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Chapter 9 Chemical Names and Formulas

Chapter 9 Chemical Names and Formulas. Ms. Wang Lawndale High School. Monatomic Ions. Chapter 9.1 – Naming Ions. Consist of a single atom with a positive or negative charge. Example: Li + , Na + , K + , Cl - , Ca 2+ , Mg 2+ , F - , S 2-. Which ones are cations? Which ones are anions?.

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Chapter 9 Chemical Names and Formulas

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  1. Chapter 9Chemical Names and Formulas Ms. Wang Lawndale High School

  2. Monatomic Ions Chapter 9.1 – Naming Ions • Consist of a single atom with a positive or negative charge • Example: Li+, Na+, K+, Cl-, Ca2+, Mg2+,F-, S2- • Which ones are cations? Which ones are anions? Polyatomic Ions • Composed of more than one atom • The entire unit is comprised of one charge • Example: SO42-, NO2-, ClO2-

  3. Chapter 9.2 – Naming Ionic Compounds • Binary Compound – composed of 2 elements

  4. Rules for Naming Chemical Formulas Write the cation first and then the anion • Cation keeps its name • Anion changes its ending The correct formula contains the fewest positive and negative ions needed to make the electrical charge ZERO.

  5. Anion changes its ending… –ine, From -ygen, To -ide -fur, -ogen Fluorine becomes fluoride Oxygen becomes oxide Example: Write the chemical formula for Calcium Chloride

  6. Practice Cesium Oxide Strontium Fluoride Tin (II) Sulfide Potassium Bromide Copper (II) Oxide Sodium Iodide Potassium Sulfide Calcium Oxide • Cs2O • SrF2 • SnS • KBr • CuO • NaI • K2S • CaO

  7. How to Write Formulas for Ionic Compounds Step 1: Write the symbol and charges for the cation and anion Question: What is the formula for aluminum oxide? Aluminum =Al3+ Oxygen = O2- Step 2: Write the symbol for the ions side by side, beginning with the cation Al3+O2- Step 3: Find the least common multiple of the ions’ charges. The least common multiple of 2 and 3 is 6. To be neutral you would need 6 + and 6- To get 6+, you need two Al3+ ions To get 6-, you need three O2- ions Al2O3

  8. How to Write Formulas for Ionic Compounds Magnesium =Mg2+ Chloride =Cl- Example: what is the formula for Magnesium Chloride? Mg2+Cl- 3. Least common multiple of 2 and 1 = 2 To get 2+, need one Mg To get 2-, need two Cl MgCl2 CHEATER METHOD: JUST CRIS-CROSS!!!!

  9. Transition Metals For metals with more than one charge, the charge on the metal ion must be stated. These are typically transition metals. Ex. Iron (II) Chloride Fe2+ Cl-  FeCl2 Ex. Iron (III) Chloride Fe3+ Cl-  FeCl3 Example Write the name of TiO? Find out the charge on the ion that only has one charge. O2- 2. Then evaluate what charge the other ion must have in order to fulfill the formula. Ti must be 2+ Titanium (II) Oxide

  10. Practice Write the formulas for the following compounds: • CuCl2 • CuCl • Cr2O3 • MnO • BeCl2 • NaF Copper (II) Chloride Copper (I) Chloride Chromium (III) Oxide Manganese (II) Oxide Beryllium Chloride Sodium Fluoride

  11. Polyatomic Ions Polyatomic Ions: ions made from more than one element. They stay together when bonding. Example: Lithium Phosphate Li + PO43- Li3PO4 Example: Magnesium Hydroxide Mg2+ OH- Mg(OH)2

  12. Write the Formula for the following Ca(NO3)2 Fe2(SO4)3 CuSO3 KMnO4 Cr(NO3)3 NaClO4 Ca(C2H3O2)2 MgCr2O7 • Calcium Nitrate • Iron (III) Sulfate • Copper (II) Sulfite • Potassium Permanganate • Chromium (III) Nitrate • Sodium Perchlorate • Calcium Acetate • Magnesium Dichromate

  13. Name the following Compounds Magnesium Hydroxide Titanium (III) Chromate Cobalt (III) Phosphate Silver Nitrate Copper (II) Sulfate Beryllium Oxalate Iron (II) Chromate Chromium (III) Phosphate • Mg(OH)2 • Ti2(CrO4)3 • CoPO4 • AgNO3 • CuSO4 • BeC2O4 • FeCrO4 • CrPO4

  14. Chapter 9.3 – Naming Molecular Compounds • the prefix in the name of a binary molecule tells how many atoms of each element are present in each molecule of the compound • Remember that molecules are composed of two nonmetals

  15. Naming Molecular Compounds

  16. Writing Formulas for Binary Molecular Compounds 1st Step: Write the cation 2nd Step: Write the anion with the appropriate prefix Example #1: NCl3 Nitrogen Trichloride Example #2: BCl3 Boron Trichloride Example #3: N2O3 Dinitrogen Trioxide Example #4: N2H4 Dinitrogen Tetrahydride

  17. Practice Sulfur Trioxide Carbon Disulfide Dichlorine Heptaoxide CBr4 P2O3 PCl5 IF7 ClF3 IO2 (1.) SO3 (2.) CS2 (3.) Cl2O7 (4.) Carbon Tetrabromide (5.) Diphosphorus Trioxide (6.) Phosphorus Pentachloride (7.) Iodine Heptafluoride (8.) Chlorine Trifluoride (9.) Iodine Dioxide

  18. Chapter 9.4 – Naming Acids and Bases Acids – compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) Bases – compound that produces hydroxide ions when dissolved in water (OH-)

  19. Rules for Naming Acids (memorize) Rules for naming bases are the same as Ionic Compounds

  20. Practice Nitrous Acid Permanganic Acid Hydrocyanic Acid Hydrosulfuric Acid Lithium Hydroxide Lead (II) Hydroxide Magnesium Hydroxide Aluminum Hydroxide (1.) HNO3 (2.) HMnO4 (3.) HCN (4.) H2S (5.) LiOH (6.) Pb(OH)2 (7.) Mg(OH)2 (8.) Al(OH)3

  21. Homework Section 9.1 – Page 258 #’s 1-9 Section 9.2 – Page 266 #’s 14-19 Section 9.3 – Page 270 #’s 22-25 Section 9.4 – Page 273 #’s 29-33 Chapter 9 Assessment Page 281 #’s 42-61, 65-70, 82, 83

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