/*! 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 28 Without using Fig. \(8.3\), pred... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 28

Without using Fig. \(8.3\), predict the order of increasing electronegativity in each of the following groups of elements. a. \(\mathrm{Na}, \mathrm{K}, \mathrm{Rb}\) c. \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}\) b. \(\mathrm{B}, \mathrm{O}, \mathrm{Ga}\) d. \(\mathrm{S}, \mathrm{O}, \mathrm{F}\)

Short Answer

Expert verified
a. Rb < K < Na b. Br < Cl < F c. Ga < B < O d. S < O < F

Step by step solution

01

a. Na, K, Rb

These elements are alkali metals (group 1) in the periodic table. As we move down the group, the electronegativity decreases. So the order of increasing electronegativity is: Rb < K < Na.
02

b. F, Cl, Br

These elements are halogens (group 17) in the periodic table. Similar to group 1 elements, the electronegativity decreases as we move down the group. Therefore, the order of increasing electronegativity is: Br < Cl < F.
03

c. B, O, Ga

Here, the elements are from different groups. B is from group 13, O is from group 16, and Ga is also from group 13. As we move across a period from left to right, electronegativity increases, and as we move down a group, electronegativity decreases. So the order of increasing electronegativity is: Ga < B < O.
04

d. S, O, F

In this group, S is from group 16, O is also from group 16, and F is from group 17. As we move across a period from left to right, electronegativity increases, and within the same group, it decreases as we move down. Therefore, the order of increasing electronegativity is: S < O < F.

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!

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 Lewis structures that obey the octet rule (duet rule for \(\mathrm{H}\) ) for each of the following molecules. a. \(\mathrm{H}_{2} \mathrm{CO}\) b. \(\mathrm{CO}_{2}\) c. HCN Except for \(\mathrm{HCN}\) and \(\mathrm{H}_{2} \mathrm{CO}\), the first atom listed is the central atom. For \(\mathrm{HCN}\) and \(\mathrm{H}_{2} \mathrm{CO}\), carbon is the central atom. Carbon is the central atom in all of these molecules.

Predict the molecular structure for each of the following. (See Exercises 105 and \(106 .\) ) a. \(\mathrm{BrFI}_{2}\) b. \(\mathrm{XeO}_{2} \mathrm{~F}_{2}\) c. \(\mathrm{TeF}_{2} \mathrm{Cl}_{3}^{-}\) For each formula there are at least two different structures that can be drawn using the same central atom. Draw all possible structures for each formula.

What do each of the following sets of compounds/ions have in common with each other? a. \(\mathrm{SO}_{3}, \mathrm{NO}_{3}^{-}, \mathrm{CO}_{3}^{2-}\) b. \(\mathrm{O}_{3}, \mathrm{SO}_{2}, \mathrm{NO}_{2}^{-}\)

For each of the following groups, place the atoms and/or ions in order of decreasing size. a. \(\mathrm{V}, \mathrm{V}^{2+}, \mathrm{V}^{3+}, \mathrm{V}^{5+}\) b. \(\mathrm{Na}^{+}, \mathrm{K}^{+}, \mathrm{Rb}^{+}, \mathrm{Cs}^{+}\) c. \(\mathrm{Te}^{2-}, \mathrm{I}^{-}, \mathrm{Cs}^{+}, \mathrm{Ba}^{2+}\) d. \(\mathrm{P}, \mathrm{P}^{-}, \mathrm{P}^{2-}, \mathrm{P}^{3-}\) e. \(\mathrm{O}^{2-}, \mathrm{S}^{2-}, \mathrm{Se}^{2-}, \mathrm{Te}^{2-}\)

When comparing the size of different ions, the general radii trend discussed in Chapter 7 is usually not very useful. What do you concentrate on when comparing sizes of ions to each other or when comparing the size of an ion to its neutral atom?
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

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.