From the Lewis structures of the species given, pick all of those in which the central atom obeys the octet rule. :Ci-B-CI: :CI: +1 H H-N-H H :F: :F-Br. :F: :ci: :CI-Si-CI: :C: O None of the Above
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.
![**Resonance Structures**
Resonance Structures are ways to represent the bonding in a molecule or ion when a single Lewis structure fails to describe accurately the actual electronic structure.
[Diagram Description: The diagram shows two resonance structures for the nitrite ion (\( \text{NO}_2^-\)). Each structure involves nitrogen centrally bonded to two oxygen atoms. In one structure, one of the nitrogen-oxygen bonds is a single bond, while the other is a double bond, and then vice versa in the other structure. The oxygen atoms have lone pairs represented by dots, and a double-headed arrow between the structures indicates resonance.]
Equivalent resonance structures occur when there are identical patterns of bonding within the molecule or ion. The actual structure is a composite, or **resonance hybrid**, of the equivalent contributing structures.
**Draw Lewis structures** for phosphoric acid and for the nitrite ion in which the central atom obeys the octet rule.
- How many equivalent Lewis structures are necessary to describe the bonding in \( \text{PO(OH)}_3 \)? [Blank Space]
- How many equivalent Lewis structures are necessary to describe the bonding in \( \text{NO}_2^- \)? [Blank Space]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa0450cc9-9104-456b-91ad-505da73c8865%2F54937875-ab73-431b-a68e-bdd894a22693%2Fh6j6y6i_processed.png&w=3840&q=75)
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