Organic Chemistry Flashcard

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Aliphatic
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Term applied to compounds that do not contain benzene or benzene-like rings as structural units.
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Aromatic
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An electron-delocalized species that is much more stable than any structure written for it in which all the electrons are localized either in covalent bonds or as unshared electron pairs.
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Alkanes
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Hydrocarbon in which all the bonds are single bonds. These have the general formula CnH(2n+2)
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Alkenes
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Hydrocarbon that contains a carbon-carbon double bond (C=C); also known by the older name olefin.
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Alkynes
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Hydrocarbon that contains a carbon-carbon triple bond.
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Valence bond model
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bases the connection between two atoms on the overlap between half-filled orbitals of the two atoms
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Molecular orbital model
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assembles a set of molecular orbitals by combining the atomic orbitals of all of the atoms in the molecule
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Sigma bond
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a bond along the internuclear axis
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Bonding orbital

Nonbonding orbital
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lower energy, sigma or pi

higher energy, sigma* or pi*
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Methane
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simplest alkane, most abundant
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Ethane
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second most abundant alkane
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Propane
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third most abundant alkane
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sp3 hybridization
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A model to describe the bonding of a carbon attached to four other atoms or groups. The carbon 2s orbital and the three 2p orbitals having 25% s character and 75% p character. These orbitals are directed toward the corners of a tetrahedron.
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Methyl
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CH3
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n-butane
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"normal" therefore unbranched, isomer of C4H10
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isobutane
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isomer of C4H10, has a branched chain
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Methylene groups

Methine groups
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CH2

CH
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n-Alkanes
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"normal" alkanes, unbranched
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n-Pentane
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has a chain 5 carbons
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n-Hexane
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has a chain of 6 carbons
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Homologous series
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Group of structurally related substances in which successive members differ by a CH2 group.
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Primary carbon
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A carbon that is attached to only one other carbon.
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Secondary carbon
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A carbon that is directly attached to two other carbons.
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Tertiary
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A carbon that is directly attached to three other carbons.
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Quarternary
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A carbon that is directly bonded to four other carbons
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Cracking
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A key step in petroleum refining in which high-molecular-weight hydrocarbons are converted to lower molecular-weight ones by thermal or catalytic carbon-carbon bond cleavage.
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Reforming
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Step in oil refining in which the proportion of aromatic and branched-chain hydrocarbons in petroleum is inceased so as to improve the octane rating of gasoline.
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Intermolecular attractive forces
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Forces between two atoms or groups in SEPARATE molecules.
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van der Waals forces
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Intermolecular forces that do no involve ions (dipole-dipole, dipole/induced dipole, and induced dipole/induced dipole forces)
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Induced dipole
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Force of attraction resulting from a mutual and complementary polarization of one molecule by another. Also referred to as London forces or dispersion forces.
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van der Waals radius
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A measure of the effective size of an atom or a group. The repulsive forces between two atoms increases rapidly when they approach each other at distances less than the sum of their van der Waals radii.
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Hydrophobic effect
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Exclusion of nonpolar molecules from water (like dissolves in like)
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Parrafin hydrocarbons
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An old name for alkanes and cycloalkanes
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Combustion
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Burning of a substance in the presence of oxygen. All hydrocarbons yield carbon dioxide and water when they undergo combustion,
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Heat of combustion
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Heat evolved on combustion of a substance. It is the value of -deltaH for the combustion reaction.
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Enthalpy
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The heat content of a substance; H.
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Potential energy
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The energy a system has exclusive of its kinetic energy.
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Intramolecular forces
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Forces between two atoms or groups WITHIN the same molecule.
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Oxidation number
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The formal charge an atom has when the atoms in its covalent bonds are assigned to the more electronegative partner.
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sp2 hybridization
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A model to describe the bonding of a carbon attached to three other atoms or groups. The carbon 2s orbital and the two 2p orbitals are combined to give a set of three equivalent _____ orbitals having 33.3% s character and 66.7% p character. One p orbital remains unhybridized. A trigonal planar geometry is characteristic of _____ hybridization.
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Pi bond
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The bond between the left over unhybridized p orbital on carbon; above and below the internuclear axis; in double and triple bonds.
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Pi electrons
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Probability of their location is highest above and below the internuclear axis
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sp hybridization
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Hybridization state adopted by carbon when it bonds to two other atoms as, for example, in alkynes. The s orbital and one of the 2p orbitals mix to form two equivalent ____-hybridized orbitals. A linear geometry is characteristic of ____ hybridization.
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1 carbon
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methane
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2 carbons
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Ethane
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2 carbons
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Ethane
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5 carbons
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pentane
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3 carbons
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propane
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4 carbons
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butane
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6 carbons
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hexane
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7 carbons
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heptane
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8 carbons
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octane
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9 carbons
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nonane
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10 carbons
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decane
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10 carbons
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decane
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11 carbons
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undecane
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12 carbons
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dodecane
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13 carbons
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tridecane
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14 carbons
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tetradecane
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15 carbons
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pentadecane
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16 carbons
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hexadecane
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17 carbons
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heptadecane
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18 carbons
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octadecane
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19 carbons
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nonadecane
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20 carbons
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icosane
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21 carbons
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henicosane
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22 carbons
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docosane
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23 carbons
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tricosane
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24 carbons
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tetracosane
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30 carbons
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triacontane
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31 carbons
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hentriacontane
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32 carbons
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dotriacontane
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40 carbons
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tetracontane
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50 carbons
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pentacontane
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100 carbons
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hectane
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