Chemistry Full Review

MATTER

Anything that has mass and takes up space.

PHYSICAL CHANGE

A change that does not produce a new substance.

CHEMICAL CHANGE

A change that produces one or more new substances.

EVIDENCE OF CHEMICAL CHANGE

Color change, gas production, precipitate formation, heat, or light.

SOLID

Has a definite shape and definite volume.

LIQUID

Has a definite volume but takes the shape of its container.

GAS

Has no definite shape or volume.

MELTING

Solid changes to liquid.

FREEZING

Liquid changes to solid.

VAPORIZATION

Liquid changes to gas.

EVAPORATION

Liquid changes to gas at the surface.

BOILING

Rapid vaporization throughout a liquid.

CONDENSATION

Gas changes to liquid.

SUBLIMATION

Solid changes directly to gas.

DEPOSITION

Gas changes directly to solid.

ENDOTHERMIC PHASE CHANGES

Melting, vaporization, and sublimation.

EXOTHERMIC PHASE CHANGES

Freezing, condensation, and deposition.

SLANTED HEATING CURVE LINES

Temperature and kinetic energy change.

FLAT HEATING CURVE LINES

Phase changes occur and potential energy changes.

JOHN DALTON

Proposed the first modern atomic theory.

J.J. THOMSON

Discovered the electron using the cathode ray tube.

ERNEST RUTHERFORD

Discovered the nucleus using the gold foil experiment.

JAMES CHADWICK

Discovered the neutron.

NIELS BOHR

Proposed electron energy levels.

SCHRODINGER

Developed the electron cloud model.

MODERN ATOMIC MODEL

Electron cloud model.

PROTON

Positively charged particle found in the nucleus.

NEUTRON

Neutral particle found in the nucleus.

ELECTRON

Negatively charged particle found outside the nucleus.

PROTON CHARGE

+1.

NEUTRON CHARGE

0.

ELECTRON CHARGE

-1.

ATOMIC NUMBER

Number of protons.

MASS NUMBER

Protons plus neutrons.

NEUTRONS

Mass number minus atomic number.

ISOTOPES

Atoms with the same number of protons but different numbers of neutrons.

GROUND STATE

Lowest energy arrangement of electrons.

EXCITED STATE

Electrons have absorbed energy.

BRIGHT-LINE SPECTRUM

Light emitted when electrons lose energy.

VALENCE ELECTRONS

Electrons in the outermost energy level.

GROUP 1

Alkali metals.

GROUP 2

Alkaline earth metals.

GROUP 17

Halogens.

GROUP 18

Noble gases.

ATOMIC RADIUS TREND

Increases down a group and decreases across a period.

ELECTRONEGATIVITY TREND

Increases up and to the right.

HIGHEST ELECTRONEGATIVITY

Fluorine.

IONIZATION ENERGY

Energy required to remove an electron.

METALLIC CHARACTER

Increases down and to the left.

ELECTRON CONFIGURATION

Arrangement of electrons.

FIRST ENERGY LEVEL

Holds 2 electrons.

SECOND ENERGY LEVEL

Holds 8 electrons.

THIRD ENERGY LEVEL

Holds 8 electrons on the Regents.

LEWIS DOT STRUCTURE

Shows valence electrons.

OCTET RULE

Atoms seek 8 valence electrons.

IONIC BOND

Transfer of electrons.

COVALENT BOND

Sharing of electrons.

POLAR BOND

Unequal sharing of electrons.

NONPOLAR BOND

Equal sharing of electrons.

INTERMOLECULAR FORCES

Forces between molecules.

LINEAR SHAPE

CO2.

BENT SHAPE

H2O.

TETRAHEDRAL SHAPE

CH4.

POLAR MOLECULE

Uneven charge distribution.

NONPOLAR MOLECULE

Even charge distribution.

ONE MOLE

6\,02 × 10^{23} particles.

AVOGADRO'S NUMBER

6\,02 × 10^{23}.

STP

273 K and 101.3 kPa.

ONE MOLE OF GAS AT STP

22\,4 liters.

MOLES FORMULA

Moles = mass ÷ GFM.

MASS FORMULA

Mass = moles × GFM.

EMPIRICAL FORMULA

Simplest whole-number ratio.

MOLECULAR FORMULA

Actual number of atoms.

PERCENT COMPOSITION

Percent by mass of each element.

THEORETICAL YIELD

Maximum amount of product possible.

ACTUAL YIELD

Amount actually produced.

PERCENT YIELD

Actual yield ÷ theoretical yield × 100.

BOYLE'S LAW

Pressure and volume are inversely related.

CHARLES'S LAW

Volume and temperature are directly related.

COMBINED GAS LAW

P1V1/T1 = P2V2/T2.

KELVIN CONVERSION

Celsius + 273.

COLLISION THEORY

Particles must collide properly and with enough energy.

ACTIVATION ENERGY

Minimum energy needed for a reaction.

CATALYST

Lowers activation energy.

EXOTHERMIC REACTION

Releases heat.

ENDOTHERMIC REACTION

Absorbs heat.

SYNTHESIS REACTION

A + B → AB.

DECOMPOSITION REACTION

AB → A + B.

SINGLE REPLACEMENT

A + BC → AC + B.

DOUBLE REPLACEMENT

AB + CD → AD + BC.

COMBUSTION

Hydrocarbon + oxygen → carbon dioxide + water.

NEUTRALIZATION

Acid + base → salt + water.

ADDITION REACTION

Adds atoms across multiple bonds.

SUBSTITUTION REACTION

One atom replaces another.

FERMENTATION

Breakdown of sugars without oxygen.

POLYMERIZATION

Small molecules join to form polymers.

SOLUTE

Substance being dissolved.

SOLVENT

Substance doing the dissolving.

MOLARITY

Moles per liter.

UNSATURATED SOLUTION

Below the solubility curve.