Which bonds allow for a large, bonded network to be more directional and why? 1. Sigma bonds 2. Pi bonds Because 1. The orbitals overlap side-to-side to hold the bond in place. 2. The orbitals overlap end-to-end in several different directions. 3. Multiple of these bonds result in delocalized electrons. O 2,1 O2,2 O 1.3 O 1,2 O 2,3 O 1,1

7. Determine the molecular shape for SO3  ? Z of S =16,  O = 8 a.octahedralb.trigonal pyramidalc.T-shaped.trigonal planar

A. What is the electron-pair geometry for C in CCl4? _______There are _____ lone pair(s) around the central atom, so the geometry of CCl4 is _________.B. What is the electron-pair geometry for P in POCl3? ________There are ______ lone pair(s) around the central atom, so the geometry of POCl3 is ________.

In an alternate universe, these are types of electron cloud shapes a D cloud (shape in blue), and a E cloud (shape in gray). The nucleus is represented by a green circle. All other rules about orbitals and types of bonding are the same as our universe. A В E (one on top of the other) Answer the following questions below in Canvas A. Which orientation of clouds do you think would create the strongest bond and why B. Which orientation of clouds do you think represents a sigma bond and why C. Which orientation of clouds do you think represents a pi bond and why make sure you label which question you are answering

For which of the following molecules will the electron-pair geometry be different than the molecular geometry? Draw Lewis structure for each molecule and write the electron pair and molecular geometries for each one in a separate sheet.      a. BH3   b. H2O   c. CH4   d. CO   e. NH4+