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