Exercises 173magnesium metal, (b) barium nitrate and sodium phos-
phate solutions, (c) calcium acetate solution with
aluminum metal, (d) silver nitrate and sodium iodide
solutions.
103.Predict whether or not a solid is formed when we mix the
following; identify any solid product by formula and by
name: (a) potassium permanganate and sodium phosphate
solutions, (b) lithium carbonate and cadmium nitrate,
(c) stannous fluoride and bismuth chloride, (d) strontium
sulfate with barium chloride solutions.Naming Compounds
104.Name the following monatomic cations, using the IUPAC
system of nomenclature: (a) Li, (b) Au^3 , (c) Ca^2 ,
(d) Zn^2 , (e) Ag.
105.Write the chemical symbol for each of the following:
(a) sodium ion, (b) lead(II) ion, (c) silver ion, (d) mer-
cury(II) ion, (e) bismuth(III) ion.
106.Write the chemical formula for each of the following:
(a) chloride ion, (b) sulfide ion, (c) telluride ion, (d) oxide
ion, (e) nitrite ion.
107.Name the following ionic compounds: (a) K 2 S, (b) SnO 2 ,
(c) RbBr, (d) Li 2 O, (e) Ba 3 N 2.
108.Name the following ionic compounds: (a) CuI 2 , (b) Hg 2 S,
(c) Li 3 N, (d) MnCl 2 , (e) CuCO 3 , (f ) FeO.
109.Write the chemical formula for each of the following com-
pounds: (a) sodium fluoride, (b) zinc oxide, (c) barium
oxide, (d) magnesium bromide, (e) hydrogen cyanide,
(f ) copper(I) chloride.
110.Write the chemical formula for each of the following
compounds: (a) copper(II) chlorate, (b) potassium nitrite,
(c) barium phosphate, (d) copper(I) sulfate, (e) sodium sul-
fite.
111.What is the name of the acid with the formula H 2 CO 3?
Write the formulas of the two anions derived from it and
name these ions.
112.What is the name of the acid with the formula H 3 PO 3?
What is the name of the HPO 32 ion?
113.Name the following binary molecular compounds: (a) NO,
(b) CO 2 , (c) SF 6 , (d) SiCl 4 , (e) IF.
114.Name the following binary molecular compounds: (a)
AsF 3 , (b) Br 2 O, (c) BrF 5 , (d) CSe 2 , (e) Cl 2 O 7.
115.Write the chemical formula for each of the following
compounds: (a) iodine bromide, (b) silicon dioxide,
(c) phosphorus trichloride, (d) tetrasulfur dinitride,
(e) bromine trifluoride, (f ) hydrogen telluride, (g) xenon
tetrafluoride.
116.Write the chemical formula for each of the following com-
pounds: (a) diboron trioxide, (b) dinitrogen pentasulfide,
(c) phosphorus triiodide, (d) sulfur tetrachloride, (e) sili-
con sulfide, (f ) hydrogen sulfide, (g) tetraphosphorus
hexoxide.
117.Write formulas for the compounds that are expected to be
formed by the following pairs of ions:118.Write the names for the compounds of Exercise 117.
119.Write balanced chemical equations for each of the fol-
lowing processes: (a) Calcium phosphate reacts with
sulfuric acid to produce calcium sulfate and phosphoric
acid. (b) Calcium phosphate reacts with water containing
dissolved carbon dioxide to produce calcium hydrogen car-
bonate and calcium hydrogen phosphate.
120.Write balanced chemical equations for each of the fol-
lowing processes: (a) When heated, nitrogen and oxygen
combine to form nitrogen oxide. (b) Heating a mixture of
lead(II) sulfide and lead(II) sulfate produces metallic lead
and sulfur dioxide.CONCEPTUAL EXERCISESAs we have seen, two substances may react to form different
products when they are mixed in different proportions under
different conditions. In Exercises 121 and 122, write balanced
equations for the reactions described by words. Assign oxidation
numbers.
121.(a) Ethane burns in excess air to form carbon dioxide and
water.
(b) Ethane burns in a limited amount of air to form car-
bon monoxide and water.
(c) Ethane burns (poorly) in a very limited amount of air
to form elemental carbon and water.
122.(a) Butane (C 4 H 10 ) burns in excess air to form carbon
dioxide and water.
(b) Butane burns in a limited amount of air to form car-
bon monoxide and water.
(c) When heated in the presence of very littleair, butane
“cracks” to form acetylene, C 2 H 2 , carbon monoxide,
and hydrogen.
123.Use the general metallic trend of the periodic table to pre-
dict which element in each of the following pairs is more- NH 4
A. Cl B. OH
Omit –
see noteC. SO 42 D. PO 43 E. NO 3
- Na
3. Mg^2
4. Ni^2
5. Fe^3
6. Ag
NOTE: The compound NH 4 OH does not exist. The solution
commonly labeled “NH 4 OH” is aqueous ammonia, NH 3 (aq).