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Physical Pharmacy > States of Matter > Flashcards

States of Matter Flashcards

1
Q

Cohesion and adhesion are manifestations of_____ bonding.

A

Intermolecular

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2
Q

A system is more stable at what point

A

When the repulsive and attractive forces are in equilibrium

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3
Q

What governs The balance of forces between two molecules

A

governed by the negatively charged electron clouds of the molecules.

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4
Q

relates to NON IONIC interaction between molecules

A

Van Der Waal forces

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5
Q

Give eg of PERMANENT van der wall dipoles

A 
Keesom forces(dipole-dipole) eg.
Peptide bonds and HCl intermolecular bonds
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6
Q

What are Debye forces

A

Induced dipole interactions

Eg. Condensation of non polar gas to for liquids or solids

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7
Q

Relationship between potential energy and distance btn molecules

A

Potential energy is inversely proportional to the distance of separation raised to the power 6

P.E=k 1/d^6

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8
Q

What interaction shows the ability of a permanent dipole to polarise a neighbouring non polar molecule (which are easily polarisable)

A

Debye forces or dipole induced dipole.

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9
Q

What are London forces and eg

A

induced dipole induced dipole attraction

two neighbouring non polar neutral molecules induce partial charge distribution

Eg. conceptualise aliphatic chains in the lipid core of a biologic membrane
Found in Noble gases, diatoms ( O2, H2,N2) and others- Ch4

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10
Q

What interactions account partly for the solubility of ionic crystalline structure in water

A

Ion dipole interactions
Eg, NaCl and Water

cation Na+ attracts the relatively charged negative oxygen and the anion Cl- attracts the hydrogen atoms of the dipolar water molecules.

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11
Q

interaction that involves charged moieties.

A

Ion ion interactions or ionic bonds

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12
Q

Weaker ion-ion interactions in salt forms are eg of what interaction

A

Ion ion interaction

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13
Q

The interaction of a hydrochloride salt of a drug and

salt bridge between counter ions in protein molecules exhibit what interactions

A

i) Ion ion interaction that is intermolecular

ii) intermolecular ion ion

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14
Q

What properties of pharmaceutical agents does the strength of ion ion interaction have profound effect

A

pka, pH, solubility

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15
Q

Interaction between a molecule containing hydrogen and a strong electronegative atom (F, O, N)

A

H bonding

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16
Q

Who discovered H bonds

A

latimer and Rudebush in 1920

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17
Q

Hydrogen bonds can exist between alcohol molecules, carboxylic acids, aldehydes, esters and polypeptides

T or F

A

True

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18
Q

solids with high vapour pressure upon heating undergo?

A

Sublimation

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19
Q

What are ideal gases

A
  1. No molecular interaction exist between molecules

2. Collisions perfectly elastic

20
Q

Boyle’s law

A

P α 1/v, PV =k

21
Q

Gay lussac and Charles Law

A

V α T, V =Kt

22
Q

Combined gas law

A

P1V1/T1= P2V2/T2

23
Q

Change Celcius to Kelvin

A

Kelvin = Celsius + 273.15.

24
Q

general ideal gas law

A

PV = nRT …… 5

25
Q

Why is the general ideal gas law called equation of state of an ideal gas

A

because it relates pressure, volume and temperature of a given mass of gas

26
Q

How do you find the molecular weight of a gas with the ideal gas law

A 
n = m/M, replacing n in the formula PV = nRT = mRT/M
M = mRT/PV
27
Q

Equation for real gas

A

Page 23

28
Q

What is critical temperature

A

temperature when exceeded no amount of pressure can cause the gas to liquify.

29
Q

What is critical pressure

A

The pressure required to liquify a gas at the critical temperature

30
Q

What is highest vapour pressure liquid can have.

A

Critical pressure

31
Q

What is the critical temp and pressure of water and helium

A

Critical temp for water 647K at critical pressure of 218atm,

that of Helium is 5.5k, 2.26atm

32
Q

the gas phase of substance that is normally liquid at room temperature

A

Vapor

33
Q

What variable affects vapor pressure

A

Temperature only

As T increases Vo increases

34
Q

When vapour pressure is equal to atmospheric pressure what happens

A

, there is boiling.

35
Q

State the Clausius- Claypeyron equation

A

log 𝑃2 /P1= ∆𝐻𝑣 𝑇2−𝑇1/
2.303𝑅𝑇1𝑇2

Hv is the molar heat of vaporization, that is, the heat absorbed by 1 mole of liquid when it passes into the vapor state.

36
Q

Solids are incompressible

T or F

A

True

37
Q

Morphology of crystalline form of a solid is called____

A

crystal habit

38
Q

What are the 6 crystal systems

A

Cubic – sodium chloride
Tetragonal – urea
Hexagonal – iodoform
Rhombic – iodine Monoclinic – sucrose Triclinic – Boric acid

39
Q

How does carbon show polymorphism

A

diamond in a cubic (tetrahedral lattice arrangement)

Graphite in sheet of a hexagonal lattice

40
Q

When change from one polymorphic form to the other is reversible , the compound is called___

A

enantiotropic

41
Q

If the change of one polymorphic form to another is just in one direction it is called –.

A

monotropic

42
Q

Characteristics of a stable polymorphic form of a solid and metastable( unstable)

A

Stable polymorph represents the lowest energy state, has highest melting point and least aqueous solubility.

Metastable form represent the higher energy state, have lower melting point and high aqueous solubility

43
Q

How do metastable form convert to stable

A

Metastable form converts to the stable form due to their higher energy state.

44
Q

What polymorphic form shows better bioavailability and therefore preferred in formulations.

A

Metastable

45
Q

What are solvates

A

solvent traces in the crystal lattice formed when crystallization occurs.

It forms part of the crystal lattice and affects its properties

46
Q

What are amorphous solids

A

They differ from crystalline solids in that they tend to flow when subjected to sufficient pressure over a period of time, and they do not have definite melting points.

47
Q

Give an eg of how a drug being amorphous or crystalline affects its therapeutic activity.

A

crystalline form of the antibiotic novobiocin acid is poorly absorbed and has no activity, whereas the amorphous form is readily absorbed and therapeutically active. This is due to the differences in the rate of dissolution

Physical Pharmacy (4 decks)

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