{"id":188761,"date":"2025-02-07T09:17:03","date_gmt":"2025-02-07T09:17:03","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=188761"},"modified":"2025-02-07T09:17:05","modified_gmt":"2025-02-07T09:17:05","slug":"hydrogen-cyanide-hcn","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/07\/hydrogen-cyanide-hcn\/","title":{"rendered":"Hydrogen Cyanide &#8211; HCN"},"content":{"rendered":"\n<p>Hydrogen Cyanide &#8211; HCN (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Anspver Observed Shape (Molecular Shape): Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer Molecular Model Carbon Disulfide &#8211; CS2 (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Anshver Observed Shape (Molecular Shape) Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer 27 Molecular Model Formaldehyde &#8211; H2CO (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape) Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer Molecular Model Tetrafluoromethane &#8211; CF4(2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule) Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape) Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer Molecular Model Nitrogen Trifluoride &#8211; NF, (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape) Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer Molecular Model Nitrogen Trichloride &#8211; NCIS (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule). Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape)! Answer Bond Anglet Answer Bond Polarity: Answer Molecular Polarity Answer Molecular Model Water &#8211; H20 (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer # of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Answer Observed Shape (Molecular Shape): Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer um Molecular Model DU . Hydrogen Sulfide &#8211; H2S (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule) Answer Central Atom: Answer of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets Answer Observed Shape (Molecular Shape) Answer Bond Anglet Answer Bond Polarity: Answer Molecular Polarity Answer ad Orang!<\/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 go through each molecule step by step:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">1. <strong>Hydrogen Cyanide (HCN)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total Number of Valence Electrons<\/strong>: H (1) + C (4) + N (5) = 10 electrons.<\/li>\n\n\n\n<li><strong>Central Atom<\/strong>: Carbon (C).<\/li>\n\n\n\n<li><strong># of Electron Sets<\/strong>: 3 electron sets (2 bonding pairs, 1 lone pair on nitrogen).<\/li>\n\n\n\n<li><strong>Geometry of Electron Sets<\/strong>: Linear.<\/li>\n\n\n\n<li><strong>Bonding Electron Sets<\/strong>: 2 bonding pairs (C-H, C\u2261N).<\/li>\n\n\n\n<li><strong>Non-bonding Electron Sets<\/strong>: 1 lone pair on nitrogen (N).<\/li>\n\n\n\n<li><strong>Observed Shape (Molecular Shape)<\/strong>: Linear.<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 180\u00b0.<\/li>\n\n\n\n<li><strong>Bond Polarity<\/strong>: C-H is nonpolar, C\u2261N is polar.<\/li>\n\n\n\n<li><strong>Molecular Polarity<\/strong>: Polar due to the asymmetrical distribution of electrons from the C\u2261N bond.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">2. <strong>Carbon Disulfide (CS2)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total Number of Valence Electrons<\/strong>: C (4) + S (6 * 2) = 16 electrons.<\/li>\n\n\n\n<li><strong>Central Atom<\/strong>: Carbon (C).<\/li>\n\n\n\n<li><strong># of Electron Sets<\/strong>: 2 bonding sets (S=C=S).<\/li>\n\n\n\n<li><strong>Geometry of Electron Sets<\/strong>: Linear.<\/li>\n\n\n\n<li><strong>Bonding Electron Sets<\/strong>: 2 bonding pairs (S=C=S).<\/li>\n\n\n\n<li><strong>Non-bonding Electron Sets<\/strong>: No lone pairs.<\/li>\n\n\n\n<li><strong>Observed Shape (Molecular Shape)<\/strong>: Linear.<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 180\u00b0.<\/li>\n\n\n\n<li><strong>Bond Polarity<\/strong>: C=S bonds are polar.<\/li>\n\n\n\n<li><strong>Molecular Polarity<\/strong>: Nonpolar, because the linear shape results in the dipoles cancelling out.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">3. <strong>Formaldehyde (H2CO)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total Number of Valence Electrons<\/strong>: H (1 * 2) + C (4) + O (6) = 12 electrons.<\/li>\n\n\n\n<li><strong>Central Atom<\/strong>: Carbon (C).<\/li>\n\n\n\n<li><strong># of Electron Sets<\/strong>: 3 bonding sets (H-C=O).<\/li>\n\n\n\n<li><strong>Geometry of Electron Sets<\/strong>: Trigonal Planar.<\/li>\n\n\n\n<li><strong>Bonding Electron Sets<\/strong>: 3 bonding pairs (C-H, C=O).<\/li>\n\n\n\n<li><strong>Non-bonding Electron Sets<\/strong>: No lone pairs.<\/li>\n\n\n\n<li><strong>Observed Shape (Molecular Shape)<\/strong>: Trigonal Planar.<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 120\u00b0.<\/li>\n\n\n\n<li><strong>Bond Polarity<\/strong>: C=O is polar, C-H is nonpolar.<\/li>\n\n\n\n<li><strong>Molecular Polarity<\/strong>: Polar because of the asymmetry of the C=O bond.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">4. <strong>Tetrafluoromethane (CF4)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total Number of Valence Electrons<\/strong>: C (4) + F (7 * 4) = 32 electrons.<\/li>\n\n\n\n<li><strong>Central Atom<\/strong>: Carbon (C).<\/li>\n\n\n\n<li><strong># of Electron Sets<\/strong>: 4 bonding sets (F-C-F-F).<\/li>\n\n\n\n<li><strong>Geometry of Electron Sets<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Bonding Electron Sets<\/strong>: 4 bonding pairs (C-F).<\/li>\n\n\n\n<li><strong>Non-bonding Electron Sets<\/strong>: No lone pairs.<\/li>\n\n\n\n<li><strong>Observed Shape (Molecular Shape)<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 109.5\u00b0.<\/li>\n\n\n\n<li><strong>Bond Polarity<\/strong>: C-F bonds are polar.<\/li>\n\n\n\n<li><strong>Molecular Polarity<\/strong>: Nonpolar because the symmetry of the tetrahedral shape cancels out the dipoles.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">5. <strong>Nitrogen Trifluoride (NF3)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total Number of Valence Electrons<\/strong>: N (5) + F (7 * 3) = 26 electrons.<\/li>\n\n\n\n<li><strong>Central Atom<\/strong>: Nitrogen (N).<\/li>\n\n\n\n<li><strong># of Electron Sets<\/strong>: 4 electron sets (3 bonding, 1 lone pair).<\/li>\n\n\n\n<li><strong>Geometry of Electron Sets<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Bonding Electron Sets<\/strong>: 3 bonding pairs (N-F).<\/li>\n\n\n\n<li><strong>Non-bonding Electron Sets<\/strong>: 1 lone pair on nitrogen.<\/li>\n\n\n\n<li><strong>Observed Shape (Molecular Shape)<\/strong>: Trigonal Pyramidal.<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 107\u00b0.<\/li>\n\n\n\n<li><strong>Bond Polarity<\/strong>: N-F bonds are polar.<\/li>\n\n\n\n<li><strong>Molecular Polarity<\/strong>: Polar due to the asymmetry caused by the lone pair.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">6. <strong>Nitrogen Trichloride (NCl3)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total Number of Valence Electrons<\/strong>: N (5) + Cl (7 * 3) = 26 electrons.<\/li>\n\n\n\n<li><strong>Central Atom<\/strong>: Nitrogen (N).<\/li>\n\n\n\n<li><strong># of Electron Sets<\/strong>: 4 electron sets (3 bonding, 1 lone pair).<\/li>\n\n\n\n<li><strong>Geometry of Electron Sets<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Bonding Electron Sets<\/strong>: 3 bonding pairs (N-Cl).<\/li>\n\n\n\n<li><strong>Non-bonding Electron Sets<\/strong>: 1 lone pair on nitrogen.<\/li>\n\n\n\n<li><strong>Observed Shape (Molecular Shape)<\/strong>: Trigonal Pyramidal.<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 107\u00b0.<\/li>\n\n\n\n<li><strong>Bond Polarity<\/strong>: N-Cl bonds are polar.<\/li>\n\n\n\n<li><strong>Molecular Polarity<\/strong>: Polar due to the lone pair and polar bonds.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">7. <strong>Water (H2O)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total Number of Valence Electrons<\/strong>: H (1 * 2) + O (6) = 8 electrons.<\/li>\n\n\n\n<li><strong>Central Atom<\/strong>: Oxygen (O).<\/li>\n\n\n\n<li><strong># of Electron Sets<\/strong>: 4 electron sets (2 bonding, 2 lone pairs).<\/li>\n\n\n\n<li><strong>Geometry of Electron Sets<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Bonding Electron Sets<\/strong>: 2 bonding pairs (O-H).<\/li>\n\n\n\n<li><strong>Non-bonding Electron Sets<\/strong>: 2 lone pairs on oxygen.<\/li>\n\n\n\n<li><strong>Observed Shape (Molecular Shape)<\/strong>: Bent.<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 104.5\u00b0.<\/li>\n\n\n\n<li><strong>Bond Polarity<\/strong>: O-H bonds are polar.<\/li>\n\n\n\n<li><strong>Molecular Polarity<\/strong>: Polar because of the bent shape and the polar bonds.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">8. <strong>Hydrogen Sulfide (H2S)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total Number of Valence Electrons<\/strong>: H (1 * 2) + S (6) = 8 electrons.<\/li>\n\n\n\n<li><strong>Central Atom<\/strong>: Sulfur (S).<\/li>\n\n\n\n<li><strong># of Electron Sets<\/strong>: 4 electron sets (2 bonding, 2 lone pairs).<\/li>\n\n\n\n<li><strong>Geometry of Electron Sets<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Bonding Electron Sets<\/strong>: 2 bonding pairs (S-H).<\/li>\n\n\n\n<li><strong>Non-bonding Electron Sets<\/strong>: 2 lone pairs on sulfur.<\/li>\n\n\n\n<li><strong>Observed Shape (Molecular Shape)<\/strong>: Bent.<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 92.1\u00b0.<\/li>\n\n\n\n<li><strong>Bond Polarity<\/strong>: S-H bonds are polar.<\/li>\n\n\n\n<li><strong>Molecular Polarity<\/strong>: Polar due to the bent shape and the polar bonds.<\/li>\n<\/ul>\n\n\n\n<p>Each molecule&#8217;s Lewis structure and properties depend on electron sharing and the shape that minimizes repulsion between electron pairs (VSEPR theory).<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Hydrogen Cyanide &#8211; HCN (2 points) Lewis Structure Diagram Required Information Total Number of Valence Electrons (Molecule): Answer Central Atom: Answer of Electron Sets: Answer Geometry of Electron Sets: Answer Bonding Electron Sets: Answer Non-bonding Electron Sets: Anspver Observed Shape (Molecular Shape): Answer Bond Angle: Answer Bond Polarity: Answer Molecular Polarity: Answer Molecular Model Carbon [&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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