coexistence of orbitals from two different atoms sharing the same region of space, leading to the formation of a covalent bond

plane separating different lobes of orbitals, where the probability of finding an electron is zero

covalent bond formed by side-by-side overlap of atomic orbitals; the electron density is found on opposite sides of the internuclear axis

covalent bond formed by overlap of atomic orbitals along the internuclear axis

description of bonding that involves atomic orbitals overlapping to form σ or π bonds, within which pairs of electrons are shared

Chemistry 2e · 8.1 Valence Bond Theory

Valence Bond Theory: practice problems

4 problems from the book, with its answers. Check your working, or have any of them explained to you on the whiteboard.

Exercises 1
Explain how σ and π bonds are similar and how they are different.
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Exercises 3
Explain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.
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Exercises 5
Use valence bond theory to explain the bonding in O₂. Sketch the overlap of the atomic orbitals involved in the bonds in O₂.
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Exercises 7
A friend tells you N₂ has three π bonds due to overlap of the three p-orbitals on each N atom. Do you agree?
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Key terms · 5

overlap: coexistence of orbitals from two different atoms sharing the same region of space, leading to the formation of a covalent bond
node: plane separating different lobes of orbitals, where the probability of finding an electron is zero
pi bond (π bond): covalent bond formed by side-by-side overlap of atomic orbitals; the electron density is found on opposite sides of the internuclear axis
sigma bond (σ bond): covalent bond formed by overlap of atomic orbitals along the internuclear axis
valence bond theory: description of bonding that involves atomic orbitals overlapping to form σ or π bonds, within which pairs of electrons are shared

The tutor teaches the whole section, drawing it out step by step and answering your questions as you go.

Valence Bond Theory: practice problems

4 problems from the book, with its answers. Check your working, or have any of them explained to you on the whiteboard.

Exercises 1

Explain how σ and π bonds are similar and how they are different.

Exercises 3

Explain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.

Exercises 5

Use valence bond theory to explain the bonding in O₂. Sketch the overlap of the atomic orbitals involved in the bonds in O₂.

Exercises 7

A friend tells you N₂ has three π bonds due to overlap of the three p-orbitals on each N atom. Do you agree?

overlap: coexistence of orbitals from two different atoms sharing the same region of space, leading to the formation of a covalent bond
node: plane separating different lobes of orbitals, where the probability of finding an electron is zero
pi bond (π bond): covalent bond formed by side-by-side overlap of atomic orbitals; the electron density is found on opposite sides of the internuclear axis
sigma bond (σ bond): covalent bond formed by overlap of atomic orbitals along the internuclear axis
valence bond theory: description of bonding that involves atomic orbitals overlapping to form σ or π bonds, within which pairs of electrons are shared

The tutor teaches the whole section, drawing it out step by step and answering your questions as you go.