Build your organic chemistry foundation with this essential flashcard deck covering the key concepts, functional groups, and reaction types you need to know. Organic chemistry studies carbon-containing compounds and is fundamental to biology, medicine, materia...
Build your organic chemistry foundation with this essential flashcard deck covering the key concepts, functional groups, and reaction types you need to know. Organic chemistry studies carbon-containing compounds and is fundamental to biology, medicine, materials science, and the pharmaceutical industry.
This deck covers IUPAC nomenclature, hydrocarbons (alkanes, alkenes, alkynes), aromatic compounds, and the major functional groups including alcohols, ethers, aldehydes, ketones, carboxylic acids, esters, amines, and amides — along with their properties and characteristic reactions.
Essential for AP Chemistry, A-Level, and first-year university organic chemistry courses.
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The study of carbon-containing compounds. Carbon is unique — it forms 4 bonds and chains of virtually unlimited length with itself and other elements, enabling millions of compounds.
An atom or group of atoms in an organic molecule that determines its characteristic chemical reactions and properties. The rest of the molecule is usually an inert carbon chain (R group).
Organic compounds containing only carbon and hydrogen. Classified as alkanes (single bonds), alkenes (double bonds), alkynes (triple bonds), and aromatic (benzene ring).
Hydrocarbons with only single C–C bonds — fully saturated. General formula: CₙH₂ₙ₊₂. Examples: methane (CH₄), ethane (C₂H₆), propane (C₃H₈).
Hydrocarbons with at least one C=C double bond — unsaturated. General formula: CₙH₂ₙ. Examples: ethene (C₂H₄), propene (C₃H₆). More reactive than alkanes.
Hydrocarbons with at least one C≡C triple bond. General formula: CₙH₂ₙ₋₂. Examples: ethyne/acetylene (C₂H₂). Very reactive and used in welding torches.
Benzene (C₆H₆) is an aromatic hydrocarbon with a ring of 6 carbons and delocalized π electrons. It is unusually stable due to resonance. Basis of all aromatic compounds.
Contains an –OH (hydroxyl) group bonded to a carbon chain. General formula: R–OH. Examples: methanol (CH₃OH), ethanol (C₂H₅OH). Properties: polar, hydrogen bonding, high boiling point.
Classified by how many carbon atoms are bonded to the carbon bearing the –OH group. Primary (1°): 1 carbon. Secondary (2°): 2 carbons. Tertiary (3°): 3 carbons.
Contains a –CHO group (carbonyl C=O at end of chain). General formula: R–CHO. Examples: formaldehyde (HCHO), ethanal (CH₃CHO). Have a distinctive sharp smell.
Contains a C=O group bonded to two carbon atoms (carbonyl in the middle of chain). General formula: R–CO–R'. Example: propanone/acetone (CH₃COCH₃). Used as a solvent.
Contains a –COOH group. General formula: R–COOH. Examples: methanoic acid (HCOOH), ethanoic acid (CH₃COOH/acetic acid). Weak acids with sharp, sour smells.
Contains a –COO– group. Formed by reaction of carboxylic acid + alcohol (esterification). Example: ethyl ethanoate (CH₃COOC₂H₅). Responsible for fruity smells and flavors.
Contains an –O– group between two carbon chains. General formula: R–O–R'. Example: diethyl ether (C₂H₅OC₂H₅). Used as a solvent and historically as an anesthetic.
Contains a –NH₂ group (or substituted versions –NHR or –NR₂). Amines are basic and have strong, fishy smells. Example: methylamine (CH₃NH₂). Building blocks of amino acids.
Contains a –CONH₂ group (carbonyl + amine). Formed from carboxylic acid + amine. Example: ethanamide (CH₃CONH₂). The peptide bond in proteins is an amide bond.
When two or more compounds have the same molecular formula but different structural arrangements. Structural isomers differ in connectivity. Stereoisomers differ in spatial arrangement.
A type of geometric stereoisomerism in alkenes. Cis: Same groups on same side of double bond. Trans: Same groups on opposite sides. Different physical properties (boiling points, polarity).
A reaction where atoms are added across a double or triple bond, converting it to a single bond. Example: ethene + H₂ → ethane (hydrogenation). Typical of alkenes.
A reaction where one atom or group is replaced by another. Typical of alkanes (e.g., halogenation: CH₄ + Cl₂ → CH₃Cl + HCl in UV light).
A reaction where atoms are removed from adjacent carbons, forming a double bond. Opposite of addition. Example: dehydration of alcohol → alkene + water.
The process of joining many small monomer molecules into a large polymer chain. Addition polymerization: monomers with double bonds join without losing atoms (e.g., polyethylene from ethene).
The systematic naming system for organic compounds. Rules: 1. Find the longest carbon chain. 2. Number from the end closest to a substituent. 3. Name substituents as prefixes. 4. Use suffixes for functional groups (-ol, -al, -one, -oic acid).
