/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 71 Describe the relative orientatio... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 5: Problem 71

Describe the relative orientations of the orbitals related to an atom鈥檚 2p sublevel.

Short Answer

Expert verified
The three orbitals in the 2p sublevel have a dumbbell shape and are oriented along the x, y, and z axes (2px, 2py, and 2pz respectively). They lie in planes perpendicular to each other, with 90-degree angles between their axes. The electron probability distribution is localized along each axis, with nodal planes separating the lobes within each orbital and between different orbitals.

Step by step solution

01

Understanding the shape of p orbitals

P orbitals have a dumbbell shape, meaning they consist of two lobes aligned along a particular axis. The two lobes are separated by a nodal plane perpendicular to the axis, where the probability of finding an electron is zero.
02

Identifying the orientation of 2px, 2py, and 2pz orbitals

The three p orbitals are oriented along the three Cartesian axes: x, y, and z. The 2px orbital is aligned along the x-axis, the 2py orbital is aligned along the y-axis, and the 2pz orbital is aligned along the z-axis. Each orbital lies in a plane perpendicular to the other two orbitals.
03

Describing the angles between the orbitals

Since the orbitals are aligned along the Cartesian axes, the angles between them are 90 degrees. Specifically, there is a 90-degree angle between 2px and 2py, another 90-degree angle between 2py and 2pz, and a final 90-degree angle between 2pz and 2px.
04

Understanding electron probability distribution in p orbitals

It is also essential to understand the probability distribution of electrons in these orbitals. Electrons in p orbitals have a higher probability of being found along the axis of the orbital, and the probability decreases as we move towards the nodal plane. The electron density in each orbital is separate and does not overlap with the other orbitals. To sum up, the three orbitals in the 2p sublevel have a dumbbell shape and are aligned along the x, y, and z axes. They are mutually perpendicular to each other, with 90-degree angles between them. The probability distribution of electrons is localized along each axis, with nodal planes separating the lobes within each orbital, and between the different orbitals.

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 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Atomic Orbitals
In the realm of atomic structure, understanding atomic orbitals is crucial to grasping how electrons behave within an atom. An orbital refers to the region surrounding an atomic nucleus where there is a high likelihood of finding electrons. These orbitals are essential for defining the structure and chemical properties of an atom.
  • Each type of orbital鈥攕, p, d, f鈥攈as a unique shape and characteristic.
  • The p orbitals, for example, have a distinctive dumbbell shape that consists of two lobes.

The orientation and shape of these orbitals help in predicting how atoms will interact during chemical reactions. This understanding provides insight into molecular formation and the bonding properties of elements, all of which are fundamental to the study of chemistry and physics.
Electron Probability Distribution
When discussing atomic orbitals, understanding electron probability distribution is pivotal. This concept refers to the likelihood of finding an electron in a particular region around the nucleus. Within the p orbitals, the probability is not evenly distributed, due to their unique shape.
  • Electrons are more likely to be found in the lobes of the p orbital, distributed along an axis.
  • The likelihood diminishes as we approach the nodal plane, where the electron presence is virtually zero.

This probability distribution is visualized through electron density plots, which show regions of high probability. By evaluating these plots, one can predict where electrons are likely to be located, which is crucial for understanding an atom's reactivity and interaction with other atoms.
Nodal Planes
Nodal planes are fascinating structures within atomic orbitals. These are regions where the probability of finding an electron is exactly zero. In the context of p orbitals, each of which possesses a nodal plane, understanding these planes is essential for visualizing how electrons orbit the nucleus.
  • Nodal planes separate the two lobes of a p orbital, affecting its electron occupancy and symmetry.
  • The presence of nodal planes can influence chemical bonding and the overlap of orbitals within molecules.

The concept of nodal planes is important in quantum chemistry because it explains why certain transitions and reactions occur, or do not occur. They directly relate to the energy levels and behavior of electrons, underpinning many aspects of atomic theory and molecular chemistry.

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

Write ground-state electron configurations for the following elements. a. bromine (Br) c. antimony (Sb) e. terbium (Tb) b. strontium (Sr) d. rhenium (Re) f. titanium (Ti)

Neon Signs To make neon signs emit different colors, manufacturers often fill the signs with gases other than neon. Write an essay about the use of gases in neon signs and the colors produced by the gases.

Which element has the ground-state electron configuration represented by the noble-gas notation \([\mathrm{Rn}] 7 \mathrm{s}^{1} ?\)

When a sulfur atom reacts with other atoms, electrons in orbitals related to the atom鈥檚 third energy level are involved. How many such electrons does a sulfur atom have?

In what sequence do electrons fill the atomic orbitals related to a sublevel?
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Inorganic 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.