PERIODIC TABLE OF THE ELEMENTS. No Nobelium. Tb Terbium. Am Americium. Ce Cerium. elements which do not occur naturally.
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1 PERIODIC TABLE OF THE ELEMENTS Be Beryllium 90 B Boron 08 6 C Carbon 0 7 N Nitrogen 0 8 O Oxygen 60 9 F Fluorine 90 H He Hydrogen Helium Ne Neon Atomic Number Symbol Name Atomic Mass 3 Li Lithium 69 Si Silicon 8 0 Na Mg Sodium Magnesium Aluminum Silicon Phosphorus Sulphur Chlorine Argon Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Ni Cu Zn Ga Ge As Se Br Kr Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Nickel Rb Y Zr Nb Mo Tc Ru Rh Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon (98) Sr Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba Cesium Barium Lanthanum Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury Thallium Lead Bismuth Polonium Astatine Radon (09) (0) () Fr Ra La Hf Ac Rf Ta Francium Radium Actinium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium (3) (6) (7) (6) (6) (63) (6) (6) (66) 7 W Db Sg Re Os Bh Hs Ir Mt Pt Au Hg Tl Pb Bi Po At Rn 8 Ce Cerium Based on mass of C at Th Thorium 30 9 Pr Praseodymium 09 9 Pa Protactinium Nd Neodymium 9 U Uranium Pm Promethium () 93 Np Neptunium (37) 6 Sm Samarium 0 9 Pu Plutonium () 63 Eu Europium 0 9 Am Americium (3) 6 Gd Gadolinium Cm Curium (7) 6 Tb Terbium Bk Berkelium (7) 66 Dy Dysprosium 6 98 Cf Californium () 67 Ho Holmium Es Einsteinium () 68 Er Erbium Fm Fermium (7) 69 Tm Thulium Md Mendelevium (8) 70 Yb Ytterbium No Nobelium (9) 7 Lu Lutetium Lr Lawrencium (6) Values in parentheses are the masses of the most stable or best known isotopes for elements which do not occur naturally
2 ATOMIC MASSES OF THE ELEMENTS Based on mass of C at 00 Values in parentheses are the mass number of the most stable or best known isotopes for elements that do not occur naturally Actinium Aluminum Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Boron Bromine Cadmium Calcium Californium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Curium Dubnium Dysprosium Einsteinium Erbium Europium Fermium Fluorine Francium Gadolinium Gallium Germanium Gold Hafnium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanum Lawrencium Lead Lithium Lutetium Magnesium Manganese Mendelevium Ac Al Am Sb Ar As At Ba Bk Be Bi B Br Cd Ca Cf C Ce Cs Cl Cr Co Cu Cm Db Dy Es Er Eu Fm F Fr Gd Ga Ge Au Hf He Ho H In I Ir Fe Kr La Lr Pb Li Lu Mg Mn Md (7) 70 (3) (0) 373 (7) () (7) (6) 6 () (7) 90 (3) (6) (8) Mercury Molybdenum Neodymium Neon Neptunium Nickel Niobium Nitrogen Nobelium Osmium Oxygen Palladium Phosphorus Platinum Plutonium Polonium Potassium Praseodymium Promethium Protactinium Radium Radon Rhenium Rhodium Rubidium Ruthenium Rutherfordium Samarium Scandium Selenium Silicon Silver Sodium Strontium Sulphur Tantalum Technetium Tellurium Terbium Thallium Thorium Thulium Tin Titanium Tungsten Uranium Vanadium Xenon Ytterbium Yttrium Zinc Zirconium Hg Mo Nd Ne Np Ni Nb N No Os O Pd P Pt Pu Po K Pr Pm Pa Ra Rn Re Rh Rb Ru Rf Sm Sc Se Si Ag Na Sr S Ta Tc Te Tb Tl Th Tm Sn Ti W U V Xe Yb Y Zn Zr (37) (9) () (09) () 30 (6) () (6) (98) Element Symbol Atomic Number Atomic Mass Element Symbol Atomic Number Atomic Mass
3 NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air ** Not stable in aqueous solutions Positive Ions (Cations) Al 3+ Aluminum Pb + Lead(IV), plumbic NH + Ammonium Li + Lithium Ba + Barium Mg + Magnesium Ca + Calcium Mn + Manganese(II), manganous Cr + Chromium(II), chromous Mn + Manganese(IV) Cr 3+ Chromium(III), chromic Hg + Mercury(I)*, mercurous Cu + Copper(I)*, cuprous Hg + Mercury(II), mercuric Cu + Copper(II), cupric K + Potassium H + Hydrogen Ag + Silver H 3 O + Hydronium Na + Sodium Fe + Iron(II)*, ferrous Sn + Tin(II)*, stannous Fe 3+ Iron(III), ferric Sn + Tin(IV), stannic Pb + Lead(II), plumbous Zn + Zinc Negative Ions (Anions) Br Bromide OH Hydroxide CO 3 Carbonate ClO Hypochlorite ClO 3 Chlorate I Iodide Cl Chloride HPO Monohydrogen phosphate ClO Chlorite NO 3 Nitrate CrO Chromate NO Nitrite CN Cyanide C O Oxalate Cr O 7 Dichromate O Oxide** H PO Dihydrogen phosphate ClO Perchlorate CH 3 COO Ethanoate, acetate MnO Permanganate F Fluoride PO 3 Phosphate HCO 3 Hydrogen carbonate, bicarbonate SO Sulphate HC O Hydrogen oxalate, binoxalate S Sulphide HSO Hydrogen sulphate, bisulphate SO 3 Sulphite HS Hydrogen sulphide, bisulphide SCN Thiocyanate HSO 3 Hydrogen sulphite, bisulphite 3
4 SOLUBILITY OF COMMON COMPOUNDS IN WATER The term soluble here means > 0 mol/l at C Negative Ions (Anions) Positive Ions (Cations) Solubility of Compounds All Alkali ions: Li +,Na +,K +,Rb +,Cs +,Fr + All Hydrogen ion: H + All Ammonium ion: NH + Nitrate, NO 3 All or or Chloride,Cl Bromide, Br Iodide, I Ag +,Pb +,Cu + Sulphate, SO Ag +,Ca +,Sr +,Ba +,Pb + Sulphide, S Alkali ions, H +,NH +,Be +,Mg +,Ca +,Sr +,Ba + Hydroxide, OH Alkali ions, H +,NH +,Sr + or or Phosphate, PO 3 Carbonate, CO 3 Sulphite, SO 3 Alkali ions, H +,NH +
5 SOLUBILITY PRODUCT CONSTANTS AT C Name Barium carbonate Barium chromate Barium sulphate Calcium carbonate Calcium oxalate Calcium sulphate Copper(I) iodide Copper(II) iodate Copper(II) sulphide Iron(II) hydroxide Iron(II) sulphide Iron(III) hydroxide Lead(II) bromide Lead(II) chloride Lead(II) iodate Lead(II) iodide Lead(II) sulphate Magnesium carbonate Magnesium hydroxide Silver bromate Silver bromide Silver carbonate Silver chloride Silver chromate Silver iodate Silver iodide Strontium carbonate Strontium fluoride Strontium sulphate Zinc sulphide Formula BaCO 3 BaCrO BaSO CaCO 3 CaC O CaSO CuI Cu IO 3 CuS FeS ( ) AgBr AgCl AgI ZnS ( ) Fe( OH) Fe OH 3 PbBr PbCl ( ) Pb IO 3 PbI PbSO MgCO 3 ( ) Mg OH AgBrO 3 Ag CO 3 Ag CrO AgIO 3 SrCO 3 SrF SrSO K sp
6 RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASES in aqueous solution at room temperature Name of Acid Acid Base K a STRONG STRENGTH OF ACID WEAK + + Perchloric HClO H + ClO Hydriodic HI H + I + Hydrobromic HBr H + Br + Hydrochloric HCl H + Cl Nitric HNO H + NO Sulphuric HSO H + HSO + Hydronium Ion H O + 3 H + HO 0 Iodic HIO + 3 H + IO3 7 0 Oxalic H C O + H + HC O ( ) + + 3, ( III) 6 + Fe( HO) ( OH) ( ) + Sulphurous SO H O H SO H HSO Hydrogen sulphate ion HSO H SO Phosphoric H PO H H PO Hexaaquoiron ion iron ion Fe H O H Citric H C H O H H C H O Nitrous HNO H NO Hydrofluoric HF H + F 3 0 Methanoic, formic HCOOH H + HCOO ( ) ( ) ( ) Hexaaquochromium ion, chromium( III) ion Cr HO H Cr H 6 O OH 0 Benzoic C6HCOOH H + C6HCOO 6 0 Hydrogen oxalate ion HCO H + CO 6 0 Ethanoic, acetic CH3COOH H + CH3COO 8 0 Dihydrogen citrate ion H C H O H + HC H O ( ) + ( ) ( ) Hexaaquoaluminum ion, aluminum ion Al HO H Al H O OH Carbonic ( CO + HO ) HCO 3 H + HCO3 3 0 Monohydrogen citrate ion + 3 HC6HO 7 H + C6HO Hydrogen sulphite ion HSO3 H + SO Hydrogen sulphide HS + H + HS Dihydrogen phosphate ion HPO H + HPO Boric H3BO3 H + HBO Ammonium ion + + NH H + NH Hydrocyanic HCN + H + CN Phenol C 6HOH H + C6HO Hydrogen carbonate ion HCO3 H + CO Hydrogen peroxide HO H + HO 0 Monohydrogen phosphate ion + HPO H + PO Water H O + H + OH Hydroxide ion OH H + O very small + 3 Ammonia NH H + NH very small WEAK STRENGTH OF BASE STRONG 6
7 ACID-BASE INDICATORS Indicator Methyl violet Thymol blue Orange IV Methyl orange Bromcresol green Methyl red Chlorophenol red Bromthymol blue Phenol red Neutral red Thymol blue Phenolphthalein Thymolphthalein Alizarin yellow Indigo carmine ph Range in Which Colour Change Occurs Colour Change as ph Increases yellow to blue red to yellow red to yellow red to yellow yellow to blue red to yellow yellow to red yellow to blue yellow to red red to amber yellow to blue colourless to pink colourless to blue yellow to red blue to yellow 7
8 STANDARD REDUCTION POTENTIALS OF HALF-CELLS Ionic concentrations are at M in water at C Oxidizing Agents Reducing Agents E ( Volts ) STRONG STRENGTH OF OXIDIZING AGENT WEAK Overpotential Effect F( g) + e F + 87 SO + e SO HO + H + e HO + 78 MnO + 8H + e Mn + H O + Au + 3e Au( s) + BrO3 + 6H + e Br ( l) + 3HO ClO + + 8H + 8e Cl + H O + 39 Cl( g) e Cl O ( g) H e HO + + MnO( s) + 3 ( s) Br( l) e Br AuCl e Au( s) Cl + 3 ( g) + Hg e Hg( l) + 7 O ( g) H M e HO Ag e Ag( s) + Hg e Hg( l) O ( ) H e g HO ( s) I( s) e I + Cu e Cu( s) ( s) + 3 O + Cu e Cu( s) SO + H + e H SO + H O Cu + e Cu Sn + e Sn S( ) + H + e s HS( g) + H + e H( g) + Pb + e Pb( s) + Sn + e Sn( s) Ni + e Ni( s) 0 6 HPO + + H + e HPO + HO Co e Co( s) + Se( s) H e HSe Cr + e Cr 0 7 H + Fe e Fe( s) AgS( s) e Ag() s S 3+ Cr e Cr( s) + Zn e Zn( s) ( s) Te HO e H( g) OH + Mn e Mn( s) 3+ Al e Al( s) + Mg e Mg( s) + Na e Na( s) + Ca e Ca( s) + Sr + e Sr( s) + Ba e Ba( s) + K e K( s) + Rb e Rb( s) + Cs e Cs( s) + Li e Li( s) O + e H + OH ( 0 M) Te H e H Cr O + H + 6e Cr + 7H O H + e Mn + H O + IO + 6H + e I + 3H O NO + H + 3e NO + H O ( 0 ) NO + H + e N O + H O Fe e Fe MnO + H O + 3e MnO + OH HSO H e S H Overpotential Effect WEAK STRENGTH OF REDUCING AGENT STRONG
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