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Organic Chemistry 1 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

A molecular compound containing only carbon and hydrogen atoms

A

Hydrocarbon

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2
Q

Hydrocarbons having only single (σ) bonds between carbon atoms; the general formula is CnH2n+2

A

Alkanes

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3
Q

Hydrocarbons having at least one double bond between carbon atoms; the general formula for monocyclic alkenes is CnH2n-2 and the general formula for acyclic alkenes is CnH2n

A

Alkenes

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4
Q

Hydrocarbons having at least one triple bond between carbon atoms; the general formula for acyclic aklynes is CnH2n-2 and the general formula for monocyclic alkenes is CnH2n+4

A

Alkynes

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5
Q

A cyclic conjugated unsaturated molecule or ion that is stabilized by π electron delocalization

A

Aromatic compounds

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6
Q

A compound that doesn’t contain any multiple bonds

A

Saturated compound

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7
Q

A compound that contains one or more multiple bonds

A

Unsaturated compound

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8
Q

The prototypical aromatic compound having the formula C6H6

A

Benzene

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9
Q

A structure in which lines are used to represent bonds

A

Kekulé structure

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10
Q

A covalent bond in which the electrons are not shared equally because of differing electronegativities of the bonded atoms

A

Polar covalent bond

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11
Q

A measure of the ability of an atom to attract electrons it is sharing with another and thereby polarize the bond

A

Electronegativity

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12
Q

A physical property associated with a polar molecule that can be measured experimentally

A

Dipole moment (µ)

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13
Q

The unit in which dipole moments are stated; 1 D = 1x10^-18 esucm

A

Debye (D)

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14
Q

The particular group of atoms in a molecule that primarily determines how the molecule reacts

A

Functional group

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15
Q

Atoms such as oxygen, nitrogen, sulfur, and the halogens that form bonds to carbon and have unshared pairs of electrons

A

Hereroatom

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16
Q

A molecule with a dipole moment

A

Polar molecule

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17
Q

The particular group of atoms in a molecule that primarily determines how the molecule reacts

A

Functional group

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18
Q

The designation given to a fragment of a molecule hypothetically derived from an alkane by removing a hydrogen atom; these group names end in “yl”

A

Alkyl group

19
Q

Compounds in which a halogen atom (fluorine, chlorine, bromine, or iodine) replaces a hydrogen atom of an alkane

A

Alkyl halides or haloalkanes

20
Q

A carbon that has one other carbon attached to it

A

Primary carbon atom

21
Q

A carbon atom that has two other carbon atoms attached to it

A

Secondary carbon atom

22
Q

A carbon atom that has three other carbon atoms attached to it

A

Tertiary carbon atom

23
Q

An organic halide in which the halogen atom is bonded to an alkene carbon

A

Alkenyl halides

24
Q

An organic halide in which the halogen atom is attached to an aromatic ring, such as a benzene ring

A

Aryl halide

25
Q

A hydroxyl group attached to a carbon that only has one other carbon attached to it

A

Primary alcohol

26
Q

A hydroxyl group attached to a carbon that is attached to two other carbon atoms

A

Secondary alcohol

27
Q

A hydroxyl group attached to a carbon that is attached to three other carbon atoms

A

Tertiary alcohol

28
Q

When a hydroxyl group is connected to a benzene ring

A

A phenol group

29
Q

A group where a carbon atom has a double bond to oxygen

A

Carbonyl group

30
Q

Properties of a substance, such as melting point and boiling point, that relate to physical (as opposed to chemical) changes in the substance

A

Physical property

31
Q

The temperature at which an equilibrium exists between a well-ordered crystalline substance and the more random liquid state; reflects the energy needed to overcome the attractive forces between the units (ions, molecules) that comprise the crystal lattice

A

Melting point

32
Q

Strong electrostatic forces of attraction between ions of opposite charges; these forces hold ions together in a crystal lattice

A

Ion-ion forces

33
Q

The temperature at which the vapor pressure of a liquid is equal to the pressure above the surface of the liquid

A

Boiling point

34
Q

Forces that act between molecules because of permanent (or temporary) electron distributions; can be attractive or repulsive; includes dipole-dipole forces (including hydrogen bonds) and dispersion forces (also called London forces)

A

Intermolecular forces (van der Waals forces)

35
Q

An interaction between molecules having permanent dipole moments

A

Dipole-dipole force

36
Q

A strong dipole-dipole interaction that occurs between hydrogen atoms bonded to small strongly electronegative atoms (O, N, or F) and the non bonding electron pairs on other such electronegative atoms

A

Hydrogen bond

37
Q

Weak forces that act between non polar molecules or between parts of the same molecule. Bringing two groups (or molecules) together first results in an attractive force between them because a temporary unsymmetrical distribution of electrons in one group induces an opposite polarity in the other. When groups are brought closer than their van der Waals radii, the force between them becomes repulsive because their electron clouds begin to inter penetrate each other

A

Dispersion force (London force)

38
Q

The extent to which a given solute dissolves in a given solvent, usually expressed as a weight per unit volume

A

Solubility

39
Q

A non polar group that avoids an aqueous surrounding and seeks a non polar environment

A

Hydrophobic group

40
Q

A polar group that seeks an aqueous environment

A

Hydrophilic group

41
Q

A type of optical spectroscopy that measures the absorption of infrared radiation; provides structural information about functional groups present in the compound being analyzed

A

Infrared (IR) spectroscopy

42
Q

A way to express the frequency of a wave; the number of waves per centimeter, expressed as cm^-1

A

Wave number (v)

43
Q

The distance between consecutive crests (or troughs) of a wave

A

Wavelength (λ)

44
Q

The number of full cycles of a wave that pass a given point in each second

A

Frequency (v)

Organic Chemistry 1 (10 decks)

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