CH301H
- Principles of Chemistry I: Honors Fall 2017, Unique 50135 Homework, Week 3 |

Homework,
week
3 Answer key 1. From data in Tables 3.1 and 3.2, determine the bond dissociation energy for NaCl, which has an equilibrium bond length of 2.36 Å. 2. Draw the Lewis dot structure of each of the following molecules, including all resonance structures. Determine the formal charge on each atom. a) P _{4}b) HNO c) XeF ^{+}d) XeF _{2}e) SCN ^{-}f) H _{3}NBF_{3}g) CH _{3}COO^{-}h) HCO _{3}^{-}3. Ozone (O _{3}) has a nonzero dipole moment.
Draw the lewis dot structure of O_{3} and determine
which of the following structures are possible for the molecule:
linear and symmetric, linear and nonsymmetric, or bent.4. Arrange the following covalent diatomic molecules in order of a) increasing bond length and b) increasing bond energy: BrCl, IBr, BrF. 5. For each of the following pairs of molecules, determine which molecule has the higher vapor pressure at room temperature. a) CI _{4} versus KIb) BaF _{2} versus OF_{2}c) SiH _{4} versus NaH6. In the water molecule, each O-H bond has a dipole moment. Because of the structure of the molecule, these two bond dipole moments lead to a molecular dipole moment. Show that the molecular dipole moment of water is twice the O-H bond dipole moment multiplied by the cosine of the angle between the O-H bonds divided by 2. The molecular dipole moment of water is 1.86 D. What is the O-H bond dipole moment? |