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 |
