MODULE 1

arsenic

non-essential ion used for leukemia; treatment for trypasonomiasis, and amoebiasis

Nitrates (NO3)

preservative

Mn(OH)2 to MnO2.H2O White to light brown ppt

product of reaction between NH4OH and Mn+2

basic solutions

salt with strong base + weak acid; will hydrolyze

Chlormerodin Hg 197 and Hg 203

scintillating scanning of the kidneys and brain

linear

shape of non-polar molecule

Solute

substance(s) present in smaller amount(s)

calamine (ZnO.xFe2O3)

type of protective; pink color, Fe2O3 for better cosmetic acceptability

Silver

"Argentum", "Shining", "Bright" Oligodynamic property (germicidal action) Toxicity: Argyria Antidote: NSS

Magnesium Citrate (Mg3(6H5O7))

"Lemonada purganti" Laxative, saline cathartic

100% ionic character

% ionic character in ionic bonds

Bismuth

"Beautiful Meadow", "Silvering Mirror" Astringent, antiseptic, internal protective for ulcer Soluble bismuth compounds are poisonous Causes dark stool, blue-black gums Antidote: BAL/Dimercaparol

Mercurous Chloride (Hg2Cl2)

"Calomel" Cathartic, local antiseptic

Potassium Hydroxide

"Caustic potash", "Lye potash" Saponifying agent (Soft Soap)

Sodium Hydroxide

"Caustic soda", "Sosa", "Lye" Saponifying agent

Ferrous Carbonate (FeCO3)

"Chalybeate Pills", "Ferrunginous Pills" Use: Hematinic

Sodium Nitrate

"Chile Salt Peter", Preservative

Chlorine as Chloride (Cl-)

"Dephlogisticated muriatic acid" Most abundant extracellular anion Used as water disinfectant, gas has bleaching and antiseptic properties

precipitation

"Double Displacement"/"Metathesis"/"Exchange Reaction" Precipitate - insoluble that separates from solution

Lithium

"Earth" Lightest metal Used as depressant and diuretic Lithium Bromide (LiBr) - depressant Lithium Carbonate (LI2CO3) - drug of choice for mania, bipolar

Magnesium Sulfate (MgSO4)

"Epsom Salt" Used as cathartic (PO), anticonvulsant (IM), antidote Ba toxicity Toxicity results in depression of DTR (deep tendon reflex) and Respiratory

Sodium Dihydrogen Phosphate

"Fleet Enema" Cathartic and source of Phosphorus and Phosphate, urinary acidifier

Sodium Sulfate

"Glauber's Salt"; Cathartic

Ferrous Sulfate (FeSO4)

"Green Vitriol", Hematinic, S/E: Constipation

Ammonium Silver Nitrate

"Howe's Solution" Dental protective, desensitizing agent

Sodium Thiosulfate

"Hypochlor", "Photographer's Hypo", "Antichlor" Treatment for CN poisoning with NaNO2, antidote for I Standard in Iodometry and Permangonometry

Potassium Chloride (KCl)

"Kalium Chloratum", "Kali Chloridum" Component of Ringer's and Lactated Ringer's Solution, Treated for familial periodic paralysis, Menier's Syndrome, Antidote for Digitalis intoxication

Potassium

"Kalium" Most abundant and predominant intracellular cation Used as diuretic and important in muscle contraction Hypokalemia (K+ deficiency) and muscle paralysis

Aluminum Silicate (Al2SiO5)

"Kaolin", "China Clay", "Native Hydrate" Adsorbent in diarrhea

Silver Nitrate

"Lapiz infernulariz", "Lunar caustic", "indelible ink", "caustic pencil" Treatment of warts, eye antiseptic for newborn babies of mother with gonorrhoea

Nitrous Oxide (N2O)

"Laughing Gas" Inhalation anesthetic Side effect: Diffusion hypoxia Container: Blue

Arsenate

"Lewisite Metal" Insecticide - Copper Aceto Arsenate (Paris Green) Choice of Professional Poisoner; Antidote: BAL First component of antisyphilis drug (Arsephenamine)

Combination Mg(OH)2 + Al(OH)3

"Magaldrate"; antacid

Calcium Chloride (CaCl2)

"Muriate of Lime" Ca replenisher, disadvantage - very irritating IV, gluconate and lactate are used instead

Sodium

"Natrium" Extracellular fluid/ion Promotes fluid retention Na - most abundant extracellular cation; for fluid retention; excess causes edema

Hemihydrated Calcium Sulfate (CaSO4.1/2H2O)

"Plaster of Paris" Supportive cast and dental impressions

Lead

"Plumbum", most metallic of the group, used as astringent, protein precipitant Poisoning: Plumbism Antidote: EDTA or Calcium Versenate Source of Poisoning: Pb pipes, Paints, Batteries, Canned Goods

Attapulgite

"Polymagma", "Diatabs", "Quintess"

Calcium Carbonate (CaCO3)

"Precipitated Chalk", "Prepared Chalk" Antacid, Ingredient in toothpaste, dentrifice

Gay-Lussac Law

At constant volume, pressure, and absolute temperature are directly related P = kt P1/T1=P2/T2

Calcium Hydroxide (Ca(OH)2)

"Slake lime", "Calcium hydrate" Antacid, saponifying agent, added to infant formula to prevent curdling of milk in the presence of gastric acid contents, promoting digestibility of milk With NaOH or KOH or both - soda lime used for CO2 absorbant, metabolism test, oxygen therapy, and anesthesia

Bentonite

"Soap Clay", "Mineral Soap," Native Colloidal Hydrated Magnesium Silicate" Suspending agent Pumice Volcanic origin Dental abrasive

Stannouos Fluoride (SnF2)

"Tin difluoride", Anticariogenic 8% solution, Topical fluoride application

Titanium

"Titan", "Sons of Earth: Powerful reducing agent

Zinc Sulfide (ZnS)

"White Lotion", "White Sulfide" Parasiticide, Topical protectant, Antiseptic

Heptahydrated Zinc Sulfate (ZnSO4.7H2O)

"White Vitriol" Emetic, Astringent Used in preparation of White Lotion

Mercuric Oxide (HgO)

"Yellow Precipitate" Ophthalmic antiseptic

Cadmium Sulfide (CdS)

"Yellow Sulfide", Anti-seborrheic

Tricalcium Phosphate (Ca3(PO4)2)

"bone ash", antacid

Barium

"heavy", toxicity: baritosis, antidote: epsom slat

Potassium Chloride

Electrolyte replenisher, given IV slow push

base

Metallic oxide/Basic oxide/Basic anhydride + Water =

Ammonium Bromide

NH4Br depressant/sedative

Sodium Tartrate

Na2C4HO6 Primary standard used for Karl Fischer for Water Content Determination

purified water

Obtained by distillation or by ion exchange treatment Extemporaneous compounding and preparation of most USP reagent

Astatine

Only metallic halogen Only synthetic and radioactive halogen

Potassium Chromate (K2Cr2O7)

Powerful oxidizing agent

Group IIIA (Metalloid)

Readily oxidized when heated in air; reacts with sulfur and halogen Hydroxides tend to show amphoteric properties

Insoluble Silver compounds

Silver Iodide (AgI) and Silver Proteinate

Condensation

The change of state from a gas to a liquid

Sodium Metabisulfate

Water soluble antioxidant

buffer solution

Weak acid/weak base + salt has the ability to resist changes in pH upon the addition of small amounts of either acid or base

Ammonium Carbonate

(NH4)2 CO3 "Sal Volatile", "Hart's horn", "Preston Salt" Expectorant, antacid, respiratory stimulant, for preparation of Aromatic NH3 Spirit

Lead (II) Acetate

(Pb(C2H3O2) or Pb(CH3COO)2) "Lead acetate", "Sugar of Lead", "Goulard's Powder" Astringent, antiseptic

Copper Aceto Acetate

([Cu3(AsO3)2.Cu(C3H3O2)2]) "Paris Green" Insecticide

Kaolin

absorbent

hydroloysis

acid + base --> salt + water

Capillary Action

caused by cohesive force within the liquid and adhesive force between the liquid and the walls of the container

(0, 2) or 0.6 - 1.6

electronegativity difference in polar covalent bonds

zinc

essential trace ion constituent of insulin and carbonic anhydrase

amphoteric

may act as acid or base

K+, Li+, Na+, NH4+

members of the basic constituent/cation Alkali/soluble group

precipitated sulfur

milk of sulfur

Activation Energy (Ea)

minimum amount of energy required to initiate a chemical reaction

Sodium Carbonate Anhydrous

Na2CO3

type III glass

soda-lime glass

Type II glass

soda-lime treated glass

examples of anti-caries agent

sodium fluoride, stannous fluoride

Combined Gas Law

P,V,T and relationship for gases can be expressed in a single equation P1V1/ T1 = P2V2/ T2

Calcium Phosphate (CaHPO4.2H2O)

source of calcium and phosphate

Barium Sulfate (BaSO4)

Radiopaque substance used for GIT imaging

Schrodinger's Equation

specifies possible energy states electrons will occupy and identifies the corresponding wave functions or probability of finding its location in a particular region surrounding the nucleus

Kinetics

speed or rate of reaction

Le Chatelier's Principle

states that - if an external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is partially offset as the system reaches a new equilibrium position

Planck's Quantum Theory

states that atoms and molecules could emit or absorb energy in discrete quantities in the form of electromagnetic radiation (quantum)

Law of Multiple Proportions

states that if two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of other element are in ratios of small whole numbers

Heisenberg's uncertainty principle

states that it is impossible to determine simultaneously the momentum and position of an electron

Evaporation

The change of state from a liquid to a gas

Law of Conservation of Mass

states that matter can be neither created nor destroyed; Matter is made of atoms that are unchanged in a chemical reaction, it follows that mass must be conserved as well

Mercuric Iodide (HgI2)

stimulant of indolent ulcer

expectorant

stimulates flow of respiratory secretion (ex. ammonium chloride, potassium iodide)

strong electrolytes

strong acids, strong bases and salts containing the ions of strong acids and bases 100% ionization/dissociation in H2O; undergoes irreversible reaction

nuclear chemistry

study of reactions involving change in atomic nuclei

compounds

substance composed of atoms of two or more elements chemically united in fixed proportions

Solvent

substance present in the larger amount

arrhenius acid

substance that produce H+ (H3O+) in water

arrhenius base

substance that produce OH- in water

protective

substance which may be applied to the skin to protect certain areas of irritation

plastic sulfur

sulfur rubbery in consistency

molecular mass (weight)

sum of the atomic masses (in amu) in a molecule is the sum of the atomic masses (in amu) in a molecule

chemical formula

symbols and ratios of atoms for the elements in a chemical compound

Antimony Potassium Tartrate ((SbO)KC4H4O6.1/2H2O)

tartar emetic used before as emetic in Brown mixture official as schistosomiasis (destroys Schistosoma japonicum)

Strontium Chloride (SrCl2)

temperature desensitizing agent

Boiling Point

temperature where liquid vapour = atm pressure

Freezing (Melting) Point

temperature where solid phase of substance = liquid phase

Gallium

Treatment of cancer related hypercalcemia by binding with transferrin Used for substitute of mercury in manufacture of arc lamp

Aluminum Carbonate (Al2(CO3)3)

Treatment of phosphatic caliculci

Ferrous Ferricyanide (Fe3[Fe(CN)6]2

Turnbull's Blue

Ferrous Chloride (FeCl3)

Used as astringent, styptic Reagent for detection of tannins

isobars

atoms with same mass numbers

Type NP Glass

general soda lime glass

bromide

non-essential ion that causes CNS depression; used for epileptic seizure

Specific Heat (s)

the amount of heat (q) required to raise the temperature of one gram of the substance by one degree Celsius J/gC

CdS Yellow ppt

product of reaction between H2S and Cd+2

nuclear fusion

the combining/union of small nuclei/2 light atoms into larger ones/bigger molecule (hydrogen bomb)

Formal Charge

the difference between the number of valence electrons in an isolated atom and the number of electrons assigned to that atom in a Lewis structure

atomic number

the number of protons in the nucleus of an atom; number of electrons

Vapor Pressure

the pressure exerted by a vapor in equilibrium with its liquid

Ca Chlorate (CaClO3)

""Chlorinated lime", "Chloride or Lime" Disinfectant and bleaching agent

Aluminum Oxide (Al2O3)

"Alumina", Treatment of Silicosis

Aluminum Hydroxide (Al(OH)3)

"Amphojel", "Cremalin gel" Acid protectant Advantage Do NOT interfere with Phosphate absorption

Gold

"Aurum", "Shining Dawn", "King of All Metal" Most malleable and ductile Best conductor of electricity Dissolved by Aqua Regia (3 HCl + 1 HNO3) and Selenic Acid Used for arthritis and gout SE: Dermatitis

Sodium Bicarbonate

"Baking Soda" Systemic antacid and carbonating agent S/E" Systemic alkalosis, rebound hyperacidity, edema Carbonating agent for effervescent tablets or preparation (reaction with organic acid like citric acid release CO2 which is used for increased palatability or mask saline taste of preparation) Antidote for Zn poisoning

Bismuth Subcarbonate & Bismuth Hydroxide (Bi2O2(CO3)+Bi(OH)3)

"Bismuth Cream" Antacid, internal protective especially for gastric patients, inhibits growth of H. pylori

Sodium Borate (Na2B4O7.10H2O)

"Borax", "Sodium tetraborate", "Dobell's solution" Antiseptic, eyewash, wet dressing for wounds

Sulfur

"Brimstone","Shubari", "Enemy of Copper" Used in preparation of scabicidal and keratolytic ointment or lotion Stimulant, cathartic, depilatory agent, fumigant, anti-dandruff

Zinc Chloride (ZnCl2)

"Burnett's Disinfectant Fluid" Disinfectant/antiseptic, dentin desensitizer, corrosive

Magnesium Oxide (MgO)

"Calcinated Magnesia" Laxative, antacid, component of universal antidote

Calcium Chloride (CaCl2.2H2O)

"Cloruro de calcio", "Muriate of Lime", "Fosforo de Homberg" Used for internal haemorrhage, in certain bone disease, nervous disorder and deficiency of Calcium

Mercuric Chloride (HgCl2)

"Corrosive Sublimate" Disinfectant

Copper

"Cuprum" Essential trace element Enhance physiological utilization of Iron Only reddish metal 3rd most malleable metal, 3rd best conductor Component of hemocyanin and cytochrome oxidase 2 important alloys: Brass (Cu + Zn); Bronze (Cu + Sn) Protein precipitant Toxicity: Wilson's disease; antidote for its poisoning is Penicillamine

Sodium Hypochlorite

"Dakin's Solution", "Chlorox" Oxidizing agent, disinfectant for inanimate object, bleaching agent

Helium

"Donald Duck" sound 2nd lightest gas Toxicity (inhalation): Donald duck sound Uses: Carrier/diluent of medically important gases and component of artificial gas Container: Brown

Hydrogen

"Inflammable Air" Lightest element Isotopes (Protium - Most Abundant; Deuterium - Heavy Hydrogen; Tritium - Radioactive)

Phosphorus

"Light Carrier", "St. Elmo's Fire" 2 Forms: White (Poisonous), Red (Non-Poisonous)

Calcium Oxide (Cao)

"Lime" "Quicklime"

Cobalt Chloride (CoCl2)

"Lover's Ink", "Sympathetic Ink" Dessicator indicator

Magnesium Carbonate (MgCO3)

"Magnesia", "Dolmite" Used as antacid, laxative

Nitrogen

"Mephitic air", "Azote", "Without life" Most abundant gas in air, 71% N2, 29% O2

Magnesium Hydroxide (Mg(OH)2)

"Milk of Magnesia", "Magnesia Magma" Used as antacid, laxative

Potassium Permanganate

"Mineral Chameleon" Oxidizing agent, antiseptic, volumetric solution in Permanganometry

Radon

"Niton" Synthetic noble gas Used for treatment of Cervical Cancer

Nitrogen Dioxide (NO2)

"Nitrite" Vasodilator, for CN poisoning

Nickel

"Old Nick's Copper" found in fossil fuel used as fancy jewelries

Dihydrated Calcium Sulfate (CaSO42H2O)

"Plaster of Paris", "Gypsum Terra Alba" Rodenticide, preparation of surgical cast and dental impression

Potassium Carbonate

"Potash", "Salt of Peter", "Perlash" Antacid, carbonating agent, carbonate source

Sodium Chloride

"Rock Salt", "Table Salt", "Solar Salt" - purest form Electrolyte replenisher, tonicity adjusting agent, preservative

Boric Acid (H2BO3)

"Sal sativum" Toxicity: Lobster appearance Used for buffer (ophthalmic solution 2%), antiseptic, tonicity adjusting agent

Potassium Nitrate

"Salt Peter", "Salitre", "Salt prunelle" Diuretic, meat preservative

Sellenium

"Selena", "Moon" Essential trace element Promotes absorption of Vit. E Used as anti-oxidant

Sellenium Sulfide (SeS2)

"Selsun Blue", Anti-dandruff

Aromatic Ammonia Spirit

"Spirit of Hartshorn", "Spirit of Sal Volatile" Respiratory stimulant

Tin

"Stannum" The lower oxidation is electrostatic, the higher oxidation is covalent Used in preparation of tin can

sodium chloride (NaCl)

"Table Salt", "Sea Salt", "Sal" Used as wet dressing for irritated body cavity or tissue

Hydrated Magnesium Silicate

"Talc", "Soapstone", "French Chalk" Softest Mineral Filtering, clarifying and dusting agent

Antimony Potassium Tartrate (K2Sb2(C4H2O6)2)

"Tartar Emetic", "Brown Mixture" Emetic, treatment of Schistosomiasis

Mercuric Aminochloride (HgNH2Cl)

"white precipitate", total antiseptic

0% ionic character

% ionic character in non-polar bonds

Copper (II) Citrate

((Cu)3(C6H5O7)2) "Cupric Citrate" Astringent in 8% concentration

Molybdenum Oxide (MoO8)

+FeSO4 use: hematinic

ringer's infection

1 L containing 8.6 g NaCl, 0.3 g KCl, & 0.33 g CaCl2

1 pascal (PA)

1 N/m^2 SI unit for pressure

Dalton's Atomic Theory

1. Elements are composed of extremely small particles called atoms 2. All atoms of a given element are identical, having the same size, mass, and chemical properties. The atoms of one element are different from the atoms of all other elements 3. Compounds are composed of atoms of more than one element. The relative number of atoms of each element in a given compound is always the same 4. Chemical reactions only involve the re-arrangement of atoms. Atoms are not created or destroyed in chemical reactions

mass of a proton

1.637x10-24 g

mass of a neutron

1.675x10-25 g

mass of an electron

1/1837 mass of proton

lactated ringer's infection

100 mL contains 600 mg NaCl, 30 mg KCl, 200 mg CaCl2, and 310 g Na lactate

1 atm

101, 325 Pa 101 kPa 760 mmHg 760 torr

Technetium

1st element produced artificially, used in preparation of radiopharmaceuticals

Carbon Monoxide (CO)

210X greater affinity to Hb than oxygen leading to asphyxia then death Treatment: 100% O2, Artificial Air (He 80% and O2 20%), Hyperbaric O2

Calcium

2nd most abundant cation in extracellular fluid Vit D. is needed for its maximum absorption Blood coagulating factor, important for muscle contraction, release of neurotransmitter and primary element of bones and teeth Deficiency: osteoporosis, osteomalacia, rickets, hypocalcemia

Silicon

2nd most abundant element Forms inert oxides which occurs in nature

pi bond (p)

2nd or 3rd bond formed between 2 atoms formed by sideways overlap of p orbitals or a p and d orbitals; weaker than the sigma bond

Heat

the transfer of thermal energy between two bodies at different temperatures

1 mol

6.0221367 X 10^23 atoms/amu - Avogadro's Number (NA)

Rem

= 1 rad * RBE = 0.01 sievert (SI) Unit of radiation dosage (such as from X-rays), applied to humans, derived from Roentgem equivalent man

Sublimation

A change directly from the solid to the gaseous state without becoming liquid

double bonds

A chemical bond formed when atoms share two pairs of electrons

Kinetic Molecular Theory of Gases

A gas is composed of molecules that are separated from each other by distances far greater than their own dimensions. The molecules can be considered to be points; that is they possess mass but have negligible volume Gas molecules are in constant motion in random directions. Collisions among molecules are perfectly elastic Gas molecules exert neither attractive nor repulsive forces on one another The average kinetic energy of the molecules is proportional to the temperature of the gas in Kelvins. Any two gases at the same temperature will have the same average kinetic energy

Surface Tension

A measure of how difficult it is to stretch or break the surface of a liquid resistance of liquid to an increase in surface area

Mercurous Chloride (HgCl or HgCl2)

toxic disinfectant, antidote is sodium formaldehyde sulfoxylate

Silicon Dioxide (SiO2)

toxicity: silicosis

Sodium Phosphate P-32 (Phosphotope)

treatment of polycythemia vera (increase in RBC and localization of intraocular tumor)

Mercurous Iodide (Hg2I2 or HgI)

treatment of syphilis

protons and neutrons

two kinds of fundamental particles present in all nuclei except hydrogen (protium)

polar covalent bond

type of covalent bond that involves unequal sharing of electrons; have large dipole and form hydrogen bonds One atom is partially (+) and another atom is partially (-); Dipole-dipole: forces present

emollient

type of laxative that acts as lubricant facilitating the passage of compacted fecal material or as stool ex. Mineral Oil

stimulant

type of laxative that acts by local irritation on the intestinal tract ex. Bisacodyl, anthraquinone - containing cascara, senna & danthron; castor oil

saline-cathartic

type of laxative that increases the osmotic load of the gastrointestinal tract

bulk forming

type of laxative that swells when wet and with the increased bulk stimulates peristalsis; water holding, safest and generally preferred ex. Psyllium methylcellulose, polysaccharides, cellulose derivatives

zinc stearate

type of protective; mild astringent and antimicrobial agent. Inhalation of powder may cause inflammation of lungs especially among children

silicon polymer

type of protective; silicon oils or dimethylsilicone ethers. Water repellent and protective against chemical irritants. Simethicone is antiflatulent and gastric protective

titanium dioxide (TiO2)

type of protective; solar ray protectant due to its opacity or high refractive index

zinc oxide (ZnO)

type of protective; zinc white for treatment of skin ulceration

1. Combination Method: Molecular Equation & Ionic Equation 2. Decomposition Reaction 3. Displacement Reaction 4. Combustion Reactions 5. Disproportionation Reaction

types of balancing redox reactions

Entropy

unavailability of system's thermal energy for conversion into mechanical work interpreted as the degree of disorder or randomness in the system

Rad

unit of absorbed radiation dose = 0.01 Gy = 0.01 J/kg

Sievert

unit of radiation damage used in medicine

Paramagnetic

unpaired electrons (up, up)

half-lives

used as "atomic clocks" to determine the ages of certain objects; rate of radioactive decay; time required for the concentration of a reactant to decrease to half of its initial concentration

iodine (I)

used as germicide 2% I2 solution with NaI 2% I2 tinctures with 50% alcohol Lugol's solution 5% I2 with Kl

sterile water for injection

used for extemporaneous compounding of parenteral

emetic

used in cough, stimulates or promotes emesis

Strontium

used in the manufacture of flares

Iopanoic acid

used in visualization of gall bladder, it has 3 I2 atoms that can be concentrated in the organ to be studied

Enthalpy (H)

used to quantify the heat flow into or out of a system in a process that occurs at constant pressure. ch.H = H (products) - H (reactants)

oral electrolyte solution

used to supply H2O in amount needed for maintenance

glass

vitreous material, used for storage and as dispensing container for most drug product

Charles' Law

volume of gas varies directly with the absolute temperature at constant pressure V = KT V1/T1 = V2/T2

water for injection

water purified by distillation

nuclear fission

when heavy nucleus (mass no. > 200) divides/splits to form smaller nuclei of intermediate mass and one or more neutrons (atomic bomb)

phosphate buffer system

Advantage of containing the dihydrogen and monohydrogen phosphate ion One of the physiological buffer pair

Mercury

Affects the brain "Quicksilver", "Messenger of God" Diuretic, antiseptic, treatment of syphilis, cathartic, parasiticidal/antifungicidal Industrial use: thermometer, amalgams Disease: Minamata (from fish) Antidote: EDTA

Boric Acid (H2BO3)

Agua Boricada Antiseptic in solution, ointment and dusting powder, eyewash buffer component

combination of antacid preparation

Al(OH)3 + Mg(OH)2 combination Al(OH)3 + 2 MgO.3SiO2.xH2O combination Al(OH)3 gel + Mg(OH)2 Simethicone Alginic Acid

Sodium Citrate

Alkalizer, Buffer, Diuretic, Expectorant, Decrease Coagulation Time, sequestering property used in Benedict's Solution

Group VIIIA (Noble Gases)

Also known as Group 0 All elements except Radon occur in the atmosphere Mono-atomic, colorless, and odourless gases under ordinary condition of temperature and pressure

examples of astringent

Alum/Tawas ([AlNH4(SO4)2.12H2O]) Ammonium Salt ([AlK(SO4)2.12H2O]) Potassium Salt - preparation of vaccines and tetanus toxoids Aluminum Chloride (AlCl3.6H2O) Aluminum Sulfate (Al(SO4)3.14H2O) - Cake Alum, Pickle Alum Aluminum Acetate Al(C2H3O2)3 - Burrow's Solution Zinc Chloride (ZnCl2) Zinc Sulfate (ZnSO4.7H2O) - White Vitriol

examples of antacid

Aluminum Hydroxide (Al(OH)3) Precipitated Calcium Carbonate (CaCO3) Tribasic Calcium Phosphate (Ca3(PO4)2) Magnesium Carbonate (Mg(CO3)4.Mg(OH)2.5H2O) Magnesium Hydroxide (Mg(OH)2) Magnesium Oxide (MgO) Magnesium Trisilicate (2MgO.3SiO2.XH2O) Magnesium Phosphate (Mg3(PO4)2.5H2O)

Strong Ammonia Solution (NH4OH)

Ammonium Hydroxide Strong Ammonia Water Caustic in nature Used as Bronsted base Used in manufacture of nitric acid and sodium bicarbonate

Bismuth Subcarbonate (Bi2O3)

Antacid, astringent, antiseptic

Potassium Acetate

Antacid, diuretic, urinary and systemic alkalinizer

Bismuth Subgallate (C7H5BiO6)

Antacid,astringent, antiseptic

Bismuth Subnitrate (Bi5O(OH)9(NO3)4)

Antacid,astringent, antiseptic

Magnesium Trisilicate (2MgO3SiO2H20)

Antacid; advantage prolonged antacid action

Sodium Fluorophosphate (Na2FPO3)

Anticariogenic

Sodium Fluoride

Anticariogenic (2% solution) Sodium Phosphite (Na2HPO3) Reducing Agent

Sodium Fluoride (NaF)

Anticariogenic at 2% solution

Stannous Fluoride (SnF2)

Anticariogenic at 8% solution

Hypophosphorus Acid (H3PO3)

Antioxidant in liquid preparations containing easily oxidizable ions like Fe+2 and I-

mechanism of antioxidants

Antioxidant is oxidized in place of the active constituent Constituent is oxidized , the antioxidant reduces it back to its normal oxidation stat

Boron

Appears in +3 oxidation state Industrial use in vulcanizing rubber

Cadmium

Astringent, Used in manufacture of stink bomb Poisoning: Itai-itai/Painful bone disease Antidote: BAL

Avogadro's Law

At constant temperature and pressure, the volume of a gas is directly related to the number of moles V = Kn V1/n1 = V2/n2

intermolecular forces

Attractive forces between molecules Responsible for non-ideal behaviour of gases; account for the existence of the condensed state of matter (liquids and solids); as the temperature of gas drops, the average kinetic energy of molecule decreases; responsible for the bulk properties of matter (ex. melting and boiling point) Weaker than intramolecular forces

nitrogen

Azote, very stable due to the triple bonds in the structure Used as air displacement/replacement Used in the space above Hg in thermometers to prevent evaporation when placed in high temperature Stored in black cylinders

Sublimed Sulfur

Azufre, Flowers of Sulfur for preparation of Vleminckx's solution with lime

examples of protective and adsorbent

Bismuth Subnitrate (Bi(OH)2(NO3)4.BiO(OH)) Bismuth Subcarbonate (BiO2(CO3)2.H2O) Milk of Bismuth (Bismuth Magma, Bismuth Cream) Kaolin (Porcelain Clay, China Clay, Bolus Alba)

Hypochlorite (OCl-) (Na,K)

Bleaching agent

I131 Human Serotonin Albumin

Blood Plasma/Volume/Cardiac Output determination

Ferrous Gluconate (C12H2FeO14)

Brand name: Fergon Advantage: Less irritating

Voltaic or Galvanic Cell

CE -> EE; Spontaneous reaction; Transfer of electrons from anode to cathode Oxidation reaction - anode (OA) Reduction reaction - cathode (CR)

Sodium Acetate

CH3COONA

Barium Hydroxide (Ba(OH)2)

CO2 absorbent

Calcium Oxalate (Ca(C3H4O3)2)

Ca supplement

Calcium Gluconate (C12H22CaO14)

Ca supplement and replenisher

Palladium

Catalyst in finely divided steel

Platinum

Catalyst in finely divided steel

Cesium

Catalyst in polymerization of resin forming material

Potassium Hydroxide (KOH)

Caustic Potash Soda Lye Very strong base with caustic effect Aqueous and alcoholic volumetric solution for titrating

Sodium Hydroxide (NaOH)

Caustic Soda Soda Lye Strong base Reacts with salt of all metal Employed for the same purpose as KOH

nuclear change

Change in the identity of the nucleus of an atom; transmutation of an element to another element; results in the formation of a new substance

specification limits for buffers

Chemical Stability, Solubility of the Drug, Patient's Comfort

water

Clear, colorless, odourless liquid which has the specification for pH, zinc, other heavy metal, foreign volatile matter, total solid content and bacteriological purity used to make official solution, tincture

Lumosol

Colloidal AgCl - prophylaxis and treatment of infection of mucus membrane

Basham's mixture

Component: Iron + Ammonium Acetate Use: Astringent, styptic

salts

Compounds made up of the cation of the base and anion of the acid Compounds made up of the metal and non-metal; weaker ions will undergo hydrolysis

Copper Sulfate

CuSO4.5H2O "Blue Vitriol, "Blue Stone" Component of Benedict's, Barfoed's, and Fehling's Reagent Antidote for Phosphorus poisoning + Iron: Increase hematinic activity Ingredient of Bordeaux mixture (used as algaecide, fungicide in swimming pools)

Bromine

Dark reddish brown fuming liquid with suffocating odor Sedative/depression Poisoning: Bromism Manifestation: skin eruption, psychosis, weakness, headache Antidote: NaCl & NH4Cl Kopperschaar's Solution - Br2 10th normal solution KBrO3 & KBr in water

Spin Orientation (ms)

Determines direction of spin or rotation of 2 e- (+1/2 or -1/2)

Uranium

Discovered by Becquerel, Radioactive element used for manufacture of atomic bomb, No pharmaceutical use

James Chadwick

Discovered the neutron

Iron

Distributed widely in nature Functions in divalent and trivalent states to from Iron (II) ferrous and Iron (III) ferric Present in proteins: Hemoglobin, Transferrin, Ferritin, and Cytochrome Oxidase Enzyme Enhance the absorption of Vit C and copper Most important element in engineering. Also used medicinally as hematinic Toxicity: GIT distress and Cardiac Collapse Antidote: Deferoxamine

Sodium Acetate

Diuretic, urinary, and systemic alkalinizer; antacid

Group IA (Alkali Metals)

Do not occur free in nature Very active chemical; displace all other elements from their chemical compound Oxides and hydroxides are strongly basic Alkali halides are soluble in water and are not hydrolyzed Univalent; valence = 1 Form simple cation; do not form complex cation with ammonia All rapidly oxidized in air

electrolytic cell

EE -> CE; Non-spontaneous reaction; Transfer of electrons from cathode to anode E0 < 0 (-)

Valence Electrons

Electrons on the outermost energy level of an atom available for bonding

Cobalt

Essential in development of erythrocytes and hemoglobins Component of Vitamin B12 Deficiency: Megaloblastic Anemia

Molybdenum

Essential trace element, Co-factor enzyme

Group IIIB (Scandium Subgroup)

Exhibit an oxidation state of +2 and +3 Have physical properties that are typically metal Oxides are basic Quite reactive Includes Scandium, Ytrium, Lanthum, Actinum, Lanthanide, and Actinide

Group VIB (Chromium Subgroup)

Exhibit oxidation state of +2 through +6 +2 good reducing agent; +3 good oxidizing agent

Group VA (Nitrogen Family)

Exhibits +3 and +5 oxidation state Reacts with chlorine to form tri- and penta- halides

Group IIB (Volatile Metal)

Exist in divalent ion except Mercury React with halogen, oxygen, nitric acid and other common oxidizing agent Readily forms complex ion

change in temperature affecting equilibrium

Exothermic (inc. temp favors backward reaction; dec. temp favors forward reaction) Endothermic (inc. temp favors forward reaction; dec temp favors backward reaction)

Sodium Iodide

Expectorant, antifungal, I2 solubilizer, ameliorating agent for goiter

Potassium Iodide

Expectorant, antiseptic, antifungal, iodine solubilizer

chemical bonds

Forces that hold atoms or ions together; formed when atoms interact; outer regions are in contact; concerned with valence electrons of the atoms

Stannous Oxide (SnO)

Germicide for Staphyloccocus infection

auto ionization of water

H2O(l) <- -> H+ (aq) + OH- (aq) At 25 C Kw = [H+][OH-] = 1.0 x 10-14 Ion product constant (Kw) pH=-log[H]; pOH=-log[OH-]; pKw=pH+Poh = 14.00

strong acids

HCl, HBr, HI, H2SO4, HClO4, HNO3

Osmium

Heaviest and densest metal

alpha particle

Heaviest and slowest of all radioactive emissions Move at slow speed about 0.1 the speed of light; penetrating power is very low and stopped by a sheet of paper or very thin sheet of Al

Ammoniated Mercury

HgNH2Cl "White Precipitate" Topical antifungal and anti-infective

intramolecular forces

Hold atoms together in a molecule Stabilize individual molecules; more stable therefore requires much less energy to evaporate a liquid than to break the bonds in the molecules of the liquid

Aurathioglucose

IM Treatment of gout and RA

Gold Sodium Thiomalate

IM Treatment of gout and RA

change in volume and pressure affecting equilibrium

Inc. pressure - favors fewest moles of gas Inc. volume - favors greater moles of gas Dec. pressure - favors greater moles of gas Dec. volume - fewest moles of gas

change in concentration affecting equilibrium

Increase conc of product/s: backward reaction favored Decrease conc of product/s: forward Increase conc of reactant/s: forward reaction favored Decrease conc of reactant/s: backward

Arsenic Trioxide

Insecticide, anti-leukemic

Xenon

Investigational with inhalatory anesthetic activity

Sulfurated Potash

K2Sx.K2S2O3 "Liver of Sulfure" Mixture of Potassium sulfide, Potassium polysulfide, Potassium thiosulfate Used in preparation of White Lotion with addition of ZnSO4

Potassium Citrate

K3C6H5O7 diuretic, expectorant, diaphoretic

Potassium Acetate

KC2H3O2

Potassium Dihydrogen Phosphate

KH2PO4 cathartic

Potassium Bitrate

KHC4H4O6 "Cream of Tartar" Laxative, cathartic

Potassium Bicarbonate

KHCO3

Hydrochloric Acid (HCl)

Lacks in patient with pernicious anemia Treatment of achlorhydria

nitrous oxide

Laughing Gas Used as dental anesthesia in extraction of teeth and opening of abscesses

Krypton

Least abundant of all noble gases, has inhalational anesthetic activity

Magnesium

Lightest of all structurally important metal and second most abundant intracellular action Chlorophyll component Component of Grignard's Reagent Used as laxative, depressant natural CCB

principal quantum number (n)

Main energy level; determines size of particle; relates average distance of electron from the nucleus in a particular orbital

Carbon

Manifestation: Crystalline - graphite, diamond Amorphous - coal, anthracite Carbon Dioxide - co2 Treatment of acne, warts, corns, callus, and eczema Most potent respiratory stimulant

Silver Proteinate

Mild Silver Proteinate - "Argyrol"; antiseptic for the eye Strong Silver Proteinate - "Protargol"; strong germicidal for ear and throat Collioidal Silver Proteinate - "Collargol"; "Neo-silvol"; General Germicidal

Sodium Carbonate (Na2CO3.H2O)

Monohydrated Sodium Carbonate Not given internally because of marked alkalinity Solubilizing agent Forms sodium salt of acidic drug

Aluminum

Most abundant metal 3rd most abundant metal Astringent, aluminium foil used for burn patient

Argon

Most abundant of all noble gas, substitute for Nitrogen in providing inert atmosphere

Group VIIA (Halogen Family)

Most active family of non-metal Exist in diatomic molecule Reduced and promote oxidation of some other substance Exhibit +1, +3, +5, +7 oxidation state

Fluorine

Most reactive of the electronegative elements Strong oxidizing agent Poisoning: Fluorosis Manifestation: Mottled enamel, abnormal bone growth

beta particle

Move at a faster velocity about 0.9 speed of light More penetrating power and able to travel 10-15 minutes in H2O to penetrate 1 inch thickness of Al

Hydrochloric Acid (HCl)

Muriatic Acid Spirit of Sea Salt Marine Acid Colorless fuming liquid Acidifying agent and gastric antiseptic 36% - disinfectant 10% - diluted HCl for treating achlohydria and hypochlorhydria Disadvantage: hygroscopic

Ammonium

NH4+ hypothetical alkali metal Conjugate acid of NH3

Ammonium Acetate

NH4CH3COO "Spirit of Minderesus" Styptic - stops bleeding of wound

Ammonium Chloride

NH4Cl "Muriate of Hartshorn" Expectorant, diuretic, systemic acidifier in alkalosis

Ammonium Iodide

NH4I Source of Iodine, Expectorant, Antifungal/antiseptic

Glass

Na2CO3 + Pure Silica

Sodium Metabisulfate

Na2S2O5

Sodium Citrate

Na3C6H5O7

Sodium Lactate

NaC3H5O3 Antacid, Diuretic

Sodium Chloride

NaCl

Sodium Dihydrogen Phosphate

NaH2PO4

Sodium Bicarbonate

NaHCO3

strong bases

NaOH, KOH, Ba(OH)2, Sr(OH)2, Ca(OH)2, Mg(OH)2

Hydrated Zinc Silicate

Natural Calamine, Topical protectant

Factors affecting reaction rate

Nature of Reactants and its State of Subdivision Concentration Temperature

Potassium Mercuric Iodide (K2HgI4)

Nessler's Reagent antiseptic component of Mayer's reagent

Beryllium

Never employed in medicine because it is the most toxic metal Fluorescent lamp

Group VI1 (Oxygen Family)

Non-metallic and exhibit oxidation state of -2, 0, +2, +4, and +6 Hydrides are all gases, highly odoriferous, and poisonous

acid

Non-metallic oxide/Acid oxide/Acid anhydride + Water =

Tantalum

Not affected by any body fluid, therefore inert in our body Sheet form use in repair of bones, nerve and tissue

Oxygen

O2 - Molecular O3 - Ozone "Empyreal air", "Dephlogisticated air", "Yne" Most abundant element Used in the treatment of hypoxia/asphyxia Container: Green

Group IB (Coinage Metal)

Occurs free in nature and are easily recovered from their compound by reduction Low in electromotive series and not very reactive Oxides and hydroxides are weakly basic Divalent Forms complex anions, forms chelates Oligodynamic property

Sulfuric Acid (H2SO4)

Oil of Vitriol Strong diptrotic acid, dehydrating, oxidizing, sulfonating or sulphating agent

Group VIIB (Manganese Group)

Only metal of pharmaceutical importance Exhibit +2 to +7 oxidation state Most important trace element Occurs mainly as oxide of MnO2 Difficult to prepare the pure state Co-factor in protein synthesis, phosphorylation, fatty acid, and cholesterol synthesis Poisoning: Parkinson's like

Titanium Dioxide (TiO2)

Opacifying agent, UV ray protectant

Magnetic (ml)

Orbital restriction/orientation in space, determines the shape; represented by a (+) or (-) integer value (0, +1, +2, +3)

Phosphoric Acid (H3PO4)

Orthophosphoric acid Acidifying agent and solvent in the preparation of Anileride Injection NF XV, non-volatile and non-oxidizing

Group VB (Vanadium Subgroup)

Oxidation state of +2 through +5 Shows good reducing property

Potassium Chlorate

Oxidizing agent, component in toothpaste, gargle and mouthwash

Auranofin

PO Only oral gold preparation SE: Glossitis

gamma radiation

Photon of EMR Rays are short wavelength similar to x-rays and travel to the speed of light No mass and no charge but are of very high energy giving them excellent penetrating power

Antimony

Physiologically resembles arsenic toxic Expectorant, emetic, anthelmintic

Silver Iodide

Poisonous disinfectant

Simethicone

Polymeric dimethyl silaxane, Antiflatulence

Zinc

Present in insulin Used as astringent, antiseptic, antiperspirant and protectant Deficiency: parakeratosis, antidote: NaHCO3

Arsenic Triiodide

Primary standard in preparation of Cerric sulfate

Intensive (Intrinsic) Properties

Property of matter that does not depend upon how much (quantity) matter is being considered: density, physical state, temperature (boiling point and melting point), color

Ferric Ferrocyanide (Fe4[Fe(CN)5]3)

Prussian Blue

Law of Definite (Constant) Proportion

Published by Joseph Proust and credited to Dalton, it states that different samples of same compound always contain its constituent elements in the same proportion by mass

Ion Product (Q)

Q < Ksp: Unsaturated solution (no ppt.) Q = Ksp: Saturated solution (no ppt.) Q > Ksp: Supersaturated solution (ppt.)

Equilibrium concentration computations

Qc > Kc system proceeds from left to reach equilibrium Qc = Kc the system is at equilibrium Qc < Kc system proceeds from right to reach equilibrium

beta decay

Radiation similar to gamma rays seen in the emission of X-rays Nucleus "capture" an electron from K-shell (1s orbital) to combine with proton to form neutron

Freon (CCl2F2)

Refrigerant, aerosol propel

Group IIA (Alkaline Earth Metal)

Shows definite metallic properties Strong reducing agent Combines directly with oxygen, halogen, nitrogen and sulfur & hydrogen (except Mg)

Soluble Silver compounds

Silver Nitrate (AgNO3) and Ammonium Silver Nitrate (Ag(NH3)2NO3)

Calcium Hydroxide (Ca(OH)2)

Slaked Lime Calcium Hydrate Used as fluid electrolyte and topical astringent

Sodium Carbonate Anhydrous

Soda ash Antacid, source of carbonate, carbonating agent Na2CO3.2H2O - trona, official form Na2CO3.10H2O - washing soda, sal soda, soda crystal

electrolytes in acid and base therapy

Sodium Acetate (CH3COONa.3H2O) Potassium Acetate (CH3COOK) Sodium Bicarbonate (NaHCO3) Potassium Bicarbonate (KHCO3) Sodium Citrate (C6H5Na3O7) Potassium Citrate (C6H5K3O7.H2O)

examples of official saline cathartic

Sodium Biphosphate (NaH2PO4.H2O) Sodium Phosphate (Na2HPO4.7H2O) Potassium Sodium Tartrate (KNaC4H4O6.4H2O) Magnesium Sulfate (MgSO4.7H2O) Magnesium Citrate (Mg3(C6H5O7)2)

examples of non-official saline cathartic

Sodium Sulfate Potassium Phosphate Potassium Bitartrate Calomel

Nitric Acid (HNO3)

Spirit of Nitre Aqua Fortis Aqua Ferte Acidifying and nitrating agent Used to destroy warts and chancres Strong oxidizing agent utilized in making TNT Xanthoproteic Test - yellow stain on tissue due to nitration of amino acid

Osmic Acid/Osmium Tetroxide (OsO4)

Staining microorganism for microscopic study especially electron microscopy

octet rule

States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons

Angular Momentum/Azimuthal (l)

Subshell/sublevel; determines the shape of orbital; represented by 0-(n—1)

Potassium Bicarbonate

Systemic antacid, carbonating agent, bicarbonate source

Factors affecting solubility

Temperature: increase solubility solid in liquid; decrease solubility of gas in liquid Pressure: increase pressure, constant solubility of solid in liquid Concentration - solute that dissolves in a solvent that has a limit Agitation

Group VIIIB (First Triad)

The important oxidation states are +2, achieved by the loss of 2 electrons and +3 in which an additional d electron is lost.

Thermodynamics

The study of heat change in chemical reactions

Chemistry

The study of matter, its properties, and changes it undergoes

Dalton's Law

The total pressure in a container is the sum of the pressure each gas would exert if it were alone in the container Ptotal = P1 + P2 + P3 +... (for each gas P = nRT/V)

Na125

Thyroid function

Ferrous Fumarate (C4H2FeO4)

Toleron

borate buffer system

Use in the preparation containing metals that would otherwise precipitate the phosphate buffer Suitable in external preparation, ophthalmic and nasal solution

Iodine

Used as expectorant and anti-fungal Deficiency: Goiter Elemental Iodine Preparation a. Strong Iodine Solution - Lugol' Solution b. Iodine Tincture - Disinfectant c. Povidone Iodine - Betadine

Sodium Nitrite

Vasodilator, meat preservative, antidote for CN poisoning

N2

Very stable because of 3 covalent bonds Used as inert atmosphere for readily oxidazable substance. Liquid Nitrogen is used as refrigerant Container: Black

Alum

[AlNH4(SO4)2.12H2O] - Ammonium Salt [AlK(SO4)2.12H2O]- Potassium Salt Astringent, antiperspirant/deodorant

Electronegativity

a measure of the ability of an atom to attract electrons

Heterogeneous Mixture

a mixture in which the composition is NOT uniform throughout

Homogenous Mixture

a mixture in which the composition is uniform throughout

Unsaturated Solution

a solution that contains less solute than the solvent has the capacity to dissolve at a specific temperature

Saturated Solution

a solution that contains maximum amount of solute that will dissolve in a given solvent at a specific temperature

Supersaturated Solution

a solution that contains more solute than is present in a saturated solution at a specific temperature; not very stable; dissolved solute will crystallize

hydrogen bond

a special dipole-dipole interaction between the Hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom

Element

a substance that cannot be broken down into simpler substances

Ionization Energy/Potential

ability to remove an electron from a (+) atom

Purified Siliceous Earth

absorbent

Chemical Equilibirium

achieved when rates of the forward and reverse reactions are equal and the concentrations of the reactants and products remain constant; rf=rr concentration constant

Acid-Base/Neutralization reaction

acid + base --> salt + water

suspending agent

agent that acts by altering the surface character of the solvent (ex. bentonite)

lubricant

agent used in ejection of tablet

molecule

aggregate of 2 or more atoms in a definite arrangement held together by chemical bonds

Group I-A (periodic table)

alkali

Saponification

alkali + fats/oil --> soap + glycerol

Group II-A (periodic table)

alkali earth

Diamagnetic

all electrons paired (up down, up down)

Howe

ammoniacal silver nitrate solution used in dentistry t protect the dentin

examples of respiratory stimulants

ammonium carbonate aromatic ammonia spirit

mole (mol)

amount of a substance that contains as many elementary entities (atoms, molecules, formula units or other particles) as there are atoms in exactly 12.00 grams of 12 C

buffer capacity

amount of acid or base the buffer can neutralize before the pH begins to change an appreciable degree

Heat Capacity (C)

amount of heat (q) required to raise the temperature of a given quantity (m) of the substance by one degree Celsius C = Gj/gC C = ms C = J/C

Solubility

amount of solute that will dissolve in a specific amount of solvent

Phosphate (PO4)

antacid, cathartic

Carbon Trioxide (CO3)

antacid, for effervescent tablet

Ca Gluconate

antidote to magnesium

selenium sulfide (SeS2)

antiseborrheic, antidandruff

Zinc Oxide (ZnO)

antiseptic

hydrogen peroxide (H2O2)

antiseptic; Agua Oxigenada; Thenard's Oxygenated Acid Official preparation: 3% or 10 volumes Oxidizing antiseptic Continuous use as mouthwash produce "hairy tongue" (hypertrophied filiform papillae) acid to increase its stability

Endothermic process

any process in which heat has to be supplied to the system from the surroundings

Exothermic process

any process that gives off heat - transfers thermal energy from the system to the surroundings

Matter

anything that takes up space and has mass

Heterogenous Equilibrium

applies to reaction in which reactants and products are in different phase

Homogenous Equilibrium

applies to reactions in which all reacting species are in the same phase

Electrochemistry

area of chemistry that deals with interconversion of electrical energy and chemical energy

Electrolytic Cell

area of chemistry that deals with interconversion of electrical energy and chemical energy

Newlands

arranged all known elements, starting with hydrogen and ending with thorium into 7 groups of eight which he likened to octaves of music

radioactive

atoms emitting particles or radiation; atoms with atomic number greater than 83; unstable

isotopes

atoms of same element (X) with different number of neutrons in the nuclei; same with atomic number but different mass number or number of neutrons

triple bonds

atoms share three pairs of electrons

fermentation

bacteria/microorganism + organic substance --> alcohol

Tc99m Etidroonate

bone imaging

Group III-A (periodic table)

boron

Tc99m Glucoheptonate

brain imaging

Tc99m sodium pertechnetate

brain scanning to determine presence and location of neoplastic lesions

Hund's Principle

building process where electrons occupy orbitals with the lowest level and filling each to capacity before the next is started; order of occupancy of sublevels with the notation nl^x - n (energy level), l (sublevel), and x (number of electrons in the orbital or subshell)

Reaction Quotient (Qc)

calculated by substituting the initial concentrations of the reactants and products into the equilibrium constant (Kc) expression

amphoteric oxide

can be base or acid

Group IV-A (periodic table)

carbon

carbon dioxide

carbon anhydride, dry ice (solid CO2) Solid form used as caustic; in carbonated beverages; and to displace air in pharmaceutical preparation Stored in gray cylinders

Silver Nitrate (AgNO3)

causes argyria a discoloration in the skin (removed by injection of 6% sodium thiosulfate and 1% potassium ferricyanide)

Reaction Rate

change in the concentration (M) of a reactant or a product with time (s) (expressed as M/s)

nuclear change

change in the identity of the nucleus of an atom; transmutation of an element to another element

sodium thiosulfate (Na2S2O3.5H2O)

chemical antidote to CN and Iodine

Single Covalent Bond

chemical bond formed when two electron pairs are shared

displacement (replacement) (substitution)

chemical change illustrated by 3 K + FeI3 --> 3 KI + Fe

combination (synthesis)

chemical change illustrated by A + B --> AB

decomposition (analysis)

chemical change illustrated by AB --> A + B

empirical formula

chemical formula based on formula units; gives the smallest whole number ratio

structural formula

chemical formula that shows the arrangement of atoms in a molecule of a compound; Compounds are connected with dashes

lewis (electron) formula

chemical formula that shows the distribution of electrons in the outermost shell of the atom; Symbols of elements are written with dots around and these dots represent the number of electrons in the outermost shell of an atom

voltaic (galvanic) cell

chemical reaction produces electrical energy

silicosis

chronic condition resembling chronic TB due to exposure to silica properties

Meyer and Mendeleev

claimed that physical and chemical properties are periodic functions of their atomic weight

Talc

clarifying, dusting agent

Ideal Gas Equation

combining all the variable involving gases PV = nRT

Haber's Process

commercial method of ammonia

povidine iodine

complex of iodine with povidone, a polymer PVP, polyvinylpyrrolidone, release I2 slowly and is non-toxic and non-irritating

ionic compound

compound formed from ions that are either cation (+) or anion (-) (metal & non-metal)

Antoine Laurent Lavoisier

constructed the first periodic table

calcarones (sicily)

crude furnace semi-circular stone wall pits dug to recover sulfur

Zinc Eugenol Cement

dental protective

Rutherford-Bohr Model

depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus - similar in structure to the Solar System

Potassium Bromide

depressant/sedative

JJ Thomson

discovered the electron

Ernest Rutherford

discovered the proton

Atomic Radius

distance between two nuclei

electron configuration

distribution of electrons in the different shells and subshells or orbitals within the atom

effect of adding a catalyst on equilibrium

does not change K; no shift in the position of an equilibrium system; only change in temperature will affect equilibrium constant

nucleon

either proton or neutron, considered in its role as a component of an atomic nucleus

lewis acid

electron acceptor

lewis base

electron donor

> 2 or 1.7 - 3.2

electronegativity difference in ionic covalent bonds

0 - 0.5

electronegativity difference in non-polar covalent bonds

Cadmium Chloride (CaCl2)

emetic, treatment of Tinea infection

Negatron

emitted by unstable nuclei having neutrons in excess of protons elements undergoing this type of transformation will decay to the element having the next highest at no.

Heat of Vaporization

energy required to change 1 g of liquid vapour at its normal boiling point energy = mass * heat of vaporization

Heat of Fusion

energy required to change 1 g of solid at its melting point into a liquid energy = mass * heat of fusion

Formation (Stability) Constant (Kf)

equilibrium constant for the complex ion; high Kf = high stability of complex

Iron (Fe+2 or Fe+3)

essential trace ion constituent of hemoglobin

Sulfur

essential trace ion constituent of protein mucopolysaccharide, heparin, biotin, detoxification

Cobalt (Co +2)

essential trace ion constituent of vit B12

copper

essential trace ion formation of Hb; constituent of oxidase enzyme

Iodine (I-)

essential trace ion constituent of thyroxin triiodothyronine

stability of nuclei

even - even (most stable) even - odd odd - even odd - odd (least stable)

talc (3MgO.4SiO3.H2O)

example of protective, a hydrated magnesium silicate with aluminium acetate

KI

expectorant in cough syrup

aristotlean and platonic theory of the atom

favored the earth, fire, air, and water approach to the nature of matter

inert gases (noble gases)

filled s or orbitals (with 8 valence e- except He)

diluent

filler material which brings the tablet up to acceptable size ex. CaSO4, colloidal silicon dioxide (SO2)

sigma bond (s)

first bond between two atoms formed by direct or head-on overlap of 2s orbitals, 2p orbitals or an s or p orbitals

yellowish green

flame test on Ba+2

brick or dull red

flame test on Ca+2

violet

flame test on K+

crimson or carmine red

flame test on Li+

colorless

flame test on Mg+2

intense yellow

flame test on Na+

crimson or carmine red

flame test on Sr+2

sodium chromate Cr 52 injection (Chromitope Na, Rachromate-51)

for RBC mass, volume and survival time, scanning of spleen

Neon

for advertising

ion-induced dipole

forces between ionic compound or ion and non-polar molecule

ion-dipole forces

forces between ionic compounds or ions and polar molecules

induced dipole-induced dipole

forces between non-polar molecules

dipole-induced dipole

forces between polar and non-polar molecules

dipole-dipole forces

forces between polar molecules

Covalent Bonds

form of chemical bond that involves the sharing of electrons; held by weaker intermolecular forces (weaker)

Ionic/Electrocovalent Bonds

form of chemical bond that involves the transfer of electrons; held by strong electrostatic forces (more stable); Alkali and alkaline earth metals form cations (+) in ionic compound [cation - atom loses an electron] Halogens and oxygen form anions (-) in ionic compound [anion - atom gains an electron]

non-polar covalent bond

form of covalent bond that involves equal sharing of electrons; no dipole moment Shared pair of electrons will be midway between the 2 atoms giving rise to an electrically symmetrical molecule; Van der Waals/London Dispersion forces: forces present

Work

form of energy transfer between a system and its surrounding in the form of compression or expansion

molecular compound

form of individual molecules composed of atoms (non-metals)

Physical Matter

form of matter that has definite composition and distinct properties

covalent compound

formed by sharing of electron; non-metals (acids, NH3, water, organic compounds, gases) Non-conductors [no ions (insoluble) in water]; low melting point, boiling point, etc Weak intermolecular forces, unstable, easier to break

ionic compound

formed by transfer of electron; metal and non-metal (salts, bases except NH3) Conductors of electricity [produce ions (soluble) in water]; high melting point, boiling point, density, solubility Bonded with strong electrostatic forces; stable; hard to break

molecular formula

formula based on actual molecule; gives the actual number of atoms of each element

representative elements

found in the outermost shell and correspond to their group number

examples of protective and adsorbent

gastrointestinal agent used for treatment of mild diarrhea

protective and adsorbent

gastrointestinal agent used for treatment of mild diarrhea

Electron Density

gives probability than an electron will be found in a particular region of an atom

(NH4)2S or Al - Fe (NH4)2S or NH4Cl, NH3 & H2S

group precipitant for (NH4)2S or Al - Fe

NH3, NH4Cl, (NH4)2CO3 & 95% C2H5OH

group precipitant for Alkaline Earth

Adjust H to 0.3 M and saturate with H2S

group precipitant for H2S / Cu-Tin

Silver or Chloride 2 M/3M HCl or NH4Cl or any soluble chloride salt

group precipitant for silver/chloride

Group VII-A (periodic table)

halogens

standard enthalpy of formation (ch H)

heat change that results when one mole of a compound is formed from its elements at a pressure of 1 atm and 25 C; expressed in KJ/mol; of any element (standard state) in its most stable form is zero

Equilibrium constant (Kc)

helps to predict the direction of a reaction

Tc99m-IDA or HIDA

hepatobillary studies

type I glass

highly resistant, borosilicate glass

Solution

homogenous mixture of 2 or more substances

Sodium Thiocyanate

hypotensive agent

Positron

identical to the electron with the exception of having a + charge Emitted from nuclei having a proton/neutron ratio above stable limits

Tc99m-phytate

imaging for liver, lymph nodes and patency studies

inner transition (lanthanide and actinide series)

incompletely filled f orbitals; 2 series of elements

Catalyst

increases the rate of chemical reaction without itself being consumed

van der Waals forces

induced dipole-induced dipole ion-induced dipole dipole-induced dipole

helium

inert gases admixed with oxygen 80% He: 20% O2 forms a respirable air 1/3 the density of air Reduced risk of bends in deep sea diving Stored in brown cylinders

bacteriostatic water for injection

intended for compounding small volume of extemporaneous parenteral for IM injection

Ernest Rutherford

investigated structure of atomic nucleus; used gold foil as experimental design

Complex Ion

ion containing a central metal cation bonded to one/more complex molecules or ions (ligands)

Lead Oxide (PbO)

litharge

Tc99m-hepatogluconate

liver imaging and potential studies

sulfurated potash

liver of sulfur

Na2PO4 Sodium Albumin

localization of ocular tumor

node

locus of points in an atom where the electron density is zero

Buffer

maintains the pH of various formulation within the prescribed limits

calcium

major physiological ion buffer constituent, acid-base balance, water balance, CO2 transport, neuromuscular irritability

potassium

major physiological ion buffer constituent, acid-base balance, water balance, CO2 transport, neuromuscular irritability

sodium

major physiological ion buffer constituent, acid-base balance, water balance, CO2 transport, osmotic pressure, cell membrane permeability, muscle irritability

magnesium

major physiological ion co-factor for PO4, transferring enzyme, constituent of bones and teeth

phosphorus

major physiological ion constituent of bones and teeth, constituent of buffer, constituent of ATP, NAD, & FAD

chloride

major physiological ion maintain normal hydration and osmotic pressure, gastric HCl, acid and base balance

number of neutrons

mass number - atomic number (A-Z)

molar mass

mass of 1 mole of atoms in grams

Mass Defect

mass of energy binding the nucleus and is the difference between the mass of a nucleus and the sum of masses of the nucleons of which it is composed

Democritus' theory of the atom

matter could not be divided into smaller and smaller pieces (atoms - atomos); Atoms are indivisible

Curie (Ci)

measure of radioactivity

Cupric Sulfate

mechanical antidote for phosphorus

activated charcoal

mechanical antidote, general purpose anditdote

Cu+2, Cd+2, Pb+2, Bi+3

members of H2S/ Cu-Tin basic constituent/cation group, Cu subgroup (insoluble in Na2S)

Hg+2, As+3+5, Sn+2+4, Sb+3+5

members of H2S/ Cu-Tin basic constituent/cation group, Tin subgroup (soluble in Na2S)

Ag+, Pb+2, Hg2+2

members of silver/chloride basic constituents/cation group

Al+3, Cr+3, Zn+2

members of the (NH4)2S or Al-Fe basic constituent/cation group, Al subgroup (soluble in NaOH and Na2O2)

Fe+2+3, Mn+2, Ni+2, Co+2

members of the (NH4)2S or Al-Fe basic constituent/cation group, Fe subgroup (insoluble in NaOH and Na2O2)

Ba+2, Sr+2, Ca+2, Mg_2

members of the Alkaline Earth basic constituent/cation group

Decantation, evaporation, magnetic separation, centrifugation, distillation, sorting, filtration, fractional distillation

methods of separating compounds

Critical Mass

minimum amount of fissionable material required to generate a self-sustaining nuclear chain reaction

Polyatomic molecule

molecule that contains more than 2 atoms of the same element or different elements (molecular compound)

Diatomic molecule

molecule that contains only 2 atoms of same element or different elements

oxygen

name means acid former by Lavoisier "Dephlogisticated Air" by Priestly and "Empyreal Air" by Scheele Commercially available by fractional distillation of liquid air and electrolysis of water Stored in green cylinders Anoxic - inadequate oxygen tension in air (high altitude)

silicate (talc, asbestos) carbonate (magnesite, dolomite) sulfate (kieserite)

natural sources of magnesium

Group V-A (periodic table)

nitrogen

Pauli's Exclusion Principle

no two electrons in an atom can have the same set of quantum numbers

Group VIII-A (periodic table)

noble gases

chromium

non essential ion used for glucose tolerance

lead

non-essential ion lead encephalopathy resulting to brain damage or mental retardation

lithium

non-essential ion that is a CNS depressant, used in maniac depressive disorder and has diuretic action

aluminum

non-essential ion that's an astringent and antiseptic, astringent, used as deodorant

fluoride

non-essential ion used as anti-cariogenic

mercury

non-essential ion used as diuretic, antiseptic, parasiticide and fungicide

silver

non-essential ion used as protein precipitant, antiseptic, astringent, irritant to corrosive

strontium

non-essential ion used as sedative, osteoporosis, dentrifice as tooth temperature, desensitizing agent

cadmium

non-essential ion used for severe bone pain, waddling gait aminoaciduria, severe osteomalacia

gold

non-essential ion used in rheumatoid arthritis and lupus erythematosus

weak electrolytes

not completely ionized/dissociated; undergoes reversible reaction (<- ->)

Johann Dobereiner

noted that there were groups of 3 elements (hence "triads") which had similar physical properties (ex. Li, Na, K; Ba, Ca, Sr; Cl, Br, I)

nuclear transmutation

nuclei will undergo change as a result of bombardment by neutrons, electrons or other nuclei

isotones

nuclides with same number of neutrons

nucleon number

number of nucleons; isotope's mass number

mass number (atomic mass)

number of protons + number of neutrons; atomic number (Z) + number of neutrons

Reduction (GEROA)

o Oxidizing Agent/Oxidant - substance gains electrons and thus decreases in oxidation state (+ -> 0 -> -) o Accepts electrons readily o Gains electrons or take up electrons (loss in oxidation number) o Said to be reduced (substance receiving electrons)

Oxidation (LEORA)

o Reducing Agent/Reductant - substance loses electrons and thus increase in oxidation state ( - -> 0 -> +) o Donates electrons o Loses electrons (gain in oxidation number) o Said to be oxidized (substance which furnishes electrons)

resonance structure

one of two or more Lewis structure for a single molecule that cannot be represented; accurately by only 1 Lewis structure

isohydric solution

one with same pH as another solution tho which it is compared

Cadmium Sulfate (CdSO4)

ophthalmic antiseptic

transition elements

outer electrons and some from the inner orbitals; incomplete filled d orbital

Group VI-A (periodic table)

oxygen

examples of inhalants

oxygen carbon dioxide helium nitrous oxide nitrogen

Gifford's borate buffer

pH 6-7.8, similar to Feldman's however in place of NaCl, KCl is used to make it hypotonic

Fieldman's borate buffer

pH 7-8.2, acid solution containing H3BO3, NaCl and alkaline solution containing Na2B4O7

Atkin's and Pantin's borate buffer

pH 7.6-11, alkaline solution of Na2CO3 and acid buffer solution of H3BO3 and NaCl

henderson-hasselbach equation

pH = pKa + log[CB/A]

Boulton's Solution

phenolated I2 solution

sodium nitrite (NaNO2)

physiological antidote for CN

"Like dissolves like"

polar dissolves polar, non-polar dissolves non-polar

silica fume

prepared from condensation of silica from its vapour phase

silica gel

prepared from the hydrolysis of organic and inorganic orthosilicates

Boyle's Law

pressure and volume are inversely related at constant temperature PV = K P1V1=P2V2

antioxidant

prevents oxidative decomposition of pharmaceutically active component

water

primary solvent of liquid phase in most liquid pharmaceutical preparation

antacid

product for altering gastric pH

Al(OH)3 white gelatinous ppt

product of reaction between Al+3 with NH4Cl and NH4OH & (NH4)2S

Soluble CoS black ppt

product of reaction between Co+2 with NH4Cl and NH4OH & (NH4)2S

Cr(OH)3 grayish green ppt

product of reaction between Cr+3 with NH4Cl and NH4OH & (NH4)2S

Soluble FeS black ppt

product of reaction between Fe+2 with NH4Cl and NH4OH & (NH4)2S

Fe(OH)3 reddish brown ppt Fe2S3 black ppt

product of reaction between Fe+3 with NH4Cl and NH4OH & (NH4)2S

As2S3 Na3AsS4 - soluble in Na2S Yellow ppt Colorless solution

product of reaction between H2S and As+3

Bi2S3 Dark brown ppt or brownish black ppt

product of reaction between H2S and Bi+3

CuS Black ppt

product of reaction between H2S and Cu+2

HgS Na2HgS2 - soluble in Na2S White to yellow to brown to black ppt Colorless solution

product of reaction between H2S and Hg+2

PbS Black ppt

product of reaction between H2S and Pb+2

Sb2S3 Na3SbS4 - soluble in Na2S Orange ppt or reddish orange ppt Colorless solution

product of reaction between H2S and Sb+3

Sn+2 SnS SnS2 Na2SnS3 - soluble in Na2 Light brown ppt Yellow ppt Colorless solution

product of reaction between H2S and Sn+2

Soluble MnS flesh or salmon ppt

product of reaction between Mn+2 with NH4Cl and NH4OH & (NH4)2S

AgOH Ag(NH3)2+ with excess NH4OH soluble, colorless solution

product of reaction between NH4OH & Ag+

Al(OH)3 White gelatinous ppt

product of reaction between NH4OH & Al+3

Cu(OH)NO3 Cu(NH3)4+2 or Cu(NH3)4(OH)2 with excess NH4OH Green basic salt Soluble - blue solution

product of reaction between NH4OH & Cu+2

Co(OH)NO3 Co(NH3)4+2 with excess NH4OH Blue basic salt Soluble - dirty yellow solution

product of reaction between NH4OH and Co+2

Cr(OH)3 Grayish green ppt

product of reaction between NH4OH and Cr+3

Fe(OH)2 white to green to brown ppt

product of reaction between NH4OH and Fe+2

Fe(OH)3 reddish brown ppt

product of reaction between NH4OH and Fe+3

Ni+2 Ni(OH)NO3 Ni(NH3)4+2 with excess NH4OH Green basic salt Soluble - blue solution

product of reaction between NH4OH and Ni+2

Zn(OH)2 Zn(NH3)4+2 with excess NH4OH White ppt Soluble - colorless ash

product of reaction between NH4OH and Zn+2

AgOH to Ag2O White to brown ppt

product of reaction between NaOH and Ag+

Al(OH)3 White gelatinous ppt

product of reaction between NaOH and Al+3

Co(OH)2 Co(OH)3 with Na2O2 or H2O2 Blue ppt. on warming pink ppt Brown ppt or black ppt

product of reaction between NaOH and Co+2

Cr(OH)3 Grayish green ppt

product of reaction between NaOH and Cr+3

Fe+2 Fe(OH)2 Fe(OH)3 with Na2O2 or H2O2 White to green to brown ppt Reddish brown ppt

product of reaction between NaOH and Fe+2

Fe(OH)3 Reddish brown ppt

product of reaction between NaOH and Fe+3

NaOH Black ppt

product of reaction between NaOH and Hg+2

Mn(OH)2 MnO2.H2O with Na2O2 or H2O2 White ppt Brown ppt

product of reaction between NaOH and Mn+2

Ni+2 Ni(OH)2 Ni(OH)3 with H2O2 no oxidation with Na2O2 Apple green ppt Green ppt

product of reaction between NaOH and Ni+2

Pb(OH)2 Pb(OH)4-2 or Na2PbO2 with excess NaOH White amorphous ppt Colorless solution

product of reaction between NaOH and Pb+2

Zn(OH)2 Na2ZnO2 with excess NaOH White ppt Soluble - colorless solution

product of reaction between NaOH and Zn+2

Soluble NiS black ppt

product of reaction between Ni+2 with NH4Cl and NH4OH & (NH4)2S

Soluble ZnS white metallic ppt

product of reaction between Zn+2 with NH4Cl and NH4OH & (NH4)2S

Extensive (extrinsic) property

property of matter that depends upon how much (quantity) matter is being considered: mass, size, length, shape, volume

Electron Affinity

property to accept an electron from a (+) atom

Solubility Product Constant (Ksp)

proportional with solubility

Plum Pudding Model

proposed by J J Thomson; he believed that the negative electrons were spread evenly throughout the positive charge of the rest of the atom

Henry Moseley

proposed that elements are to be arranged based on their atomic number

bronsted base

proton acceptor

bronsted acid

proton donor

Sodium Rose Bengal I-131 (Robengatope)

radioactive tracer for lvier function

Mixture

A combination of two or more substances wherein the substance retains their distinct identities

RBE (relative biological effectiveness)

ratio of biological effectiveness of one type of ionizing radiation relative to another, given the same amount of absorbed energy

redox reactions

reaction in aqueous solutions that bear change in the electrical charge on the reacting particles; change in oxidation number; simultaneous gain and loss of electrons

non-redox reactions

reaction in aqueous solutions that bear no change in oxidation number

Law of Mass Actions

relates the concentration of reactants and products at equilibrium in terms of quantity called equilibrium constant

Fractional Precipitation

removing selected ions from solution while leaving others with similar properties in solution

Rad & gray

replaced rad units commonly used to measure amount of exposure due to radiation

acidic solution

salt with strong acid + weak base; will hydrolyze

neutral solutions

salt with strong base + strong acid; no hydrolysis

Group IVB (Titanium Subgroup)

All members of the group occur in nature only in combined state Oxidation state +2, +4 Possess amphoteric property and their cation readily form complex

Aluminum Chloride (AlCl3.6H2O)

Astringent, antiseptic, antiperspirant/deodorant

Zirconium

same as aluminium, UV ray protectant Banned due to granuloma formation Former official compound (Oxide, Carbon Trioxide) Used as antiperspirant and athlete's foot

Sulfur

scabicide to kill mites, Sarcoptes scabiei, 3% in ointment

Gold Au 98 (Aurcoloid 198, Aureotope, Auroscan)

scanning of liver

Sodium Iodide I-131, I-123 (Iodotope-131, Iodotope 123)

scanning of thyroid gland

Calcium Bromide (CaBr2)

sedative/depressant

Chromium

Essential trace element, Glucose tolerance factor Deficiency: hyperglycemia

Potassium Sodium Tartrate

KNaC4H4O6 "Rochelle Salt", "Sal Signette" Cathartic, sequestering agent, strong oxidizing agent

bent/angular

shape of polar molecule