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

Chemical Nomenclature and Formulas: What’s in a Name?. LOL ASAP FYI BRB. Binary Compounds—Writing Chemical formulas. 1) Cation , Anion 2) Write oxidation number/charge on each element.

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

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

  2. LOL ASAP FYI BRB

  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….. • Calcium chloride • Copper (I) oxide • Sodium bromide • Potassium sulfide • 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 mono 6 hexa • 2 di 7 hepta • 3 tri 8 octa • 4 tetra 9 nona • 5 penta 10 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. (NO3)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: Al2S3

  23. Example 2: CaBr2

  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: CoBr2

  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: SBr3

  29. Example 2: CCl4

  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!!!!

  31. Example 1: Sr(NO3)2

  32. Example 2: CuSO4

  33. Homework • Test II Study Guide

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