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Physical Pharmacy > Review Concept > Flashcards

Review Concept Flashcards

1
Q

SI base units are fundamental units of measurement in what international system?

A

International System of Units (SI)

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2
Q

these units form the foundation for all measurements in science and engineering

A

SI base units

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3
Q

How many SI base units are there?

A

7

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4
Q

Give the seven SI base units following this format: Base Quantity — Name — Symbol

A

Time — second — s
Length — metre/meter — m
Mass — kilogram — kg
Electric current — ampere — A
Thermodynamic temperature — kelvin — K
Amount of substance — mole — mol
Luminous intensity — candela — cd

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5
Q

The duration of 9,192,631,770 periods of the radiation corresponding to the transition between two hyperfine levels of the ground state of the cesium-133 atom

A

Time

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6
Q

The distance light travels in vacuum in 1/299,792,458 of a second

A

Length

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7
Q

Defined by fixing the numerical value of the Planck constant (h) to 6.62607015 × 10^-34 when expressed in J•s

A

Mass

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8
Q

The flow of 1/1.602176634 × 10^-19) elementary charges per second

A

Electric current

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9
Q

Defined by fixing the numerical value of the Boltzmann constant (k) to 1.380649 × 10^-23 when expressed in J•K^-1

A

Thermodynamic temperature

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10
Q

The amount of substance containing exactly 6.02214076 × 10^23 elementary entities

A

Amount of substance

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11
Q

The luminous intensity, in a given direction, of a source that emits monochromatic radiation of frequency 540 x 10^12 Hz and that has a radiant intensity in that direction of 1/683 watt per steradian

A

Luminous intensity

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12
Q

units of measurement in the International System of Units (SI) that are formed by combining SI base units

A

SI derived units

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13
Q

used to measure various physical quantities and are derived from the seven SI base units through mathematical operations

A

SI derived units

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14
Q

mixture of two or more components that form a homogenous mixture

A

Solution

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15
Q

the dissolved agent of a solution

A

Solute

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16
Q

the component in which the solute is dissolved

A

Solvent

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17
Q

the solute when it is a liquid and will form a solution with a solvent over any concentration range

A

Miscible

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18
Q

measure of the average kinetic energy of particles in a substance

A

Temperature

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19
Q

• Scale starts at absolute zero
• Used primarily in scientific work
• No degree symbol is used

A

Kelvin (K)

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20
Q

commonly used in everyday life in most countries

A

Celsius (°C)

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21
Q

freezing point of water at standard pressure

A

0°C

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22
Q

boiling point of water at standard pressure

A

100°C

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23
Q

commonly used in the United States for everyday measurements

A

Fahrenheit (°F)

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24
Q

freezing point of water in fahrenheit

A

32°F

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25
Q

boiling point of water in fahrenheit

A

212°F

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26
Q

• Starts at absolute zero, like Kelvin
• Used in some engineering applications in the US

A

Rankine (R)

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27
Q

mostly obsolete, but still used in some food production

A

Réaumur (°Ré)

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28
Q

freezing point of water in Réaumur (°Ré)

A

0ºRé

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29
Q

boiling point of water in Réaumur (°Ré)

A

80°Ré

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30
Q

most commonly used in scientific and pharmaceutical applications

A

Celsius and Kelvin

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31
Q

preferred for precise scientific work due to its relation to absolute zero

A

Kelvin

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32
Q

mass of a unit volume of a material substance

A

Density

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33
Q

also called relative density, ratio of the density of a substance to that of a standard substance

A

Specific gravity

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34
Q

used to convert units of grams and milliliters

A

Specific gravity

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35
Q

Concentrations of solutions can be expressed in terms of? molarity (M), Molality (m), Normality (N), Mole fraction, Percentage strength (%, w/w, %w/v, v/v), Milliequivalents (mEq), part per million (ppm), parts per billion (ppb), and Osmolarity (Osm, mOsm).

A

molarity (M)
Molality (m)
Normality (N)
Mole fraction
Percentage strength (%, w/w, %w/v, v/v)
Milliequivalents (mEq)
part per million (ppm)
parts per billion (ppb)
Osmolarity (Osm, mOsm)

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36
Q

forces of attraction within the molecule while intermolecular forces are forces of attraction between molecules

A

Intramolecular Forces

37
Q

• Transfer of electrons between a nonmetal & a metal
• observed in formation of salts

A

Ionic Bond

38
Q

• sharing of electrons between two nonmetals
• observed in organic compounds

A

Covalent Bond

39
Q

• Molecules are polar with permanent polar dipoles

A

Keesom Forces (orientation effect) or Dipole-dipole

40
Q

• transient dipole induced by a permanent dipole
• polar molecules produce temporary electric dipole in nonpolar molecules

A

Debye Forces (induction effect) or Dipole-induced dipole

41
Q

• induce polarity between non polar molecules
• responsible for liquefaction of gases

A

London Forces (dispersion effect) or Induced dipole- induced dipole

42
Q

• Because of the small size of a hydrogen atom and its large field, it can move in close to the electronegative atom (fluorine, oxygen, or nitrogen) and form an electrostatic connection.
• electrostatic interaction of H with highly electronegative atoms (S, N, CL, F, O)
• accounts for unusual properties of water

A

Hydrogen bond or hydrogen bridge

43
Q

• Strong forces between counter ions

A

lon-lon Interactions

44
Q

• polar molecules are attracted to either positive or negative charges
• occurs when salt is dissolved in a polar solvent
• solubility if crystalline substances in H20

A

Ion-Dipole Interaction

45
Q

• induced by close proximity of a charged ion to a non-polar molecule
• responsible for the solubility of non-polar molecules

A

Ion-Induced Dipole

46
Q

The units that constitute the crystal structure can be atoms, molecules, or ions. The sodium chloride crystal, consists of a cubic lattice of sodium ions interpenetrated by a lattice of chloride ions, the binding force of the crystal being the electrostatic attraction of the oppositely charged ions.

A

Crystalline solids

47
Q

temperature at which a liquid pass into the solid state

A

freezing point

48
Q

the heat required to increase the interatomic or intermolecular distances in crystals, thus allowing melting

A

Heat of fusion

49
Q

when a substance exists in more than one crystalline form

A

Polymorphism

50
Q

In organic compounds, the molecules are held together by what?

A

van der Waals forces and hydrogen bonding

51
Q

they tend to flow when subjected to sufficient pressure over a period of time and they do not have definite melting points

A

Amorphous Solids

52
Q

The pressure of the saturated vapor above the liquid is then known as the

A

equilibrium vapor pressure

53
Q

When the rate of condensation equals the rate of vaporization at a definite temperature, the vapor becomes saturated and a dynamic equilibrium is established.

A

Vapor Pressure

54
Q

If a liquid is placed in an open container and heated until the vapor pressure equals the atmospheric pressure, the vapor will form bubbles that rise rapidly through the liquid and escape into the gaseous state.

A

Boiling

55
Q

temperature at which the vapor pressure of the liquid equals the external or atmospheric pressure

A

boiling point

56
Q

temperature at which a liquid transitions into a gas

A

Boiling point

57
Q

nonpolar molecules

A

Normal Hydrocarbons (Alkanes)

58
Q

Normal Hydrocarbons (Alkanes) main intermolecular force

A

London Dispersion Forces (LDFs)

59
Q

polar molecules due to the Q-H bond and can participate in hydrogen bonding along with LDFs

A

Simple Alcohols

60
Q

even more polar than alcohols due to the presence of a carboxyl group (COOH)

A

Carboxylic Acids

61
Q

Have a positive and negative end due to uneven sharing of electrons that allows them to participate in dipole-dipole interactions where the positive end of one molecule attracts the negative end of another

A

Polar molecules

62
Q

Have a relatively even distribution of electrons, resulting in weak LDFs as the main intermolecular force

A

Nonpolar molecules

63
Q

states that at constant temperature, the pressure of a gas is inversely proportional to its volume

A

Boyle’s Law

64
Q

states that at constant pressure, the volume of a gas is directly proportional to its absolute temperature (temperature in Kelvin)

A

Charles’s Law

65
Q

if you squeeze a gas into a smaller container (decrease volume), the pressure of the gas will increase proportionally (and vice versa)

A

Boyle’s Law

66
Q

as you heat a gas (increase temperature), its volume will expand proportionally (and vice versa)

A

Charles’s Law

67
Q

states that at constant volume, the pressure of a gas is directly proportional to its absolute temperature

A

Gay-Lussac’s Law

68
Q

as you heat a gas in a sealed container (constant volume), the pressure of the gas will increase proportionally (and vice versa)

A

Gay-Lussac’s Law

69
Q

states that at constant pressure and temperature, equal volumes of ideal gases contain the same number of molecules

A

Avogadro’s Law

70
Q

if you have two containers of different gases at the same pressure and temperature, the container with the larger volume will have a proportionally larger number of gas molecules

A

Avogadro’s Law

71
Q

a powerful tool that combines Boyle’s Law, Charles’s Law, and Gay-Lussac’s Law into a single equation. It states that for a fixed amount of gas (meaning the number of moles, n, remains constant).

A

Combined Gas Law

72
Q

takes the combined gas law one step further by introducing the concept of the universal gas constant (R). It describes the behavior of ideal gases, which are hypothetical gases that perfectly obey the kinetic molecular theory.

A

Ideal Gas Law

73
Q

Gases can be liquefied under high pressures in a closed chamber as long as the chamber is maintained below the critical temperature. When the pressure is reduced, the molecules expand and the liquid reverts to a gas.

A

Aerosols

74
Q

material that is liquid under the pressure conditions existing inside the container but that forms a gas under normal atmospheric conditions

A

Propellant

75
Q

These devices deliver medication as a pressurized aerosol

A

Metered Dose Inhalers (MDIs)

76
Q

convert liquid medication into a mist for inhalation

A

Nebulizers

77
Q

often contain desiccant pouches to absorb moisture

A

Blister Packs

78
Q

Many antibiotics and other drugs are produced through it, where microorganisms grow in a controlled environment

A

fermentation

79
Q

This process removes water from a product by sublimation

A

Lyophilization (Freeze Drying)

80
Q

This analytical technique separates and identifies volatile compounds in a mixture

A

Gas Chromatography (GC)

81
Q

The combined gas law helps determine the appropriate flow rate and concentration of anesthetic gases to be delivered to patients based on their lung volume and other physiological parameters.

A

Anesthetic Gas Delivery

82
Q

a unique phase of matter that exhibits properties intermediate between those of conventional liquids and crystalline solids

A

Liquid Crystalline

83
Q

Type of LC phases that is the most common, with rod-shaped molecules aligned along the director but lacking positional order

A

Nematic

84
Q

Type of LC Phases in which molecules are also parallel, layered and have some degree of positional order within each layer

A

Smectic:

85
Q

Similar to nematic but in this type of crystal the molecules are parallel but arranged in layers

A

Cholesteric:

86
Q

Microscopic spheres with a bilayer membrane structure similar to cell membranes

A

Liposomes

87
Q

can be used to encapsulate drugs and enhance their solubility, stability, and delivery to target sites

A

Nanoparticles

88
Q

LC materials can be designed to respond to specific stimuli (e.g., temperature, light) to release drugs in a controlled manner.

A

Controlled release

89
Q

Cholesteric liquid crystals can be used in biosensors for rapid detection of diseases or biological molecules.

A

Diagnostic Applications

Physical Pharmacy (3 decks)

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