(d) Can two s orbitals combine to form a p bond? Explain.

Verified step by step guidance

Understand the nature of atomic orbitals: s orbitals are spherical in shape, while p orbitals are dumbbell-shaped and have directional characteristics.

Recognize the types of bonds: Sigma (σ) bonds are formed by the head-on overlap of orbitals, while pi (π) bonds are formed by the side-to-side overlap of orbitals.

Consider the overlap possibilities: s orbitals can overlap with each other or with other orbitals to form sigma bonds due to their spherical symmetry.

Analyze the formation of pi bonds: Pi bonds require parallel, side-to-side overlap, which is characteristic of p orbitals, not s orbitals.

Conclude based on orbital characteristics: Since s orbitals lack the directional nature needed for side-to-side overlap, they cannot combine to form pi bonds.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Orbital Hybridization

Orbital hybridization is the process by which atomic orbitals mix to form new hybrid orbitals that can accommodate bonding. In the context of s and p orbitals, hybridization allows for the formation of bonds that are stronger and more directional than those formed by the original atomic orbitals alone.

Types of Chemical Bonds

Chemical bonds can be classified into sigma (σ) and pi (π) bonds. Sigma bonds are formed by the head-on overlap of orbitals, while pi bonds result from the side-to-side overlap of p orbitals. Understanding these types of bonds is crucial for determining how different orbitals can combine to form stable molecular structures.

Orbital Overlap

Orbital overlap refers to the interaction between atomic orbitals when atoms approach each other to form a bond. For a bond to form, there must be sufficient overlap between the orbitals involved. In the case of s orbitals, they can only form sigma bonds due to their spherical shape, while p orbitals can form both sigma and pi bonds depending on their orientation.

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Related Practice

Textbook Question

(b) What would you expect for the magnitude and direction of the bond dipoles in this series?

Textbook Question

(a) Draw a picture showing how two p orbitals on two different atoms can be combined to make a σ bond. (b) Sketch a π bond that is constructed from p orbitals.

Textbook Question

(b) Imagine that you could hold two atoms that are bonded together, twist them, and not change the bond length. Would it be easier to twist (rotate) around a single s bond or around a double 1s plus p2 bond, or would they be the same?

Textbook Question

(a) Draw Lewis structures for chloromethane (CH₃Cl), chloroethene (C₂H₃Cl), and chloroethyne (C₂HCl).