since Paling and also not setric. SP How many "central" atoms are part of methanol (CH,OH)? What are the molecular geometries of each central atom? 2 Centro otorns (14)+6+4= 2-8-4 5. 4. C/ G: tetra taure O EG tetrala B: 2 MG bent NB: 2 4 How many "central" atoms are part of ethylene glycol (HOCH₂CH₂OH), a component of antifreeze? What are the molecular geometries of each central atom? Is the molecule polar or nonpolar? Why? (Note: the modeling kits technically only contain one carbon and one oxygen via color coding, however, in this example, other spheres can be used to represent these elements within this molecule ... why?) 1 (1 x 6 ) + ( 2 x 6 ) + ( 4 x 2) == (2x6)+(4xz). 6 12 :8

D Lewis strct molecalar iodie, and the dide in

C, exhibits two TT bonds: one to Ca, and the other to Cc. Imagine a picture of C₂, Cb, and the two different p orbitals that C is utilizing to form its two TT bonds. (It may be helpfu Also consider the p orbitals on C₂ and C that are being used by each of those atoms. De orbitals on C₂ and Co. The norbitale aro alic

Give detailed Solution with explanation needed..don't give Handwritten answer...

Describe the types of bonds and the orbitas in CH3-CH=CH-CH3 Drawa strcture indicating the sigma and pi bonds. (USse colors to represen te orbitals and the overlapping of the orbitals.)

Attractive Energy EA and repulsive Energy ER for Na+ and Cl- is dependent on distance r between 1,436 ions and: EA== 1 ER = 7,32.10-6 7-8 -Calculate equilibrium spacing, To and bonding energy Eo.

The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) LiBe+ (b) CO+ (c) CN (d) OF Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.

Compare the electron density in the 1g and 1u* molecular orbitals for H2+ shown in Figure 6.5 with the classical model for bonding for H2+ summarized in Figure 3.22b. Which of these molecular orbitals describes the bond in H2+ ?

Discuss the nature of the bonding in the nitrate ion (NO3) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central N atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized MO. What bond order is predicted by the MO model for the NO bonds in the nitrate ion?

Explain why N22+ is diamagnetic, while O24+, which has the same number of valence electrons, is paramagnetic.