Review Module / Chapters 5�8 43 by G2iv1V

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									SECTION 6.1: INTRODUCTION TO CHEMICAL BONDING
1. Give the name and symbol of the ion formed when
          a. a chlorine atom gains one electron.
          b. a potassium atom loses one electron.
          c. an oxygen atom gains two electrons.
          d. a barium atom loses two electrons.
2. How many electrons are lost or gained in forming each ion?
          a. Mg2+            b. Br-              c. Ag+          d. Fe3+
3. Classify each of the following as a cation, anion, or atom.
          a. Be              c. Cu2+             e. O2-          g. Cs+
          b. Na +
                             d. I-
                                                 f. Ca 2+
                                                                 h. Ne
4. Classify each of the following as a molecular compound or an ionic compound.
          a. CO2             c. NaCl             e. MgCl2
          b. N2              d. H2O
5. What types of elements tend to combine to form molecular compounds?
6. What types of elements tend to combine to form ionic compounds?
SECTION 6.2: REPRESENTING CHEMICAL COMPOUNDS
Use the dimensional analysis problem solving approach from Chapter 4.
1. Sulfur forms two molecular compounds with oxygen. Compound A contains 3.505 g of sulfur combined with 3.810 g of oxygen.
          Compound B contains 6.553 g of sulfur combined with 10.743 g of oxygen. What is the lowest whole-number mass ratio of
          sulfur that combines with a given mass of oxygen?
2. A chemistry student prepared a series of compounds containing only sulfur and fluorine. The following table shows the amount of
          each element in each compound.
        Compound           Mass of sulfur (g) Mass of fluorine (g)
               A                 20.18                  47.85
               B                 14.44                  8.53
               C                 16.79                  59.68
          a. Calculate the mass of fluorine per gram of sulfur in each compound.
          b. How do the numbers in part a. support the law of multiple proportions?
3. Nitrogen reacts with hydrogen to form two compounds. Compound A contains 18.8 g of nitrogen for each 2.7 g hydrogen.
          Compound B contains 13.3 g of nitrogen for each 2.9 g hydrogen. What is the mass ratio of nitrogen per gram of hydrogen
          in the two compounds?
4. Identify the number and kinds of atoms present in a molecule of each compound.
          a. citric acid, C6H8O7                 c. glycine, C2H5NO2
          b. chloroform, CHCl3                   d. sulfur hexafluoride, SF6
SECTION 6.3: IONIC CHARGES
1. What is the charge on the ion typically formed by each element?
     a. oxygen           c. sodium            e. nickel, 2 electrons lost
     b. iodine           d. aluminum          f. magnesium
2. How many electrons does the neutral atom gain or lose when each
ion forms?
     a. Cr3+             c. Li+               e. Cl-
     b. P3-              d. Ca2+              f. O2-
3. Name each ion. Identify each as a cation or anion.
     a. Sn2+             c. Br-               e. H-
     b. Co3+             d. K+                f. Mn2+
4. Write the formula (including charge) for each ion. Use Table 6.4
from text if necessary.
     a. carbonate ion    c. sulfate ion             e. chromate ion
     b. nitrate ion      d. hydroxide ion           f. ammonium ion
5. Name the following ions. Identify each as a cation or anion.
      a. CN-               c. PO43-               e. Ca2+
      b. HCO3-             d. Cl-                 f. SO32-
SECTION 6.4: IONIC COMPOUNDS
1. Write the formulas for these binary ionic compounds.
a. magnesium oxide         c. potassium iodide         e. sodium sulfide
b. tin(II) fluoride        d. aluminum chloride f. ferric bromide
2. Write the formulas for the cmpds formed from these pairs of ions.
      a. Ba2+, Cl-               c. Ca2+, S2-                 e. Al3+, O2-
      b. Ag+, I-                 d. K+, Br-                   f. Fe2+, O2-
3. Name the following binary ionic compounds.
a. MnO2               c. CaCl2              e. NiCl2                g. CuCl2
b. Li3N               d. SrBr2              f. K2S                  h. SnCl4
4. Write formulas for the following ternary ionic compounds.
a. sodium phosphate        c. sodium hydroxide         e. ammonium chloride
b. magnesium sulfate d. potassium cyanide              f. potassium dichromate
5. Write formulas for compounds formed from these pairs of ions.
      a. NH4+, SO42-       c. barium ion and hydroxide ion
           +      -
      b. K , NO3           d. lithium ion and carbonate ion
6. Name the following compounds.
      a. NaCN              c. Na2SO4                   e. Cu(OH)2
      b. FeCl3             d. K2CO3                    f. LiNO3
SECTION 6.5: MOLECULAR COMPOUNDS AND ACIDS
1. Name the following molecular compounds.
a. PCl5               c. NO2                e. P4O6                 g. SiO2
b. CCl4               d. N2F2               f. XeF2                 h. Cl2O7
2. Write the formulas for the following binary molecular compounds.
      a. nitrogen tribromide          c. sulfur dioxide
      b. dichlorine monoxide          d. dinitrogen tetrafluoride
3. Give the name or formula for these common acids.
a. HCl           b. H3PO4             c. acetic acid          d. sulfuric acid
4. Name and give the charge of the metal cation in each of the following ionic
compounds.
    a. Na3PO4                    c. CaS                     e. FeCl3
    b. NiCl2                     d. K2S                     f. CuI
5. For each of the following binary compounds, decide whether the
compound is expected to be ionic or molecular.
     a. SeF4                  c. NH3                 e. CO2
     b. KBr                   d. MgBr2               f. PCl5
SECTION 6.6: SUMMARY OF NAMING AND FORMULA WRITING
1. Write the formulas for these compounds.
a. potassium sulfide     e. hydrobromic acid      i. sulfur hexafluoride
b. tin (IV) chloride     f. aluminum fluoride     j. magnesium chloride
c. dihydrogen sulfide    g. dinitrogen pentoxide k. phosphoric acid
d. calcium oxide         h. iron (III) carbonate l. nitric acid
2. Complete the table below by writing correct formulas and names for
the compounds formed by combining the positive and negative ions
given.
           SO42-         NO3-             OH-          PO43-

Ca2+

Al3+

Na+

Pb4+


3. Name the following compounds; identify them as molecular (M) or
ionic (I); & if ionic, identify them as binary or ternary.
a. K3PO4         c. NaHSO4       e. N2O5        g. PI3
b. Al(OH)3       d. HgO          f. NBr3        h. (NH4)2SO4

								
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