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Molecule
A group of two or more atoms bonded together, representing the smallest fundamental unit of a chemical compound.
Diatomic Molecule
A molecule composed of two atoms, which can be of the same or different elements.
Covalent Bond
A type of chemical bond where two atoms share one or more pairs of electrons.
Binary Covalent Compound
A chemical compound composed of two different nonmetals, where atoms are bonded together by covalent bonds.
Lewis Structure
A diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons that may exist.
Duet Rule
A guideline stating that hydrogen and helium atoms are stable when they have two electrons in their outer shell.
Octet Rule
The principle that atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration.
Superoctet
An extension of the octet rule that allows certain elements to have more than eight electrons in their valence shell, typically seen in elements from the third period and beyond.
Suboctet
A term describing atoms that are stable with fewer than eight electrons in their valence shell, such as boron and aluminum.
Structural Formula
A graphical representation of a molecule that shows how atoms are arranged and bonded, indicating the connections between atoms.
VSEPR Model
A theory used to predict the geometry of molecular structures based on the repulsion between electron pairs around a central atom.
Polarity
The distribution of electrical charge over the atoms in a molecule, resulting in a molecule having a positive end and a negative end.
Polar Covalent Bond
A type of chemical bond where electrons are shared unequally between two atoms, resulting in partial positive and negative charges.
Nonpolar Covalent Bond
A type of chemical bond where electrons are shared equally between two atoms, resulting in no overall charge difference.
Molecular Polarity
The property of a molecule that describes the uneven distribution of electron density, leading to distinct positive and negative ends.
Electronegativity
The ability of an atom in a molecule to attract shared electrons towards itself, influencing the polarity of the bond.
Lewis Dot Structure (LDS)
A diagram that represents the valence electrons of atoms within a molecule, showing how they are arranged and bonded.
Lone Pairs
pairs of valence electrons that are not shared with another atom.
Mono
a prefix indicating one atom or group.
Di
a prefix indicating two atoms or groups.
Tri
a prefix indicating three atoms or groups.
Tetra
a prefix indicating four atoms or groups.
Penta
a prefix indicating five atoms or groups.
Hexa
a prefix indicating six atoms or groups.
Hepta
a prefix indicating seven atoms or groups.
Octa
a prefix indicating eight atoms or groups.
Nona
a prefix indicating nine atoms or groups.
Deca
a prefix indicating ten atoms or groups.
Single Bond
a type of chemical bond where two atoms share one pair of electrons.
Double Bond
a type of covalent bond where two pairs of electrons are shared between two atoms.
Triple Bond
a type of chemical bond where two atoms share three pairs of electrons.
