Atomic Structure and Chemical Bonds

These flashcards cover key concepts related to atomic structure and chemical bonding, including definitions of important terms and rules that govern chemical interactions.

Hybridization

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

Lewis Structure

A diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons that may exist.

Bond Angle

The angle formed between three atoms across at least two bonds.

Octet Rule

A rule that states that atoms tend to bond in such a way that they each achieve a full outer shell of eight electrons.

Electron Configuration

The distribution of electrons in an atom or ion across different orbitals and sub-levels.

Isoelectronic Species

Atoms or ions that have the same number of electrons.

Valence Electrons

Electrons in the outermost shell of an atom that are involved in forming bonds.

Ionic Bond

A chemical bond formed between two ions with opposite charges.

Covalent Bond

A chemical bond formed when two atoms share one or more pairs of electrons.

Hydrogen Bond

A weak bond between a hydrogen atom and an electronegative atom.

Polar Molecule

A molecule with a net dipole moment due to the presence of polar bonds.

Nonpolar Molecule

A molecule that has no distinct positive or negative poles and whose electrons are symmetrically distributed.

Resonance Structures

Different possible configurations of the same molecule that differ in the distribution of electrons.

Nodal Surface

A region in an atom where there is a 0 probability of finding an electron.

Bond Strength

A measure of the energy required to break a bond between two atoms.

Octet Expansion

The phenomenon where elements can accommodate more than 8 electrons in their valence shell.

Electronegativity

The tendency of an atom to attract electrons to itself.