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

This guide covers writing chemical formulas easily, including steps for binary compounds, transition elements, and compounds with polyatomic ions. It explains how to determine oxidation numbers, balance charges, and use prefixes correctly. Examples provided for clarity.

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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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