Pharmaceutical Inorganic Chemistry Lecture Notes 2024 PDF

# Lecture Notes on Pharmaceutical Inorganic Chemistry 2024 Edition ## Preface Lecture Notes for Pharmaceutical Inorganic Chemistry is a comprehensive guide designed to provide students with a thorough understanding of the fundamental concepts and applications of inorganic chemistry within the pharm...

# Lecture Notes on Pharmaceutical Inorganic Chemistry 2024 Edition ## Preface Lecture Notes for Pharmaceutical Inorganic Chemistry is a comprehensive guide designed to provide students with a thorough understanding of the fundamental concepts and applications of inorganic chemistry within the pharmaceutical sciences. This material is meticulously structured to bridge the gap between theoretical principles and practical applications, ensuring a holistic learning experience. ## Module 1: Fundamentals of Inorganic Chemistry The course begins with an exploration of the core principles that form the foundation of inorganic chemistry. This module introduces the basics of matter and atomic structure. Students will explore atomic models, quantum numbers, and electron configurations, and learn how these factors influence chemical properties. Additionally, students will examine the periodic table and its role in organizing elements. A solid grasp of these fundamentals is essential, as they underpin the more complex topics covered in subsequent modules. ## Module 2: Chemistry of Elements in the Periodic Table Building on the foundational knowledge, the second module offers an in-depth study of the elements in the periodic table. Each element's unique properties and their interactions will be explored in detail, with a particular focus on their relevance to pharmaceutical applications. This module covers the chemistry of main group elements, transition metals, and inner transition metals, highlighting their roles in various chemical processes and their significance in the development of pharmaceutical agents. ## Module 3: Inorganic Compounds of Biological and Pharmaceutical Significance The final module integrates the principles and knowledge from the previous modules to focus on inorganic compounds that play crucial roles in biological systems and pharmaceutical applications. Students will learn about essential elements, inorganic compounds, and their therapeutic uses. By the end of this module, students will gain a deeper understanding of how inorganic chemistry contributes to health and medicine, bridging the gap between chemical science and its practical applications in biological systems. ## Disclaimer and Fair Use Statement The content within this compiled lecture notes material includes references to copyrighted works. The use of such copyrighted material is intended solely for educational purposes and is presented in accordance with the principles of "fair use," as defined under applicable intellectual property laws. The inclusion of copyrighted material here does not imply endorsement or authorization by the copyright holders. For any use of these materials beyond the scope of "fair use," explicit permission from the respective copyright owners must be obtained. This statement is provided to ensure clarity on the use of copyrighted content and to comply with intellectual property regulations. # Module 1: Fundamentals of Inorganic Chemistry ## Chemistry - The science that describes matter - its properties, the changes it undergoes, and the energy changes that accompany those processes - The Central Science ## Branches of Chemistry - Organic chemistry - Hydrocarbons and its derivatives - Inorganic chemistry - Inorganic compounds, metals, minerals - Analytical chemistry - Detection and identification of substances present (qualitative analysis) or amount of each substance (quantitative analysis) - Biochemistry - Processes in living organisms - Physical Chemistry - Behavior of matter ## States of Matter | State | Description | |---|---| | Solid | Molecules packed close together orderly, rigid | | Liquid | Molecules are close but randomly arranged, flows and assumes shape of container | | Gas | Molecules are far apart, fills any container completely | ## Changes of States - Solid - Melting - Freezing - Sublimation - Deposition - Liquid - Boiling - Condensation - Gas ## A1. Matter ### Matter and Energy - **Matter** - anything that has mass and occupies space - **Mass** - measure of the quantity of matter - **Volume** - amount of space - **Energy** - the capacity to do work or to transfer heat - **Types:** - Kinetic energy: Energy in motion - Potential energy: Energy at rest - **Energy Changes:** - Exothermic - release (heat) - Endothermic - absorbs (heat) ### Extensive and Intensive Properties - **Extensive Properties** - Dependent on the amount of substance - e.g. MASS: more substance, greater mass - e.g. VOLUME: more substance, greater volume - **Intensive Properties** - Independent on the amount of substance - e.g. DENSITY, Electrical Conductivity ### Physical and Chemical Changes - **Chemical Change** - one or more substances are used up - one or more new substances are formed - energy is absorbed or released - **IRREVERSIBLE** - e.g. burning of paper, cooking an egg, souring of milk - **Physical Change** - no change in chemical composition - **REVERSIBLE** - e.g. shredding paper, boiling of water, breaking a bottle ### Classification of Matter - **Matter** - Does it have constant properties and composition? - **No:** Mixture - **Yes:** Pure substance - **Mixture** - Is it uniform throughout? - **No:** Heterogeneous - **Yes:** Homogeneous - **Pure Substance** - Can it be simplified chemically? - **No:** Element - **Yes:** Compound ### The Atomic Number (Z) - The number of protons in the nucleus of an atom determines its identity; this number is known as the atomic number of that element. - e.g. Hydrogen atom contains 1 proton. Lithium atom contains 3 protons. ### The Mass Number (A) - The mass number of an atom is the sum of the number of protons and the number of neutrons in its nucleus; that is: - Mass Number = # of p + # of n - Mass Number = Atomic Number + Neutron Number ### Isotopes - Isotopes are atoms of the same element with different masses. - They are atoms containing the same number of protons but different numbers of neutrons. ### The Atomic Weight - Many elements occur in nature as mixtures of isotopes. - The atomic weight of such an element is the weighted average of the masses of its isotopes. - Atomic weights are fractional numbers, not integers. ### A2. Atom and Its Electronic Structure ### The Atom - The smallest unit that retains the properties of an element. - **Dalton's Theory** - All matter is composed of atoms and these cannot be made or destroyed. ### Atomic Structure - The nucleus is composed of protons and neutrons. Protons are positively charged and neutrons have no charge. - The nucleus is surrounded by electrons which are negatively charged and occupy space outside the nucleaus. ### A3. Development of Atomic Models #### Early History - **Leucippus and Democritus (500 BC)** - Greek word "Atomos" - uncuttable - Atom as solid indivisible sphere - **Aristotle and Others** - Matter is made up of four elements #### Dalton's Atomic Theory - **John Dalton (1807)** - Solid Sphere (Billiard Ball) Model - Atom as solid sphere but NOT indivisible #### The Discovery of Electrons - **Humphry Davy (1800s)** - Elements of a chemical compound are held together by electrical forces. - **Michael Faraday (1832)** - Relationship between the amount of electricity used in electrolysis and the amount of chemical reaction that occurs. - "Electrons"; Electric ions - **George Stoney (1891)** - "Electrons" #### The Discovery of Electrons - **Cathode-Ray Tube Experiment** - Joseph John Thomson (1897) - Most convincing evidence of electrons - Plum pudding model - **Oil-drop Experiment** - Robert Millikan (1909) - Determine the charge of electrons #### The Discovery of Protons - **Canal Rays Experiment** - Eugen Goldstein (1886) - Cathode-ray tube also generates a stream of positively charged particles - These positive rays, or positive ions, are created when the gaseous atoms in the tube lose electrons. #### Rutherford's Model - **The Scattering Experiment** - Ernest Rutherford (1910) - Assumption: If the Thomson model of the atom were correct, any alpha-particles passing through the foil would have been deflected by very small angles. Quite unexpectedly, nearly all of the a-particles passed through the foil with little or no deflection. - **Rutherford's Conclusion:** - Atoms consist of very small, very dense positively charged nuclei surrounded by clouds of electrons at relatively large distances from the nuclei. - **Nuclear Model** - Positive charge localized in the NUCLEUS #### The Discovery of Neutrons - **J. Chadwick (1932)** - bombardment of beryllium with high-energy alpha-particles produced NEUTRONS #### Bohr's Model - **Niels Bohr** - described the electron of a hydrogen atom as revolving around its nucleus in one of a discrete set of circular orbits. - **Bohr's Planetary Model** - Each orbit thus corresponds to a definite energy level for the electron. - When an electron is excited from a lower energy level to a higher one, it absorbs a definite (quantized) amount of energy. - Electrons occupy only certain energy levels in atoms. #### The Wave Nature of Electron - **Louis de Brogli** - proposed the idea of wave-like nature of electrons - Electrons can be treated as waves more effectively than as small compact particles traveling in circular or elliptical orbits. #### Quantum Mechanics - **Quantum mechanics** - Based on the wave properties of matter - **Werner Heisenberg's Uncertainty Principle (1927)** - For electrons, it is not possible to determine the exact momentum and the exact position at the same moment in time. - **The mathematical approach of quantum mechanics** - involves treating the electron in an atom as a standing wave. #### Erwin Schrödinger's Wave Equation - It estimates the position of electrons and quantifies energy levels. #### Atomic Orbitals - A region of space in which the probability of finding an electron is high. #### Atomic Number of an Element - **H.G.J. Moseley (1913)** studied X-rays given off by various elements. - "The number of protons in the nucleus of an atom determines its identity; this number is known as the atomic number of that element." ### A4. Quantum numbers - Each atomic orbital is described by a set of quantum numbers. - Principal QN (n) - Orbital QN (1) - Magnetic QN (m₁) - Spin QN (ms) - **Principal Quantum Number (n)** - n = 1, 2, 3, ... (n) - Orbital → SHELL or ENERGY LEVEL - Distance of the electron from the nucleus - Higher n, higher energy - **Angular momentum quantum number (l)** - l = 0, 1, 2, 3, ... (n-1) - Orbital → SUBSHELL/ SUBLEVEL - Shape of the orbital - l=0: s: spherical - l=1: p: dumb-bell - l=2: d: clover leaf - l=3: f: complex - **Magnetic Quantum Number (m₁)** - m₁ = -l... 0 ... + 1 - Orbital → Specific orbital - Orientation in space of the orbital - **Spin Quantum Number (ms)** - For each INDIVIDUAL ELECTRON only - 2 - _ms_ = +- - Direction of spin (clockwise or counter-clockwise) - Quantum Number and Electron Configuration ### A5. Electron Configuration - **Electron Configuration** - "Distribution of electrons" - describes the number and arrangement of electrons in orbitals, subshells and shells in an atom. - **Ground state:** Atom in its lowest energy, or unexcited, state. - **Rules in Predicting the Electron Configuration of an Atom** - **Aufbau principle:** Orbitals fill in order of increasing energy, from lowest to highest. - **Pauli Exclusion Principle:** No more than two electrons can occupy each orbital, and if two electrons are present, they must have opposite spins. - **Hund's Rule:** The order of fill is the same but as you can see from above the electrons are placed singly into the boxes before filling them with both electrons. A single electron will occupy an empty orbital first before pairing. - **Orbital Diagrams** - Another way to represent the order of fill for an atom is by using an orbital diagram often referred to as "the little boxes." - **Simplified Notation: Noble Gas Configuration** - An atom consists of the elemental symbol of the last noble gas prior to that atom, followed by the configuration of the remaining electrons. - **Writing the Electron Configuration using the Periodic Table** - Start from left to right and continue writing down the electron configuration. - If you reach the d-block, use n-1 for the energy level, e.g. 3d1. - If you reach the f-block, use n-2 for the energy level, e.g. 3f1 ### A6. The Periodic Table of Elements - **Dimitri Mendeleev** - Based on chemical properties - **Lothar Meyer** - Based on physical properties - **Both emphasized the periodicity, or regular periodic repetition of properties with increasing atomic weight.** - **Elements are now arranged in the periodic table in order of increasing atomic number.** - **Periodic Law:** "The properties of the elements are periodic functions of their atomic numbers." ### Periodic Trends - **Atomic radius** - LOWER LEFT - **Ionization energy** - UPPER RIGHT corner - **Electronegativity** - UPPER RIGHT corner - **Electron affinity** - UPPER RIGHT corner - **Nonmetallic character** - UPPER RIGHT corner - **Metallic character** - LOWER LEFT # Module 2: Chemistry of Elements in the Periodic Table ## B1. Group IA - The Alkali Metals - Li, Na, K, Rb, Cs - Univalent, +1 - Soft, waxy, and has high metallic luster - Low sp.gr.; low MP - Alkali salts are freely-soluble in water - Forms simple cations - Most active, electro-positive metals - Easily oxidized in air (stored under mineral oil) - Reacts with water violently - M + H2O → H2 + MOH - Oxides and hydroxides are strongly BASIC ### B1.1 Lithium - Greek word lithos - "stone" - Lightest metal - Carmine red in non-luminous flame - Former ingredient of 7Up® - contained lithium citrate - As hangover cure - Li was removed following death of 4 US Patients - Li+ - CNS depressant - Li toxicity - nephrotoxicity (kidney damage) - **Lithium bromide** - hypnotic - **Bromide syrup** - Bromides of Li, Na, K, Ca and NH4+ - sedative - **Lithium carbonate** - Antacid, antirheumatic, diuretic - **Lithium citrate** - Antacid - less irritating to stomach ### B1.2 Sodium - Latin name Natrium, obtained from niter - Discovered by Sir Humphry Davy (electrolysis of NaOH - caustic soda) - Abundant in nature in the form of NaCl - rock salt - Bright golden yellow in non-luminous flame - Na+ - predominant cation in ECF - **Sodium hydroxide** - "Caustic soda, lye" - Very deliquescent - absorbs moisture in air and liquifies - Escharotic - corrosive to tissue - Uses: - in soap preparations - as standard solution in acid-base titrations - **Sodium chloride** - "Rock salt, table salt" - Electrolyte replenishment - Renders solutions to be isotonic - Prescription "fiat isotonic collyrium" - Normal saline solution (NSS), 0.9% NaCl - Physiological salt solution - **Sodium acetate** - Diuretic, treatment of cystitis and UTI - **Sodium carbonate** - Anhydrous → "soda ash" - Decahydrate → "sal soda", "washing soda" - as anhydrous - buffer preparations - as solution - lotion preparations - **Sodium bicarbonate** - "Baking soda" - Antacid - Misuse can lead to "rebound acidity" - Urinary alkalizer - **Sodium nitrite** - Smooth muscle relaxant (slow onset) for angina pectoris - Treatment for cyanide poisoning - **Sodium citrate** - Oral: alkalizer, diuretic - Parenteral: anticoagulant - **Sodium phosphate** - disodium hydrogen phosphate - dibasic sodium phosphate - Saline laxative, cathartic - **Sodium biphosphate** - sodium dihydrogen phosphate - monobasic sodium phosphate - Urinary acidifier - **Sodium thiocyanate** - antihypertensive - **Sodium thiosulfate** - External: ringworm infection - IV: dermatitis - Treatment for iodine and cyanide poisoning - **Sodium sulfate** - "Glauber's salt" - Saline laxative - **Sodium borate** - "Borax", sodium tetraborate - Bacteriostatic (as eye-wash and wet dressing) - Water-softener - **Sodium bromide** - Sedative - **Sodium iodide** - Solubilizing agent in iodine solution - Histolytic - destroys tissues - Expectorant - **Sodium hypochlorite** - Sodium hypochlorite Solution (5% NaOCl) - laundry bleaching agent - "Labarraque's Solution" - NaOCI diluted with equal volume of water - Oxidizing and bleaching agent - Modified Dakin's solution - Diluted NaOCI solution (0.5%) - Disinfectant, irrigating solution for wound - **Compound effervescent powders** - "Seidlitz powders" - Mild laxative - Comes in: - Blue paper: sodium bicarbonate and potassium sodium tartrate - White paper: tartaric acid - Reaction → CO2 (effervescence) → Increases palatability - **Soda Mint** - Sodium bicarbonate + aromatic ammonia - Carminative, antacid - **Soda lime** - Calcium hydroxide + Na/K hydroxides - Absorbs CO2 - For metabolism tests, anesthesia, oxygen therapy - **Sodium bicarbonate and Calcium carbonate powder** - "Sippy Powder No. 1" - Antacid - **Sodium citrate solution** - Diaphoretic - increases sweating - **Compound sodium borate solution** - "Dobell's solution" - Astringent, antiseptic - **Theobromine and Sodium acetate** - Diuretic in cardiac edemas - **Sodium nitrate** - "Chile saltpeter" - Manufacture of nitric acid and fertilizer ### B1.3 Potassium - Latin name Kalium, obtained from Salsola kali - Isolated by Sir Humphry Davy from potash - various mined and manufactured potassium salts - Violet color in non-luminous flame - K+ - predominant cation in ICF - **Potassium acetate** - diuretic - **Potassium bicarbonate** - Antacid, urinary alkalizer - **Potassium bitartrate** - "Cream of Tartar" - Diuretic, laxative - **Potassium bromide** - sedative - **Potassium carbonate** - Alkalizer in pharmaceutical preparations - **Potassium chlorate** - Oxidizing germicide - Manufacture of pyrotechnics, matches - **Potassium chloride** - diuretic - **Potassium citrate** - Diuretic, expectorant, laxative - **Potassium hydroxide** - "Caustic potash" - Similar to NaOH but more deliquescent, stronger and more expensive than NaOH - **Potassium mercuric iodide** - Germicide - **Potassium nitrate** - "Saltpeter" - Diuretic, diaphoretic - **Potassium permanganate** - "Chameleon mineral" - Very powerful oxidizing agent - Antiseptic, treatment of urethritis - **Potassium sodium tartrate** - "Rochelle salt, Sal Seignette" - Mild laxative and hydragogue - Component of Fehling's solution - **Sulfurated Potash** - "Liver of sulfur, hepar sulfuris" - Mixture of K polysulfides and thiosulfate - Treatment of parasitic skin diseases - **Potassium thiocyanate** - Smooth muscle relaxant ### B1.4 Rubidium - Discovered by Bunsen and Kirchhoff - seldom used in medicine ### B1.5 Cesium - Discovered by Bunsen; first element discovered using spectroscope - No commercial importance; never used in medicine ### B1.6 Ammonium - NH4+ cation behaves like an alkali metal - "hypothetical metal ion" - **Ammonium bromide** - sedative - **Ammonium carbonate** - "Sal volatile, Preston salt, Hartshorn, Salt of Hartshorn" - Reflex stimulant - Expectorant - **Ammonium hydroxide** - Strong ammonia solution - Stronger ammonia water - 27-29% NH3 - Used in manufacture of ammonium salts, nitric acid, fertilizers - Diluted ammonia solution - Ammonia water - 9-10% NH3 - "Spirit of hartshorn" - Product of destructive distillation of horns of male deer - "Household ammonia" - For cleaning and washing due to water softening and saponifying properties - **Aromatic Ammonia Spirit** - Gastric stimulant, carminative, antacid - **Ammonium acetate solution** - "Spirit of Mindererus" - **Expectorant Mixture** - "Mistura pectoralis, Stoke's Expectorant" - **Ammonium Chloride** - "Muriate of Ammonia, Sal ammoniac" - Expectorant, diuretic ## B2. Group IIA - The Alkaline Earth Metals - Be, Mg, Ca, Sr, Ba - Bivalent, +2 - **Reactions:** - M + H2O → H2 + M(OH)2 - M + H2 → MH2 - M(OH)2 + heat → MO + H2O - **Solubility:** - Hydroxide salts are less water-soluble than those of alkalis - Carbonates, sulfate, phosphates and fluoride salts are INSOLUBLE in water ### B2.1 Calcium - Discovered by Sir Humphry Davy (through electrolysis) - Found in nature in the form of carbonate (chalk, marble, limestone) - Brick red in non-luminous flame - Ca+2 ion - 2nd most abundant cation in the ECF - Pharmacologic action: - Nerve transmission - Proper cardiac function - Blood coagulation - Structural basis of skeleton - **Calcium bromide** - sedative - **Calcium carbonate** - Most abundant and widely distributed calcium salt - Forms: - Amorphous - Chalk - Crystalline - Limestone, marble - Used as building material - Precipitated calcium carbonate - Precipitated chalk - External: as dentifrice (tooth powder) due to mild abrasive property - Internal: antacid - Prepared Chalk - Drop chalk - Antacid - **Calcium chloride** - Urinary acidifier - **Ringer's Solution** - Isotonic solution of Three Chlorides - Ca, Na and K chlorides - **Lactated Ringer's Solution** - Ca, Na and K chlorides + sodium lactate - **Calcium gluconate** - Calcium supplement - **Calcium hydroxide:** "hydrated lime or slaked lime" - Mixed with 3-4x of water → "Milk of Lime" - Saturated aqueous solution → "Lime Water" - Uses: - Antacid - Mild astringent - Saponifying agent for oils - **Calcium oxide** - "Lime, Calx, Quicklime" - Slaking: CaO + H2O → Ca(OH)2 - Used in making insecticides - **Sulfurated Lime Solution:** "Vleminckx' Solution" - Lime + sublimed sulfur - Treatment of acne - **Dibasic calcium phosphate** - "Lime Water" - Source of calcium and phosphorus - Can be supplied with - Vitamin D → increases Ca absorption - **Tribasic calcium phosphate** - Precipitated calcium phosphate - "Bone ash" - Antacid - **Bleaching Powder** - Chlorinated Lime, Chloride of Lime - CaOCI(CI) H2O - Disinfectant, bleaching agent - **Calcium sulfate** - As dihydrate → Gypsum - filler for wall paper - As hemihydrate → Plaster of Paris - used in surgery for making casts - **Calcium sulfide** - Sulfurated lime, calcic liver of sulfur, hepar calcis - Treatment of acne ### B2.2 Strontium - Isolated by Sir Humphry Davy (through electrolysis) - Found in nature in the form of sulfate (barite, heavy spar) - Crimson red in non-luminous flame - Similar with Ca+2 ion but has weaker effect and less toxic - **Strontium bromide** - sedative - **Strontium hydroxide** - Used in sugar industry - **Strontium nitrate** - Used in pyrotechnics ### B2.3 Barium - Yellowish green in non-luminous flame - Ba+2 is highly toxic - **Barium chloride** - Used in the treatment of Stokes-Adams disease "heart-block" - Veterinary use: constipation in horses - Rat poison - **Barium sulfate** - Radiopaque contrast media - Oral: Barium meal - Rectal: Barium enema - Commercial use: making lithopone paints - **Barium hydroxide** - "Caustic baryta" - Aqueous solution → baryta water - Use: CO2-absorbent - **Barium nitrate** - Used in manufacture of green fire - **Barium oxide** - "Calcined baryta" - Used in manufacture of hydrogen peroxide - **Barium sulfide** - Depilatory - removes hair from skin ### B2.4 Beryllium - Named after mineral beryl - Aka "glucinum" - sweet taste - Be+2 - toxic - Never employed in medicine; used in wires for pianos and scientific instruments ### B2.5 Magnesium - First isolated by Sir Humphry Davy, named after town called Magnesia - Found in the forms of - Talc - native hydrated magnesium silicate - Dolomite - CaCO3 MgCO3 - Kieserite - native magnesium sulfate - Burns with a blinding white light - used in photography and pyrotechnics - Mg-salts are laxative. - Mg+2 - 2nd most abundant cation in the ICF - **Magnesium carbonate** - "Magnesia alba" - Antacid, laxative - Clarifying or filtering agent in syrups - Abrasive in tooth powders - **Magnesium citrate** - Laxative, cathartic - **Magnesium hydroxide** - Antacid with mild laxative effect - Magnesia magma - "Milk of Magnesia" - A suspension prepared by hydration of MgO - **Magnesium oxide:** "Magnesia" - Antacid, laxative - Light - made by heating MgCO3 to dull redness - Heavy - MgSO4 + Na2CO3 → heat - **Tribasic magnesium phosphate** - Antacid - **Magnesium sulfate** - As heptahydrate → Epsom salt - Saline cathartic - **Magnesium trisilicate** - Antacid with adsorbent and protective property - Emulsifying agent - **Asbestos** - Fibrous minerals and poor heat conductors - **Talc** - native hydrated magnesium silicate - filtering agent ## B3. Group IB - The Coinage Metals - Cu, Ag, Au - employed for ornamental and coinage purposes - "Noble metals" - Occur free in nature - Chemically inert - Slowly oxidized in air - Malleable and ductile - Best Metals for electrical conductivity - 1st Ag→ 2nd Cu → 3rd Au - Best Metals for heat conductivity - 1st Ag→ 2nd Au → 3rd Cu - Possess oligodynamic effect - toxic effect of metals on microbes ### B3.1 Copper - Latin name Cuprum, from "Cyprus" where many ores are mined - red metal - Cu+2 salts - blue to emerald green in non-luminous flame - **Cu ions** - protein precipitant, fungicide - astringent, emetic - acts as catalyst for the storage and release of iron - **Menke's Disease** - Cu Deficiency - **Wilson's Disease** - Cu Toxicity - Hepatolenticular degeneration - Antidote: - British Anti-Lewisite (BAL) or Dimercaprol - Penicillamine - **Copper alloys** - Brass - Cu + Zn - Bronze - Cu + Sn - German silver - Cu + Zn + Ni - Sterling - Cu + Ag - **Cupric citrate** - Astringent, antiseptic - **Cupric sulfate** - "Blue vitriol or blue stone" - Component of Fehling's solutions and Benedict's solution → solutions used to detect reducing sugars - Emetic - Antidote for phosphorus poisoning - **Cupric acetate and acetic acid** - Components of Barfoed's reagent - test for reducing sugars - **Basic cupric acetate** - "Green verdigris" - **Cupric hydrogen arsenite** - "Scheele's mineral, Swedish Green" - **Cupric acetoarsenite** - "Paris Green, Parrot Green" - Insecticide - **CuSO4 5H2O and CaO** - "Bordeaux mixture" - algaecide and fungicide for swimming pool ### B3.2 Silver - Latin name Argentum, "shining" - white metal with metallic luster - Ag+ ion - Protein precipitant - Colloidal silver preparations - Antiseptic, astringent - Irritant, corrosive - **Argyria** - darkening of skin due to long period of use of silver preparations - **Silver nitrate** - Eye antiseptic for newborn babies - Silver nitrate pencil - Lunar caustic - Toughened silver nitrate - Ammoniacal silver nitrate solution - Howe's solution - **Mild silver protein (19-23% Ag)** - "Mild protargin" - Mild antiseptic - Brands: Silvol, Argyrol - **Strong protein silver (7.5-8.5% Ag)** - "Strong protargin" - Stronger antiseptic action than mild silver protein - Brand: Protargol - **Colloidal silver chloride** - Antiseptic - **Colloidal silver iodide** - Antiseptic - **Silver sulfadiazine** - prophylaxis, treatment of infections in burn wounds - **Silver bromide** - Antiseptic - Photography - **Silver oxide** - CO absorbent - **Silver picrate** - Picragol, Picrotol - Antiseptic ### B3.3 Gold - Latin name Aurum, "shining dawn, aurora" - "King of all metals" - Due to color, scarcity and permanency - Universal symbol of highest purity and value - Most malleable and ductile metal - Yellow color - Selenic acid: Only single acid that can dissolve gold - Aqua regia: Best reagent for dissolving gold - A mixture of nitric acid and hydrochloric acid (1:3) - Pure gold = 24-carat or 1000 fine - % Au = carat/24 x 100 % Au = fineness/1000 x 100 - Pure gold is too soft → often alloyed with Cu or Ag for hardness - Uses: - Gilding and plating - As dental crowns, bridges and inlays (gold leaf) ### Chrysotherapy - Treatment of diseases (especially RA) with gold compounds - Disease-modifying antirheumatic drugs (DMARDs) - **Sodium aurothiomalate** - Commonly used gold-based DMARD - **Auranofin** - Orally available gold drug for RA