Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 73b

Chapter 9, Problem 73b

Draw a picture that shows all three 2p orbitals on one atom and all three 2p orbitals on another atom. (b) How many p bonds can the two sets of 2p orbitals make with each other?

Verified step by step guidance

Step 1: To draw the 2p orbitals, you need to understand that each p orbital is dumbbell-shaped and oriented along one of the three axes (x, y, z). So, for one atom, you will draw three dumbbell-shaped orbitals, each oriented along a different axis. Repeat this for the second atom.

Step 2: Label each of the orbitals as 2px, 2py, and 2pz to indicate their orientation along the x, y, and z axes respectively.

Step 3: To answer part (b), you need to understand that a pi (π) bond is formed by the sideways overlap of two p orbitals. This can happen between the 2px orbitals of the two atoms, the 2py orbitals, and the 2pz orbitals.

Step 4: Therefore, the two sets of 2p orbitals can form up to three pi (π) bonds with each other, one for each pair of overlapping orbitals (2px-2px, 2py-2py, and 2pz-2pz).

Step 5: Keep in mind that this is a theoretical maximum. In reality, the number of pi bonds that can form depends on the specific atoms involved and their electron configurations.

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Key Concepts

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

Atomic Orbitals

Atomic orbitals are regions in an atom where there is a high probability of finding electrons. The 2p orbitals are a set of three degenerate orbitals (2px, 2py, 2pz) that can hold a maximum of six electrons. Each orbital has a distinct orientation in space, which is crucial for understanding how atoms bond with each other.

p Bonds

p bonds, or pi bonds, are a type of covalent bond formed when two atomic orbitals overlap laterally. In the case of p orbitals, this occurs when the lobes of the orbitals align side-by-side. Each pair of p orbitals from different atoms can form one p bond, which is essential for the formation of double and triple bonds in molecules.

Orbital Overlap

Orbital overlap is a fundamental concept in chemical bonding that describes how atomic orbitals from different atoms interact to form bonds. The extent of overlap between orbitals determines the strength and type of bond formed. In the context of the question, the overlap of the 2p orbitals from two atoms will dictate how many p bonds can be formed between them.

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Related Practice

Draw a picture that shows all three 2p orbitals on one atom and all three 2p orbitals on another atom. (c) How many antibonding orbitals, and of what type can be made from the two sets of 2p orbitals?

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Textbook Question

Consider the H₂⁺ ion. (c) Write the electron configuration of the ion in terms of its MOs. (d) What is the bond order in H₂⁺?

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Textbook Question

Indicate whether each statement is true or false. (d) Electrons cannot occupy a nonbonding orbital.

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Textbook Question

Consider the H₂⁺ ion. (e) Suppose that the ion is excited by light so that an electron moves from a lower-energy to a higher-energy MO. Would you expect the excited-state H₂⁺ ion to be stable or to fall apart?

Indicate whether each statement is true or false. c. Antibonding orbitals are higher in energy than bonding orbitals (if all orbitals are created from the same atomic orbitals).

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