Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 9: Problem 45

For each statement, indicate whether it is true or false. (a) In order to make a covalent bond, the orbitals on each atom in the bond must overlap. (b) A p orbital on one atom cannot make a bond to an s orbital on another atom. (c) Lone pairs of electrons on an atom in a molecule influence the shape of a molecule. (d) The 1 s orbital has a nodal plane. (e) The \(2p\) orbital has a nodal plane.

Short Answer

Expert verified
(a) True - Covalent bonds require orbital overlap. (b) False - p orbitals can bond with s orbitals. (c) True - Lone pairs affect the molecular shape. (d) False - 1s orbitals do not have nodal planes. (e) True - 2p orbitals have a nodal plane.

Step by step solution

01

Statement (a) - Covalent Bond Requirement

Statement (a) is true. In order to form a covalent bond, the orbitals on each atom in the bond must overlap. This overlap allows for the sharing of electrons between the two atoms, resulting in a stable covalent bond.
02

Statement (b) - Bonding Between p and s Orbitals

Statement (b) is false. A p orbital on one atom can indeed form a bond with an s orbital on another atom. This can occur, for example, in the formation of a sigma bond, where the probability of finding the shared electrons is highest along the axis that connects the two nuclei.
03

Statement (c) - Lone Pairs and Molecular Shape

Statement (c) is true. Lone pairs of electrons on an atom in a molecule have a significant influence on the shape of the molecule. This is because lone pairs of electrons still occupy space and create repulsion, pushing other atoms in the molecule away from them, ultimately affecting the overall geometry of the molecule.
04

Statement (d) - Nodal Plane in 1s Orbital

Statement (d) is false. The 1s orbital does not have a nodal plane. A nodal plane is a region in an orbital where the probability of finding an electron is zero. The 1s orbital is a spherical shape with uniform electron density, and there is no such region with zero electron probability.
05

Statement (e) - Nodal Plane in 2p Orbital

Statement (e) is true. The 2p orbital has a nodal plane. The 2p orbital has a dumbbell shape, with two lobes separated by a nodal plane. In this nodal plane, the probability of finding an electron is zero.

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.

Start your free trial

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

In which of the following \(\mathrm{AF}_{n}\) molecules or ions is there more than one \(\mathrm{F}-\mathrm{A}-\mathrm{Fbond}\) angle: \(\mathrm{SiF}_{4}, \mathrm{PF}_{5}, \mathrm{SF}_{4}, \mathrm{AsF}_{3} ?\)

Draw sketches illustrating the overlap between the following orbitals on two atoms: (a) the 2 s orbital on each atom, (b) the 2\(p_{z}\) orbital on each atom (assume both atoms are on the \(z\) -axis), (c) the 2 s orbital on one atom and the 2\(p_{z}\) orbital on the other atom.

Draw a picture that shows all three 2\(p\) orbitals on one atom and all three 2\(p\) orbitals on another atom. (a) Imagine the atoms coming close together to bond. How many \(\sigma\) bonds can the two sets of 2\(p\) orbitals make with each other? (b) How many \(\pi\) bonds can the two sets of 2\(p\) orbitals make with each other? (c) How many antibonding orbitals, and of what type, can be made from the two sets of 2\(p\) orbitals?

Indicate whether each statement is true or false. (a) \(s\) orbitals can only make \(\sigma\) or \(\sigma^{*}\) molecular orbitals. (b) The probability is 100\(\%\) for finding an electron at the nucleus in a \(\pi^{*}\) orbital. (c) Antibonding orbitals are higher in energy than bonding orbitals (if all orbitals are created from the same atomic orbitals). (d) Electrons cannot occupy an antibonding orbital.

Name the proper three-dimensional molecular shapes for each of the following molecules or ions, showing lone pairs as needed: \((\mathbf{a}) \mathrm{ClO}_{2}^{-}(\mathbf{b}) \mathrm{SO}_{4}^{2-}(\mathbf{c}) \mathrm{NF}_{3}(\mathbf{d}) \mathrm{CCl}_{2} \mathrm{Br}_{2}(\mathbf{e}) \mathrm{SF}_{4}^{2+}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

Organic Chemistry

Read Explanation
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