<p> Chemical Bonding Worksheet #1 (Ionic Bonding) 1. Write the noble gas electron configuration for the following: a. nitrogen atom b. sodium atom c. sulfur atom d. bromine atom</p><p>2. How many valance electrons do the above atoms have? Label that next to each configuration. </p><p>3. Draw the Lewis valance electron dot structures for the following atoms:</p><p> a. nitrogen atom b. sodium atom c. sulfur atom d. bromine atom</p><p> e. magnesium atom f. aluminum atom g. carbon atom h. neon atom</p><p>4. Why do atoms become ions?</p><p>5. How many valance electrons are needed in order for an atom or ion to be stale? (What are the “magic” numbers?)</p><p>6. Which type of atom will always lose valance electrons to become an ion?</p><p>7. Which type of atom will always gain valance electrons to become an ion?</p><p>8. When the following become IONS what will the charge be? a. nitrogen b. sodium c. sulfur d. bromine e. magnesium f. aluminum </p><p>9. Define Ionic Bond:</p><p>10. Draw the electron dot structures showing the transfer of electrons that occurs when the following form ionic compounds: a. calcium and bromine b. potassium and bromine</p><p> c. strontium and sulfur d. potassium and chlorine</p><p> e. magnesium and fluorine f. barium and iodine</p><p> g. sodium and nitrogen h. rubidium and phosphorus</p><p>11. What is the net charge on each of the above compounds?______Why? Chemical Bonding Worksheet #2 (Types of Bonds) 1. Determine the type of bond (ionic, polar covalent, or nonpolar covalent) that will form between the following atoms. a. Ca and Cl b. C and S c. Mg and F d. N and O e. H and O f. S and O g. Br and Cl h. F and O i. P and S j. H and Cl k. C and H l. H and H</p><p>2. Using the table of electronegativity values, calculate the EN difference for the atoms that bonded in the following table. Then state whether the bond is nonpolar covalent, polar covalent, or ionic. State which atom has the greater EN, and in your drawing show which atom is partially positive or partially negative. Chemical Bonding Worksheet # 3 (Molecular/Covalent Dot Structures) Formula EN difference Type of bond Atom with Drawing and Shape greater EN</p><p>PCl3</p><p>Br2O</p><p>SCl2</p><p>Br2</p><p>CF4</p><p>Na2S</p><p>CaO 1. The following molecules have only single covalent bonds. Draw a Lewis structure for each. a. H2O b. PCl3</p><p> c. NH3 d. CCl4</p><p> e. HCl f. H2S</p><p> g. Cl2 h. NI3</p><p> i. F2 j. PF3</p><p> k. CBr4 l. SeI2 </p><p> m. SeBr2 n. PBr3</p><p> o. ClAt p. CI2Br2</p><p>2. The following structures may have a double, triple, or coordinate covalent bond. Draw Lewis structures for each. a. CO2 b. HCN</p><p> c. N2 d. SO3</p><p> e. SO4 f. CS2</p><p> g. As2 h. O3</p><p> i. CO</p><p>Chemical Bonding Test Review 1. Define ionic bonding:</p><p>2. Devine covalent bonding:</p><p>3. Determine if the following bonds are covalent or ionic (determine which ones are metals and which ones are nonmetals and then use that info to determine bond type): a. C-H b. F-F c. Li-Br d. O-Si e. K-I</p><p>4. Determine if the following atoms will lose or gain electrons when forming ionic bonds </p><p>Na Mg F S</p><p>5. Draw the dot structure for the following covalent compounds. State the molecular shape or structure (linear, bent, trigonal planar, trigonal pyramidal, or tetrahedral).</p><p>H2O CH4 CO2 SO3</p><p>NF3 F2 N2</p><p>6. Draw the dot structure for the following ionic compounds:</p><p>NaBr Al2O3 CaBr2 MgO</p><p>7. Write the noble gas electron configuration for the following: b. nitrogen atom b. sodium atom c. sulfur atom d. bromine atom</p><p>8. How many valance electrons do the above atoms have? Label that next to each configuration. </p><p>9. Draw the Lewis valance electron dot structures for the following atoms:</p><p> a. nitrogen atom b. sodium atom c. sulfur atom d. bromine atom</p><p>10. How many valance electrons are needed in order for an atom or ion to be stale? (What are the “magic” numbers?)</p><p>11. Which type of atom will always lose valance electrons to become an ion?</p><p>12. Which type of atom will always gain valance electrons to become an ion?</p><p>13. When the following become IONS what will the charge be? a. nitrogen b. sodium c. sulfur d. bromine e. magnesium f. aluminum </p>