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3.12: End of Chapter Problems

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    Ions

    1. Identify each as a cation, an anion, or molecule.

    a. H+ b. Cl− c. O2 d. Ba2+

    e. CH4 f. CS2 g. NH3 h. Br−

    i. H− j. Hg2+ k. CCl4 l. SO3

    2. What are ionophores? Explain how ionophores act as antibiotics.

    Main Group Elements

    1. Which of these ions is not likely to form?

    a. Mg+ b. K+

    c. S3− d. N3−

    2. When the following atoms become ions, what charges do they acquire?

    a. Li b. S

    c. Ca d. F

    3. What characteristic charge do atoms in the first column of the periodic table have when they become ions?

    4. What characteristic charge do atoms in the second column of the periodic table have when they become ions?

    5. What characteristic charge do atoms in the third-to-last column of the periodic table have when they become ions?

    6. What characteristic charge do atoms in the next-to-last column of the periodic table have when they become ions?

    7. Starting with lithium and bromine atoms, use Lewis diagrams to show the formation of the ionic compound.

    a. LiBr

    b. MgO

    Nomenclature of Ions

    1. Name each ion.

    a. Ca2+ b. S2− c. SO42− d. NH4+

    e. Ba2+ f. HCO3− g. Ca2+ h. P3−

    i. H2PO4− j. Sn4+ k. K+ l. Fe3+

    m. HSO4− n. Sn2+ o. Ca2+ p. S2−

    q. SO32− r. NH4+ s. Cu+ t. Fe2+

    2. Write the formula for each ion.

    a. the bromide ion b. the phosphate ion c. the cupric ion

    d. the magnesium ion e. the fluoride ion f. the carbonate ion

    g. the ferrous ion h. the potassium ion i. the bromide ion

    j. the phosphate ion k. the cupric ion l. the magnesium ion

    m. the fluoride ion n. the carbonate ion o. the potassium ion

    Formula of Ionic Compounds

    1. Starting with lithium and bromine atoms, use Lewis diagrams to show the formation of the ionic compound.

    LiBr MgO

    2. Write the chemical formula for an ionic compound composed of each pair of ions.

    a. the 3+ iron ion and the oxygen ion b. the calcium ion and the oxygen ion

    c. the 2+ copper ion and the sulfur ion d. the 1+ copper ion and the sulfur ion

    e. the potassium ion and the sulfate ion f. the calcium ion and the nitrate ion

    g. the magnesium ion and the carbonate ion h. the aluminum ion and the acetate ion

    i. the sodium ion and the sulfur ion j. the aluminum ion and the fluoride ion

    Nomenclature of Ionic Compounds

    1. Name each ionic compound using both Stock and common systems if necessary.

    Ca3(PO4)2 (NH4)2Cr2O7 KCl

    CuCl SnF2 ZnBr2

    Fe(NO3)3 Al2O3 CuF2

    AgF Ca3(PO4)2 (NH4)2Cr2O7

    KCl CuCl SnF2

    ZnBr2 Fe(NO3)3 Al2O3

    CuF2 AgF

    2. Give two names for each compound

    a. Al(HSO4)3

    b. Mg(HSO4)2

    c. Co(HCO3)2

    d. LiHCO3

    Formula and Nomenclature of Ionic Compounds

    Give the formula and the name of the ionic compound formed by each pair of ions. Use both the Stock and common systems, where appropriate.

    a. Na+ and Br−

    b. Mg2+ and Br−

    c. Mg2+ and S2−

    d. K+ and Cl−

    e. Mg2+ and Cl−

    f. Mg2+ and F−

    g. Na+ and N3−

    h. Mg2+ and N3−

    i. Al3+ and S2−

    j. Li+ and N3−

    k. Mg2+ and P3−

    l. Li+ and P3−

    m. Fe3+ and Br−

    n. Fe2+ and Br−

    o. Fe3+ and S2−

    p. Cu+ and S2−

    q. Cr3+ and O2−

    r. Cr2+ and O2−

    s. Pb2+ and Cl−

    t. Pb4+ and Cl−

    u. Cr3+ and NO3−

    v. Fe2+ and PO43−

    w. Ca2+ and SO42−

    x. Al3+ and OH−

    y. NH4+ and NO3−

    z. K+ and SO42−

    Covalent Bonds

    Predict the number of covalent bonds formed by each nonmetal atom.

    N Cl C O Br H

    Ionic vs. Molecular Compounds

    1. Which compounds would you predict to be ionic? Circle.

    a. Li2O b. (NH4)2S c. CO2 d. FeSO3

    e. C6H6 f. C2H6O g. Ba(OH)2 h. CH2O

    i. NH2CONH2 j. (NH4)2CrO4 k. C8H18 l. NH3

    2. Identify each compound as ionic or molecular.

    a. Na2O b. PCl3 c. NH4Cl d. OF2

    e. N2O f. FeCl3 g. (NH4)3PO4 h. SOCl2

    3. Is each compound formed from ionic bonds, covalent bonds, or both?

    a. Na2O b. Na3PO4 c. N2O4

    d. Ba(OH)2 e. F2 f. PCl3

    4. Write the molecular formula for each compound.

    1. chlorine trifluoride b. phosphorus pentachloride c. sulfur dioxide

    d. nitrogen dioxide e. dioxygen difluoride f. dinitrogen pentoxide

    g. sulfur hexafluoride h. nitrogen monoxide

    5. Write the name for each compound.

    1. BrF5 b. S2F2 c. CO

    d. CF4 e. SeCl2 f. SO3

    Formula Weight and Molecular Weight

    1. Use the atomic weights rounded to two decimal places to determine the formula weight for each ionic compound.

    1. TiO2
    2. AgBr
    3. Au(NO3)3
    4. Fe3(PO4)2

    2. Calculate the molecular weight of each covalent compound? Use the atomic weights rounded to two decimal places.

    a. C2H2

    b. CO

    c. CO2

    d. BF3

    Mass-Mole Conversions

    1. A biochemist needs 0.00655 mol of bilirubin (C33H36N4O6) for an experiment. How many grams of bilirubin will that be?

    2. A chemist needs 457.8 g of KMnO4 to make a solution. How many moles of KMnO4 is that?

    3. What is the mass of 62.5 moles of carbon tetrachloride?

    4. How many moles of ammonium hydroxide are present in 0.475 g?

    This page titled 3.12: End of Chapter Problems is shared under a not declared license and was authored, remixed, and/or curated by Deboleena Roy (American River College).

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