Chemistry Reference Tables

Μέγεθος: px

Εμφάνιση ξεκινά από τη σελίδα:

Download "Chemistry Reference Tables"

Ευρώπη Αθανασίου
6 χρόνια πριν
Προβολές:

1 Chemistry Reference Tables Name Value Avogadro s number particles/mole L atm mole K Gas constant (R) 6. L mmhg mole K 8.1 L kpa mole K Standard pressure 1.00 atm = 101. kpa = 760. mmhg = 760. torr Standard temperature 0C or 7K Volume of 1 mole of any gas at STP. L Thermodynamic Constants Symbol Value (.18 J = 1 cal) Heat of fusion of water Heat of vaporization of water Specific heat of water H f (water) H v (water) C p (water) J/g,60 J/g.05 J for ice,.0 J for steam, g C g C.18 J for liquid g C Metal Specific Heat J g C Density (g/cm ) Melting Point ( C) Aluminum Copper Gold Iron Lead Magnesium Mercury Nickel Titanium Zinc NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 1

2 Organic Substances Name Density Melting Point ( C) Boiling Point ( C) Ethanol (CH CH OH) Glucose (C H O ) Hexane (C H ) 6 1 Methane (CH ) Methanol (CH OH) Sucrose (C H O ) g/cm g/cm 86 Decompose g/cm g/l g/cm g/cm 86 Decompose Inorganic Substances Name STP Melting Point ( C) Boiling Point ( C) Chlorine.1 g/l Hydrogen g/l 59 5 Hydrogen chloride 1.60 g/l Hydrogen sulfide 1.5 g/l Nitrogen 1.5 g/l Nitrogen monoxide 1. g/l Oxygen 1. g/l Sodium carbonate Sodium chloride.5 g/cm 851 Decomposes.165 g/cm Sulfur dioxide.9 g/l 7 10 *Water (at C) 1.00 g/cm NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page

3 Formulas D = m D = density V K = C + 7 m = mass PV T PV = V = volume T 1 1 t 1 P = P + P + P + K = Kelvin M V 1... = M V P = pressure 1 1 PV = nrt R = gas constant M = moles of solute T = temperature liters of solution q = mc p ΔT M = molarity q = mh v n = number of moles q = mh f q = quantity of heat energy ph + poh = 1 C p = specific heat ph = log[ H + ] H v = heat of vaporization poh = log[ OH ] H f = heat of fusion K = [ H ][ OH ] = 1 10 w [H ] = 10 + ph [OH ] = 10 E=hν c=λν + 1 poh K w = equilibrium constant for the ionization of water E = energy of a photon h = Planck s constant = 6.66 x 10 - Js ν = frequency of light c = speed of light =.00 x 10 8 m/s λ = wavelength of light 1 m = 10 9 nm NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page

4 NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 56 Ba Barium Cs Cesium 1 57 La Lanthanum Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Ra Radium (6) 87 Fr Francium () 89 Ac Actinium (7) 10 Rf Rutherfordium (61) 105 Db Dubnium (6) 106 Sg Seaborgium (6) 107 Bh Bohrium (6) 108 Hs Hassium (69) 109 Mt Meitnerium (68) 7 Rb Rubidium Rh Rhodium Ru Ruthenium Tc Technetium (98) Mo Molybdenum Nb Niobium Zr Zirconium Y Yttrium Sr Strontium Ca Calcium K Potassium Sc Scandium.96 Ti Titanium 7.88 V Vanadium 50.9 Cr Chromium 59 5 Mn Manganese Fe Iron Co Cobalt Mg Magnesium.1 11 Na Sodium.99 IVB 5 VB 6 VIB 7 VIIB 8 VIIIB 9 VIIIB IIIB Be Beryllium 9.01 Li Lithium H Hydrogen IIA 1 IA 91 Pa Protactinium Th Thorium.0 9 U Uranium Np Neptunium (7) 9 Pu Plutonium () 95 Am Americium () 96 Cm Curium (7) 59 Pr Praseodymium Ce Cerium Nd Neodymium Pm Promethium (15) 6 Sm Samarium Eu Europium Gd Gadolinium PERIODIC TABLE

5 NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 5 78 Pt Platinum Au Gold Hg Mercury Tl Thallium Pb Lead Bi Bismuth Po Polonium (09) 85 At Astatine (10) 86 Rn Radon () 110 Ds Darmstadtium (71) 111 Rg Roentgenium (7) 11 Uub Ununbium (77) 8 Cd Cadmium Ag Silver Pd Palladium Xe Xenon 1 5 I Iodine Te Tellurium Sb Antimony Sn Tin In Indium Ni Nickel Cu Copper Zn Zinc Ga Gallium 69.7 Ge Germanium 7.61 As Arsenic 7.9 Se Selenium Br Bromine Kr Krypton Ar Argon Cl Chlorine S Sulfur P Phosphorus Si Silicon Al Aluminum VIIIB 11 IB 1 IIB 5 B Boron C Carbon N Nitrogen O Oxygen F Fluorine Ne Neon 0.18 He Helium VIIA 1 IIIA 1 IVA 15 VA 16 VIA 18 VIIIA 97 Bk Berkelium (7) 98 Cf Californium (51) 99 Es Einsteinium (5) 100 Fm Fermium (57) 101 Md Mendelevium (58) 10 No Nobelium (5) 10 Lr Lawrencium (6) 65 Tb Terbium Dy Dysprosium Ho Holmium Er Erbium Tm Thulium Yb Ytterbium Lu Lutetium OF THE ELEMENTS

6 SOLUBILITY RULES Soluble: All Nitrates, Acetates, Ammonium, and Group 1 (IA) salts All Chlorides, Bromides, and Iodides, except Silver, Lead, and Mercury(I) All Fluorides except Group (IIA), Lead(II), and Iron(III) All Sulfates except Calcium, Strontium, Barium, Mercury, Lead(II), and Silver Insoluble (0.10 M or greater): All Carbonates and Phosphates except Group 1 (IA) and Ammonium All Hydroxides except Group 1 (IA), Strontium, Barium, and Ammonium All Sulfides except Group 1 (IA), (IIA), and Ammonium All Oxides except Group 1 (IA) Guidelines for Predicting the Products of Selected Types of Chemical Reaction Key: M = Metal NM = Nonmetal 1. SYNTHESIS: a. Formation of binary compound: A + B AB b. Metal oxide-water reactions: MO + H O base c. Nonmetal oxide-water reactions: (NM)O + H O acid. DECOMPOSITION: a. Binary compounds: AB A + B b. Metallic carbonates: MCO MO + CO c. Metallic hydrogen carbonates: MHCO MO+ H O (l) + CO (g) d. Metallic hydroxides: MOH MO + H O e. Metallic chlorates: MClO MCl + O f. Oxyacids decompose to nonmetal oxides and water: acid (NM)O + H O. SINGLE REPLACEMENT: a. Metal-metal replacement: A + BC AC + B b. Active metal replaces H from water: M + H O MOH + H c. Active metal replaces H from acid: M + HX MX + H d. Halide-Halide replacement: D + BC BD + C. DOUBLE REPLACEMENT: AB + CD AD + CB a. Formation of a precipitate from solution b. Acid-Base neutralization reaction 5. COMBUSTION REACTION Hydrocarbon + oxygen carbon dioxide + water NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 6

7 ACTIVITY SERIES of Halogens: F Cl Br I ACTIVITY SERIES of Metals Li Rb K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb [ H ] Sb Bi Cu Hg Ag Pt Au Replace hydrogen from cold water Replace hydrogen from steam Replace hydrogen from acids React with oxygen to form oxides + NH BrO CN CHO (CHCOO ) ClO ClO ClO ClO IO MnO NO NO OH HCO HSO SCN CO CrO 7 CrO SO SO PO Polyatomic Ions Ammonium Bromate Cyanide Acetate Perchlorate Chlorate Chlorite Hypochlorite Iodate Permanganate Nitrate Nitrite Hydroxide Hydrogen carbonate Hydrogen sulfate Thiocyanate Carbonate Dichromate Chromate Sulfate Sulfite Phosphate Boling Point Elevation and Freezing Point Depression ΔT = i K b m ΔT = i K f m i = van't Hoff factor Substance K b ( C/m ) K f ( C/m ) benzene camphor carbon tetrachloride ethyl ether water NCDPI Reference Tables for Chemistry (October 006 form A-v1) Page 7

8 Bohr Model for Hydrogen Atom (measurement in nanometers) n = 6 n = 5 n = n = n = E=hν h = 6.66 x 10 - Js c=λν c =.00 x 10 8 m/s 1 m = 10 9 nm n = 1 UV = Ultraviolet IR = Infrared IR Visible UV Electromagnetic Spectrum (measurement in meters) Microwaves X rays Radio waves Infrared Ultraviolet Gamma rays Longer Wavelength Visible Light Shorter Wavelength Red Orange Yellow Green Blue Violet NCDPI Reference Tables for Chemistry (October 006 form A-v1) Stock No Page 8

9 Common Polyatomic Ions ammonium C H O - - NH acetate CO - carbonate PO + - H O - hydronium hypochlorite chromate PO ClO - ClO - ClO - chlorite chlorate dichromate sulfate ClO - perchlorate sulfite CN - cyanide peroxide NO - NO - HCO - OH - MnO - nitrate C O - nitrite hydrogen carbonate (bicarbonate) hydroxide permanganate CrO Cr O - 7 SO - SO - O - oxalate phosphate phosphite Prefixes Used in Naming Common Metal Ions Binary Molecular Compounds Ion Systematic Common Name Name Prefix Number Fe + iron (II) ferrous mono 1 Fe + iron (III) ferric di Cu + copper (I) cuprous tri Cu + copper (II) cupric tetra Pb + lead (II) plumbous penta 5 Pb + lead (IV) plumbic hexa 6 Cr + chromium (II) chromous hepta 7 Cr + chromium (III) chromic octa 8 Sn + tin (II) stannous nona 9 Sn + tin (IV) stannic deca 10 Co + cobalt (II) cobaltous Co + cobalt (III) cobaltic + Hg mercury (I) mercurous Hg + mercury (II) mercuric ** ALWAYS: Zn +, Ag +, Cd + **

10 Periodic Table with Electronegativities 1A A B B 5B 6B 7B 8B 1B B A A 5A 6A 7A 8A 1 H.1 He Li 1.0 Be B.0 6 C.5 7 N.0 8 O.5 9 F.0 10 Ne 11 Na Mg 1. 1 Al Si P.1 16 S.5 17 Cl.0 18 Ar 19 K Ca Sc 1. Ti 1.5 V 1.6 Cr Mn Fe Co 8 Ni 9 Cu 0 Zn Ga 1.6 Ge 1.8 As.0 Se. 5 Br.8 6 Kr.0 7 Rb Sr Y 1. 0 Zr 1. 1 Nb 1.6 Mo 1.8 Tc Ru. 5 Rh. 6 Pd. 7 Ag 8 Cd In Sn Sb 5 Te.1 5 I.5 5 Xe.6 55 Cs Ba La Hf 1. 7 Ta W Re 76 Os. 77 Ir. 78 Pt. 79 Au. 80 Hg 81 Tl Pb 8 Bi 8 Po.0 85 At. 86 Rn. 87 Fr Ra Ac Rf 105 Db 106 Sg 107 Bh 108 Hs 109 Mt 110 Ds 111 Uuu 11 Uub 11 Uut 11 Uuq 115 Uup 116 Uuh 58 Ce Pr Nd Pm 1. 6 Sm 1. 6 Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np 1. 9 Pu Am Cm Bk Cf Es Fm Md No Lr Type of bond Electronegativity difference Nonplar covalent bond Polar covalent bond Ionic bond 0 to to and above

11 ::c "' O'J ~ ::::J 0 60 UI... 0 UI E <U... (.!) Solubility Curve I v v / - Kl/ / / ) ~/ v, /j / I , gases - NaN0 '---v J solids. v I \ /... / / v / KN0....t j HCI. NHCI"" ' "'l. I /.... ~, I /"" \......, ' I / NH..., NaS~ ~ I/ --. ',,... ~...- ' / ~ - ~ KC!>- / I y - '"/ ~KC I _,,, ,,,_... ~ " - ' NaCl / / / ~ ,, so , ; Temperature ( C)

12 Table H Vapor Pressure of Four Liquids 00 propanone ethanol 150 water Vapor Pressure (kpa) kpa ethanoic acid Temperature ( C) Reference Tables for Physical Setting/CHEMISTRY

13 Thermodynamic Quan ti ties for Selected Substances at K (5 C) Substance Aluminum Al(s) AlClJ(s) Al0J(s) Barium Ba(s) BaC0 (s) BaO(s) Beryllium Be(s) BeO(s) Be(OHh(s) Bromine Br(g) Br-(aq) Br(g) Br(1) HBr(g) Calcium Ca(g) Ca(s) CaC0 (s, calcite) CaC1(s) CaF(s) CaO(s) Ca(OHh(s) CaS0(s) Carbon C(g) C(s, diamond) C(s, graphite) CC1(g) CC1(1) illfo I!::.GJ 50 illfo I!::.GJ 50 (kj/mol) (kj/mol) O/mol-K) Substance (kj/mol) (kj/mol) O/mol-K) CF(g) CH(g) CH(g) CH(g) CH5(g) C H 8 (g) CH1o(g) CH10U) C5H5(g) C 6 H 6 (1) CH 0H(g) CH 0H(Z) CH 5 0H(g) CH 5 0H(l) C5H1P5(s) CO(g) C0(g) HCH 0(1) Cesium Cs(g) Cs(s) CsCl(s) Chlorine Cl(g) Ci-(aq) Cl(g) HCl(aq) HCl(g) Chromium Cr(g) Cr(s) Cr0 (s)

14 100 Appendix C / Thermodynamic Quantities for Selected Substances at K (5 C) illfo f1go so M:I/!:t.GJ so f 'f Substance (kj/mol) (kj/mol) (J/mol-K) Substance (kj/mol) (kj/mol) (J/mol-IO Cobalt Magnesium Co(g) Mg(g) Co(s) Mg(s) MgClz(s) Copper MgO(s) Cu(g) Mg(OHh(s) Cu(s) CuClz(s) Manganese CuO(s) Mn(g) Cu0(s) Mn(s) MnO(s) Fluorine Mn0(s) F(g) Mn0-(aq) p-(aq) F(g) Mercury HF(g) Hg(g) Hg(l) Hydrogen HgC1(s) H(g) HgCl(s) H+(aq) H+(g) Nickel H(g) Ni(g) Ni(s) Iodine NiC1(s) l(g) NiO(s) r(aq) l(g) Nitrogen 1(s) N(g) Hl(g) Nz(g) NH (aq) Iron NH (g) Fe(g) NH/(aq) Fe(s) Fe +(aq) Nz~(g) Fe +(aq) NHCN(s) 0.0 FeC1(s) N~Cl(s) NHN0(s) FeC1 (s) NO(g) FeO(s) Fez0 (s) N0 (g) Fe0(s) NzO(g) FeS(s) Nz0(g) NOCl(g) Lead HNOJ{aq) Pb(s) HN0(g) PbBr(s) PbC0(s) Oxygen Pb(N0 )i(aq) O(g) Pb(N0)z(s) -5 0(g) PbO(s) (g) OH-(aq) Lithium H0(g) Li(g) HzO(l) Li(s) Hz0(g) u+(aq) H0(l) u+(g) LiCl(s)

15 Appendix C I Thermodynamic Quantities for Selected Substances at K (5 C) 101 i Substance AH/ A.Gl so tjlo A.Gl S (kj/mod (kj/mol) (J/mol-IO Substance (kj/mol) (kj/mol) (J/mol-:K) Phosphorus Sodium P(g) Na(g) P(g) Na(s) P(g) Na+(aq) P(s, red) Na+(g) Pis, white) NaBr(aq) PC1(g) NaBr(s) PClJ(l) NaCOJ(s) PF 5 (g) NaCl(aq) PH(g) NaCl(g) PP6(s) NaCl(s) P01 0 (s) NaHCOJ(s) POC1(g) NaN0 (aq) POC1(1) NaNOJ(s) HP0(aq) NaOH(aq) NaOH(s) Potassium K(g) Strontium K(s) SrO(s) KCl(s) Sr(g) KC10(s) KCl0 (aq) Sulfur S(s, rhombic) K0(s) S0(g) KOi(s) sol-(aq) KN0(s) S0(g) K0i(s) SOC!i(l) -5.6 KOH(s) KOH(aq) HS(g) H S0(aq) Rubidium HS0(1) Rb(g) Rb(s) Titanium RbCl(s) Ti(g) ;_ RbC10(s) Ti(s) TiC1(g) Scandium TiClil) Sc(g) Ti0(s) Sc(s) Vanadium Selenium V(g) HSe(g) V(s) Silicon Zinc Si(g) Zn(g) Si(s) Zn(s) SiC(s) ZnC1(s) SiC~(l) ZnO(s) Si0(s, quartz) Silver Ag(s) Ag+(aq) AgCl(s) Ag0(s) AgN0(s) f

Σχετικά έγγραφα

ΜΟΡΙΑΚΟ ΒΑΡΟΣ ΟΡΥΚΤΟΥ (MB)

ΜΟΡΙΑΚΟ ΒΑΡΟΣ ΟΡΥΚΤΟΥ (MB) Oρυκτό: A x B y C z A x B y C z (MB) = x*a (AB) + y*b (AB) + z*c (AB) Κοβελλίνης (Cv): CuS Ατομικά βάρη: Cu=64, S=32 Cv (ΜΒ) = Cu (AB) + S (AB) = 64 + 32 = 96 Χαλκοπυρίτης (Cp):