   # What is the trend in sizes of the ions K + , S 2− , and Cl − ? (a) K + &gt; S 2− &gt; Cl − (b) K + &lt; S 2− &lt; Cl − (c) S 2− &lt; Cl − &lt; K + (d) S 2− &gt; Cl − &gt; K + ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 7.5, Problem 1RC
Textbook Problem
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## What is the trend in sizes of the ions K+, S2−, and Cl−? (a) K+ > S2− > Cl− (b) K+ < S2− < Cl− (c) S2− < Cl− < K+ (d) S2− > Cl− > K+

Interpretation Introduction

Interpretation:

The ionic size should be identified given the statement of three different (s-block and p-block) ions.

Concept Introduction:

Atomic radius: The concept explain chemical element is a measured of the size of its atoms, in other words to measure the distance from the center of the nucleus to the boundary of the surrounding cloud of number of electrons.

Increase and decrease electronegativity: The less vacancy electrons an atoms has the least it will gain of electrons. Moreover the electron affinity decrease down the groups and from right to left across the periods on the periodic table, the reason is electrons are placed in a higher energy level far from the nucleus thus a decrease from its pull.

Electron attachment enthalpy: ΔEAH is defined as the enthalpy change occurring when a gaseous atom adds an electron forming a gaseous anion.

A(g)+e-A-(g)----ElectronattachmententhalpyEAH

### Explanation of Solution

According to periodic table was clearly explained the all (s, p, d, f) block elements atomic size will increase when left side to right side. Than all atomic size will be increase when above to below.

Further we analyzed for increasing sizes of given three different ions are shown below.

The sulfur ions (S2-) atomic radius greater than the Chlorine, and potassium (Cl-, K+) ions because addition of shells for (S2-) ions. Hence atomic number of S=16, Chlorine and potassium atomic number (Z=17 and 19), in this statement (S) ions having larger atomic radius than (Cl, K) ions (Figure: 1). This attraction between the nucleus and the electrons decreases as you move to the left of a period and down a group.

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