In your own words, define the following terms or symbols: (a) \(s p^{2} ;\) (b) \(\sigma_{2 p}^{*} ;\) (c) bond order; (d) \(\pi\) bond.

Short Answer

Expert verified
(a) \(s p^{2}\) hybridization is the mixing of one \(s\) and two \(p\) orbitals to form three identical hybrid orbitals in a molecule with a trigonal planar arrangement. (b) \(\sigma_{2 p}^{*} \) orbital is an anti-bonding molecular orbital formed by the out-of-phase overlap of \(2 p\) atomic orbitals. (c) Bond order indicates the number of chemical bonds between a pair of atoms. (d) A \(\pi\) bond is a type of covalent bond that exists between atoms, formed by the side-on overlap of atomic orbitals and is present in addition to a \( \sigma\) bond in molecules where double or triple bonds exist.

Step by step solution

01

Define the \(s p^{2} \) Hybridization

\(s p^{2} \) hybridization refers to the mixing of one \(s\) and two \( p\) orbitals, resulting in three identical hybrid orbitals in a molecule. This type of hybridization is found in atoms with a 'trigonal planar' arrangement of atoms such as \( BCl_3 \), \( CO_3^{2-} \).
02

Define the \(\sigma_{2 p}^{*} \) Orbital

The \(\sigma_{2 p}^{*} \) orbital refers to the anti-bonding molecular orbital formed by the out-of-phase overlap of \(2 p\) atomic orbitals. 'Anti-bonding' means the electrons in this orbital do not help in the formation of a bond; instead, they can weaken or even break a bond.
03

Define Bond Order

The 'Bond order' indicates the number of chemical bonds between a pair of atoms. It can be calculated as: (Number of electrons in bonding orbitals - Number of electrons in anti-bonding orbitals) / 2. A higher bond order generally means a stronger bond.
04

Define the \(\pi\) Bond

A \(\pi\) bond is a type of covalent bond that exists between atoms where the electrons are on top and bottom of the axis connecting the nuclei of the atoms. It's formed by the side-on overlap of atomic orbitals, typically \( p\) orbitals, and is present in addition to a \( \sigma\) bond in molecules where double or triple bonds exist.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free