Objectives: To meet the requirements of Goal I, you must be able to:

1. explain the distinction, on the atomic level, between ionic and covalent molecular compounds; 

2. identify the electrons in a given element most closely involved in bond formation; 

3. for ionic compounds..... 
1. describe an ionic bond, and explain the term lattice energy;
2. use electron configurations to illustrate the formation of ions and ionic bonds, and write chemical formulas for ionic compounds;
3. predict relative lattice energies for ionic compounds;

4. outline the sequence of steps in the formation of a binary ionic compound from its elements (the Born-Haber cycle); name the chemical change occurring in each step, and give the name of the energy change associated with each step;

5. use a Born-Haber cycle with energies known for all steps but one to calculate the unknown energy; 

6. define electronegativity, and; 
1. relate the value for electronegativity assigned to an element related to its position in the periodic table;
2. use electronegativities to decide whether a given compound and/or bond is predominantly ionic or covalent;

7. for covalently bonded elements and compounds... 
1. write and interpret Lewis dot symbols for atoms;
2. combine Lewis dot symbols for atoms into Lewis structures for covalent molecules and ions. [Top]

Objectives: To meet the requirements of Goal II, you must be able to:

8. use the electronegativities of two covalently bonded atoms to identify polar and non-polar covalent bonds;

9. determine the direction of polarity and compare the degree of polarity among polar covalent bonds; 

10. state the bond order of any bond illustrated by a Lewis structure and compare bond lengths and bond energies for single, double and triple bonds;

11. recognize and write resonance structures for appropriate molecules and ions; 

12. identify and explain based on theory the exceptions to the octet rule; 

13. use the Valence Shell Electron Pair Repulsion Model (VSEPR) to predict the shapes of covalently bonded molecules and ions and to write stereochemical formulas to represent these three-dimensional molecular shapes. (Fig. 10.5, 10.6, 10.7, 10.8, 10.9, 10.10, 10.11);

14. predict polarity and identify whether or not a covalently bonded molecule has a dipole moment, based on its shape. [Top] 

Objectives: To meet the requirements of Goal III, you must be able to: 

15. analyze the structural formula of a covalently bonded molecule or ion, for: 
1. the total number of covalent bonds represented;
2. the number and position of sigma and pi bonds;
3. the presence of unshared electron pairs (lone pairs);

16. understand the two fundamental concepts of the valence bond model: 
1. bond formation by overlap of atomic orbitals;
2. hybridization of atomic orbitals;

17. reproduce the energy level diagrams for a carbon atom in sp³, sp², and sp hybridization; identify the orbitals involved in sigma bonds and in pi bonds in each of these hybridizations;

18. extend the concept of orbital hybridization to molecules and ions with a central atom other than carbon; 

19. interrelate: Lewis diagram, VSEPR-derived stereochemical structural formula hybridization of atomic orbitals, sigma and pi bonding, bond angles and geometry. (Sample Problems 10.1-10.5 illustrate these relationships.) [Top]