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• The rate at which an object loses heat depends on its surface area and emissivity (the ability to emit radiation).
• Sections of PHCH 203 (Pharmaceutical Inorganic Chemistry)


  • 01- Hydrogen and its compounds (2 hours)
  • 02- Group properties of elements (4 hours)
  • 03- Pharmaceutical applications of the group I to VIII elements (1 hour)
  • 04- Transition elements and their pharmaceutical applications (4 hours)
• Chemistry plays a major role in the world. It can be classified under various headings such as organic chemistry, inorganic chemistry, biochemistry, nuclear chemistry and so on.
• Inorganic chemistry


  Deals with the study of synthesis and behavioural aspects of various analogues of inorganic elements of the periodic table. It also deals with the organometallic compounds.
• Inorganic compound


  A substance that contains two or more elements other than carbon combined in appropriate proportions.
• Subdivisions of inorganic chemistry

  • Descriptive inorganic chemistry
  • Theoretical inorganic chemistry
  • Thermodynamics and inorganic chemistry
  • Mechanistic inorganic chemistry
• Hydrogen

  Although hydrogen is placed at the top of Group 1A in most versions of the periodic table, it is very different from the other members of the alkali metal group.
• Hydrogen is the first element on the periodic table. It is the smallest element with one proton and one electron. It is highly abundant and has unique and important chemical properties.
• Isotopes of hydrogen

  Hydrogen-1 (protium), Hydrogen-2 (deuterium), Hydrogen-3 (tritium)
• Hydrogen compounds


  Hydrogen typically does not form cations, but instead forms compounds through covalent bonding.
• Potable water


  Natural water rendered safe and suitable for human use based on standards and tests for purity stated in the official compendia.
• Purified water


  Prepared from portable water by complete removal of soluble salts either by distillation or demineralization (deionization) using ion exchange resins.
• Water for injection


  Water intended for use in the preparations of medicines for parenteral administration when water is used as a vehicle and for dissolving or diluting substances or preparations for injectables.
• Sterile water for injection


  Water for injection that has been suitably packaged for dissolving or diluting substances or preparations for injectable preparations.
• Uses of hydrogen peroxide

  • Bleaching agent
  • Antiseptic and antibacterial agent
  • Antidote to cyanide and phosphorus poisoning
• Applications of hydrides

  • Reducing agents
  • Strong bases in organic syntheses
  • Desiccants or drying agents
  • Catalysts and catalytic intermediates
• Types of hydrides

  • Ionic hydrides
  • Covalent hydrides
  • Interstitial hydrides
• Hydride


  Hydrogen atom bound to an extremely electropositive metal, generally an alkali metal or an alkaline earth metal
• Hydride complexes

  • Catalysts and catalytic intermediates in a variety of homogeneous and heterogeneous catalytic cycles
  • Important example is hydrogenation catalyst
  • Certain enzymes, like hydrogenase, operate via hydride intermediates
  • The energy carrier NADH reacts as a hydride donor or hydride equivalent
• Types of hydrides

  • Ionic hydrides
  • Covalent hydrides
  • Interstitial or metallic hydrides
• Interstitial or metallic hydrides

  • Most commonly exist within metals or alloys, with generally metallic bonding
  • Bulk transition metals form interstitial binary hydrides when exposed to hydrogen, usually non-stoichiometric, with variable amounts of hydrogen atoms in the lattice
• Alkali metal hydrides are used as strong reducing agents in organic synthesis
• The objective of classification of elements is to study the maximum number of elements with least effort
• Elements are grouped into families with similar properties so that it becomes easy to compare one with the other
• First classification of elements

  • Metals
  • Non-metals
• Mendeleev's periodic law


  The properties of elements are a periodic function of their atomic weight
• Mendeleev periodic table

  • 9 groups numbered from 0 to 8
  • Group 8 is the transition elements
  • Group 0 is the noble gases
  • 7 horizontal rows known as periods
• Modern periodic table


  • Designed by Moseley, who arranged the elements based on their atomic numbers
  • Drawback of Mendeleev's periodic table (the presence of anomalous pairs and the position of isotopes of elements) disappeared
• Important features of the modern periodic table

  • 16 vertical columns known as groups, numbered as IA, IB, IIA, IIB...VIIA, VIIB, VIII, 0
  • Horizontal rows are called periods and are seven in number
  • The first period is the shortest and consists of two elements
  • The second and third period each have eight elements
  • The fourth and fifth periods are long periods of 18 elements each
  • The sixth period is the longest, having 32 elements
  • The seventh period is incomplete having 17 elements
  • The Lanthanides and Actinides were grouped separately at the bottom of the table
• Advantages of the modern periodic table over Mendeleev's table

  • The classification shows the similarities, differences and chemical properties of the elements clearly
  • The position of the element in the periodic table is properly related to its electronic configuration in its atoms
  • The elements present in a group are closely related to each other
• Alkali metals (Group IA)


  • The name 'alkali metal' comes from the fact that when these metals or their oxides are dissolved in water, a basic (alkaline) solution results
  • Members are lithium, sodium, potassium, rubidium, caesium and francium
  • Have ns1 electron in the outermost orbital
  • Hydrogen is included in this family because of its univalency character and, in certain of its chemical properties, it acts as though it were a member of the family
• General properties of alkali metals

  • Electropositive, monovalent, soft, malleable metals of low melting point and low density; the most active of all metallic elements
  • The valence electrons are capable of easy removal with the relative difficulty of removal decreasing as the radius increases
  • Ionization potential decreases with increase in atomic weight, hence reactivity and electropositive character increases down the series
  • The melting and boiling point of the elements decrease down the group
  • Have high affinity for oxygen; Li forms a normal oxide,Li2O and sodium forms a peroxide,Na2O2
  • React vigorously with water to form hydrogen gas and the metallic hydroxide
  • Form crystalline ionic monohalides except LiI which is covalent
  • Virtually all salts of alkali metals are ionic, stable and water soluble
• Pharmaceutically important compounds of group IA metals

  • Hydrogen (not used therapeutically, but used in preparation of many compounds)
  • Lithium carbonate, lithium citrate, lithium hydroxide
  • Sodium and potassium compounds (sodium salts are usually cheaper, but potassium salts are favored for certain properties)
• Sodium


  The major cation of the extracellular fluids, used in maintaining acid-base balance, muscle contraction, and neurotransmitter release
• Potassium


  The major intracellular cation, necessary for maintaining electrophysiology of the cell, protein and nucleic acid synthesis, and glucose to glycogen conversion
• Electrolytes


  Compounds that dissociate completely into ions in solution, with the capability of conducting electricity
• Importance of electrolytes in the body

  • Maintain voltage across muscles and nerves
  • Maintain homeostasis
  • Carry out electrical impulses like nerve impulses and muscular contractions
  • Maintain acid-base balance
  • Regulated by hormones and excreted by kidneys
• Major electrolytes in the body

  • Na, K, Cl-, Mg, Ca, HCO3-, Cu, Fe, Phosphorus
• Oral rehydration salt BP


  Compound containing NaCl, KCl, NaHCO3 and glucose, administered orally to prevent or treat dehydration due to acute diarrhoeal diseases
• Other potassium compounds

  • Potassium carbonate (potash, used in glass manufacturing)
  • Potassium hydroxide (caustic potash, used in soaps and detergents)
  • Potassium nitrate (saltpeter, used in topical formulations for sensitive teeth and asthma treatment)
  • Potassium chlorate (powerful oxidizer, used in match heads and fireworks)
  • Potassium superoxide (reacts with CO2 to produce K2CO3 and O2, used in respiration equipment)