Organic Chemistry Overview

Organic Chemistry

• Organic chemistry is the study of carbon compounds.
• Over 10 million carbon compounds have been identified.
• About 1000 new ones are identified each day.
• Carbon (C) is a small atom.
• It forms single, double, and triple bonds.
• Carbon's electronegativity is intermediate (2.5).
• Carbon forms strong bonds with carbon (C), hydrogen (H), oxygen (O), nitrogen (N), and some metals.
• Organic compounds are found in many things, including foods, flavors, fragrances, medicines, toiletries, cosmetics, plastics, films, fibers, resins, paints, varnishes, glues, adhesives, fuels, lubricants, and living organisms.

Functional Groups

• A functional group is an atom or group of atoms within a molecule that exhibits specific chemical reactivity.
• Functional groups are important because they:
  • Define classes of organic compounds.
  • Indicate sites of chemical reactions.
  • Provide a basis for naming organic compounds.

Hydrocarbons

• Hydrocarbons are a major class of organic compounds that contain only carbon and hydrogen atoms.
• They are categorized as aliphatic or aromatic.
  • Aliphatic hydrocarbons:
    • Open-chain (non-cyclic)
    • Saturated (Alkanes) — single bonds
    • Unsaturated (Alkenes) — double bonds
    • Unsaturated (Alkynes) — triple bonds
  • Aromatic hydrocarbons:
    • Cyclic
    • Saturated (Cycloalkanes) — single bonds
    • Unsaturated (Cycloalkenes) — double bonds
• Alkanes are also called paraffins.
• Alkenes are also called olefins.
• Alkynes are also called acetylenes.

Classification of Carbon Atoms

• Carbon atoms in a molecule can be classified as:
  • Primary (1° C): Bonded to one other carbon.
  • Secondary (2° C): Bonded to two other carbons.
  • Tertiary (3° C): Bonded to three other carbons.
  • Quaternary (4° C): Bonded to four other carbons.

Covalent Bonding and Molecular Shapes

• Covalent bonding involves sharing of electrons between atoms.
• Molecular shapes are determined by the arrangement of atoms and bonds.

s and p Orbital Shape

• s and p orbitals are fundamental to understanding atomic structure and bonding.

Hybridization of Atomic Orbitals

• Hybrid orbitals are formed by combining atomic orbitals.
• The number of hybrid orbitals formed equals the number of atomic orbitals combined.
• Elements in the second period (like carbon) can form sp³, sp², and sp hybrid orbitals.

sp³ Hybridization

• The combination of one 2s and three 2p orbitals results in four sp³ hybrid orbitals.
• These orbitals are equivalent in energy and shape.
• They form sigma bonds.
• Methane (CH₄) is an example of an sp³ hybridized molecule. Example of a tetrahedral structure.

sp² Hybridization

• The combination of one 2s and two 2p orbitals results in three sp² hybrid orbitals.
• These orbitals are equivalent in energy and shape.
• They form three sigma bonds and one pi bond.
• Ethylene (C₂H₄) is an example of an sp² hybridized molecule. Example of a trigonal planar structure.

sp Hybridization

• The combination of one 2s and one 2p orbital results in two sp hybrid orbitals.
• These orbitals are equivalent in energy and shape.
• They form two sigma bonds and two pi bonds.
• Acetylene (C₂H₂) is an example of an sp hybridized molecule. Example of a linear structure.

Explore the fascinating world of organic chemistry, a field dedicated to the study of carbon compounds. Discover the significance of functional groups in defining organic compound classes and their reactivity. This quiz covers essential concepts including the properties of carbon and the vast array of organic compounds present in everyday life.