Acetone
64.6 °C
The study of structures, properties, and reactions of carbon compounds.
It reflects the ongoing synthesis of new compounds by scientists in laboratories.
CH2 = CH2
Methanamide is a liquid at room temperature.
The general formula for alkanols is CnH2n+1OH.
Ethanamide has a melting point of 80.2 °C and a boiling point of 222 °C.
Examples of alcohols include ethanol, propan-1-ol, and cyclohexanol.
Because nitrogen is less electronegative than oxygen, making the N-H bond less polar than the O-H bond.
They can be presented by a molecular formula, a structural formula, a condensed structural formula, or a skeletal formula.
Ester group, carbon-carbon double bond, amine group (–NH2), amide group, and ether group (–O–).
Propanone
CH4
Hydrogen bonds form between methanamine molecules.
−88.6 °C
Hexane
Ethyl methanoate
Ester, Amide, and Hydroxyl.
2,2-dimethylbutane
C_nH_{2n+2}.
As the number of branches increases, the boiling point decreases.
It is bonded to at least one hydrogen atom and is at the terminal position of the main chain.
0.626 g cm−3
Amines have lower boiling points than alcohols with a comparable relative molecular mass.
In Chapter 21, pages 60–63.
C_nH_{2n} (n = 2, 3, 4…)
C_nH_{2n}
They make up the cells in our bodies, the clothes we wear, the food we eat, and the plastic objects we use.
The intermolecular forces between propane molecules are stronger than those between ethane molecules due to propane's larger molecular size, resulting in higher boiling points.
Propane is a non-polar compound, while 1-chloropropane is polar. The van der Waals' forces between propane molecules are weaker than those between 1-chloropropane molecules, leading to a lower boiling point for propane.
C6H14
The first word indicates the alkyl group of the parent alcohol, and the second indicates the parent acid with the suffix -oate.
Alkanes are soluble in non-polar solvents such as benzene and tetrachloromethane.
It is produced from the reaction between propan-1-ol and 2-methylpentanoic acid.
Butanamide is slightly soluble in water.
The amide group can form hydrogen bonds with water molecules, contributing to the solubility of unsubstituted amides in water.
Soluble
The water solubility of alcohols is related to the length of the hydrocarbon chain; shorter chains are more soluble due to the hydrophilic hydroxyl group forming hydrogen bonds with water.
Dimer
A group of carbon compounds that have the same general formula.
All liquid alkanes have densities less than 1.0 g cm–3, making them the least dense among all groups of carbon compounds.
RCOR’ (e.g., CH3COCH3 for propanone)
−47.7 °C
–CHO
Unsubstituted amides with fewer carbon atoms are soluble in water, but their solubility decreases as the length of the hydrocarbon chain increases.
31.7 °C
Chloroform
Ethyl propanoate
CH4
Insoluble
RNH2 (e.g., CH3NH2 for methanamine)
Propanamide can form more extensive hydrogen bonds due to having two partially positively charged hydrogen atoms, while propanoic acid has only one.
Aldehydes and ketones do not have hydrogen bonds between their own molecules, unlike alcohols.
'-en' should be inserted into the name.
Branched-chain alkanes are more spherical in shape, resulting in a smaller area of contact and weaker van der Waals' forces between molecules.
Propanal
Extensive hydrogen bonding occurs between unsubstituted amide molecules due to the partially positively charged hydrogen atoms forming bonds with lone pairs on oxygen atoms.
3-methylpentane
Alkane molecules are non-polar and cannot form hydrogen bonds with water molecules, making them insoluble in water.
Unsubstituted amides have higher boiling points due to extensive hydrogen bonding between their molecules.
Because the carboxyl group in their molecules can form hydrogen bonds with water molecules.
HCOOH, known as methanoic acid
CH3CH(CH3)CH2CH2CH3
Alkene molecules are non-polar and cannot form hydrogen bonds with water molecules.
The solubility of carboxylic acids in water decreases.
RCOOR’ (e.g., HCOOCH3 for methyl methanoate)
Methyl ethanoate, butan-1-amine, propanoic acid, propanamide
C_nH_{2n+2}
Omega-3 fatty acids are polyunsaturated fatty acids that cannot be synthesized by the body and must be obtained from food. They are essential for normal brain function and can reduce the risk of heart diseases.
The boiling point gradually increases from methanol to hexan-1-ol due to stronger van der Waals' forces between the alcohol molecules.
The increase in branching reduces the surface area, leading to weaker van der Waals forces and lower boiling points.
It is bonded to alkyl groups on both sides.
Aldehydes and ketones are polar due to the carbonyl group, leading to stronger van der Waals' forces compared to non-polar alkanes.
CH3I
They represent alkyl groups, which may be the same or different.
Propanoic acid.
Their water solubility decreases.
Longer carbon chains are hydrophobic and block the hydroxyl group, making it less favorable to form hydrogen bonds with water.
Avian influenza (H5N1)
Esters have a pleasant fruity smell, and each ester has its own characteristic smell.
-dial
Alcohols have higher boiling points than alkanes with a comparable relative molecular mass.
-dione
Formaldehyde
propanedial
Aldehydes and ketones with fewer carbon atoms are soluble in water.
pentan-2-one
The condensed structural formula for pentanoic acid is CH3(CH2)3COOH.
Prefixes are inserted into their names.
Saturated hydrocarbons.
HCONH2, known as methanamide
The condensed structural formula of propanamide is CH3CH2CONH2.
The bulky hydrocarbon chain blocks the –COOH group, making it less favorable to form hydrogen bonds with water molecules.
Esters cannot form hydrogen bonds with each other.
HCHO
Haloalkanes are carbon compounds in which one or more hydrogen atoms in an alkane have been replaced by halogen atoms (fluorine, chlorine, bromine, or iodine).
Yes, primary amines with fewer carbon atoms are very soluble in water, similar to ammonia.
Branched-chain alkanes have lower boiling points.
Haloalkanes have polar carbon-halogen bonds, leading to stronger van der Waals' forces compared to non-polar alkanes.
Only alcohols with three or fewer carbon atoms, such as methanol, ethanol, and propan-1-ol, are miscible with water.
The boiling point increases with the length of the hydrocarbon chain.
CHCl3
Aldehydes and ketones have higher boiling points than alkanes but lower boiling points than alcohols with a comparable relative molecular mass.
The boiling point of butanoic acid is 163.8 °C.
Alkanes are insoluble in water.
132.8 °C
The last letter 'e'.
290 °C
An amide group is a functional group derived from a carboxylic acid, where the hydroxyl group is replaced by a nitrogen atom.
47.2 °C
But-1-ene has a smaller molecular size than pent-1-ene, resulting in weaker van der Waals' forces between but-1-ene molecules compared to those between pent-1-ene molecules.
Docosahexaenoic acid (DHA) is an omega-3 fatty acid that contains six C=C double bonds, important for maintaining health.
Propan-2-ol
HCOOCH2CH3
The solubility decreases as the length of the hydrocarbon chain increases.
The hydroxyl group (–OH) is hydrophilic and can form hydrogen bonds with water, enhancing solubility.
Hydrogen bonds
An ester is often represented as RCOOR’, where R is a hydrogen atom or an alkyl group from the parent acid, and R’ is an alkyl group from the parent alcohol.
The lone pairs of electrons on the oxygen atom of the carbonyl group can form hydrogen bonds with hydrogen atoms in water molecules.
101.3 °C
The boiling point of Fluoromethane (CH3F) is -78.4 °C.
It is an aldehyde with a carbon-carbon double bond.
Chloromethane (CH3Cl) is slightly soluble in water.
Ethanoic acid is very soluble in water.
The condensed structural formula for 1-bromobutane is CH3(CH2)3Br.
HCHO
The correct systematic name should assign a lower numeral to the carbonyl group instead.
Alkanoic acid has the general formula CnH2n+1COOH.
C6H11COOH is a carboxylic acid but not an alkanoic acid.
CH3(CH2)5OH
Due to the ability to form hydrogen bonds, which are stronger in carboxylic acids.
Molecules of methyl ethanoate are held together by van der Waals’ forces, which are the weakest intermolecular forces compared to the hydrogen bonds in the other compounds.
63.5 °C
-al
Yes, the N atom in the methanamide molecule can participate in hydrogen bond formation due to the presence of the –NH2 group.
Yes, alkenes are soluble in non-polar solvents.
130.5 °C
Propanamide can participate in hydrogen bond formation through both the amide group and the –NH2 group, while butan-1-amine can only participate through the amine group.
Add a numeral before the suffix.
C_nH_{2n+1}X or RX
Pentane is non-polar, while butanal is polar, leading to weaker van der Waals’ forces in pentane.
CH3X
CH3(CH2)3OH
CH3NH2
They become less soluble in water.
Propan-2-ol
97.2 °C
Haloalkanes have higher boiling points than alkanes with a comparable relative molecular mass.
5-溴-4-氟-3-甲基己-2-胺
It incorrectly suggests a position for the carbonyl group in a ketone.
Aldehydes have higher boiling points than alkanes but lower boiling points than alcohols with a comparable relative molecular mass.
Esters are formed from the reactions between carboxylic acids and alcohols.
They are listed in Table 42.3.
-one
H2C=CH2
Haloalkanes are often represented as RX, where R is an alkyl group and X is a halogen atom.
A lower numeral should be assigned to the carbonyl group instead of the doubly-bonded carbon atom.
Their solubility in water decreases as the length of the hydrocarbon chain increases.
Yes, the oxygen atoms in an ester group can form hydrogen bonds with the hydrogen atoms of water molecules.
The systematic name is propanal.
Most aldehydes have an unpleasant and pungent smell, whereas ketones usually have a pleasant and sweet smell.
Extensive hydrogen bonding between carboxylic acid molecules contributes to their higher boiling points compared to alcohols with a comparable relative molecular mass.
The boiling point of 1-chlorobutane (CH3(CH2)3Cl) is 78.4 °C.
Very soluble
Slightly soluble
Alcohols with fewer carbon atoms are soluble in water.
An unsubstituted amide is an amide where the nitrogen atom is bonded to two hydrogen atoms, often represented as RCONH2.
Slightly soluble
As the molecular size increases, the van der Waals' forces become stronger, requiring more energy to separate the molecules during boiling, thus increasing the boiling point.
Tamiflu
Carboxylic acids have a characteristic pungent smell and a sour taste.
They are held together by van der Waals’ forces, which are weaker than the hydrogen bonds in butan-1-ol and propanoic acid.
Carboxylic acids are all weak acids and non-corrosive in dilute solution.
The boiling point of methanoic acid is 101 °C.
Propanoic acid can form more extensive hydrogen bonding due to both the carbonyl and hydroxyl groups, unlike butan-1-ol which can only use the hydroxyl group.
CH3OH
Alcohol molecules can form hydrogen bonds with each other.
77.0 °C
The boiling point increases as the molecular size increases.
Carboxylic acids are often represented as RCOOH where R is a hydrogen atom or an alkyl group.
No, it is always at one end of the main chain.
Hydrogen bonding occurs between carboxylic acid molecules.
Very soluble
16.5 °C
Esters have boiling points similar to those of aldehydes and ketones with a comparable relative molecular mass.
Ethanoic acid
Very soluble
Examples of esters include methyl methanoate and ethyl methanoate.
Haloalkanes are generally insoluble in water, with some being slightly soluble if they have fewer carbon atoms.
56.1 °C
Slightly soluble.
The physical properties of haloalkanes include boiling points and solubility in water, which vary among different haloalkanes.
Examples of carboxylic acids include methanoic acid, ethanoic acid, and propanoic acid.
CH3CH(OH)CH2OH
Most haloalkanes are insoluble in water.
Carboxylic acids with fewer carbon atoms are very soluble in water.
The systematic name is formed by replacing '-oic acid' with '-amide' from the name of the parent carboxylic acid.
The systematic name for formic acid is methanoic acid.
The part ‘-en’ should be incorporated into their names.
The systematic name for oxalic acid is ethanedioic acid.
Substituted amides are derived from carboxylic acids by replacing the carboxyl group with an amide group.
Unsubstituted amides are often represented as RCONH2, where R is a hydrogen atom or an alkyl group.
The systematic name for isooctane is 2,2,4-trimethylpentane.
The part '-en' should be incorporated into the name.
Most commercial white vinegars are aqueous solutions of acetic acid (about 5% of acetic acid by mass).
The systematic name for acetylene is ethyne.
The systematic name for toluene is methylbenzene.
Primary amines have lower boiling points than alcohols with a comparable relative molecular mass.
The systematic name for butyric acid is butanoic acid.
The systematic name for iodoform is triiodomethane.
The systematic name for tert-butyl alcohol is 2-methylpropan-2-ol.
Acetone is used as a solvent in nail polish remover.
The systematic name for adipic acid is hexanedioic acid.
The systematic name for benzyl alcohol is phenylmethanol.
The systematic name for glycerine is glycerol.
The systematic name for isobutane is 2-methylpropane.
The systematic name for succinic acid is butanedioic acid.
The systematic name for acetaldehyde is ethanal.
The systematic name for ethyl alcohol is ethanol.
The systematic name for isobutyl alcohol is 2-methylpropan-1-ol.
The systematic name for terephthalic acid is benzene-1,4-dicarboxylic acid.
The systematic name for wood alcohol is methanol.
The name of each substituent is written first, followed by the name of the amide, with a capital letter N added in front of each substituent.
