Properties and Uses of Alkali and Coinage Metals

Alkali Metals

Ha, Li, Na, K, Rb, Cs, Fr (HaLiNaKaRubyCesaFrancs)

Common Properties of Alkali Metals

one valence electron, most reactive, does not occur in its natural state (but in compound)

Chemical Properties of Alkali Metals

high affinity for oxides, readily form white solid hydrides when exposed to hydrogen gas, stored under kerosene to prevent the reaction with h20 and oxygen, only lithium readily reacts with nitrogen

Compounds of Alkali Metals

alkali formed are more basic than 2A and 3A, alkali salts are soluble in water, alkali metals in liquid ammonia form blue solutions, Li and Na = hydration and crystallization, do not form complexes

Hydrogen

lightest element, found as compound, hydrogenium

Lithium

lithos, earth stone, diuretic and depressant properties, used to treat bipolar disorders, readily reacts with nitrogen

Sodium

Most abundant EC cation, fluid retention, osmotic effects, Natrium, hypokalemia: lead to weakness

Potassium

Predominant IC cation, diuretic effects and muscle contraction, High level in potassium will lead into cardiac arrest, kalium

Cesium

catalyst in the polymerization of resin-forming materials, caesius

Francium

in medical equipments, stopped using due to discoloration

Coinage Metals

Cu, Ag, Au

Properties of Coinage Metals

polyvalent except silver, covalent bond (much harder to break) especially with halides, one valence electron on the outside of the shell and followed by 18 electrons in the next shell, less reactive than 1a, complex ions, halides are insoluble, occur in free metallic state

Copper

Cuprum, only metal used in water purification, 3rd most malleable, 3rd most best conductor, Salts are blue in color, occur in respiratory pigments such as hemocyanin (blood), cytochrome oxidase (drug metabolism), biotransformation of drugs (drug inactivation), protein precipitant (astringent), utilization of Fe, Toxicity: Wilson's disease (mental retardation), Treatment: Penicillamine

Silver

Argentum, 2nd most malleable, oligodynamic action (antimicrobial effect- inhibits microorganisms), wound dressing and catheters to prevent infections, Toxicity: Argyria (blue discoloration in the skin), Treatment: NSS, sodium thiosulfate

Gold

Aurum, King of all metals, the most malleable and conductive metal, soluble only in aqua regia (1 part HNO3, 3 part HCl), prized for chemical stability

Alkali Earth Metals

Be, Mg, Ca, Sr, Ba, Ra (BeMegCaSirBaRa)

Properties of Alkali Earth Metals

Bivalent, Less reactive than 1A but can still form ionic salts and oxides, Salts are insoluble except for hydroxides

Beryllium

most toxic metal, fluorescent lighting industry

Magnesium

lightest of all structurally important metals, 2nd most abundant IC cation, in chlorophyll, laxative and depressant properties, muscle relaxants, natural source: silicates in the form of talc, Calcium channel blockers

Calcium

calx, 2nd most abundant EC cation, muscle contraction, Vitamin D (important for the accumulation of calcium), Deficiency: Osteomalacia (weakened bones), natural source: gypsum, dolomite, fluorite

Strontium

strontian, Used in red pyrotechnics (fireworks)

Barium

baryum, Heavy, Most active of Group 2A

Radium

Radius, Radioactive, Mario Curie (death: exposure to radiation), In chemotherapy

Third Transition Metals

Zn, Cd, Hg (ZenCadHug)

Properties of Third Transition Metals

Both ionic and covalent, Divalent (Hg is both monovalent and divalent), Halides are soluble, Form complex ions, Oxides are stable

Zinc

Cadmia; metal present in insulin, container for dry cells, astringent, antiseptic, antiperspirant, protectant, Deficiency: Parakeratosis

Cadmium

Wood's metal, Rose's metal, used in some alloy, soluble salts are astringent, Toxicity: Itai-Itai, Treatment: BAL (British Anti-Lewisite)

Mercury

Hydrargyrum, Quicksilver, Liquid silver, Toxicity: Minamata disease, Treatment: BAL, sodium thiosulfate, penicillamine, A true metal, Used previously as cathartic and parasiticide, but now used as a germicidal, Mercury and its compounds are toxic, Natural source: Cinnabar (HgS)

Boron

Antiseptic, In +3 oxidation state and non-metal (very toxic)

Aluminum

Gastric antacid, Source: cryolite, most abundant metal, 3rd most abundant element

Rare Earth Metals

Lanthanides and Actinides have no pharmaceutical applications, Trivalent (Lanthinides have +3, +4 valence, Only cerium in the lanthanides is used as analytical reagent in pharmacy, Hydroxides formed are very weak