our course material does not agree that the Octet rule should be the ultimate target. In the table below, draw two Lewis dot diagrams for 6 simple compounds. One, enforcing the Octet rules and a second, enforcing the “lowest charge” rules from your course notes. Note: the two diagrams may actually be the same but draw them both anyway. Below the table, for each species tell which model is the better one and explain why it’s better than the other model you drew of the same species. An example for Carbon monoxide is given in the first row. In this case, both diagrams are the same.
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.
Your course material does not agree that the Octet rule should be
the ultimate target. In the table below, draw two Lewis dot diagrams for 6 simple compounds. One, enforcing the
Octet rules and a second, enforcing the “lowest charge” rules from your course notes.
Note: the two diagrams may actually be the same but draw them both anyway. Below the
table, for each species tell which model is the better one and explain why it’s better than
the other model you drew of the same species.
An example for Carbon monoxide is given in the first row. In this case, both diagrams are the same.
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