Chapter 1.14, Problem 38P

Atom A has 4 valence electrons. Atom Z has 6 valence electrons.  For the AZ3-2 ion How many valence electrons are in the structure?       b. How many single bonds are in the structure?     c. How many double bonds are in the structure?      d. How many triple bonds are in the structure?     e. How many lone pairs are on the central atom in the structure?   f. What is the shape of the structure?      g. What are the bond angles of this ion?

Answer the following questions about acetonitrile (CH;C=N:). c. In what type of orbital does the lone pair on N reside? d. Label all bonds as polar or nonpolar. a. Determine the hybridization of both C atoms and the N atom. b. Label all bonds as o or r.

Which of these bonds will be polar? A. S-H B.N-H C.N-O D.O-O E. Both C and D

Do all of the following for each molecule or ion. a. Draw the Lewis Dot structure that minimizes formal charges. b. Draw the 3-D structure. c. Determine the Hybridization designation. d. Determine the VSEPR designation. e. State what is its Molecular Geometric shape and state the bond angles. f. Determine whether it is Polar (P) or Non-polar (N).     1. CS2 2. CH2O 3. IF3 4. BrF4^-1 5. SeO4^-2

. Draw the Lewis diagram for acetamide. ( CH3CONH2)                                                                                        a. What is the electron geometry around each of the two carbon atoms.                                                  b. What is the hybridization type of each of the carbon atoms.                                                               c. What are the bond types and orbitals involved in bonding for all bonds between the C and O atoms.

Predict the geometry around each highlighted atom.

A. CHF i. Best Lewis Structure B. HNO (H is connected to one of the O's) i. Best Lewis Structure ii. Electron geometry on the C atom ii. Electron geometry on the N atom iii. Approximate bond angles about the C atom iii. Approximate bond angles around the N atom v. Draw the shape with in and out wedges (as necessary) and dipole arrows around the C atom. v. Draw the shape with in and out wedges (as necessary) and dipole arrows around the N atom. vi. Is the molecule polar or nonpolar? vi. Is the molecule polar or nonpolar?

Benzene is especially stable due to   a. the electrons of the double bonds are delocalized b. its planar shape c. the total number of carbons in the molecule d. each carbon has four bonds

1. Draw a single valid Lewis structure for the molecule. 2. Identify the number of charge clouds around the central atom. 3. Identify the approximate bond angle of the charge clouds around the central atom.4. Identify the molecular geometry corresponding to the bond angles.5. classify as polar or nonpolar