Chemical Names and Formulas

1. Chemical Names and Formulas Chapter 9

2. Essential Questions • How does the periodic table help you determine the names and formulas of ion and compounds? • What is the difference between an ionic and molecular formula?

3. How do we determine the charges of monatomic ions? • Monotomic ions are the simplest ions • They eithercationsoranions • Positive, metals, give away electrons to obtain the configuration of a noble gas state. • Negative, nonmetals, take electrons to obtain the configuration of a noble gas.

4. Naming Monotomic Ions • Metals are named using the name of the metal and the charge • Na+, Ca+2, Al3+ • Anions • Start with the stem of the element and end in ide • Oxide, Sulfide, Nitride

5. Naming Monotomic Ions • Some metals form more than one ion • Transition metals 1B-8B • Two ways used to name these metals • Stock method • Fe2+ • Iron(II) • Fe3+ • Iron(III)

6. Naming Monotomic Ions • Classical System • The classical name of the element is used to form the root • Ferrous ion, Ferric ion • List the symbols and names of common metal ions with more than one charge. Make flash cards for memorization (HW)

7. Practice • Write the symbol, including the charge for the ion formed by each element; classify each as anion or cation; then write the name of each ion. • Arsenic • Beryllium • Fluorine • Gallium • Sodium

8. As3-; anion; arsenide ion • Be2+; cation; beryllium ion • F-; anion; fluoride ion • Ga3+; cation; gallium • Na+; cationsodium ion

9. Polyatomic Ions • polyatomic ions

10. Naming Ionic Compounds • Writing ionic formulas

11. Writing the Formulas for Ionic Compounds • Practice problem 9.2 pg 246

12. Naming Binary Ionic Compounds • If you know the formula, you can write its name • Place the cation name first and the anion name second • For compounds with elements that form only one ion, it is straight forward as in NaBr • For compounds with elements that form more than one ion, the name of the metal must be . SnF2, SnO2 • Sample Problem 9.3 pg 249

13. Practice • Write the names of these binary compounds • Li2O • MgS • MnCl3 • FeO • CaI2

14. Lithium oxide • Magnesium sulfide • Manganes(III) chloride • Iron(II) oxide • Calcium iodide

15. Compounds with Polyatomic Ions • The procedure is similar to binary compounds • Write the symbol (or formula) for the cation • Write the symbol (or formula) for the anion • Add subscripts as needed to balance the charges • Use which ever method you are comfortable with • Use parenthesis when more than one polyatomic ion is necessary to balance charges • Sample problem 9.4 pg 251

16. Naming Compounds with Polyatomic Ions • First write the cation name • If the cation has than one charge, use a roman numeral in the cation name • Identify the polyatomic ions and write that in the name • Sample problem 9.5 pg 253

17. Practice • Name the following compounds • Na2CO3 • Pb(OH)2 • FeN • NH4NO3 • Mg(NO3)2

18. Naming and Writing Formulas for Molecular Compounds • Write the of the elements in the order listed in the formula • Use prefixes to indicate the number of each kind of atom. You do not have to use mono. The vowel at the end of a prefix is dropped if the element begins with a vowel • End the name with the suffix ide • Memorize the chart of prefixes on page 257 • Practice problems 9.6 pg 258

19. Naming and Writing Formulas for Molecular Compounds • Writing formulas for Binary Molecular Compounds • Use the prefixes to determine the subscript • Write the correct symbols for each element with the appropriate subscripts

20. Naming and writing formulas for acids and bases • Naming Acids • The general formula for an acid is HnX • n is the number of hydrogen ions combined with the anion • The naming depends on the anion (X) • If the anion ends in ide, the prefix is hydro, the anion has the suffix ic hydrochloric acid • If the anion ends in ite, the stem ends in oussulfuous acid • If the anion ends in ate, the stem ends in icnitric acid • Chart pg 260