1. ' ) Draw all bonding orbitals (i.e. “balloons" for s, sp, sp², sp³ and л) for the following compounds: a) b) c) H H C... H C=C=CH H H H -CEN

1. Choose the correct atomic orbital overlap for A-D.  2. Rank in order of decreasing energy the pair of electrons indicated as A, B, C & D.

The figure that follows contains ball-and-stick drawings ofthree possible shapes of an AF4 molecule. (a) For each shape,give the electron-domain geometry on which the moleculargeometry is based. (b) For each shape, how many nonbondingelectron domains are there on atom A? (c) Which of thefollowing elements will lead to an AF4 molecule with theshape in (iii): Be, C, S, Se, Si, Xe? (d) Name an element A thatis expected to lead to the AF4 structure shown in (i).

A research student used a new software package to calibrate the electronic map using a material containing only gallium and bromine bonds, Ga and Br. On which atoms might you expect to see the highest electron density?

You hear a student from a nearby group say that “Electron domains repel one another.” Citeevidence from Figure 1.2 to support or refute this statement.

Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?

Consider the following computer-generated model of caffeine: Complete a Lewis structure for caffeine in which all atoms have a formal charge of zero (as is typical with most organic compounds). How many C and N atoms are sp2 hybridized? How many C and N atoms are sp3 hybridized? sp hybridized? How many and bonds are there?

What charge would be needed on F2 to generate an ion with a bond order of 2?

Explain in terms of bonding theory why all four hydrogen atoms of allene, H2CCCH2, cannot lie in the same plane.

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H2O. Switch between the real and model modes. Explain the difference observed.