Let’s break down the molecular structures and their key features for each compound:<\/p>\n\n\n\n
1. SO3 (Sulfur Trioxide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 24<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Trigonal<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Trigonal Planar<\/li>\n\n\n\n
- Bond Angles<\/strong>: 120\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
SO3 has 24 valence electrons, and in its structure, the central sulfur atom is bonded to three oxygen atoms through double bonds. This leads to a trigonal planar geometry with 120\u00b0 bond angles. Because the molecule has symmetry and no lone pairs on the central sulfur, it is nonpolar.<\/p>\n\n\n\n
2. HCN (Hydrogen Cyanide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 10<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Bond Angles<\/strong>: 180\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/li>\n<\/ul>\n\n\n\n
HCN has 10 valence electrons, with a linear structure. The molecule consists of a hydrogen atom bonded to a carbon atom, which is triple-bonded to a nitrogen atom. This molecule is linear with a bond angle of 180\u00b0. Since the electronegativities of carbon and nitrogen differ, HCN is polar.<\/p>\n\n\n\n
3. SO2 (Sulfur Dioxide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 18<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Trigonal<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Bent<\/li>\n\n\n\n
- Bond Angles<\/strong>: 120\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/li>\n<\/ul>\n\n\n\n
SO2 has 18 valence electrons and adopts a trigonal electron pair geometry, with a bent molecular geometry due to the lone pair on sulfur. This results in a bond angle of approximately 120\u00b0. SO2 is polar because of its asymmetric structure.<\/p>\n\n\n\n
4. CS2 (Carbon Disulfide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 16<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Bond Angles<\/strong>: 180\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
CS2 has 16 valence electrons, and its structure is linear, with a carbon atom bonded to two sulfur atoms by double bonds. The bond angle is 180\u00b0, and the molecule is nonpolar due to its symmetric linear shape.<\/p>\n\n\n\n
5. CH4 (Methane)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 8<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Bond Angles<\/strong>: 109.5\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
CH4 has 8 valence electrons and adopts a tetrahedral electron pair geometry, with four single bonds between carbon and hydrogen atoms. The bond angles are approximately 109.5\u00b0. Methane is nonpolar because of its symmetrical shape.<\/p>\n\n\n\n
\n\n\n\nSummary:<\/h3>\n\n\n\n\n- SO3<\/strong>: Nonpolar, trigonal planar (120\u00b0)<\/li>\n\n\n\n
- HCN<\/strong>: Polar, linear (180\u00b0)<\/li>\n\n\n\n
- SO2<\/strong>: Polar, bent (120\u00b0)<\/li>\n\n\n\n
- CS2<\/strong>: Nonpolar, linear (180\u00b0)<\/li>\n\n\n\n
- CH4<\/strong>: Nonpolar, tetrahedral (109.5\u00b0)<\/li>\n<\/ul>\n\n\n\n
These molecules differ in polarity and geometry based on the distribution of electrons and bonding arrangements.<\/p>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-897.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"Compound Total Valence Lewis Structure Electron Pair Molecular Approximate Polar? Electrons Geometry Geometry Bond Angles SO3 24 trigonal trigonal planar planar HCN H-C?N SO2 18 CS2 CH4 8 H H-C-H tetrahedral tetrahedral H The Correct Answer and Explanation is: Let’s break down the molecular structures and their key features for each compound: 1. SO3 (Sulfur […]<\/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-246603","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603","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=246603"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246603"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246603"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246603"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
SO3 has 24 valence electrons, and in its structure, the central sulfur atom is bonded to three oxygen atoms through double bonds. This leads to a trigonal planar geometry with 120\u00b0 bond angles. Because the molecule has symmetry and no lone pairs on the central sulfur, it is nonpolar.<\/p>\n\n\n\n
2. HCN (Hydrogen Cyanide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 10<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Bond Angles<\/strong>: 180\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/li>\n<\/ul>\n\n\n\n
HCN has 10 valence electrons, with a linear structure. The molecule consists of a hydrogen atom bonded to a carbon atom, which is triple-bonded to a nitrogen atom. This molecule is linear with a bond angle of 180\u00b0. Since the electronegativities of carbon and nitrogen differ, HCN is polar.<\/p>\n\n\n\n
3. SO2 (Sulfur Dioxide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 18<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Trigonal<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Bent<\/li>\n\n\n\n
- Bond Angles<\/strong>: 120\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/li>\n<\/ul>\n\n\n\n
SO2 has 18 valence electrons and adopts a trigonal electron pair geometry, with a bent molecular geometry due to the lone pair on sulfur. This results in a bond angle of approximately 120\u00b0. SO2 is polar because of its asymmetric structure.<\/p>\n\n\n\n
4. CS2 (Carbon Disulfide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 16<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Bond Angles<\/strong>: 180\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
CS2 has 16 valence electrons, and its structure is linear, with a carbon atom bonded to two sulfur atoms by double bonds. The bond angle is 180\u00b0, and the molecule is nonpolar due to its symmetric linear shape.<\/p>\n\n\n\n
5. CH4 (Methane)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 8<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Bond Angles<\/strong>: 109.5\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
CH4 has 8 valence electrons and adopts a tetrahedral electron pair geometry, with four single bonds between carbon and hydrogen atoms. The bond angles are approximately 109.5\u00b0. Methane is nonpolar because of its symmetrical shape.<\/p>\n\n\n\n
\n\n\n\nSummary:<\/h3>\n\n\n\n\n- SO3<\/strong>: Nonpolar, trigonal planar (120\u00b0)<\/li>\n\n\n\n
- HCN<\/strong>: Polar, linear (180\u00b0)<\/li>\n\n\n\n
- SO2<\/strong>: Polar, bent (120\u00b0)<\/li>\n\n\n\n
- CS2<\/strong>: Nonpolar, linear (180\u00b0)<\/li>\n\n\n\n
- CH4<\/strong>: Nonpolar, tetrahedral (109.5\u00b0)<\/li>\n<\/ul>\n\n\n\n
These molecules differ in polarity and geometry based on the distribution of electrons and bonding arrangements.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Compound Total Valence Lewis Structure Electron Pair Molecular Approximate Polar? Electrons Geometry Geometry Bond Angles SO3 24 trigonal trigonal planar planar HCN H-C?N SO2 18 CS2 CH4 8 H H-C-H tetrahedral tetrahedral H The Correct Answer and Explanation is: Let’s break down the molecular structures and their key features for each compound: 1. SO3 (Sulfur […]<\/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-246603","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603","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=246603"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246603"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246603"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246603"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
HCN has 10 valence electrons, with a linear structure. The molecule consists of a hydrogen atom bonded to a carbon atom, which is triple-bonded to a nitrogen atom. This molecule is linear with a bond angle of 180\u00b0. Since the electronegativities of carbon and nitrogen differ, HCN is polar.<\/p>\n\n\n\n
3. SO2 (Sulfur Dioxide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 18<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Trigonal<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Bent<\/li>\n\n\n\n
- Bond Angles<\/strong>: 120\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Polar<\/li>\n<\/ul>\n\n\n\n
SO2 has 18 valence electrons and adopts a trigonal electron pair geometry, with a bent molecular geometry due to the lone pair on sulfur. This results in a bond angle of approximately 120\u00b0. SO2 is polar because of its asymmetric structure.<\/p>\n\n\n\n
4. CS2 (Carbon Disulfide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 16<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Bond Angles<\/strong>: 180\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
CS2 has 16 valence electrons, and its structure is linear, with a carbon atom bonded to two sulfur atoms by double bonds. The bond angle is 180\u00b0, and the molecule is nonpolar due to its symmetric linear shape.<\/p>\n\n\n\n
5. CH4 (Methane)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 8<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Bond Angles<\/strong>: 109.5\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
CH4 has 8 valence electrons and adopts a tetrahedral electron pair geometry, with four single bonds between carbon and hydrogen atoms. The bond angles are approximately 109.5\u00b0. Methane is nonpolar because of its symmetrical shape.<\/p>\n\n\n\n
\n\n\n\nSummary:<\/h3>\n\n\n\n\n- SO3<\/strong>: Nonpolar, trigonal planar (120\u00b0)<\/li>\n\n\n\n
- HCN<\/strong>: Polar, linear (180\u00b0)<\/li>\n\n\n\n
- SO2<\/strong>: Polar, bent (120\u00b0)<\/li>\n\n\n\n
- CS2<\/strong>: Nonpolar, linear (180\u00b0)<\/li>\n\n\n\n
- CH4<\/strong>: Nonpolar, tetrahedral (109.5\u00b0)<\/li>\n<\/ul>\n\n\n\n
These molecules differ in polarity and geometry based on the distribution of electrons and bonding arrangements.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Compound Total Valence Lewis Structure Electron Pair Molecular Approximate Polar? Electrons Geometry Geometry Bond Angles SO3 24 trigonal trigonal planar planar HCN H-C?N SO2 18 CS2 CH4 8 H H-C-H tetrahedral tetrahedral H The Correct Answer and Explanation is: Let’s break down the molecular structures and their key features for each compound: 1. SO3 (Sulfur […]<\/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-246603","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603","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=246603"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246603"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246603"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246603"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
SO2 has 18 valence electrons and adopts a trigonal electron pair geometry, with a bent molecular geometry due to the lone pair on sulfur. This results in a bond angle of approximately 120\u00b0. SO2 is polar because of its asymmetric structure.<\/p>\n\n\n\n
4. CS2 (Carbon Disulfide)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 16<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Bond Angles<\/strong>: 180\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
CS2 has 16 valence electrons, and its structure is linear, with a carbon atom bonded to two sulfur atoms by double bonds. The bond angle is 180\u00b0, and the molecule is nonpolar due to its symmetric linear shape.<\/p>\n\n\n\n
5. CH4 (Methane)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 8<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Bond Angles<\/strong>: 109.5\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
CH4 has 8 valence electrons and adopts a tetrahedral electron pair geometry, with four single bonds between carbon and hydrogen atoms. The bond angles are approximately 109.5\u00b0. Methane is nonpolar because of its symmetrical shape.<\/p>\n\n\n\n
\n\n\n\nSummary:<\/h3>\n\n\n\n\n- SO3<\/strong>: Nonpolar, trigonal planar (120\u00b0)<\/li>\n\n\n\n
- HCN<\/strong>: Polar, linear (180\u00b0)<\/li>\n\n\n\n
- SO2<\/strong>: Polar, bent (120\u00b0)<\/li>\n\n\n\n
- CS2<\/strong>: Nonpolar, linear (180\u00b0)<\/li>\n\n\n\n
- CH4<\/strong>: Nonpolar, tetrahedral (109.5\u00b0)<\/li>\n<\/ul>\n\n\n\n
These molecules differ in polarity and geometry based on the distribution of electrons and bonding arrangements.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Compound Total Valence Lewis Structure Electron Pair Molecular Approximate Polar? Electrons Geometry Geometry Bond Angles SO3 24 trigonal trigonal planar planar HCN H-C?N SO2 18 CS2 CH4 8 H H-C-H tetrahedral tetrahedral H The Correct Answer and Explanation is: Let’s break down the molecular structures and their key features for each compound: 1. SO3 (Sulfur […]<\/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-246603","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603","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=246603"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246603"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246603"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246603"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
CS2 has 16 valence electrons, and its structure is linear, with a carbon atom bonded to two sulfur atoms by double bonds. The bond angle is 180\u00b0, and the molecule is nonpolar due to its symmetric linear shape.<\/p>\n\n\n\n
5. CH4 (Methane)<\/strong><\/h3>\n\n\n\n\n- Total Valence Electrons<\/strong>: 8<\/li>\n\n\n\n
- Electron Pair Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Bond Angles<\/strong>: 109.5\u00b0<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar<\/li>\n<\/ul>\n\n\n\n
CH4 has 8 valence electrons and adopts a tetrahedral electron pair geometry, with four single bonds between carbon and hydrogen atoms. The bond angles are approximately 109.5\u00b0. Methane is nonpolar because of its symmetrical shape.<\/p>\n\n\n\n
\n\n\n\nSummary:<\/h3>\n\n\n\n\n- SO3<\/strong>: Nonpolar, trigonal planar (120\u00b0)<\/li>\n\n\n\n
- HCN<\/strong>: Polar, linear (180\u00b0)<\/li>\n\n\n\n
- SO2<\/strong>: Polar, bent (120\u00b0)<\/li>\n\n\n\n
- CS2<\/strong>: Nonpolar, linear (180\u00b0)<\/li>\n\n\n\n
- CH4<\/strong>: Nonpolar, tetrahedral (109.5\u00b0)<\/li>\n<\/ul>\n\n\n\n
These molecules differ in polarity and geometry based on the distribution of electrons and bonding arrangements.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Compound Total Valence Lewis Structure Electron Pair Molecular Approximate Polar? Electrons Geometry Geometry Bond Angles SO3 24 trigonal trigonal planar planar HCN H-C?N SO2 18 CS2 CH4 8 H H-C-H tetrahedral tetrahedral H The Correct Answer and Explanation is: Let’s break down the molecular structures and their key features for each compound: 1. SO3 (Sulfur […]<\/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-246603","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603","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=246603"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246603"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246603"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246603"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
CH4 has 8 valence electrons and adopts a tetrahedral electron pair geometry, with four single bonds between carbon and hydrogen atoms. The bond angles are approximately 109.5\u00b0. Methane is nonpolar because of its symmetrical shape.<\/p>\n\n\n\n
\n\n\n\n
Summary:<\/h3>\n\n\n\n\n- SO3<\/strong>: Nonpolar, trigonal planar (120\u00b0)<\/li>\n\n\n\n
- HCN<\/strong>: Polar, linear (180\u00b0)<\/li>\n\n\n\n
- SO2<\/strong>: Polar, bent (120\u00b0)<\/li>\n\n\n\n
- CS2<\/strong>: Nonpolar, linear (180\u00b0)<\/li>\n\n\n\n
- CH4<\/strong>: Nonpolar, tetrahedral (109.5\u00b0)<\/li>\n<\/ul>\n\n\n\n
These molecules differ in polarity and geometry based on the distribution of electrons and bonding arrangements.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Compound Total Valence Lewis Structure Electron Pair Molecular Approximate Polar? Electrons Geometry Geometry Bond Angles SO3 24 trigonal trigonal planar planar HCN H-C?N SO2 18 CS2 CH4 8 H H-C-H tetrahedral tetrahedral H The Correct Answer and Explanation is: Let’s break down the molecular structures and their key features for each compound: 1. SO3 (Sulfur […]<\/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-246603","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603","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=246603"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246603"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246603"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246603"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
These molecules differ in polarity and geometry based on the distribution of electrons and bonding arrangements.<\/p>\n\n\n\n Compound Total Valence Lewis Structure Electron Pair Molecular Approximate Polar? Electrons Geometry Geometry Bond Angles SO3 24 trigonal trigonal planar planar HCN H-C?N SO2 18 CS2 CH4 8 H H-C-H tetrahedral tetrahedral H The Correct Answer and Explanation is: Let’s break down the molecular structures and their key features for each compound: 1. SO3 (Sulfur […]<\/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-246603","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603","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=246603"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246603\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246603"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246603"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246603"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}<\/figure>\n","protected":false},"excerpt":{"rendered":"