General Chemistry I - Molecular Structure and Bonding

A set of vocabulary flashcards covering key concepts from General Chemistry I, focusing on molecular structure, bonding, and related principles.

Isomer

Different molecules with the same molecular formula but different structural arrangements.

Octet Rule

Atoms tend to bond in such a way that they have eight electrons in their valence shell, achieving a stable electron configuration.

Covalent Bond

A bond formed when two nonmetals share a pair of electrons.

Lewis Structure

A diagram that represents the valence electrons of atoms within a molecule, showing how they are shared or transferred.

Sigma Bond (σ bond)

The first bond formed between two atoms, resulting from the direct overlap of atomic orbitals.

Pi Bond (π bond)

A bond formed by the sideways overlap of p orbitals, found in double and triple bonds.

Formal Charge (FC)

A calculated charge on an atom in a molecule that helps determine the most stable Lewis Structure, calculated as FC = Valence - Assigned.

Resonance Structures

Different Lewis structures for the same molecule that show the same placement of atoms but different placements of electrons.

Hybridization

The mixing of atomic orbitals to create new hybrid orbitals for bonding.

VSEPR Theory

Valence Shell Electron Pair Repulsion Theory; used to predict the geometry of individual molecules based on the repulsion between the electron pairs.

Electronegativity

The tendency of an atom to attract electrons in a bond, leading to polar or nonpolar characteristics.

Polar Molecule

A molecule with a net dipole moment due to the presence of polar bonds, resulting in an uneven distribution of charge.

Nonpolar Molecule

A molecule that has a symmetrical distribution of electrons, resulting in no net dipole moment.

Lone Pairs

Pairs of valence electrons that are not shared or involved in bonding.

Covalent Compound

A chemical compound formed by the sharing of electrons between nonmetals.