PERIODIC TABLE OF THE ELEMENTS. Fm Fermium. Tb Terbium. elements which do not occur naturally. stable or best known isotopes for
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1 PERIODIC TABLE OF THE ELEMENTS Be Beryllium 90 5 B Boron 8 6 C Carbon 7 N Nitrogen 40 8 O Oxygen 60 9 F Fluorine 90 H He Hydrogen Helium 40 Ne Neon Atomic Number Symbol Name Atomic Mass 3 Li Lithium 69 4 i Si i i 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 Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Ni Cu Zn Ga Ge As Se Br Kr 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 Cs Ba La Hf Ta W Re Os Ir Cesium Barium Lanthanum Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury Thallium Lead Bismuth Polonium Astatine Radon (09) () () Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Francium Radium Actinium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium (3) (6) (7) (6) (6) (63) (6) (65) (66) Sg Bh Hs Mt 58 Ce Cerium Based on mass of C at Th Thorium Pr Praseodymium Pa Protactinium 3 60 Nd Neodymium 44 9 U Uranium Pm Promethium (45) 93 Np Neptunium (37) 6 Sm Samarium Pu Plutonium (44) 63 Eu Europium Am Americium (43) 64 Gd Gadolinium Cm Curium (47) 65 Tb Terbium Bk Berkelium (47) 66 Dy Dysprosium Cf Californium (5) 67 Ho Holmium Es Einsteinium (5) 68 Er Erbium Fm Fermium (57) 69 Tm Thulium 689 Md Mendelevium (58) 70 Yb Ytterbium 730 No Nobelium (59) 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 Chemistry Data Page
2 ATOMIC MASSES OF THE ELEMENTS Based on mass of C at 0 Values in parentheses are the mass number of the most stable or best known isotopes for elements that do not occur naturally Data Page Chemistry 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 (43) () 373 (47) (5) (47) (6) 65 (5) (57) 90 (3) (6) (58) 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) (59) (44) (09) (45) 3 (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 4+ Lead(IV), plumbic NH 4 + Ammonium Li + Lithium Ba + Barium Mg + Magnesium Ca + Calcium Mn + Manganese(II), manganous Cr + Chromium(II), chromous Mn 4+ 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 4+ 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 4 Monohydrogen phosphate ClO Chlorite NO 3 Nitrate CrO 4 Chromate NO Nitrite CN Cyanide C O 4 Oxalate Cr O 7 Dichromate O Oxide** H PO 4 Dihydrogen phosphate ClO 4 Perchlorate CH 3 COO Ethanoate, acetate MnO 4 Permanganate F Fluoride PO 4 3 Phosphate HCO 3 Hydrogen carbonate, bicarbonate SO 4 Sulphate HC O 4 Hydrogen oxalate, binoxalate S Sulphide HSO 4 Hydrogen sulphate, bisulphate SO 3 Sulphite HS Hydrogen sulphide, bisulphide SCN Thiocyanate HSO 3 Hydrogen sulphite, bisulphite Chemistry Data Page 3
4 SOLUBILITY OF COMMON COMPOUNDS IN WATER The term soluble here means > 0 mol/l at 5 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 4 + Nitrate, NO 3 All or or Chloride, Cl Bromide, Br Iodide, I Ag +, Pb +, Cu + Sulphate, SO 4 Ag +, Ca +, Sr +, Ba +, Pb + Sulphide, S Alkali ions, H +, NH 4 +, Be +, Mg +, Ca +, Sr +, Ba + Hydroxide, OH Alkali ions, H +, NH + 4, Sr + or or Phosphate, PO 4 3 Carbonate, CO 3 Sulphite, SO 3 Alkali ions, H +, NH 4 + Data Page 4 Chemistry
5 SOLUBILITY PRODUCT CONSTANTS AT 5 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 4 BaSO 4 CaCO 3 CaC O 4 CaSO 4 CuI Cu(IO 3 ) CuS Fe(OH) FeS Fe(OH) 3 PbBr PbCl Pb(IO 3 ) PbI PbSO 4 MgCO 3 Mg(OH) AgBrO 3 AgBr Ag CO 3 AgCl Ag CrO 4 AgIO 3 AgI SrCO 3 SrF SrSO 4 ZnS K sp Chemistry Data Page 5
6 RELATIVE STRENGTHS OF BRØNSTEDLOWRY ACIDS AND BASES in aqueous solution at room temperature Name of Acid Acid Base K a STRONG STRENGTH OF ACID WEAK 4 4 Perchloric HClO Æ H + ClO Hydriodic HI Æ H + I Hydrobromic HBr Æ H + Br Hydrochloric HCl Æ H + Cl 3 3 Nitric HNO Æ H + NO Sulphuric HSO4 Æ H + HSO4 + + Hydronium Ion H3O Æ H + HO Iodic HIO3 Æ H + IO3 7 Oxalic H C O Æ H + HC O Sulphurous ( SO + HO) HSO3 Æ H + HSO3 Hydrogen sulphate ion HSO4 Æ H + SO4 5 Phosphoric H PO Æ H + H PO Hexaaquoiron ion iron III ion Fe( HO) 6 Æ H + Fe( HO) ( OH) +, ( ) 5 Citric H3C6H5O7 Æ H + HC6H5O7 Nitrous HNO Æ H + NO Hydrofluoric HF Æ H + + F 35 4 Methanoic, formic HCOOH Æ H + HCOO Hexaaquochromium ion, chromium( III) ion Cr( HO) Æ H + Cr( H O) ( OH) 6 5 Benzoic C6H5COOH Æ H + C6H5COO Hydrogen oxalate ion HCO4 Æ H + CO4 Ethanoic, acetic CH COOH 3 H CH3COO Dihydrogen citrate ion H C H O Æ H + HC H O 7 Hexaaquoaluminum ion, aluminum ion Al( H O) Æ H + Al( H O) ( OH) 4 Carbonic ( CO + HO) HCO3 Æ H + HCO3 43 Monohydrogen citrate ion + HC6H5O7 Æ H + CHO Hydrogen sulphite ion HSO3 Æ H + SO3 Hydrogen sulphide HS Æ H + HS 9 + Dihydrogen phosphate ion HPO4 Æ H + HPO4 6 Boric H3BO3 Æ H + HBO Ammonium ion NH4 Æ H + NH3 56 Hydrocyanic HCN Æ H + CN 49 Phenol C6H5OH Æ H + C6H5O 3 + Hydrogen carbonate ion HCO3 Æ H + CO3 56 Hydrogen peroxide HO Æ H + HO 4 Monohydrogen phosphate ion HPO4 Æ H + PO4 Water H O Æ H + OH Hydroxide ion OH H + O very small 3 Ammonia NH H + NH very small 4 WEAK STRENGTH OF BASE STRONG Data Page 6 Chemistry
7 ACIDBASE 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 Chemistry Data Page 7
8 STANDARD REDUCTION POTENTIALS OF HALFCELLS Ionic concentrations are at M in water at 5 C Oxidizing Agents Reducing Agents F ( g)+ e Æ F + 87 SO 8 + e Æ SO4 + 0 HO + H + e Æ HO MnO4 + 8H + 5e Æ Mn + 4HO Au + 3e Æ Au() s + 50 BrO3 + 6H + 5e Æ Br()+ l 3HO + 48 ClO4 + 8H + 8e Æ Cl + 4HO + 39 Cl( g)+ e Æ Cl CrO 7 + 4H + 6e Æ Cr + 7HO + 3 O( g)+ H + e Æ HO MnO()+ s 4H + e Æ Mn + HO + IO3 + 6H + 5e Æ I()+ s 3HO + Overpotential Br ()+ l e Æ Br + 9 Effect AuCl4 + 3e Æ Au()+ s 4Cl + 0 NO3 + 4H + 3e Æ NO( g)+ HO +096 Hg + e Æ Hg() l O ( g 7 )+ H ( M)+ e Æ HO + 08 NO3 + 4H + e Æ NO4 + HO Ag + e Æ Ag() s Hg + e Æ Hg() l Fe + e Æ + Fe O( g)+ H + e Æ HO MnO4 + HO + 3e Æ MnO()+ s 4OH I()+ s e Æ I Cu + e Æ Cu() s + 05 HSO 3 + 4H + 4e Æ Ss ()+ 3HO Cu + e Æ Cu() s SO4 + 4H + e Æ HSO3 + HO + 07 Cu + e Æ + Cu Sn + e Æ + Sn + 05 Ss ()+ H + e Æ HSg ( ) + 04 H + e Æ H( g) Pb + e Æ Pb() s 03 Sn + e Æ Sn() s 04 Ni + e Æ Ni() s 06 HPO H + e Æ HPO HO 08 Co + e Æ Co() s 08 Se()+ s H + e Æ HSe Cr + e Æ + Cr 04 7 HO + e Æ H + OH ( M) 04 Fe + e Æ Fe() s 045 Overpotential AgS()+ s e Æ Ag()+ s S 069 Effect 3 Cr + 3e Æ Cr() s 074 Zn + e Æ Zn() s 076 Te()+ s H + e Æ HTe 079 HO + e Æ H( g)+ OH 083 Mn + e Æ Mn() s 9 3 Al + 3e Æ Al() s 66 Mg + e Æ Mg() s 37 Na + e Æ Na() s 7 Ca + e Æ Ca() s 87 Sr + e Æ Sr() s 89 Ba + e Æ Ba() s 9 K + e Æ K() s 93 Rb + e Æ Rb() s 98 Cs + e Æ Cs() s 303 Li + e Æ Li() s 304 Data Page 8 Chemistry STRONG STRENGTH OF OXIDIZING AGENT WEAK E ( Volts ) WEAK STRENGTH OF REDUCING AGENT STRONG
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