[IPS1] PhyPharm SUPER CRAM REVIEWER

Drug product

- a finished dosage form that contains an active drug ingredient (palatable, convenient, safe, and effective)

Ionic/electrovalent Bonds, Covalent Bonds, Metallic Bonds, Hydrogen Bonds

Examples of Intramolecular Forces (4)

Van der Waals, Ion-Dipole, Ion-induced dipole Interaction, Hydrogen Bonds

Examples of Intermolecular Forces (4)

Hydrogen Bonds

This bond can be both intermolecular and intramolecular

Cohesive forces

Attractive forces between like molecules

Adhesive forces

Attractive forces between unlike molecules

Van der Waals Forces

[Intermolecular Forces] Non-ionic but charge-charge interactions

Keesom Forces; Debye Forces; London Forces

[Intermolecular Forces] Three Van der Waals Forces

Keesom Forces

[Van der Waals] orientation/alignment effect

Keesom Forces

[Van der Waals] Dipole-dipole forces

Keesom Forces

[Van der Waals] Polar molecule + Polar molecule

Keesom Forces

[Van der Waals] Ex. water, alcohols, acetone

Debye Forces

[Van der Waals] induction effect

Debye Forces

[Van der Waals] Dipole-Induced dipole forces

Debye Forces

[Van der Waals] Polar molecule + Nonpolar molecule

Debye Forces

[Van der Waals] ether, ethyl acetate

London Forces

[Van der Waals] Dispersion Forces

London Forces

[Van der Waals] Induced dipole-Induced dipole

London Forces

[Van der Waals] Originate from molecular vibrations

London Forces

[Van der Waals] Non-polar + Nonpolar

London Forces

[Van der Waals] Ex. hexane, CCl4

Ion-dipole Forces

[Intermolecular Forces] (+/-) charged ion + Polar

Ion-dipole Forces

[Intermolecular Forces] Ex. Quaternary ammonium + Tertiary amine

Ion-dipole Forces

[Intermolecular Forces] Solubility of salts in water

Ion-Induced Dipole

[Intermolecular Forces] (+/-) charged ion + Non-Polar

Ion-Induced Dipole

[Intermolecular Forces] Ex. Iodine + KI (formation of tri-iodide complex)

Hydrogen Bonds

[Intermolecular Forces] Hydrogen + strongly EN atom (F, S, O, N)

Hydrogen Bonds

[Intermolecular Forces] Unique type of Dipole-Dipole

Water, Alcohol, Carboxylic Acids, Esters, Aldehydes

[Intermolecular Forces] Functional Groups that have hydrogen bonds (5)

Ether and Ketones

[Intermolecular Forces] Two Functional Groups with NO hydrogen bonds

HIGH dielectric, LOW vapor pressure, HIGH BP

[Intermolecular Forces] Hydrogen bonds are responsible for the unusual properties of water such as (1) (High/Low) dielectric constant, (2) (high/low) vapor pressure, and (3) (high/low) boiling point

proteins (as a helices and b pleated sheets), and in nucleic acids (in DNA base pairs, A-T, and G-C)

[Intermolecular Forces] Hydrogen bonds can exist intramoleuclarly in _________ and in __________

A-T = 2 H bonds, G-C = 3 H bonds

How many h bonds have A-T and G-C have

London Dispersion < Dipole-Dipole < Hydrogen Bonding

Arrange the ff. IMFA according to increasing bond strength: London Dispersion, Hydrogen Bonding, Dipole-Dipole

Hydrophobic Forces

[Intermolecular Forces] Nonpolar + water

Deposition

Gas to solid

Sublimation

Solid to Gas

Boyle's Law

[Gas Laws] P and V have an inverse relationship at constant T

Charles' Law

[Gas Laws] V an T have a direct relationship at constant P

Gay-Lussac's Law

[Gas Laws] P and T have a direct relationship at constant V

Avogadro's Law

[Gas Laws] States that equal volume of mass at the same temperature and pressure contain the same number of molecules

6.02 x 10^23

Avogadro's number

0.08205 L*atm/Mol*K

Molar Gas Constant (R) value

273.15 K

Standard Temperature (0 deg C) in Kelvin

760 mmHg

Standard Pressure (1 atm) in mmHg/torr

Kinetic Molecular Theory (KMT)

This theory explains the behavior of gases; it supports the validity of gas laws

Perfect

According to KMT, gas molecules exhibit (partial/perfect) elasticity, causing gas pressure when molecules collide with the walls of the container.

Directly

According to KMT, the Average KE of gas particles is (directly/inversely) proportional to K

Real gases

(Real/Ideal) gases are said to have finite volume and tend to attract one another, as stated by van der Waals Equation

Dalton's Law of Partial Pressure

A law that states that the total pressure of a system is the sum of individual partial pressures of each component

Graham's Law

A law that states that the speed of diffusion of a gas is relative to the molecular weight of density of the gas

Raoult's law

A law that states that the partial vapor pressure of each volatile constituent is equal to the vapor pressure of the pure constituent multiplied by its mole fraction in the solution

Henry's Law

A law that states that the solubility of a gas is directly proportional to the pressure at constant temperature

Clausius-Clapeyron equation

The relationship between the vapor pressure and the absolute temperature of a liquid is exhibited in this equation

Van der Waals

He stated that real gases are not composed of infiinitely small and perfectly elastic non-attracting spheres

Pure Covalent

[Bond Type] EN Difference: < 0.4

Polar Covalent

[Bond Type] EN Difference: < 0.4-1.7

Ionic

[Bond Type] EN Difference: > 1.7

Higher polarity

[Polarity] Higher EN Difference = (lower/higher) polarity

DIPOLE moment

[Polarity] A large EN difference creates a ____________ moment between atoms, increasing polarity

ZERO dipole moments

[Polarity] Non-polar molecules with perfect symmetry have _______ dipole moments (e.g. CO2, CCl4)

NONZERO dipole moments

Polar molecules that are asymmetric have ________ dipole moments (e.g. HCl, H2O, NH3)

3-4 x 10^-8 cm

The distance at which attractive and repulsive forces are equal

Less KE

Liquids possess (more/less) kinetic energy than gases

Equilibrium Vapor Pressure

the pressure of the saturated vapor above the liquid

Directly

Temperature is (directly/inversely) proportional to vapor pressure

Critical temperature

Temperature above which liquid no longer exist

Critical pressure

Pressure required to liquefy a gas at critical temperature

CT = 647 K (374 deg C); CP = 218 atm

CT and CP of Water

Aerosol

A suspension of fine solid particles or liquid droplets in a gas

HIGH pressure, LOW temperature

A gas can be liquefied at (high/low) pressure in a closed chamber and (high/low) temperature

Equilibrium vapor pressure

The pressure of the saturated vapor above the liquid

Elevated = Lower VP = Lower BP

Elevated places = (lower/higher) VP = (lower/higher) BP

Boiling point

The temperature at which the vapor pressure of a liquid is equal to the pressure of the surrounding environment (VP = P atm)

Latent Heat of Vaporization

heat absorbed when liquid vaporizes at normal BP

Clausius-Clapeyron Equation

An equation exhibiting the relationship of vapor pressure and absolute temperature of liquid

Increases

For HC, simple ROH and RCOOH, a higher MW or longer chains of structures (increases/decreases) the compound's boiling point

Decreases

For HC, simple ROH and RCOOH, structure branching (increases/decreases) the compound's boiling point

London forces

Non-Polar molecules have low BP and molar heat of vaporization due to _______________

H-bonds

Polar molecules have high BP and molar heat of vaporization due to ________________

Crystalline solid

[Crystalline vs. Amorphous] Fixed geometric pattern

Crystalline solid

[Crystalline vs. Amorphous] Definite MP

Crystalline solid

[Crystalline vs. Amorphous] Anisotropic

Crystalline solid

[Crystalline vs. Amorphous] Less Soluble

Crystalline solid

[Crystalline vs. Amorphous] Polymorphs, hydrates, solvates, salts

Amorphous solids

[Crystalline vs. Amorphous] Randomly arranged molecules

Amorphous solids

[Crystalline vs. Amorphous] No definite MP

Amorphous solids

[Crystalline vs. Amorphous] Isotropic

Amorphous solids

[Crystalline vs. Amorphous] more soluble

Polymeric

A type of solid that can exhibit both crystalline and amorphous characteristics

cubic

[Crystalline Structure Type] sodium chloride

tetragonal

[Crystalline Structure Type] urea

hexagonal

[Crystalline Structure Type] iodoform

rhombic

[Crystalline Structure Type] iodine

monoclinic

[Crystalline Structure Type] sucrose

monoclinic

[Crystalline Structure Type] Ritonavir (I)

triclinic

[Crystalline Structure Type] boric acid

Orthorhombic

[Crystalline Structure Type] Ritonavir (II)

Solvate

complex formed when solvent is incorporated within the crystal lattice

Hydrate

A solvate, but water is used as the solvent