Organic Chemistry Nomenclature

cycloalkanes

cycloalkanes

- alkanes forming a ring  \n - use the "cyclo "prefix to specify

Properties of Alkanes

- unreactive  \n - boiling/melting point increases with size  \n - intermolecular forces are weak

Crackling

- reaction for alkane \n - large alkane + H2 >(heat)> smaller alkane

Refroming

small alkane >(heat)> large alkane + H2

Halogenation

- replacing H with a halogen

Isomers

different molecules wiht the same moolecular formula

Structural Isomers

- different pattern of atoms attachment

Alkenes

- C=C double bonds  \n - aliphatic and unsaturated  \n - more reactive than alkanes

Alkynes

- known as acetylenes  \n - aliphatic, unsaturated  \n - CC triple bond  \n - more reactive than alkenes  \n - ending -yne

Geometric Isomerism

- cis: same side  \n - trans: opposite side

Alcohol

• OH ending

• ol ending

3 types of Alcohols

• primary

• secondary

• tertiary

Polyalcohols

• alcohols containing one or more hydroxyl groups

Properties of Alcohols

• higher boiling points than parent alkanes

• more soluble than their parent alkanes

• properties are due to the presence of H-bonding

Hydration Reaction (Alcohol)

• alkene + water > alcohol

Combustion of Alcohols

• alcohol + oxygen > water + CO2

Ethers

• C-O-C

• ending -oxy, -ane

Properties of Ethers

• do not for, hydrogen bonds

• more polar than hydrocarbons of the dipole

Condensation Reactions

• reaction of 2 alcohols and the elimination of a water molecule

Hydrogenation

• adding H2

• converts unsaturated molecule to saturated

• alkene/alkyne +H2 > alkane

Halogenation

• adding halogens (F,Cl, Br, I)

Hydrohalogenation

• adding HX

• when adding a polar reagent to double or triple bond the positive part attaches to the carbon with the most H’s

Hydration Reaction

• adding H2O

• converts hydrocarbon into an alcohol

Markovnikov’s rule

• in addition reaction HX to an alkene or alkyne.

• The hydrogen atom of HX becomes bonded to the carbon atom that had the greatest number of hydrogen atoms in the starting alkene or alkyne

Reactions of Aromatic Hydrocarbons

• undergo substitution reactions

• ex. benzene + Br2 >(catalyst)> benzen bromide

Properties of Organic Halides

• bonds between C and halogens are more polar

• more soluble in polar solvent than and have higher boiling points

• More halogenated = more polar

Aldehydes

• C = O

• alkyl group bonded to a carbonyl group with a hydrogen atom

• -al ending

Ketones

• two alcohol groups attached to a central carbonyl group

• -one ending

Properties of Aldehydes and Ketones

• low boiling points

• less soluble than alcohols

• aldehydes and ketones can mix with both polar and non polar substances

Oxidation reaction

• loss of electrons

• loss of hydrogens

• gain of oxygens

Reduction Reaction

• gain of electrons

• gain of hydrogens

• loss of oxygens

Preparing an Aldehyde

• Primary Alcohol + Oxidizing agent > aldehyde + water

Preparing a Ketone

• secondary alcohol + oxidizing agent > Ketone + Water

Carboxylic Acids

• (R-COOH)

• -oic acid ending

Properties of Carboxylic acids

• highly polar molecules

• high boiling points than alkanes

• small = soluble, large = insoluble

• conduct electricity

Preparing Carboxylic acid

1. alcohol + (O) > Aldehyde + H2O

2. aldehyde + (O) > Carboxylic acid

Esters

• (R-COO-R)

• formed when carboxylic reacts with an alcohol

• -oate ending

Properties of Esters

• carbonyl group makes esters more polar, but less polar thean carboxylic acids (lack -OH group, therefore no H-bonding)

• less soluble in water

• low melting and boiling point

• small esters = soluable at (ST), large esters = insoluable

Esterification

• carboxylic acid + alcohol > ester + water

Reaction of Esters

• Hydrolysis produces an acid and an alcohol

• ester + base > carboxylic acid + alcohol

Amines

• (R-NH2)

• amino is put in front of the name of the parent chain

  • ex. aminomethane

Properties of AMines

• primary & Secondary are very polar due to N-H

• high boiling & melting points than similar sized ethers

• smaller amines are soluble in water

Preparing amines

• primary amines;

  • ammonia + alkyl halide > amine + HX

• secondary amines

  • primary amine + alkyl halide > secondary amine + HX

• Tertiary amine

  • secondary amine + alkyl halide > tertiary

  • amine + HX

fractional distillation

• amines can be isolated based on boiling points or specific synthesis methods

Amides

• (R=O-C-N-R)

• -amide ending

Preparing amides

• carboxyclic acids + (1st & 2nd) amine > amide

Properties of amides

• polar carbonyl group with one -NH group can form strong hydrogen bonds

• high boiling points than their corresponding hydrocarbon derivatives

• weak bases that are insoluble