There are two compounds of the formula Pt $\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2} :$The compound on the right is called cisplatin, and the compound on the left is called transplatin. (c) Would the bonding in allene be described as delocalized? (b) How can you determine whether a molecule or ion will exhibit delocalized $\pi$ bonding? Does this offer experimental proof that the molecule cannot be planar? Organic azides engage in useful organic reactions. The $\mathrm{O}-\mathrm{H}$ bond lengths in the water molecule $\left(\mathrm{H}_{2} \mathrm{O}\right)$ are$0.96 \mathrm{A},$ and the $\mathrm{H}-\mathrm{O}-\mathrm{H}$ angle is $104.5^{\circ} .$ The dipole moment of the water molecule is 1.85 $\mathrm{D}$ . (c) Which molecule has the stronger $N-N$ bond? Sodium azide is a shock-sensitive compound that releases N2upon physical impact. How does a trigonal pyramid differ from a tetrahedron so far as molecular geometry is concerned? How many $\sigma$ bondscan the two sets of 2$p$ orbitals make with each other? Explain in each case. Rate constants for the reaction of water or azide ion with various substituted benzylic carbocations can be calculated from the equilibrium constants for cation formation and distortion energies by means of the No Barrier Theory. (d) Sketch the energy-level diagram for the $\mathrm{Sc}_{2}$ molecule, assuming that only the3$d$ orbital from part (a) is important. (c) Is the C-Cbond in ethylene stronger or weaker in the excited state than in the ground state? Assume that the molecular orbitals of IBr are analogous to the homonuclear diatomic molecule $F_{2} .$ (a) Which valence atomic orbitals of I and of Br are used to construct the MOs of IBr? (a) What does the term paramagnetism mean? Why is this justified? Many compounds of the transition-metal elements contain direct bonds between metal atoms. (a) What is the molecular formula of the compound? (g) How many electrons are in the $\pi$ system of borazine? (c) Write the formulas for the analogous species of the elements of period 3; would you expect them to have the same hybridization at the central atom? ... driven by hybridization of N atomic orbitals, which changes. (d) The 1 s orbital has a nodal plane. (b) Now, on the $x$ -axis to the right of M, draw the Lewis structure of a CO molecule, with the carbon nearest the M. The CO bond axis should be on the $x$ -axis. (c) Predict which molecules, if any, are planar. (a) Balance the equation. (b) What hybrid orbitals are used about the central atom of each of these angles? Given the electronegativities of $\mathrm{B}$ and $\mathrm{N},$ do the formal charges seem favorable or unfavorable? Which one has the larger HOMO-LUMO gap? (c) For the $\mathrm{P}_{2}$ molecule, how many electrons occupy the MO in the figure? Azide is also a functional group in organic chemistry, RN3.[1]. (c) Suppose the B atoms are halogen atoms. (a) Imagine the atoms coming close together to bond. Using Figures 9.35 and 9.43 as guides, draw the molecular orbital electron configuration for (a) $\mathrm{B}_{2}^{+},(\mathbf{b}) \mathrm{Li}_{2}^{+},(\mathbf{c}) \mathrm{N}_{2}^{+},(\mathbf{d})$ $\mathrm{Ne}_{2}^{2+} .$ In each case indicate whether the addition of an electron to the ion would increase or decrease the bond order of the species. (b) The $\mathrm{NH}_{3}$ molecule is trigonal pyramidal, while $\mathrm{BF}_{3}$ is trigonal planar. (a) What does the term diamagnetism mean? The HOMO-LUMO transition corresponds to molecules going from their ground state to their first excited state. Carbon monoxide, CO, is isoelectronic to $\mathrm{N}_{2}$ . NH3 Bond angles (c) Naphthalene, the active ingredient in mothballs, is a white solid. (Arrangement of atoms: NNN.) Lewis Structure: ... the molecular shape of Azide ion is linear. Does the value of the $\mathrm{B}-\mathrm{N}$ bondlength seem to favor one Lewis structure over the other? (a) How many nonbonding domains are on atom A? We have three molecules of iodine here which along with an extra elec… Rate constants for the water reactions span 10 orders of magnitude. [ Section 9.5$]$, The following is part of a molecular orbital energy-level diagram for MOs constructed from 1s atomic orbitals. The energy-level diagram in Figure 9.36 shows that the sideways overlap of a pair of porbitals produces two molecular orbitals, one bonding and one antibonding. [\mathrm{Section} 9.6]$, The molecule shown below is called furan. (e) Look at the Lewis structure for HF. Choose the hybridization schemes for the following species. (c) Consider the $\pi_{2 p}$ MOs of the molecule. (a) An AB $_{6}$ molecule has no lone pairs of electrons on the A atom. Principles of Microeconomics for AP Courses 2e. (c) The electronic absorption spectrum of the $N_{2}$ molecule has the lowest energy peak at 170 nm. Sodium azide is made industrially by the reaction of nitrous oxide, N2O with sodium amide in liquid ammonia as solvent:[2]. (a) What is the difference between a localized $\pi$ bond and a delocalized one? [Section 9.8$]$. (e) What kind of bond is being made with the orbitals between $\mathrm{M}$ and $\mathrm{C}, \sigma$ or $\pi ? = (b) For which of the following molecules or ions could this be the energy-level diagram:\begin{equation}\mathrm{H}_{2}, \mathrm{He}_{2}, \mathrm{H}_{2}^{+}, \mathrm{He}_{2}^{+}, \text { or } \mathrm{H}_{2}^{-} ?\end{equation}(c) What is the bond order of the molecule or ion? Rate constants for the reaction of water or azide ion with various substituted benzylic carbocations can be calculated from the equilibrium constants for cation formation and distortion energies by means of the No Barrier Theory. (a) What is the electron configuration of an isolated B atom? What is the hybridization state of the central N atom in the azide ion, N 3-? (d) If an electron is added to the system, into which of the MOs will it be added? (b) Does BeCl$_{2}$ have a dipole moment? (e) Which of the following statements about part (d) is correct: (i) The light excites an electron from a bonding orbital to an antibonding orbital, (ii) The light excites an electron from an antibonding orbital to a bonding orbital, or (iii) In the excited state there are more bonding electrons than antibonding electrons? (b) The molecule IF has a pentagonal bipyramid structure: five fluorines are equatorial, forming a flat pentagon around the central iodine atom, and the other two fluorines are axial. (c) The middle $C-$ bond length in butadiene $(1.48$ A) is a little shorter than the average $\mathrm{C}-\mathrm{C}$ single bond length$(1.54 \hat{\mathrm{A}}) .$ Does this imply that the middle $\mathrm{C}-\mathrm{Cbond}$ in butadiene is weaker or stronger than the average $\mathrm{C}-\mathrm{C}$? (a) Using only the valence atomic orbitals of a hydrogen atom and a fluorine atom, and following the model of Figure 9.46, how many MOs would you expect for the HF molecule? CS1 maint: multiple names: authors list (. The azide ion is $\mathrm{N}_{3}^{-} .$ (a) Draw the Lewis structure of the azide ion that minizes formal charge (it does not form a triangle). Shriver and Atkins. (c) Write the electron configuration of the ion in terms of its MOs. ; With N 3-you'll need to form two double bonds between the Nitrogen atoms to fill the octets and still use only the 34 valence electrons available for the molecule. Horst H. Jobelius, Hans-Dieter Scharff "Hydrazoic Acid and Azides" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. (b) How many of the MOs from part (a) would be occupied by electrons? (e) Is the N-N bondin the first excited state stronger or weaker compared to that in the ground state? Many inorganic azides can be prepared directly or indirectly from sodium azide.