Download - Chap 1-1 intra and intermolecular forces
Instrumental techniquesPhar 6521
1
Chromatography is a physical method of
separation in which the components to be
separated are distributed between two
phases (KD/P = Distribution/partition constant)
one of which is stationary (stationary phase)
while the other (the mobile phase) moves
through it in a definite direction.
The chromatographic process occurs due to
differences in the distribution constant of the
individual sample components.
3
Chromatography
KD of Cpd A = [A]S / [A]M
KD = Distribution constant of compound A
[A]S = concentration of compound A in stationary phase
[A]M = concentration of compound A in mobile phase
For eg. TLC Chromatography compounds distributes itself b/n a liquid mobile phase and a solid
stationary phase The rate of migration for a chemical compound is determined by
how much of it distributes into the mobile and stationary phases
Case 1. A compound that distributes itself 100% into the mobile phase
will migrate at the same rate of the mobile phase
Case 2: On the other hand, a compound that distributes itself 100%in the stationary phase will not migrate at all 4
In most molecular substances, there are two types of attractive forces:
1. Intramolecular and 2. Intermolecular forces
5
Chromatographic separation is achieved due to
Different compounds have different KD values
Distribution constant (KD) is affected by
the type of intermolecular forces that present in
molecules
force that hold atoms in a single molecule or a force of attraction within a molecule
e.g. covalent bond, ionic bond
H-Cl, Na+Cl
-
Intramolecular forces
6
an attraction between two or more separate
molecules.
are the result of attractions between positively and
negatively charged regions of separate molecules.
They are not as strong as intramolecular force
(chemical bonds).
Intermolecular forces
7
These intermolecular forces as a group are referred to as van der Waals forces.
There are three types of intermolecular forces,
1. Dipole-dipole interactions2. Hydrogen bond3. London force/Dispersion force
8
A very approximate strength order would be:
Bond type Relative strength
Ionic bonds 1000
Hydrogen bonds 100
Dipole-dipole 10
London forces 1
9
Intermolecular Forces
They are, however, strong enough to control physical properties such as, solubility, boiling and melting points, vapor pressures, and viscosities.
10
Dipole-Dipole Interactions
• Molecules that have permanent dipoles are attracted to each other.
√ The positive end of one is attracted to the negative end of the other and vice-versa.
√ These forces are only important when the molecules are close to each other.
11
It occurs in polar compounds These work in a similar manner to ionic
interactions, but are weaker because only partial charges are involved.
An example of this can be seen in Acetone
Dipole-Dipole Interactions
12
----------
Dipole-Dipole Interactions
The more polar the molecule, the higher is its boiling point.
13
Hydrogen BondingHydrogen bonding occurs when
Hydrogen is bonded to N, O, or F are unusually strong.
Hydrogen atom has a partial positive charge and can interact with another highly electronegative atom in an adjacent molecule (N, O, or F).
it is a special type of dipole-dipole force
The result is a dipolar molecule e.g H2O, NH3, HF 14
London/Dispersion Forces
While the electrons in the 1s orbital of helium would repel each other (and, therefore, tend to stay far away from each other), it does happen that they occasionally wind up on the same side of the atom.
It involve the attraction between temporarily induced dipoles 15
London/Dispersion Forces
At that instant, then, the helium atom is polar, with an excess of electrons on the left side and a shortage on the right side.
16
London/Dispersion Forces
Another helium nearby, then, would have a dipole induced in it, as the electrons on the left side of helium atom 2 repel the electrons in the cloud on helium atom 1.
17
London/Dispersion Forces
London dispersion forces, or dispersion forces, are attractions between an instantaneous /temporary dipole and an induced dipole.
18
London/Dispersion Forces
These forces are present in all molecules, whether they are polar or non-polar.
The tendency of an electron cloud to distort in this way is called polarizability.
19
This polarization can be induced either by A polar molecule or A non-polar molecule (the repulsion
of negatively charged electron clouds in non-polar molecules)
London/Dispersion Forces
20
21
Factors Affecting London Forces
The strength of dispersion forces tends to increase with increased molecular weight.
Larger atoms have larger electron clouds, which are easier to polarize.
22
Factors Affecting London Forces
The shape of the molecule affects the strength of dispersion forces: long, skinny molecules (like n-pentane tend to have stronger dispersion forces than short, fat ones (like neopentane).
This is due to the increased surface area in n-pentane.
23
Which Have a Greater Effect:Dipole-Dipole Interactions or Dispersion Forces?
• If two molecules are of comparable size and shape, dipole-dipole interactions will likely be the dominating force.
• If one molecule is much larger than another, dispersion forces will likely determine its physical properties.
24
Ion-Dipole Interactions
25
• A fourth type of force, ion-dipole interactions are an important force in solutions of ions.
• The strength of these forces are what make it possible for ionic substances to dissolve in polar solvents.
Anthocyanins (also anthocyans) are
belong to a parent class of molecules called flavonoids cationic organic compound well water-soluble pigments due to ion-dipole interaction
Quaternary ammonium cationare salts of quaternary ammonium cations.Soluble in water
Polar Molecule
A Molecule with a Positive and Negative Side
Dipole Moment
• A Measure of Molecular Polarity
• A Non-polar Molecule will have a Zero Dipole Moment
28
Molecular Polarity
Why is Polarity Important?
Many Properties Depend on Polarity
Melting and Boiling Point
Surface Tension, Viscosity
Reactivity
Solubility (e.g., will it dissolve in water)
29
Requirements
A Polar Molecule Requires
Polar Bonds
A Molecular Shape that Separates the by
the partial Positive from the Negative Side
30
Unequal sharing of e- in a bond called Polar Covalent Bond or Polar Bond
Partial Charge indicated by delta +/-
Polar Covalent Bonds
-+
31
Polar Covalent Bonds
NON-polar covalent bonds
Bonds between identical atoms such as H-H, F-F involve equal sharing of e-
Polar covalent bonds
Bonds between different atoms involve unequal sharing of e-
Polar Covalent Bonds have a Partial Charge Separation
32
Electronegativity
Electronegativity is the ability of an
atom to attract electrons in a bond.
Nonmetals bonded to N, O, F usually
have polar bonds
33
Electronegativity Index of Some Elements
34
Electronegativity Used to Determine Bond Polarity
EN < 0.45 Non-polar Bond
1.75 > EN > 0.45 Polar Bond
EN > 1.75 Ionic Bond Atoms
35
Polar or Non-polar Bond?
O-H EN = 1.4 Polar Bond
C-H EN = 0.4 Non-polar Bond
C-O EN = 1.0 Polar Bond
H-Cl EN = 0.8 Polar Bond
Polar Molecules
The molecule is usually polar
If all atoms attached to central atom
are not the same
Or if central atom has 1 or more lone
pairs of electrons
36
Examples
Polar compounds
HCN, H2O, CHCl3, CH2Cl 2
Non-polar
CO2, CCl4
37
In Conclusion
Polarity Determined from
Polar Bonds ( EN > 0.45)
Molecular Shape with + & - sides
N and O in Molecules often lead to
Polar Molecules or Regions
38
In Conclusion
Polarity will be important
In Determining Intermolecular Forces
Vapor Pressure, Boiling and Melting Points
Surface Tension, Viscosity
Solubility
Reactivity (Organic Chemistry)
39
Intermolecular Forces Affect Many Physical Properties
The strength of the attractions between particles can greatly affect the properties of a substance or solution.
Solubility
Defines as the amount of a solute that will dissolve in a specific solvent at given condition
41
Degree of solubility (types of saturation)Saturated solution: A solution with solute that dissolves
until it is unable to dissolve anymore, leaving the undissolved substances at the bottom.
Unsaturated solution: A solution (with less solute than the saturated solution) that completely dissolves, leaving no remaining substances.
Supersaturated solution: solution (with more solute than the saturated solution) that contains more undissolvedsolute than the saturated solution because of its tendency to crystallize and precipitate
Factors that affects solubility
The nature of solute and solvent Temperature Pressure (only applicable to gases)
42
The nature of solute and solvent When two substances are similar they can dissolve in
each other
Polar solutes dissolve in polar solventNon-polar solutes tend to dissolve in non-polar solvent
“Like dissolve like” two liquids dissolve in each other b/c the molecules
are alike in polarity
43
Note: solvents are grouped either polar or non-polar solvent
Polar Solvent: a liquid made up of polar moleculesNon-polar Solvent: a liquid made up of non-polar molecules
The nature of solute and solvent
Ionic compounds are made up of charged ionssimilar to polar compounds e.g. NaCl
Ionic compounds are more soluble in polarsolvent than in a non-polar solvent ion-dipole interaction
44
The nature of solute and solvent
45
Temperature
Solubility of solids in liquids The solubility of a solid increases as temp increases
Solubility of gases in liquid are affected by temperature Opposite to the solubility of solids in liquidsAs the temperature increases, the solubility of a GAS
in a liquid decreases
WHY ? As the temperature increases, the kinetic energy of
the solute gas increases and the gas can escape
46
Pressure when the pressure is increased over the
solvent, the solubility of gas is increased
WHY ? Pressure increases as gas molecules strike the
surface to enter the solution increased
47
Factors of Dissolving
Rate of which a solid solute dissolves in a solutiondepends on three factors Surface area: speed up the solubility by
increasing surface area Stirring: increases contact b/n solvent and
solute Temperature: kinetic energy increase
48