<p> Unit 3 Chemical Compound Problems - Key</p><p>Complete each question on your own paper.</p><p>1. Write the symbol for each element and identify each as a metal (M) or non- metal (N).</p><p> a. barium Ba, M c. phosphorus P, N e. copper Cu, M g. potassium K, M i. sodium Na, M b. lead Pb, M d. chlorine Cl, N f. arsenic As, N h. gold Au, M j. tin Sn, M</p><p>2. What are valence electrons? Outer shell electrons that may participate in chemical activity</p><p>3. Write the symbol, number of valence electrons, and charge of each element. </p><p> a. Magnesium Mg, s2, +2 cation c. phosphorus P, s2p3, -3 anion e. oxygen O, s2p4, -2 anion g. potassium K, s1, +1, cation i. sodium Na, s1, +1, cation b. selenium Se s2p4, -2 anion d. chlorine Cl, s2p5, -1 anion f. sulfur S, s2p4, -2 anion h. silicon Si, s2p2, +/-4 j. neon Ne, s2p6, 0</p><p>4. Identify each of the elements in Number 3 as a cation or an anion. See above</p><p>5. Draw the Bohr Models and Electron Dot Diagrams for each of the elements in Number 3 above.</p><p> a. magnesium c. phosphorus e. oxygen g. potassium i. sodium The following dot diagrams represent generic dot diagrams that apply to all elements in the same column.</p><p> b. selenium d. chlorine f. sulfur h. silicon j. neon</p><p>6. What elements create ionic, covalent and metallic bonds? Ionic (primarily metals w/ nonmetals) Covalent (primarily nonmetals w/ nonmetals) Metallic (metals w/in themselves and alloyed with other metals)</p><p>7. What are the 7 diatomic gases? Name two allotropes. H2, N2, O2, F2, Cl2, Br2, I2, S8 & ?</p><p>8. For each of the following compounds indicate if it is ionic, covalent, or metallic.</p><p> a. NO3 covalent d. Al(NO3)3 ionic g. CCl4 covalent</p><p> b. NaCl ionic e. Fe2(SO4)3 ionic h. H2 covalent</p><p> c. K2O ionic f. XeF2covalent i. Co3N2 ionic</p><p>9. Draw the Lewis structure for each of the following covalent compounds.</p><p> a. CF4 e. BF3 i. NF3</p><p>Adapted from Dawn Wakely, Lindberg High School, 1999 b. H2CS f. CH2F2 j. O2</p><p> c. PF3 g. H2S k. N2</p><p>2- - d. F2 h. carbonate ion (CO3 ) l. nitrate ion (NO3 )</p><p>10. Draw the Lewis Structure for each organic compound.</p><p> a. CH4 f. CH3OH l. CH2O q. HCOOH</p><p> a. C2H6 g. C2H5OH m. CH3CHO r. CH3COOH</p><p> b. C3H8 h. C3 H7OH n. C2H5CHO s. C2H5COOH</p><p> c. C4H10 i. C2H4 o. HCN</p><p> d. C5H12 j. C2H2 p. C2H4NH2</p><p>11. Write formulas for the following covalent compounds.</p><p> a. Chlorine dioxide e. selenium difluoride i. disulfur trioxide</p><p>ClO2 SeF2 S2O3</p><p> b. Iodine tribromide f. triphosphorus tetrabromide j. tetrasulfur hexabromide</p><p>IBr3 P3Br4 S4Br6</p><p> c. Sulfur dioxide g. dichorine monoxide k. xenon hexafluoride</p><p>SO2 Cl2O XeF6</p><p> d. Dinitrogen pentoxide h. dinitrogen triiodide l. carbon tetrachloride</p><p>N2O5 N2I3 CCl4</p><p>12. Write names for the following covalent compounds.</p><p>Adapted from Dawn Wakely, Lindberg High School, 1999 a. SiC d. OF2 g. N2O5 j. PCl3 Silicon monocarbide, oxygen difluoride, dinitrogen pentoxide, phosphorus trichloride</p><p> b. CS2 e. SO2 h. NO k. CI4 Carbon disulfide, sulfur dioxide nitrogen monoxide carbon tetra-iodide</p><p> c. NO2 f. SO3 i. P4O10 l. S2Cl6 Nitrogen dioxide sulfur trioxide tetraphosphorus deca-oxide, disulfur hexachloride</p><p>13. Write formulas for the following ionic compounds.</p><p> a. Sodium fluoride NaF e. cesium chloride CsCl2 i. Gallium sulfide Ga2S3</p><p> b. Aluminum nitride AlN f. barium bromide BaBr2 j. potassium iodide KI</p><p> c. Aluminum bromide AlBr3 g. cesium sulfide Cs2S k. strontium nitride Sr3N2</p><p> d. Magnesium sulfide MgS h. potassium oxide K2O l. aluminum iodide AlI3</p><p>14. Write formulas for the following ionic compounds.</p><p> a. scandium oxide Sc2O3 e. manganese V sulfide Mn2S5 i. iron III phosphide FeP</p><p> b. nickel II nitride Ni3N2 f. silver chloride AgCl j. mercury I nitride (Hg2)3N2</p><p> c. zinc II chloride ZnCl2 g. gold bromide AuBr3 K. mercury II nitride Hg3N2</p><p> d. nickel IV oxide NiO2 h. iron II phosphide Fe3P2 l. copper II iodide CuI2</p><p>15. Write formulas for the following ionic compounds.</p><p> a. silver nitrate AgNO3 e. iron II sulfite FeSO3 i. ammonium acetate NH4C2H3O2</p><p> b. silver nitride Ag3N f. iron II sulfide FeS k. ammonium sulfate (NH4)2SO4</p><p> c. magnesium nitrite Mg(NO2)2 g. aluminum oxide Al2O3 l. zinc II carbonate ZnCO3</p><p> d. iron II sulfate FeSO4 h. aluminum oxalate Al2(C2O4)3 m. cesium phosphate Cs3PO4</p><p>16. What is the charge on the metal of the following:</p><p> a. Al2O3 +3 d. Cu(NO3)2 +2 g. Fe(C2H3O2)2 +2 j. KC2H3O2 +1</p><p> b. ZnCO3 +2 e. Ca(OH)2 +2 h. Na2SO4 +1 k. CoC2O4 +2</p><p> c. Au(NO3)3 +3 f. Al2(SO4)3 +3 i. Sn(NO2)2 +2 l. Ag3PO4 +1</p><p>17. Name each of the following ionic compounds (Remember to place the roman numeral on transition metals.).</p><p> a. Al2O3 d. Cu(NO3)2 g. Fe(C2H3O2)2 j. KC2H3O2 Aluminum oxide copper(II) nitrate iron(II) acetate potassium acetate</p><p> b. ZnCO3 e. Ca(OH)2 h. Na2SO4 k. CoC2O4 Zinc carbonate calcium hydroxice sodium sulfate cobalt(II) oxalate</p><p> c. Au(NO3)3 f. Al2(SO4)3 i. Sn(NO2)2 l. Ag3PO4 Gold nitrate aluminum sulfate tin(II) nitrite silver phosphate</p><p>18. Identify each of the following formulas as ionic or covalent. Write the name for each.</p><p> a. MgO ionic d. NaI ionic g. N2O5 covalent j. Al2O3 ionic Magnesium oxide sodium iodide dinitrogen pentoxide aluminum oxide</p><p> b. CO covalent e. CaBr2 ionic h. S2Cl3 covalent k. PCl3 covalent Carbon monoxide calcium bromide disulfur trichloride phosphorus trichloride</p><p> c. NO2 covalent f. SO3 covalent i. Rb2O ionic l. Ga2S3 ionic Nitrogen dioxide sulfur trioxide rubidium oxide gallium sulfide</p><p>Adapted from Dawn Wakely, Lindberg High School, 1999 19. Write the name or formula for the following (both ionic and covalent compounds).</p><p> a. Aluminum chloride h. dinitrogen pentoxide o. MnO2</p><p>AlCl3 N2O5 manganese(IV) oxide</p><p> b. Cobalt II chloride i. Cobalt p. cobalt III fluoride</p><p>CoCl2 Co CoF3</p><p> c. Al2S3 j. N2O3 q. CCl4 Aluminum sulfide dinitrogen trioxide carbon tetrachloride</p><p> d. HgO k. iron II chlorate r. aluminum nitrate</p><p>Mercury(II) oxide Fe(ClO3)2 Al(NO3)3</p><p> e. CS2 l. Cr2O3 s. Ni3P2 Carbon disulfide chromium(III) oxide nickel(II) phosphide -3 f. CO m. CO3 t. NO2 Carbon monoxide carbonate ion nitrogen dioxide</p><p>-2 g. Oxygen gas n. SO3 u. PO5</p><p>O2 sulfite phosphorus pentoxide</p><p>20. Write the formula or name of the following (both ionic and covalent compounds).</p><p> a. C2O4 f. Sn(NO3)2 k. dinitrogen tetroxide</p><p>Dicarbon tetroxide tin(II) nitrate N2O4</p><p> b. Copper II chloride g. K2Cr2O7 l. potassium oxalate</p><p>CuCl2 potassium dichromate K2C2O4</p><p> c. Al(NO3)3 h. Ni2C2O4 s. Hg(NO3)2 Aluminum nitrate nickel(I) oxalate mercury(II) nitrate</p><p> d. CuCO3 i. Aluminum fluoride n. XeCl4</p><p>Copper(II) carbonate AlF3 xenon tetrachloride</p><p> e. H2CO3 j. vanadium IV carbonate o. Bi(NO3)2</p><p>Carbonic acid V(CO3)2 bismuth(II) nitrate</p><p>21. What is the difference between a(n) atom, molecule, element, compound, and a mixture? Give an example of each. </p><p>22. Give an example of the following:</p><p> a. A radical d. a nonmetal atom g. a metal atom j. a metal ion</p><p> b. A negative radical e. a compound h. an anion k. diatomic gas</p><p> c. A metal ion f. a transition metal i. A positive radical m. a mixture</p><p>23. Explain clearly the difference between Co and CO. Co is cobalt a single element. There is only one capital letter. The small o goes with the big C. CO is 2 capital letters and therefore 2 different elements. C is for carbon & O is for oxygen. </p><p>Adapted from Dawn Wakely, Lindberg High School, 1999</p>