Chapter 7: Ionic Bonding and Ionic Naming Test date: In-Class Quiz: Moodle 7 Quiz:

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1 Chapter 7: Ionic Bonding and Ionic Naming Test date: In-Class Quiz: Moodle 7 Quiz: preap Learning Objectives Relate ion charge to position on periodic table and predict charge on a monatomic ion. Name common polyatomic ions, know their formulas and charges. Given an ionic compound formula, write the correct name including any variable charges. Given an ionic compound name, write the correct formula including accounting any variable charges. Explain variable charge and memorize the charges and names of some common variable metals. Given a periodic table, identify the metals which have more than one charge. Note placement of the metal ions and nonmetal ions in ionic compounds. Define ionic compound and list 5 characteristics of these types of compounds. Differentiate between ionic compound and covalent compound given the formula. *Explain the meaning and significance of electrolytes.* *Observe colors of 24 ionic compounds, identify patterns between colors and periodic table * *Correctly write products of a double replacement reaction involving two ionic reactants.* *Mix the two ionic solutions and observe the formation of the ionic products.* *Define crystal lattice, formula unit, lattice energy. Relate lattice energy to position on periodic table* *Predict relative melting points of various ionic compounds based on lattice energy. * Determine the molar mass of an ionic compound. Convert between moles, formula units, and ions. Convert between moles and mass. Convert between mass, formula units and ions. Apply the rules of sig figs when solving for your answers. PreAP Extensions: SWBAT: Name Acids SWBAT: Predict the formula for a polyatomic ion that they have never seen before SWBAT: Write the formula for complex polyatomics (ex: hydrogen sulfate) SWBAT: Explain the reason for a polyatomic ion s charge SWBAT: Give an in depth explanation for the mechanism of ionic bonding and electrostatic attraction. Concepts Forming Chemical Bonds The Formation and Naming of Ions Fixed vs. Variable charges Monatomic vs Polyatomic Ions The Formation and Nature of Ionic Bonds TEKS c.7 Science concepts. The student knows how atoms form ionic, metallic, and covalent bonds. The student is expected to: c.7.a Name ionic compounds containing main group or transition metals, covalent compounds, acids, and bases, using International Union of Pure and Applied Chemistry (IUPAC) nomenclature rules; c.7.b Write the chemical formulas of common polyatomic ions, ionic compounds containing main group or transition metals, covalent compounds, acids, and bases; c.7.c Construct electron dot formulas to illustrate ionic and covalent bonds; c.7.d Describe the nature of metallic bonding and apply the theory to explain metallic properties such as thermal and electrical conductivity, malleability, and ductility; 1

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3 7.1 Ion Formation Practice Problems For each of the following atoms, write the electron configuration, referring to the periodic table. Then write the formula of the ion the atom is most likely to form and identify that ion as a cation or an anion. Finally, write the electron configuration of the ion. 1. bromine (Br), element 35 2.gallium (Ga), element sulfur (S), element rubidium (Rb), element Ionic Bonds and Ionic Compounds Practice Problems Write the most likely ions for the atoms in each pair, referring to the periodic table as necessary. Then determine the ratio of the atoms in the ionic compound formed in each case. 5. aluminum (Al) and fluorine (F) 6. lithium (Li) and oxygen (O) 7. beryllium (Be) and selenium (Se) 8. gallium (Ga) and sulfur (S) 7.3 Names and Formulas for Ionic Compounds Practice Problems Write the correct formula for the ionic compound formed between atoms of each of the following pairs of elements. 11. sodium (Na) and sulfur (S) 12. magnesium (Mg) and nitrogen (N) 13. potassium (K) and phosphorus (P) 14. barium (Ba) and fluorine (F) 15. aluminum (Al) and nitrogen (N) Write the correct formula for the ionic compounds that contain the following ions. Refer to a table of polyatomic ions as necessary. 16. sodium and phosphate 17. ammonium and carbonate 18. aluminum and chromate 19. calcium and hydroxide 3

4 Practice Problems Name the ionic compounds that have the following formulas. 20. NH 4I 21. NaBrO Mg(NO 3) KHSO NH 4ClO Al(ClO) FeF 2 Practice Problems Write the symbol and charge for these ions: 1. sodium ion 6. chloride 11. chlorate 2. calcium ion 7. oxide 12. sulfate 3. aluminum ion 8. nitride 13. nitrate 4. lithium ion 9. carbide 14. carbonate 5. magnesium ion 10. fluoride 15. phosphate What patterns do you see in the names? Name these ions: 16. Br K Sn P S SO CrO * OH 1- Polyatomic ions Fill in the Blanks hypo ite -ite -ate per - ate No nitrate NO 1-3 Mean permanganate MnO 1-4 Clowns hypoclorite ClO 1- Cook Soft Caramel chromate CrO 2-4 Popcorn Other Polyatomic Ions you must know: (see your yellow memory sheet) hydroxide ammonium acetate bicarbonate dichromate cyanide bisulfate biphosphate iodate Variable ions: FeO vs Fe 2O 3 PbSO 4 vs Pb(SO 4) 2 Variable ions = 4

5 Write chemical formulas for the compounds in each box. The names are found by finding the intersection between the cations and anions. Example: The first box is the intersection between the zinc cation and the chloride anion, so you should write ZnCl 2, as shown. Chloride ZnCl 2 Zinc iron (II) iron (III) gallium silver lead (IV) Acetate Nitrate Oxide Nitride Sulfate Write the names for the following compounds: 1) CuCl 2 2) LiC 2H 3O 2 3) V 2Se 3 4) Mn 3N 4 5) BeO 6) Na 2SO 4 7) AlAs 8) KMnO 4 9) Cr(CN) 6 10) SnSO 3 11) VF 5 12) NH 4NO 3 Vocabulary: Bond = Ionic Bond = Coefficient = Subscript = Binary = Ternary = Oxyanion = Polyatomic ion= Anion= Cation= 5

6 Fill in the blank with the missing information: 1. copper (II) hydroxide 24. ZnCrO 4 2. tin (IV) oxide 25. Sn 3S 4 3. strontium selenide 26. FeCO 3 4. strontium chloride 27. Zn 3(PO 2) 2 5. lead (IV) persulfate 28. (NH 4) 2CO 3 6. cadmium bicarbonate 29. Cu(OH) 2 7. magnesium phosphate 30. K 3N 8. cadmium cyanide 31. Mg 3(PO 3) 2 9. zinc hypochlorite 32. (NH 4) 3P 10. ammonium phosphide 33. SnCl tin (II) permanganate 34. GaAs 12. iron (II) chloride 35. FePO 5 Name the following compounds: KI Given the name, write the formula: Iron (II) Iodide CuIO 3 Copper (II) Phosphide SnI 2 Beryllium Nitrate Fe 2Se 3 Magnesium Oxide CaSeO 5 Potassium Chlorate FeSe Tin (IV) Sulfate 6

7 Nomenclature Worksheet 1 Simple Binary Ionic Compounds Directions: Please complete the following table. Name of Ionic Compound 1. Sodium bromide 2. Calcium chloride 3. Magnesium sulfide 4. Aluminum oxide 5. Lithium phosphide 6. Cesium nitride 7. Potassium iodide 8. Barium fluoride 9. Rubidium nitride 10. Barium oxide 11. K 2O Formula of Ionic Compound 12. MgI AlCl CaBr Na 3N 16. LiF 17. Ba 3P Cs 2S 19. SrF NaCl Directions: Complete each of the following tables. LiBr # of Li atoms # of Br atoms Al 2S 3 # of Al atoms # of S atoms 3 Al 2S 3 # of Al atoms # of S atoms 2 LiBr # of Li atoms # of Br atoms Ca 3P 2 # of Ca atoms # of P atoms 2 Ca 3P 2 # of Ca atoms # of P atoms 7

8 Nomenclature Worksheet 2 Ionic Compounds Containing Polyatomic Ions Name of Ionic Compound Formula of Ionic Compound 1. Sodium chromate 2. Calcium carbonate 3. Magnesium nitrate 4. Aluminum sulfate 5. Lithium phosphate 6. Ammonium chloride 7. Cesium chlorate 8. Potassium sulfate 9. Barium acetate 10. Rubidium cyanide 11. KC 2H 3O Mg 3(PO 4) Al(ClO 3) CaSO Sr(HCO 3) NaNO Li 2CO Ba(NO 3) Cs 2CrO NH 4OH Directions: Complete each of the following tables. KC 2H 3O 2 # of K atoms # of C atoms # of H atoms # of O atoms Mg 3(PO 4) 2 # of Mg atoms # of P atoms # of O atoms 3 KC 2H 3O 2 # of K atoms # of C atoms # of H atoms # of O atoms 2 Mg 3(PO 4) 2 # of Mg atoms # of P atoms # of O atoms 3 Al(ClO 3) 3 # of Al atoms # of Cl atoms # of O atoms 8

9 Nomenclature Worksheet 3 Ionic Compounds Containing Transition Metals Name of Ionic Compound 1. Copper (II) sulfate Formula of Ionic Compound 2. Copper (I) oxide 3. Chromium (III) cyanide 4. Cobalt (II) hydroxide 5. Silver bromide 6. Zinc nitrate 7. Iron (III) acetate 8. Lead (IV) sulfate 9. FeCl PbSO Co 2(CO 3) AgNO Zn(CN) CuClO Cr(OH) Hg 2O 17. Gold (I) nitride 18. AuPO Manganese (II) nitrite 20. Tin (IV) dichromate 21. Sn(OH) Mn 2(SO 4) Zinc phosphide 24. Ni (NO 3) NiPO What is the difference between a subscript behind an atom and a subscript behind a parenthesis? 27. Why is it always important to determine the charge of the anion when writing names of ionic compounds involving transition metals? 9

10 Name the following compounds: Nomenclature Worksheet 4 Ionic Compounds Summary Give the formula for each compound: Symbol 1. CaF 2 2. Na 2O 3. BaS 4. CuSO 4 5. Fe 2O 3 6. HgCl 2 7. AgNO 3 8. MgCO 3 9. KC 2H 3O K 2Cr 2O Al(OH) PbBr ZnSO NaHCO NH 4Cl 16. Li 3PO SnCl Al(NO 2) Rb 2CrO KMnO CuCl 22. FeSO 4 Name Symbol Name 23. Sodium fluoride 24. Potassium sulfide 25. Calcium carbonate 26. Magnesium hydroxide 27. Zinc nitrate 28. Silver acetate 29. Copper (II) oxide 30. Iron (III) chloride 31. Barium chromate 32. Aluminum oxide 33. Lead (II) sulfate 34. Tin (IV) oxalate 35. Calcium phosphate 36. Lithium permanganate 37. Mercury (I) nitrate 38. Radium sulfite 39. Chromium (III) chloride 40. Ammonium sulfide 41. Copper (II) acetate 42. Calcium bicarbonate 43. Tin (II) oxide 44. Silver sulfite Directions: Predict the products if given these reactants. 1. Al(NO 2) 3 and CaI 2 2. FeSO 4 and ZnS: 3. Au(BrO 3) 3 and KNO 3: 4. RbCl and Ni 3(PO 4) 2: 5. Sn 3N 4 and MgSO 4: 6. Pb(SO 3) 2 and AlP 10

11 NAMING COMPOUNDS MIXED PRACTICE Write the correct name or formula for each of the following acids, ionic compounds or covalent molecules. 23. Ca(NO 2) 2 1. HNO Ag 3PO 4 2. KClO magnesium bromide 3. FeCl silver phosphide 4. Hg(NO 2) barium nitrite 5. K 2SO chromium(iii) carbonate 6. PCl Lead (IV) chloride 7. ZnS 33. sodium sulfate 8. Al(ClO 3) nickel (III) sulfate 10. K 3PO potassium sulfate 12. PbS 38. ammonium nitrate 13. Na 3N 39. lead (II) hydroxide 14. BaSO calcium phosphate 15. KCl 43. aluminum phosphide 16. Al 2(SO 4) iron(iii) sulfide 17. Li 2SO potassium acetate 20. ZnCO tin (II) nitrate 21. SnI copper (I) oxide 22. Cu 2CO gold (III) phosphite Ionic Compounds and the Mole Directions: Determine how many moles of cations and anions are in each of the following: 7. 1 mole aluminum nitrite: 8. 2 mols of calcium iodide: 9. 3 mols of iron (III) sulfate: mol zinc chlorate: mol gold (III) sulfite: mols of potassium hydroxide: mol magnesium oxide: 11

12 Ionic Compounds and the Mole Notes One-Step Mole and Formula Unit Conversions 1. How many moles are equal to x formula units of FeCl 3? 2. How many formula units are in 10.0 moles of sodium sulfate? Moles, Formula Units and Ion Conversions 3. How many ions of nitrate are in zinc nitrate? 4. How many cations are in potassium phosphite? Molar Mass and Formula Units 5. Find the mass of 1 mole of each of the following substances: a. Aluminum oxide: b. Lead (IV) sulfate: c. Copper (II) hydroxide: d. Silver chloride: One-Step Mole and Mass Conversions 6. What is the mass of 2.25 moles of calcium nitrate? 7. How many moles is equivalent to 15.0 grams of barium hydroxide? Multi-Step Problems with Moles, Formula Units, Ions and Mass 8. What is the mass of 4.2 x formula units of ammonium chloride? 9. How many formula units are in grams of tin (IV) oxide? 10. How many metal ions are present in 15.0 grams of nickel (III) dichromate?

13 Ionic Compounds and the Mole Practice Directions: Show all work where appropriate. Round all answers to the correct number of sig figs. Answer in complete sentences when asked to explain. 1. How do you determine the mass of one mole of an ionic compound? 2. What is the mass of one mole of: a. Sodium carbonate: b. Magnesium bromide: c. Lithium phosphate: 3. Calculate the mass of mols of cobalt (II) nitride. 4. Calculate the number of anions in 1.95 mols of aluminum acetate. 5. Calculate the mass of 3.65 x formula units of calcium phosphate. 6. Determine the number of mols that are equal to grams of chromium (II) chlorite. 7. How many formula units are in 24.3 grams of iron (III) oxide? 8. How many mols is 7.85 x formula units of ammonium sulfate? 9. Which of the following has the most number of cations: 25.0 grams of magnesium acetate, 3.2 mols of iron (III) chloride or 10.0 grams of silver nitride? 10. Which has a greater mass: 2.00 moles of sodium hydroxide, 3.21 x formula units of copper (I) nitrite or 9.55 x formula units of lithium fluoride?

14 Test Review 1. Define the term chemical bond. Account for such bonding in terms of the concept of noble gas configuration. 2. Explain the difference between a cation and an anion in terms of electron transfer. Give an example of each type of ion. 3. Define the term ionic bond. Explain how atoms of potassium (group 1) and iodine (group 17) bond ionically with one another. 4. Explain how to determine the formula for an ionic compound, given its name. 5. Know the following vocabulary: Coefficient Binary Subscript Ternary Polyatomic ion Anion Cation 6. What is meant by a variable cation? Where are they located? Be able to write the formula and name of ionic compounds. Given the following names, write the correct formulas: 7. Iron (III) chloride 14. MnO 2 8. Barium phosphide 15. Fe 2(CrO 5) 3 9. Ammonium chloride 16. Copper (I) oxide 10. Aluminum hydroxide 17. Tin (II) bromide 11. Na 2CO Lithium sulfate 12. NiI Magnesium phosphate 13. GaPO Silver nitrate Given the following formulas, Identify how many atoms of each element are in each compound. 21. Pb(OH) CoCl CdCrO Fe(NO 3) KMnO Ca(HCO 3) 2 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 27. The name for the cation Mg 2+ is: a. manganese ion. b. manganese (II) ion. c. magnesium ion. d. magnesium (II) ion. 28. The name for the anion ClO 2 is: a. chloride ion. b. chlorite ion. c. chlorate ion. d. perchlorate ion. 29. What is the formula of calcium phosphate, which is made up of the ions Ca 2+ and PO 4 3? a. Ca 3PO 4 b. Ca 3(PO 4) 2 c. Ca 6PO 4 d. Ca 2(PO 4) Where do you write a subscript that indicates the number of atoms in a formula? a. to the upper left b. to the upper right c. to the lower left d. to the lower right 31. According to this information, what is the chemical formula for aluminum sulfate? a. AlSO 4 b. Al 2(SO 4) 3 c. Al 3(SO 4) 2 d. Al 6SO 4

15 32. Which of these is not an ionic compound? a. Mg(NO 3) 2 b. Iron (II) phosphate c. Carbon dioxide d. SnCl The chemical formula for calcium chloride is a. Ca 2Cl b. CaCl c. CaCl 2 d. Ca 2Cl Which of the following comparisons of ionic and covalent bonds is NOT true? a. Ionic bonds create ionic compounds; covalent bonds create molecules. b. Ionic bonds are held together by the attraction of opposing charges; the shared electrons hold covalent bonds together. c. Ionic compounds form solid crystals. d. The charges in all covalent compounds must be balanced 35. What is the mass of moles of strontium cyanide? 36. How many formula units are in grams of lead (II) bisulfate? 37. How many cations are in 0.67 moles of gold (I) phosphide? 38. What is the mass of 7.40 x formula units of iron (III) nitrate? 39. What is the molar mass of calcium permanganate? chromium (III) acetate? 40. How many moles is 1.52 x formula units of magnesium bromide? Complete the table below: Formula CaCO 3 LiF NiNO 2 NH 3 ZnO Name calcium carbonate Silver sulfate Magnesium Dichromate Sodium chlorite Chromium (II) oxide