Organic Chemistry and Instrumental Analysis

A collection of vocabulary flashcards covering key concepts and terms related to organic chemistry and instrumental analysis.

Molecular Orbital Theory

A theory explaining bonding in complex molecules through the combination of atomic orbitals to form molecular orbitals.

Hybridization

The process of mixing atomic orbitals within an atom to create a new set of degenerate orbitals called hybrid orbitals.

HOMO (Highest Occupied Molecular Orbital)

The highest bonding molecular orbital that contains electrons.

LUMO (Lowest Unoccupied Molecular Orbital)

The lowest antibonding molecular orbital that is unoccupied by electrons.

Cis Isomer

A geometric isomer where the substituent groups are on the same side of a double bond.

Trans Isomer

A geometric isomer where the substituent groups are on opposite sides of a double bond.

Radical

A species with an unpaired electron, often formed during homolytic bond fission.

Nucleophile

An electron-rich species that donates an electron pair and is attracted to positively charged or partially positive regions.

Electrophile

An electron-deficient species that accepts an electron pair and is attracted to negatively charged or partially negative regions.

Curly Arrow Notation

A way to represent the movement of electrons in chemical reactions; single-headed arrows indicate single electron movement, while double-headed arrows indicate electron pairs.

Delocalisation

The distribution of electrons across several atoms in a molecule, as seen in aromatic systems like benzene.

Chromophore

A part of a molecule responsible for its color due to absorption of light, typically involving conjugated systems.

Conjugated System

A system of adjacent unhybridised p orbitals that overlap side-on, allowing for delocalised electrons.

Bond Fission

The process of breaking bonds in reactant molecules to form new bonds in product molecules.

Homolytic Fission

Breaking of a covalent bond resulting in two neutral radicals; each atom retains one electron.

Heterolytic Fission

Breaking of a covalent bond resulting in two oppositely charged ions; one atom retains both electrons.

Aromatic Compound

A compound containing a stable ring of conjugated pi electrons, typically represented by benzene.

Electrostatic Attraction

The force that causes oppositely charged particles to attract each other, fundamental in bonding.

Hydrogen Bonding

Attractive forces between a hydrogen atom bonded to a highly electronegative atom and another electronegative atom.

Isomer

Compounds with the same molecular formula but different structural or spatial arrangements.

Enantiomer

A type of optical isomer that is a non-superimposable mirror image of another.

Racemic Mixture

A mixture containing equal amounts of two optical isomers, resulting in no optical activity.

Markovnikov's Rule

A principle stating that in the addition of a polar reagent to an unsymmetrical alkene, hydrogen will attach to the carbon already having the most hydrogen atoms.