Part VI. Draw a complete molecular orbital (MO) diagram for the following molecule. State the number of nodes in each MO. ● ● ● ● Shade the provided atomic orbitals (AO) to reflect the number of nodes. Not all provided AOS are necessary, clearly mark out the unused AOS. Show the relative energy of each MO. Label the bonding, nonbonding, and antibonding MOS. Show the location of the electrons in the MOS. Indicate which MOs are nonbonding, bonding, and antibonding.
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
a. Number of AOs in this molecule: _____________
b. Number of MOs in this molecule: _____________
c. Number of p electrons in this molecule: ___________
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