Hydrocarbon

containing carbon and hydrogen and other possible elements

Aliphatic

straight chain and branched, saturated and unsaturated hydrocarbons,

Aromatic

hydrocarbons containing benzene and related compounds

Cyclic hydrocarbons

any ring structures

Heterocyclic aromatics

ring structures containing at least one atom that is not carbon

Saturated hydrocarbon

containing the maximum number of hydrogens

Unsaturated hydrocarbon

having double or triple bonds (less than max. hydrogens)

Alkane

saturated HC's straight chained, branched or cyclic.

Alkene

unsaturated HC's (only double bonds) straight chained, branched or cyclic

Alkyne

unsaturated HC's having at least one triple bond.

Functional group

elements within a molecule that are chemically reactive

Alcohol

OH

Ether

R-O-R

Aldehyde

Ketone

Acid

Ester

Nitrile(Cyano)

Amine

Amide

R-C-NH₂

Covalent Bonding Lewis Dot Structures

shared electron pairs

Coordinate covalent bond

a covalent bond having an electron pair coming from one of the two atoms making the bond.

Hybridized Orbitals

modification of electron orbitals to accommodate the spatial orientation of the bonding and non-bonding electron pairs

sp³ hybrid orbitals

hybridization leading to the tetrahedral shape

sp² hybrid orbitals

hybridization leading to a trigonal planar shape

sp hybrid orbitals

hybridization leading to a linear shape

sigma bonds

covalent bonds defined by the bonding pair being located between the nuclei

pi bonds

covalent bonds defined by the bonding pair being located above and below the plane of the nuclei

MO theory

An alternate theory to valence bond theory. The molecular orbital is considered as atomic orbitals applied to the bonds between two atoms.

Lewis Acid (electrophile)

electron pair acceptor

Lewis Base (nucleophile)

electron pair donor