Chemistry Glossary CliffsNotes Flashcards
Finished. Very basic. I want everyone to go over it to gain basic chemistry knowledge.
Acid
A compound that yields H+ ions in solution or a solution in which the concentration of H+ exceeds OH-.
Acid ionization constant
The equilibrium constant describing the degree of ionization of an acid.
Actinides
The row of elements below the main section of the periodic table, from thorium to lawrencium.
Alkali
Synonym for base.
Alkali metals
The column of elements from lithium to francium.
Alkaline earth metals
The column of elements from beryllium to radium.
Alkene
A hydrocarbon with one or more double bonds and no triple bond.
Alkane
A hydrocarbon without a double bond, triple bond, or ring structure.
Alkyne
A hydrocarbon with one or more triple bonds.
Alpha particle
A cluster of two protons and two neutrons emitted from a nucleus in one type of radioactivity.
(Helium-4 Nucleus)
Anoin
A chemical species with a negative charge.
Anode
The electrode at which oxidation occurs.
Aqueous
Refers to a solution with water as the solvent.
Aromatic
Refers to an organic compound with a benzene-like ring.
Atom
The smallest amount of an element; a nucleus surrounded by electrons.
Atomic number
The number of protons in the nucleus of the chemical element.
Atomic mass
The mass in grams of one mole of the chemical element; approximately the number of protons and neutrons in the nucleus.
Avogadro’s Law
Equal volumes of gases at the same temperature and pressure contain the same number of molecules.
Avogadro’s Number (or Avogadro’s constant)
6.02 x 10^23, the number of molecules in one mole of a substance.
Base
A compound that yields OH- ions in solution or a solution in which the concentration of OH- exceeds H+.
Beta particle
An extremely fast moving electron emitted from a nucleus in one type of radioactivity.
Boiling point
the temperature at which a liquid changes to a gas. (Technically, boiling point is the temperature at which the vapor pressure of the liquid is equal to atmospheric pressure).
Boiling point elevation
An increase in the boiling point of a solution, proportional to the concentration of solute particles.
Boyle’s Law
The volume of a gas varies inversely with pressure.
Calorie
A unit of energy, equal to 4.184 joules.
Catalyst
A substance that accelerates a chemical reaction without itself being consumed.
Cathode
The electrode at which reduction occurs.
Cation
An atom or molecules with a positive charge.
Charles’ Law
The volume of a gas varies directly with absolute temperature.
Chemical Equation
A shorthand way of describing a chemical change using symbols of elements and formulas of compounds.
Compound
A substance formed by the chemical combination of two or more elements.
Concentration
The relative amount of a solute in a solution.
Congeners
Related chemical substances “related to each other by origin, structure, or function”
Conjugate
An acid and a base that are related by removing or adding a single hydrogen ion.
Covalent bond
Atoms linked together by sharing valence electrons.
Critical point
A point in a phase diagram where the liquid and gas states cease to be distinct.
Crystalline
The regular, geometric arrangement of atoms in a solid.
Decomposition
A chemical reaction in which a compound is broken down into simpler compounds or elements.
Dissociation
The separation of a solute into constituent ions.
Electrochemical cell
A device that uses a chemical reaction to produce or use an electric current.
Electrode
The point in an electrochemical cell at which reduction or oxidation occurs.
Electrolysis
The decomposition of a substance by an electric current.
Electrolyte
A substance that forms ions when dissolved in water.
Electromotive force
The electrical potential produced by a chemical reaction, voltage.
Electron
A light subatomic particle with negative charge; found in orbitals surrounding an atomic nucleus.
Electronegativity
A number describing the attraction of an element for electrons in a chemical bond.
Element
A substance that cannot be decomposed; each chemical element is characterized by the number of protons in the nucleus.
EMF
Electromotive force (See that card)
Endothermic
Refers to a reaction that absorbs heat.
Energy
The concept of motion or heat required to do work.
Enthalpy
The thermodynamic quantity measuring the heat content of a substance.
Entropy
The thermodynamic quantity measuring the disorder of a substance.
Equilibrium
A balance condition resulting from two opposing reactions or processes.
Equilibrium constant
The ratio of concentrations of products to reactants for a reaction at chemical equilibrium.
Exothermic
Refers to a reaction that releases heat.
Faraday
A unit of electric charge equal to that of one mole of electrons.
Faraday’s Laws
Two laws of electrolysis relating the amount of substance to the quantity of electric charge.
Fluid
Any substance that flows or deforms under an applied shear stress; any liquid or gas.
Free energy
The thermodynamic quantity measuring the tendency of a reaction to proceed; also called Gibbs free energy.
Freezing point
The temperature at which a liquid changes into a solid.
Freezing point depression
The decrease in freezing point of a solution, proportional to the concentration of solute particles.
Fusion
Melting. (?)
Gamma radiation
Energy released from a nucleus during radioactive decay.
gas
A state of matter in which molecules are widely separated, fluid, expandable, and compressible.
Gas constant
R equals 0.082 liter-atmospheres per mole-unit Kelvin.
Gram formula mass
An amount of a substance equal in grams to the sum of the atomic mass.
Ground state
The electronic configuration of lowest energy for an atom.
Group
A column of elements in the periodic table.
Half-reaction
An oxidation or reduction reaction with free electrons as a product or reactant.
Halogens
The column of elements from fluorine to astatine.
Heat
A form of energy that spontaneously flows from a warm body to a cold body. (Snuggles! :)
Heat capacity
The amount of energy needed to raise the temperature of a substance by one degree Celsius.
Hydrocarbon
An organic compound containing only carbon and hydrogen.
Hydrogen bond
A weak, secondary bond between a partially positive hydrogen atom and a partially negative N, O, or F atom; an intermolecular force of attraction.
Hydroxide
Refers to the OH- ion.
Ideal gas equation
The equation relating the volume of a gas to its pressure, temperature, and moles of gas.
Inert gases
The column of elements from helium to radon; also called noble gases.
Ion
An atom with an electric charge due to gain or loss of electrons.
Ionic bond
Atoms linked together by the attraction of opposite charges.
Ionic disassociation
Separation of cations and anions from an ionic compound by polar water molecules.
Ionization
Removing electrons from an atom; alternatively, the dissociation of a solute into ions.
Isoelectronic
Refers to several dissimilar atoms or ions with identical electronic configurations.
Isomers
Several molecules with the same composition but different structures.
Isotope
A variety of an element characterized by a specific number of neutrons in the nucleus.
Joule
A unit of energy equal to 0.239 calorie.
Lanthanides
The row of elements beneath the main section of the periodic table, from cerium to lutetium; also called rare earths.
Le Chatelier’s Principle
A system that is in equilibrium is disturbed adjusts so as to minimize the disturbance.
Liquid
A state of matter in which the molecules are touching, fluid, and incompressible.
Litmus
An indicator that turns red in acid and blue in alkaline solution.
Mass number
The sum of the number of neutrons and protons in the nucleus of an atom.
Mass percent
The percentage found by taking the mass of an element and dividing it by the mass of a sample and then multiplying by 100.
Melting point
The temperature at which a solid changes to a liquid.
Metallic bond
Atoms linked together by the migration of electrons from atom to atom.
Metals
The elements in the middle and left parts of the periodic table, except for hydrogen.
Molality
The number of moles of solute in one kilogram of solvent.
Molar heat capacity
the amount of heat required to raise the temperature of one mole of substance one degree Celsius.
Molarity
The number of moles of solute in one liter of solution.
Mole
An amount of a substance equal in grams to the sum of the atomic weights.
Mole fraction
The fraction of moles (or molecules) of one substance in the total moles (or molecules) of all substances in the mixture. If the mole fraction of substance A is 0.1, one tenth of all the molecules in a mixture are A molecules.
Molecular formula
Describes the ration of moles of the elements in a molecule.
Molecule
A group of atoms linked together by covalent bonds.
Neutralization
The chemical reaction of an acid and base to yield a salt and water.
Neutron
A heavy subatomic particle with zero charge; found in an atomic nucleus.
Noble gases
The column of elements from helium to radon; also called inert gases.
Nonmetals
The elements in the upper right part of the periodic table, and also hydrogen.
Nucleon
A proton or neutron found in an atomic nucleus.
Nucleus
The core of an atom, containing protons and neutrons.
Orbital
A region in space surrounding the nucleus, which is occupied by up to two electrons. (bullcrap- can have 8)
Organic
Refers to compounds based on carbon.
Organic chemistry
An area of chemistry dealing principally with the chemistry of carbon.
Oxidation
The loss of electrons by a species.
Oxidation number
A signed integer representing the real or hypothetical charge of an atom due to the gain or loss of electrons.
Oxidation-reduction reaction
Reaction in which electrons are transferred between atoms.
Oxide
A compound of oxygen and another element.
Oxidizing agent
The species that is reduced during a redox reaction.
Period
A horizontal row of elements in the periodic table.
pH
A number describing the concentration of hydrogen ions in a solution; equals -log[H+]
Phase
A substance with uniform composition and definite physical state.
Polar bond
A bond with both ionic and covalent characteristics.
Polyprotic
Refers to an acid with several hydrogens that can ionize.
Precipitate
A solid that separates from solution.
Product
A substance on the right side of a chemical equation, which is produced or formed during a chemical reaction.
Proton
A heavy subatomic particle with a positive charge; found in an atomic nucleus.
Radioactive decay
The spontaneous disintegration of an unstable nucleus producing a different nucleus and various types of radiation particles.
Radioactivity
The emission of subatomic particles from a nucleus.
Rare earths
The elements from cerium to lutetium; lanthanides.
Reactant
A substance on the left side of a chemical equation which is one of the beginning substances in a chemical reaction.
Redox
Refers to a reaction in which simultaneous reduction and oxidation occur.
Reducing agent
The species that is oxidized during a redox reaction.
Reduction
The gain of electrons by a species.
Salt
A solid compound composed of both metallic and nonmetallic elements, often as ions.
Saturated
Describes a solution that holds as much solute as possible.
Saturated hydrocarbon
A hydrocarbon containing only single bonds between the carbon atoms.
Shell
A set of electron orbitals with the same principal quantum number.
Solid
A state of matter in which the molecules are touching and possessing rigid shape and which is not compressible.
Solubility
The upper limit of concentration of a solute.
Solubility product
The constant obtained by multiplying the ion concentrations in a saturated solution raised to their balancing coefficients.
Solute
The substance that is dissolved in a solution.
Solution
A homogenous mixture consisting of a solvent and one or more solutes.
Solvent
The host substance of dominant abundance in a solution.
Specific heat capacity
The amount of heat required to raise 1 gram of a substance 1 degree Celsius.
Standard Temperature and Pressure (STP)
0 degrees Celsius and 1 atmosphere pressure. (Note: 1 mole of any gas at STP has a volume of 22.4 liters.)
States of matter
Solid, liquid, gas.
Stoichiometric
Refers to compounds or reactions in which the components are in fixed, who-number rations.
Strong electrolyte
An acid, base, or salt that dissociates almost completely to ions in aqueous solution.
Structural formula
Depicts the bonding of atoms in a molecule.
Sublimation
The transformation of a solid directly to a gas without an intervening liquid state.
Subshell
A set of electron orbitals with the same principal and second quantum number. 2p, 3s, etc are examples.
Supersaturated
Describes a solution that holds more solute than is theoretically possible at that given temperature.
Symbol
An abbreviation for the name of an element.
Thermodynamics
The study of energy, principally heat energy, that accompanies chemical or physical changes.
Transition metals
The three rows of elements in the middle of the periodic table, from scandium to zinc, the yttrium to cadmium, and lanthanum to mercury.
Transmutation
The process of changing one chemical element to another element during radioactive decay.
Triple point
A point in a phase diagram where the three states of matter are in equilibrium.
Unsaturated
Describes a solution that does not hold as much solute as possible.
Unsaturated hydrocarbon
A hydrocarbon that contains double or triple bonds between at least two of its carbon atoms.
Valence
A signed integer describing the combining power of an atom.
Valence electrons
The outermost shell of electrons in an atom or ion.
Voltaic cell
A device that uses chemical reaction to produce electricity.
Weak electrolyte
An acid, base, or salt that dissociates only slightly to form ions in solution.
