1. Alcohols Suffix = ol hydroxy
1.1. Different classifications based on where the OH is located
1.1.1. Primary alcohol
1.1.1.1. The OH group is attached to a carbon that is all on its own
1.1.2. Secondary alcohol
1.1.2.1. the OH group is attached to a carbon that is attached to 2 other carbons
1.1.3. Tertiary alcohol
1.1.3.1. The OH group is attached to a carbon that is attached to 3 other carbons
1.2. Physical properties
1.2.1. OH group is polar
1.2.2. Solubility
1.2.2.1. small alcohols are soluble due too HYDROGEN BONDNG
1.2.3. Boiling point
1.2.3.1. higher boiling points then hydrocarbons do to the hydrogen bonding
1.2.3.1.1. BP increases as the number of carbons increases
1.2.3.1.2. BP decreases from primary to tertiary alcohols due to top steric hindrance
1.3. Functional group
1.3.1. Hydroxyl group OH
1.4. Chemical preperation
1.4.1. Hydration (oxidation) of alkenes make alcohols
1.4.2. Hydrogenation (reduction) of an aldehyde or ketone
1.4.2.1. aldehydes will be reduced to primary alcohols
1.4.2.2. ketones will be reduced to secondary alcohols through the addition of an H2
1.5. Chemical reactions
1.5.1. Combustion
1.5.1.1. methanol and ethanol in race cars
1.5.1.2. oxygenated gas
1.5.2. Oxidation
1.5.2.1. Only primary and secondary alcohols undergo oxidation with mild oxidizing agents
1.5.2.1.1. to form aldehydes and ketones because 2 hydrogen atoms are removed
1.5.2.1.2. Aldehydes further oxidized to carboxylic acids
1.5.3. Dehydration (removal of water molecule)
1.5.3.1. Intramolecular dehydration (elimination reaction)
1.5.3.1.1. removal of water from a singe alcohol
1.5.3.1.2. can be done to 1*,2* and 3*alcohols
1.5.3.2. Zaitsev's rule
1.5.3.2.1. applies to the intramolecular dehydration of 2* and 3* alcohol
1.5.3.2.2. used to determine the major product because more then one alkene can be produces
1.5.3.2.3. the adjacent carbon containing fewer H's will lose the H atom
1.5.3.3. Intermolecular dehydration (condensation reaction)
1.5.3.3.1. removal of water collectively from 2 alcohols to form an ether and water
1.5.3.3.2. only occurs with primary alcohols
1.5.4. Halogenation
1.5.4.1. halogen atom substituted for the OH group
1.5.4.1.1. produces alkyl halide
1.5.4.1.2. single product is formed using heat
1.5.5. Polymerization
1.5.5.1. alcohol monomers repeatedly added together
2. need 180 degrees and an acid catalyst
3. Phenols OH is always carbon 1 phenol
3.1. functional group
3.1.1. hydroxyl group attached to a benzene ring
3.2. Physical proerties
3.2.1. solubility
3.2.1.1. slightly soluble in water
3.2.2. state at room temperature
3.2.2.1. solids or oily liquids
3.2.3. properties
3.2.3.1. antiseptic: a substance that kills microorganisms on living tissue
3.2.3.2. disinfectant is a substance that kills microorganisms on an inanimate objects
3.3. Chemical properties
3.3.1. flammible
3.3.1.1. cannot be dehydrated
3.3.2. can be oxidyzed with strong oxidizing agengts
3.3.2.1. weak acids in solution
3.4. Uses
3.4.1. 2% phenol is used as a surgical antiseptic
3.4.2. derivatives used as an antiseptic and a disenfectant
3.4.3. foods
3.4.3.1. used as an antioxidant
3.4.3.2. used as a peservatives
3.4.4. anaesthetic
4. Carboxylic Acids
5. Amines
6. Esters
7. New Node
8. Ethers oxy
8.1. oxygen single bonded to 2 carbons c-o-c
8.2. ethers are produced through intermolecular dehydration of primary alcohols
8.3. Uses
8.3.1. MTBE is a gasoline additive
8.3.2. diethyl ether is was ageneral anaesthetic
8.4. Isomerism
8.4.1. constitutional isomers
8.4.1.1. due to different partitioning of R groups or functional groups isomers with alcohols
8.5. Physical properties of ethers
8.5.1. solubility
8.5.1.1. more soluble in water than alkanes due to H-bonds with water
8.5.1.2. similar solubility to alcohols
8.5.2. Boiling point
8.5.2.1. similar to alkanes
8.5.2.1.1. lower then alcohols
8.6. Chemical properties
8.6.1. flamible
8.6.1.1. form explosives
8.6.2. unreactive with acids, bases, and oxidizing agents
8.6.3. good solvents due to there unreactivity
8.6.3.1. easy to remove after areaction
8.7. Cyclic ethers
8.7.1. oxygen atom contained in carbon ring (o replaces a c in the ring)
8.8. Thiols
8.8.1. sulphur analog of alcohols because of the functional group R-SH
8.8.2. lower boiling points than alcohols
8.8.2.1. NO hydrogen bonds
8.8.3. strong and bad odour
8.8.4. easily oxidized to form disulfides R-S-S-R
8.8.4.1. important in protein structure (hair)
9. Aldehydes al
9.1. contain the carbonyl functional group C=O
9.1.1. polar bond with trigonal planar shape
9.2. have a carbonyl group at the end carbon ONLY
9.3. prepared by
9.3.1. oxidizing a primary alcohol with a mild oxidizing agent
9.3.1.1. removes 2 H atoms to form C=O
9.3.1.2. can be further oxidized to form a carboxilic acid by adding an oxygen atom
9.3.1.2.1. thus aldehydes must be protected from the air if you do not want further oxidation to occur
9.4. Simple aldehydes
9.4.1. Methanal
9.4.1.1. formed by oxidizing methenol an irritating gas carcinogenic to the skin
9.4.1.2. used to preserve biological speciments
9.4.2. Benzaldehyde
9.4.2.1. benzene ring attatched to methanal
9.4.2.1.1. gives almonds their flavour
10. What they both have in common
10.1. physical properties
10.1.1. boiling points
10.1.1.1. between alcohols and alkanes
10.1.1.2. higher boiling points than alkanes because C=O is polar thus dipole dipole atrtactions between the carbonyl groups
10.1.1.3. lower boiling points then alcohols because they can't H-bond between molecules
10.1.2. solubility
10.1.2.1. aldehydes and ketones H-bond with water so low molecular mass compounds are soluble in water
10.1.2.2. the longer the chain the less soluble or eventually insoluble they become
10.2. Uses
10.2.1. high molecular massed aldehydes and ketones have a pleasant smell and pleasant flavours
10.2.2. found widely in nature
10.3. Isomerism
10.3.1. Constitutionally isomerism, skeletal for both positional for ketones and functional groups subtypes
10.4. Chemical reactions
10.4.1. Oxidation
10.4.1.1. only aldehydes will further oxidize
10.4.1.2. Tollens test (silver mirror) AgNO3 added to an aldehyde soution
10.4.1.2.1. positive test indicated by the oxidation of aldehyde to carboxylic acid and the reduction of Ag+ ions to silver metal, Ag
10.4.1.2.2. example of a redox reaction, where Ag is the oxidizing agent
10.4.1.3. Benedict's test (copper brick) solution of CuSO4 added to unknown solution
10.4.1.3.1. if clear blue solution turns into a brick read suspension aldehydes were oxidized to carboxilic acids, the blue Cu2+ ions were reduced to red Cu+ ions
10.4.1.3.2. example of a redox reaction where Cu2+ is the oxidizing agen
10.4.1.3.3. originally used to detect glucose in the blood and urine to diagnose diabetes
10.4.2. Reduction
10.4.2.1. can be reduced by adding hydrogen gas to reform primary and secondary alcohols
10.4.3. Hemiacital formation
10.4.3.1. can be intermolecuar - to form a straight chain o rit can be an intramolecular reaction to form a cyclic hemiacital which are more stable
10.4.3.2. caused by a reaction of an aldehyde or ketone with an alcohol
10.4.3.2.1. the H atom of the alcohol is added to the O atom of the carbonyl group and or OR portion of the alcohol is added to the C atom of the carbonyl group in the presence of an acid catylist
10.4.3.3. hemiacital is an alcohol group and ether group attached to the same carbon
10.4.4. Acetal formation
10.4.4.1. reaction of a hemiacital with another alcohol molecule
10.4.4.2. condensation reaction because there is a removal of water (still need an acid catalyst)
10.4.4.3. more stable
10.4.4.4. functional group is made up of 2 ether groups bonded to the same carbon
10.4.5. Polymerization
10.4.5.1. under acidic conditions phenol and formaldehyde monomers react to form phenol-formaldehyde network polymers
10.4.5.2. network polymers
10.4.5.2.1. monomers connected in a 3D cross-linked network
10.4.5.3. first man-made plastic was a phenol-formaldehyde polymer called makelite
10.4.5.3.1. today used as adhesive for plywood
11. Ketones one
11.1. prepared
11.1.1. through oxidation of seconday alcohols
11.1.1.1. with mild oxidizing agent to remove 2 hydrogen atoms to form C=O
11.1.1.2. can not be further oxidized
11.2. contain the carbonyl functional group C=O and R-CO-R
11.2.1. polar bond with trigonal planar shape
11.2.2. carbonyl group is located in the carbon chain
11.3. Cyclic ketones exist
11.4. Ketone functional group has lower priority than an aldehyde when both are present the ketone is named as a substituent (oxo) (oxopentanal)
11.5. Uses
11.5.1. propanone (acetone
11.5.1.1. simplest ketone formed by the oxidation of 2-propanol
11.5.1.1.1. used as a solvent because it is soluble in both water and nonpolar subsances
11.5.1.2. byproduct of fat breakdown
11.5.1.3. component of nail polish remover
11.5.2. steroid hormones
11.5.2.1. testosterone, progesterone,and cortisone
11.5.3. sunscreens and sun-tannng agents