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Definition
hydrocarbons containing carbon and hydrogen joined together in straight chains, branched trains or non-aromatic rings
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Definition
| hydrocarbons that contain only single bonds |
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Definition
| hydrocarbons that contain carbon-carbon double bonds |
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| substiuents derived from alkanes |
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Definition
| hydrocarbons that contain carbon-carbon triple bonds |
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Definition
| compound that can act as either an acid or a base |
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Term
| angular momentum quantum number |
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Definition
| s, p, d, f orbitals and so on (=principal qn -1) |
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Definition
| conformation in which the dihedral angle is 180 |
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Definition
| two bonds that have a dihedral relationship of 180 |
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Term
| antibonding molecular orbital |
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Definition
| a region in which the wave is zero; electrons in [] decreaase bonding becae the region between the nuclei contains no electron density |
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Term
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Definition
| description of the wave properties of an electron in an atom; the allowed state of an electron |
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Definition
| electrons are placed one by one into orbitals of lowest energy in a manner consistent with the Pauli exclusion principle and Hund's rule |
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Definition
| temperature at which the vapor pressure of a substance equals atompheric pressure |
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Definition
| the angle between each pair of bonds to the same atom |
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Definition
| a polar bond's associated dipole moment contribution |
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Definition
| direct measure of bond strength |
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Definition
| distance between centers of the bonded nuclei |
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Definition
| describes the number of covalent bonds shared by two atoms |
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Term
| bonding molecular orbital |
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Definition
| continuous orbital that includes the region between the two nuclei; electrons in [] are attracted to both cuclei simultaneously |
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Definition
| species that donates a proton in a chemical reaction |
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Term
| Bronsted acid-base reaction |
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Definition
| electron-pair displacement reaction on a hydrogen |
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Definition
| species that accepts a proton in a chemical reaction |
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Definition
| rapid reaction with oxygen to give carbon dioxide and water, initiated by a suitable heat source |
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Definition
| compounds that contain the same functional group |
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| condensed structural fomula |
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Definition
| simpler structural representation of a molecule in which it is assumed that the hydrogens are connected |
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Term
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Definition
| the spatial arrangement of its atoms when all of its dihedral angles are specified |
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Term
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Definition
| investigation of molecular conformations and their relative energies |
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Term
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Definition
| formed when a Bronsted base gains a proton |
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Term
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Definition
| results when a Bronsted acid loses a proton or Bronsted base gains a proton |
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Definition
| results when a Bronsted acid loses a proton |
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Term
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Definition
| order in which an molecule's atoms are connected |
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Term
| constitutional isomers (structural isomers) |
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Definition
| isomers taht differ in the connectivity of their atoms |
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Term
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Definition
| nonionic compound which consists of an electron pair that is shared between bonded atoms |
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Term
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Definition
| symbolic device for keeping track of electron pairs in chemical reactions; "flow" of electrons from the electron donor to the electron acceptor |
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Definition
| no matter how the molcule turns about a line joing two nuclei, its electron density looks the same |
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Term
| dihedral angle (torsion angle) |
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Definition
| angle between two planes of a molecule |
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Term
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Definition
| unevent electron distiburtion in a comound containing covalent bonds |
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Definition
| bond consisting of two electron pairs |
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Definition
| the groups along a Newman projection are superimposed |
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Term
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Definition
| energye required to transfer an electron to a bonded atom in the breaking of that bond |
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Term
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Definition
| the magnetic property of the elctron; only two values possible (up +1/2 or down -1/2); fourth quantum number |
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| electron-deficient compounds |
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Definition
| atoms that are short of an octet by one or more electron pairs |
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Definition
| groups that do NOT pull electrons toward themselves and away from the carbon to which they are attached |
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Term
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Definition
| the more an tom attracts elctrons, more [] it is |
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Definition
| tendency of an atom to attract electrons to itself in a covalent bond |
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Term
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Definition
| the way an atom's electrons are distributed among their atomic orbitals |
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Term
| electron-pair displacement reaction |
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Definition
| reaction in which one electron pair is displaced from an atom by the donation of another elctron pair from another atom |
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| electron-withdrawing polar effect |
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Definition
| polar effect of halogens and other elctronegative groups; they pull electrons toward themselves and away from the carbon to which they are attached |
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Definition
| atom that receives a pair of electrons from the Lewis base |
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Definition
| stabilizing interaction between opposite charges |
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| electrostatic potential map |
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Definition
| illustrates the charge distributions of molecules three dimensionally |
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Definition
| effect of changing the directly attached atom (A) on the acidity of H-A |
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Term
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Definition
| assigned charge on each atom |
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Definition
| mixture of compounds is slowly boiled; the vapor is collected, cooled, and recondensed to a liquid |
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Definition
| characteristically bonded group of atoms that has about the same chemical reactivity whenever it occurs in a variety of compounds |
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Definition
| two bonds with dihedral relationship of 60 |
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Term
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Definition
| conformation with dihedral angles of 60 and 300 |
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Term
| Heisenberg uncertainty principle |
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Definition
| the accuracy with which we can determine the position and velocity of a particle is inherently limited |
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Definition
| series of compounds that fdiffere by the addition of methylene groups |
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Term
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Definition
| first, to distribute electrons among identical orbitals of equal energy, single elctrons are placed into separate orbitals before the orbitals are filled; second, the spins of these unpaired elctrons are the same |
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Definition
| new orbitals formed by hybridization |
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Term
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Definition
| process in which atomic orbitals convert to molecular orbitals |
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Term
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Definition
| when a second molecules is located nearby, its electron cloud distorts to form a complementary dipole |
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Definition
| one conformation converting to another relative to others about the carbon-carbon bond |
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Definition
| electrostatic attraction that holds ions together |
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Definition
| chemical compound in whitch the component atoms exist as ions |
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Definition
| energy required for the loss of an electron from the bonded atom |
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| isomers (isomeric compounds) |
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Definition
| different compounds that have the same molecular formula |
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Definition
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Definition
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Definition
| one of its atoms accepts an electron pair from a break bond (takes a pair of bonding elctrons and runs) |
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Term
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Definition
| species that accepts an electron pair to form a new bond in a chemical reaction |
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Term
| Lewis acid-base association |
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Definition
electron-deficient Lewis acid and a Lewis base combine to give a single product
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Term
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Definition
| species that donates the electron paire to a Lewis acid to form a new bond |
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Term
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Definition
| molecular structures that use the Lewis dot notation for the electron pair bond |
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Term
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Definition
| molecular geometry for an atom with two surrounding groups (angle = 180) |
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Definition
| (=+/- angular momentum qn) |
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Definition
| the temperature at which a substance is transformed spontaneously and completely from the solid to liquid state |
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Definition
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Definition
| gives its atomic composition |
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Definition
| specification of how far apart the atoms are and how they are situated in space |
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Definition
| commercially available scale models from which you can construct simple organic molecules |
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Definition
| orbitals for the entire molecule |
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Definition
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Definition
| type of planar projection along one bond |
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Term
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Definition
| point, or a surface in 3D, at which the wave is zero |
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| normal alkanes (n-alkanes) |
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Definition
| alkanes with unbranched carbon chains |
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Term
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Definition
| Lewis base that donates an electron pair to an atom otehr than hydrogen |
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Term
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Definition
| tendency of atoms to gain or lose valence electrons to form ions with noble-gas configuartion |
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Term
| orbital interaction diagram |
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Definition
| plot of orbital energy versus the postion of the two interacting nuclei |
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Term
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Definition
| branch of science that deals generally with compounds of carbon |
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| Pauli exclusion principle |
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Definition
| no two electrons may have all four quantum numbers the same |
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Definition
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Definition
| bond in which electrons are shared unevenly |
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| polar effect (inductive effect) |
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Definition
| effect on chemical properties caused by the interaction between charges, dipols, or both |
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Term
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Definition
| molecules that have permanent dipole moments |
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Term
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Definition
| longest continuous carbon chain in the molecule |
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Definition
| number associated with the valence shell (counted out from the nuclei in increasing energy) |
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Term
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Definition
| in the mathematics of "electron waves" each orbital has an [] |
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Term
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Definition
| representation of a molecule using several structures to demonstrate the "true" form |
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Definition
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Term
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Definition
| bonds in which the electron density is cylindrically symmetrical about the internuclear axis |
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Term
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Definition
| structure-drawing convention that only shows the carbon-carbon bonds |
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Term
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Definition
| bond of one group bisects the angle between two other groups down a Newman projection |
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Term
| standard free energy of dissociation |
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Definition
| deltaG = -RTln(Ka) = -2.3RTlog(Ka) |
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Term
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Definition
| a molecule's Lewis structure, which shows its connectivity of its atoms |
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Term
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Definition
| know [] of a molecule when we know its atomic connectivity and molecular geometry |
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Term
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Definition
| branching groups on hydrocarbons |
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| substitutive nomenclature |
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Definition
| mostly widely applied nomenclature system in use today |
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Definition
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Definition
| 3D object with four triangular faces (angle = 109.5) |
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Definition
| probability of finding electrons in the region of a molecule |
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Definition
| molcular geometry for an atom with three surrounding groups (angle =120) |
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Definition
| molecular geometry for an atom with three surrounding groups and an unshared pair |
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Definition
| bond involving three electron pairs |
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Term
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Definition
| unshared valence electrons in Lewis structures are depicted as paired dots |
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Definition
| electrons in the outer most shell of an atom |
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Definition
| the orbitals of an atom that contain the valence electrons |
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Term
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Definition
| outermost shell of electrons in an atom |
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| van der Waals attractin (dispersion interaction) |
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Definition
| attraction between temporary dipoles |
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Definition
| measure of an atom's effective size |
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Definition
| extra energy required to force two nonbonded atoms within the sum of their van der Waals radii |
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Term
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Definition
| bonds and electrons are arranged about a central atom so that the bonds are as far apart as possible |
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Term
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Definition
| atomic orbital described in physics by this mathematical function |
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Term
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Definition
| sum of all shared and unshared valence electrons around each atom in many stable covalent compounds is eight (two for the hydrogen atom) |
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Term
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Definition
| the less an atom attracts electrons, the more [] it is |
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Definition
| repulsion between electrons in bonds that effects the energy of conformations and effects the bond angles of molecules |
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| Lewis acid-base dissociation |
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Definition
single molecule reacts to form a Lewis acid and Lewis base; reverse of Lewis acid-base association
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