Organic Chemistry - Unit 1

Compounds with the same chemical formula but different arrangements of atoms.

Compounds with a hydroxyl (OH) group bonded to a carbon atom.

Compounds with a carbonyl group (C=O) connected to two other groups.

Compounds with a carbonyl group (C=O) connected to one R group and one hydrogen.

A reaction where electrons are lost. Primary alcohols form aldehydes, secondary alcohols form ketones, and aldehydes form carboxylic acids.

A reaction where hydrogen is added across a double or triple bond. Alkynes and alkenes become alkanes.

A reaction where water is added across a double bond. Alkenes become alcohols.

A reaction where a halogen atom is added across a double bond. Alkenes become dihalides.

A chemical reaction where an alkene reacts with a hydrogen halide (HCl, HBr) to form an alkyl halide.

A chemical reaction where a nucleophile replaces a halide group (X) in an alkyl halide (R-X).

A chemical reaction where a hydrogen atom in an aromatic compound is replaced by an electrophile.

A large molecule formed by the linking of many smaller repeating units called monomers.

A small molecule that can be linked to other similar molecules to form a polymer.

The process of linking monomer units together to form a polymer.

A polymer formed by the addition of monomers with double bonds, without any byproducts.

A polymer formed by the reaction of two or more monomers, with the elimination of small molecules like water or alcohol.

The weakest type of intermolecular force present in all molecules, regardless of polarity. These forces are caused by temporary fluctuations in electron distribution, creating temporary dipoles.

A type of intermolecular force occurring only in polar molecules. It arises from the attraction between the positive end of one polar molecule and the negative end of another.

The strongest type of intermolecular force, specifically occurring in molecules containing hydrogen bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine.

The process of determining whether a molecule is polar or nonpolar, based on its molecular shape and the electronegativity difference of its atoms.

A measure of an atom's ability to attract electrons within a chemical bond. Greater the difference in electronegativity between atoms, stronger the polarity of the bond.

Molecules with zero net dipole moment due to their symmetrical shape and/or equal sharing of electrons.

Molecules with asymmetric shapes and a net dipole moment due to unequal sharing of electrons.

The temperature at which a substance transitions from a liquid state to a gaseous state. Substances with stronger intermolecular forces (IMFs) have higher boiling points.

Catalysts speed up reactions by providing an alternative pathway with lower activation energy.

Catalysts do not change the position of equilibrium or the equilibrium constant (K). They only speed up the rate at which equilibrium is reached.

Catalysts do not affect the enthalpy change (ΔH) of a reaction. They simply make the reaction faster.

The minimum energy required for a collision between molecules to result in a reaction.

Reactions occur when molecules collide with enough energy and in the correct orientation.

The process of a substance gaining electrons, resulting in a decrease in oxidation number.

The process of a substance losing electrons, resulting in an increase in oxidation number.

A chemical reaction involving both oxidation and reduction, where one substance is oxidized while another is reduced.

A model of the atom that describes electrons as existing in probability clouds or orbitals, where their positions are uncertain. Unlike the Bohr model, it considers electrons as both waves and particles, using quantum numbers to describe their energy levels and positions.

A principle that states that you cannot know both an electron's position and momentum exactly at the same time.

The arrangement of atoms in a molecule, determined by the repulsion between electron pairs in the valence shell.

A chemical reaction that releases heat to the surroundings, and the equilibrium constant (K) decreases with increasing temperature.

A chemical reaction that absorbs heat from the surroundings, and the equilibrium constant (K) increases with increasing temperature.

A change in reaction conditions (like temperature, pressure, or concentration) that shifts the equilibrium to relieve the stress and favor either reactants or products.

A substance that speeds up a chemical reaction without being consumed in the process.

The ratio of products to reactants at equilibrium, representing the extent to which a reaction proceeds to completion.