When comparing single, double, and triple covalent bonds formed between two atoms X and Y, decreasing the number of π bonds between the atoms will:decrease the overall bond dissociation energy and bond strength.increase the bond length.decrease the bond rigidity (allow more bond twisting or rotation).A.I and II onlyB.I and III onlyC.II and III onlyD.I, II, and III
Question
When comparing single, double, and triple covalent bonds formed between two atoms X and Y, decreasing the number of π bonds between the atoms will:decrease the overall bond dissociation energy and bond strength.increase the bond length.decrease the bond rigidity (allow more bond twisting or rotation).A.I and II onlyB.I and III onlyC.II and III onlyD.I, II, and III
Solution
D. I, II, and III
Here's why:
I. Decreasing the number of π bonds between the atoms will decrease the overall bond dissociation energy and bond strength. This is because π bonds are weaker than σ bonds. So, when you decrease the number of π bonds, you're removing some of the weaker bonds, which decreases the overall bond strength and dissociation energy.
II. Decreasing the number of π bonds between the atoms will increase the bond length. This is because π bonds are shorter than σ bonds. So, when you decrease the number of π bonds, you're removing some of the shorter bonds, which increases the overall bond length.
III. Decreasing the number of π bonds between the atoms will decrease the bond rigidity (allow more bond twisting or rotation). This is because π bonds are more rigid than σ bonds. So, when you decrease the number of π bonds, you're removing some of the more rigid bonds, which allows for more bond twisting or rotation.
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