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Naming Chemical Compounds and Stoichiometry

This chapter covers the naming of ionic and molecular compounds, as well as the calculation of stoichiometry in chemical reactions.

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Naming Chemical Compounds and Stoichiometry

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  1. Chapter 6 0 6.1 -6.4 Naming Ionic Compounds A. Type I compounds 1. Metal in compounds forms only one type of ion 2. Most main group metals form type I compounds Naming type I binary ionic compounds 1. Name of cation (metal) + (base name of anion + ide) 2. Example, NaCl is sodium chloride B.Type II compounds 1. Metal forms more than one type of ion 2. Transition metals usually, but not exclusively, form type II compounds Naming type II binary ionic compounds 1. Name of cation + (charge of cation) + (base name of anion + ide) 2. Charge of cation given in roman numerals 3. FeCl3 is iron (III) chloride C. Naming Molecular Compounds BINARY(Greek prefixes!!) A. Formed between 2 or more nonmetals B. (Prefix)name of first element + (prefix) base name of second element + ide C. 1 = mono; 2 = di; 3 = tri; 4 = tetra… D. Example, N2O is dinitrogen monoxide

  2. 6.6 Naming Acids A. Molecular compounds that dissolve in water to form H+ ions B. Binary acids 1. Hydrogen and nonmetal 2. (Hydro + base name of nonmetal + ic) + acid 3. Example, HCl is Hydrochloric acid ___Up to here for TEST 2_____________________________ 6.5 . Naming ionic compounds containing a polyatomic ion 1. Use the same procedure as ionic compounds 2. Use name of polyatomic ion, not constituent atoms 3. Example, NaNO3 is sodium nitrate C. Oxyacids 1. Hydrogen and polyatomic oxyanion 2. Oxyanions ending with –ate a. (Base name of oxyanion + ic) + acid b. Example, HNO3 is nitric acid 3. Oxyanions ending with –ite a. (Base name of oxyanion + ous) + acid b. Example, HNO2 is nitrous acid 6.7 Formulas and Nomenclature Summary A. Ionic compounds B. Molecular compounds C. Acids

  3. Quantitative Composition 7 7.1 Stoichiometry—What is it?- Quantities in a chemical reactions 7.2-7.3 Mole: Counting Atoms by the Gram A. Pair =2; dozen = 12; 1 mole = 6.02 x 1023 B. 1 mole of Au atoms = 6.02 x 1023 Au atoms C. The periodic table gives the mass of 1 mole of that atom in grams 1 mole of S atoms = 32.06 g S ; 1 mole of C atoms = 12.01 g C D. Unit conversions between grams and moles of atoms Moles = grams/Molar mass Extend idea to Molecules by the Gram A. Mass of 1 mole H2O = mass of 2 moles of H + 1 mole O B. Calculations performed in a similar fashion C. Learn to calculate molar mass of compounds by adding units 7.4-7.5Chemical Formulas as Conversion Factors A. Molecular formula gives ratios of atoms in molecule B. Converting moles of atoms to moles of molecules C. Converting grams of atoms to grams of molecules 1 mol H2O 6.02 x 1023 H2O molecules 18.016 g H2O

  4. 7.6 Learn the % composition- EASY!!! Mass Percent Composition of Compounds A. Percentage of molecule's total mass that is due to atom X B. Convert between mass of element and mass of compound C. Mass Percent Composition from a Chemical Formula 7.7-7.8Calculating Empirical Formulas for Compounds A. Empirical formula is the smallest whole number ratio of atoms B. Mostly different from molecular formula C. Many different compounds may have the same empirical formula Calculating Molecular Formulas for Compounds A. Empirical formula molar mass B. Compare molar mass to empirical formula mass C. Ratio= (Molar mass/emp. Mass) = (molecular formula/Emp. Formula) D. Ratio n is the nearest whole number 4 steps in Empirical formula problem 1) % to grams 2) Grams/Molar mass = Moles 3) Divide all moles by Smallest moles 4) Use appropriate rounding rules to get Empirical formulas For finding molecular formula Ratio the molecular mass and empirical mass to concert empirical formula to molecular formula 0

  5. Chemical Equations 8 0 8.1-8.2 The Chemical Equation A. Reactants go to products B. Cannot create or destroy atoms in a chemical equation C. Reaction must be balanced Evidence of a Chemical Reaction A. Color change B. Formation of solid or gas C. Heat/light absorption or emission D. transfer of electron 8.3 Balancing Chemical Equations How to Write Balanced Chemical Equations A. Write reactant and product species, including physical states (s, l, g, aq.) B. If an element occurs only once on each side of the reaction, balance that first C. Balance free reactants last D. Clear non-integer coefficients Practice from Lab manual Exercise on Balancing chemical equation

  6. Chemical Equations 8 0 8.1 -8.2 Identify Evidence of a Chemical Reaction Aqueous Solutions and Solubility: Compounds Dissolved in Water A. Aqueous: mixture of substance in water B. Soluble: dissolves in water Li+, Na+, K+, NH4+,NO3-, C2H3O2- C. Insoluble: does not dissolve in water (CO3 2–, PO43– except Li+, Na+, K+, NH4+ etc) D. Solubility rules –Check in the back of lab manual Important: Practice with Single double displacement :Labs 8.3 Writing equations: 1) First break reactants into ions with the correct charges 2) Then swap anions and cations, and come up with correct formula for products 3) Then identify physical states (s, l, g, aq.), 4) Last step BALANCE!; Ignore total and net ionic equations 8.4 Acid - Base and Gas Evolution Reactions (H2CO3, H2SO3, NH4OH) Reactions of Acids and Bases-Forms salt and water • Acids produce H+ , bases produce OH- and they react to form water B. Gas evolution – many different possible products (CO2 , SO2 ,NH3, H2S) (H2CO3 splits as H2O and CO2 )

  7. 8.5 Single displacement reaction- also called redox reaction • Remember the activity series of metal • 1A strongest metals, then IIA metals, Fe, …Zn….. • Pb H Cu, Ag and Au least reactive…… • A + BC B + AC A is stronger than B • 8.6 Other ways to Classify Types of Chemical Reactions • A. Synthesis or combination reactions A + B  AB • B. Decomposition reactions AB  A + B • C. Single Displacement reactions A + BC AC + B • D. Double-displacement reactions AB + CD AD + CB

  8. Chapter 9 Chemical QuantitiesSections (9.1, 9.2 9.3) omit Rest of the sections • Moles  moles of reactants and products • Start from Balanced chemical Equation • Moles is like cups in a recipe • In moles to moles problem – Moles from Balanced chemical equation • NO NEED TO CALCULATE molar mass, Avogadro number etc. • Grams Grams of reactants and products • Start from Balanced chemical Equation • Calculate the molar masses for things in question • Multiply by the coefficients with molar masses for stoichiometric equivalence • Moles  Grams of reactants and products • Moles = weight in grams/molar mass Chapter 9 Balance equations First!!! Calculations in chemical reaction how much reactant will produce how much product, moles to moles, grams to grams etc- STOICHIOMETRY

  9. 0 EXAM 3- 100 POINTS Part 1 Multiple Choice –Show calculations for partial/full credit (60 points) BRING SCANTRON Part 2, 3 Complete and Balance equations (10 points) Part 4 Moles, empirical formula and % compositions (30 points) Stoichiometry-Chapter 9

  10. 0 Sample questions—Exam 3 Part I MULTIPLE CHOICE on all sections, nomenclature Part II and III 1. Ba(NO3)2 + K2CO3 • HCl + NaOH  SO2 + O2  SO3 -Balance! Part IV Moles to grams to # of atoms/molecules empirical formula problems, % compositions Chemical quantities, mole to moles in a reaction

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