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States of matter Flashcards

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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
Strongest subset of dipole-dipole forces.
Hydrogen bonds
26
What are hydrophobic interactions?
forces of attraction between nonpolar atoms and molecules in water
27
How do hydrophobic interactions form?
through disrupting hydrogen bonding network between molecules due to introduction of non-hydrogen bonding nonpolar molecules
28
Gas characteristics.
- no regular shape - capable of filling all available space - compressible - invisible
29
Gas: kinetic energy
high KE that produces rapid motion
30
Gas: IMF
weak intermolecular forces
31
What are the important blood gasses?
oxygen carbon dioxide
32
Liquid characteristics
- occupies definitive volume - takes the shape of container - flows readily
33
Liquid compared to gases
- denser than gasses - less compressible than gasses
34
Liquid compared to solids
more compressible than solids
35
List physical properties of liquids
- can be solid (frozen) - have boiling points (become gasses) - vapor pressure - surface tension
36
Factor affecting vapor pressure
temperature only
37
Vapor pressure
measure of tendency of a material to change into gas/vapor
38
Explain mechanism of vapor pressure
molecules with these break away from surface of liquid and turn into gaseous state: - highest KE - closest proximity to surface
39
What are the dimensions of surface tension?
force per unit length dynes cm-1
40
Surface tension relationship with temperature
inversely proportional surface tension decreases with increasing temperature
41
What is surface tension?
property of a liquid's surface to resist external forces
42
Surface tension mechanism.
- surface molecules are attracted inward - bulk molecules are attracted in all directions this creates an unqeual distribution of attractive and repulse forces
43
Solid characteristics.
- has fixed shape - nearly incompressible - atoms vibrate in fixed positions so there is little translational motion
44
Solid: kinetic energy
very little KE
45
Solid: IMF
strong IMF
46
What are the types of solids?
crystalline amorphous polymeric
47
What are the types of crystalline solids?
polymorphs hydrates/solvates salts/cocrystals
48
What are crystalline solids?
Atoms/molecules that arranged in repetitious three-dimensional lattice units infinitely throughout the crystal
49
Seven common lattice units.
cubic tetragonal orthrombic rhombohedral hexagonal monoclinic triclinic
50
Lattice system with highest symmetry.
cubic system
51
Lattice system with lowest symmetry.
triclinic system
52
What lattice system do drugs usually have?
Lower-symmetry systems as they are relatively larger compared to inorganic molecules
53
What defines lattice systems?
length angles
54
What are polymorphs?
Chemicals (including pharmaceutical agents) that may exist in more than one crystalline structure.
55
Explain the properties of polymorphs.
Polymorphs have different physical properties: melting point solubility stability density pharmacologic effect
56
How many polymorphic forms does acetaminophen have?
3 forms
57
How many polymorphic forms does theophylline have?
2 forms
58
Give example of polymorphic crystals.
Quartz cristobalite
59
What are allotropes?
Same element in the same physical state but different forms.
60
What causes allotropes?
Difference in atomical bonding.
61
What are hydrates?
Crystals in which water is included in a lattice
62
What are solvates?
Crystals in which a solvent is included in a lattice
63
Solvates as drug substances.
Most are not chosen as drug substances due to possible toxicity of common solvents
64
How are salt crystals formed?
Two ionized compounds interact in the lattice to form crystalline salt.
65
How do ionized compounds form within a crystal to form salt crystals?
pKa difference causes proton transfer from one molecule to another, forming one positively charge and one negatively charged
66
Describe amorphous solid structure.
no long-range order over many molecular units to produce a lattic or crystalline structure.
67
Other names of amorphous solids.
glasses supercooled liquids
68
Amorphous solid properties
- no melting point - defined by glass transition temperature
69
What is Tg temperature?
temperature at which an amorphous material converts from a glass to a supercooled liquid upon heating
70
Stability in amorphous solids vs crystalline solids
amorphous solids less physically stable than crystalline due to weak interactions
71
What is amorphous dispersion?
stabilized amorphous drug by a polymer/combination of polymers/surfactants
72
What happens when amorphous material is stabilized?
solubility increases physical stability becomes similar to crystalline material
73
Wnhat are polymeric solids?
Large molecules formed by covalent bonding of monomers into a chain or network of repeating structural units
74
Give examples of polymeric solids.
rubber - polyisoprene polypeptides cellulose
75
Function of polymeric solids.
- stabilizes amorphous drug - prevent crystallization of amorphous drug upon dissolution - used as excipients in solid, semisolids and liquid formulation
76
What is boiling point?
temperature at which vapor pressure is equal to atmospheric pressure
77
What is heat of vaporization?
Heat absorbed when 1g or 1 mole of liquid is vaporized
78
What is heat of fusion?
Heat required to increase the intermolecular distance in the solid state to the liquid state
79
What is eutectic point?
lowest temperature at which the existence of liquid phase is possible
80
How is liquefaction of eutectic mixture prevented?
mixing eutectic components with other powders
81
What are eutectic mixtures?
A mixture that has a lower melting point than its constituents
82
What is the triple point of water?
temperature and pressure at which the three phases of a substance coexists in a thermodynamic equilibrium
83
Examples of eutectic mixtures
menthol - thymol phenol - camphor antipyrine - aspirin
84
Triple point of water: pressure
0.006atm
85
Triple point of water: temperature
0.01 degrees celsius
86
Relate the relationships between forces and heat of fusion.
stronger IMF -> higher molecular weight -> higher heat of fusion -> higher melting point
87
Relate the relationships between forces and heat of vaporization.
higher molecular weight -> higher IMF -> higher heat of vaporization -> higher boiling point
88
Describe the relationship between temperature and positive heat of solution
increasing temp. = increased solubility
89
Describe the relationship between temperature and negative heat of solution
decreased temp. = decreased solubility

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