CHEM 261

Introduction to Organic Chemistry

Alkane

Single carbon-carbon bond

Alkene

Double carbon-carbon bond

Alkyne

Triple carbon-carbon bond

Arene

Aromatic ring

Haloalkane

C-X (x= halogen)

Alcohol

C-OH

Ether

C-O-C

Aldehyde

Ketone

Carboxylic Acid

Ester

Acid Halide

Anhydride

Amide

Amine

Primary Carbon

1 substituent on carbon

Secondary Carbon

2 substituent on carbon

Tertiary Carbon

3 substituent on carbon

Quaternary Carbon

4 substituent on carbon

Covalent Bonding

Sharing of electrons between atoms

SP³ Hybridization

tetrahedron, bond angles are 109°

SP² Hybridization

planar, bond angles are 120° (double bond)

SP Hybridization

linear, bond angles are 180° (triple bond)

Steroid Molecule

Decane

C10H22

Undecane

C11H24

Dodecane

C12H26

Tridecane

C13H28

Tetradecane

C14H30

Pentadecane

C15H32

Eicosane

C20H42

Heneicosane

C21H44

Docosane

C22H46

Tricosane

C23H62

Triacontane

C30H62

Hentriacontane

C31H64

Dotriacontane

C32H66

Tetracontane

C40H82

Pentacotane

C50H102

Hexacotane

C60H122

Structural isomer

same molecular formula as another molecule but a different arrangement

Stereoisomer

same molecular formula and connectivity of atoms but different three-dimensional arrangement of atoms

Chemistry

Study of matter

Organic Chemistry

Study of compounds containing carbon

Atomic Number

Number of protons in the nucleus of an atom (Z)

Atomic Weight

Mass of protons (p+) and neutron (n) (unit: amu)

Molecular Weight

Mass of atoms in a molecule

Isotopes

same element that contain equal number of protons but different number of neutrons

s-Orbital

Spherical shaped cloud of electrons (electron density)

p-Orbital

Dumbbell-shaped cloud of electrons (Three orientations: placed on the x, y and z-axis)

Isoelectronic

same electronic structure

Ionic Bonding

positive and negative species are bonded to each other

Hybridization

Mixing of atomic orbitals (with the wrong geometry for bonding) to form hybrid orbitals with the correct geometry for bonding

sigma orbital

molecular wave function (orbital) made by linear combination of atomic orbitals having an s component

enthalpy

bond energy

pi orbital

molecular wave function (orbital) made by linear combination of two p atomic orbitals

electronegativity

desire (attraction) of an atom for electrons (negative charge)

London forces

intermolecular attraction due to temporary dipoles

Lewis acid

A substance that can accept a pair of electrons