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Unit 6 Chemical Nomenclature and Chemical Reactions Naming Binary Compounds A binary compound is To properly name the binary compound you must first decide if it is ionic or covalent. How do you determine this? The binary compound must Naming Binary Ionic Compounds - Type 1 1. The cation is always written first, then the anion. 2. Examine the cation, decide if it is a transition metal or a main group metal. 3. If it is a main group metal, the binary compound is Type 1. Charges on Type 1 cations: 1 = Group Group 2 = Group 13 = 1 Naming Binary Ionic Compounds - Type 1 1. Name the cation first using the name of the element. 2. Name the anion using the root of the element name and adding - “ide” as the suffix. NaCl - CaO - AlN - Naming Binary Ionic Compounds - Type 2 1. Examine the cation, decide if it is a transition metal or a main group metal. 2. If it is a transition metal, the binary compound is Type 2. Transition metals form multiple types of cations. Charges on Type Cu1+ , Cu2+ Cr3+ , Mn2+, 2 cations: Cr6+ Mn4+ Naming Binary Ionic Compounds - Type 2 1. Name the cation first using the name of the element. 2. Use the charge on the anion to determine the charge on the cation, remembering that the overall charge of the compound must be zero. 3. Add a Roman numeral after the cation to denote the charge on the cation. 4. Name the anion using the root of the element name and adding - “ide” as the suffix. TiO2 CuBr - CrS3 - 2 Exceptions Main group: Compounds containing Pb, Sn, and Bi need Roman numerials to indicate the charge on the cation Transition metals: Zn, Ag, and Cd only form one type of cation. No Roman numeral is necessary. Naming Binary Covalent Compounds Binary covalent compounds contain two types of nonmetals bonded together, or a metalloid and a nonmetal. 1. Name the elements in the order listed in the formula. 2. Use prefixes to indicate the number of each kind of atom. 3. Omit the prefix mono- when the formula contains only one atom of the first element in the name. 4. The suffix of the name of the second element is -ide. Naming Binary Covalent Compounds Prefixes 3 Practice 1. CS2 2. IF7 3. B2O3 4. SiO4 5. H2O Naming Ionic Compounds Containing Polyatomic Ions 1. To name a compound containing a polyatomic ion, state the cation first. You must determine if it is a main group metal or transition metal and name the cation properly. 2. Then name the anion. Use the proper name of the polyatomic ion. Examples: NaClO AgNO2 PbSO4 Writing Formulas from Names For ionic Compounds: 1. Write the symbol of the cation and then the anion with their respective charges. (For polyatomic ions you are expected to know their charges and names.) 2. Add whatever subscripts are needed to balance the charges, or criss-cross. 1. Calcium nitride - 2. Cobalt (III) chloride - 3. Iron (II) hydroxide - 4. Magnesium sulfate - 5. Lead (IV) sulfide - 4 Practice Tin (II) Naming Acids An acid is a compound that contains one or more hydrogen atoms and produces Ex: Naming Binary Acids – HCl 1. Identify the anion Cl = 2. Name the anion with an –ic suffix Cl- = 3. Add a hydro- prefix to the anion name Add the word acid to the end 4. Tro's Introductory Chemistry, Chapter 5 15 5 Naming Oxyacids H2SO4 1. Identify the anion SO4 = SO42- 2. If the anion has –ate suffix, change it to –ic. If the anion has –ite suffix, change it to -ous SO42- = 3. Write the name of the anion followed by the word acid Tro's Introductory Chemistry, Chapter 5 16 Naming Oxyacids H2SO3 1. Identify the anion SO3 = 2. If the anion has –ate suffix, change it to –ic. If the anion has –ite suffix, change it to -ous SO32- = 3. Write the name of the anion followed by the word acid Tro's Introductory Chemistry, Chapter 5 17 Practice HI HIO HIO2 HIO3 HIO4 6 Unit 6 Chemical Nomenclature and Chemical Reactions Chemical Equations Chemical Reaction = process whereby one or more reactants are changed into products • indicate physical states: (s), (l), (g), (aq) • equation must be balanced • matter must be conserved (same number of each kind of atom on reactant and product sides) • Charge must be conserved (same overall charge) • only change coefficients; never change subscripts to balance an equation Balancing Chemical Equations Step 1 Write an unbalanced equation containing the correct formulas of the reactants and products. Step 2 Write the symbol for each element underneath the yield symbol. Step 3 Write the number of each element present on the reactant side of the equation in front of the element symbol. Write the number of each element present on the product side of the equation behind the element symbol. 7 Balancing Chemical Equations Step 4 Balance each element. Leave the elements that are present in multiple compounds until the very end; they might take care of themselves. Step 5 Verify that the number of atoms of each element is balanced. Examples NH3(g) + O2(g) NO(g) + H2O(g) Examples C7H14(g) + O2(g) CO2(g) + H2O(g) 8 Examples Glass is sometimes decorated by etching patterns on its surface. Etching occurs when hydrofluoric acid reacts with silicon dioxide in the glass to form gaseous silicon tetrafluoride and liquid water. Write and balance the equation for this reaction. Balancing Chemical Equations Patterns of Chemical Reactions Combination Reactions (Synthesis) - Two or more substances react to form a single product. 1. 1. X + Y --> XY 2. 2Na(s) + Cl2(g) --> 2NaCl (s) 9 Combination Reaction Patterns of Chemical Reactions 2. Decomposition Reactions - One substance decomposes to form two or more products. XY --> X + Y 2H2O (l) --> 2H2 (g) + O2(g) Decomposition Reaction 10 Patterns of Chemical Reactions 3. Combustion Reaction A combustion reaction is a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light. CxHy + O2 -> CO2 + H2O +ENERGY! Combustion Reaction 4. Single Replacement One element displaces another in a compound Type 1: element is a metal M + M’A → M’ + MA Cu(s) + 2 AgCl(aq) → 2 Ag(s) + CuCl2 Type 2: element is a halogen X2 + 2 BX’ → X’2 + BX Cl2 + 2 KBr → Br2 + 2 KCl Use activity series to predict whether reaction “goes” element + compound → element + compound 11 Metal Activity Series Metal Ion(s) Processes Used to obtain the Metal State of Metal Li+ K+ Ca2+ Na+ Mg2+ Al3+ Pass electricity through molten mineral (electrometallurgy) Li(s) K(s) Ca(s) Na(s) Mg(s) Al(s) Manganese Zinc Chromium Iron Mn2+ Zn2+ Cr3+, Cr2+ Fe3+, Fe2+ Heat mineral with charcoal or carbon monoxide (CO) (pyrometallurgy) Mn(s) Zn(s) Cr(s) Fe(s) Lead Copper Mercury Silver Platinum Gold Pb2+ Cu2+, Cu+ Hg2+ Ag+ Pt2+ Au3+, Au+ Element Lithium Potassium Calcium Sodium Magnesium Aluminum most Active Heat mineral in air (pyrometallurgy) or find the element free least active Pb(s) Cu(s) Hg(s) Ag(s) Pt(s) Au(s) Trends in Metal Activity A more reactive metal (higher in the activity series) will cause ions of a less reactive metal (lower in the activity series) to change to its corresponding metal Mg + ZnCl2 Zn + MgCl2 Mg + ZnCl2 MgCl2 + Zn What are the charges on the metals? Details: 12 Oxidation of Cu(s) occurs with reduction of Ag+ (aq) Cu(s) Cu: + 2 Ag+(aq) + Ag+ + Ag+ Cu2+(aq) + 2 Ag(s) Cu2+ + Ag + Ag Cu is oxidized: it loses 2 electrons; Cu is the _____________ Ag+ is reduced: it gains 1 electrons; Ag+ is the ____________ Mnemonics for Oxidation/Reduction OIL RIG: LEO (the lion) says GER: Terminology - Redox Reactions OXIDATION — REDUCTION — OXIDIZING AGENT—electron acceptor; species is reduced. REDUCING AGENT—electron donor; species is oxidized. 13 Oxidation Numbers An oxidation number is a positive or negative number assigned to an atom to indicate its degree of oxidation or reduction. As a general rule, a bonded atom’s oxidation number is the charge that it would have if the electrons in the bond were assigned to the more electronegative element. Assign an oxidation number to each Cr atom. K2CrO4 Cr2O3 14 Single Replacement 15 Patterns of Chemical Reactions 5. Double Replacement - There is an interchange of partners between two compounds AB + XY --> AY + XB Pb(NO3)2 (aq) + K2CrO4 (aq) --> PbCrO4 (s) +2KNO3 (aq) The reaction proceeds only if one of the products is insoluble in the reaction mixture ZnBr2(aq) + 2 Ag(NO3)2(aq) → Zn(NO3)2(aq) LiCl(aq) + Na2SO4(aq) 2 NaCl(aq) + Li2SO4(aq) → + 2 AgBr(s)↓ Double Replacement Predicting Whether a Reaction Will Occur Keys to understanding spontaneous chemical processes: 1. Energy spread. Reactions occur so that more stable products are formed 2. Matter spread. The most common “driving forces” that pull reactants toward products are Formation of Formation of Transfer of electrons Formation of 16 Practice Classify each reaction as one of the four general types a) Pt(s) + 2F2(g) PtF4(l) b) 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g) c) 2H3BO3(s) B2O3(s) + 3H2O(l) d) BaCl2(aq) + Na2SO4(aq) BaSO4(s) + 2NaCl (aq) 17