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Chapter 6 Lesson 3 (Part I)

Chapter 6 Lesson 3 (Part I). “Names and Formulas for Ionic Compounds”. I. Oxidation Charges. A. Def – a positive or negative number assigned to an atom or compound. 1. Use the Periodic Table 2. Ex: Lithium a. Li loses 1 electron and becomes 1+ 3. Ex: Fluorine

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Chapter 6 Lesson 3 (Part I)

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  1. Chapter 6Lesson 3 (Part I) “Names and Formulas for Ionic Compounds”

  2. I. Oxidation Charges A. Def – a positive or negative number assigned to an atom or compound. 1. Use the Periodic Table 2. Ex: Lithium a. Li loses 1 electron and becomes 1+ 3. Ex: Fluorine a. F gains 1 electron and becomes 1-

  3. II. Binary Compounds A. Def – composed of 2 elements 1. Ex: Sodium Chloride (NaCl) 2. Groups 1-8 have set oxidation numbers. (1, 2, 3, -3, -2, -1, 0) B. Multiple Oxidation Numbers 1. Transition Metals a. Use Roman numerals to represent charge -Ex: Cu (II) = -Ex: Cu (III) = Cu2+ Cu3+ *Metals always have a positive charge / lose electrons

  4. III. Writing Formulas A. 4 step system 1. Write the Symbol with positive oxidation # 2. Write the Symbol with negative oxidation # 3. Done if superscripts equal zero. If unequal #4 4. Criss Cross Method B. Ex: Chlorine and Sodium combine Na1+ + Cl1- =‘s 0 Oxidation numbers equal zero NaCl

  5. C. Sodium combines with oxygen 1. Na1+ + O2- rule #4 Na 1+ O 2- Drop the superscript charges Criss Cross Na2O *oxidation numbers equal zero

  6. Examples 1. Sodium Fluoride 2. Calcium Chloride 3. Aluminum Oxide 4. Iron (II) Chloride 5. Iron (IV) Bromide 6. Copper (II) Nitride 7. Magnesium Oxide 8. Mercury (I) Nitride

  7. IV. Naming Binary Compounds A. 4 step system 1. Write the name of the 1st element 2. Write the “root” name of the second element. 3. Add “ide” 4. Check for Transition Metals B. Ex: CaCl2 1. Calcium Chlor ide

  8. 2. Examples K3N Al2S3 Mo2O FeCl3 ZnF2

  9. V. Polyatomic Ions A. Def – having many atoms 1. Works as a covalent group 2. Have a single charge (usually negative) 3. List of Polyatomic Ions – pg. 173 B. Naming 1. Write name of positive ion 2. Write name of negative ion 3. Check for Transition Metal 4. Ex: NaNO3 + Nitrate Sodium

  10. C. Writing the formula 1. Write symbol of positive ion 2. Write symbol of negative ion 3. Check oxidation #’s to see if they equal zero 4. Criss Cross Method -Use parenthesis to “set apart” a polyatomic ion when more than one is needed. 5. Ex: Write the formula for calcium nitrate. 1- 2+ ( ) Ca(NO3)2 NO3 Ca

  11. Reminders with Transition Metals • For naming compounds with transition metals always include the Roman Numeral. • To determine the oxidation number of a transition metal in a formula add up all charges of the opposite ion. • Chemical formula do not need Roman Numerals.

  12. Chapter 6Lesson 3 (Part II) “Names and Formulas for Molecular (Covalent) Compounds”

  13. Common prefixes • Only use with non-metals • Pg. 175 • **Do not use ionic charges!!!**

  14. VI. Naming Molecular Compunds A. Rules 1. Most metallic element listed 1st 2. Prefix + element name 3. Prefix + element name + add “ide” B. Ex: N2O4 Di Nitrogen Tetra Oxygen Oxide

  15. B. Name the following molecular compounds. 1. CO 2. H2O 3. NO 4. N2O 5. C4H8 6. Br2F8 7. P2O5

  16. C. Writing Formulas for Molecular Compounds 1. Use the prefixes for each element and convert them to subscripts 2. Ex: Tetraiodine nonaoxide = I4O9 3. Ex: Dicarbon pentafluoride = C2F5

  17. D. Write the formulas for the following molecular compounds 1. Carbon Dioxide 2. Sulfur Hexafluoride 3. Phosphorus Tribromide 4. Diphosphorus pentaoxide 5. Carbon Heptaoxide 6. Dicarbon decafluoride

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