Module 1 MatterAnything that has mass and takes up
space
Scientific notation 1.591 x (10)-20 accuracy
An indication of how close a measurement is to the true value
precisionAn indication of the
scale on the measuring device
that was used
meniscusThe curved surface of a liquid, typically in a glass container
Derived unit
A unit formed by the multiplication and/or
division of other units
slug English unit for mass
massA measure of the
amount of matter in an object
gram
The metric unit of mass
Module 2 work
The force applied to an object times the distance that the
object ravels parallel to that force
energy The ability to do work
The First Law of Thermodynamics
Energy cannot be created or destroyed – it can only change
formhypothesis
An educated guess that attempts to
explain observations
theoryA hypothesis that
has been confirmed by experimental
dataScientific Law
A description of the natural world that
has been confirmed by an enormous amount of data
Joule The metric unit for energy
Celsius
A temperature scale defined so that
water freezes at 0 degrees and boils at
100 degrees
calorie
4.184 Joules 1 food calorie 1,000 chemical calories
Specific heat
The amount of heat necessary to raise
the temperature of 1 gram of a substance by 1 degree Celsius
Module 3 Continuous Theory of Matter
The idea that substances are
composed of long, unbroken blobs of
matter
Discontinuous Theory of Matter
The idea that substances are
composed of tiny, individual particles like grains of sand
The Law of Mass Conservation
Matter cannot be created or destroyed – it can only change
formsquantitative
Expression in terms of quantity or
amount
decompositionThe process by
which a substance is broken down into its constituent elements
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The number of elements element
Any substance that cannot be
decomposed into less massive substances
metalloids
An element intermediate in
properties between typical metals and
non-metals
compounds
Substances that can be decomposed into
elements by chemical means
The Law of Definite Proportions
The proportion of elements in any
compound is always the same
Dimensionless quantity
A quantity with no units
The Law of Multiple Proportions
If 2 elements combine to form
different compounds, the ratio of masses of the 2nd
element that react with a fixed mass of the 1st element will be a simple, whole
ratio
isotopesAtoms with the same
number of protons but different
numbers of neutrons
moleculesMore than one atom bound together to form a compound
Chemical symbol
The abbreviation for an element Chemical formula
A notation that indicates the number
of type of each element in a compound
Ionic compound A compound formed by ions Covalent compound
A compound formed by atoms that share
electronsdistilled
Liquid made pure by heating until it is a
gas and then cooling it as a liquid again
Elements Aluminum Al
Argon Ar Arsenic
As Barium Ba
Bismuth Bi Boron
B Bromine Br
Cadmium Cd Calcium
Ca Carbon C
Chlorine Cl Chromium
Cr Copper Cu
Fluorine F Francium
Fr Cold Au
Helium He Hydrogen
H Iodine I
Iron Fe Krypton
Kr Lead Pb
Lithium Li Magnesium
Mg Mercury Hg
Neon Ne Nickel
Ni Oxygen O
Phosphorus P Platinum
Pt Plutonium Pu
Potassium K Radium
Ra Radon Rn
Silicon Si Silver
Ag Sodium Na
Sulfur S Thallium
Tl Titanium Ti
Tungsten W Xenon
Xe Zinc Zn
Zirconium Zr
Module 4 Pure substanceA substance that contains only 1
element or compound
MixtureA substance that contains different
elements or compounds
Heterogeneous mixture
A mixture with a composition that it different depending on what part of the
sample you are observing
Homogeneous mixture
A mixture with a composition that is always the same no matter what part of the sample you are
observing
Chemical changeA change that affects
the type of molecules or atoms
in a substancePhysical change
A change in which the atoms or
molecules in a substance stay the
same
Phase changeWhen a substance
changes form from a solid to liquid, liquid
to gas, etc.
Kinetic Theory of Matter
Molecules and atoms are in constant motion, and the
higher the temperature the
greater their speed
Homonuclear diatomics
Elements composed of individual
molecules, not individual atoms
Elements that are homonuclear
diatomics
Nitrogen, oxygen, chlorine, fluorine,
bromine, iodine and hydrogen
ReactantsThe substances
found on the left side of a chemical
equation
Module 5 Decomposition reactions
A reaction that changes a compound into its constituent
elements
Formation reaction
A reaction that starts with 2 or more
elements and produces 1 compound
Complete combustion reaction
A reaction in which O2 is added to a
compound containing carbon
and hydrogen, producing CO2 and
H2O
Incomplete combustion
A reaction in which O2 is added to a
compound containing carbon
and hydrogen
Atomic massA number that tells how heavy an atom
is
MoleA group of atoms or
molecules that number 6.02 x 1023
Module 6 Stoichiometry
The process by which the amount of one substance in a chemical reaction is
related to the amount of another
substance in a chemical reaction
Gay-Lussac’s Law
The stoichiometric coefficients in a
chemical equation relate the volumes
of gases in the equation as well as
the number of moles of substances in the
equation
Molecular formula
A chemical formula that provides the
number of each type of atom in a
molecule
Empirical formula
A chemical formula that tells you a simple, whole
number ratio for the atoms in a molecule
Molar massThe mass of one mole in a given
compound
Module 7 ElectronsNegatively charged particle that orbits the nucleus of an
atom
ProtonPositively charged
particle in the nucleus of the atom
Neutron
Neutral particle in the nucleus of an
atomAtomic number
Tells how many protons are in an
atom
Mass numberThe total number of
neutrons and protons in an atom
Isotopic enrichment
The process by which the abundance of one isotope in an element is increased
Rutherford or Planetary model of
the atom
Photons “Particles” of light Particle/Wave Duality Theory
The theory that light sometimes behaves
as a particle and sometimes behaves
as a wave
AmplitudeA measure of the
height of the creasts or the depths of the troughs on a wave
Bohr Model of the Atom
Quantum Mechanical Model
Visible spectrumThe range of light
wavelengths that are visible to the human
eye
Physical constantA measurable
quantity in nature that does not change
Frequency
The number of wave crests (or troughs) that pass a given point each second
Hertz Hz
Electromagnetic spectrum
The total range of wavelengths of light that come from the
sun
Electromagnetic radiation
Another tem for light including all
wavelengths – visible and non-visible
SpectrometerA device that analyzes light
emitted or absorbed by a substance
Ground stateThe lowest possible energy state for a given substance
Electron configuration
A notation that lists the number of electrons that
occupy each orbital in an atom
Module 8 Inert Not chemically reactive
Noble gasesHelium, Neon,
Argon, Krypton, Radon, Xenon
Valence electrons
The electrons that exist farthest from an atom’s nucleus
Octet ruleMost atoms strive to
attain 8 valence electrons
Lewis Structures
A schematic representation of
the valence electrons in an atom
or molecule
Ionization
The process by which an atom turns
into an ion by gaining or losing
electrons
Ionization potential
The amount of energy needed in order to take an
electron away from an atom
Periodic propertyA characteristic of atoms that varies
regularly across the periodic chart
Electronegativity
A measure o how strongly an atom
attracts extra electrons to itself
Atomic radius The average radius of an atom
Double bondA total of 4 electrons
shared between atoms