Chapter 6 Chemical Bonding 1. Define electronegativity.

2. How does electronegativity vary as the atomic number of an element increases within the same period of the periodic table?

3. How is the strength of a bond between two elements in a molecule related to their electronegativities?

4. What is the difference between an ionic and a covalent bond?

5. How is the character of a bond (ionic or covalent) between two elements related to their electronegativities?

6. Referring to electronegativit.ies, in your text, arrange the following compounds in order of increasing ionic character of their bonds:

LiBr, KCI, KI, LiF 7. Referring to Tables of electronegativities in your text, classify each of'the following

bonds as either ionic: (I) or covalent (C) a. A1-O f. N-O

b. Al-S g. Na-S c. Bi-CI h. P-O d. Bi-O i. S-O e. C- Cl j. Ti-Br 8. What force holds the two ions together in an ionic bond?

9. What is the meaning of the valence or charge of an element that forms an ionic bond?

H. Cannon, C. Clapper and T. Guillot

Klein High School

Chemical Bonding

10. Given the electron configurations for the following neutral atoms, predict the oxidation number each is most likely to have. Element Configuration Oxidation number A 1s22s22p63s2 B 1s22s22p63s1 C 1s22s22p6 D 1s22s22p5 E 1s22s22p1

11. Write the correct formula for each of the following combinations of elements from question 13. (If no reaction occurs, write none)

a. B and D b. E and D c. A and D d. A and C

12. Underline the atom in each of the following pairs that has the lower electronegativity.

a. Li Na b. Cs Rb c. Cs Ba d. Cl Br e. Fe Ni f. S Cl

13. List four general characteristics of compounds that have ionic bonds

14. Bonds between the which of the following pairs are Al—Cl N—O K—F S—O Ba—Cl Fe—O

15. List three general characteristics of compounds formed entirely by covalent

compounds. _________________________ ________________________________ ________________________________

16. List three characteristics of metals. ___________________________________ ___________________________________ ___________________________________

17. How does the bonding of atoms in a metal differ from the bonding in a nonmetal?

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Chemical Bonding

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Chemical Bonding

Chapter 6 Bonding Worksheet 1) A chemical bond between atoms results

from the attraction between electrons and what else? a. neutrons b. isotopes c. protons d. valence electrons

2) What makes up a covalent bond? a. a shared electron b. two different ions c. an octet of electrons d. a shared electron pair

3) As the electronegativity difference between two atoms bonded together increases, the percentage of what else increases? a. ionic character b. covalent character c. metallic character d. electron sharing

4) Which of the following would describe the electronegativity of an atom with a strong attraction for the electrons they share with another atom? a. high electronegativity b. low electronegativity c. zero electronegativity d. Lewis electronegativity

5) What type of chemical bond results from the electrostatic attraction between positive and negative ions? a. ionic bond b. metallic bond c. polar covalent bond d. nonpolar covalent bond

6) In a crystal of an ionic compound, each cation is surrounded by what? a. molecules b. positive ions c. dipoles d. negative ions

7. ________ What do we call the electrons involved in forming a chemical bond?

8. ________ If a bond’s character is more than 50% ionic, what type of bond is formed?

9. ________ If a bond’s character is more than 50% ionic, what can we say about the electronegativity difference between the two atoms?

10. ________ What is an example of an ionic compound?

11. Name two elements that form compounds that are exceptions to the octet rule.

12. How does the energy of the crystal lattice formed in an ionic compound compare with the energy of the neutral atoms involved in its formation? a. higher in potential energy b. lower in potential energy c. equal in potential energy d. unstable

13. ____ What type of energy best represents the strength of an ionic bond? 14. ____ What type of bonding holds a polyatomic ion together? 15. ____ What type of forces holds two atoms together in an ionic bond?

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Chemical Bonding

Metallic Bonds 1) Which of the following best describes

the valence electrons in metals? a. attached to particular positive ions b. shared by all surrounding ions c. immobile d. involved in covalent bonding

2) Which of these best explains why metals are malleable while ionic crystals are brittle? a. chemical bonds b. London dispersion forces c. heats of vaporization d. polarity

3) How does the strength of metallic bonds vary moving from left to right in any row of the periodic table? a. increases b. decreases c. remains the same

4) How does drawing a metal into a wire affect the metallic bonds? a. break easily b. break with difficulty c. do not break d. become ionic bonds

5. Use the concept of electron configuration to explain why the number of valence

electrons in metals tends to be less than the number in most nonmetals.

6. How does the behavior of the electrons in metals contribute to the distinctive properties of metals?

a. luster

b. conductivity

c. malleability

d. ductility Complete the following table Metallic Ionic Components 7. 8. Overall charge 9. 10. Conductivity 11. 12. Melting point 13. 14. Hardness 15. 16. Malleability 17. 18. Ductility 19. 20.

6-5

HC/CC/TG KHS

Chemical Names and Formulas

Write the balanced ionic formulas:

Na +1

Mg +2

Fe +3

Pb +4

NH4 +1

Cl -1

O -2

P -3

OH -1

SO4 -2

PO4 -3

HSO3 -1

Cr2O7 -2

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Chemical Names and Formulas

Draw dot diagrams for the following compounds: 1. Na + Cl 2. K + Br 3. Ba + F 4. Li + P 5. Mg + P 6. Ra + C! 7. Mg + S 8. Sr + 1 9. Cs + S 10. K + P 11. Ca + 0 12. Fr + F 13. Rb + 0 14. Ba + S

6-7 HC/CC/TG KHS

Chemical Names and Formulas

Binary Ionic Compounds Write the formula for the following:

1. Sodium bromide 18. Zinc phosphide

2. Calcium oxide 19. Chromium (III) oxide

3. Manganese(II) oxide 20. Antimony (V) sulfide

4. Silver (I) Chloride 21. Barium iodide

5. Nickel(III)Bromide 22. Potassium Sulfide

6. Ferric Oxide 23. Stannous oxide

7. Cupric nitride 24. Manganese (IV) fluoride

8. Silver (I) oxide 25. Zinc Sulfide

9. Aluminum nitride 26. Cobalt (II) iodide

10. Aluminum oxide 27. Plumbous Chloride

11. Magnesium sulfide 28. Mercury (I) oxide

12. Chromium (III) phosphide

29. Tin (IV) fluoride

13. Zinc iodide 30. Iron (III) Chloride

14. Ferrous fluoride 31. Tin (II) Sulfide

15. Lithium oxide 32. Copper (I) Bromide

16. Cuprous sulfide 33. Silver (I) iodide

17. Strontium nitride Binary Ionic Compounds *Name using the Latin system

6-8 HC/CC/TG KHS

Chemical Names and Formulas

1. chromium (II) oxide 21. CaBr2 2. strontium bromide 22. AlCl3 3. copper (I) sulfide 23. PbO2* 4. mercuric iodide 24. Co3N2

5. iron (II) sulfide 25. ZnO 6. ferrous fluoride 26. Mn3P4 7. potassium bromide 27. MgI2 8. cuprous oxide 28. AlP 9. iron (II) bromide 29. Fe2O3* 10. silver iodide 30. SnF2 * 11. plumbous phosphide 31. BaS 12. barium sulfide 32. MnO2 13. Lead (II) fluoride 33. NaCl 14. copper (II) chloride 34. HgO* 15. lead (IV) sulfide 35. SnCl4* 16. mercury (II) bromide 36. NiBr2 17. lithium chloride 37. AlI3 18. tin (IV) nitride 38. CuF* 19. mercury (I) nitride 39. B2S3 20. stannous chloride 40. Na2O Ionic compounds Name the following compounds 1. NH4NO2 21. AgC2H3O2

6-9 HC/CC/TG KHS

Chemical Names and Formulas

2. Fe2(SO3)3 22. NaI 3. BaCl2 23. FeSO3 4. FeI2 24. Hg2Cl2 5. CsS 25. Pb(C2H3O2)4 6. Sn(NO3)4 26. NaOH 7. NaHCO3 27. KNO3 8. KCl 28. SrSO4 9. AlN 29. SrSO4 10. Ca3(PO4)2 30. MgSO4 11. Li2O 31. (NH4)3PO4 12. CrCl3 32. CuHCO3 13. Pb(NO3)2 33. CoCO3 14. Cu2S 34. SnSO3 15. Ca(C2H3O2)2 35. Na2CO3 16. Sb2S3 36. NH4CO3 17. Fe(C2H3O2)2 37. NaI 18. Ba(OH)2 38. (NH4)2SO4 19. Ag2SO4 39. Ca(C2H3O2)2 20. MgO2 40. ZnBr2 Naming Compounds Write the name for:

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Chemical Names and Formulas

1. Fe(NO2)2 11. KIO 2. (NH4)2SO4 12. LiCN 3. Ag2SO4 13. CuCl2 4. Zn(NO3)2 14. CuBr 5. NH4Br 15. Fe(NO3)2 6. BaCO3 16. FeCl3

7. Na3PO4 17. SnO2 8. K2CrO4 18. HgCO3 9. FeSO4 19. As(C2H3O2)3 10. (NH4)3PO4 20. NaClO2 Write the formula for: 1. sodium chlorite 11. ammonium dichromate 2. iron (III) perbromate 12. lead (II) acetate 3. calcium chlorate 13. iron (III) oxide 4. calcium hypochlorite 14. cobalt (II) nitrate 5. copper (II) chlorate 15. strontium nitrite 6. cadmium iodate 16. tin (IV) oxide 7. chromium (III) sulfite 17. aluminum phosphate 8. bismuth (III) chromate 18. cobalt (II) hydroxide 9. barium nitrite 19. potassium permanganate 10. aluminum sulfate 20. Iron (II) sulfate

Write the name of the following compounds: 1. Ba(ClO3)2 12. HMnO4

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Chemical Names and Formulas

2. Na3P 13. Mg(OH)2 3. KOH 14. HBr 4. K2SO3 15. CaSO4 5. Al2(C2O4)3 16. Ba(OH)2 6. NH4OH 17. Al(OH)3 7. Cu3(PO3)2 18. HMnO4 8. Li2CO3 19. H2CrO4 9. Ag3PO4 20. Au(OH)3 10. K2SO4 21. NaCN 11. KF 22. K2SO4

6-12 HC/CC/TG KHS

Chemical Names and Formulas

Naming Acids and Bases Name the following compounds: 1. HF 13. HCl 2. HI 14. H2S 3. H3N 15. HBr 4. H3AsO4 16. H3AsO3 5. NaOH 17. H3BO3 6. H3PO4 18. H3PO3 7. HNO3 19. H3P 8. NH4OH 20. HClO3 9. H2Cr2O7 21. HC2H3O2 10. Ca(OH)2 22. H2SO3 11. H2SO4 23. HIO3 12. HIO4 Write the formula for the following: 1. sodium hydroxide 2. barium hydroxide 3. potassium hydroxide 4. calcium hydroxide 5. ammonium hydroxide 6. iron (III) hydroxide 7. cobalt (II) hydroxide 8. gold (III) hydroxide 9. tungsten (IV) hydroxide 10. cesium hydroxide 11. copper (II) hydroxide 12. mercury (I) hydroxide

13 HC/CC/TG KHS

Chemical Names and Formulas

Write the formula of the following compounds: 1. hydrochloric acid 14. hypochlorous acid 2. ammonium hydroxide 15. gold (III) hydroxide 3. barium phosphate 16. phosphoric acid 4. hydroselenic acid 17. acetic acid 5. hydroiodic acid 18. oxalic acid 6. hydrophosphoric acid 19. perchloric acid 7. permanganic acid 20. chlorous acid 8. chloric acid 21. nitrous acid 9. sulfurous acid 22. nitric acid 10. chromic acid 23. phosphorus acid 11. cyanic acid 24. hydronitric acid 12. hydrofluoric acid 25. hydrosulfuric acid 13. silicic acid

14 HC/CC/TG KHS

Naming Compounds Lab #1

Naming Compounds Lab

Purpose: To gain practice in writing formulas and naming compounds. Procedure: Using a spot plate as a reaction vessel, combine the first chemical and the second chemical. Be careful to use the bottle with the correct formula of the chemical named. Record any changes observed following the addition of the second chemical. Be careful not to touch the dropper to the spot plate well. If you do, it will cross-contaminate the reagent bottles. Each solution contains two ions, one positive and one negative. The product that we are interested in will be formed by combination of the underlined ions in the reactants. Reactants Formula Pos.

ion Neg ion

Ppt Color

Formula Name

Copper (II) sulfate 1. Sodium sulfide

Copper (II) sulfate 2. Ammonium hydroxide

Aluminum iodide 3. Ammonium hydroxide

Potassium chromate 4. Ammonium hydroxide

Potassium chromate 5. Silver (I) nitrate

Potassium chromate 6. Lead (II) nitrate

Lead (II) nitrate 7. Sodium phosphate

Aluminum iodide 8. Sodium phosphate

Aluminum iodide 9. Lead (II) nitrate

Aluminum iodide 10. Silver (I) nitrate

Sodium phosphate 11. Silver (I) nitrate

Sodium sulfide 12. Silver (I) nitrate

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