Chem 302 Organic Chemistry Intro

# carbons in meth-

1 carbon

# carbons in ethane

2 carbons

# carbons in propane

3 carbons

# carbons in butane

4 carbons

# carbons in pentane

5 carbons

# carbons in hexane

6 carbons

# carbons in heptane

7 carbons

functional groups

reactive parts of a molecule that undergo the same chemical reaction regardless of position

alkene

organic compound with a double bond

alkyne

organic compound with a triple bond

alcohol

R-OH (-ol)

aldehyde

R-C=O-H

ketone

R-C=O-R

carboxylic acid

R-COOH

ether

R-O-R

ester

R-C=O-O-R (-oate)

amide

R-C=O-N-R-R

amine

R-NR

Addition

Addition of adjacent atoms to a molecule--seen in organic
polymer reactions. Has a double in the beginning that turns into a single bond

Elimination

Removal of adjacent atoms from a molecule. carboxylic acid + amide = amide linkage

Substitution

atom or group of atoms are replaced by another

Rearrangement

An atom or group of atoms move to different carbons.

Carboxylic acids combine with hydrocarbons to make …

fatty acids

Monosaccharides combine to make polysaccharides to form …

carbohydrates

amino acids make polypeptides that make …

proteins

The monomers (basic building blocks) form
polymers through …

dehydration synthesis (water is eliminated).

Polysaccharides (polymerized sugars) are
formed from what kind of bonds?

ether

polystyrene

addition reaction

polyurethane

addition reaction

polypropylene

addition reaction

polyvinylchloride

addition reaction

polyethylene terephthalate (PET)

condensation polymerization reaction

polyamide (PA)

condensation polymerization reaction

polyethylene

addition reaction

Collision theory is based on …

kinetic molecular theory of gas

Ek = ½ kT = ½ mv2

A collision must occur for the reaction to happen

doesn’t explain first order decay.

Collision must be effective which requires

1) sufficient energy (high enough temp)

2) correct orientation of collision

The rate of reaction is concentration dependent

Kinetic Theory – Transition State

Most easily depicted on a reaction profile of E vs. t

Based on energy not collisions

Kinetic Theory – Transition State

In this profile, that has been used in thermo, an energy hill, called the activation barrier, rises, positively above the thermodynamic profile.

This barrier is what spontaneous - ΔG (-) – processes don’t happen (like combustion)

The top of the activation barrier is the “transition state” or
“activated complex.”

It is theoretical. It is not an intermediate.

At top of energy hill, a transition state is equally likely to fall to

the left or the right

Combined Arrhenius

Looks like Van’t Hoff and Clausius Clapeyron

Ea Always (+) so T increasing means k increases

k = Ae-Ea/RT

Give [ ] vs t at 2 temperatures yields x, k, A, Ea, data

The pre-exponential factor provides a measure of the frequency of collisions and therefore is larger for gases

Combined Arrhenius

The activation energy term describes an endothermic process

Combined Arrhenius

Because the temperature term is the denominator of the
exponent term, as temperature increases, the rate constant
increases

Combined Arrhenius

Structural Isomers

Due to the flexible nature of carbon bonding, the same chemical formula can exist in many different forms

carbohydrates

functional groups before polymerization - 2 alcohols

functional group after polymerization - ether sugars

monosaccharides make up the polymer

protein

functional groups before polymerization - carboxylic acid + amine

functional group after polymerization - amide

amino acid make up the polymer

lipids

functional groups before polymerization - carboxylic acid + alcohol

functional group after polymerization - ester

glycerol make up the polymer

bond energies

IMF - 10^0 to 10^1 kJ/mole

Covalent bonds: 10^2 to 10^3 kJ/mole

Nuclear reactions (fission and fusion): 10^9 to
10^10 kJ/mole

Hydrogen > Ion-dipole> ionic> nuclear

nuclear fusion and fisson are both

exothermic

Transiton states can have more (can’t be less) energy than the prior species.

tetrahedral

4 areas of electron density: 4 bonds, 0 lone pairs

Trigonal pyramidal

4 areas of electron density: 3 bonds, 1 lone pair

Bent

4 areas of electron density 2 bonds, 2 lone pairs

Trigonal planar

3 area of electron density, 3 bonds, 0 lone pairs

Linear

2 areas of electron density, 2 bonds, 0 lone pairs

Nonpolar covalent bonds

< 0.5

Polar covalent bonds

0.5-1.9

Ionic bond

>1.9

Enantiomers

Isomers

Diastereomers