Atomic & Molecular Structure

Get essential facts about atoms and the basics of atomic theory, work problems to test your skills, then take a quiz to make sure you understand the concepts.

Do you understand the basic concepts of atomic theory? Do you have your protons, electrons, and neutrons all sorted out? Here's a ten question multiple choice quiz to test your knowledge.

This ten question multiple choice quiz tests your comprehension of the electric nature of atoms, components of atomic structure, oxidation numbers, valence, quantum numbers, electron configuration, and Lewis dot structures.

Test your understanding of atomic structure and the periodic table with this 10-question multiple choice quiz. Use the atomic structure and periodic table quiz to help yourself study for the AP chemistry exam or a first year college chemistry test.

Are you confused about atoms, elements, protons, neutrons, electrons, isotopes, and ions? Here's a basic look at the model of the atom. It's a great overview for kids or anyone looking to grasp the essentials of atomic theory.

Stable atoms have as many electrons as they do protons. How do these electrons orient themselves around the nucleus? They fill their electron orbitals by the aufbau principle.

The Bohr Model has an atom consisting of a small, positively-charged nucleus orbited by negatively-charged electrons. Here's a closer look at the Bohr Model, which is sometimes called the Rutherford-Bohr Model.

This ten question multiple-choice quiz will test your understanding of the types of chemical bonds, how electrons are transferred between elements in a compound, and how compounds form.

Chemistry is mostly the study of electron interactions between atoms and molecules. Understanding the behavior of the electrons in an atom is an important part of understanding chemical reactions. Electron orbitals depended on three properties: the amount of energy, angular momentum and magnetic moment of the individual electron.

Get the definition for a chemical element.

This table is a compilation of the electron configurations of the elements up through number 104. Tips for writing out stable configurations and for shorthand notation are included.

Molecular geometry is the three-dimensional arrangement of atoms within a molecule. Here's an introduction to molecular geometry with instructions for how to predict configuration and a table of VSEPR geometries.

Learn about Lewis structures, also called electron dot structures and get step-by-step help drawing them.

Learn about molecules, moles, and Avogadro's number.

Monomers are the building blocks of more complex molecules, called polymers. Polymers consist of repeating molecular units which usually are joined by covalent bonds. Here is a closer look at the chemistry of monomers and polymers.

Learn to distinguish between ionic and covalent bonds, and determine whether a bond will be polar or nonpolar.

Learn about the different types of chemical bonds and the forces that affect the way electrons are shared.

If you're given the nuclear symbol for an element, can you identify how many protons and neutrons it has? If you see an ion symbol, do you know how many electrons are present? Here's your chance to test yourself.

The p orbital is a volume of space where an electron is most likely to be found. Here's what it looks like.

Take a look at the probability distrubution of the s orbital, a volume of space describing the likely location of an electron.

These are the molecular geometry configurations predicted using VSEPR theory or Valence Shell Electron Pair Repulsion theory.

Illustrating hydrogen atoms and some small molecules. FromW. R. Salzman, University of Arizona.

Introductory concepts to advanced topics. From CHEMystery.

Included is the description of filling subshells with electrons.

A look at protons, neutrons, and electrons. From Anthony Carpi, John Jay College, CUNY.

Includes thermodynamics, quantum mechanics, and structure of the nucleus. From Carl R. Nave, Georgia State University.

Nuclear structure, sources and detection of radioactivity, and clinical and diagnostic uses. From Richard D. Piccard, Ohio University.

Structures of protein molecules. From Robert M. Hanson, St. Olaf College.

Moveable molecules using RasMol plug-in. From W. R. Salzman,University of Arizona.

Sub-atomic particles, forces, and types of nuclear reactions. From Michael I. Sobel, Brooklyn College, City University of New York.

Emphasis on ion formation, ionic bonds, and ionic compounds. From Walt Volland, Bellevue Community College.

Includes definitions of coordination chemistry and the 18-electron rule. From Interactive Learning Paradigms.

Required reading for understanding the Standard Model.

Lewis electronic structure diagrams. From Liina Ladon, Towson University.

Modeling atomic structures. From the MathMol Hypermedia Textbook.

Fundamental subatomic particles of nature. From Kelley L. Ross.

Using quantum mechanics to predict chemical structure. From Richard F. W. Bader, McMaster University, Hamilton, Ontario.

Atoms are fundamental units of matter that cannot be broken down using any chemical means. Here are some examples of atoms.