a Lewis base.

A combination of one or more compounds or anions with a metal ion by coordination covalent bonding, also called complex.

A combination of two or more elements into a distinct substance with definite physical properties.

A qualitative term indicating a large amount of solute in a given amount of solvent.

An expression of the amount of solute mixed with a solvent.

A graph of reactant or product concentration as a function of time

The conversion of gas into a liquid.

A polymerization reaction between an acid and either an alcohol or an amine.

Any substance that has a proton that may be donated to a base.

A pair of substances whose formulas differ by one H+ ion.

A series of two or more double bonds, each separated by only a single bond in a molecule.

A graph showing the changes that occur while a substance is cooling.

The covalent bond between two atoms that is formed when one substance donates both electrons.

The bond between two atoms that arises from the sharing of a pair of electrons

A chemical compound in which the atoms are held together with covalent bonds

The crystal that consists of only one molecule. All atoms are joined to others with covalent bonds. Also called network crystal

The minimum mass of a fissile (fissionable)material needed to sustain a nuclear chain reaction.