Worksheet 5 Nomenclature 1 Ionic Compounds I. Naming compounds containing only two elements (binary compounds)

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Egbert Hines
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1 Worksheet 5 Nomenclature 1 Ionic Compounds I. Naming compounds containing only two elements (binary compounds) 1. Name the first element. 2. Name the second element with an ide ending Example: NaCl A1 2 O 3 sodium chloride aluminum oxide Symbol Binary Name Symbol Binary Name Br Bromide I Iodide C 4 Carbide N 3 Nitride C1 Chloride O 2 Oxide F Fluoride P 3 Phosphide H Hydride S 2 Sulfide Exercise: Name the following binary compounds: 1. A1 4 C 3 6. BaC HF (g) 7. MgO 3. ZnS 8. KI 4. A1 2 S 3 9. Ag 2 S 5. Ca 3 P LiH

2 II. Assigning oxidation numbers (electron bookkeeping rules): 1. Oxidation number of atoms in elemental form is zero. 2. Oxidation number of monatomic ion equals charge of ion. 3. H = +1 in most compounds; 0 = 2 in most compounds. 4. Li group = +1, Be Group = +2, B Group = +3 in their compounds. 5. N Group = 3, O Group = 2, F Group = 1 in binary compounds in which they are the negative element 6. The sum of oxidation numbers of all atoms in a compound is zero. Example: Fe 2 S 3 Rule 3 says S = 2; there is no rule for Fe, so apply Rule 6 2Fe + 3S = 0 2Fe + 3(2) = 0 2Fe6 = 0 2Fe = +6 Fe = +3 Exercise: Assign oxidation numbers to the underlined element in each of the following compounds. Remember an oxidation number is for one atom of the element. 1. FeO 6. Cu 2 O 2. A1 4 C 3 7. SnBr 4 3. CuI 8. PbO 2 4. FeBr 3 9. Hg 2 C CoC Cr 2 O 3

3 III. Naming binary compounds containing a metal and a nonmetal 1. Name first element, then name second element with ide ending. If first element is a metal check its possible oxidation states on your periodic table. If more than one oxidation number is listed, put proper oxidation number in Roman numerals in parentheses after the name of the metal. Example: CuBr 2 copper (II) bromide CuBr copper (I) bromide Exercise: Name the following compounds. Include oxidation state if metal has more than one possible oxidation number 1. AuC Cr 2 O 3 2. CdS 7. HgC BaBr 2 8. Cu 2 O 4. Fe 2 O 3 9. Ag 2 S 5. K 2 O 10. PbC1 2

4 Worksheet 6 Nomenclature 2 Covalent compounds, Binary Acids I. Naming binary containing only two nonmetals(covalent compounds) Basic rule: Name of first element plus name of second element with "ide." Use the prefixes below to indicate the number of atoms of each element present. Number Prefix Number Prefix 1 mono* 6 hexa 2 di 7 hepta 3 tri 8 octa 4 tetra 9 nona 5 penta 10 deca Note*: the prefix mono is often omitted from the first element. Example: CO carbon monoxide CO 2 carbon dioxide N 2 O 5 dinitrogen pentoxide Exercise: Name the following compounds: 1. OF 2 4. SF 6 2. XeF 2 5. NO 2 3. SO 3 _ 6. KrF 4

5 II. Naming binary compounds starting with hydrogen.(acids) These are often named as acids. they are named hydro ic acid with the blank containing the element other than H. Example: HF(g) hydrogen fluoride HF(aq) hydrofluoric acid Note: This compound can also be named hydrogen fluoride. Usually HF is called hydrofluoric acid when it is dissolved in water(aq) and hydrogen fluoride when it is a gas (g). Exercise: Name the following binary compounds: Next to the name classify each as Ionic (I), Ionic Acid (IA), or covalent (C). 1. BF NaF 2. KC1 12. HBr(aq) 3. NiO 13. SiO 2 4. HCl(aq) 14. CaF 2 5. HCl (g) 15. A1N 6. CaO 16. H 2 S(g) 7. PbS 17. Li 2 O 8. FeC N 2 O 9. Cr 2 S CrF NiBr H 2 O

6 Worksheet 7 Nomenclature 3 Ionic Ternary Compounds Polyatomic ions The following is a partial list of polyatomic ions. These compounds are made up of more than one type of atom but act as a single ion. Compounds with three or more elements: Memorize the following polyatomic ions. Learn the name, formula, and charge: Acetate, C 2 H 3 O 2 Chromate, CrO 4 2 Hydroxide, OH Permanganate, MnO 4 Sulfate, SO 4 2 Sulfite, SO 3 2 Ammonium, NH 4 + Chlorate, C1O 3 Chlorite Iodate, IO 3 3 Phosphate, PO 4 3 Phosphite, PO 3 Hydrogen sulfate, HSO 4 Carbonate, CO 3 2 ClO 2 Cyanide, CN Nitrate, NO 3 Monohydrogen Nitrite, NO 2 Phosphate, HPO 4 2 Bicarbonate or Hydrogen carbonate, HCO 3 Dichromate, Cr 2 CO 7 Dihydrogen phosphate, H 2 PO 4 Look at sulfate and sulfite: How are the formulas the same and how are they different? Look at nitrate and nitrite: How are the formulas the same and how are they different? If you memorized the ate ions how would you remember the ite ions?

7 To name ternary ionic compounds: recognize the compound is ionic, name the cation and give it a roman numeral if it needs one. Find the polyatomic ion and name it. Put the two together as follows:: 1. Cu (NO 3 ) 2 cooper (II) nitrate Remember copper needs a roman numeral 2. K 2 SO 4 potassium sulfate 3. (NH 4 ) 3 PO 4 ammonium phosphate Ammonium is the only polyatomic cation Name the following compounds with 3 or more elements. Look for the polyatomic ions that you memorized last week. Follow the rule for binary compounds unless a polytomic ion appears; then use its name Exercise: 1. K 2 CrO NaH 2 PO 4 2. CuSO Zn(C 2 H 3 O 2 ) 2 3. (NH 4 ) 2 Cr 2 O NaHCO 3 4. Mg(OH) Cu(C1O 3 ) 2 5. Pb(NO 3 ) BaSO 4 6. Na 3 PO AgIO 3 7. KMnO SO 2 8. NH 4 C1 18. NaOH 9. KCN 19. Fe(NO 3 ) CaCO NiS

8 Worksheet 8 Nomenclature 4 When enough H + s are added to one of the polyatomic ate ions to make it electrically neutral, an ic acid results. Example: C 2 H 3 O 2 acetate SO 4 2 Sulfate HC 2 H 3 O 2 acetic acid H 2 SO 4 sulfuric acid H + s are added to a polyatomic ite ion to make it electrically neutral and form an ous acid. Example: ClO 2 Chlorite HClO 2 chlorous acid Fill in the following table: Polyatomic ion formula NO 3 Polyatomic ion name Acid formula Acid name chromate H 2 SO 3 Phosphoric acid Nitrous acid H 2 CO 3 iodate

9 Nomenclature worksheet 8 Name Exercise: Name the following compounds 1. KNO CaC 2 2. HBr (gas) 12. ZnCO 3 3. KrF H 3 PO 4 4. PbSO HC1 (aq) 5. (NH 4 ) 2 S 15. HNO 3 6. Hg 2 C SnC H 2 SO Na 2 Cr 2 O 7 8. Ag 2 CrO Cu 2 S 9. CsOH 19. Fe 3 (PO 4 ) P 2 O A1(OH) 3

Experiment #4. Chemical Nomenclature

Experiment #4. Chemical Nomenclature Many everyday and historically important chemical compounds have common names. For example, water is the common name for H 2 O, baking soda is the common name for NaHCO