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Q: Use molecular orbital theory to predict if each molecule or ion exists in a relatively stable form.…
A: Use molecular orbital theory to predict if each molecule or ion exists in a relatively stable form.…
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- The bond angles in antimony trifluoride are 87°. Describe the bonding in SbF3, including a picture of the orbital overlap interaction that creates the Sb-F bonds. ✓orbitals from the inner atom. An outer halogen atom always uses one of ✓valence orbitals, and fluorine has n = vvalence orbitals, Bond angles near 90° signal interactions of valence its valence ✓orbitals to form a bond. Antimony has n = so each of the three bonds in SbF3 can be described as resulting from overlap between a orbital from F. There are three vorbital from Sb and a bonds that point at near-right angles to one another.Platinum hexafluoride is an extremely strong oxidizing agent. It can even oxidize oxygen, its reaction with O2 giving O2+PtF6−.a. Sketch the molecular orbital energy level diagram for the O2+ ion.b. How many net σ and π bonds does the ion have?c. What is the O-O bond order?d. How has the bond order changed on taking away electrons from O2 to obtain O2+?e. Is the O2+ ion paramagnetic?42. [BiF7] and [SbF6]³- ions have pentagonal bipyramidal and octahedral structures, respectively. Are these observations consistent with the VSEPR predictions. F Bi-F F F FIF Sb F F Hint: Remind yourself of the VSEPR models. Take the number of valence electrons of the central atom, add/substract the electrons from the charge, substract the number of bonding pairs from this number, if this turns zero, there are no lone pairs. If not place lone pairs.
- The average bond energy (enthalpy) for a C=C double bond is 614 kJ/molkJ/mol and that of a C−C single bond is 348 kJ/molkJ/mol. If it takes 4.42×10−19 J/molecule to break the C=C double bond. What is the longest wavelength λ of light that will provide photons of sufficient energy to break the π bond and cause the isomerization? Express your answer numerically in nanometers.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 arrangement5.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*.
- Construct the molecular orbital diagram for SrCl. Would yo u expect the bond length of SrCl+ to be longer or shorter than that of SrCl? Explain and elaborate.1. Mark the following statements (A-E) as true or false A. The halogen bond dissociation energy decreases in the row Cl2 Br2 I2 because of repulsion between the electrons in the lower shells. B. The melting points of the dihalogens increase down the group because the interactions between the dihalogen molecules get stronger C. The electronegativity of the halogens decreases down the group because of the decrease of the electron affinity and the increase of the ionization energy. D. The unusually low bond dissociation energy of the F2 molecule is a direct result of the high electronegativity of fluorine E. The high reactivity of fluorine is in part due to the low bond dissociation energy of the F2 molecule1. The sigma bond between the Br and F atom in BrF4- is formed from the overlap of which two orbitals?a. 4sp3d-2sb. 4sp3d-2pc. 4sp3d2-2sd.4sp3d2-2p2. Consider the following species F2-, F2, and F2+. Which of these species will be paramagnetic? 3. Which of the following exhibits resonance?a. ClO3-b. BrF3c. OF2d. N2
- The molecular orbital energy diagram for F2 is shown below. Based on this diagram, what is the bond order of F2? 111 1LL 111 11 2p 2p 111. lewis structure of Cesium 2-hydroxyacetate, HOCH2CO2Cs 2. 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 arrangementIII. Place the following molecules in order of increasing CN bond length: HCN, NHCH2, NHẠCH3