Introductory Chemistry: A Foundation - Zumdahl S.S., DeCoste D.J. 2019

Nomenclature
Chapter Review

Key Terms

· binary compound (5.1)

· binary ionic compound (5.2)

· polyatomic ion (5.5)

· oxyanion (5.5)

· acid (5.6)

For Review

· Binary compounds are named by following a set of rules.

o For compounds containing both a metal and a nonmetal, the metal is always named first. The nonmetal is named from the root element name.

o If the metal ion can have more than one charge (Type II), a Roman numeral is used to specify the charge.

o For binary compounds containing only nonmetals (Type III), prefixes are used to specify the numbers of atoms present.

· Polyatomic ions are charged entities composed of several atoms bound together. They have special names and must be memorized.

· Naming ionic compounds containing polyatomic ions follows rules similar to those for naming binary compounds.

· The names of acids (molecules with one or more ions attached to an anion) depend on whether the acid contains oxygen.

Active Learning Questions

These questions are designed to be considered by groups of students in class. Often these questions work well for introducing a particular topic in class.

· 1.

In some cases the Roman numeral in a name is the same as a subscript in the formula, and in some cases it is not. Provide an example (formula and name) for each of these cases. Explain why the Roman numeral is not necessarily the same as the subscript.

· 2.

The formulas and look very similar. What is the name for each compound? Why do we name them differently?

· 3.

The formulas and look very similar. What is the name for each compound? Why do we name them differently?

· 4.

Explain how to use the periodic table to determine that there are two chloride ions for every magnesium ion in magnesium chloride and one chloride ion for every sodium ion in sodium chloride. Then write the formulas for calcium oxide and potassium oxide and explain how you got them.

· 5.

What is the general formula for an ionic compound formed by elements in the following groups? Explain your reasoning and provide an example for each (name and formula).

a. Group 1 with group 7

b. Group 2 with group 7

c. Group 1 with group 6

d. Group 2 with group 6

· 6.

An element forms an ionic compound with chlorine, leading to a compound having the formula . The ion of element has mass number and electrons. Identify the element , tell how many neutrons it has, and name the compound.

· 7.

Name each of the following compounds.

a.

b.

c.

d.

· 8.

Why do we call barium nitrate but call iron(II) nitrate?

· 9.

What is the difference between sulfuric acid and hydrosulfuric acid?

Questions and Problems: 5.1 Naming Compounds

Questions and Problems with answers below also have full solutions in the Student Solutions Guide.

Questions

directs you to the Chemistry in Focus feature in the chapter

· 1.

The “Chemistry in Focus” segment Sugar of Lead discusses , which originally was known as sugar of lead.

a. Why was it called sugar of lead?

b. What is the systematic name for ?

c. Why is it necessary to have a system for the naming of chemical compounds?

· 2.

What is a binary chemical compound? What are the two major types of binary chemical compounds? Give three examples of each type of binary compound.

Questions and Problems: 5.2 Naming Binary Compounds That Contain a Metal and a Nonmetal (Types I and II)

Questions and Problems with answers below also have full solutions in the Student Solutions Guide.

Questions

· 3.

Cations are ions, and anions are ions.

· 4.

In naming ionic compounds, we always name the second.

· 5.

In a simple binary ionic compound, which ion (cation/anion) has the same name as its parent element?

· 6.

Although we write the formula of sodium chloride as , we realize that is an ionic compound and contains no molecules. Explain.

· 7.

For a metallic element that forms two stable cations, the ending is used to indicate the cation of lower charge and the ending is used to indicate the cation of higher charge.

· 8.

We indicate the charge of a metallic element that forms more than one cation by adding a(n) after the name of the cation.

· 9.

Give the name of each of the following simple binary ionic compounds.

a.

b.

c.

d.

e.

f.

· 10.

Give the name of each of the following simple binary ionic compounds.

a.

b.

c.

d.

e.

f.

· 11.

In each of the following, identify which names are incorrect for the given formulas, and give the correct name.

a. , calcium hydride

b. , lead(IV) chloride

c. , chromium(III) iodide

d. , disodium sulfide

e. , cupric bromide

· 12.

In each of the following, identify which names are incorrect for the given formulas, and give the correct name.

a. , copper(I) chloride

b. , silver oxide

c. , lithium oxide

d. , calcium(II) sulfide

e. , cesium sulfide

· 13.

Write the name of each of the following ionic substances, using the system that includes a Roman numeral to specify the charge of the cation.

a.

b.

c.

d.

e.

f.

· 14.

Write the name of each of the following ionic substances, using the system that includes a Roman numeral to specify the charge of the cation.

a.

b.

c.

d.

e.

f.

· 15.

Write the name of each of the following ionic substances, using -ous or -ic endings to indicate the charge of the cation.

a.

b.

c.

d.

e.

f.

· 16.

Write the name of each of the following ionic substances, using -ous or -ic endings to indicate the charge of the cation.

a.

b.

c.

d.

e.

f.

Questions and Problems: 5.3 Naming Binary Compounds That Contain Only Nonmetals (Type III)

Questions and Problems with answers below also have full solutions in the Student Solutions Guide.

Questions

· 17.

Write the name of each of the following binary compounds of nonmetallic elements.

a.

b.

c.

d.

e.

f.

· 18.

Write the name for each of the following binary compounds of nonmetallic elements.

a.

b.

c.

d.

e.

f.

Questions and Problems: 5.4 Naming Binary Compounds: A Review

Questions and Problems with answers below also have full solutions in the Student Solutions Guide.

Questions

· 19.

Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal and a nonmetal) or nonionic (containing only nonmetals).

a.

b.

c.

d.

e.

f.

· 20.

The formulas and look very similar. What is the name for each compound? Why do we use a different naming convention between the two compounds?

· 21.

Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal and a nonmetal) or nonionic (containing only nonmetals).

a.

b.

c.

d.

e.

f.

· 22.

Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal or a nonmetal) or nonionic (containing only nonmetals).

a.

b.

c.

d.

e.

f.

Questions and Problems: 5.5 Naming Compounds That Contain Polyatomic Ions

Questions and Problems with answers below also have full solutions in the Student Solutions Guide.

Questions

· 23.

What is a polyatomic ion? Give examples of five common polyatomic ions.

· 24.

A(n) is a polyatomic ion containing at least one oxygen atom and one or more atoms of at least one other element.

· 25.

For the oxyanions of sulfur, the ending -ite is used for to indicate that it contains than does .

· 26.

In naming oxyanions, when there are more than two members in the series for a given element, what prefixes are used to indicate the oxyanions in the series with the fewest and the most oxygen atoms?

· 27.

Complete the following list by filling in the missing names or formulas of the oxyanions of chlorine.

· 28.

A series of oxyanions of iodine, comparable to the series for chlorine discussed in the text, also exists. Write the formulas and names for the oxyanions of iodine.

· 29.

Write the formula for each of the following phosphorus-containing ions, including the overall charge of the ion.

a. phosphide

b. phosphate

c. phosphite

d. hydrogen phosphate

· 30.

Write the formula for each of the following carbon-containing ions, including the overall charge of the ion.

a. cyanide

b. carbonate

c. hydrogen carbonate

d. acetate

· 31.

Write the formulas for the following compounds (refer to your answers to Problem 30).

a. sodium cyanide

b. calcium carbonate

c. potassium hydrogen carbonate

d. magnesium acetate

· 32.

Carbon occurs in several common polyatomic anions. List the formulas of as many such anions as you can, along with the names of the anions.

· 33.

Give the name of each of the following polyatomic ions.

a.

b.

c.

d.

e.

f.

· 34.

Give the name of each of the following polyatomic ions.

a.

b.

c.

d.

e.

f.

· 35.

Name each of the following compounds, which contain polyatomic ions.

a.

b.

c.

d.

e.

f.

· 36.

Name each of the following compounds, which contain polyatomic ions.

a.

b.

c.

d.

e.

f.

Questions and Problems: 5.6 Naming Acids

Questions and Problems with answers below also have full solutions in the Student Solutions Guide.

Questions

· 37.

Give a simple definition of an acid.

· 38.

Many acids contain the element in addition to hydrogen.

· 39.

Name each of the following acids.

a.

b.

c.

d.

e.

f.

g.

h.

i.

· 40.

Name each of the following acids.

a.

b.

c.

d.

e.

f.

g.

h.

Questions and Problems: 5.7 Writing Formulas from Names

Questions and Problems with answers below also have full solutions in the Student Solutions Guide.

Problems

· 41.

Write the formula for each of the following simple binary ionic compounds.

a. cobalt(II) chloride

b. cobaltic chloride

c. sodium phosphide

d. iron(II) oxide

e. calcium hydride

f. manganese(IV) oxide

g. magnesium iodide

h. copper(I) sulfide

· 42.

Write the formula for each of the following simple binary ionic compounds.

a. magnesium fluoride

b. ferric iodide

c. mercuric sulfide

d. barium nitride

e. plumbous chloride

f. stannic fluoride

g. silver oxide

h. potassium selenide

· 43.

Write the formula for each of the following binary compounds of nonmetallic elements.

a. carbon disulfide

b. water

c. dinitrogen trioxide

d. dichlorine heptoxide

e. carbon dioxide

f. ammonia

g. xenon tetrafluoride

· 44.

Write the formula for each of the following binary compounds of nonmetallic elements.

a. diphosphorus monoxide

b. sulfur dioxide

c. diphosphorus pentoxide

d. carbon tetrachloride

e. nitrogen tribromide

f. silicon tetrafluoride

g. sulfur dichloride

· 45.

Write the formula for each of the following compounds that contain polyatomic ions. Be sure to enclose the polyatomic ion in parentheses if more than one such ion is needed to balance the oppositely charged ion(s).

a. ammonium nitrate

b. magnesium acetate

c. calcium peroxide

d. potassium hydrogen sulfate

e. iron(II) sulfate

f. potassium hydrogen carbonate

g. cobalt(II) sulfate

h. lithium perchlorate

· 46.

Write the formula for each of the following compounds that contain polyatomic ions. Be sure to enclose the polyatomic ion in parentheses if more than one such ion is needed to balance the oppositely charged ions.

a. ammonium acetate

b. ferrous hydroxide

c. cobalt(III) carbonate

d. barium dichromate

e. lead(II) sulfate

f. potassium dihydrogen phosphate

g. lithium peroxide

h. zinc chlorate

· 47.

Write the formula for each of the following acids.

a. hydrosulfuric acid

b. perbromic acid

c. acetic acid

d. hydrobromic acid

e. chlorous acid

f. hydroselenic acid

g. sulfurous acid

h. perchloric acid

· 48.

Write the formula for each of the following acids.

a. hydrocyanic acid

b. nitric acid

c. sulfuric acid

d. phosphoric acid

e. hypochlorous acid

f. hydrobromic acid

g. bromous acid

h. hydrofluoric acid

· 49.

Write the formula for each of the following substances.

a. sodium peroxide

b. calcium chlorate

c. rubidium hydroxide

d. zinc nitrate

e. ammonium dichromate

f. hydrosulfuric acid

g. calcium bromide

h. hypochlorous acid

i. potassium sulfate

j. nitric acid

k. barium acetate

l. lithium sulfite

· 50.

Write the formula for each of the following substances.

a. calcium hydrogen sulfate

b. zinc phosphate

c. iron(III) perchlorate

d. cobaltic hydroxide

e. potassium chromate

f. aluminum dihydrogen phosphate

g. lithium bicarbonate

h. manganese(II) acetate

i. magnesium hydrogen phosphate

j. cesium chlorite

k. barium peroxide

l. nickelous carbonate

Additional Problems

· 51.

Iron forms both and cations. Write formulas for the oxide, sulfide, and chloride compound of each iron cation, and give the name of each compound in both the nomenclature method that uses Roman numerals to specify the charge of the cation and the -ous/-ic notation.

· 52.

Before an electrocardiogram is recorded for a cardiac patient, the leads are usually coated with a moist paste containing sodium chloride. What property of an ionic substance such as is being made use of here?

· 53.

Nitrogen and oxygen form numerous binary compounds, including , , , , and . Give the name of each of these oxides of nitrogen.

· 54.

On some periodic tables, hydrogen is listed both as a member of Group 1 and as a member of Group 7. Write an equation showing the formation of ion and an equation showing the formation of ion.

· 55.

Examine the following table of formulas and names. Which of the compounds is/are named correctly?

· 56.

Complete the following list by filling in the missing oxyanion or oxyacid for each pair.

· 57.

Name the following compounds.

a.

b.

c.

d.

e.

f.

g.

· 58.

Name the following compounds.

a.

b.

c.

d.

e.

f.

g.

· 59.

Name the following compounds.

a.

b.

c.

d.

e.

f.

g.

· 60.

A compound has the general formula , with representing an unknown element or ion and representing oxygen. Which of the following could not be a name for this compound?

a. sodium oxide

b. iron(II) oxide

c. copper(I) oxide

d. dinitrogen monoxide

e. water

· 61.

Most metallic elements form oxides, and often the oxide is the most common compound of the element that is found in the earth’s crust. Write the formulas for the oxides of the following metallic elements.

a. potassium

b. magnesium

c. iron(II)

d. iron(III)

e. zinc(II)

f. lead(II)

g. aluminum

· 62.

Consider a hypothetical simple ion . Determine the formula of the compound this ion would form with each of the following anions.

a. acetate

b. permanganate

c. oxide

d. hydrogen phosphate

e. hydroxide

f. nitrite

· 63.

Consider a hypothetical element , which is capable of forming stable simple cations that have charges of , , and , respectively. Write the formulas of the compounds formed by the various cations with each of the following anions.

a. chromate

b. dichromate

c. sulfide

d. bromide

e. bicarbonate

f. hydrogen phosphate

· 64.

A metal ion with a charge has electrons and forms a compound with a halogen ion that contains protons.

a. What is the identity of the metal ion?

b. What is the identity of the halogen ion and how many electrons does it contain?

c. Determine the compound that it forms and name it.

· 65.

Complete Table 5.A by writing the names and formulas for the ionic compounds formed when the cations listed across the top combine with the anions shown in the left-hand column.

Table 5.A.

· 66.

Complete Table 5.B by writing the formulas for the ionic compounds formed when the anions listed across the top combine with the cations shown in the left-hand column.

Table 5.B.

· 67.

The noble metals gold, silver, and platinum are often used in fashioning jewelry because they are relatively .

· 68.

The formula for ammonium phosphate is .

· 69.

The elements of Group 7 (fluorine, chlorine, bromine, and iodine) consist of molecules containing atom(s).

· 70.

Under what physical state at room temperature do each of the halogen elements exist?

· 71.

When an atom gains two electrons, the ion formed has a charge of .

· 72.

An ion with one less electron than it has protons has a charge.

· 73.

An atom that has lost three electrons will have a charge of  .

· 74.

An ion with two more electrons than it has protons has a charge.

· 75.

For each of the negative ions listed in column 1, use the periodic table to find in column 2 the total number of electrons the ion contains. A given answer may be used more than once.

· 76.

For each of the following processes that show the formation of ions, complete the process by indicating the number of electrons that must be gained or lost to form the ion. Indicate the total number of electrons in the ion, and in the atom from which it was made.

a.

b.

c.

d.

e.

f.

· 77.

For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simple ion that the element is most likely to form.

a.

b.

c.

d.

e.

f.

· 78.

For the following pairs of ions, use the principle of electrical neutrality to predict the formula of the binary compound that the ions are most likely to form.

a. and

b. and

c. and

d. and

e. and

f. and

g. and

h. and

· 79.

Give the name of each of the following simple binary ionic compounds.

a.

b.

c.

d.

e.

f.

g.

h.

· 80.

In which of the following pairs is the name incorrect? Give the correct name for the formulas indicated.

a. , disilver monoxide

b. , dinitrogen monoxide

c. , iron(II) oxide

d. , plumbous oxide

e. , chromium(III) sulfate

· 81.

Write the name of each of the following ionic substances, using the system that includes a Roman numeral to specify the charge of the cation.

a.

b.

c.

d.

e.

f.

· 82.

Write the name of each of the following ionic substances, using -ous or -ic endings to indicate the charge of the cation.

a.

b.

c.

d.

e.

f.

· 83.

Name each of the following binary compounds.

a.

b.

c.

d.

e.

f.

· 84.

Name each of the following compounds.

a.

b.

c.

d.

e.

f.

· 85.

Which oxyanion of nitrogen contains a larger number of oxygen atoms, the nitrate ion or the nitrite ion?

· 86.

Examine the following table of formulas and names. Which of the compounds is/are named incorrectly?

· 87.

Write the formula for each of the following chromium-containing ions, including the overall charge of the ion.

a. chromous

b. chromate

c. chromic

d. dichromate

· 88.

Give the name of each of the following polyatomic anions.

a.

b.

c.

d.

e.

f.

· 89.

Name each of the following compounds, which contain polyatomic ions.

a.

b.

c.

d.

e.

f.

· 90.

A member of the alkali metal family whose most stable ion contains electrons forms a compound with chlorine. What is the correct formula for this compound?

· 91.

Write the formula for each of the following binary compounds of nonmetallic elements.

a. sulfur dioxide

b. dinitrogen monoxide

c. xenon tetrafluoride

d. tetraphosphorus decoxide

e. phosphorus pentachloride

f. sulfur hexafluoride

g. nitrogen dioxide

· 92.

Write the formula of each of the following ionic substances.

a. sodium dihydrogen phosphate

b. lithium perchlorate

c. copper(II) hydrogen carbonate

d. potassium acetate

e. barium peroxide

f. cesium sulfite

· 93.

Write the formula for each of the following compounds, which contain polyatomic ions. Be sure to enclose the polyatomic ion in parentheses if more than one such ion is needed to balance the oppositely charged ion(s).

a. silver(I) perchlorate (usually called silver perchlorate)

b. cobalt(III) hydroxide

c. sodium hypochlorite

d. potassium dichromate

e. ammonium nitrite

f. ferric hydroxide

g. ammonium hydrogen carbonate

h. potassium perbromate

ChemWork Problems

These multiconcept problems (and additional ones) are found interactively online with the same type of assistance a student would get from an instructor.

· 94.

Complete the following table to predict whether the given atom will gain or lose electrons in forming the ion most likely to form when in ionic compounds.

· 95.

What are the formulas of the compounds that correspond to the names given in the following table?

· 96.

What are the names of the compounds that correspond to the formulas given in the following table?

· 97.

Provide the name of the acid that corresponds to the formula given in the following table.

· 98.

Which of the following statements is(are) correct?

a. The symbols for the elements magnesium, aluminum, and xenon are , , and , respectively.

b. The elements , , and are in the same family on the periodic table.

c. All of the following elements are expected to gain electrons to form ions in ionic compounds: , , and .

d. The elements , , and are all transition elements.

e. The correct name for is titanium dioxide.

Chapters 4-5. Cumulative Review

Questions

Questions with answers below also have full solutions in the Student Solutions Guide.

Questions

· 1.

What is an element? Which elements are most abundant on the earth? Which elements are most abundant in the human body?

· 2.

Without consulting any reference, write the name and symbol for as many elements as you can. How many could you name? How many symbols did you write correctly?

· 3.

The symbols for the elements silver , gold , and tungsten seem to bear no relation to their English names. Explain and give three additional examples.

· 4.

Without consulting your textbook or notes, state as many points as you can of Dalton’s atomic theory. Explain in your own words each point of the theory.

· 5.

What is a compound? What is meant by the law of constant composition for compounds and why is this law so important to our study of chemistry?

· 6.

What is meant by a nuclear atom? Describe the points of Rutherford’s model for the nuclear atom and how he tested this model. Based on his experiments, how did Rutherford envision the structure of the atom? How did Rutherford’s model of the atom’s structure differ from Kelvin’s “plum pudding” model?

· 7.

Consider the neutron, the proton, and the electron.

a. Which is(are) found in the nucleus?

b. Which has the largest relative mass?

c. Which has the smallest relative mass?

d. Which is negatively charged?

e. Which is electrically neutral?

· 8.

What are isotopes? To what do the atomic number and the mass number of an isotope refer? How are specific isotopes indicated symbolically (give an example and explain)? Do the isotopes of a given element have the same chemical and physical properties? Explain.

· 9.

Complete the following table by giving the symbol, name, atomic number, and/or group(family) number as required.

· 10.

Are most elements found in nature in the elemental or the combined form? Why? Name several elements that are usually found in the elemental form.

· 11.

What are ions? How are ions formed from atoms? Do isolated atoms form ions spontaneously? To what do the terms cation and anion refer? In terms of subatomic particles, how is an ion related to the atom from which it is formed? Does the nucleus of an atom change when the atom is converted into an ion? How can the periodic table be used to predict what ion an element’s atoms will form?

· 12.

What are some general physical properties of ionic compounds such as sodium chloride? How do we know that substances such as sodium chloride consist of positively and negatively charged particles? If ionic compounds are made up of electrically charged particles, why doesn’t such a compound have an overall electric charge? Can an ionic compound consist only of cations or anions (but not both)? Why not?

· 13.

What principle do we use in writing the formula of an ionic compound such as or ? How do we know that two iodide ions are needed for each magnesium ion, whereas only one chloride ion is needed per sodium ion?

· 14.

When writing the name of an ionic compound, which is named first, the anion or the cation? Give an example. What ending is added to the root name of an element to show that it is a simple anion in a Type I ionic compound? Give an example. What two systems are used to show the charge of the cation in a Type II ionic compound? Give examples of each system for the same compound. What general type of element is involved in Type II compounds?

· 15.

Describe the system used to name Type III binary compounds (compounds of nonmetallic elements). Give several examples illustrating the method. How does this system differ from that used for ionic compounds? How is the system for Type III compounds similar to those for ionic compounds?

· 16.

What is a polyatomic ion? Without consulting a reference, list the formulas and names of at least ten polyatomic ions. When writing the overall formula of an ionic compound involving polyatomic ions, why are parentheses used around the formula of a polyatomic ion when more than one such ion is present? Give an example.

· 17.

What is an oxyanion? What special system is used in a series of related oxyanions that indicates the relative number of oxygen atoms in each ion? Give examples.

· 18.

What is an acid? How are acids that do not contain oxygen named? Give several examples. Describe the naming system for the oxyacids. Give examples of a series of oxyacids illustrating this system.

Problems

Problems with answers below also have full solutions in the Student Solutions Guide.

Problems

· 19.

Complete the following table by giving the symbol, name, atomic number, and/or group (family) number as required.

· 20.

Your text indicates that the Group 1, Group 2, Group 7, and Group 8 elements all have “family” names (alkali metals, alkaline earth metals, halogens, and noble gases, respectively). Without looking at your textbook, name as many elements in each family as you can. What similarities are there among the members of a family? Why?

· 21.

Using the periodic table shown in Fig. 4.9, for each of the following symbols, write the name of the element and its atomic number.

a.

b.

c.

d.

e.

f.

g.

h.

i.

j.

k.

l.

m.

n.

o.

p.

q.

r.

s.

t.

u.

v.

w.

x.

y.

z.

· 22.

How many electrons, protons, and neutrons are found in isolated atoms having the following atomic symbols?

a.

b.

c.

d.

e.

f.

g.

h.

· 23.

What simple ion does each of the following elements most commonly form?

a.

b.

c.

d.

e.

f.

g.

h.

i.

j.

k.

l.

m.

· 24.

For each of the following simple ions, indicate the number of protons and electrons the ion contains.

a.

b.

c.

d.

e.

f.

g.

h.

i.

j.

k.

l.

· 25.

Using the ions indicated in Problem 24, write the formulas and give the names for all possible simple ionic compounds involving these ions.

· 26.

Write the formula for each of the following binary ionic compounds.

a. copper(I) iodide

b. cobaltous chloride

c. silver sulfide

d. mercurous bromide

e. mercuric oxide

f. chromium(III) sulfide

g. plumbic oxide

h. potassium nitride

i. stannous fluoride

j. ferric oxide

· 27.

Which of the following formula—name pairs are incorrect? Explain why for each case.

· 28.

Give the name of each of the following polyatomic ions.

a.

b.

c.

d.

e.

f.

g.

h.

i.

j.

· 29.

Using the negative polyatomic ions listed in Table 5.4, write formulas for each of their sodium and calcium compounds.

· 30.

Give the name of each of the following compounds.

a.

b.

c.

d.

e.

f.

g.

h.

· 31.

Write formulas for each of the following compounds.

a. mercuric chloride

b. iron(III) oxide

c. sulfurous acid

d. calcium hydride

e. potassium nitrate

f. aluminum fluoride

g. dinitrogen monoxide

h. sulfuric acid

i. potassium nitride

j. nitrogen dioxide

k. silver acetate

l. acetic acid

m. platinum(IV) chloride

n. ammonium sulfide

o. cobalt(III) bromide

p. hydrofluoric acid