2. For each of the following compounds: a. Draw a Lewis structural diagram b. Using electronegativity, predict whether bonds will be polar or nonpolar c. Using bond polarity and shape, predict whether the molecule will be polar or nonpolar d. Identify the greatest Intermolecular force present Molecule CS₂ NHS Structural Diagram (include bond polarity and partial or full charges) Bond Type (ionic/polar covalent/ nonpolar covalent) Molecule Type Intermolecular (ionic/polar Force /nonpolar)

The following five questions relate to this structure. All bonding pairs have been drawn, but lone pairs have been left out. Which atom(s) is/are expected to carry a partial negative charge in this structure? a. ND and OB b. OB only c. CE only d. CC and CE e. CC only f. ND only   How many lone pairs are on Atom D? What is the steric number of atom C? What is the molecular geometry around atom A? a. See-saw b. Trigonal planar c. Tetrahedral d. Square planar   Rank the given bond angles from largest to smallest. H—CF—CE            OB—CC—CA            H—CA—H

2. This question uses sulfur trioxide and the sulfite ion and sulfur trioxide a. Draw both Lewis structures. b. Give the shape and geometry of each structure.

Steps for Lewis Structures: 1. Determine the total number of valence electrons. Add electrons for negative charges, subtract electrons for positive charges. 2. Place least electronegative atom (except H) as central atom in structure. 3. Connect atoms by singles bonds. Each single bond = 2 electrons. 4. “Sprinkle” remaining electrons around outside atoms first to complete octets. Don’t use more electrons than the total found in step 1. Then complete the central atom’s octet last if you have enough electrons. 5. Make double or triple bonds as needed to complete octets. 6. Place brackets and charge for ions. For the central atom in each formula, draw the Lewis Structure with all valence electrons shown. 1. PH3 2. H2O 3. CO2 4. CHCl3 5. O2 6. N2 7. CF4 8. C3H8 9. CH3COOH 10. N2O 11. OCN-

Which of the following best describes electronegativity trends in the periodic table?I.   Electronegativity inreases from right to left across a period.II.  Electronegativity inreases from left to right across a period.III. Electronegativity inreases from bottom to top within a group.IV. Electronegativity inreases from top to bottom within a group. Select one: a. I and III b. I and IV c. II and III d. II and IV e. None of these.

SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question. 1. Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example.

question 7

12. For the following compound, select the total number of hydrogen alloons present in the compound so that each carbon would satisfy the octet rule c-c-c-c Ca A. 12 H atoms B. 10 H atoms C&H atoms D. 6 H atoms