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Inorganic and Organic Pharmaceutical
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Lecture Notes No. 1Pharmaceutical Chemistry
Part 1
Inorganic and Organic Pharmaceutical
, General Chemistry
Chemistry – study of matter
Matter – anything that occupies space and has mass
UNITS OF MEASUREMENT
1. Composition
2. Structure Length Meter (m)
3. Changes that matter undergoes Mass Kilogram (kg)
Time Seconds (sec)
4. Energy involved in such changes or interactions
Temperature Kelvin (K)
Mass – refers to the amount of matter present in the material
Weight = Mass x Pull of gravity
Classification of Matter
• Element - simplest form of matter, 1 kind of material or atom
• Compound - substances composed of two or more elements united chemically in definite proportion
• Mixture - composed of 2 or more substances that are not chemically combined
Plasma
• Colorless fluid part of blood, lymph, or milk in which corpuscles or fat globules are
suspended
S
• Amber- colored protein-rich liquid that separates out when blood coagulates
• Used to provide immunity
• Diagnostic agent
,Classification of Mixture
A. According to the Nature of Particles
a. Homogenous
b. Heterogenous
B. According to the Size of Particles
a. Solution - uniform mixture (homogenous), composed of solute and solvent where solute is soluble
b. Suspension - Coarse Mixture, finely divided solid materials distributed in a liquid where solid is insol.
c. Colloid - particles of solute not broken down to the size of the molecules but are small enough to
remain suspended and evenly dispersed throughout the medium
Process of Separating Components of Mixtures
1. Decantation - difference in specific gravity or density
2. Distillation - evaporation and then condensation
3. Evaporation
4. Magnetic Separation
5. Filtration
6. Sorting
7. Centrifugation - speeding up of settling process of a precipitate
8. Fractional Crystallization - lowering of temp so that the more insoluble comp crystallizes out first
9. Chromatography - difference in solvent affinity
Properties of Matter
1. Intrinsic/Intensive - INDEPENDENT of mass or amount (density, specific gravity, melting point)
2. Extrinsic/Extensive - DEPENDENT on mass (weight, volume, pressure, heat content)
Changes that matter undergoes
1. Physical Change - change in phase
, 2. Chemical Change - change in both intrinsic and extrinsic properties
Evidences of Chemical Change
• Evolution of gas
• Formation of precipitate
• Emission of light
• Generation of electricity
• Production of mechanical energy
• Absorption/liberation of heat
Types of Chemical Reactions
• Direct Union- Fe + S FeS (all sulfides are BLACK)
• Decomposition/Analysis- Na2CO3 Na2O + CO2
• Single Replacement- Na + HCl NaCl + H2
• Double Displacement - NaCl + AgNO3 NaNO3 + AgCl
Processes Involved in Chemical Change
1. Oxidation +𝑂
2. Reduction − 𝑂 𝑜𝑟 + 𝐻
3. Neutralization 𝑎𝑐𝑖𝑑 + 𝑏𝑎𝑠𝑒 𝑠𝑎𝑙𝑡 + 𝑤𝑎𝑡𝑒𝑟
4. Hydrolysis 𝑤𝑎𝑡𝑒𝑟 + 𝑠𝑎𝑙𝑡 𝑎𝑐𝑖𝑑 + 𝑏𝑎𝑠𝑒
5. Saponification 𝑎𝑙𝑘𝑎𝑙𝑖 + 𝑓𝑎𝑡𝑠 𝑠𝑜𝑎𝑝 + 𝑔𝑙𝑦𝑐𝑒𝑟𝑜𝑙
6. Fermentation 𝑜𝑟𝑔𝑎𝑛𝑖𝑐 𝑠𝑢𝑏𝑠𝑡𝑎𝑛𝑐𝑒+ 𝑚𝑖𝑐𝑟𝑜𝑏𝑒𝑠 𝑎𝑙𝑐𝑜𝑜𝑙
• Nuclear Change – ∆ in structure, properties, composition of the nucleus in the of the element
• Nuclear Fission - splitting of a heavy atom
• Nuclear Fusion - union of 2 light atoms to form a bigger molecule
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