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Biopharm > Exam I > Flashcards

Exam I Flashcards

1
Q

Substances intended for use in curing, treating, mitigating, diagnosing, or preventing disease.

A

Drugs

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2
Q

The product by which a drug is given or administered. (e.g. tablets, capsules, ointments, etc)

A

Drug dosage form (drug product)

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3
Q

The release of the drug substances from the drug product.

A

Drug performance

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4
Q

Biopharmaceutics examines the interrelationship of what three things?

A
  1. Physical/chemical properties of the drug
  2. dosage form
  3. rate and extent of absorption
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5
Q

Repulsive and attractive forces are equal, potential energy is minimum, and the system is most stable at __ to __ angstroms.

A

3 to 4

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6
Q

Nonionic interaction or charge-charge interaction between molecules

A

Van der Waals forces

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7
Q

Are Van der Waals forces strong or weak?

A

weak

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8
Q

Involves a dispersion of charge across a molecule called dipole or permanent dipole

A

Van der Waals forces

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9
Q

Three types of van der waals forces:

A
  1. Keesom
  2. Debye
  3. London
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10
Q

Type of force that arises due to differences in electronegativity (e.g. peptide bond)

A

Permanent dipole

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11
Q

Force between two permanent dipoles when interacting with one another in an ion-like fashion.

A

Keesom forces

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12
Q

Ability of a permanent dipole to polarize charge in neighboring molecule

A

Debye forces

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13
Q

Two neighboring neutral molecules induce partial charge distribution

A

London forces

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14
Q

Interaction between the pi-electron orbitals in a system.

A

Orbital overlap

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15
Q

Attraction forces that occur between polar or non-polar molecules and ions

A

Ion-Dipole and Ion-Induced Dipole Forces

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16
Q

Cause the solubility of crystalline substances in water (cation attracts negative O and anion attracts positive H)

A

Ion-dipole interaction

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17
Q

Force involved in the formation of the iodid complex

A

Ion-induced dipole forces

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18
Q

Interaction that has effect on physical properties of pharmaceutical agents.

A

Ion-ion interaction

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19
Q

Interaction between a molecule containing a hydrogen atom and a strongly electronegative atom.

A

Hydrogen bond

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20
Q

When solids pass directly from solid to gaseous phase without melting at room temperature.

A

Sublimation

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21
Q

When gases pass directly from gaseous phase to solid phase.

A

Deposition

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22
Q

Dehydration process where the water is removed from solid state to vapor state using sublimation.

A

Lyophilization

23
Q

How does lyophilization (freeze drying) work?

A

Reduced pressure

24
Q

Can the liposome structure break?

A

Yes

25
Q

How does the liposome structure break?

A

Temp, pH, changing solvent, etc

26
Q 
Which of the following is not charge-charge interaction? 
Keesom forces
Debye forces
Hydrogen bond
London forces
A

Hydrogen bond

27
Q

Transfer of material from gaseous state to solid state is defined as:

A

Deposition

28
Q

Term used to describe the different crystalline forms of a drug substance.

A

Polymorphs

29
Q

Cortisone acetate has __ polymorphic forms

A

5

30
Q

Ranitidine Hcl has __ polymorphic forms

A

2

31
Q

Mizolastine has __ polymorphic forms

A

3

32
Q

Carbamazepine has __ polymorphic forms and ___

A

2; dihydrate

33
Q

Use of nanoparticles in technology

A

Nanotechnology

34
Q

One of the major characteristics on nanoparticles is what?

A

Enhanced surface area

35
Q

What makes up a solution?

A

A solute and a solvent

36
Q

What is the minor component in a solution (e.g. drug substance)

A

Solute

37
Q

What is the major component of a solution (e.g. water, dissolution media)

A

Solvent

38
Q

A homogenous mixture containing two or more components is what?

A

A solution

39
Q

Moles of solute in 1 liter of soltuion

A

Molarity

40
Q

Gram equivalent weight of solute in 1 liter of solution

A

Normality

41
Q

Moles of solute in 1000 g of solvent

A

Molality

42
Q

Ratio of the moles of one constituent of a solution to the total moles of all constituents.

A

Mole fraction

43
Q

Gram of solute in 100g of solution

A

Percent by weight (w/w)

44
Q

Mililiters of solute in 100 mL of solution

A

Percent by volume (v/v)

45
Q

Grams of solute in 100 mL of solution

A

Percent by weight-in-volume (w/v)

46
Q

Atomic weight divided by the valence

A

Equivalent weight

47
Q

Solution which has no change in properties of the constituents other than dilution, when they are mixed to form the solution.

A

Ideal solution

48
Q

A solution which has a change in properties of its constituents such as volume, heat when mixed.

A

Real solution

49
Q

In an ideal solution, the partial vapor pressure of each volatile component is equal to the vapor pressure of the pure constituent multiplied by its mole fraction in the solution.

A

Roult’s Law

50
Q

A-A, B-B, and A-B interactions are equal.

A

Roult’s Law

51
Q

A-B interactions stronger than A-A or B-B interactions.

A

Negative deviation from Roult’s Law

52
Q

A-B interactions weaker than A-A or B-B interactions

A

Positive deviation from Roult’s Law

53
Q

The temperature at which the vapor pressure of the liquid equals the pressure surrounding the liquid.

A

Boiling point

Biopharm (1 decks)

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