Question

33) There is/are \( \pi \) bond \( (s) \) in the molecule below. A) 7 B) 6 (i) 2 D) 1

Answer 1

The molecule shown has a total of 6 π bonds.

Step-by-step explanation:

To determine the number of π bonds in a molecule, we need to count the number of double bonds (π bonds) and triple bonds (π bonds) as each contributes two π electrons. In the given molecule, we have three double bonds, contributing a total of 6 π electrons.

To break it down further, a double bond consists of one σ bond and one π bond, while a triple bond consists of one σ bond and two π bonds. Therefore, for each double bond, there is one π bond, and for each triple bond, there are two π bonds. Adding these up, we find that the molecule has a total of 6 π bonds.

In conclusion, the presence of double and triple bonds in the molecule results in the contribution of 6 π electrons, indicating the presence of 6 π bonds. This understanding is crucial in predicting the reactivity and properties of the molecule, as π bonds play a significant role in chemical reactions and molecular stability.

Answer 2

By recognizing the structural arrangement and applying the concept of pi bonds in conjugated systems, the count of 6 pi bonds becomes evident, leading to the final answer of 6 pi bonds in the molecule. Thus, the correct option is B) 6

Step-by-step explanation:

In this molecule, to determine the number of pi bonds (π), it's crucial to identify the presence of double bonds and rings with alternating single and double bonds. The molecule in question features one benzene ring, which contains 6 delocalized pi electrons, symbolizing 3 pi bonds. The benzene ring, a cyclic structure with alternating double and single bonds among carbon atoms, has a unique resonance structure where pi electrons are delocalized. Each double bond in the ring accounts for 2 pi electrons, totaling 6 delocalized electrons or 3 pi bonds in the ring.

Additionally, while considering the rest of the molecule, there are no other double bonds or ring structures present that contribute to additional pi bonds. Hence, the total count of pi bonds in this molecule is 6, corresponding to option B.

The molecule's structure involves understanding the nature of pi bonds and their occurrence in conjugated systems. Benzene, being a classic example of a compound with delocalized pi electrons, showcases the concept of resonance and aromaticity, where 6 pi electrons exist in the ring, equivalent to 3 pi bonds, due to the delocalization of electrons among the carbon atoms. By recognizing the structural arrangement and applying the concept of pi bonds in conjugated systems, the count of 6 pi bonds becomes evident, leading to the final answer of 6 pi bonds in the molecule. Thus, the correct option is B) 6