Covalent Bonding and Molecular Compounds

A neutral group of atoms that are held together by covalent bonds.

A single molecule of a compound is capable of existing on its own.

Atoms can be bonded ionically (charge) or covalently (by sharing electrons)

​"All compounds are molecules but not all molecules are compounds"

Indicates the relative numbers of atoms of each kind in a compound.

Shows the types and numbers of atoms in a single molecule of a molecular compound (a covalent substance).

"Molecular Compound" = "Covalent Compound"

​Only covalently bonded atoms form "MOLECULES"

​All compounds are molecules but not all molecules are compounds.

​Compounds can be covalent OR ionic (we'll talk about ionic compounds next).

​All compounds have a chemical formula, but ONLY COVALENT COMPOUNDS have a MOLECULAR FORMULA.

Atoms have lower potential energy when bonded (more stability

Bond length is the average distance between two bonded atoms.

Bond energy is the amt. of energy required to break a chemical bond.

A "full outer shell" means more stability/lower potential energy.

H and He are exceptions to the octet rule.

The group number can tell you how many valence electrons an atom has.

Groups 1 and 2 have "1" and "2" e^- respectively.

Group 13 has "3",, group 14 has "4", and so on through group 18...

Transition metals can "move" their valence electrons around, so we need to consider what they're bonding with.

You'll be able to figure this out later...

Boron typically achieves 6 valence e^-, and beryllium with 4.

Highly electronegative atoms, like fluorine, oxygen, and chlorine, can have more than 8 valence e-

Each dot represents an electron.

A total of 4 PAIRS of electrons shows an octet

Dots are unpaired electrons

Dashes are a shared pair of electrons

Single bonds = 1 line = 1 PAIR of electrons

Multiple bonds = more than 1 line

"mirror" images of a molecule; when one diagram can't suffice.

shown by a double-headed arrow between the structures.

more simple