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Experiment 1:
STRUCTURE, INTERMOLECULAR FORCES AND SOLUBILITY
OBJECTIVES
To learn how to identify which intermolecular forces exist between organic compounds.
To investigate the relationship between structure, intermolecular forces and solubility using solubility testing.
ROLE OF INTER- AND INTRAMOLECULAR FORCES
Physical state solid, liquid & gas
Distillation difference in BP
Extraction difference in solubility
Chromatography different IMF between analyte and stationary vs. mobile
phase
Biology secondary structure of proteins DNA and DNA-RNA base pairing
TYPES OF INTERMOLECULAR FORCES
London Dispersion Forces
Dipole-Dipole Forces
Hydrogen Bonding Acceptors Donors
Ion-dipole Forces
LONDON DISPERSION FORCES The London dispersion force is the weakest
intermolecular force.
It is a temporary attractive force that results when the electrons in two neighboring atoms occupy positions that make the atoms form temporary dipoles.
Since electrons are constantly in motion, they can be distributed unevenly about the nucleus. This results in the formation of a temporary dipole.
A second atom or molecule, in turn, can be distorted by the appearance of the dipole in the first atom or molecule (because electrons repel one another) which leads to an electrostatic attraction between the two atoms or molecules.
+ - --------------- +
LONDON DISPERSION FORCES
Dispersion forces are present between all molecules, whether they are polar or nonpolar.
Larger and heavier atoms and molecules exhibit stronger dispersion forces than smaller and lighter
ones.
Compounds which contain carbons and hydrogens ONLY possess LDF ONLY.
LESS LDF MORE LDF
DIPOLE - DIPOLE FORCES
Dipole moment (): Electrostatic attraction between polar molecules.
It is a measure of the unevenness of electron density in a bond or molecule.
It depends on both electronegativity of atoms and on molecular geometry.
H Cl C O+ -
= 1.08 D = 0.00 D
O C O
= 2.33 D
- - -+ +H
H
DIPOLE - DIPOLE FORCES
Dipole-dipole forces are present only in polar molecules.
They occur when the + end of one polar molecule is attracted to the - end of another.
HYDROGEN BONDING
Hydrogen bonds are a result of the large difference in electronegativity between H and N, O, or F.
They occur when the H of one molecule attached to an O or N is attracted to an O or N of a different molecule.
Some compounds have a H to donate to hydrogen bonding, while others can only accept a H from other compounds to form hydrogen bonds.
O H O N H O+ +
N H N +
O H N+
donor donor donor donor acceptoracceptoracceptor acceptor
HYDROGEN BONDING
H O H R O H
water alcohols
OH....
..
......
phenols
R N
H
H R N
R
HR C
O
O H R C
O
N
R
H
.. .. ....
... . . . . . . .
1o amines 2o aminescarboxylic acids amides
H-Bond donors and acceptors
H-Bond acceptors
R C
O
O R....
. . . . R N
R
R..
R O R.... R C
O. . . .
R C
O. . . .
H RR N
O
O+ ..
..
.. -
ethers aldehydes ketones esters 3o amines nitro compounds
*** Notice that compounds containing an O or N with a H DIRECTLY bound to it are donors and acceptors!***
ION-DIPOLE An ion-dipole force exists between an ion and the
partial charge on the end of a polar molecule.
They are especially important for solutions of ionic substances in polar solvents, such as NaCl in water.
EXPERIMENTAL OUTLINE
A: Test solubility of compounds in hexane and water.
B: Test solubility of organic liquids in water.
C: Test solubility of alcohols in hexane and water.
D: Test solubility of organic solids in diethyl ether, water, acidic and basic solutions.
Table 1.1
Organic Liquid Structure
Intermolecular Force(s) (list all present)
Miscibility in hexane
Miscibility in water
hexaneLondon dispersion M I
toluene
diethyl ether
ethylacetate
1-butanol
methanol
waterM
Tables 1.2 and 1.3
Solute StructuresIntermolecular
Force(s)# drops
miscible in 1 mL of water
toluene 1
ethyl acetate
2
1-butanol 4
Alcohol StructureBoiling Point (Co)
Miscibility in
hexane
Miscibility in
water
methanol
64.7
ethanol 78.5
1-propanol
97.0
1-butanol
117.7
Acid-Base Chemistry
OH + H O H + H3O+
acid base conjugate base
conjugate acid
N +H O H
+ OH
base conjugate base
conjugate acid
acid
N H
O
R O
O
R
Table 1.4
Organic SolidMol. FormulaMol. Weight
Melting pointHazards
Structure
Intermolecular
Force(s)
Solubilities
diethyl ether
water 10% NaHCO3
1M HCl
benzoic acidC7H6O2
122.12 g/mol122-123 oCHarmful if swallowedEye irritant
sodium benzoateC7H5NaO2
144.10 g/mol>300 oC
Avoid contact with skin and
eyes
IMF FLOW CHARTInteracting molecules
or ions
Are ions involved?
YESNO Are polar molecules and
ions both present?
Are polar molecules involved?
NONO
YES
Are hydrogen atoms bonded to N, O, or F atoms?LDF
ONLYEx: CH3CH3
DIPOLE-DIPOLE
Ex: CH3Cl
HYDROGEN BOND
AcceptorEx: CH3OCH3
IONIC BONDINGEx: NaCl
ION-DIPOLEEx: NaCl in H2O
NO YES
YES
HYDROGEN BONDDonor
Ex: H2O, NH3
NO YES
SAFETY CONCERNS
All solvents used in today’s lab are volatile. Wear safety goggles at all times, and use fume hoods.
WASTE DISPOSAL
Pour all liquid waste from this experiment into the container labeled “LIQUID ORGANIC WASTE”.
Do NOT pour any waste down the drain!
LABORATORY NOTEBOOK(Pre-lab)
OBJECTIVE (Must clearly state…)
What you will evaluate How you will evaluate it
TABLE OF PHYSICAL DATA (Single organized table, must include...)
LIQUIDS: (MW, bp, density, hazards) hexane, toluene, diethyl ether, ethyl acetate, acetone, butanol, propanol, ethanol, methanol, and hydrochloric acid.
SOLIDS: (MW, mp, hazards) sodium benzoate, sodium bicarbonate, and benzoic acid.
REFERENCE TO PROCEDURE (Must include…)
Full title Edition Authors page numbers where actual procedure can be found
LABORATORY NOTEBOOK(In-lab)
o DATA/CALCULATIONS o Not applicable for this experiment. All observations will be recorded
directly onto the Final Lab Report.
o EXPERIMENTAL PROCEDUREo In paragraph form, briefly describe the procedure that you actually
followed during the lab. o Paragraph must be written in PAST TENSE, PASSIVE VOICE.o Include any mistakes, accidents or observations if necessary.
FOR NEXT LAB…
Experiment 1 Final Lab Report due.
Experiment 2 Pre-lab Notebook entry due.
It is *highly recommended* that you watch the following video prior to coming to lab. http://www.youtube.com/watch?v=3JlIPnyrZMw