Polarity and Formal Charge

This set of flashcards focuses on key vocabulary related to polarity, formal charge, and Lewis structures based on the lecture notes.

Electronegativity

The ability of an atom to attract electrons in a covalent bond.

Formal Charge

The difference between the number of valence electrons of an atom in a neutral free state and the number of electrons assigned in a Lewis structure.

Ionic Bond

When electronegativity is so different that two atoms exchange one or more electrons.

Non-polar Covalent Bond

When electrons are attracted equally to two atoms.

Polar Covalent Bond

When electrons are attracted more strongly by one atom than by the other.

Dipole

The partial charges associated with each end of a polar covalent bond.

Lewis Structure

A diagram that shows the bonding between atoms in a molecule and the lone pairs of electrons.

Valence Electrons

The electrons in the outer shell of an atom that are involved in forming bonds.

Molecular Dipole

The overall polarity of a molecule resulting from the distribution of electron density.

Octet Rule

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