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Organic Chem 1 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

Bond Dipole Moment

A

A measure of the polarity of an individual bond in a molecule.

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2
Q

Positive end of the crossed arrow

A

The positive looking end of the crossed arrow corresponds to the less electron negative end of the dipole. This end will have a partial positive charge.

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3
Q

Molecular Dipole Moment

A

The vector sum of the bond dipole moments in a molecule. It is also a measure of the polarity of a molecule.

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4
Q

What are the 3 kinds of attractive forces that cause molecule to associate into solids and liquids?

A
  1. dipole-dipole forces of polar molecules
  2. London dispersion forces that affect all molecules
  3. “Hydrogen bonds” that link molecules having -OH or -NH groups
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5
Q

Dipole-dipole forces

A

Attractive intermolecular forces that result from the attraction of the positive and negative ends of the permanent dipole moments of polar molecules.

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6
Q

London Dispersion Forces

A

These are intermolecular forces that result form the attraction that is formed from a temporary dipole induced in adjacent molecules.

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7
Q

Hydrogen Bond

A

Hydrogen bond occurs when it is being bonded to (O, N, or F). (Organic compounds do not bond with H-F;therefore we are only looking at H-N and H-O bonds).

This is a strong attractive force between a non bonding pair of electrons and an electrophilic (O-H or N-H) hydrogen.

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8
Q

Hydrophobic

A

Non-polar substances or groups that do not readily dissolve in water

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9
Q

Hydrophilic

A

Polar substances that readily dissolve in water; are water attractive

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10
Q

Arrhenius Theory

A

Acids: substances that dissociate in water to give hydronium ions.

Bases: substances that dissociate in water to give hydroxide ions.

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11
Q

Bronsted-Lowry Acids and Bases

A

Acid: is any species that can donate a proton
Base: Any species that can accept a proton

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12
Q

Conjugate acids

A

The acid that results from the protonation of a base

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13
Q

Acid-dissociation constant

A

(Ka)- Is is the equilibrium constant for the reaction of the acid with water to generate H3o+

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14
Q

Organic Acids

A

Most organic acids are weak acids and have a Ka value of less than 10^-4.

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15
Q

PKa equations

A

pKa = -log10Ka

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16
Q

Base Strength Concept

A

For an acid (HA) to be strong its conjugate base (A-) must be stable in its an ionic form because if not then HA would not easily lose its proton. A weak acid has a strong base as its conjugate base pair.

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17
Q

What does equilibrium favor?

A

Equilibrium favors the yield of the weaker acid or base.

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18
Q

Electron negativity

A

A more electronegative elements will obtain a negative charge more easily which which it a more stable conjugate base and a stronger acid.

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19
Q

Electronegative trend

A

Electronegativity increases from left to right in the periodic table.

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20
Q

Electronegativity and atom size

A

The negative charge of the anion is more stable if it’s spread over a larger region of space.

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21
Q

Acidity trend

A

Acidity increase from left to right and going down the periodic table (as atomic size increases).

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22
Q

Inductive effect

A

The magnitude of the inductive effect depends on the number of bonds between the electronegative elements

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23
Q

Lewis Bases

A

Species with available electrons that can be donated to form new bonds

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24
Q

Lewis Acids

A

Species that can accept electron pairs to form new bonds

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25
Electrophile
A Lewis acid that accepts a pair of electrons
26
Nucleophile
A Lewis base that donates electrons to a nucleus with an empty orbital.
27
Hydrocarbons
Compounds composed entirely of carbon and hydrogen. The major classes of hydrocarbons are alkanes, alkenes, alkynes, and aromatic hydrocarbons.
28
Alkanes
Hydrocarbons that contain a single bond. Generally has the -ane suffix.
29
Methane
CH4
30
Ethane
CH3-CH3 (2 carbons)
31
Propane
CH3-CH2-CH3 (Has 3 carbons)
32
Butane
CH3-CH2-CH2-CH3 (Has 4 carbons)
33
Pentane
5 carbons
34
Hexane
6 Carbons
35
Heptane
7 Carbons
36
Octane
8 carbons
37
Nonane
9 carbons
38
Decane
10 carbons
39
Cycloalkanes
These are a class of alkanes that are in the form of a ring.
40
Characteristics of alkanes
Alkanes mainly undergo combustion rxns and are major components of heating gases such as gasoline, jet fuel, diesel fuel, motor oil, fuel oil, and paraffin (wax). Other than combustion rxns, alkanes re not very reactive because they do not have a functional group.
41
Functional Groups
The part of a molecule where reactions typically occur. They are distinct chemical units such as double bonds, hydroxy groups, or halogen atoms that are really reactive.
42
Alkyl Group
An alkane portion of a molecule with one hydrogen atom removed.
43
Alkenes
Contain carbon-carbon double bonds. This c-c double bond is the most reactive park of an alkene. The double bond in this alkene is the functional group.
44
Naming alkenes
When the double bonds can be in more than one position, the chain is numbered and the lower number of the two double-bonded carbons is added to the name.
45
(Trans) in alkenes
In a large ring, a trans double bonds might occur which gives it the name trans-cycloalkene.
46
Alkynes
Carbon-carbon triple bonds as their functional groups. The triple bond here is linear so there is no geometric isomerism in alkynes.
47
Aromatic hydrocarbon (aka Arenes)
All derivatives of benzene and are six members ring with three double bonds.
48
Functional Groups with Oxygen
The major classes of oxygen containing compounds are alcohols, ethers, ketones, aldehydes, carboxylic acids, and acid derivatives.
49
Alcohols
Organic compounds that contain the hydroxy (-OH) group as their functional group. R-OH
50
Characteristics of alcohols
Are very polar organic compounds because the hydroxy group is strongly polar and can participate in hydrogen bonding.
51
Ethers
Composed of two alkyl groups bonded to an oxygen atom. Its formula is R-O-R’.
52
R’ in an alkyl group
Represents another alkyl group either the same as or different than the first one.
53
Characteristics of ethers
More polar than hydrocarbons, but cannot bond to hydrogen by themselves because they do not have an O-H bond.
54
Carbonyl Group
C=O functional group for aldehydes and ketones
55
Ketone
Two alkyl groups bonded to the carbonyl group
56
Aldehyde
One alkyl group and a hydrogen atom bonded to the carbonyl group.
57
Characteristics of carbonyl groups
This is a strongly polar group
58
Carboxylic acids
Contain the carboxyl group (-COOH) as their functional group. The general formula for a carboxylic acid is R-COOH.
59
Carboxyl group
A combination of the carbonyl group and a hydroxy group.
60
Characteristics of Carboxylic Acids
Strongly polar and its strongly hydrophilic carboxyl group enhances their solubility in water.
61
Acid chlorides
An acid derivative with a chlorine atom in place of the hydroxy group.
62
Esters
Acid derivative where the hydroxy group of the acid is replaced by an alkoxy group. An ester is a composite of a carboxylic acid and an alcohol.
63
Amide
An acid derivative where the hydroxy group of the acid is replaces by a nitrogen atom and its attached hydrogens or alkyl groups. An amide is a composite of a carboxylic acid and an amine.
64
Common nitrogenous compounds
These are amines, amides, and nitriles. Nitrogen is an element often fond in the functional group of organic compounds.
65
Amines
A derivative of ammonia with one or more alkyl or aryl groups bonded to the nitrogen atom.
66
Amides
Acid derivatives that result from a combination of an acid with ammonia or an amine. Proteins have the structure of long-chain complex amides.
67
Characteristics of Amides
These are the most stable acid derivatives. They have strong hydrogen bonds that gives them high melting points and high boiling points.
68
Nitrile
A compound containing a cyano group (-C triple bond N)
69
Cyano group
Is a functional group that has Carbon triple bonded to Nitrogen.

Organic Chem 1 (4 decks)

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