1. WRITING FORMULAS AND NAMING COMPOUNDS

2. Binary Compounds  Made up of only 2 elements  Two types of Binary Compounds 1. Ionic Compounds- metal and nonmetal Ex: NaCl, MgBr 2, K 2 O 2. Covalent Compounds- 2 nonmetals Ex: CO 2, H 2 O, SO 3

3. Ionic or Covalent? 1. NO 2 covalent 2. P 2 O 4 covalent 3. Fe 2 O 3 ionic 4. CaF 2 ionic

4. Covalent Compounds NAMING A. Use prefixes to indicate the number of atoms of each element mono-1 hexa-6 di-2 hepta-7 tri-3 octa-8 tetra-4 nona-9 penta-5 deca-10

5. B. Name the first element. If you have only one atom of the first element, do NOT use the prefix mono. C. Name the second element with prefixes. Change the ending to “ide”.

6. Name the following: 1. CO 2 carbon dioxide 2. SO 3 sulfur trioxide 3. N 2 O 4 dinitrogen tetroxide 4. CCl 4 carbon tetrachloride 5. H 2 O dihydrogen monoxide

7. Write the formula 1. phosphorus trichloride PCl 3 2. nitrogen dioxide NO 2 3. sulfur hexabromide SBr 6 4. diphosphorus pentoxide P 2 O 5

8. Ionic Compounds NAMING A. Name the first element (metal) B. Name the second element (nonmetal) and change the ending to “ide” C. NO PREFIXES!!!

9. Name the following: 1. NaCl sodium chloride 2. CaF 2 calcium fluoride 3. Ag 2 O silver oxide 4. AlBr 3 aluminum bromide 5. ZnS zinc sulfide

10. Writing Formulas Ionic compounds are composed of a positive ion called a cation and a negative ion called an anion. A. Write the metal ion first. (+ ion: cation) B. Write the nonmetal last. (- ion: anion) C. Balance the charges! Charges must add up to zero to form a neutral compound.

11. How to determine the charge You can look at the position of the element on the periodic table to determine the charge of the element when it forms an ion. There is a difference between a neutral element (K) and an ion (K + ).

12. Using the Periodic Table

13. Writing Formulas 1. sodium chloride Na + Cl - NaCl 2. calcium chloride Ca +2 Cl - Cl - CaCl 2

14. Writing Formulas 3. aluminum chloride Al +3 Cl - Cl - AlCl 3

15. Writing Formulas 4. potassium bromide K + Br - KBr 5. potassium oxide K + O -2 K + K 2 O

16. Writing Formulas 6. aluminum oxide Al +3 O -2 O -2 Al 2 O 3

17. Review  Covalent compounds are made up of nonmetals only.  Use prefixes in the names of covalent compounds.  Covalent compounds do not have charges!  Ionic compounds are made up of a metal and a nonmetal.  Balance the charges when you write a formula for ionic compounds.  Never use prefixes in the names of ionic compounds!

18. Ionic Compounds with Roman Numerals  The roman numeral gives the charge of the metal ion.  Ex: Fe(II) Fe+2 Fe(III) Fe+3  Transition metals need roman numerals in the name.  Pb and Sn need roman numerals because they have charges of +2 and +4.  Ag and Zn do NOT need roman numerals because Ag is always +1 and Zn is always +2.

19. Write the Formula 1. nickel (II) bromide NiBr 2 2. lead (IV) oxide PbO 2 3. iron (III) sulfide Fe 2 S 3

20. Name the following 1. CrCl 3 chromium (III) chloride 2. FeO iron (II) oxide 3. SnCl 4 tin (IV) chloride 4. Cu 2 O copper (I) oxide

21. Review: Write the Formula 1. strontium fluoride 2. chromium (III) oxide 3. sulfur hexabromide 4. iron (III) sulfide 5. carbon disulfide 1. SrF 2 2. Cr 2 O 3 3. SBr 6 4. Fe 2 S 3 5. CS 2

22. Review: Name the following. 1. K 2 Se 2. CaI 2 3. NiCl 2 4. PCl 3 5. BaNa 2 1. potassium selenide 2. calcium iodide 3. nickel (II) chloride 4. phosphorus trichloride 5. banana

23. Compounds with Polyatomic Ions Naming  Name the metal  Name the polyatomic ion  Use roman numeral if needed

24. Naming 1. MgCO 3 magnesium carbonate 2. Na 2 SO 4 sodium sulfate 3. Cu(OH) 2 copper (II) hydroxide 4. Zn(C 2 H 3 O 2 ) 2 zinc acetate

25. Write the Formula: 1. aluminum nitrate Al(NO 3 ) 3 2. ammonium sulfite (NH 4 ) 2 SO 3 3. iron (III) chlorate Fe(ClO 3 ) 3 4. calcium phosphate Ca 3 (PO 4 ) 2