Which of the following statements are true? c. A 𝜋 bond is made from the sideways overlap of two p orbitals.

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Identify the type of bond being discussed: a \( \pi \) bond.

Recall the definition of a \( \pi \) bond: it is formed by the sideways overlap of two parallel \( p \) orbitals.

Understand that \( \pi \) bonds are different from \( \sigma \) bonds, which are formed by the head-on overlap of orbitals.

Consider the orientation of \( p \) orbitals: they have lobes that can overlap sideways to form a \( \pi \) bond.

Conclude that the statement is true based on the definition and characteristics of \( \pi \) bonds.

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Key Concepts

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

Bonding Orbitals

Bonding orbitals are regions in a molecule where the probability of finding electrons is high, resulting from the overlap of atomic orbitals. In covalent bonding, these orbitals can be classified as sigma (σ) and pi (π) bonds, which differ in their formation and electron distribution.

Pi Bonds

A pi (π) bond is a type of covalent bond that occurs when two atomic orbitals overlap sideways, typically involving p orbitals. This overlap allows for the sharing of electrons above and below the bond axis, contributing to the overall stability and geometry of the molecule.

Orbital Hybridization

Orbital hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can explain the geometry of molecular bonding. For example, in the case of double bonds, one σ bond is formed from head-on overlap, while the π bond arises from the lateral overlap of unhybridized p orbitals.

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What is the hybridization of the central atom in c. SO3?

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What is the hybridization of the central atom in d. TeCl2?

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Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle. (a)

(b)

(c)

Textbook Question

Which of the following statements are true? d. A 𝜋 bond has two regions of overlap on opposite sides of the internuclear axis.

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(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

(b) What is the hybridization of the carbon atoms in each molecule?

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