CHM 102 WEEK 2: CLASSIFICATION OF ORGANIC COMPOUNDS

A comprehensive vocabulary review of the classification of organic compounds, functional groups, carbon atom types, and covalent bonding (sigma and pi).

Aliphatic Compounds (AFC)

Organic compounds that have no aromatic character and are either acyclic or cyclic, and can be saturated or unsaturated.

Acyclic Aliphatic Hydrocarbons

Hydrocarbons without a ring structure where carbon atoms are arranged in straight or branched chains, categorized as 'ane', 'ene', or 'yne'.

Cyclic Aliphatic Hydrocarbons

Compounds where the end carbon atoms of acyclic carbon chains join together to form a ring structure.

Aromatic Compounds

Cyclic organic compounds that possess at least one benzene ring in their structure and behave like benzene in their properties.

Saturated Hydrocarbons

Compounds where carbon atoms have the highest number of hydrogen atoms possible, featuring only single bonds.

Unsaturated Hydrocarbons

Hydrocarbons that contain double ('ene') or triple ('yne') bonds between carbon atoms.

Cyclic Organic Compounds

Molecules containing one or more closed rings of atoms, typically involving $C$, $N$, $O$, or $S$, with a minimum of three atoms in the ring.

Aliphatic Non-Hydrocarbons

Derivatives of aliphatic compounds including functional groups such as alkanols, aldehydes, ketones, and carboxylic acids.

Straight Chain Alkanes (n-alkanes)

Alkanes such as methane ($CH_4$), ethane ($C_2H_6$), propane ($C_3H_8$), and butane ($C_4H_{10}$) that form a continuous chain.

Branched Chain Alkanes (ISO-alkanes)

Alkanes like methylpropane ($C_4H_{10}$) or 2,2,4-trimethylpentane ($(CH_3)_3CCH_2CH(CH_3)_2$) where the carbon atoms form branches.

Alicyclic Compounds

A class of non-aromatic, cyclic organic compounds that combine aliphatic and cyclic characteristics and can be saturated or unsaturated.

Arenes

Aromatic hydrocarbons and their derivatives, such as benzene, xylene, styrene, toluene, and phenol.

Functional Groups

Specific atoms or bonds within molecules that determine the characteristic chemical reactions and properties of a given organic compound.

Alkanols

Oxygen-containing organic compounds with the functional group $-OH$ (hydroxyl), represented by the general formula $R-OH$.

Ether

Organic compounds containing an oxygen atom connected to two alkyl or aryl groups, represented as $R-O-R^1$ (alkoxyalkane).

Aldehydes

Compounds containing a terminal carbonyl group, represented as $R-CHO$.

Ketones

Compounds containing an internal carbonyl group, represented as $R-CO-R^1$.

Carboxylic Acid

Organic compounds containing the functional group $-COOH$, represented as $R-COOH$.

Esters

Oxygen-containing compounds represented by the formula $R-COO-R^1$.

Amine

Nitrogen-containing group represented as $R-NH_2$, $R_2NH$, or $R_3N$.

Amide

Nitrogen-containing group represented by $-CONH_2$, $-CONHR$, or $-CONR_2$.

Nitrile

Nitrogen-containing group with the structure $R-C \biguplus N$.

Thiols

Sulphur-containing functional group with the structure $R-SH$.

Sulphides (thioether)

Sulphur-containing group with the structure $R-S-R^1$.

Epoxide

A cyclic ether belonging to the 'other groups' classification.

Homologous Series (H.S)

A series of organic compounds with the same general formula, similar chemical and physical properties, and a constant functional group.

Primary ($1^o$) Carbon

A carbon atom attached to only one other carbon atom, typically found at the end of a chain (terminal carbon).

Secondary ($2^o$) Carbon

A carbon atom that is bonded to exactly two other carbon atoms.

Tertiary ($3^o$) Carbon

A carbon atom that is bonded to three other carbon atoms.

Quaternary ($4^o$) Carbon

A carbon atom bonded to four other carbon atoms; it cannot bear a functional group.

Sigma Bonds ($\sigma$)

The first and strongest covalent bonds formed by head-on orbital overlap between any two atoms.

Pi Bonds ($\pi$)

Weaker secondary bonds formed by side-to-side p-orbital overlap, appearing as extra bonds in double or triple bonds.

Pi Electrons ($\pi$-electrons)

The electrons involved in the side-by-side p-orbital overlap; a simple $\pi$-bond contains $2$ electrons, while a triple bond contains $4$ electrons.