L2: Polarity

Atoms

The basic units of matter that bond to form compounds and attain stability.

Chemical Bond

The force that holds atoms together in a compound.

Ionic Bond

A type of chemical bond involving the transfer of valence electrons from one atom to another.

Covalent Bond

A type of chemical bond where electrons are shared between nonmetal atoms.

Metallic Bond

A type of chemical bond characterized by a sea of delocalized electrons around metal cations.

Element

A substance consisting of only one type of atom.

Compound

A substance formed from two or more different types of atoms bonded together.

Diatomic Elements

Elements that naturally exist as molecules consisting of two atoms.

Metalloids

Elements with properties intermediate between metals and nonmetals, represented by the acronym "Boring Silly Germans Are At The Party."

Intramolecular Force

The forces that hold atoms together within a molecule.

Monoatomic Ion

An ion consisting of a single atom with an unequal number of protons and electrons.

Polyatomic Ion

An ion made up of two or more atoms that can be classified as anion or cation.

Anion

A negatively charged ion.

Cation

A positively charged ion.

Polar Covalent Bond

A bond where electrons are shared unequally between two atoms, resulting in partial charges.

Nonpolar Covalent Bond

A bond where electrons are shared equally between two atoms, resulting in no charges.

Electronegativity

The tendency of an atom to attract electrons toward itself.

Ionic Bond Electronegativity Range

A difference of 1.8 and above indicates an ionic bond.

Polar Bond Electronegativity Range

A difference between 0.41 to 1.79 indicates a polar covalent bond.

Nonpolar Bond Electronegativity Range

A difference between 0 to 0.40 indicates a nonpolar covalent bond.

Lewis Electron Dot Structure (LEDS)

A representation of the valence electrons of an atom using dots around the element's symbol.

Octet Rule

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

Duet Rule

The principle that hydrogen can achieve stability with two valence electrons.

Single Bond

A bond represented by a single line, involving one shared pair of electrons.

Double Bond

A bond represented by two lines, involving two pairs of shared electrons.

Triple Bond

A bond represented by three lines, involving three pairs of shared electrons.