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PhyPharm > States of matter > Flashcards

States of matter Flashcards

1
Q

Cohesive forces

A

Forces that attracts molecules of the same substance

Forces between like substances

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2
Q

Adhesive forces

A

Forces that attracts molecules between different substances

Forces between unlike substances

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3
Q

Forces between like substances

A

Cohesive forces

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4
Q

Forces between unlike substances

A

Adhesive forces

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5
Q

List the IMF

A

Van der Waal forces
hydrogen bonds

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6
Q

Coulombic attraction

A

Attractive forces between oppositely charged particles

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7
Q

What are polar molecules?

A

Molecules with permanent dipoles due to partial moments within the molecule

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8
Q

What are nonpolar molecules?

A

Molecules with no dipole moment

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9
Q

List the van der waal forces.

A

Dipole-dipole forces
Dipole-induced dipole forces
Induced dipole-induced dipole (london forces)

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10
Q

Dipole-dipole forces synonym

A

Keesom forces

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11
Q

Dipole-induced dipole forces synonym

A

debye forces

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12
Q

Explain Dipole-dipole forces

A

Interaction between polar molecules (with partial positive and partial negative) that forms permanent dipole

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13
Q

Alignment of molecules with keesom forces

A

negative pole of one molecule interacts with positive pole of other molecules

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14
Q

Examples of molecules with keesom forces

A

water
hydrochloric acid
alcohol
acetone
phenol

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15
Q

Explain Dipole-induced dipole forces

A

Force between polar molecules and nonpolar molecule
produced by inducing a temporary electric dipole in the nonpolar molecule

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16
Q

Examples of nonpolar molecules that can undergo Debye forces

A

ethyl acetate
methylene chloride
ether

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17
Q

What are london forces?

A

temporary forces between nonpolar molecules

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18
Q

How do london forces form?

A

Attraction that arises due to synchronized fluctuating dipoles in neighboring atoms

fluctuating dipoles is produced due to asymmetry in the electron distribution around the nucleus

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19
Q

Forces responsible for liquefaction of gasses

A

london forces

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20
Q

Example of compounds that can have london forces

A

carbon disulfide
carbon tetrachloride
hexane

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21
Q

What are ion-dipole force

A

Interaction of polar molecules: One molecule with full charge due to ion, and other with a partial charge

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22
Q

Ion-dipole forces in drugs

A

force of attraction between ionized drug molecule and counterion

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23
Q

Ion-induced dipole

A

Force between charged ion and nonpolar molecule

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24
Q

Explain formation of ion-induced dipole

A

results from close proximity between charged ion and nonpolar molecule

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25
Q

Strongest subset of dipole-dipole forces.

A

Hydrogen bonds

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26
Q

What are hydrophobic interactions?

A

forces of attraction between nonpolar atoms and molecules in water

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27
Q

How do hydrophobic interactions form?

A

through disrupting hydrogen bonding network between molecules due to introduction of non-hydrogen bonding nonpolar molecules

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28
Q

Gas characteristics.

A
  • no regular shape
  • capable of filling all available space
  • compressible
  • invisible
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29
Q

Gas: kinetic energy

A

high KE that produces rapid motion

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30
Q

Gas: IMF

A

weak intermolecular forces

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31
Q

What are the important blood gasses?

A

oxygen
carbon dioxide

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32
Q

Liquid characteristics

A
  • occupies definitive volume
  • takes the shape of container
  • flows readily
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33
Q

Liquid compared to gases

A
  • denser than gasses
  • less compressible than gasses
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34
Q

Liquid compared to solids

A

more compressible than solids

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35
Q

List physical properties of liquids

A
  • can be solid (frozen)
  • have boiling points (become gasses)
  • vapor pressure
  • surface tension
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36
Q

Factor affecting vapor pressure

A

temperature only

37
Q

Vapor pressure

A

measure of tendency of a material to change into gas/vapor

38
Q

Explain mechanism of vapor pressure

A

molecules with these break away from surface of liquid and turn into gaseous state:
- highest KE
- closest proximity to surface

39
Q

What are the dimensions of surface tension?

A

force per unit length
dynes cm-1

40
Q

Surface tension relationship with temperature

A

inversely proportional

surface tension decreases with increasing temperature

41
Q

What is surface tension?

A

property of a liquid’s surface to resist external forces

42
Q

Surface tension mechanism.

A
  • surface molecules are attracted inward
  • bulk molecules are attracted in all directions

this creates an unqeual distribution of attractive and repulse forces

43
Q

Solid characteristics.

A
  • has fixed shape
  • nearly incompressible
  • atoms vibrate in fixed positions so there is little translational motion
44
Q

Solid: kinetic energy

A

very little KE

45
Q

Solid: IMF

A

strong IMF

46
Q

What are the types of solids?

A

crystalline
amorphous
polymeric

47
Q

What are the types of crystalline solids?

A

polymorphs
hydrates/solvates
salts/cocrystals

48
Q

What are crystalline solids?

A

Atoms/molecules that arranged in repetitious three-dimensional lattice units infinitely throughout the crystal

49
Q

Seven common lattice units.

A

cubic
tetragonal
orthrombic
rhombohedral
hexagonal
monoclinic
triclinic

50
Q

Lattice system with highest symmetry.

A

cubic system

51
Q

Lattice system with lowest symmetry.

A

triclinic system

52
Q

What lattice system do drugs usually have?

A

Lower-symmetry systems as they are relatively larger compared to inorganic molecules

53
Q

What defines lattice systems?

A

length
angles

54
Q

What are polymorphs?

A

Chemicals (including pharmaceutical agents) that may exist in more than one crystalline structure.

55
Q

Explain the properties of polymorphs.

A

Polymorphs have different physical properties:
melting point
solubility
stability
density
pharmacologic effect

56
Q

How many polymorphic forms does acetaminophen have?

A

3 forms

57
Q

How many polymorphic forms does theophylline have?

A

2 forms

58
Q

Give example of polymorphic crystals.

A

Quartz
cristobalite

59
Q

What are allotropes?

A

Same element in the same physical state but different forms.

60
Q

What causes allotropes?

A

Difference in atomical bonding.

61
Q

What are hydrates?

A

Crystals in which water is included in a lattice

62
Q

What are solvates?

A

Crystals in which a solvent is included in a lattice

63
Q

Solvates as drug substances.

A

Most are not chosen as drug substances due to possible toxicity of common solvents

64
Q

How are salt crystals formed?

A

Two ionized compounds interact in the lattice to form crystalline salt.

65
Q

How do ionized compounds form within a crystal to form salt crystals?

A

pKa difference causes proton transfer from one molecule to another, forming one positively charge and one negatively charged

66
Q

Describe amorphous solid structure.

A

no long-range order over many molecular units to produce a lattic or crystalline structure.

67
Q

Other names of amorphous solids.

A

glasses
supercooled liquids

68
Q

Amorphous solid properties

A
  • no melting point
  • defined by glass transition temperature
69
Q

What is Tg temperature?

A

temperature at which an amorphous material converts from a glass to a supercooled liquid upon heating

70
Q

Stability in amorphous solids vs crystalline solids

A

amorphous solids less physically stable than crystalline due to weak interactions

71
Q

What is amorphous dispersion?

A

stabilized amorphous drug by a polymer/combination of polymers/surfactants

72
Q

What happens when amorphous material is stabilized?

A

solubility increases
physical stability becomes similar to crystalline material

73
Q

Wnhat are polymeric solids?

A

Large molecules formed by covalent bonding of monomers into a chain or network of repeating structural units

74
Q

Give examples of polymeric solids.

A

rubber - polyisoprene
polypeptides
cellulose

75
Q

Function of polymeric solids.

A
  • stabilizes amorphous drug
  • prevent crystallization of amorphous drug upon dissolution
  • used as excipients in solid, semisolids and liquid formulation
76
Q

What is boiling point?

A

temperature at which vapor pressure is equal to atmospheric pressure

77
Q

What is heat of vaporization?

A

Heat absorbed when 1g or 1 mole of liquid is vaporized

78
Q

What is heat of fusion?

A

Heat required to increase the intermolecular distance in the solid state to the liquid state

79
Q

What is eutectic point?

A

lowest temperature at which the existence of liquid phase is possible

80
Q

How is liquefaction of eutectic mixture prevented?

A

mixing eutectic components with other powders

81
Q

What are eutectic mixtures?

A

A mixture that has a lower melting point than its constituents

82
Q

What is the triple point of water?

A

temperature and pressure at which the three phases of a substance coexists in a thermodynamic equilibrium

83
Q

Examples of eutectic mixtures

A

menthol - thymol
phenol - camphor
antipyrine - aspirin

84
Q

Triple point of water: pressure

A

0.006atm

85
Q

Triple point of water: temperature

A

0.01 degrees celsius

86
Q

Relate the relationships between forces and heat of fusion.

A

stronger IMF -> higher molecular weight -> higher heat of fusion -> higher melting point

87
Q

Relate the relationships between forces and heat of vaporization.

A

higher molecular weight -> higher IMF -> higher heat of vaporization -> higher boiling point

88
Q

Describe the relationship between temperature and positive heat of solution

A

increasing temp. = increased solubility

89
Q

Describe the relationship between temperature and negative heat of solution

A

decreased temp. = decreased solubility

PhyPharm (2 decks)

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