Chemistry I Honors - Bonding and Molecular Structures

These flashcards cover key concepts related to ionic and covalent compounds, bonding types, and properties crucial for Chemistry I Honors.

Ionic Compound

A compound formed by the transfer of electrons from a metal to a nonmetal, resulting in ionic bonds.

Covalent Compound

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

Bond Length

The average distance between bonded atoms.

Bond Energy

The energy required to break a chemical bond and form neutral isolated atoms.

Octet Rule

The principle that atoms tend to bond in such a way that they have eight electrons in their valence shell.

Lone Pair

A pair of valence electrons that are not shared with another atom.

Single Bond

A chemical bond formed by the sharing of one pair of electrons.

Double Bond

A chemical bond formed by the sharing of two pairs of electrons.

Triple Bond

A chemical bond formed by the sharing of three pairs of electrons.

Metallic Bonding

A type of bonding found in metals where electrons are shared among a lattice of positively charged ions.

Polyatomic Ion

An ion composed of two or more atoms that are tightly bonded together, behaving as a single unit.

Lewis Structure

A diagram showing the bonding between atoms of a molecule and the lone pairs of electrons.

Prefix Notation

A system used in naming covalent compounds that indicates the number of atoms present using Greek numerical prefixes.

Conductivity of Ionic Compounds

Ionic compounds can conduct electricity when melted or dissolved in water.

Conductivity of Covalent Compounds

Covalent compounds generally do not conduct electricity.

Melting Point of Ionic Compounds

Ionic compounds have very high melting points.

Melting Point of Covalent Compounds

Covalent compounds typically have lower melting and boiling points.