Chemistry Lecture Notes Review

A collection of vocabulary terms and definitions based on the provided lecture notes in chemistry.

Matter

The physical material of the universe, anything that has mass and occupies space.

Atom

The tiny building blocks that compose all matter.

Molecule

A group of atoms bonded together.

Compound

A substance composed of two or more different elements combined in specific proportions.

Mixture

A combination of two or more pure substances in which each retains its own chemical properties.

Solid

A physical state of matter with a definite shape and volume.

Liquid

A physical state of matter with a definite volume but no definite shape.

Gas

A physical state of matter with no definite shape or volume.

Filtration

A separation technique based on differences in solubility.

Physical Property

A characteristic of matter that can be observed without altering its composition.

Chemical Property

The ability of a substance to undergo a chemical change.

Significant Figures

Digits in a measurement that carry meaningful information about its precision.

Molar Mass

The mass of one mole of a substance, usually expressed in grams per mole.

Avogadro's Number

The number of atoms, ions, or molecules in one mole of a substance, approximately $6.022 imes 10^{23}$.

Stoichiometry

The calculation of reactants and products in chemical reactions.

Electrolyte

A substance that dissolves in water to give a conducting solution.

Precipitate

An insoluble solid that separates from a solution during a chemical reaction.

Acid

A substance that donates protons (H+) in a reaction.

Base

A substance that accepts protons (H+) in a reaction.

Redox Reaction

A reaction involving the transfer of electrons between two species.

Oxidation

The loss of electrons or an increase in oxidation number.

Reduction

The gain of electrons or a decrease in oxidation number.

Net Ionic Equation

An equation that shows only the species that actually change during the reaction.

Solution

A homogeneous mixture of two or more substances.

Titration

A laboratory method used to determine the concentration of an unknown solution by adding a solution of known concentration.

Dilution

The process of reducing the concentration of a solute in a solution.

Density

The mass per unit volume of a substance, typically expressed in g/cm³ or kg/m³.

Isotope

Atoms of the same element that have different numbers of neutrons.

Homogeneous Mixture

A mixture that is uniform in composition and appearance.

Heterogeneous Mixture

A mixture that consists of two or more identifiable regions.

Chemical Reaction

A process in which substances interact to form new substances.

Molarity (M)

The concentration of a solution expressed as moles of solute per liter of solution.

Exponential Notation

A way to express very large or very small numbers using powers of ten.

Absolute Uncertainty

The uncertainty associated with the measurement, expressed in the same units as the measured quantity.

Percentage Uncertainty

The uncertainty of a measurement relative to the measurement itself, expressed as a percentage.

H

Hydrogen

He

Helium

Li

Lithium

Be

Beryllium

B

Boron

C

Carbon

N

Nitrogen

O

Oxygen

F

Fluorine

Ne

Neon

Na

Sodium

Mg

Magnesium

Al

Aluminum

Si

Silicon

P

Phosphorus

S

Sulfur

Cl

Chlorine

Ar

Argon

K

Potassium

Ca

Calcium