1. Nomenclature and Chapter 7 5.7 Nomenclature: Naming Compounds A. Systematic name, e.g. sodium chloride B. Common name, e.g. table salt 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 B. Naming type I binary ionic compounds 1. Name of cation (metal) + (base name of anion + ide) 2. Example, NaCl is sodium chloride C. Type II compounds 1. Metal forms more than one type of ion 2. Transition metals usually, but not exclusively, form type II compounds D. 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. FeCl 3 is iron (III) chloride E. 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, NaNO 3 is sodium nitrate Naming Molecular Compounds 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, N 2 O is dinitrogen monoxide

2. 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 C. Oxyacids 1. Hydrogen and polyatomic oxyanion 2. Oxyanions ending with –ate a. (Base name of oxyanion + ic) + acid b. Example, HNO 3 is nitric acid 3. Oxyanions ending with –ite a. (Base name of oxyanion + ous) + acid b. Example, HNO 2 is nitrous acid Nomenclature Summary A. Ionic compounds B. Molecular compounds C. Acids

3. 7.1 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 absorption or emission D. Light emission 7.3 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 7.4 Classifying 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 Chemical Reactions Chapter 7

4. 7.5 Aqueous Solutions and Solubility: Compounds Dissolved in Water A. Aqueous: mixture of substance in water B. Soluble: dissolves in water Li+, Na+, K+, NH4+,NO 3 -, C 2 H 3 O 2 - C. Insoluble: does not dissolve in water (CO 3 2–, PO 4 3– except Li, Na, K, NH4 etc) D. Solubility rules –Check in the back of lab manual Precipitation Reactions: Reactions in Aqueous Solution that Form a Solid A. Aqueous ions combine to form insoluble products B. Predicting precipitation reactions 1. Predict potential solid products 2. Check solubility rules 3. If all potential solid products are soluble, there is no reaction Important: Practice with Single double displacement :Labs Writing equations: First break reactants into ions with the correct charges Then swap anions and cations, and come up with correct formula for products Then identify physical states (s, l, g, aq.), Last step BALANCE! 7.8 Acid - Base and Gas Evolution Reactions Reactions of Acids and Bases-Forms salt and water Acids produce H +, bases produce OH - B. Gas evolution – many different possible products (CO 2, SO 2,NH 3, H 2 S)

5. Sample questions—Exam 3 Write chemical formulas and write chemicals names SO 2 + O 2 → SO3 -Balance! Which of the following compounds are INSOLUBLE? potassium carbonate lithium acetate magnesium bromide aluminum sulfide Complete the following: 1.Ba(NO 3 ) 2 + K 2 CO 3 → 2.HCl + NaOH →