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- 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?Compare Figs. 4-47 and 4-49. Why are they different? Because B2 is known to be paramagnetic, the 2p and 2p molecular orbitals must be switched from the first prediction. What is the rationale for this? Why might one expect the 2p to be lower in energy than the 2p? Why cant we use diatomic oxygen to help us decide whether the 2p, or 2p, is lower in energy?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?
- VSEPR: Molecular Geometry 1. For the following molecules: 1) draw a Lewis Dot structure, including contributing resonance structures, if present; 2) use VSEPR to draw an appropriate structure; 3) give an appropriate designation for the ideal molecular geometry; 4) describe any deviations to the ideal molecular geometry; *don't worry about corrections for e and h. d. SF4 e.* CHŞN f. H;COUse the References to access important values if needed for this question. Sigma Bonding Ao bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. sp3 hybrid orbital Example: Sigma Bonding in methane, CH. 1s orbital What atomic or hybrid orbitals make up the sigma bond between C, and Cl in dichloroethylene, CH,CC1, ? (C, is the second carbon in the structure as written.) orbital on C, + orbital on Cl What is the approximate C1-Cz-Cl bond angle ?Predict the hybridization and geometry around each highlighted atom. а. b. С. d. е. =NOCH3
- VSEPR: Molecular Geometry 1. For the following molecules: 1) draw a Lewis Dot structure, including contributing resonance structures, if present; 2) use VSEPR to draw an appropriate structure; 3) give an appropriate designation for the ideal molecular geometry; 4) describe any deviations to the ideal molecular geometry; *don't worry about corrections for e and h. g. HOCI h.* SO;2 i. NO2*Which of the following bonds possesses the largest dipole moment? а. О- Н b. S-H c. N-H d. C-HThe C-N single bond (indicated by the highlighted portion) is a bond. It is formed from the overlap of orbitals on C with orbitals on N. Hint: Do not forget the implicit lone pair of electrons. sp hybrid sp2 hybrid sp3 hybrid sp3d hybrid pz unhybrid dxy unhybrid s unhybrid H sigma pi H. N С —н H. N. N Z-I
- Consider the molecule OA || H;CA- CB – OBH 1. Indicate the hybridization employed by each central atom. CA : b. Св: а. OA : d. Ов: с. 2. Indicate the electron pair geometry about each central atom. CA : b. Св: а. OA : d. Ов: с. 3. Indicate the predicted bond angles around each central atom having more than one bond. CA : b. Св: Ов: а. с. 4. Describe all the o and t bonds in this molecule in the form of a hybridization and bonding scheme. For example, a hypothetical O-H bond = 0 (2 sp) – H (1 s). sigma bond(s) pi bond(s) 5. Which bond is the: а. shortest? b. strongest?e. 16. XeF a. C. d. e. Lewis structure Drawing of shape (label angles) Name of shape. Polar or nonpolar? HybridizationMolecule C2H2 SFs- NO3- Lewis structure include lone pairs & formal charges on each atom Resonance structures don't have to include lone pairs; write N/A if there are none Electron Geometry Hybridization on central atom Overlapping orbitals O: O: include value of n in the orbital name (e.g. 1s, not s). Write N/A if that kind T: of bond is not present in T: the molecule Molecular Geometry Bond angle(s) include < as necessary 3D structure and polarity don't have to include lone pairs; draw the dipole arrow on the molecule or write "non- polar"