{"id":187548,"date":"2025-02-05T05:10:24","date_gmt":"2025-02-05T05:10:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=187548"},"modified":"2025-02-05T05:10:27","modified_gmt":"2025-02-05T05:10:27","slug":"compute-the-percents-ionic-character-of-the-interatomic-bonds-for-the-following-compounds","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/05\/compute-the-percents-ionic-character-of-the-interatomic-bonds-for-the-following-compounds\/","title":{"rendered":"Compute the percents ionic character of the interatomic bonds for the following compounds"},"content":{"rendered":"\n<p>Compute the percents ionic character of the interatomic bonds for the following compounds: TiO2, ZnTe, CsCl, InSb, and MgCl2.<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>To calculate the <strong>percent ionic character<\/strong> of a bond, we use the equation: %&nbsp;Ionic&nbsp;Character=(1\u2212e(\u2212(\u03c7A\u2212\u03c7B)24))\u00d7100\\% \\text{ Ionic Character} = \\left(1 &#8211; e^{\\left(\\frac{- ( \\chi_A &#8211; \\chi_B )^2}{4}\\right)}\\right) \\times 100<\/p>\n\n\n\n<p>where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>\u03c7A\\chi_A and \u03c7B\\chi_B are the electronegativities of the atoms in the bond.<\/li>\n\n\n\n<li>The exponent accounts for the difference in electronegativity squared, divided by 4.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Electronegativity Values (Pauling Scale)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Ti (Titanium):<\/strong> 1.54<\/li>\n\n\n\n<li><strong>O (Oxygen):<\/strong> 3.44<\/li>\n\n\n\n<li><strong>Zn (Zinc):<\/strong> 1.65<\/li>\n\n\n\n<li><strong>Te (Tellurium):<\/strong> 2.10<\/li>\n\n\n\n<li><strong>Cs (Cesium):<\/strong> 0.79<\/li>\n\n\n\n<li><strong>Cl (Chlorine):<\/strong> 3.16<\/li>\n\n\n\n<li><strong>In (Indium):<\/strong> 1.78<\/li>\n\n\n\n<li><strong>Sb (Antimony):<\/strong> 2.05<\/li>\n\n\n\n<li><strong>Mg (Magnesium):<\/strong> 1.31<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Calculations<\/strong>:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>TiO\u2082<\/strong>:<br>\u03c7Ti=1.54,\u03c7O=3.44\\chi_{\\text{Ti}} = 1.54, \\chi_{\\text{O}} = 3.44<br>\u0394\u03c7=3.44\u22121.54=1.90\\Delta\\chi = 3.44 &#8211; 1.54 = 1.90<br>%\u00a0Ionic\u00a0Character=(1\u2212e(\u2212(1.90)24))\u00d7100=55.0%\\% \\text{ Ionic Character} = \\left(1 &#8211; e^{\\left(\\frac{- (1.90)^2}{4}\\right)}\\right) \\times 100 = 55.0\\%<\/li>\n\n\n\n<li><strong>ZnTe<\/strong>:<br>\u03c7Zn=1.65,\u03c7Te=2.10\\chi_{\\text{Zn}} = 1.65, \\chi_{\\text{Te}} = 2.10<br>\u0394\u03c7=2.10\u22121.65=0.45\\Delta\\chi = 2.10 &#8211; 1.65 = 0.45<br>%\u00a0Ionic\u00a0Character=(1\u2212e(\u2212(0.45)24))\u00d7100=7.6%\\% \\text{ Ionic Character} = \\left(1 &#8211; e^{\\left(\\frac{- (0.45)^2}{4}\\right)}\\right) \\times 100 = 7.6\\%<\/li>\n\n\n\n<li><strong>CsCl<\/strong>:<br>\u03c7Cs=0.79,\u03c7Cl=3.16\\chi_{\\text{Cs}} = 0.79, \\chi_{\\text{Cl}} = 3.16<br>\u0394\u03c7=3.16\u22120.79=2.37\\Delta\\chi = 3.16 &#8211; 0.79 = 2.37<br>%\u00a0Ionic\u00a0Character=(1\u2212e(\u2212(2.37)24))\u00d7100=67.5%\\% \\text{ Ionic Character} = \\left(1 &#8211; e^{\\left(\\frac{- (2.37)^2}{4}\\right)}\\right) \\times 100 = 67.5\\%<\/li>\n\n\n\n<li><strong>InSb<\/strong>:<br>\u03c7In=1.78,\u03c7Sb=2.05\\chi_{\\text{In}} = 1.78, \\chi_{\\text{Sb}} = 2.05<br>\u0394\u03c7=2.05\u22121.78=0.27\\Delta\\chi = 2.05 &#8211; 1.78 = 0.27<br>%\u00a0Ionic\u00a0Character=(1\u2212e(\u2212(0.27)24))\u00d7100=3.7%\\% \\text{ Ionic Character} = \\left(1 &#8211; e^{\\left(\\frac{- (0.27)^2}{4}\\right)}\\right) \\times 100 = 3.7\\%<\/li>\n\n\n\n<li><strong>MgCl\u2082<\/strong>:<br>\u03c7Mg=1.31,\u03c7Cl=3.16\\chi_{\\text{Mg}} = 1.31, \\chi_{\\text{Cl}} = 3.16<br>\u0394\u03c7=3.16\u22121.31=1.85\\Delta\\chi = 3.16 &#8211; 1.31 = 1.85<br>%\u00a0Ionic\u00a0Character=(1\u2212e(\u2212(1.85)24))\u00d7100=53.2%\\% \\text{ Ionic Character} = \\left(1 &#8211; e^{\\left(\\frac{- (1.85)^2}{4}\\right)}\\right) \\times 100 = 53.2\\%<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation:<\/strong><\/h3>\n\n\n\n<p>The percent ionic character of a bond depends on the electronegativity difference between the two atoms. A higher difference results in a more <strong>ionic bond<\/strong>, while a smaller difference results in a <strong>more covalent bond<\/strong>.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>CsCl has the highest ionic character (67.5%)<\/strong> because it consists of a highly electropositive metal (Cs) and a highly electronegative non-metal (Cl), leading to a strong electrostatic attraction.<\/li>\n\n\n\n<li><strong>TiO\u2082 and MgCl\u2082 have moderately high ionic characters (~55%)<\/strong> since both involve a metal and a highly electronegative element (oxygen or chlorine).<\/li>\n\n\n\n<li><strong>ZnTe and InSb have the lowest ionic characters (~3.7%\u20137.6%)<\/strong>, meaning their bonds are mostly covalent.<\/li>\n<\/ul>\n\n\n\n<p>This calculation is important in materials science to determine the <strong>physical and electrical properties<\/strong> of compounds. Highly ionic compounds (e.g., CsCl, MgCl\u2082) tend to have <strong>high melting points and solubility in water<\/strong>, while covalent compounds (e.g., InSb) are often <strong>semiconductors<\/strong> due to their lower ionic character.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Compute the percents ionic character of the interatomic bonds for the following compounds: TiO2, ZnTe, CsCl, InSb, and MgCl2. The Correct Answer and Explanation is : To calculate the percent ionic character of a bond, we use the equation: %&nbsp;Ionic&nbsp;Character=(1\u2212e(\u2212(\u03c7A\u2212\u03c7B)24))\u00d7100\\% \\text{ Ionic Character} = \\left(1 &#8211; e^{\\left(\\frac{- ( \\chi_A &#8211; \\chi_B )^2}{4}\\right)}\\right) \\times 100 where: [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-187548","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187548","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=187548"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187548\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187548"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187548"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187548"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}