Term
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Definition
| Anything (except food) administered to the body that has a physiological affect |
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Term
| List the properties of a drug in the order that it affects the next property |
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Definition
| Physical -> chemical -> biological |
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Term
| Give an example of a physical property affecting biological property |
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Definition
Example: physical grinding of wheat has biological properties once
ingested. Too whole is unhealthy (diarrhea), too ground is also unhealthy |
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Term
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Definition
A property that results from the sum of the properties of the individual atoms
Ex. Molar mass |
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Term
| Define constitutive property |
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Definition
| A property that is dependent on the structural arrangement of atoms within the molecule |
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Term
| Define additive-constitutive property |
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Definition
Constitutive properties with some additivity
Most of the physical properties of a molecule are party additive and party constitutive |
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Term
| How do atoms respond to EMR? |
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Definition
| By translocating electrons to the next orbital |
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Term
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Definition
| A drug for TB that can be seen physically in urine as a red color |
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Term
| What is the relationship between wavelength and frequency? |
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Definition
| They are inversely related |
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Term
| What is the relationship between wavelength and wavenumber? |
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Definition
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Term
| If you increase wavelength, do you increase or decrease photon energy? |
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Definition
| Decrease photon energy, they are inversely related |
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Term
| What is the relationship between mass and wave energy? |
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Definition
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Term
| Give the equation for energy |
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Definition
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Term
| Define excitation of an electron |
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Definition
| Light (hv) exciting an electron to the next orbital level |
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Term
| Define ionization of an electron |
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Definition
| When light energy(hv) is so large that the electron is knocked out of the electron orbital |
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Term
| What is the Rydberg constant? |
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Definition
For a hydrogen atom at ground state, the energy of an electron
-109,700cm-1 |
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Term
| When does electronic transition happen? |
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Definition
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Term
| When does vibrational transition happen? |
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Definition
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Term
| When does rotational transition happen? |
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Definition
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Term
| When do low energy transitions happen? |
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Definition
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Term
| What are the allowed transitions in molecules absorbing wavelength light? |
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Definition
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Term
| What dictates the region of the spectrum in which absorption can take place? |
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Definition
| The types of electronic orbitals present in the ground state |
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Term
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Definition
| Parts of a molecule responsible for UV or visible absorption |
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Term
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Definition
| The magnitude of light absorption (A) is directly proportional to the concentration of the absorbing substance (c) and the thickness of the sample (pathlength, l) |
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Term
| What is the equation that represents Beer's law? |
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Definition
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Term
| Define (a) as in Beer's law |
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Definition
| Absorbtivity of the chemical species, abosrbitivity of 1 M concentration is called molar Absortivity Ɛ (L mole-1 cm-1) |
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Term
| Describe how a spectrometer basically works |
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Definition
| A source is split into different waves and then mirrored into a reference (darker) and a sample before going through to the receptor |
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Term
| What is the different between fluorescence and phosphorescence? |
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Definition
| Fluorescence is short time emission (a microsecond to a nanosecond), phosphorescence is longer time |
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Term
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Definition
| Absorption of light to reach an excited state and then emission of light in returning to ground state |
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Term
| Mathematically, how is photoluminescence expressed? |
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Definition
| S*=flourescence, T*=phosphorescence |
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Term
| Why is it important for pharmacists to know acid/base chemistry? |
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Definition
| "Several drugs and pharmaceutical ingredients are weak electrolytes. Their degree of ionization is an important feature and has several applications starting from drug formulation to pharmacological effects shown in the body." |
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Term
| Give some examples of drugs that are weak bases |
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Definition
| Morphine, scopdamine, and the active ingredients in some inhalers |
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Term
| Define acid vs base according to the Arrhenius theory |
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Definition
| An acid is a substance that dissociates in water to give hydrogen ions (H+), and a base is a substance that dissociates in water to give hydroxide ions (OH-). |
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Term
| What is the proper name for (OH-) ? |
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Definition
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Term
| What happens to the hydrogen an acid produces in water? |
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Definition
| It combines with water molecules to form hydronium ion (H3O+) |
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Term
| What are some limits to the Arrhenius definition of acid/base? |
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Definition
It limits acid-base relations to aqueous solution.
Also, some bases such as ammonia (NH3) do not contain an OH group in them, but their dissociation in water produces hydroxide ions. |
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Term
| Define acid/base according to the Bronsted-Lowry concept |
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Definition
| An acid is a proton donor and a base is a proton acceptor. |
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Term
| Define conjugate acid-base pair |
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Definition
| The reactants (acid and base, respectively) become the products and switch roles to become the conjugate base and conjugate acid, respectively |
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Term
| Is water an acid or a base? |
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Definition
| It can act as either, demonstrating that a molecule is defined as an acid or a base depending on the reaction |
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Term
| What defines how strong an acid or a base is? |
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Definition
| The greater the tendency of an acid to lose a proton, the stronger it is, and greater the tendency of a base to accept the proton, the stronger it is. |
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Term
| Define acid/base according to the Lewis concept |
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Definition
| An acid is an electron pair acceptor and a base is an electron pair donor. |
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Term
| How can BCl3 be considered an acid when it doesn't have a hydrogen? |
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Definition
| According to the Lewis definition of acid, it accepts electrons in a reaction with NH3 and is therefore acidic |
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Term
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Definition
When a substance has the ability to act either as acid or base, depending on the situation, it is called amphoteric
Such property is called amphoterism. |
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Term
| Give some examples of an amphoteric molecule |
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Definition
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Term
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Definition
An amphiprotic molecule can either donate or accept a proton, thus acting either as an acid or a base.
Essentially amphoteric, but specifically the ability to accept/give up hydrogen makes it amphiprotic |
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Term
| Give some examples of amphiprotic molecules |
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Definition
| Water, ammonia, certain amino acids, HSO4- and HCO3- |
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Term
| Are all molecules that are amphoteric amphiprotic? |
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Definition
| No, only the amphoterics that accept/give up hydrogen(protons) |
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Term
| If an acid/base is defined as "strong," how dissociated will it be in water? |
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Definition
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Term
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Definition
No, because it has no hydrogen to give up
However, it is amphoteric |
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Term
| Which definition of acids/bases can incorporate defining conjugate acid and conjugate base? |
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Definition
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Term
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Definition
| A quantitative measure of the dissociation of weak acids and bases |
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Term
| Give a formula that relates pH to [H+] |
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Definition
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Term
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Definition
The ion product constant of water, 10-14
Kw=[H+][OH-]= 10-14
Kw=Kax Kb= 10-14 |
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Term
| Give the equation that relates pH to pKa and [C] of a weak acid |
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Definition
| pH= 1/2 pKa - 1/2 log [C] |
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Term
| What is the Henderson-Hasselbach equation for a weakly acidic drug? |
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Definition
pH= pKa + log ([ionized]/[unionized])
or
pH= pKa + log ([base]/[acid])
or
pH= pKa + log ([salt]/[acid]) |
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Term
| Would a larger Ka indicate more or less dissociation? |
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Definition
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Term
| Would a larger pKa indicate more or less dissociation? |
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Definition
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Term
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Definition
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Term
| What is the Henderson-Hasselbach equation for a weakly basic drug? |
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Definition
pH= pKa + log ([unionized]/[ionized])
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Term
| Give the equation that relates pH to pKa and [C] of a weak base |
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Definition
| pH= 1/2 pKw + 1/2 pKa + 1/2 log [C] |
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Term
| Give an example of a buffer system |
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Definition
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Term
| What buffer systems does the blood have? |
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Definition
| Hemoglobin, bicarbonate, phosphate, plasma |
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Term
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Definition
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Term
| How effective are buffers? |
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Definition
| Effective only for small quantities added |
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Term
| What are buffers normally composed of? |
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Definition
A weak acid and its conjugate base
(Can be a weak base and its conjugate acid, but not as common) |
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Term
| If [salt]=[acid], without doing any math, what do you know about the solution? |
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Definition
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Term
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Definition
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Term
| How do you get mol fraction from the mol ratio? |
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Definition
| mol fraction = (ratio)/(1+ratio) |
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Term
| What two things affect the pH of a buffer solution? |
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Definition
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Term
| When does the maximum buffer capacity occur? |
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Definition
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Term
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Definition
| Osmotic pressure exerted by salts in aqueous solution |
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Term
| What is the difference between isotonic and isosmotic? |
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Definition
Isotonicity refers to physiological osmotic pressure.
Isosmotic solutions are only isotonic if they are isosmotic to the body. |
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Term
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Definition
| Equal osmolarity to the human body physiology |
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Term
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Definition
| Two solutions with equal tonicity |
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Term
| Describe the osmotic pressure of body fluids in relation to sodium chloride |
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Definition
| Body fluids have osmotic pressure about equal to .9% sodium chloride solution |
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Term
| Why would we give a patient a hypertonic NaCl solution for the eye? |
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Definition
| If the patient had corneal edema, it could reduce the swelling by pulling the water out |
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Term
| If you give a .6% sodium chloride solution to the eye, will the eye swell from the hypotonic solution? |
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Definition
| No, the eye can tolerate a range of sodium chloride from around .5-1.8% |
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