• The rules for naming these compounds:
1. Write the name of the cation.
2. Write the name of the anion.
6.6 aCIdS
• The rules for naming acids can be summarized in the chart that follows:
kEy TERM polyatomic ion
review Questions 115
Acid (begins with H)
Anion contains oxygen
Change anion name to end in -ous acid
Change anion name to end
in -ic acid Check ending on anion
Anion does not contains oxygen
1. Use prefix hydro- and suffix -ic 2. Add word acid
-ite -ate
r e v i e W Q u e s T i o N s
1. List two compounds almost always referred to by their common names. What would be their systematic names?
2. What must happen in order to convert an atom into an anion? Into a cation?
3. Does the fact that two elements combine in a one-to-one atomic ratio mean that the charges on their ions are both 1?
Explain.
4. When naming a binary ionic compound, how do you determine which element to name first?
5. Use the common ion table on the back endpapers of your text to determine the formulas for compounds composed of the following ions:
(a) potassium and sulfide (b) cobalt(II) and bromate (c) ammonium and nitrate (d) hydrogen and phosphate (e) iron(III) oxide
(f) magnesium and hydroxide
6. Explain why P2O5 is named dinitrogen pentoxide, using prefixes, but Al2O3 is named aluminum oxide, without prefixes.
7. Explain why FeCl2 is named iron(II) chloride, using a Roman numeral, and BaCl2 is named barium chloride, using no Roman numeral. Why does neither use prefixes?
8. The names of the nitrogen oxides are nitrogen dioxide (NO2) and dinitrogen monoxide (N2O). Why is the mono- prefix used only on the second molecule?
9. What is the advantage of using the Stock System for naming metals with variable charge instead of using the common name?
10. Write formulas for the compounds formed when a nickel(II) ion is combined with
(a) sulfate (f) acetate (b) phosphide (g) dichromate (c) chromate (h) bromide (d) hydroxide (i) nitrate (e) iodite (j) hypochlorite
(Use the common ion table on the back endpapers of your text.) 11. Write the names and formulas for the four oxy-acids containing
(a) bromine, (b) iodine.
12. How do you differentiate between different anions formed from a polyprotic acid?
116 CHapTer 6 • Nomenclature of Inorganic Compounds
P a i r e d e x e r C i s e s
1. Write the formula of the compound that will be formed between these elements:
(a) Ba and S (d) Mg and N (b) Cs and P (e) Ca and I (c) Li and Br (f) H and Cl 3. Write formulas for the following cations:
(a) potassium (h) calcium (b) ammonium (i) lead(II) (c) copper(I) (j) zinc (d) titanium(IV) (k) silver (e) nickel(III) (l) hydrogen (f) cesium (m) tin(II) (g) mercury(II) (n) iron(III) 5. Write the systematic names for the following:
(a) baking soda (NaHCO3) (d) vinegar (HC2H3O2)
(b) quicksilver (Hg) (e) Epsom salts (MgSO4
#
7 H2O) (c) lime (CaO) (f) lye (NaOH)7. Complete the table, filling in each box with the proper formula.
Anions
8. Complete the table, filling in each box with the proper formula.
Anions
6. Write the systematic names for the following:
(a) hypo (Na2S2O3) (d) table salt (NaCl)
(b) laughing gas (N2O) (e) milk of magnesia (Mg(OH)2) (c) alumina (Al2O3) (f) galena (PbS)
4. Write formulas for the following anions:
(a) fluoride (h) oxide
(b) acetate (i) dichromate (c) iodide (j) hydrogen carbonate (d) carbonate (k) phosphate
(e) sulfide (l) sulfate (f) nitrate (m) nitride (g) phosphide (n) chloride
2. Write the formula of the compound that will be formed between these elements:
(a) Al and S (d) Sr and O
(b) H and F (e) Cs and P (c) K and N (f) Al and Cl
Most of the exercises in this chapter are available for assignment via the online homework management program, WileyPLUS (www.wileyplus.com).
All exercises with blue numbers have answers in Appendix VII.
9. Write the names of each of the compounds formed in Question 7. 10. Write the names of each of the compounds formed in Question 8.
11. Write formulas for each of the following binary compounds, all of which are composed of nonmetals:
(a) diphosphorus pentoxide (e) carbon tetrachloride (b) carbon dioxide (f) dichlorine heptoxide (c) tribromine octoxide (g) boron trifluoride (d) sulfur hexachloride (h) tetranitrogen hexasulfide 13. Name each of the following binary compounds, all of which are
composed of a metal and a nonmetal:
(a) BaO (e) Al2O3
(b) K2S (f) CaBr2
(c) CaCl2 (g) SrI2
(d) Cs2S (h) Mg3N2
15. Name these compounds by the Stock System (IUPAC):
(a) CuCl2 (d) FeCl3
(b) FeCl2 (e) SnF2
(c) Fe(NO3)2 (f) VPO4 17. Write formulas for these acids:
(a) hydrochloric acid (d) carbonic acid (b) chloric acid (e) sulfurous acid (c) nitric acid (f) phosphoric acid
12. Write formulas for each of the following binary compounds, all of which are composed of a metal and nonmetal:
(a) potassium nitride (e) calcium nitride (b) barium oxide (f) cesium bromide (c) iron(II) oxide (g) manganese(III) iodide (d) strontium phosphide (h) sodium selenide
14. Name each of the following binary compounds, all of which are composed of nonmetals:
(a) PBr5 (e) SiCl4
(b) I4O9 (f) ClO2
(c) N2S5 (g) P4S7
(d) S2F10 (h) IF6
16. Write formulas for these compounds:
(a) tin(IV) bromide (d) mercury(II) nitrite (b) copper(I) sulfate (e) cobalt(III) carbonate (c) nickel(II) borate (f) iron(II) acetate 18. Write formulas for these acids:
(a) acetic acid (d) boric acid (b) hydrofluoric acid (e) nitrous acid (c) hydrosulfuric acid (f) hypochlorous acid
3– 21. Write formulas for these compounds:
(a) silver sulfite (m) potassium dichromate
(n) bismuth(III) chromate 23. Write the name of each compound:
(a) ZnSO4 (f) CoF2
(b) Hg2S (g) Cr(ClO3)3 (c) CuCO3 (h) Ag3PO4 (d) Cd(NO3)2 (i) MnS (e) Al(C2H3O2)3 (j) BaCrO4
25. Write the chemical formulas for these substances:
(a) slaked lime (e) cane sugar (b) fool’s gold (f) borax (c) washing soda (g) wood alcohol (d) calcite (h) acetylene
26. Write the chemical formulas for these substances:
(a) grain alcohol (e) muriatic acid (b) cream of tartar (f) plaster of paris
(c) gypsum (g) lye
(d) brimstone (h) laughing gas 24. Write the name of each compound:
(a) Ca(HSO4)2 (f) BiAsO4 (b) As2(SO3)3 (g) (NH4)2CO3 (c) Sn(NO2)2 (h) (NH4)2HPO4
(d) CuI (i) NaClO
(e) KHCO3 (j) KMnO4
22. Write formulas for these compounds:
(a) sodium chromate (b) magnesium hydride (c) nickel(II) acetate (d) calcium chlorate (e) magnesium bromate
(f) potassium dihydrogen phosphate (g) manganese(II) hydroxide
Additional exercises 117
a d d i T i o N a l e x e r C i s e s
27. Write equations similar to those found in Section 6.2 for the forma-tion of
(a) potassium ion (d) iron(II) ion (b) iodide ion (e) calcium ion (c) bromide ion (f) oxide ion 28. Name each of the following polyatomic ions:
(a) (d)
(b) (e)
(c) (f)
29. Write formulas for all possible compounds formed between the calcium ion and the anions shown in Question 28.
30. Write formulas for all possible compounds formed between the potassium ion and the anions shown in Question 28.
31. Write the formula and name for each of the following compounds:
(a)
118 chapter 6 • Nomenclature of Inorganic Compounds
32. Write the formula and name for the following compound:
33. State how each of the following is used in naming inorganic com-pounds: ide, ous, ic, hypo, per, ite, ate, Roman numerals.
34. Several excerpts from newspaper articles follow. Tell the chemi-cal formula of the chemichemi-cal spilled and indicate whether this spill should raise concern in the local area.
(a) A mistake at the Columbia Water and Light Department’s West Ash Street pumping station sent an estimated 7200 gallons of calcium-carbonate-laden water into Harmony Creek early yes-terday, forcing crews to spend hours cleaning up the mess.
(b) A tanker truck carrying 6000 gallons of acetic acid overturned on the I-5 freeway in San Diego, California.
(c) A university in New Hampshire was discovered dumping dihy-drogen oxide into the local sewer system.
35. How many of each type of subatomic particle (protons and elec-trons) is in
(a) an atom of tin?
(b) a Sn2+ ion?
(c) a Sn4+ ion?
36. The compound X2Y3 is a stable solid. What ionic charge do you expect for X and Y? Explain.
37. The ferricyanide ion has the formula Fe(CN)36-. Write the formula for the compounds that ferricyanide would form with the cations of elements 3, 13, and 30.
38. Compare and contrast the formulas of (a) nitride with nitrite
(b) nitrite with nitrate
(c) nitrous acid with nitric acid
K+ Cl–
C H A L L E N G E E x E r C i s E
39. After studying chemistry, you should be able to recognize more of the substances listed on consumer products. A list of ingredients for dog food follows:
Chicken By-Product Meal (Natural source of Chondroitin Sulfate and Glucosamine), Corn Meal, Ground Whole Grain Sorghum, Ground Whole Grain Barley, Fish Meal (source of fish oil), Chicken, Chicken Fat (preserved with mixed Tocopherols, a source of Vitamin E), Dried Beet Pulp, Chicken Flavor, Dried Egg Product, Potassium Chloride, Brewers Dried Yeast, Salt, So-dium Hexametaphosphate, Fructooligosaccharides, Fish Oil (pre-served with mixed Tocopherols, a source of Vitamin E), Calcium Carbonate, Flax Meal, Choline Chloride, Minerals (Ferrous Sul-fate, Zinc Oxide, Manganese SulSul-fate, Copper SulSul-fate, Manganous Oxide, Potassium Iodide, Cobalt Carbonate), Vitamin E Supple-ment, Dried Chicken Cartilage (Natural source of Chondroitin Sulfate and Glucosamine), DL-Methionine, Vitamins (Ascorbic
Acid, Vitamin A Acetate, Calcium Pantothenate, Biotin, Thiamine Mononitrate (source of Vitamin B1), Vitamin B12 Supplement, Niacin, Riboflavin Supplement (source of Vitamin B2), Inositol, Pyridoxine Hydrochloride (source of Vitamin B6), Vitamin D3 Supplement, Folic Acid), Beta-Carotene, L-Carnitine, Marigold, Citric Acid, Rosemary Extract.
Many of the substances in this bag of dog food are ionic com-pounds that you should be able to recognize. The manufacturers of this dog food did not completely identify some of the compounds.
Write the chemical formula of the following compounds found in this ingredient list.
(a) potassium chloride (f) copper sulfate (b) calcium carbonate (g) manganous oxide (c) ferrous sulfate (h) potassium iodide (d) zinc oxide (i) cobalt carbonate (e) manganese sulfate (j) sodium chloride
A N s w E r s t o P r A C t i C E E x E r C i s E s
6.1 phosphorus stem is phosph- 1 -ide 5 phosphide; nitrogen stem is nitr- 1 -ide 5 nitride; boron stem is bor- 1 -ide 5 boride;
carbon stem is carb- 1 -ide 5 carbide
6.2 (a) KF; (b) CaBr2; (c) Mg3N2; (d) Na2S; (e) BaO; (f) As2(CO3)5 6.3 (a) SrCl2; (b) KI; (c) AlN; (d) CaS; (e) Na2O
6.4 (a) lead(II) iodide; (b) tin(IV) fluoride; (c) iron(III) oxide;
(d) copper(II) oxide
6.5 (a) Sn(CrO4)2; (b) CrBr3; (c) SnF2; (d) Cu2O
6.6 (a) dichlorine monoxide; (b) sulfur dioxide; (c) carbon tetra-bromide; (d) dinitrogen pentoxide; (e) ammonia; (f) iodine trichloride
6.7 (a) potassium bromide; (b) calcium nitride;
(c) sulfur trioxide; (d) tin(II) fluoride; (e) copper(II) chloride;
(f) dinitrogen tetroxide
6.8 (a) sodium nitrate; (b) calcium phosphate; (c) potassium hydroxide; (d) lithium carbonate; (e) sodium chlorate
6.9 (a) potassium hydrogen carbonate; (b) sodium hydrogen oxa-late; (c) barium ammonium phosphate; (d) sodium aluminum sulfate
6.10 (a) hydrochloric acid; (b) hydrobromic acid 6.11 (a) carbonic acid; (b) acetic acid; (c) nitric acid;
(d) nitrous acid