/*! 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 2 The number of incomplete orbital... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 2

The number of incomplete orbitals in inner transitior elements is? (a) 1 (b) 4 (c) 2 (d) 3

Short Answer

Expert verified
The question does not provide enough information to give a specific answer as incomplete orbitals may vary among different inner transition elements; typically, there can be 1 to 7 incomplete f orbitals.

Step by step solution

01

Definition of Inner Transition Elements

First, understand that inner transition elements are the elements that include the lanthanides and actinides, which are found in the f-block of the periodic table.
02

Electronic Configuration of Inner Transition Elements

Next, learn that inner transition elements have their last electron added to an f subshell. An f subshell can hold a maximum of 14 electrons, which can be distributed over 7 orbitals.
03

Determination of Incomplete Orbitals

Since each orbital can hold a maximum of 2 electrons, with 14 electrons, the f subshell can be full with 7 orbitals. However, not all inner transition elements have a full f subshell, leading to incomplete orbitals. These incomplete orbitals correspond to the question asked.
04

Counting Incomplete Orbitals

In general, inner transition elements can have anywhere from 0 to 7 incomplete f orbitals. But typically, most of the elements in their ground states will have less than 7 orbitals filled, resulting in some incomplete orbitals. To identify the exact number of incomplete orbitals, it's important to look at individual electron configurations. However, since no specific element is mentioned, an exact number cannot be given without additional information.

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.

f-block Elements
Understanding the f-block elements is pivotal in building a solid foundation in chemistry, especially when dealing with inner transition elements. These elements are characterized by the filling of their f-orbitals and are located in the f-block of the periodic table, including the lanthanides (cerium to lutetium) and the actinides (thorium to lawrencium).

These periods of elements are nestled at the bottom of the periodic table to preserve the table's structure due to their unique properties and long periods. The f-block elements are known for their variable oxidation states and the properties of their compounds, which are often determined by their incomplete f-orbitals. This characteristic is vital for understanding the complex chemistry of these elements, including their use in catalysts, in the production of strong magnets, and in various other technological applications.
Electronic Configuration
The electronic configuration of an atom is essentially a map showing the distribution of electrons across different energy levels and subshells. For the f-block elements鈥攐ur focus on inner transition elements鈥攖he last electron enters the f-orbital. Here's where it gets nuanced: the f-orbital can house up to 14 electrons, and these are distributed across seven orbitals.

Each of these seven f-orbitals can hold two electrons鈥攖he spin pairing rule where electrons fill orbitals so that their spins are opposite. The intriguing part is as electrons populate these orbitals, they illustrate the element's properties and determine its incomplete orbitals. Grasping the electronic configurations of these elements allows chemists and students alike to predict reactivity, magnetic properties, and color of the compounds formed by inner transition elements.
Incomplete Orbitals
An incomplete orbital is one that does not have its maximum possible number of electrons鈥攎eaning it's not completely occupied. For the f-subshell, with its seven orbitals, this status of completion or incompletion decides the chemical behavior. When inner transition elements have one or more of these f-orbitals unfilled, they are referred to as having incomplete orbitals.

This incompleteness leads to the variety and complexity seen in the chemistry of lanthanides and actinides. The number of incomplete orbitals can affect the element's magnetism, color, and bonding capacity. For many f-block elements in their ground states, not all seven orbitals are fully occupied, resulting in a lower number of incomplete orbitals than the seven possible. Therefore, having a clear picture of electron configurations can aid in predicting the number of incomplete orbitals and subsequently the physical and chemical characteristics of these intricate elements.

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

Lanthanoides are (a) 14 elements in the VI period (atomic number = 58 to 71) that are filling the \(4 \mathrm{f}\) -sublevel (b) 14 elements in the VII period (atomic number = 50 to 71) that are filling the \(4 \mathrm{f}\) -sublevel (c) 14 elements in the VII period (atomic number = 90 to 103 ) that are filling the 5 f-sublevel (d) 14 elements in the VI period (atomic number = 90 to 103 ) that are filling the \(4 \mathrm{f}\) -sublevel

Which compound is coloured due to charge transfer spectra and not due to \(\mathrm{d}-\mathrm{d}\) transitions? (a) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) (b) \(\mathrm{KMnO}_{4}\) (c) \(\mathrm{CrO}_{3}\) (d) All of these

The correct order of ionic radii of \(\mathrm{Y}^{3+}, \mathrm{La}^{3+}, \mathrm{Eu}^{3+}\) and \(\mathrm{Lu}^{3+}\) is: (a) \(\mathrm{Lu}^{3+}<\mathrm{Eu}^{3+}<\mathrm{La}^{3+}<\mathrm{Y}^{3+}\) (b) \(\mathrm{La}^{3+}<\mathrm{Eu}^{3+}<\mathrm{Lu}^{3+}<\mathrm{Y}^{3+}\) (c) \(\mathrm{Y}^{3+}<\mathrm{La}^{3+}<\mathrm{Eu}^{3+}<\mathrm{Lu}^{3+}\) (d) \(\mathrm{Y}^{3+}<\mathrm{Lu}^{3+}<\mathrm{Eu}^{3+}<\mathrm{La}^{3+}\)

Which one of the following ions is colourless in its aqueous solution? (a) \(\mathrm{T}_{1}^{3+}\) (b) \(\mathrm{Cu}^{2+}\) (c) \(\mathrm{Ni}^{2+}\) (d) \(\mathrm{Zn}^{2+}\)

Which of the following set represents only coloured ions? (1) \(\mathrm{Fe}^{3+}\) (2) \(\mathrm{Sc}^{3+}\) (3) \(\mathrm{Cu}^{2+}\) (4) \(\mathrm{Cr}^{3+}\) (a) 1,3 (b) \(2,3,4\) (c) \(1,2,4\) (d) 1,3 and 4
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Kinetics

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.