{"id":245267,"date":"2025-07-05T20:10:25","date_gmt":"2025-07-05T20:10:25","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=245267"},"modified":"2025-07-05T20:10:27","modified_gmt":"2025-07-05T20:10:27","slug":"draw-the-lewis-structure-for-each-of-the-following-molecules-or-ions-and-predict-their-electron-domain-and-molecular-geometries","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/05\/draw-the-lewis-structure-for-each-of-the-following-molecules-or-ions-and-predict-their-electron-domain-and-molecular-geometries\/","title":{"rendered":"Draw the Lewis structure for each of the following molecules or ions, and predict their electron-domain and molecular geometries"},"content":{"rendered":"\n
Draw the Lewis structure for each of the following molecules or ions, and predict their electron-domain and molecular geometries: HCN, SO2, SF4, PF6-, NH4+, N2, AsF5, CH4, BrF3, ClO2, XeF2, BrO2<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
1. HCN (Hydrogen Cyanide)<\/strong><\/h3>\n\n\n\n
Lewis Structure:<\/strong><\/p>\n\n\n\n
\n
H is bonded to C, and C is triple-bonded to N (C\u2261N).<\/li>\n\n\n\n
There are 10 valence electrons in total, which are distributed as follows: H (2), C (4), N (5).<\/li>\n\n\n\n
The C\u2261N bond is a triple bond, with one lone pair on C and one lone pair on N.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Linear Molecular Geometry:<\/strong> Linear The molecule has a straight line structure, with no lone pairs on the central atoms.<\/p>\n\n\n\n\n\n\n\n
2. SO2 (Sulfur Dioxide)<\/strong><\/h3>\n\n\n\n
Lewis Structure:<\/strong><\/p>\n\n\n\n
\n
S is double-bonded to both O atoms (O=S=O).<\/li>\n\n\n\n
The sulfur has one lone pair, and each oxygen has two lone pairs.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Trigonal Planar Molecular Geometry:<\/strong> Bent The lone pair on sulfur causes a bent shape due to electron repulsion.<\/p>\n\n\n\n\n\n\n\n
P is in the center, bonded to six F atoms (P-F).<\/li>\n\n\n\n
There are no lone pairs on the phosphorus atom, and the ion has an extra electron, giving it a negative charge.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Octahedral Molecular Geometry:<\/strong> Octahedral There is symmetry with no lone pairs, so the geometry is octahedral.<\/p>\n\n\n\n\n\n\n\n
5. NH4+ (Ammonium Ion)<\/strong><\/h3>\n\n\n\n
Lewis Structure:<\/strong><\/p>\n\n\n\n
\n
N is bonded to four H atoms (N-H).<\/li>\n\n\n\n
There are no lone pairs on nitrogen.<\/li>\n\n\n\n
The positive charge is on the nitrogen atom, indicating it has lost one electron.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Tetrahedral Molecular Geometry:<\/strong> Tetrahedral The geometry remains tetrahedral, as all four bonds are equivalent.<\/p>\n\n\n\n\n\n\n\n
6. N2 (Nitrogen Molecule)<\/strong><\/h3>\n\n\n\n
Lewis Structure:<\/strong><\/p>\n\n\n\n
\n
N\u2261N with each nitrogen having one lone pair.<\/li>\n\n\n\n
There are 10 valence electrons, distributed as follows: N (5) + N (5).<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Linear Molecular Geometry:<\/strong> Linear The molecule is linear with a triple bond between the nitrogen atoms.<\/p>\n\n\n\n\n\n\n\n
As is in the center, bonded to five F atoms (As-F).<\/li>\n\n\n\n
There are no lone pairs on arsenic.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Trigonal Bipyramidal Molecular Geometry:<\/strong> Trigonal Bipyramidal The arrangement is symmetric with no lone pairs.<\/p>\n\n\n\n\n\n\n\n
8. CH4 (Methane)<\/strong><\/h3>\n\n\n\n
Lewis Structure:<\/strong><\/p>\n\n\n\n
\n
C is in the center, bonded to four H atoms (C-H).<\/li>\n\n\n\n
There are no lone pairs on carbon.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Tetrahedral Molecular Geometry:<\/strong> Tetrahedral The geometry is tetrahedral, with all bonds equal and no lone pairs.<\/p>\n\n\n\n\n\n\n\n
Br is bonded to three F atoms (Br-F).<\/li>\n\n\n\n
There are two lone pairs on bromine.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Trigonal Bipyramidal Molecular Geometry:<\/strong> T-shaped The lone pairs occupy equatorial positions, leading to the T-shaped geometry.<\/p>\n\n\n\n\n\n\n\n
There is one lone pair on chlorine, and each oxygen has two lone pairs.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Bent Molecular Geometry:<\/strong> Bent The lone pair on chlorine causes the molecule to be bent, even though it would have been linear without the lone pair.<\/p>\n\n\n\n\n\n\n\n
There are three lone pairs on xenon.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Octahedral Molecular Geometry:<\/strong> Linear The three lone pairs occupy the equatorial positions, and the two F atoms are placed in a linear arrangement.<\/p>\n\n\n\n\n\n\n\n
There are two lone pairs on bromine.<\/li>\n<\/ul>\n\n\n\n
Electron-Domain Geometry:<\/strong> Trigonal Planar Molecular Geometry:<\/strong> Bent The two lone pairs on bromine push the O atoms into a bent shape.<\/p>\n\n\n\n\n\n\n\n
In summary, the molecular geometries vary due to the number of bonding and nonbonding electron pairs around the central atoms.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
Draw the Lewis structure for each of the following molecules or ions, and predict their electron-domain and molecular geometries: HCN, SO2, SF4, PF6-, NH4+, N2, AsF5, CH4, BrF3, ClO2, XeF2, BrO2 The Correct Answer and Explanation is: 1. HCN (Hydrogen Cyanide) Lewis Structure: Electron-Domain Geometry: LinearMolecular Geometry: LinearThe molecule has a straight line structure, with […]<\/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-245267","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/245267","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=245267"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/245267\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=245267"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=245267"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=245267"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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