1. Chemical Nomenclature and Formulas: What’s in a Name?

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3. Binary Compounds— Writing Chemical formulas 1) Cation, Anion 2) Write oxidation number/charge on each element. 3) Balance charges by the smallest common multiplier between the two elements. Charges must add to 0 for a neutral compound. 4) Add the subscripts for each element in the chemical compound.

4. Example 1: Magnesium bromide

5. Example 2: Aluminum oxide

6. 5) If the first element is a transition element, the oxidation number or charge of the element is given by a Roman numeral (I, II, III, IV, etc.) following the element name. Exceptions: Ag +1 and Zn +2 —they will always have these charges.

7. Example 3: Tin (IV) sulfide

8. Example 2: Mercury (II) fluoride

9. Example 4: Iron (III) oxide

10. Try….. 1)Calcium chloride 2)Copper (I) oxide 3)Sodium bromide 4)Potassium sulfide 5)Calcium oxide

11. Binary Compounds— Writing Chemical formulas (Cont.) 6) If a binary compound has a prefix or prefixes in front of an element name, these prefixes are the subscripts for that element in the chemical formula. Prefixes represent the number of element atoms present in a molecule of the chemical compound.

12. Prefixes 1 mono6 hexa 1 mono6 hexa 2 di7 hepta 2 di7 hepta 3 tri8 octa 3 tri8 octa 4 tetra9 nona 4 tetra9 nona 5 penta10 deca 5 penta10 deca

13. Example 1: Carbon tetrachloride

14. Example 2: Diphosphorus trioxide

15. Polyatomic Chemical Compounds—Writing Chemical Formulas. 1) Cation, Anion—reference table 2) Write the oxidation number/charge on each element and polyatomic ion. 3) Balance charges by the smallest common multiplier between the cation and anion. Charges must add to 0 for a neutral compound. 4) Add the subscripts for each element/polyatomic ion to the chemical compound. *Polyatomic ions: place polyatomic ions in parentheses when adding subscript (ex. (NO 3 ) 2 ) *Polyatomic ions: place polyatomic ions in parentheses when adding subscript (ex. (NO 3 ) 2 )

16. Example 1: Silver nitrate

17. Example 2: Magnesium acetate

18. Example 3: Calcium carbonate

19. Example 4: Ammonium chloride

20. Can we go in reverse?

21. Binary Compounds: Chemical Nomenclature 1) Write an element’s oxidation number over the element symbol. 2) Cation, Anion—write the element name 3) Add the ending -IDE to the second element/anion

22. Example 1: Al 2 S 3

23. Example 2: CaBr 2

24. Transition Elements 4) Place a Roman numeral matching the charge/oxidation # on an element after the positive element’s name. Roman numeral is put in () (ex. (II)). Roman numeral indicates the oxidation number on an element can vary. -Go back to Step #3

25. Example 1: CuS

26. Example 2: CoBr 2

27. 5) If both elements are found on the RIGHT side of the periodic table, use the appropriate prefix for a given element. -Go back to Step #3

28. Example 1: SBr 3

29. Example 2: CCl 4

30. Compounds with Polyatomic Ions: Chemical Nomenclature 1) Write oxidation # for each element/polyatomic ion in the formula 2) Write the element and/or polyatomic ion names. 3) If a transition element (an element where the oxidation # varies), use a Roman numeral to indicate an element’s oxidation # in the chemical name. *NO –IDE ENDING!!!! *NO –IDE ENDING!!!!

31. Example 1: Sr(NO 3 ) 2 Example 1: Sr(NO 3 ) 2

32. Example 2: CuSO 4

33. Homework Test II Study Guide Test II Study Guide