M5 TTS

Transfer of Electron

Ionic

Equal sharing of electron

Nonpolar covalent bond

Unequal sharing of electron

Polar covalent bond

Metal + Nonmetal

Ionic

Alloy formation

Metallic bond

Keesom, Debye and London forces

Van der Waals

Solubility of ionic crystals in water

Ion-dipole

Formation of iodide complex, which accounts for the solubility of iodine in KI solution.

ion-induced dipole

Accounts for the unusual properties of water (high dielectric constant, abnormally low vapor pressure and high BP)

Hydrogen bonds

Forces necessary to cohere and forces necessary to prevent molecular interpenetration.

Repulsive attractive forces

Weak electrostatic force that brings about condensation of nonpolar gas molecules

Van der Waals

Characteristic frequency, wavelength or wavenumber

Electromagnetic radiation

Non-ionic phenomenon wherein the molecule has no net charge

Permanent dipole moment

Measurement of the angle of rotation

Optical rotation

n= sin i / sin r

Refractive index

Absorption spectroscopy based on differential absorption of left or right circularly polarized light.

Circular dichroism

Law of thermodynamics where energy is transferred or transformed or interconverted

First law of thermodyamics

Defines the law of conservation of energy

First law of thermodyamics

Defines Entropy (S)

Second Law of thermodynamics

Entropy never decreases

Second Law of thermodynamics

The entropy of a pure substance is zero when that substance is in a physical state

Third Law of thermodynamics

A measure of chemical energy. Represents the combined contribution of enthalpy and entropy

Gibb’s Free energy

Identify the weak intermolecular forces, examples of which are the Keesom-Debye, and London forces.

A. Ion-dipole, ion-induced dipole forces

B. Van der Waals forces

C. Hydrogen bonds

D. Repulsiveandattractiveforces

B. Van der Waals forces

Identify the forces that account in part for the solubility of ionic crystalline substances in water and are presumed to account for the solubility of iodine in a solution of KI.

A. Hydrogen bonds

B. Repulsive and attractive forces

C. Ion-dipole, ion- induced dipole forces

D. Electrovalentforces

C. Ion-dipole, ion- induced dipole forces

Identify the weak electrostatic forces that bring about condensation of nonpolar gas molecules to form liquids and solids when molecules are bought quite close to one another.

A. Hydrogen bonds

B. Van der Waals forces

C. Ion-dipole, ion-induced dipole forces

D. Repulsiveandattractiveforces

B. Van der Waals forces

Identify the Law/ Principle which states that when the reaction is reversible, delta S=0.

A. Gibbs Free Energy

B. Ideal Gas Law

C. Henry’s Law

D. Faraday’sLaw

A. Gibbs Free Energy

Identify the statement/mathematical expression, which does NOT express the First Law of Thermodynamics.

A. States that energy is conserved

B. Forms of energy can be interconverted, but the sum of energies remains

constant

C. ∆E is equal to zero for a cyclic process in a closed system.

D. ∆E=EB+EA

D. ∆E=EB+EA

Select the concept that explains the thermodynamics state of a perfect crystal at absolute zero.

A. 3rd Law of Thermodynamics

B. 2nd Law of Thermodynamics

C. 1st Law of Thermodynamics

D. 1st, 2nd, 3rd Laws of Thermodynamics

A. 3rd Law of Thermodynamics

If 0.55 g of a gas dissolves in 1.0 L of water at 2 atm of pressure, how much will dissolve at 4.5 atm?

A. 1.24

B. 0.55

C. 0.01

D. NOTA

A. 1.24

A 600 mL sample of nitrogen is warmed from 200K to 273K. Find its new volume if the pressure remains constant.

A. 150 mL

B. 500 mL

C. 819 mL

D. NOTA

C. 819 mL

According to Boyle's Law, the volume of a gas has an inverse relationship with ____.

A. Moles

B. Temperature

C. Pressure

D. Weight

C. Pressure

What term describes the solubility of a substance when 800 mg of solute can dissolve in 95 mL of water?

A. Slightly soluble

B. Soluble

C. Sparingly soluble

D. Practically insoluble

A. Slightly soluble

<1

Very Soluble

1-10

Freely Soluble

10-30

Soluble

30-100

Sparingly Soluble

100-1000

Slightly Soluble

1000-10000

Very Slightly Soluble

> or = 10000

Practically insoluble

Select the statement that BEST describes the solubility of solids in liquids.

A. The solubility of a solid in an ideal solution depends on the temperature, melting point of the solid, and molar heat of fusion.

B. Ideal solubility is affected by the nature of the solvent.

C. In an ideal solution, the heat of fusion is NOT

equal to the heat of solution.

A. The solubility of a solid in an ideal solution depends on the temperature, melting point of the solid, and molar heat of fusion.

Find the statement that is INCORRECT regarding the influence of some factors on the

solubility of solids.

A. The configuration of a solid molecule has NO effect on its solubility.

B. A symmetric arrangement in the crystal may render a solid less soluble than unsymmetric one.

C. Solubility depends in part on the work required to separate the particles of the crystalline solute.

D. Solubility increases with decreasing particlesize.

A. The configuration of a solid molecule has NO effect on its solubility.

Colligative properties depend primarily on which of the following:

a. The identity of the solute

b. the size of the solute particles

c. the concentration of solute particles in a solution

d. the temperature of the solution

c. the concentration of solute particles in a solution

A hypertonic solution is expected to freeze at what temp?

below zero degrees celsius

At what temp will an isotonic solution freeze?

-0.52 degree celsius

Freezing point of water

0 degree celsius

Which of the following statements about boiling point elevation is true?

a. It occurs when a non-volatile solute is added to a solvent

b. It occurs when a volatile solute is added to a solvent

c. It is independent of the concentration of the solute

d. It decreases the vapor pressure of the solvent

a. It occurs when a non-volatile solute is added to a solvent

If 1 mol of a non-volatile, non-electrolyte solute is dissolved in 1 kg of water, what is the expected freezing point of the solution? (Assume the freezing point depression constant for water is 1.86 oC/molal.)

a. -1.86 oC

b. 3.72 oC

c. -0.93 oC

d. 0 oC

a. -1.86 oC

Calculate the amount of NaCl (in mg) needed to make 60mL of an isotonic solution containing 0.15g of Drug A (D1%=0.070OC)

522 mg

Calculate the approximate E value of boric acid. (MW 61.84, Liso 1.8)

A. 0.6

B. 0.5

C. 0.8

D. 0.7

B. 0.5

A prescription requires 100 mL of a 1 percent solution of apomorphine hydrochloride (MW 312.79) that is isotonic with blood serum. The freezing point lowering of the drug is 0.08 degrees C and that of 1 percent sodium chloride is 0.58 degrees C. how many grams of sodium chloride will be added to make 100 mL of isotonic solution?

A. 0.44 g

B. 0.76 g

C. 0.88 g

D. 0.52g

B. 0.76 g

Substance that resist change in pH

Buffers

Governs buffer system

Buffer Equation

Other name of Buffer System

Henderson-Hasselbalch equation

HLB Value of Antifoaming activity

1-3

HLB value of Emulsifiers (w/o)

3-6

Wetting agents

7-9

Emulsifiers (o/w)

8-18

Solubilizers

15-20

Detergents

13-16

The difference between work of adhesion (Wa) and work of cohesion (Wc)

Spreading coefficient

If the surface tension of water γS is 72.8 dynes/cm at 20°C, the surface tension of benzene, γL, is 28.9 dynes/cm, and the interfacial tension between benzene and water, γLS, is 35.0 dynes/cm, Following equilibration, γS′ is 62.2 dynes/cm and γL′ is 28.8 dynes/cm. What is the final spreading coefficient?

A. – 1.6 dynes/cm

B. + 1.6 dynes/cm

C. + 8.9 dynes/cm

D. – 8.9 dynes/cm

A. – 1.6 dynes/cm

The difference in potential between the actual surface and the electroneutral region.

Nernst Potential

Resistance of the surface to an expansion in area

Surface tension

Scale of values by means of which it is possible to establisharangeofoptimumefficiencyforeachclassof surfactants

HLB

Molecules or ions that are adsorbed at interfaces

Surfactant

The difference between work of adhesion and work of cohesion

Spreading coefficient

Wetting agents allows contact between solid and liquid particles

True

Emulsifiers increase tension between oil and water.

False

Detergents reduce tension and aid in wetting the surface and the dirt

True

Solubilizers have HLB value of 0-40

False

Find the antifoaming agent.

A. Sodium stearate

B. Dodecyl sulfate

C. Polysorbate 20

D. Castor oil

D. Castor oil

Analyze and identify the arbitrary scale of values by means of which it is possible to establish a range of optimum efficiency for each class of surfactant.

A. Surface potential

B. Zeta potential

C. Nernst potential

D. Hydrophilic-lipophilicBalance

D. Hydrophilic-lipophilicBalance

Select the INCORRECT statement about the HLB system.

A. Each surface-active agent is assigned an HLB value which is indicative of the substance's polarity.

B. HLB values range from 1-40.

C. Substances that are highly polar or hydrophilic have been assigned higher numbers.

D. In using the HLB concept in the preparation of an emulsion,one selects emulsifying agents having higher or lower HLB values as the oleaginous phase of the emulsion.

D. In using the HLB concept in the preparation of an emulsion,one selects emulsifying agents having higher or lower HLB values as the oleaginous phase of the emulsion.

Select the INCORRECT statement about Surfactants.

A. Wetting agents aid in attaining intimate contact between solid particles and

liquids.

B. Detergents reduce the surface tension and aid in wetting the surface and the dirt.

C. Surface-active agents with HLB values 3-6 are greatly lipophilic and produce water-

in-oil emulsion.

D. The usual range of HLB values for surfactants used as solubilizing agents isbetween 1-3.

D. The usual range of HLB values for surfactants used as solubilizing agents isbetween 1-3.

Identify which statement is correct about adsorption and absorption.

A. When molecules and ions are partitioned in favor of the interface, the

phenomenon is called negative adsorption.

B. When the molecules of a liquid or gas penetrate into the capillary spaces of the medium, this phenomenon is called absorption.

C. An example of adsorption is the taking up of water by a sponge.

D. An example of absorption is the concentrating of alkaloid molecules on the surface of clay.

B. When the molecules of a liquid or gas penetrate into the capillary spaces of the medium, this phenomenon is called absorption.

Choose which statement is NOT true regarding the adsorption at solid interfaces.

A. The degree of adsorption of a gas by a solid depends solely on the chemical nature

of the adsorbent and the adsorbate.

B. The principle of solid-liquid adsorption is employed in a decolorizing solution,

adsorption chromatography and wetting.

C. The principle of adsorption is used when activated charcoal and acetylcysteine are

used in the treatment of acetaminophen poisoning.

D. The adsorption of gases by a solid finds application in the removal of objectionableodors from rooms and food using charcoal.

A. The degree of adsorption of a gas by a solid depends solely on the chemical nature

Determine the contact angle exhibited by complete nonwetting.

A. 0°

B. 45°

C. 90°

D. 180°

D. 180°

Identify the terminology which refers to the difference between work of adhesion and work of cohesion.

A. Surface tension

B. Spreading coefficient

C. Hydrophilic-Lipophilic Balance

D. Surfactant

B. Spreading coefficient

Have definite geometric shapes

Crystalline solids

NaCl

Cubic

Urea

Tetragonal

Iodine

Rhombic

Sucrose

monoclinic

Boric acid

triclinic

Iodoform

hexagonal

Absorbs moisture then dissolves

Deliquescence

Absorbs moisture but does not dissolve

Hygroscopic

Water of hydration (crystallization) removal

Efflorescence

Desiccants are examples of

hygroscopic

CuSO4.7H2O → Anhydrous

Efflorescence

Study of small particles

Micrometrics

Coulter counter

Electrical resistance

Sieving

Mesh number

Gelman counter

Farady-Tyndall effect

HIAC/Royco apparatus

Light blockade

Andreasen app (with pipet)

Stoke’s Law

Governs sedimentation rate

Stoke’s Law

Select the Non-Newtonian liquids

A. Virgin coconut oil, Gold Colloid

B. Tobramycin, Chloramphenicol Palmitate Suspension

C. Olive Oil, Chloroform

D. Ethylalcohol,Mayonnaise

B. Tobramycin, Chloramphenicol Palmitate Suspension

Select the viscometers which can be used for both the Newtonian and Non- Newtonian system.

A. Cone and Plate, Capillary

B. Cup and Bob, Cone and Plate

C. Cone and Plate, Falling Sphere

D. Capillary,FallingSphere

B. Cup and Bob, Cone and Plate