Chapter 13: Bonding: General Concepts Flashcards

Vocabulary flashcards covering chemical bonding concepts, Lewis structures, formal charges, resonance, and octet rule exceptions from Chapter 13.

Lewis Bond Theory

A theory representing chemical bonding where valence electrons play a fundamental role, electron transfer forms ionic bonds, electron sharing forms covalent bonds, and atoms achieve an octet.

Octet

A noble gas electron configuration consisting of eight valence electrons achieved by transferring or sharing valence electrons.

Lewis Symbol

A chemical representation consisting of an element's chemical symbol (representing the nucleus and core electrons) combined with dots representing valence electrons in the shell of highest $n$.

Ionic Bonding

Chemical bonding that results from the transfer of electrons from one atom to another.

Covalent Bonding

Chemical bonding that results from the sharing of one or more pairs of electrons between atoms.

Single Covalent Bond

A covalent bond formed by the sharing of a single pair of electrons between two bonded atoms.

Bond Pair of Electrons

A pair of electrons that participate in chemical bonding.

Lone Pair of Electrons

A pair of electrons that do not participate in chemical bonding.

Coordinate Covalent Bond

A covalent bond in which the two shared electrons derive from the same atom.

Double Covalent Bond

A covalent bond in which two bonded atoms share two pairs of electrons.

Triple Covalent Bond

A covalent bond in which two bonded atoms share three pairs of electrons.

Electronegativity (EN)

An atom's ability to compete for electrons with other atoms to which it is bonded, increasing from bottom to top in a group and left to right in a period.

Polar Covalent Bond

A covalent bond in which electrons are not shared equally between two atoms due to an electronegativity difference.

Skeletal Structure

The representation showing the connectivity of atoms within a species by identifying central and terminal atoms.

Central Atoms

Atoms in a molecular skeletal structure connected to more than one atom, generally having the lowest electronegativity.

Terminal Atoms

Atoms in a molecular skeletal structure connected to only one atom, such as hydrogen atoms.

Formal Charge

The electric charge an atom in a molecule or polyatomic ion has, assuming that all bond-pair electrons are shared equally between atoms.

Resonance Structures

The contributing Lewis structures that average together to represent the actual electronic structure and molecular geometry when more than one plausible Lewis structure exists.

Odd-Electron Species

Chemical species having unpaired electrons, which causes them to be paramagnetic, unstable, and highly reactive.

Incomplete Octet

A state in which an atom has less than eight electrons in its valence shell, found mostly in boron ($B$) and aluminum ($Al$).

Expanded Octets

A state in which central atoms in period 3 or higher have more than 8 valence electrons, typically 10, 12, or 14.