Chemical Bonding and Lewis Structures Review

A set of vocabulary flashcards covering chemical bond types, electronegativity trends, octet rules, and Lewis structure guidelines based on the lecture transcript.

Ionic bond

A chemical bond involving complete electron transfer from a metal to a nonmetal.

Coulomb's law

A formula ($F \approx \frac{q_1 q_2}{r^2}$) showing that electrostatic attraction force is directly proportional to the product of charges and inversely proportional to the square distance between charge centers.

Covalent bond

A chemical bond characterized by equal electron sharing between nonmetal atoms.

Polar covalent bond

A bond involving partial electron transfer or unequal electron sharing between two different nonmetals.

Lowercase delta

A Greek letter symbol used to denote a small, partial charge in a polar covalent bond.

Metallic bond

A bonding arrangement in metals where all valence electrons are shared by all metal atoms, allowing nuclei to sit in a sea of moving electrons.

Electronegativity

The ability of an atom in a molecule or compound to attract bonding electrons to itself.

Electron affinity

The addition of an electron to an atom in a gas state.

Ionization energy

The process opposite to electron affinity, which involves removing electrons from an atom.

Octet rule

A rule requiring eight valence electrons around an atom to achieve stability.

Duet rule

A rule specifying that hydrogen requires only two valence electrons.

Period 2 elements

Elements including carbon, nitrogen, oxygen, and fluorine that never violate the octet rule.

Amphoteric

Describing an element or substance that has both metallic and nonmetallic properties, allowing it to give and gain electrons.

Resonance

A situation where more than one correct Lewis structure exists for the same molecule.