knowt logo

Chapter 1 - Classifying Organic Compounds

  • Organic chemistry: the study of compounds based on carbon

    • Ex. of organic compounds: natural gas, rubbing alcohol, aspirin, compounds that give fragrance to rose

Chapter 1.1: Bonding and the Shape of Organic Molecules

  • Organic compounds: compounds based on carbon; usually contains carbon-carbon and carbon-hydrogen bonds

  • Million of organic compounds, only a quarter of million of inorganic compounds

  • So many organic compounds because of carbon:

    • It forms four covalent bonds and connects to four other atoms

    • It forms strong single, double, or triple bonds with other carbons

  • Saturated bonds: molecules that contain only single carbon-carbon bonds

  • Unsaturated bonds: molecules that contain double or triple bonds

  • Carbon unique bonding properties formation of chains and rings with a variety of sizes

  • The shape of a molecule depends on the type of bond, examples include:

    • Carbon with four single bonds: tetrahedral shape

    • Carbon with one double bond and two singular bonds: trigonal planar shape

    • Carbon with two double bonds or one triple bond and one single bond: linear shape

    • Oxygen with two single bonds: bent shape

  • 2-D diagrams good for condensed structural diagrams and line structures

  • 3-D diagrams atoms are drawn with wedges to indicate it is in front, but lines when it is pushed back

  • Polar covalent bond: the covalent bond between two atoms with different electronegativities

  • Electronegativity: a measure of how strongly an atom attracts electrons in a chemical bond; partial negative or partial positive atom

  • Every polar bond has a bond dipole

  • Bond dipole: partial negative charge and partial positive charge, separated by the length of the bond

  • Polar molecule or molecular polarity: when the molecule has an overall imbalance of charge

    • A molecule has a region with a partial positive charge and a region with a partial negative charge

    • Not all molecules with polar bonds are polar molecules

    • To determine molecular polarity, must consider the shape of molecule and bond dipoles within the molecule

  • If equal bond dipoles act in opposite directions in three-dimensional space, they counteract each other

1.2 Hydrocarbons

  • Hydrocarbons: simplest type of organic compounds, composed of entirely carbon and hydrogen atoms

    • Aliphatic hydrocarbons: contains carbon atoms that are bonded in one or more chains and rings

    • Aromatic hydrocarbons: based on aromatic benzene group

      • Benzene is the simplest aromatic compound

  • Alkane: hydrocarbon that has only single bonds

    • CnH2n+2

    • Cycloalkane: alkane in a shape of a ring

      • CnH2n

  • Alkene: hydrocarbon with at least one double bond

    • CnH2n

  • Functional Group: a reactive group of bonded atoms that appears in all the members of a chemical family

  • Alkyne: hydrocarbon with at least one triple bond

    • CnH2n-2

  • Rules for Naming Organic Compounds:

    • Prefix + root + suffix

      • Root: number of carbon atoms in the main chain or ring

        • Number of carbon atoms:

          • 1: -meth-

          • 2: -eth-

          • 3: -prop-

          • 4: -but-

          • 5: -pent-

          • 6: -hex-

          • 7: -hept-

          • 8: -oct-

          • 9: -non-

          • 10: -dec-

      • Suffix: type of compound according to functional groups present

        • Alkanes: -ane

        • Alkenes: -ene

        • Alkynes: -yne

      • Prefix: indicates name and location of each branch and functional group on the main carbon chain

        • Alkyl group: removing one hydrogen from an alkane; branches attached to the main chan, common Alkyl groups:

          • Methyl

          • Ethyl

          • Propyl

          • Isopropyl

          • Butyl

          • Sec-butyl

          • Iso-butyl

          • Tert-butyl

  • Aromatic compounds*:*** cyclic compound with alternating single and double bonds, such as benzene

Chapter 1.3: Single-Bonded Functional Groups

  • OH (hydroxyl) group: a functional group that contains OH

  • general formula: R+ functional, family of simple organic compounds

    • R' and R’’ are used for more than one alkyl group

  • Compounds with the same functional group often have similar physical properties

  • Compounds with the same functional group react chemically in very similar ways

  • Common Functional Groups:

    • Alkane

    • Alkyne

    • Alcohol

    • Amine

    • Aldehyde

    • Ketone

    • Carboxylic acid

    • Ester

  • Intermolecular forces: forces of attraction and repulsion between particles; organic compounds with the same functional groups have the same physical properties, which are often caused by intermolecular forces, which include:

    • Hydrogen bonding: strong intermolecular attraction between the hydrogen atom with an N, O, F atom

    • Dipole-Dipole interactions: attractive forces between polar molecules

    • Dispersion forces: attractive forces that occur between all covalent molecules

  • Alcohol, alkyl halides, ethers, and amines are all functional groups with single bonds

  • Alcohol: an organic compound that contains the -OH functional group

    • Alcohols are named after parent alkane

    • Parent alkane: alkane with the same basic carbon structure

    • Very polar due to O-H bond, soluble in water

    • Flammable and most are poisonous

  • Alkyl halide/haloalkane: alkane in which one or more hydrogen atoms have been replaced with halogen atoms (F, Cl, Br, or I); R-X Similar properties to alcohols

  • Ether: organic compound that has two alkyl groups joined by an oxygen atom; R-O-RAlkoxy group: alkyl singularly bonded to oxygen Less polar than water and alcoholUsually soluble in water but decreases as the alkyl group increasesLower boiling point than water

  • Amine: An organic compound with the functional group -NH2, -NHR, or -NR2

    • Polar compounds

Chapter 1.4: Functional Groups With the C=O Bond

  • Carbonyl group: carbon atom double-bonded to an oxygen atom; C=O

  • Aldehyde: organic compound that has double-bonded oxygen on the last carbon of a carbon chain; R-CHO

  • Ketone: organic compound that has double-bonded oxygen on any carbon within the carbon chain; RCOR’

    • Contains C=O, usually polar

    • Soluble in water

    • Boiling points lower than corresponding alcohols, but higher to corresponding alkanes

  • Carboxylic acid: carbon atom is bonded to an oxygen atom by a double bond and to a hydroxyl group (-OH) by a single bond

    • Polar because of O-H and C=O bonds

    • Contains hydrogen bonds, which makes it have higher boiling points

    • If it has lower mass, then it becomes soluble in water

    • Decreases in solubility as carbon atom increases

    • Unpleasant odors

    • Carboxylic acid derivative: exchange in hydroxyl group of carboxylic acid with a different organic compound

  • Carboxyl group: COOH group

  • Ester is a derivative of carboxylic acid

  • Ester: general formula for an ester is RCOOR’

    • R is a hydrogen atom or a hydrocarbon, and R′ is a hydrocarbon

    • Polar Molecule

    • Cannot form hydrogen bonds with other ester atoms, only with water

    • Low boiling point

    • Volatile at room temperature

  • Amide: carbon atom double-bonded to an oxygen atom and single-bonded to a nitrogen atom

    • C-N and N-H bonds make it polar, acts like carboxylic acids

    • Stronger hydrogen bonds than carboxylic acids

    • Soluble in water

    • High melting and boiling points

    • Simple amides are solid at room temperature

Chapter 1 - Classifying Organic Compounds

  • Organic chemistry: the study of compounds based on carbon

    • Ex. of organic compounds: natural gas, rubbing alcohol, aspirin, compounds that give fragrance to rose

Chapter 1.1: Bonding and the Shape of Organic Molecules

  • Organic compounds: compounds based on carbon; usually contains carbon-carbon and carbon-hydrogen bonds

  • Million of organic compounds, only a quarter of million of inorganic compounds

  • So many organic compounds because of carbon:

    • It forms four covalent bonds and connects to four other atoms

    • It forms strong single, double, or triple bonds with other carbons

  • Saturated bonds: molecules that contain only single carbon-carbon bonds

  • Unsaturated bonds: molecules that contain double or triple bonds

  • Carbon unique bonding properties formation of chains and rings with a variety of sizes

  • The shape of a molecule depends on the type of bond, examples include:

    • Carbon with four single bonds: tetrahedral shape

    • Carbon with one double bond and two singular bonds: trigonal planar shape

    • Carbon with two double bonds or one triple bond and one single bond: linear shape

    • Oxygen with two single bonds: bent shape

  • 2-D diagrams good for condensed structural diagrams and line structures

  • 3-D diagrams atoms are drawn with wedges to indicate it is in front, but lines when it is pushed back

  • Polar covalent bond: the covalent bond between two atoms with different electronegativities

  • Electronegativity: a measure of how strongly an atom attracts electrons in a chemical bond; partial negative or partial positive atom

  • Every polar bond has a bond dipole

  • Bond dipole: partial negative charge and partial positive charge, separated by the length of the bond

  • Polar molecule or molecular polarity: when the molecule has an overall imbalance of charge

    • A molecule has a region with a partial positive charge and a region with a partial negative charge

    • Not all molecules with polar bonds are polar molecules

    • To determine molecular polarity, must consider the shape of molecule and bond dipoles within the molecule

  • If equal bond dipoles act in opposite directions in three-dimensional space, they counteract each other

1.2 Hydrocarbons

  • Hydrocarbons: simplest type of organic compounds, composed of entirely carbon and hydrogen atoms

    • Aliphatic hydrocarbons: contains carbon atoms that are bonded in one or more chains and rings

    • Aromatic hydrocarbons: based on aromatic benzene group

      • Benzene is the simplest aromatic compound

  • Alkane: hydrocarbon that has only single bonds

    • CnH2n+2

    • Cycloalkane: alkane in a shape of a ring

      • CnH2n

  • Alkene: hydrocarbon with at least one double bond

    • CnH2n

  • Functional Group: a reactive group of bonded atoms that appears in all the members of a chemical family

  • Alkyne: hydrocarbon with at least one triple bond

    • CnH2n-2

  • Rules for Naming Organic Compounds:

    • Prefix + root + suffix

      • Root: number of carbon atoms in the main chain or ring

        • Number of carbon atoms:

          • 1: -meth-

          • 2: -eth-

          • 3: -prop-

          • 4: -but-

          • 5: -pent-

          • 6: -hex-

          • 7: -hept-

          • 8: -oct-

          • 9: -non-

          • 10: -dec-

      • Suffix: type of compound according to functional groups present

        • Alkanes: -ane

        • Alkenes: -ene

        • Alkynes: -yne

      • Prefix: indicates name and location of each branch and functional group on the main carbon chain

        • Alkyl group: removing one hydrogen from an alkane; branches attached to the main chan, common Alkyl groups:

          • Methyl

          • Ethyl

          • Propyl

          • Isopropyl

          • Butyl

          • Sec-butyl

          • Iso-butyl

          • Tert-butyl

  • Aromatic compounds*:*** cyclic compound with alternating single and double bonds, such as benzene

Chapter 1.3: Single-Bonded Functional Groups

  • OH (hydroxyl) group: a functional group that contains OH

  • general formula: R+ functional, family of simple organic compounds

    • R' and R’’ are used for more than one alkyl group

  • Compounds with the same functional group often have similar physical properties

  • Compounds with the same functional group react chemically in very similar ways

  • Common Functional Groups:

    • Alkane

    • Alkyne

    • Alcohol

    • Amine

    • Aldehyde

    • Ketone

    • Carboxylic acid

    • Ester

  • Intermolecular forces: forces of attraction and repulsion between particles; organic compounds with the same functional groups have the same physical properties, which are often caused by intermolecular forces, which include:

    • Hydrogen bonding: strong intermolecular attraction between the hydrogen atom with an N, O, F atom

    • Dipole-Dipole interactions: attractive forces between polar molecules

    • Dispersion forces: attractive forces that occur between all covalent molecules

  • Alcohol, alkyl halides, ethers, and amines are all functional groups with single bonds

  • Alcohol: an organic compound that contains the -OH functional group

    • Alcohols are named after parent alkane

    • Parent alkane: alkane with the same basic carbon structure

    • Very polar due to O-H bond, soluble in water

    • Flammable and most are poisonous

  • Alkyl halide/haloalkane: alkane in which one or more hydrogen atoms have been replaced with halogen atoms (F, Cl, Br, or I); R-X Similar properties to alcohols

  • Ether: organic compound that has two alkyl groups joined by an oxygen atom; R-O-RAlkoxy group: alkyl singularly bonded to oxygen Less polar than water and alcoholUsually soluble in water but decreases as the alkyl group increasesLower boiling point than water

  • Amine: An organic compound with the functional group -NH2, -NHR, or -NR2

    • Polar compounds

Chapter 1.4: Functional Groups With the C=O Bond

  • Carbonyl group: carbon atom double-bonded to an oxygen atom; C=O

  • Aldehyde: organic compound that has double-bonded oxygen on the last carbon of a carbon chain; R-CHO

  • Ketone: organic compound that has double-bonded oxygen on any carbon within the carbon chain; RCOR’

    • Contains C=O, usually polar

    • Soluble in water

    • Boiling points lower than corresponding alcohols, but higher to corresponding alkanes

  • Carboxylic acid: carbon atom is bonded to an oxygen atom by a double bond and to a hydroxyl group (-OH) by a single bond

    • Polar because of O-H and C=O bonds

    • Contains hydrogen bonds, which makes it have higher boiling points

    • If it has lower mass, then it becomes soluble in water

    • Decreases in solubility as carbon atom increases

    • Unpleasant odors

    • Carboxylic acid derivative: exchange in hydroxyl group of carboxylic acid with a different organic compound

  • Carboxyl group: COOH group

  • Ester is a derivative of carboxylic acid

  • Ester: general formula for an ester is RCOOR’

    • R is a hydrogen atom or a hydrocarbon, and R′ is a hydrocarbon

    • Polar Molecule

    • Cannot form hydrogen bonds with other ester atoms, only with water

    • Low boiling point

    • Volatile at room temperature

  • Amide: carbon atom double-bonded to an oxygen atom and single-bonded to a nitrogen atom

    • C-N and N-H bonds make it polar, acts like carboxylic acids

    • Stronger hydrogen bonds than carboxylic acids

    • Soluble in water

    • High melting and boiling points

    • Simple amides are solid at room temperature

robot