(a)
Interpretation:
The chemical formula for the ternary compound, lead
Concept introduction:
Compounds containing a metal and more than one other element are termed as ternary ionic compounds. The charge on the ternary ionic compounds must always be neutral, no matter what the charges on the individual ions are.
Answer to Problem 20E
The chemical formula for the ternary compound, lead
Explanation of Solution
The ternary compound, lead
The chemical formula for the ternary compound, lead
(b)
Interpretation:
The chemical formula for the ternary compound, tin
Concept introduction:
Compounds containing a metal and more than one other element are termed as ternary ionic compounds. The charge on the ternary ionic compounds must always be neutral, no matter what the charges on the individual ions are.
Answer to Problem 20E
The chemical formula for the ternary compound, tin
Explanation of Solution
The ternary compound, tin
The chemical formula for the ternary compound, tin
(c)
Interpretation:
The chemical formula for the ternary compound, cobalt
Concept introduction:
Compounds containing a metal and more than one other element are termed as ternary ionic compounds. The charge on the ternary ionic compounds must always be neutral, no matter what the charges on the individual ions are.
Answer to Problem 20E
The chemical formula for the ternary compound, cobalt
Explanation of Solution
The ternary compound, cobalt
The chemical formula for the ternary compound, cobalt
(d)
Interpretation:
The chemical formula for the ternary compound, mercury
Concept introduction:
Compounds containing a metal and more than one other element are termed as ternary ionic compounds. The charge on the ternary ionic compounds must always be neutral, no matter what the charges on the individual ions are.
Answer to Problem 20E
The chemical formula for the ternary compound, mercury
Explanation of Solution
The ternary compound, mercury
The chemical formula for the ternary compound, mercury
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Chapter 6 Solutions
Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
- Consider the nickel salt: (NH4 )2Ni(SO4 )2 ·y H2O (Ammonium Nickel Sulfate Hydrate), where y is the number of coordinated waters. The actual yield of product was 9.640 g - obviously containing coordinated water. The product was then heated strongly until all the water had been driven off. The resulting anhydrous salt had mass 7.000 g. What is the value of y?arrow_forwardWrite the empirical formula of the compound formed by (a) Al3+ and Cl- ions, (b) Al3+ and O2 - ions, (c) Mg2+ and NO3- ions.arrow_forward1) A sample of blue crystals of copper (II) sulfate pentahydrate was heated to produce the copper(Il)sulfate tetrahydrate. (a) Write the chemical formulas of the copper(II)sulfate pentahydrate and copper(II)sulfate tetrahydrate. (b) Calculate mass percent of water in copper(II)sulfate pentahydrate (c) If 7.491 g of the copper (II) sulfate pentahydrate produces 6.951 g of the copper (II) sulfate tetrahydrate, how many grams of anhydrous copper(I1)sulfate could be obtained? (Cu=63.5 g/mol, S=32.0 g/mol, O=16.0 g/mol, H=1 g/mol)arrow_forward
- Write the balanced chemical equation for the following and identify the type of reaction in each case.(a) Potassium bromide (s) + Barium iodide (aq) Potassium iodide (aq) + Barium bromide(s)(b) Zinc carbonate (s) Zinc oxide (s) + Carbon dioxide (g)(c) Hydrogen (g) + Chlorine (g) Hydrogen chloride (g)(d) Magnesium (s) + Hydrochloric acid (aq) Magnesium chloride (aq) + Hydrogen (g)arrow_forwardFor many years the recovery of gold—that is, the separation of gold from other materials—involved the use of potassium cyanide: Au + KCN + O2 + H2O à KAu(CN)2 + KOH (a) Balance the above chemical equation. (b) What is the minimum amount of potassium cyanide in grams needed to extract 29.0 g (about an ounce) of gold?arrow_forwardWrite balanced equations for the following reactions: (a) Hydrochloric acid reacts with calcium carbonate to form carbon dioxide and calcium chloride and water.(b) Liquid bromine reacts with solid potassium metal to form solid potassium bromide.(c) Gaseous propane 1C3H82 burns in oxygen to form gaseous carbon dioxide and water vapor.arrow_forward
- With the advent of techniques such as scanning tunneling microscopy, it is now possible to “write” with individual atoms by manipulating and arranging atoms on an atomic surface.(A) If the image is prepared on a platinum surface that is exactly 20 platinum atoms high and 14 platinum atoms wide, what is the mass (grams) of the atomic surface? Show all work. [2](B) If the atomic surface were changed to ruthenium atoms and the same surface mass as determined in part (B) is used, what number of ruthenium atoms is needed to construct the surface? Show all work. [2]arrow_forwardWhich is correct and which is incorrect from the following sentences? Proposition True False (a) The nitrogen ions N + and oxygen O + are products of the decay of the corresponding molecules under the influence of sunlight near the earth's surface. (b) Red phosphorus is more active than white phosphorus and is therefore used in the manufacture of matches. (c) The oxidation number (a.o.) of nitrogen in all chemicals NO, NO + and NO- is +2. (d) Of the elements Al, Cl2, Na, Mg and Ca, only Na reacts with cold water to produce H2. (e) Of the two common carbon oxides, monoxide is less acidic.arrow_forwardQ4(B) Define mass number. Explain the following redox reactions.arrow_forward
- Write balanced equations for each of the following reactions.(a) When mercury(II) oxide is heated, it decomposesto form O2 and mercury metal. (b) When copper(II) nitrateis heated strongly, it decomposes to form copper(II) oxide,nitrogen dioxide, and oxygen. (c) Lead(II) sulfide, PbS(s),reacts with ozone to form PbSO4(s) and O2(g). (d) Whenheated in air, ZnS(s) is converted to ZnO. (e) Potassiumperoxide reacts with CO2(g) to give potassium carbonateand O2. (f) Oxygen is converted to ozone in the upperatmosphere.arrow_forwardwrite a balanced chemical equation for each (A) Iron (III) chloride reacts with sodium hydroxide to produce iron (III) hydroxide and sodium chloride. (B) Magnesium nitrite reacts with perchloric acid to produce magnesium perchlorate and nitrous acid. (C) Copper(II) hydroxide reacts with hydrosulfuric acid to produce copper (II) sulfide and water.arrow_forwardWrite the balanced chemical equation for the reaction of these pairs of reactants: (a) Calcium and bromine (b) Aluminum and oxygenarrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax