Modern Chemistry Chapter 7 Chemical Formulas and Chemical Compounds Sections 1, 3 & 4 Chemical Names and Formulas Using Chemical Formulas Determining Chemical Formulas Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Monatomic ion Binary compound Nomenclature Oxyanion Salt Formula Mass Percent Composition Empirical Formula Chapter Vocabulary Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Chemical Names and Formulas Section 1 Chemical Names and Formulas Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Chemical Formula C H Molecular compounds – for one molecule Ionic compounds – for one formula unit; the simplest ratio of cations to anions C H 8 18 Eighteen hydrogen atoms in the molecule Eight carbon atoms in the molecule Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Chemical Formula 5 ions – two Al 3+ ions and three (SO4) 2- ions Al (SO ) 2 4 3 4 SO4 ions 2 Al atoms 4 O atoms Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Definitions Hydrocarbon – compounds containing hydrogen and carbon Binary Compound – compound with only two types of atoms Nomenclature – a naming system Oxyanions – negative polyatomic ions with oxygen in them Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Definitions Monatomic ions – ions formed from a single atom For negative monatomic ions, -ide is added to the root name Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

How can I tell if the compound is ionic or covalent ???? Ionic compounds contain a metal and/or a polyatomic ion !!! Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Writing Fomulas and Naming Ionic Compounds Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Charges on Monatomic Ions 1+ 2+ 3+ 3- 2- 1- Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Charges on Transition Metals Ag 1+ Zn 2+ Cu 1+ or 2+ Fe/Cr 2+ or 3+ Sn 2+ or 4+ Pb 2+ or 4+ Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Charges of Metals PbO2 and PbO Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Polyatomic Ions Page 226 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Ionic Compounds Formulas Write the symbols Determine the charges Monatomic ions from the periodic table Transition metals from a roman numeral Polyatomic ions from a chart on p. 226 Cross the charges. Reduce to lowest ratio. Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Ionic Compounds Names Write the cation name. Write the anion name. Add –ide to the anion if monatomic Add the roman numeral for any transition or group 14 metal. NO PREFIXES!!!! Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ionic Binary Compounds Aluminum Oxide FORMULAS 3+ 2- Al O 3 2 (3+ x ) + (2- x ) = 0 2 3 Al2O3 (charge x subscript)+(charge x subscript) = 0 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ionic Binary Compounds Aluminum Oxide FORMULAS 3+ 2- Al O 3 2 REDUCE IF NECESSARY!! Al2O3 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ionic BinaryCompounds NAMING Mg3N2 NO PREFIXES!! Magnesium Nitrogen ide Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 1. Write formulas for the binary ionic compounds formed between the following elements: a. potassium and iodine b. magnesium and chlorine c. sodium and sulfur d. aluminum and sulfur e. aluminum and nitrogen 2. Name the binary ionic compounds indicated by the following formulas: a. AgCl e. BaO b. ZnO f. CaCl2 c. CaBr2 d. SrF2 Practice Page 223 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ionic Compounds with Transition Metals FORMULAS Iron (III) Chloride 3+ 1- Fe Cl 1 3 (3+ x ) + (1- x ) = 0 1 3 FeCl3 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ionic Compounds with Transition Metals FORMULAS Tin (II) Oxide 2+ 2- Sn O 1 1 (2+ x ) + (2- x ) = 0 1 1 SnO Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ionic Compounds with Transition Metals FORMULAS Tin (II) Oxide 2+ 2- Sn O 2 1 1 2 REDUCE! SnO Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 1. Write the formula and give the name for the compounds formed between the following ions: a. Cu 2+ and Br − d. Hg 2+ and S 2− b. Fe 2+ and O 2− e. Sn 2+ and F − c. Pb 2+ and Cl − f. Fe 3+ and O 2− 2. Give the names for the following compounds: a. CuO c. SnI4 b. CoF3 d. FeS Practice Page 225 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ionic Compounds with Transition Metals NAMING PbO ( x 1 ) + ( 2- x 1 ) = 0 2+ NO PREFIXES!! Lead II Oxygen ide Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ionic Compounds with Polyatomic Ions FORMULAS Ammonium Sulfate + 2- (NH ) (SO ) 4 2 4 1 (1+ x ) + (2- x ) = 0 2 1 (NH4)2SO4 Parenthesis are needed if the p. ion has a subscript from the crossed charge – outside the ( ). Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ionic Compounds with Polyatomic Ions NAMING Ca(NO3)2 NO PREFIXES!! Calcium Nitrate Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 1. Write formulas for the following ionic compounds: a. sodium iodide e. copper(II) sulfate b. calcium chloride f. sodium carbonate c. potassium sulfide g. calcium nitrite d. lithium nitrate h. potassium perchlorate 2. Give the names for the following compounds: a. Ag2O b. Ca(OH)2 c. KClO3 d.NH4OH e. Fe2(CrO4)3 f. KClO Practice Page 227 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Writing Fomulas and Naming Molecular Compounds Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Prefixes for Covalent Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 p. 228

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Molecular Compound Formulas Write the symbols. Use prefixes for subscripts. DON’T reduce. Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Molecular Compound Names Write the name of the elements. Order: Smaller group number first; Same group? Greater period number first. Add –ide to the second element. Add prefixes to each element for the number of atoms. Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Binary Molecular Compounds FORMULAS Disulfur difluoride S F 2 2 DON'T REDUCE! S2F2 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Binary Molecular Compounds NAMING O N 2 4 di nitrogen tetra oxygen ide Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 1. Name the following binary molecular compounds: a. SO3 b. ICl3 c. PBr5 2. Write formulas for the following compounds: a. carbon tetraiodide b. phosphorus trichloride c. dinitrogen trioxide Practice Page 229 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Acids and Salts Acids – Chapter 14 Binary Acids – two elements; hydrogen and one other element Oxyacids – contain hydrogen, one other element and oxygen Acid – a solution of the compound in water. Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Acids and Salts Salt – an ionic compound Made from the cation of a base and the anion of an acid Some retain an H in the anion Example: CO3 2- carbonate HCO3 1- hydrogen carbonate or bicarbonate Ch 7 Sec 1 Chemical Names & Formulas pages 219-231

Salt Definition Animation Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 p. 230

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 List of Acids Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 p. 230

Ch 7 Sec 1 Chemical Names & Formulas pages 219-231 Section 1 Homework Section Review Page 231 #1-5 Ch 7 Sec 1 Chemical Names & Formulas pages 219-231