General Nomenclature Review Stoichiometry Review

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1 chem101/3, wi2010 pe 08 1 CB I Chemical Bonding General Nomenclature Review Stoichiometry Review Ref 2: 8 3: all Prob see list next page HMWK #4 and #5 Adv Rdg 9: 5, 10: 1 chem101/3, wi2010 pe 08 2 Nomenclature & Stoichiometry Suitable Textbook Problems General Advice If you can do the in-text problems you should be OK. In each section, try the more difficult FUP problems, listed below, first. If you have difficulties try the simpler ones also, until you are fully proficient with the topic. Of course, also do my HMWK s. Nomenclature 2: 7-14 Mole Concept 3: 1-2 Balancing Chemical Equations 3: 8 Percent Composition/ Empirical Formula 3: 3-7 Stoichiometry 3: 10, 12-17, 19, 20 chem101/3, wi2010 pe 08 3 General At STP (standard temp. & pressure), few elements exist as single atoms: N. G., (noble gases) only The rest of the elements have bonds: metals: metallic bond non-metals: covalent bond In compounds, 2 kinds of bonds exist ionic covalent transfer of e s sharing of e s Driving force: to get octet of e s = full shells = max Z eff on each atom chem101/3, wi2010 pe 08 4 Ionic Bonding metal loses e s cation non-metal gains e s anion Ions held together (bound) by electrostatic ( Coulombic ) forces. Notes: In solids, 3- D lattice (grid, network) exists (no one - on - one relationship!) see Pet. Fig (SB Fig. 9.2) ion pairs, Na + Cl, may exist in gas state or liquid (molten) phase generally, in aqueous solution cations and anions are separated by H 2 O

2 chem101/3, wi2010 pe 08 5 Pet. Fig D Lattice of Ionic Solids (SB Fig. 9.2, similar) chem101/3, wi2010 pe 08 6 Covalent Bonding e s shared to get octet for every atom lowest energy at certain distance = bond length this energy = bonding energy, = energy required to separate bonded atoms completely Ex. Covalent bonding in H 2 molecule see Pet. Fig (also SB Fig. 9.2) chem101/3, wi2010 pe 08 7 Pet. Fig Covalent Bonding in H 2 chem101/3, wi2010 pe 08 8 Pet. Fig. 3.4 Covalent Bonding in S and P S 8 P 4

3 chem101/3, wi2010 pe 08 9 Nomenclature chem101/3, wi2010 pe Binary acids in H 2 O: hydro ic acid 1. Know symbol name & find position in P.T. quickly for first 36 elements plus HF (aq) 5. Binary Ionic Cmpds HI (aq) Sr Pd Ag Cd Sn Sb I Xe Cs Ba Pt Au Hg Pb Bi U 2. Diatomic/ Multiatomic Elements in their standard states : Cl i f Br o h n Cl 2, I 2, F 2, Br 2, O 2, H 2, N 2 also S 8, P 4 A. main group elements cation, anion ( ide) determine charge on ions (group in P.T.) smallest whole number ratio, balance for electroneutrality = crossover method CaO beryllium fluoride 3. Binary Covalent Cmpds ( nonmetal + nonmetal ) SrI 2 magnesium nitride less electronegative element first more electronegative element second (ending ide) use Latin/Greek prefixes ((mono), di, tri, tetra, penta, hexa, hepta, octa, nona, deca) K 2 S barium sulfide B. transition metals, also Sn, Pb Indicate charge on cation w/ Roman numeral CO TiCl 4 chromium(ii) chloride SF 6 NiS copper(i) oxide P 4 O 10 Fe 2 S 3 iron(iii) sulfide chem101/3, wi2010 pe Standard Oxoacids & Derived Anions H 2 CO 3 carbonic acid CO 3 2 carbonate chem101/3, wi2010 pe Acidic Anions (incomplete loss of H from acid): hydrogen.ate, ite, HNO 3 nitric acid NO 3 HSO 4 sodium hydrogen sulfate H 3 PO 4 phosphoric acid PO 4 3 NaHSO 3 dihydrogen phosphate anion H 2 SO 4 sulfuric acid SO 4 2 K 2 HPO3 sodium hydrogen carbonate HClO 3 chloric acid ClO 3 HBrO 3 bromic acid BrO 3 9. Hydrates: indicate # of H 2 O by Greek/Latin letters CuSO 4 5H 2 O copper(ii) sulfate pentahydrate Na 2 SO 4 10H 2 O HIO 3 iodic acid IO 3 7. More or Less O than standard acid/anion 2 less O : hypo..ous acid; hypo..ite 1 less O :..ous acid;..ite 1 more O: per..ic acid; per..ate HClO 2 potassium perchlorate HIO 4 sodium nitrite HNO 2 sodium sulfite KBrO ammonium phosphite 10. Special Cases NH 3 ammonia OH hydroxide NH 4 + ammonium CN cyanide H 2 O water MnO 4 permanganate H 2 O 2 hydrogen peroxide 2 CrO 4 chromate HC 2H 3O 2 (= CH 3CO 2H) acetic acid 2 Cr 2 O 7 dichromate C 2 H 3 O 2 acetate

4 chem101/3, wi2010 pe Nomenclature w/ Answers 1. Know symbol name & find position in P.T. quickly for first 36 elements plus Sr Pd Ag Cd Sn Sb I Xe Cs Ba Pt Au Hg Pb Bi U 2. Diatomic/ Multiatomic Elements in their standard states : Cl i f Br o h n Cl 2, I 2, F 2, Br 2, O 2, H 2, N 2 also S 8, P 4 3. Binary Covalent Cmpds ( nonmetal + nonmetal ) less electronegative element first more electronegative element second (ending ide) use Latin/Greek prefixes ((mono), di, tri, tetra, penta, hexa, hepta, octa, nona, deca) chem101/3, wi2010 pe Binary acids in H 2 O: hydro ic acid HF (aq) hydrofluoric acid 5. Binary Ionic Cmpds A. main group elements cation, anion ( ide) HI (aq) hydroiodic acid determine charge on ions (group in P.T.) smallest whole number ratio, balance for electroneutrality = crossover method CaO calcium oxide beryllium fluoride BeF 2 SrI 2 strontium iodide magnesium nitride Mg 3 N 2 K 2 S potassium sulfide barium sulfide BaS B. transition metals, also Sn, Pb Indicate charge on cation w/ Roman numeral TiCl 4 titanium(iv) chloride chromium(ii) chloride CrCl 2 CO carbon monoxide SF 6 sulfur hexafluoride NiS nickel(ii) sulfide copper(i) oxide Cu 2 O P 4 O 10 tetraphosphorus decaoxide Fe 2 S 3 iron(iii) sulfide iron(iii) sulfide Fe 2 S 3 chem101/3, wi2010 pe Standard Oxoacids & Derived Anions chem101/3, wi2010 pe Acidic Anions H 2 CO 3 carbonic acid 2 CO 3 HNO 3 nitric acid NO 3 H 3 PO 4 phosphoric acid 3 PO 4 H 2 SO 4 sulfuric acid 2 SO 4 HClO 3 chloric acid ClO 3 HBrO 3 bromic acid BrO 3 HIO 3 iodic acid IO 3 carbonate nitrate phosphate sulfate chlorate bromate iodate (incomplete loss of H from acid): hydrogen.ate, ite, HSO 4 hydrogen sulfate sodium hydrogen sulfate NaHSO 4 NaHSO 3 sodium hydrogen sulfite dihydrogen phosphate anion H 2 PO 4 K 2 HPO 3 potassium hydrogen phosphite sodium hydrogen carbonate NaHCO 3 9. Hydrates: indicate # of H 2 O by Greek/Latin letters CuSO 4 5H 2 O copper(ii) sulfate pentahydrate Na 2 SO 4 10H 2 O sodium sulfate decahydrate 10. Special Cases 7. More or Less O than standard acid/anion 2 less O : hypo..ous acid; hypo..ite 1 less O :..ous acid;..ite 1 more O: per..ic acid; per..ate HClO 2 chlorous acid potassium perchlorate KClO 4 HIO 4 perchloric acid sodium nitrite NaNO 2 HNO 2 nitrous acid sodium sulfite Na 2 SO 3 NH 3 ammonia OH hydroxide NH 4 + ammonium CN cyanide H 2 O water MnO 4 permanganate H 2 O 2 hydrogen peroxide 2 CrO 4 chromate HC 2H 3O 2 (= CH 3CO 2H) acetic acid 2 Cr 2 O 7 dichromate C 2 H 3 O 2 acetate KBrO potassium hypobromite ammonium phosphite (NH 4 ) 3 PO 3

5 chem101/3, wi2010 pe Chem. Formulas chem101/3, wi2010 pe Derivation of Avogadro s Number, N A empirical smallest whole number ratio of atoms Ex. hydrogen peroxide The following are definitions: (arbitrary, optimised for high precision) (relative) atomic mass of C-12 = 12 u (exact) 1 mol of C-12 = 12 g C-12 (exact) molar mass (MM) of C-12 = 12 g/mol molecular gives the number of each atom in molecule structural shows all bonds, may include geometric info, To find the number of atoms per mol (N A ), we need to determine the absolute mass (m) of a C-12 atom; (this can be done by mass spectrometry, X-ray crystalography...) m of C-12 (by experiment) = x g N A = MM m = 12 g/mol 1.993x10 23 g = x mol 1 chem101/3, wi2010 pe Mole Concept 1 mol = 6.02 x things N A = Avogadro s #; units: mol 1 chem101/3, wi2010 pe Mass Moles Use MM as CF (conversion factor) Practice can refer to atoms molecules formula units ions electrons photons electronic transitions molecular conversions ( dogs?) # of moles in 89.2 g NaF? Molar Mass (MM) mass of 1 mol of particles ; g units: mol to determine, see Pet., p. 72; (or SB, p. 93)

6 chem101/3, wi2010 pe Balancing Chem. Equations # of atoms of each kind same on both sides total charges same on both sides chem101/3, wi2010 pe balancing... Ex. PCl 5 + H 2 O H 3 PO 4 + HCl systematic trial & error method - start with an element in most complicated cmpd - balance O, H near end - do elements last - multiply/ divide to get simplest whole number coefficients chem101/3, wi2010 pe Stoichiometric Calculations MM W G MM chem101/3, wi2010 pe Limiting Reactant (L.R.) Check how much Product each Reactant can make Reactant that makes least Product = L.R. mass G moles G moles W mass W W G = M.R. (molar ratio) of W/G actual: Yield obtained in experiment ( g or mol) Ex. In the synthesis of NH 3, how many g of N 2 are needed to convert 35.2 g H 2? theoretical: calculated by stoichiometry ( g or mol) (take into account L.R.) % yield: actual theoretical x 100%

7 chem101/3, wi2010 pe % Composition from Chem. Formula Ex. Percentage of U in Yellow Cake? yellow cake = U 3 O 8 Imaginary Reaction: chem101/3, wi2010 pe Determination of Empirical Formula (from mass data, or combustion data, or...) convert to mole data for each element, then find simplest whole number ratio Ex. A cmpd contains 74.1% C, 8.64% H, 17.3% N. Empirical formula? Base on 100g cmpd: mass (g) divide by MM moles (mol) divide by lowest moles nearest whole numbers C H N Empirical Formula: chem101/3, wi2010 pe Molecular Formula Need MM data (from experiment) chem101/3, wi2010 pe Miscellaneous Density Divide MM of cmpd by MM of empirical formula to get multiplication factor usually: solids, liquids : g/ml gases: g/l (can be used as C.F. s) Ex. Empirical formula = (CH); MM 80 g/mol Molecular Formula? MM of empirical formula : 13.0 g/mol Concentration usually: mol/l ( M ) Dilution a.) c 1 V 1 = c 2 V 2, or b.) c 1 x V 1 V 2 x V 3 V 4 x... = c final

8 chem101/3, wi2010 pe CB I Summary Distinguish between ionic and covalent bonding Systematic Nomenclature Review: distiguish 8 different cases; convert name formula Systematic Stoichiometry Review mole concept balancing chem. equations mass relations in chem. rxns chem. compostion from formula empirical formula from composition or reaction data molecular formula from molecular mass and empirical formula

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