Lecture 8_9-18-25 Ionic and Covalent Bonds File

Flashcards covering key vocabulary related to chemical bonding, ionic and covalent compounds, and Lewis structures from the lecture notes.

Covalent bonds

When atoms of similar electronegativity (generally two nonmetals) share electrons.

Nonpolar covalent bond

A type of covalent bond where atoms of similar electronegativity (generally two like nonmetals, or carbon and hydrogen) share electrons equally, resulting in an electronegativity difference of approximately 0.

Ionic bonds

Chemical bonds formed when a transfer of electrons occurs due to atoms with a very large difference in electronegativity, often resulting in electrostatic attraction between a cation and an anion.

Cation

An ion with a positive charge, typically formed when an atom loses electrons.

Anion

An ion with a negative charge, typically formed when an atom gains electrons.

Ionization energy

The energy input required to remove an electron from an atom.

Electronegativity

The tendency of an atom to attract a bonding pair of electrons.

3D lattice network

The extended three-dimensional structure formed by oppositely charged ions packing around one another in solid binary ionic compounds.

Polyatomic ion

An ion composed of more than one atom (usually nonmetals) covalently bound together.

Oxoanions

Polyatomic anions that contain one or more oxygen atoms and one central atom of another element.

Polar covalent bond

A type of covalent bond where electrons are shared unequally between two different nonmetal atoms due to a small difference in electronegativity.

Bond dipole

An unequal sharing of electrons within a covalent bond, indicated by a dipole arrow and/or partial charges (δ+ and δ-).

Naming Binary Ionic Compounds

A system where the name of the cation is followed by the nonmetal anion with an "-ide" ending, with Roman numerals optionally indicating the charge of certain metal cations.

Naming Binary Covalent Compounds

A system that uses Greek prefixes for both elements, with the less electronegative element named first (without "mono" if it's the first element) and the more electronegative element ending with "-ide".

Lewis Symbols

Representations showing an atom's valence electrons spread out in four regions, remaining unpaired until each region has at least one electron, used to represent bonding atoms.

Electron pair

Two electrons occupying the same orbital in an atom or molecule, which can be a bonding or a lone pair.

Bonding pair

A pair of electrons shared between atoms, creating a chemical bond.

Lone pair

A pair of electrons on an atom that is not involved in a bond.

Unpaired electron

An electron that occupies an orbital of an atom singly, rather than as part of an electron pair.

Octet Rule

A principle stating that nonmetals tend to achieve stable valence shells of eight electrons by sharing electrons.

Duet Rule

A principle stating that certain atoms, like hydrogen, achieve stability with two valence electrons.

Bond order

The number of chemical bonds between a pair of atoms.

Single Bond

A chemical bond with a bond order of 1, involving one shared electron pair.

Double Bond

A chemical bond with a bond order of 2, involving two shared electron pairs.

Triple Bond

A chemical bond with a bond order of 3, involving three shared electron pairs.

Bond Energy

The energy input required to break a chemical bond and fully separate the two bound atoms.

Bond length

The distance between the nuclei of two atoms engaged in a chemical bond.