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Physical Pharmacy Lec > 1 > Flashcards

1 Flashcards

1
Q

concerned with the entire process of
converting drugs into medicines.

A

Pharmaceutics

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2
Q

Recognized in an official pharmacopoeia or formulary

A

Drug

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3
Q

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

A

Drug

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4
Q

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

A

Drug

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5
Q

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

A

Drug

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6
Q

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

A

Active Pharmaceutical Ingredient

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7
Q

INN, “generic” names

A

International nonproprietary names

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8
Q

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

A

Pharmaceutical excipients/additives

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9
Q

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

A

Drug delivery system

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10
Q

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

A

Intravascular administration
Extravascular administration

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11
Q

Enumerate some times of Intravascular Administration

A

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

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12
Q

Enumerate Enteral Extravascular administrations

A

Oral
Sublingual
Buccal
Rectal

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13
Q

Enumerate Parenteral Extravascular administrations

A

Subcutaneous
Intramuscular
Intradermal
Intraperitoneal
Intraocular
Intrathecal

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14
Q

Enumerate other Extravascular administrations

A

Inhalationals
Intranasal
Topical and Transdermal
Vaginal
Urethral
Ocular and Otic

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15
Q

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

A

Coated tablets, sealed ampules

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16
Q

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

A

enteric-coated tablets

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17
Q

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

A

Capsules, Coated tablets, flavored syrups

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18
Q

To provide liquid preparations of drug substances, either as
dispersions

A

Suspensions

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19
Q

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

A

Solutions

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20
Q

To provide rate-controlled drug action

A

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

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21
Q

To provide optimal drug action from topical administration sites

A

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

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22
Q

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

A

(rectal or vaginal suppositories)

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23
Q

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

A

injections

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24
Q

To provide for optimal drug action through inhalation therapy

A

inhalatans and inhalation aerosols

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25
Q

What are different classification of dosage forms

A

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

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26
Q

What are some examples of solid oral dosage forms?

A

Powders and granules
Tablet
Capsule
Modified-release

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27
Q

What are some examples of liquid dosage forms?

A

Solutions
Dispersed systems
Colloidal Systems

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28
Q

Examples of gaseous dosage forms

A

Gases
Aerosols

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29
Q

another word for semi-solid

A

Dematologicals

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30
Q

Examples of semi-solid dermatologicals

A

Paste
Oily paste
Ointment
Cream
Lotion
Hydrogel

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31
Q

what are the 2 components of ointment?

A

Lipophilic ointmenet
Hydrophilic ointment

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32
Q

What are the 2 components of cream?

A

Lipophilic cream
Hydrophilic cream

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33
Q

What are the two components of lotion?

A

Suspension
Emulsion

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34
Q

What are the two componend of liquid dosage forms of solutions

A

Aqueos solution
Alcoholic tincture

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35
Q

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

A

Physical pharmaccy

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36
Q

what is difference between physical reaction and a chemical reaction?

A

Composition

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37
Q

Enumerate some physical properties

A

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

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38
Q

Enumerate some chemical properties

A

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

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39
Q

Freezing liquid
Mercury

A

physical

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40
Q

Adding yellow to
blue to make green

A

physical

41
Q

Cutting a piece of
paper into two
pieces

A

physical

42
Q

Dropping a sliced
orange into a vat of sodium hydroxide

A

Chemical

43
Q

Filling a balloon with
natural air

A

physical

44
Q

Shattering Glass with
a baseball

A

physical

45
Q

Corroding Metal

A

chemical

46
Q

Fireworks Exploding

A

chemical

47
Q

Lighting a match

A

chemical

48
Q

Baking a cake

A

physical

49
Q

painting a wall blue

A

physical

50
Q

a bicycle rusting

A

chemical

51
Q

ice cream melting

A

physical

52
Q

scratching a key across a desk

A

physical

53
Q

making a sand castle

A

physical

54
Q

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

A

Ionic

55
Q

sharing of electrons between two nonmetals
responsible for numerous organic compounds

A

Covalent

56
Q

what are the two types of forces of attraction

A

Binding Forces
Attractive Forces

57
Q

Enumerate some binding forces

A

Cohesion
Adhesion
Repulsion

58
Q

Enumerate some attractive forces

A

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

59
Q

Caused by dipoles and induced-diples

A

Attractive forces

60
Q

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

A

Van der Waals Forces

61
Q

What are the three groups of Van der Waals Forces

A

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

62
Q

Interaction between two polar molecules

A

Dipole-Dipole

63
Q

What is the other name for dipole-dipole

A

Keesom forces

64
Q

what is the mechanism for dipole-dipole

A

Orientation or alignment

65
Q

What are some examples of dipole-dipole

A

Water, ethanol, HCl (gas), phenol

66
Q

Interaction between polar and non-polar molecules

A

dipole-induced dipole

67
Q

other name for dipole-induced dipole

A

Debye forces

68
Q

What is the mechanism of dipole-induced dipole

A

Induction

69
Q

what are the examples of dipole-induced dipole

A

Ethyl acetate, ether, methylene chloride,

70
Q

Interaction between two non-polar molecules

A

Induced dipole-induced dipole

71
Q

what is the other name induced dipole-induced dipole

A

London forces

72
Q

What is the mechanism for induced dipole-induced dipole

A

Dispersion

73
Q

Whata re some examples of induced dipole-induced dipole

A

Carbon disulfide, carbon tetrachloride, hexane

74
Q

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

A

Hydrogen bonds

75
Q

has strong IMF

A

Hydrogen bonds

76
Q

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

A

Hydrogen bonds

77
Q

Accounts for unusual properties of water?

A

Indicative of solubility in water

78
Q

As the hydrogen bonds increases the solubility in water also?

A

Increases

79
Q

As the number of carbon chain increases, the hydrogen bond

A

Decreases

79
Q

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

A

decreases

80
Q

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

A

Hydrogen bonds

81
Q

is hydrogen bonding possible in methylene chloride (CH2Cl2)

A

No

82
Q

is hydrogen bonding possible among phosphine (PH3)

A

No

83
Q

Is hydrogen bonding possible in hydrogen peroxide (HOOH)

A

Yes

84
Q

is hydrogen bonding possible in acetone (CH3COCH3)?

A

No

85
Q

polar molecules are attracted to either positive or negative charges

A

Ion-dipole interactions

86
Q

occurs when a salt is dissolved in a polar solvent

A

ion-dipole interactions

87
Q

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

A

Ion-Induced dipole Interaction

88
Q

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

A

example of Ion-induced dipole interaction

89
Q

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

A

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)

90
Q

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

CH3CH3, CH3OH, and CH3CH2OH

A

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.

91
Q

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

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.

92
Q

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

A

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

93
Q

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

A
  1. Extensive
  2. Extensive
  3. Extensive
  4. Intensive
  5. Intensive
  6. Intensive
  7. Intensive
  8. Intensive
  9. Intensive
  10. Intensive
94
Q

Constitutive
* depends on the ______________________________within a
molecule.

A

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

95
Q

Additive
* depends on the _________________ in the molecules.

A

number of atoms

96
Q

Colligative
* depends on the ___________________ in solution.

A

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

97
Q
A

Physical Pharmacy Lec (3 decks)

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