1 Flashcards by San Felipe Michael Josh

concerned with the entire process of
converting drugs into medicines.

Pharmaceutics

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Recognized in an official pharmacopoeia or formulary

Drug

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Intended for use in the diagnosis, cure, mitigation, treatment, or prevention of disease

Drug

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Other than food, intended to affect the structure or function of the body

Drug

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intended for use as a component of a medicine but not
a device or a component, part, or accessory of a device

Drug

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Chemical compound with
pharmacological (or other direct
effect ) intended for used in
diagnosis, treatment or prevention
of diseases

Active Pharmaceutical Ingredient

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INN, “generic” names

International nonproprietary names

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“inactive” ingredients for technological, biopharmaceutical and/or stability reasons

Pharmaceutical excipients/additives

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formed by
technological processing (drug formulation)
must therapeutic intentions, route of administration,
dosing, etc.

Drug delivery system

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What are the two routes of administration of drug delivery system?

Intravascular administration
Extravascular administration

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Enumerate some times of Intravascular Administration

Intravenous (IV) Administration
Intra-arterial (IA) Administration
Intracardiac (IC) Administration

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Enumerate Enteral Extravascular administrations

Oral
Sublingual
Buccal
Rectal

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Enumerate Parenteral Extravascular administrations

Subcutaneous
Intramuscular
Intradermal
Intraperitoneal
Intraocular
Intrathecal

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Enumerate other Extravascular administrations

Inhalationals
Intranasal
Topical and Transdermal
Vaginal
Urethral
Ocular and Otic

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To protect the drug substance from the destructive influences of
atmospheric oxygen or humidity

Coated tablets, sealed ampules

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To protect the drug substance from the destructive influence of
gastric acid after oral administration

enteric-coated tablets

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To conceal the bitter, salty, or offensive taste or odor of a drug
substance

Capsules, Coated tablets, flavored syrups

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To provide liquid preparations of drug substances, either as
dispersions

Suspensions

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To provide liquid preparations of drug substances, either as
clear preparations

Solutions

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To provide rate-controlled drug action

(various controlled-release
tablets, capsules, and suspensions)

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To provide optimal drug action from topical administration sites

(ointments, creams, transdermal patches, and ophthalmic, ear, and
nasal preparations)

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To provide for insertion of a drug into one of the body’s orifices

(rectal or vaginal suppositories)

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To provide for placement of drugs directly in the bloodstream or body
tissues

injections

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To provide for optimal drug action through inhalation therapy

inhalatans and inhalation aerosols

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What are different classification of dosage forms

Solid Oral Dosage forms Liquid Dosage forms Gaseous dosage forms Semi-solid dosage forms Drug delivery system

What are some examples of solid oral dosage forms?

Powders and granules Tablet Capsule Modified-release

What are some examples of liquid dosage forms?

Solutions Dispersed systems Colloidal Systems

Examples of gaseous dosage forms

Gases Aerosols

another word for semi-solid

Dematologicals

Examples of semi-solid dermatologicals

Paste Oily paste Ointment Cream Lotion Hydrogel

what are the 2 components of ointment?

Lipophilic ointmenet Hydrophilic ointment

What are the 2 components of cream?

Lipophilic cream Hydrophilic cream

What are the two components of lotion?

Suspension Emulsion

What are the two componend of liquid dosage forms of solutions

Aqueos solution Alcoholic tincture

Concerned with the use of physico-chemical principles as applied to various branches of pharmacy

Physical pharmaccy

what is difference between physical reaction and a chemical reaction?

Composition

Enumerate some physical properties

Color Smell Freezing point Boiling point Melting point Capacitance Density Volume Mass Viscosity Etc.

Enumerate some chemical properties

Reactivity Flammability Heat of Combustion Oxidation states Coordination Number Half-life Etc.

Freezing liquid Mercury

physical

Adding yellow to blue to make green

physical

Cutting a piece of paper into two pieces

physical

Dropping a sliced orange into a vat of sodium hydroxide

Chemical

Filling a balloon with natural air

physical

Shattering Glass with a baseball

physical

Corroding Metal

chemical

Fireworks Exploding

chemical

Lighting a match

chemical

Baking a cake

physical

painting a wall blue

physical

a bicycle rusting

chemical

ice cream melting

physical

scratching a key across a desk

physical

making a sand castle

physical

transfer of electrons between a metal & nonmetal usually observed in the formation of salts

Ionic

sharing of electrons between two nonmetals responsible for numerous organic compounds

Covalent

what are the two types of forces of attraction

Binding Forces Attractive Forces

Enumerate some binding forces

Cohesion Adhesion Repulsion

Enumerate some attractive forces

Van der waal forces Hydrogen bonding Ion-Dipole Ion-induced dipole

Caused by dipoles and induced-diples

Attractive forces

Weak forces that involve displacement of charge and exist in all molecules and atoms

Van der Waals Forces

What are the three groups of Van der Waals Forces

Dipole-Diple Dipole-Induced Dipole Induced dipole-Induced dipole

Interaction between two polar molecules

Dipole-Dipole

What is the other name for dipole-dipole

Keesom forces

what is the mechanism for dipole-dipole

Orientation or alignment

What are some examples of dipole-dipole

Water, ethanol, HCl (gas), phenol

Interaction between polar and non-polar molecules

dipole-induced dipole

other name for dipole-induced dipole

Debye forces

What is the mechanism of dipole-induced dipole

Induction

what are the examples of dipole-induced dipole

Ethyl acetate, ether, methylene chloride,

Interaction between two non-polar molecules

Induced dipole-induced dipole

what is the other name induced dipole-induced dipole

London forces

What is the mechanism for induced dipole-induced dipole

Dispersion

Whata re some examples of induced dipole-induced dipole

Carbon disulfide, carbon tetrachloride, hexane

electrostatic interaction of H with highly electronegative atoms (S, N, Cl, F, O) accounts for unusual properties of water

Hydrogen bonds

has strong IMF

Hydrogen bonds

Partly covalent as the electron of the H atom is substantially delocalized to the electronegative atom

Hydrogen bonds

Accounts for unusual properties of water?

Indicative of solubility in water

As the hydrogen bonds increases the solubility in water also?

Increases

As the number of carbon chain increases, the hydrogen bond

Decreases

As the carbon chain increases and hydrogen bonding decreases, the solubility in water?

decreases

what is the bond happening the sugar phosphate backbone among base pairs of A T and G C,

Hydrogen bonds

is hydrogen bonding possible in methylene chloride (CH2Cl2)

is hydrogen bonding possible among phosphine (PH3)

Is hydrogen bonding possible in hydrogen peroxide (HOOH)

Yes

is hydrogen bonding possible in acetone (CH3COCH3)?

polar molecules are attracted to either positive or negative charges

Ion-dipole interactions

occurs when a salt is dissolved in a polar solvent

ion-dipole interactions

induced by close proximity of a charged ion to the nonpolar molecules

Ion-Induced dipole Interaction

formation of the iodide complex (I2 + K+I- → K+I3-)

example of Ion-induced dipole interaction

List the substances BaCl2, H2, CO, HF, and Ne in order of increasing boiling points.

Ne (weakest London dispersion forces) H2 (weak London dispersion forces) CO (dipole-dipole forces and London dispersion forces) HF (hydrogen bonding and London dispersion forces) BaCl2 (strong ionic bonds)

Identify the intermolecular forces present in the following substances, and select the substance with the highest boiling point: CH3CH3, CH3OH, and CH3CH2OH

Both methanol (CH3OH) and ethanol (CH3CH2OH) have hydrogen bonding, dipole-dipole forces, and London dispersion forces. However, ethanol has a longer carbon chain than methanol, which increases its molecular weight and the strength of its London dispersion forces. Therefore, ethanol (CH3CH2OH) has the highest boiling point due to the combination of hydrogen bonding, dipole-dipole forces, and stronger London dispersion forces.

The dipole moments of acetonitrile, CH3CN, and methyl iodide, CH3I, are 3.9 D and 1.62 D, respectively. (a) Which of these substances will have the greater dipole-dipole attractions among its molecules? (b) Which of these substances will have the greater London dispersion attractions? (c) The boiling points of CH3CN and CH3I are 354.8 K and 315.6 K, respectively. Which substance has the greater overall attractive forces?

a) Acetonitrile (CH3CN) will have greater dipole-dipole attractions. b) Methyl iodide (CH3I) will have greater London dispersion attractions. c) Acetonitrile (CH3CN) has greater overall attractive forces.

Determine the types of forces present in each: 1. H2O 2. CCl4 3. SO2 4. LiF 5. Ca(NO3)2 aqueous solution 6. HF 7. PCl3

H₂O (water) Hydrogen bonding: Due to the presence of O-H bonds. Dipole-dipole forces: Polar molecule due to the electronegativity difference between oxygen and hydrogen. London dispersion forces: Present in all molecules, regardless of polarity. 2. CCl₄ (carbon tetrachloride) London dispersion forces: Nonpolar molecule due to the symmetrical arrangement of chlorine atoms. 3. SO₂ (sulfur dioxide) Dipole-dipole forces: Polar molecule due to the electronegativity difference between sulfur and oxygen. London dispersion forces: Present in all molecules. 4. LiF (lithium fluoride) Ionic bonding: Ionic compound composed of a metal (Li) and a nonmetal (F). 5. Ca(NO₃)₂ aqueous solution Ion-dipole forces: Interaction between the ions (Ca²⁺ and NO₃⁻) and the polar water molecules. Hydrogen bonding: Water molecules interact through hydrogen bonding. London dispersion forces: Present in all molecules. 6. HF (hydrogen fluoride) Hydrogen bonding: Due to the presence of the O-H bond. Dipole-dipole forces: Polar molecule due to the electronegativity difference between hydrogen and fluorine. London dispersion forces: Present in all molecules. 7. PCl₃ (phosphorus trichloride) Dipole-dipole forces: Polar molecule due to the electronegativity difference between phosphorus and chlorine. London dispersion forces: Present in all molecules

Extensive Property versus Intensive Property 1.Mass 2.Length 3.Volume 4.Temperature 5.Pressure 6.Density 7.Viscosity 8.Surface tension 9.Specific gravity 10.Color

1. Extensive 2. Extensive 3. Extensive 4. Intensive 5. Intensive 6. Intensive 7. Intensive 8. Intensive 9. Intensive 10. Intensive

Constitutive * depends on the ______________________________within a molecule.

Constitutive properties depend on the arrangement of atoms or groups of atoms within a molecule

Additive * depends on the _________________ in the molecules.

number of atoms

Colligative * depends on the ___________________ in solution.

Colligative properties depend on the number of solute particles in a solution