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Chapter 2: Q57E (page 127)

Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:

a. Cr2O3

b. FeCl2

c. CrO3

d. TiCl4

e.CoO

f. MoS2

Short Answer

Expert verified

a. Chromium (III) oxide

b. Iron (II) chloride or ferrous chloride

c. Chromium trioxide

d. Titanium tetrachloride

e. Cobalt (II) oxide

f. Molybdenum sulfide

Step by step solution

01

Understanding the concept of ionic charges.

Generally, many metals exhibit the property of showing multiple positive charges or ionic states. This property depends upon the entity forminga bond with the metal.The metal loses its electron according to the requirement of electrons by the other entity.

For example, Iron (Fe) can show two ionic states, i.e., +2 and +3.

02

Determining the names of the compounds

(a) Cr2O3- Chromium (III) oxide

(b)FeCl2- Ferrous chloride

(c) CrO3- Chromium trioxide

(d) TiCl4- Titanium tetrachloride

(e) CoO- Cobalt Oxide

(f)MoS2- Molybdenum sulfide

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Most popular questions from this chapter

Using the periodic table, classify each of the following elements as a metal or a nonmetal, and then further classify each as a main-group (representative) element, transition metal, or inner transition metal:

  1. Uranium
  2. Bromine
  3. Strontium
  4. Neon
  5. Gold
  6. Americium
  7. Rhodium
  8. Sulfur
  9. Carbon
  10. Potassium

Question : Write the formulas of the following compounds:

(a) lithium carbonate

(b) sodium perchlorate

(c) barium hydroxide

(d) ammonium carbonate

(e) sulfuric acid

(f) calcium acetate

(g) magnesium phosphate

(h) sodium sulfite

The following compounds are found in common household products. Name each of these compounds:

a. Ca(H3PO4)2

b. FeSO4

c. CaCO3

d. MgO

e. NaNO2

f. KI

Variations in average atomic mass may be observed for elements obtained from different sources. Lithium provides an example of this. The isotopic composition of lithium from naturally occurring minerals is 7.5% 6Li and 92.5% 7Li, which have masses of 6.01512 amu and 7.01600 amu, respectively. A commercial source of lithium, recycled from a military source, was 3.75% 6Li (and the rest 7Li). Calculate the average atomic mass values for each of these two sources.

Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the 鈥淢ix Isotopes鈥� tab, hide the 鈥淧ercent Composition鈥� and 鈥淎verage Atomic Mass鈥� boxes, and then select the element boron.

(a) Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts.

(b) Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice.

(c) Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes fromtheir bins or click on 鈥淢ore鈥� and then move the sliders to the appropriate amounts.

(d) Reveal the 鈥淧ercent Composition鈥� and 鈥淎verage Atomic Mass鈥� boxes. How well does your mixture match withyour prediction? If necessary, adjust the isotope amounts to match your prediction.

(e) Select 鈥淣ature鈥檚鈥� mix of isotopes and compare it to your prediction. How well does your prediction comparewith the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match 鈥淣ature鈥檚鈥漚mounts as closely as possible.
See all solutions

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