Consider the two resonance structures below (i and ii): :N N: ii A) Which structure obeys the octet rule? (circle one) i ii both neither B) On each structure, write the formal charge for each element. C) Which resonance structure do you anticipate being the major contributor? (Circle) :ö:
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 Analysis**
**3. Consider the two resonance structures below (i and ii):**
*Structure i:*
- Nitrogen (N) with a lone pair, double-bonded to another Nitrogen (N), which is triple-bonded to Oxygen (O) with two lone pairs.
*Structure ii:*
- Nitrogen (N) with one lone pair, triple-bonded to another Nitrogen (N), which is single-bonded to Oxygen (O) with three lone pairs.
**A) Which structure obeys the octet rule? (Circle one)**
- i
- ii
- both
- neither
**B) On each structure, write the formal charge for each element.**
Guidance: To determine the formal charge, use the formula:
\[ \text{Formal charge} = \text{Valence electrons} - \text{Non-bonding electrons} - \frac{\text{Bonding electrons}}{2} \]
**C) Which resonance structure do you anticipate being the major contributor? (Circle)**
- i
- ii
- both
- neither
Note: The preference for the major contributor typically depends on which structure has the atoms with the lowest formal charges and complete octets.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7d848391-a5b1-45af-b291-d5739fd6d88e%2F36db553d-bcb8-4e1c-b670-23037fb60e19%2Fskgn01x_processed.png&w=3840&q=75)
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