Structure and Properties of Organic Compounds

This set of flashcards covers the fundamental concepts of chemical bonding, quantum mechanics, hybridization, and acid-base chemistry as presented in the lecture notes.

Ionic Bond (1916)

A type of chemical bond proposed by Kossel Walther.

Covalent Bond

A chemical bond proposed by G. N. Lewis that is characteristic of carbon compounds and of great importance in organic chemistry.

Erwin Schrodinger (1926)

The scientist who introduced quantum mechanics.

Wave Equations

Equations based on the concept that electrons exhibit both particle and wave properties, describing the probability of finding an electron in space.

Orbital

A region of space where there is the highest probability of finding an electron.

Atomic Orbitals

Specific spatial regions occupied by electrons ($s, p, d, f$) depending on their energy levels.

Molecular Orbitals (Bonding Orbitals)

Formed when atomic orbitals of two atoms overlap to create a covalent bond, containing two electrons with opposite spins.

Sigma ($\sigma$) and Pi ($\pi$) Bonds

Types of bonding orbitals that are lower in energy and more stable than the original atomic orbitals.

Valence Bond Theory

A theory stating that unpaired electrons in one element tend to pair with unpaired electrons of another atom, where the number of bonds equals the number of unpaired electrons.

Hybridization

A concept used to explain the tetravalency of carbon ($1S^2, 2S^2, 2P^2$) and the formation of specific bond geometries.

Polar Covalent Bond

A bond in which electrons are attracted more strongly by one atom than the other, resulting from a difference in electronegativity.

Electronegativity

The inherent ability of an atom to attract electrons in a covalent bond.

Brønsted-Lowry Acid

A substance that releases a proton ($H^+$).

Brønsted-Lowry Base

A substance that accepts a proton ($H^+$).

Lewis Acid

A substance that has the ability to accept an electron pair.

Lewis Base

A substance that provides an electron pair.

Conjugate Relationship

A principle stating that a strong acid generally has a weak conjugate base, and vice versa.

Organic Acids

Compounds characterized by a hydrogen atom with positive polarization, such as methyl alcohol ($pK_a = 15.54$), acetic acid ($pK_a = 4.76$), and acetone ($pK_a = 19.3$).

Organic Bases

Compounds characterized by an atom with a non-bonding electron pair (lone pair) that can connect to $H$, such as trimethylamine or oxygen-containing compounds like methyl alcohol and acetone.