Lewis Structures Guided Notes

These flashcards cover the key vocabulary related to Lewis Structures, covalent bonding, and molecular properties.

Single bond

A covalent bond formed by sharing one electron pair, represented by a single line: H—H.

Double bond

A covalent bond formed by sharing two electron pairs, represented by a double line: O═O.

Triple bond

A covalent bond formed by sharing three electron pairs, represented by a triple line: N≡N.

Ionic formula

Gives the ratio of ions in an ionic compound, which is made of ions.

Molecular formula

Gives the exact number of atoms in one molecule.

Octet rule

Atoms tend to form bonds until they are surrounded by eight valence electrons, achieving a stable electron configuration.

Covalent bond

A chemical bond that involves the sharing of electron pairs between atoms.

Lewis structure

A diagram that shows the arrangement of valence electrons for a molecule.

Polyatomic ion

A covalent molecule that has an overall charge due to the loss or gain of electrons.

Forman charge

A measure of the number of electrons an atom has in a structure compared to the number it would have in an isolated atom.

Properties of molecules

Molecules are made of covalent bonds and generally have lower boiling and melting points than ionic compounds due to weaker interactions.