{"id":188061,"date":"2025-02-06T10:04:01","date_gmt":"2025-02-06T10:04:01","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=188061"},"modified":"2025-02-06T10:04:03","modified_gmt":"2025-02-06T10:04:03","slug":"molecular-formula-total-number-of-valence-electrons-lewis-structure-molecular-geometry-sih4-h20-so2-cifs","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/06\/molecular-formula-total-number-of-valence-electrons-lewis-structure-molecular-geometry-sih4-h20-so2-cifs\/","title":{"rendered":"Molecular Formula Total Number of Valence Electrons Lewis Structure Molecular Geometry SiH4 H20 SO2 CIFs"},"content":{"rendered":"\n<p>Molecular Formula Total Number of Valence Electrons Lewis Structure Molecular Geometry SiH4 H20 SO2 CIFs Molecular Formula Total Number of Valence Electrons Lewis Structure Molecular Geometry NH4 XeF4 CO2 NO: H2CO<\/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>Let&#8217;s analyze the molecular formulas, total number of valence electrons, Lewis structures, and molecular geometries for the specified compounds:<\/p>\n\n\n\n<p><strong>1. SiH\u2084 (Silane):<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons:<\/strong> Silicon (Si) contributes 4 valence electrons, and each hydrogen (H) contributes 1, totaling 8 valence electrons.- <strong>Lewis Structure:<\/strong> Silicon is the central atom bonded to four hydrogen atoms, forming single bonds.- <strong>Molecular Geometry:<\/strong> Tetrahedral, with bond angles of approximately 109.5\u00b0.<br><strong>2. H\u2082O (Water):<\/strong><\/li>\n\n\n\n<li><strong>Valence Electrons:<\/strong> Oxygen (O) contributes 6 valence electrons, and each hydrogen contributes 1, totaling 8 valence electrons.- <strong>Lewis Structure:<\/strong> Oxygen is bonded to two hydrogen atoms with two lone pairs of electrons.- <strong>Molecular Geometry:<\/strong> Bent (angular), with a bond angle of approximately 104.5\u00b0.<br><strong>3. SO\u2082 (Sulfur Dioxide):<\/strong><\/li>\n\n\n\n<li><strong>Valence Electrons:<\/strong> Sulfur (S) contributes 6 valence electrons, and each oxygen contributes 6, totaling 18 valence electrons.- <strong>Lewis Structure:<\/strong> Sulfur is double-bonded to two oxygen atoms, with one lone pair on sulfur and two lone pairs on each oxygen.- <strong>Molecular Geometry:<\/strong> Bent, with a bond angle of approximately 120\u00b0.<br><strong>4. ClF\u2083 (Chlorine Trifluoride):<\/strong><\/li>\n\n\n\n<li><strong>Valence Electrons:<\/strong> Chlorine (Cl) contributes 7 valence electrons, and each fluorine (F) contributes 7, totaling 26 valence electrons.- <strong>Lewis Structure:<\/strong> Chlorine is the central atom bonded to three fluorine atoms, with two lone pairs on chlorine.- <strong>Molecular Geometry:<\/strong> T-shaped, with bond angles of approximately 90\u00b0 and 180\u00b0.<br><strong>5. NH\u2084\u207a (Ammonium Ion):<\/strong><\/li>\n\n\n\n<li><strong>Valence Electrons:<\/strong> Nitrogen (N) contributes 5 valence electrons, and each hydrogen contributes 1, totaling 8 valence electrons. The positive charge indicates the loss of one electron, so 7 valence electrons are considered.- <strong>Lewis Structure:<\/strong> Nitrogen is the central atom bonded to four hydrogen atoms, with no lone pairs on nitrogen.- <strong>Molecular Geometry:<\/strong> Tetrahedral, with bond angles of approximately 109.5\u00b0.<br><strong>6. XeF\u2084 (Xenon Tetrafluoride):<\/strong><\/li>\n\n\n\n<li><strong>Valence Electrons:<\/strong> Xenon (Xe) contributes 8 valence electrons, and each fluorine contributes 7, totaling 36 valence electrons.- <strong>Lewis Structure:<\/strong> Xenon is the central atom bonded to four fluorine atoms, with two lone pairs on xenon.- <strong>Molecular Geometry:<\/strong> Square planar, with bond angles of 90\u00b0 and 180\u00b0.<br><strong>7. CO\u2082 (Carbon Dioxide):<\/strong><\/li>\n\n\n\n<li><strong>Valence Electrons:<\/strong> Carbon (C) contributes 4 valence electrons, and each oxygen contributes 6, totaling 16 valence electrons.- <strong>Lewis Structure:<\/strong> Carbon is double-bonded to two oxygen atoms, with no lone pairs on carbon and two lone pairs on each oxygen.- <strong>Molecular Geometry:<\/strong> Linear, with a bond angle of 180\u00b0.<br><strong>8. NO (Nitric Oxide):<\/strong><\/li>\n\n\n\n<li><strong>Valence Electrons:<\/strong> Nitrogen (N) contributes 5 valence electrons, and oxygen (O) contributes 6, totaling 11 valence electrons.- <strong>Lewis Structure:<\/strong> Nitrogen is double-bonded to oxygen, with one lone pair on nitrogen and one lone pair on oxygen.- <strong>Molecular Geometry:<\/strong> Linear, with a bond angle of 180\u00b0.<br><strong>9. H\u2082CO (Formaldehyde):<\/strong><\/li>\n\n\n\n<li><strong>Valence Electrons:<\/strong> Carbon (C) contributes 4 valence electrons, oxygen (O) contributes 6, and each hydrogen contributes 1, totaling 12 valence electrons.- <strong>Lewis Structure:<\/strong> Carbon is double-bonded to oxygen and single-bonded to two hydrogen atoms.- <strong>Molecular Geometry:<\/strong> Trigonal planar, with bond angles of approximately 120\u00b0.<br><strong>Explanation:<\/strong><\/li>\n<\/ul>\n\n\n\n<p>The molecular geometry of a compound is determined by the Valence Shell Electron Pair Repulsion (VSEPR) theory, which posits that electron pairs around a central atom arrange themselves to minimize repulsion. This theory helps predict the three-dimensional shapes of molecules based on the number of bonding and non-bonding electron pairs.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Tetrahedral Geometry:<\/strong> ccurs when a central atom is bonded to four atoms with no lone pairs, as seen in SiH\u2084 and NH\u2084\u207a.- <strong>Bent Geometry:<\/strong> esults from two bonding pairs and one or two lone pairs on the central atom, leading to a non-linear shape, as observed in H\u2082O and SO\u2082.- <strong>T-shaped Geometry:<\/strong> rises when there are three bonding pairs and two lone pairs on the central atom, as in ClF\u2083.- <strong>Square Planar Geometry:<\/strong> ccurs when there are four bonding pairs and two lone pairs on the central atom, as in XeF\u2084.- <strong>Linear Geometry:<\/strong> ound in molecules with two bonding pairs and no lone pairs on the central atom, such as CO\u2082 and NO.- <strong>Trigonal Planar Geometry:<\/strong> esults from three bonding pairs and no lone pairs on the central atom, as in H\u2082CO.<br>Understanding these geometries is crucial for predicting the physical and chemical properties of molecules, including polarity, reactivity, and interaction with other substances.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Molecular Formula Total Number of Valence Electrons Lewis Structure Molecular Geometry SiH4 H20 SO2 CIFs Molecular Formula Total Number of Valence Electrons Lewis Structure Molecular Geometry NH4 XeF4 CO2 NO: H2CO The Correct Answer and Explanation is : Let&#8217;s analyze the molecular formulas, total number of valence electrons, Lewis structures, and molecular geometries for the [&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 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