Bonding Concepts
9 concepts · Grades 9-12 · 11 prerequisite connections
This family view narrows the full chemistry map to one connected cluster. Read it from left to right: earlier nodes support later ones, and dense middle sections usually mark the concepts that hold the largest share of future work together.
Use the graph to plan review, then use the full concept list below to open precise pages for definitions, examples, formulas, and related mistake guides. That combination keeps the page useful for both human study flow and crawlable internal linking.
Concept Dependency Graph
Concepts flow left to right, from foundational to advanced. Hover to highlight connections. Click any concept to learn more.
Connected Families
Bonding concepts have 6 connections to other families.
All Bonding Concepts
Chemical Bond
A lasting force of attraction between atoms that holds them together in molecules, compounds, or crystal lattices, formed when atoms share electrons (covalent bond), transfer electrons (ionic bond), or pool electrons in a metallic sea (metallic bond).
Ionic Bond
A bond formed when one atom transfers electrons to another, creating oppositely charged ions that attract.
Covalent Bond
A bond formed when two atoms share one or more pairs of electrons, holding them together.
Octet Rule
A chemical bonding principle stating that atoms tend to gain, lose, or share electrons in order to achieve a stable configuration of 8 electrons in their outermost shell, resembling the electron arrangement of the nearest noble gas.
Lewis Structure
A diagram showing atoms, bonds, and lone pairs of electrons in a molecule, following the octet rule.
Electronegativity
A measure of how strongly an atom attracts the shared electrons in a covalent bond toward itself.
Molecular Geometry
The three-dimensional arrangement of atoms in a molecule, determined by electron pair repulsion.
Polar Covalent Bond
A covalent bond in which electrons are shared unequally, creating partial positive and negative charges.
Molecular Polarity
The overall asymmetric distribution of electric charge in a molecule, arising from the combination of individual bond polarities and the three-dimensional molecular geometry. A molecule is polar if bond dipoles do not cancel, resulting in a net dipole moment.