This is related to medical courses, especially those that specialize in pharmacology. This is a great help for them in their studies and in their future career.

1. PHYSICAL PHARMACY
Shanaiah Bautista, RPh

2. Definition of Terms

3. Physical Pharmacy
• The area in pharmacy that deals with the
quantitative and theoretical principles of
physiochemical science as they applied to the
practice of pharmacy.
• Physical chemistry in pharmacy.

4. Overview in General Chemistry
Atoms (Subatomic Particle: E,
P, N)
Molecule (Polar and Non-
polar
Ion (Cation and Anion)
Repulsion Attraction
Cohesion
Adhesion

5. FORCES OF ATTRACTION
INTRAMOLECULAR FORCES
• Ionic Bond – transfer of electron
• Covalent Bond- sharing of electrons
INTERMOLECULAR FORCES
• Van der waals – Keesom, Debye, London
• Ion Dipole- polar molecule are attracted in either positive/ negative
• Ion-Induced dipole – the force of attraction induced by a clone
proximity of a charged ion into a non- polar molecule
• Hydrogen bonds- attraction of a strongly electronegative ion

6. PHYSICAL PROPERTIES OF SYSTEMS
ADDITIVE
PROPERTY
• Depends on the sum of the
individual properties of the
components present in a
system
CONSTITUTIVE
PROPERTY
• Depends on the type and
arrangement of the
components present in a
system
COLLIGATIVE
PROPERTY
• Depends on the number of
component present in a
system

7. STATES
OF
MATTER
LIQUID
GAS
PLASMA
SOLID

8. TYPES OF PROPERTIES
EXTENSIVE • Depends on the
size
• Entropy, enthalpy,
electronic
resistance, mass
INTENSIVE • Does not depend
on the size
• Spgr, viscosity,
density, velocity

9. DENSITY
D=𝑀
𝑉
Unit:
𝑔
𝑚𝐿
Types of Density 1. ABSOLUTE (in vacuum)
2. APPARENT (in air)
3. RELATIVE (@ specific condition)
SPECIFIC GRAVITY
(Methods of
Determining Sp.Gr)
- Density of Τ
𝑠𝑥 𝑑𝑒𝑠𝑖𝑡𝑦 𝑜𝑓 𝑠𝑡𝑑.
1. Pycnometer
2. Mohr Westphal Balance
3. Hydrometer

10. - Partly solid and partly liquid.
- Tends to flow like liquid and under extreme
conditions.
A. SMECTIC
B. NEMATIC
C. CHOLESTERIC
PLASMA

11. GASES
- Have kinetic energy that produces rapid motion
- Held together by weak intermolecular forces
- Capable of filling all available space
- Compressible
KINETIC MOLECULAR THEORY OF GASES
1. Total volume of gas molecules is negligible as compared to the volume of
space in which they are continued.
2. Gas particles do not attract one another but rather move independently
from each other.
3. Particles exhibit continuous random movement due to their kinetic
energy.
4. Gas molecules exhibit perfect elasticity.

12. BOYLE’S LAW 𝑷𝟏𝑽𝟏 = 𝑷𝟐𝑽𝟐
CHARLES LAW 𝑇1
𝑉1
=
𝑇2
𝑉2
GAY LUSSAC’S
𝑃1
𝑇1
=
𝑃2
𝑇2
COMBINED GAS LAW 𝑃1𝑉1
𝑇1
=
𝑃2𝑉2
𝑇2
REAL GAS EQUATION 𝑃 + 𝑎𝑛2
𝑉2
𝑉
𝑛𝑏
= 𝑁𝑟𝑡

13. HENRY’S LAW States the amount of gas dissolved in a
solution is proportional to the partial
pressure of the gas in equilibrium with
the solution.
DALTONS LAW OF PARTIAL
PRESSURE
- States that the total pressure in a
mixture of gases is equal in the sum
of the partial pressure of each gas.
- The partial pressure is the pressure a
gas would evert if it alone occupied
the whole volume of the mixture.
GRAHAMS LAW - Speed of diffusion of gas is inversely
proportional to the density

14. LIQUIDS
- Possess less kinetic energy than do gases
- Occupy a definite volume take the shape of the containers that
hold them
- Denser than gases
- Not compressible
VAPOR PRESSURE
- Is the pressure of the saturated vapor above a liquid resulting from the
escape of surface liquid molecules.
CLAUSIUS-CLAPEYRON EQUATION
Log
𝑃2
𝑃1
∆𝐻𝑣(𝑇2−𝑇1)
2.303𝑅𝑇1𝑇2

15. SOLIDS
- Characterized as having fixed shapes.
- Nearly incompressible
- Have strong intermolecular forces
- Very little kinetic energy
- Their atoms vibrate in fixed positions about an equilibrium position,
and so there is very little transformation
CRYSTALLINE AMORPHOUS

16. CRYSTALLINE
1. CUBIC- NaCl
2. TETRAGONAL- Urea
3. HEXAGONAL- Iodoform
4. RHOMBIC- Iodine
5. MONOCLINIC- Sucrose
6. TRICLINIC- Boric Acid
7. ORTHORHOMBIC-
ritonavir

17. Types of Crystals Characteristic/
Chemical bond
involve
Exampes
ATOMIC - Strong carbon
covalent bond
Diamond
Graphite
METALLIC - Strong metal bond. Group 1A and 2A
MOLECULAR - Van der waals Co2 and Naphthalene
IONIC - Electrostatic ionic
bond
NaCl

18. AMORPHOUS
• Non- crystalline; no definite order
• Have no definite and sharp melting points

19. POLYMORPHISIM
• Solids that have more than one crystalline form.
ENANTIOTROPIC o Polymorphism involves a change
in various direction
MONOTROPIC o Unidirectional
ISOTROPIC o Identical in all direction
ANISOTROPIC o Different in all direction

20. DIFFERENCE BETWEEN ENANTIOTROPY AND
MONOTROPY
ENANTIOTROPIC PAIR MONOTROPIC PAIR
Reversible phase transition Irreversible phase transition
Metastable stable Metastable stable
Lower melting form is
thermodynamically stable below the
transition temperature and higher
melting point form is stable above
the transition temp
Higher melting form is always
thermodynamically stable form.
Transition is endothermic Transition is exothermic
Lower melting point has lower heat
of fusion
Higher melting point has high heat
of fusion.