Concept explainers
a. Draw these structures.
b. Find the molecular orbital in Figure 5.32 that shows this delocalization and explain yourchoice.
c.
d. What is the relationship between the orbitals identified in Parts b and c?
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Inorganic Chemistry
- The formula for nitryl chloride is CINO2 (in which N is the central atom). a.Draw the Lewis structure for the molecule, including all resonance structures. b.What is the N-O bond order? c.Describe the electron-pair and molecular geometries and give values for all bond angles. d.What is the most polar bond in the molecule? Is the molecule polar? e.The computer program used to calculate electrostatic potential surfaces gave the following charges on atoms in the molecule: A =-0.03, B = -0.26, and C = +0.56. Identify the atoms A, B, and C. Are these calculated charges in accord with your predictions?arrow_forwarda. Predict the molecular structure and bond angles for ClO4¯. Approximate bond angles are sufficient. Molecular Structure = Bond Angles b. Predict the molecular structure and bond angles for PO3³-. = Approximate bond angles are sufficient. Molecular Structure = Bond Angles =arrow_forward5.a. Explain how the lattice energy of an ionic compound such as KCI can be determined using the Born-Haber cycle. On what law is this procedure based? How do the ionization energy and the electron affinity determine whether atoms of elements will combine to form ionic compounds? b. Explain in molecular orbital terms the changes in H-H inter-nuclear distance that occurs as the molecular H2 is ionized first to H2* and then to H2²*. Explain why the bond order of N2 is greater than that of N2*, but the bond order of 02 is less than that of O2*.arrow_forward
- Do the Lewis structure of Urea (NH2)2CO 1. lewis structure2. assign the VSEPR model of the central atom3. Value of the corresponding theoretical angle4. classify 3 of the different bonds around the central atom as ionic or covalent5. draw the complete 3-D structure with respect to the central atom (s)6. draw the lewis structure for another mnolecule or species with a different atomic arrangementarrow_forward4. Answer the following questions about the molecules SbF5^2-.a. Draw the Lewis structure.b. Write the valence shell electron configuration for Sb^2-.c. Draw the valence orbital diagram for Sb^2-.d. Draw the hybridized orbital diagram for Sb^2-.e. Give a bond description for each bond in the molecule.arrow_forward1.You have made structures of NH3 and H2CO molecules in the Part A of your lab report.Both NH3 and H2CO molecules have three electron groups around the central atom.However, their molecular geometries are not the same. Explain this difference. 2. Draw the Lewis electron dot structure for SCl2 and discuss its molecular geometry. IsSCl2 molecule polar or nonpolar? Explain your answer.arrow_forward
- For the following molecules: A. XeO₂F2 (neutron diffraction experiment by Peterson, Willett and Huston.[¹] showed that F-Xe-F bond angle is 180°) B. CIF 3 (1) Draw the valid Lewis structure, identify the (2) molecular group geometry, (3) electron group geometry, (4) polarity of the bonds, (5) over-all polarity, (6) number of lone pairs, and (7) number of bonding pairs.arrow_forwardDraw the lewis structure for PCl3. Does this molecule have a dipole. Why or Why not?arrow_forward3. Draw the most appropriate Lewis structure(s) for the ion BH. What is the electron domain geometry and the molecular geometry? Does the molecule have a dipole? What is the hybridization of the central atom? How many o and n bonds are there?arrow_forward
- Draw the Lewis Structure of carbonate ion, CO32-. Please include the resonance structures and the formal charges on each atom. Consider the compound: sulfur tetrafluoride. a. Draw the Lewis Structure, b. What is its AXE notation? c. What is its Molecular geometry? d. What is its Electron pair geometry? e. Is it polar or non-polar? 3. Consider the Ne2 molecule. a. Draw its molecular orbital diagram, b. Compute the bond order, c. Is it more stable compared to its non-bonded form?arrow_forwardBiotin is being studied in a lab. a. What is the IMF(s) of biotin (C10H16N2O3S)? b. What are the sigma/pi bondings and bond angles of biotin? c. What are the resonance functional groups?arrow_forwardConsider bonding in elemental oxygen and elemental sulfur. a.Why is O2 more stable as a diatomic molecule than S2? b.Why does S8 form much more stable ring structure than O8?arrow_forward
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