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Pre-Pharm > Organic 2: Alkanes & Cycloalkanes - Intro to Hydrocarbons > Flashcards

Organic 2: Alkanes & Cycloalkanes - Intro to Hydrocarbons Flashcards

1
Q

Hydrocarbons

A

2 classes - alliphatic & aromatic

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2
Q

Alkanes

A

hydrocarbons in which all the bonds are single bonds; general formula = CnH2n+2

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3
Q

Alkenes

A

hydrocarbons with at least one carbon-carbon double bond

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4
Q

Alkynes

A

hydrocarbons with at least one carbon-carbon triple bond

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5
Q

Arenes

A

another name for aromatic hydrocarbons

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6
Q

Benzene

A

most important aromatic hydrocarbon

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7
Q

Constructive interference

A

occurs when 2 waves combine so as to reinforce each other (in phase)

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8
Q

Destructive interference

A

occurs when 2 waves oppose each other (out of phase)

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9
Q

Valence Bond Model

A

bases the connection between 2 atoms on the overlap between half-filled orbitals of the 2 atoms; pictures a covalent bond between 2 atoms in terms of an in-phase overlap of a half-filled orbital of 1 atom with a half-filled orbital of the other

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10
Q

Molecular Orbital Model

A

assembles a set of molecular orbitals by combining the atomic orbitals of all of the atoms in the molecule; rests on the notion that, as electrons in atoms occupy atomic orbitals, electrons in molecules occupy molecular orbitals

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11
Q

Sigma bond

A

a bond in which the orbitals overlap along a line connecting the atoms (the internuclear axis); electron distribution is cylindrically symmetrical

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12
Q

Linear Combination of Atomic Orbitals-Molecular Orbital Method (LCAO-MO)

A

representing molecular orbitals as combinations of atomic orbitals

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13
Q

Bonding Orbital

A

the additive combination (of 2 wave functions)

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14
Q

Antibonding Orbital

A

the subtractive combination (of 2 wave functions)

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15
Q

Alkane Boiling Point Rule

A

as the number of carbon atoms increases, so does the boiling point

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16
Q

Sp3 hybrid orbitals

A

4 new orbitals coming from 1 s orbital and 3 p orbitals

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17
Q

Methyl groups

A

the group -CH3

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18
Q

n-butane

A

four carbons are joined in a continuous chain; n = normal (carbon chain is unbranched)

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19
Q

Isobutane

A

common name for 2-methylpropane (CH3)3CH; 2nd isomer - has a branched carbon chain

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20
Q

Methylene

A

-CH2 group

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21
Q

Methine

A

-CH group

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22
Q

Homologous series

A

series in which successive members differ by a -CH2- group

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23
Q

IUPAC rules

A

International Union of Pure and Applied Chemistry; alkane names form the foundation of the system

24
Q

Common names

A

names not derived from a set of rules

25
Q

Systematic names

A

names derived according to a prescribed set of rules

26
Q

Preferred IUPAC Name (PIN)

A

2004 IUPAC recommendations established this concept suitable for use in formal communications (patents, international commerce, occupational health/safety, environmental regulation, etc); distinguished from “general” IUPAC names

27
Q

Generic drug names

A

not derived from systematic nomenclature; US Adopted Names Council (USAN), a private organization founded by the American Medical Association, the American Pharmacists Association, and the US Pharmacopeial Convention; International Proprietary Names (INN) are designated by the World Health Organization

28
Q

Locants

A

in IUPAC nomenclature, a prefix that designates the atom that is associated with a particular structural unit; most often a number; structural unit is usually an attached substituent as in 2-chlorobutane

29
Q

Alkyl group

A

lacks one of the hydrogens of an alkane

30
Q

Primary carbon

A

a carbon directly attached to one other carbon

31
Q

Secondary carbon

A

a carbon directly attached to 2 other carbons

32
Q

Tertiary carbon

A

a carbon directly attached to 3 other carbons

33
Q

Quaternary carbon

A

a carbon directly attached to 4 other carbons

34
Q

Cycloalkanes

A

alkanes that contain a ring of 3 or more carbons

35
Q

Refining

A

conversion of crude oil to useful materials, especially gasoline

36
Q

Cracking

A

increases the proportions of hydrocarbons at the expense of higher-molecular-weight ones by processes that involve the cleavage of carbon-carbon bonds induced by head (thermal ____) or with the aid of certain catalysts (catalytic ____)

37
Q

Reforming

A

converts the hydrocarbons in petroleum to aromatic hydrocarbons and highly branched alkanes, both of which show less tendency for knocking than unbranched alkanes and cycloalkanes

38
Q

Intermolecular attractive forces

A

forces, either attractive or repulsive, between 2 atoms or groups in separate molecules; greater in the liquid than in the gas phase

39
Q

van der Waals forces

A

intermolecular forces that do not involve ions (dipole-dipole, dipole/induced-dipole, and induced-dipole/induced-dipole forces)

40
Q

Induced-dipole/induced-dipole attractive force

A

force of attraction resulting from a mutual and complementary polarization of one molecule by another; also referred to as London forces or dispersion forces

41
Q

van der Waals radius

A

distance of closest approach characteristic

42
Q

Hydrophobic effect

A

the exclusion of nonpolar molecules, such as alkanes, from water

43
Q

Paraffin hydrocarbons

A

older name for alkanes; “with little affinity” - testifies to the low level of reactivity of alkanes

44
Q

Combustion

A

burning in air is the best known and most important example of alkanes participating in redox reactions; exothermic, gives CO2 and H20 as products

45
Q

Heat of combustion

A

heat released on combustion of a substance

46
Q

Enthalpy

A

heat content of a compound in its standard state

47
Q

Heat of formation

A

enthalpy change for formation of 1 mole of a compound directly from its elements; 1 type of heat of reaction

48
Q

Potential energy

A

comparable with enthalpy; it is the energy a molecule has exclusive of its kinetic energy; a molecule with more of this is less stable than an isomer with less of this

49
Q

Intramolecular forces

A

forces, either attractive or repulsive, between 2 atoms or groups within the same molecule

50
Q

Oxidation-reduction

A

a reaction in which an electron is transferred from 1 atom to another so that each atom undergoes a change in oxidation number

51
Q

Oxidation number (oxidation state)

A

the formal charge an atom has when the atoms in its covalent bonds are assigned to the more electronegative partner

52
Q

Sp2 hybrid orbitals

A

mixing the 2s orbital with 2 of the 2p orbitals; 1 of the 2p orbitals is left unhybridized

53
Q

Pi bond

A

a bond in which the electron distribution is concentrated above and below the internuclear axis, rather than along it as in a sigma bond; most often associated with a side-by-side overlap of p orbitals on adjacent atoms that are already connected by a sigma bond

54
Q

Pi electrons

A

electrons in a pi bond; probability of finding one of these is highest in the region above and below the plane of the molecule

55
Q

sp hybridization

A

applies when carbon is directly bonded to 2 atoms (ex. acetylene)

Pre-Pharm (182 decks)

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