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Chapter 10: Problem 39

How would you distinguish between a sigma bond and a pi bond?

Short Answer

Expert verified
Sigma bonds are formed from the end-to-end (head-on) overlap of atomic orbitals, allow free rotation around the bond axis, and are stronger in comparison to Pi bonds. Pi bonds form from the side-on overlap of atomic orbitals, do not allow free rotation around the bond, and are generally weaker than sigma bonds.

Step by step solution

01

Definition of Sigma bond

Understand that a sigma bond is a type of covalent bond that forms when two atomic orbitals overlap along the axis connecting the two bonding atoms. This overlap along the axis allows for free rotation around the sigma bond.
02

Definition of Pi bond

Comprehend that a pi bond, on the other hand, forms when the overlap of atomic orbitals is above and below, or in front of and behind the axis connecting the two bonding atoms. This kind of bonding does not permit free rotation.
03

Difference in formation

Recognize that Sigma bonds can form from the end-to-end overlap (head-on) of atomic orbitals, while Pi bonds are formed from the side-on overlap of two atomic orbitals.
04

Difference in strength

Recognize the difference in strength, where sigma bonds are stronger due to the greater extent of overlap, while pi bonds are weaker in comparison.
05

Presence of free rotation

Understand that Sigma bonds allow for free rotation of atoms around the bond axis, whereas Pi bonds do not permit such rotation due to sideways overlap

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Key Concepts

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

Sigma Bond
A sigma bond is a fundamental type of covalent bond. It forms when two atomic orbitals overlap directly along the axis that connects the two atoms. This direct overlap makes sigma bonds stronger than other types of bonds such as pi bonds.
  • Strength comes from greater overlap.
  • Allows for free rotation around the bond axis.
  • Permits a single line of electron density between the bonded nuclei.

Because of their strength and rotational freedom, sigma bonds are generally the first bonds to form between two atoms.
Pi Bond
A pi bond is also a type of covalent bond, but it differs from a sigma bond in formation and properties. Pi bonds form when orbital overlap occurs above and below the axis of the bonding atoms. This means they arise from the sideways overlap of atomic orbitals.
  • Weaker than sigma bonds due to less overlap.
  • Restricts the rotation of bonded atoms.
  • Typically found in double and triple bonds after the sigma bond has formed.

Because pi bonds limit rotation, they help to maintain the shape and rigidity of molecules, such as in double-bonded alkenes.
Covalent Bond
Covalent bonds are a fundamental aspect of chemistry and involve the sharing of electron pairs between atoms. This bond type is essential in the formation of many types of molecules.
  • Can form between similar or different atoms.
  • Results in a molecule with filled outer electron shells.
  • Includes both sigma and pi bonds.

Understanding covalent bonds is crucial for grasping how molecules, like water or carbon dioxide, are formed and stabilized.
Atomic Orbitals
Atomic orbitals are regions around an atom's nucleus where electrons are likely to be found. These orbitals have distinct shapes and can overlap to form different types of covalent bonds, like sigma and pi bonds.
  • Include s, p, d, and f orbitals, each with unique shapes.
  • The s orbital is spherical, while p orbitals are dumbbell-shaped.
  • The overlap of these orbitals determines bond type and strength.

Grasping the concept of atomic orbitals is key to understanding how chemical bonds are formed and how they contribute to molecule structure.
Bond Rotation
Bond rotation refers to the ability of atoms connected by a bond to rotate around the bond axis. Sigma bonds, due to their head-on overlapping, allow for this free rotation, which contributes to the flexibility of molecular structures.
  • Free rotation occurs around single (sigma) bonds.
  • Pi bonds restrict this rotation, found in double and triple bonds.
  • Influences the 3D conformation and reactivity of the molecule.

Understanding bond rotation is important for predicting the behavior and properties of complex molecules, particularly in organic chemistry.

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Most popular questions from this chapter

For each pair listed here, state which one has a higher first ionization energy and explain your choice: (a) \(\mathrm{H}\) or \(\mathrm{H}_{2},\) (b) \(\mathrm{N}\) or \(\mathrm{N}_{2},\) (c) \(\mathrm{O}\) or \(\mathrm{O}_{2},\) (d) \(\mathrm{F}\) or \(\mathrm{F}_{2}\).

Describe the geometry and hybridization for the reactants and product in the following reaction: $$ \mathrm{ClF}_{3}+\mathrm{AsF}_{5} \longrightarrow\left[\mathrm{ClF}_{2}^{+}\right]\left[\mathrm{AsF}_{6}^{-}\right] $$

Compare the relative stability of the following species and indicate their magnetic properties (that is, diamagnetic or paramagnetic): \(\mathrm{O}_{2}, \mathrm{O}_{2}^{+}, \mathrm{O}_{2}^{-}\) (superoxide ion), \(\mathrm{O}_{2}^{2-}\) (peroxide ion).

Predict the geometries of the following ions: (a) \(\mathrm{NH}_{4}^{+}\) (b) \(\mathrm{NH}_{2}^{-},\) (c) \(\mathrm{CO}_{3}^{2-},\) (d) \(\mathrm{ICl}_{2}^{-}\), (e) \(\mathrm{ICl}_{4}^{-}\) (f) \(\mathrm{AlH}_{4}^{-},(\mathrm{g}) \mathrm{SnCl}_{5}^{-}\) (h) \(\mathrm{H}_{3} \mathrm{O}^{+}\) (i) \(\mathrm{BeF}_{4}^{2-}\).

The compounds carbon tetrachloride \(\left(\mathrm{CCl}_{4}\right)\) and silicon tetrachloride \(\left(\mathrm{SiCl}_{4}\right)\) are similar in geometry and hybridization. However, \(\mathrm{CCl}_{4}\) does not react with water but \(\mathrm{SiCl}_{4}\) does. Explain the difference in their chemical reactivities. (Hint: The first step of the reaction is believed to be the addition of a water molecule to the \(\mathrm{Si}\) atom in \(\left.\mathrm{SiCl}_{4} .\right)\)
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