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6 of 6 individual&family development ‘ X C9_GI_MOs Wl OO O E E E T - -=00 @ CHEM106 Molecular Orbitals Spring 2016 Some of the most beautiful colors in aurora’s comes from the movement of electrons in molecular orbitals. For example, when an electron falls from an excited state position to the ground state, there is an emission of light that can be in the visible region of the spectra, producing color. For example, the transition N, >N, produces a deep red color (the * represents a molecule in an excited state — meaning it has an electron that is not in the lowest energy orbital). The transition N, > N, produces a blue violet color. Draw a MO diagram for N," and N,"". Assume the excited electron in N, is in the next available electronic orbital above the ground state. Would you expect the bond in N, or N, to be stronger, and why? Which better explains molecular geometry: valence bond theory (hybridization) or molecular orbital theory? Why? Which better explains magnetic properties of a diatomic molecule: valence bond theory (hybridization) or molecular orbital theory? Why?
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Consider the ring cation, called "cyclopentadienyl cation".... one of five possible resonance structures that can be drawn for it is shown below. In the actual ring cation, what is the charge on any one carbon atom, and what is the bond order of any one C,C bond? 4? charge on one C = ? bond order of C,C bond ? Select one: O A. +2/5; 4/3 OB. + 1/6; 1.5 O C. + 2/5; 7/5 OD. + 1/5; 6/5 O E. + 1/5; 7/5
Number of Molecule valence electrons Formal Charge Electron-Group Geometry Molecular Geometry Resonance IBR3 I: Select one .. I: Select one .. No Where are the lone-pair electrons on the central atom located? O axial O equatorial O there are no lone pairs PFA P: Trigonal Bipyramidal v P: Distorted tetrahedral (see-saw) P: -1 No Where are the lone-pair electrons on the central atom located? O axial O equatorial O there are no lone pairs AtCl3 At: 0 At: Select one ... At: Select one .. No Where are the lone-pair electrons on the central atom located? O axial O equatorial O there are no lone pairs AtO2Br At: 0 At: Select one . At: Select one .. No What is the O-At-O bond angle? O 90
Draw the Lewis structure of AsO³- showing all lone pairs. Select Draw Rings More ||||||||| As G Erase Q2 Q 3- Identify the molecular geometry of AsO³. 4 see-saw O T-shaped tetrahedral octahedral linear square pyramidal trigonal planar trigonal pyramidal bent square planar O trigonal bipyramidal
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Like many of the molecules we have studied in this class, propene (structure shown below) can be thought of as a particle in a box. There are three t-electrons. Since I can put two electrons in each energy level, the highest-energy electron is in the n = 2 state (the HOMO). What does the wave for this electron look like? n = 3 lowest unoccupie molecular orbital (LUMO) n = 2 highest occupiedi molecular orbital (НОМО) . n = 1 Select one: Оа. O b. О с. O d. None of these shapes are right.
Show work. don't give Ai generated solution
For the molecule shown below, identify the hybridization on the N atom and the bond angle labeled alpha: |L | H-N-C-C-H a H .. H hybridization: sp³ bond angle: < 109.5° hybridization: sp? bond angle: 120° hybridization: sp bond angle: 90° hybridization: sp3 bond angle: 109.5°
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