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 9/25 Inorganic Nomenclature worksheet Inorganic Nomenclature worksheet Read over lab procedure for Thursday Read over lab procedure for Thursday Liquid Chromatography Lab due Thursday Liquid Chromatography Lab due Thursday Study for Element/Polyatomic quiz next Tuesday, October 3rd Study for Element/Polyatomic quiz next Tuesday, October 3rd