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Configuration
the order and relative spatial arrangement of the atoms in a molecule. Absolute configuration is when the relative 3-dimensional arrangement in space of atoms in a chiral molecule have been correlated with an absolute standard.
Configurational isomers
a series of compounds which have the same constitution and bonding of atoms, but which differ in their atomic spatial arrangement. [Glucose and mannose]. Also called stereoisomers.
Conformation
the spatial arrangement of a molecule in space at any moment in time.
Co-ordinate bond
The linkage of two atoms by a pair of electrons, both electrons being provided by one of the atoms (the donor).
Acid
an agent able to produce positively charged hydrogen ions (H+).
Bronsted acid
Proton donor
Covalency number
refers to the number of unpaired electrons in the orbital of an atom; determines the number of covalent bonds
Covalent bond
the linkage of two atoms by the sharing of two electrons
Dextrorotatory
the phenomenon in which plane polarized light is turned in a clockwise direction.
Optical Activity
capability of organic compounds to rotate polarized light to the left or right
Polarimeter
Instrument used to measure optical activity
Diastereomers
stereoisomeric structures which are not enantiomers (mirror images) of one another.
Dissociation
The process whereby a molecule is split into simpler fragments which may be smaller molecules, atoms, free radicals, or ions
Dissociation constant
the measure of the extent of dissociation, measured by the dissociation constant K. For the process:
AB = A + B K = ([A][B])/[AB]
Electronegativity
the tendency for atoms in a molecule to attract electrons.
Electronic configuration
the order in which electrons are arranged in an atom or molecule
Electrophile
an atom, molecule, or ion able to accept an electron pair. Electron poor specie/s?) [E.g. H3O+, BF3, AlCl3, Br2, Cl2, I2]
EWG
Electron withdrawing Group
Electrophilic substitution
an overall reaction in which an electrophile binds to a substrate with the expulsion of another electrophile
Electrovalent (ionic) bond
bonding by electrostatic attraction. Formed by transfer of electron/s from one atom to another
Element
a substance which cannot be further subdivided by chemical methods.
Enantiomers
a pair of isomers which are related as mirror images of one another.
Endothermic
a reaction in which heat is absorbed.
Enthalpy
a thermodynamic state function, generally measured in kilojoules per mole. In chemical reactions the enthalpy change (deltaH) is related to changes in the free energy (deltaG) and entropy (deltaS) by the equation: deltaG = deltaH - T.deltaS
Entropy
a thermodynamic quantity which is a measure of the degree of disorder within any system. [The greater the degree of order the higher the _____; for an increase in ______ S is positive.
Epimerization
a process in which the configuration of one chiral center of a compound, containing more than one chiral atom, is inverted to give the opposite configuration.
Equilibrium constant
according to the law of mass action, for any reversible chemical reaction: aA + bB = cC + dD, the equilibrium constant (K)is defined as: K = ([C]c[D]d)/([A]a[B]b)
Excited state
the state of an atom, molecule, or group when it has absorbed energy and becomes excited to a higher energy state as compared to the normal ground state. The excited state may be electronic, vibrational, rotational, etc.
Fischer projection
a convention for drawing carbon chains so that the relative 3-dimensional stereochemistry of the carbon atoms is relatively easy portrayed on a 2-dimensional drawing.
Free energy (deltaG)
a thermodynamic state function; the free energy change (G) in any reaction is related to the enthalpy and entropy: deltaG = deltaH - T.deltaS
Functional group
the atom or group of atoms that defines the structure and at the same time determines the properties of a class or family of organic compounds.
Gauche
a conformational isomer in which the groups are neither eclipsed nor trans to one another.
Ground state
the lowest energy state of an atom, molecule, or ion.
Heat of reaction
the amount of heat absorbed or evolved when specified amounts of compounds react under constant pressure.
Hybridization
the process whereby atomic orbitals of different types but similar energies are combined to form a set of equivalent hybid orbitals which are more stable in directional manner.
Hydrolysis
the addition of the elements of water to a substance, often with the partition of the substance into two parts, such as in the hydrolysis of an ester to an acid and an alcohol.
Ion
an atom or group of atoms that has lost or gained one or more electrons to become a charged species.
Isomers
compounds having the same atomic composition (constitution) but differing in their chemical structure
Mechanism of reaction
refers to the detailed course of an overall reaction, its sequence of steps and the details of electron movement, bond breaking, bond making and timing
bond cleavage
Homolytic cleavage and Heterolytic cleavage
Homolytic cleavage
characterized by homolytic fission of bonds and the formation of free radicals. creates reactive oxygen species /ROS.
Heterolytic cleavage
characterized by heterolytic fission and the formation of charged species.
Fundamental Classification of Organic Reactions
Substitution reactions, Additional reactions, Elimination reactions, Rearrangement reactions, Oxidation, Reduction
Rearrangement reactions
one or more atoms in a molecule move to other positions within that molecule
Elimination reactions
a molecule or stable ion is lost from a structure leaving behind a double
Additional reactions
a reagent reacts with a double or triple bond in a substrate to form a single product.
Substitution reactions
an atom or group is replaced by a different atom or group
ISOMERS
compounds having the same molecular formula but different structural formulas
CONSTITUTIONAL or STRUCTURAL ISOMERS
isomers with different atom to atom bonding sequence. Chain or skeletal
STEREOISOMERS
isomers with the same atom-to-atom bonding sequence but with the atoms arranged differently in space
CONSTITUTIONAL ISOMERS
Chain or Skeletal Isomers, Positional Isomers, Functional Isomers
Chain or Skeletal Isomers
compounds that differ in the arrangement of carbons Example: CH3CH2CH2CH2CH3
Positional Isomers
differ in the position of a non carbon group Example: CH3CH2CH2CH2Br
Functional Isomers
differ in the functional group
Example: CH3CH2CH2CHO
Entropy
has the units of joules per degree K per mole.]
Conjugation
a sequence of alternating double (or triple) and single bonds. [E.g. C=C-C=C and C=C-C=O. It can also be relayed by the participation of lone pairs of electrons or vacant orbitals