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
