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Chapter 4: Problem 55

Which is not characteristic of a \(\pi\) bond? (1) A \(\pi\) -bond is formed when a sigma bond is already formed. (2) \(\pi\) -bonds are formed by hybrid orbitals. (3) \(\pi\) -bonds may be formed by the overlapping of atomic orbitals. (4) \(\pi\) -bond results from lateral overlap of atomic orbitals.

Short Answer

Expert verified
(2) \( \pi \) -bonds are formed by hybrid orbitals.

Step by step solution

01

Understand the characteristics of a \( \pi \) bond

A \( \pi \) bond typically forms when two atomic orbitals overlap laterally (side-by-side) rather than head-on. A \( \pi \) bond is usually found in conjunction with a \( \sigma \) bond in double and triple bonds.
02

Analyze each option

Evaluate the given statements to determine which one is not a characteristic of \( \pi \) bonds. A true characteristic should describe properties related to the formation or structure of \( \pi \) bonds.
03

Examine Option (1)

A \( \pi \) bond is formed when a \( \sigma \) bond is already formed. This is a true characteristic because \( \pi \) bonds are formed in the presence of a \( \sigma \) bond, typically in double or triple bonds.
04

Examine Option (2)

\(\pi\) bonds are formed by hybrid orbitals. This statement is false because \( \pi \) bonds are formed by the lateral overlap of unhybridized p-orbitals, not hybrid orbitals.
05

Examine Option (3)

\( \pi \) bonds may be formed by the overlapping of atomic orbitals. This is a true statement because the lateral overlap between p-orbitals creates a \( \pi \) bond.
06

Examine Option (4)

A \( \pi \) bond results from lateral overlap of atomic orbitals. This is a true characteristic since \( \pi \) bonds are specifically created by the side-to-side overlap of p-orbitals.
07

Conclusion

Only option (2) does not correctly describe a \( \pi \) bond because \( \pi \) bonds are not formed by hybrid orbitals.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

pi bond formation
A \( \pi \) bond is unique compared to a \( \sigma \) bond. It forms when two atomic orbitals overlap laterally (side-by-side) rather than overlapping head-on. This side-to-side overlap primarily occurs between unhybridized p orbitals. Unlike \( \sigma \) bonds, which are generally single bonds, \( \pi \) bonds often occur alongside \( \sigma \) bonds in the structure of the bond.
sigma bond presence
In chemical bonding, a \( \sigma \) bond is usually formed first before a \( \pi \) bond can exist. This happens because the head-on overlap associated with \( \sigma \) bonds creates a very stable bonding environment, which is a prerequisite for the formation of the additional \( \pi \) bonds in double and triple bonds.
In summary:
  • The \( \pi \) bond is formed after the \( \sigma \) bond.
  • This setup allows for stronger and more rigid bonding in molecules like \( \text{C=C} \) and \( \text{N\texttriplebond{}N} \).
atomic orbital overlap
Atomic orbital overlap is crucial in bond formation. When forming a \( \pi \) bond, the lateral (side-by-side) overlap of p-orbitals is essential. This differs from the head-on overlap seen in \( \sigma \) bonds, which involve s or sp\textsuperscript{3} hybridized orbitals. The nature of this overlap determines the type of bond formed.
Key points:
  • \( \pi \) bonds result from the lateral overlap.
  • \( \sigma \) bonds result from the head-on overlap.
lateral overlap
In the context of \( \pi \) bond formation, lateral overlap plays a fundamental role. This type of overlap occurs when two p-orbitals align parallel to each other, allowing their electron clouds to merge and form a bonding interaction. This interaction is less strong than the head-on overlap in \( \sigma \) bonds, yet it stabilizes multiple bond structures.
In essence:
  • Lateral overlap is characteristic of \( \pi \) bonds.
  • It involves parallel p-orbitals.
unhybridized p orbitals
The unhybridized p orbitals are essential for the formation of \( \pi \) bonds. Unlike sp\textsuperscript{2} or sp\textsuperscript{3} hybrid orbitals, these p orbitals remain in their original form, enabling the lateral overlap necessary for \( \pi \) bonds. These p orbitals are typically perpendicular to the plane of the atoms鈥� sp\textsuperscript{2} hybridized orbitals.
Points to remember:
  • \( \pi \) bonds use unhybridized p orbitals.
  • These p orbitals are crucial for the double and triple bonds.

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