Vocabulary
Acid-Base
reaction: a
reaction that involves the neutralization of an acid and a base.
Anion:
a negative ion
Atom: the smallest unit of an element
Atomic
mass:
the weighted average mass of the atoms in a naturally occurring element
Avogadro's
number: the number of particles in
one mole of a substance (6.022 x 1023)
Balanced
equation: a chemical equation where
there are equal numbers of atoms each element and charges on both reactant and
product sides.
British: the system of measurement
generally used in the USA (includes feet, pounds and seconds)
Cation: a positive ion
CGS:
a metric system of
measurement that used centimeters, grams, and seconds as standards
Chemical
equation: a representation of a
chemical reaction showing the relative numbers of reactant and product molecules
Chemical
property: a characteristic of a substance that when demonstrated changes the
identity of the substance
Chemical
symbol: an
abbreviation for the name of an element
Chromatography: the general name for a
series of methods for separating mixtures by employing a system with a mobile
phase and a stationary phase
Compound: a substance with constant
composition that can be broken down into elements by chemical processes
Concentration: an expression that relates
how solute molecules relate solvent molecules in a solution
Conversion
factor: a ratio of equivalent
quantities that is used to change one unit into another
Dimensional
analysis: a
method used to convert units by multiplying by ratios equivalent to one
Distillation: a method for separating
the components of a liquid mixture that depends on differences in the ease of
vaporization of the components
Electron: a negatively charged
particle that moves around the nucleus of an atom
Element: a substance that cannot be
decomposed into simpler substances by chemical or physical means
Empirical
formula: the
simplest whole number ratio of atoms in a compound
Experimental: numerical values that are
based on measurements taken during a laboratory exercise
Exponential
notation: expresses
a number as N x 10M, a convenient method for representing a very
large or very small number and for easily indicating the number of significant
figures
Filtration: a method for separating
the components of a mixture containing a solid and a liquid
Gas
forming reaction: a
chemical reaction in which a gas is formed during the reaction
Heterogeneous: a
mixture that has more than one phase
Homogeneous: a mixture that has only
one phase
Ionic
compound: a compound that results
when a metal reacts with a nonmetal to form a cation and an anion.
Ionic
reaction: a reaction where the
component ions of reactant compounds realign to form new compounds
Isotope: atoms of the same element
(the same number of protons) with different numbers of neutrons.
They have identical atomic numbers but different mass numbers.
Law
of Conservation of Mass:
mass is neither created or destroyed
Law
of Definite Composition: a
compound always contains exactly the same proportion of elements by mass
Law
of Multiple Proportions: a law
stating that when two elements form a series of compounds, the ratios of the
masses of the second element that combine with one gram of the first element can
always be reduced to small whole numbers
Main-group
elements:
elements which belong to the Groups 1A – VIIIA
Mass: the
amount of matter a material contains
Mass
percentage: the percent by mass of a
component of a mixture or of a given element in a compound
Mixture: a mixture of variable
composition that contains two or more substances
MKS: a metric system of
measurements that uses meters, kilograms, and seconds as basic units
Model:
a
set of assumptions put forth to explain the observed behavior of matter.
The models of chemistry usually involve assumptions about the behavior of
individual atoms or molecules
Molality: the numbers of moles of
solute per kilogram of solvent in a solution
Molarity: mole
of solute per volume of solution in liters
Mole:
the number equal to the
number of carbon atoms in exactly 12 grams of pure 12C:
Avogadro’s number
Molecular
formula: the exact formula of a
molecule, giving the types of atoms and number of each type
Molecular
mass:
the mass in grams of one
mole of molecules or formula units of a substance; the same as molar mass
Molecule: a bonded collection of two
or more atoms on the same or different elements
Monatomic
ion: a
charge particle that contains only one atom
Neutron: a particle in the atomic
nucleus with mass virtually equal to the proton’s but with no charge
Normality: the number of equivalents
of a substance dissolved in a liter of solution
Oxidation-reduction
reaction: a
reaction in which one or more electrons are transferred
Physical
property: a characteristic of a
substance that when tested does not alter the identity of the chemical
Precipitation
reaction: a
reaction in which an insoluble substance forms and separates from the solution
Proton: a
positively charge particle in an atomic nucleus
Recrystalization: a method for separating
components of mixture by producing solid crystals from a solution
Significant
figures: the
certain digits of a measurement
Solution: a
homogeneous mixture
Spectral
lines: the
emission spectrum of an element
States
of matter: the three different forms
in which matter can exist; solid, liquid, and gas
Stoichiometric
ratio of moles: the
ratio of the coefficients of two components in a balanced equation
Stoichiometry: the study of quantities of
reactants and products that can be determined from a balanced chemical equation
Subatomic
particle: a
particle that is smaller than a hydrogen atom.
Includes protons, electrons, and neutrons
Substance: a material that has its
own unique set of chemical and physical properties.
Theoretical: computations
that are based on values that were not taken from actual measurements
Volume: the
amount of space an object occupies