{"id":307,"date":"2024-04-01T14:13:10","date_gmt":"2024-04-01T13:13:10","guid":{"rendered":"https:\/\/tutors4you.com\/?page_id=307"},"modified":"2024-04-01T14:13:11","modified_gmt":"2024-04-01T13:13:11","slug":"chemical-bonding-and-molecular-structure","status":"publish","type":"page","link":"https:\/\/tutors4you.com\/index.php\/chemical-bonding-and-molecular-structure\/","title":{"rendered":"Chemical Bonding and Molecular Structure"},"content":{"rendered":"\n\n\t\t<div class=\"well well-sm\">\n\t\t\t\n\t\t\t<p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><b><u>Chemical\n        Bond:<\/u><\/b> <\/font><font color=\"#004080\" face=\"Arial\">It\n        is the force which keeps atoms together in a molecule.\n        The causes of formation of a chemical bond are:<\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Tendency of atoms to complete their\n                octets or duplets by rearrangement of their\n                valence electrons (octed theory).<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">The system acquires minimum energy\n                when atoms are at some equilibrium distance where\n                attractive forces dominate over repulsive forces.<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Types\n        of Chemical Bonds:<\/u><\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Ionic bond<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Covalent bond<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Metallic bond<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Co-ordinate bond<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Ionic\n        Bond:<\/u><\/strong><\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>a)\n        <\/strong><strong><u>Favourable conditions to form Ionic\n        Bond:<\/u><\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Formed between electro positive\n                element (group 1,2,13) and electro negative\n                element (group 15,16,17)<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\"><img loading=\"lazy\" decoding=\"async\" src=\"\/wp-content\/uploads\/2024\/03\/delta.jpg\" width=\"16\"\n                height=\"17\"> E.N &gt;=2<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Lower I.E of one atom and high E.A\n                of second atom<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Higher lattice energy<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Larger cations, smaller anions<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>b)\n        <\/strong><strong><u>Properties:<\/u><\/strong><strong> <\/strong>Crystaline,\n        stronger force of attraction, thermally stable, low\n        volatality, high density, high melting point and boiling\n        point, highly soluble in polar solvent, good conductor of\n        electricity in molten or solution state, nondirectional\n        bond.<\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Covalent\n        Bond:<\/u><\/strong><\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>a)\n        <\/strong><strong><u>Favourable conditions to form\n        Covalent Bond:<\/u><\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Formed between two electronegative\n                elements (group 14,15,16,17)<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\"><img loading=\"lazy\" decoding=\"async\" src=\"\/wp-content\/uploads\/2024\/03\/delta.jpg\" width=\"16\"\n                height=\"17\">E.N &lt; 1.9<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Small cations, larger anions\n                (Fajan&#8217;s Rule)<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">High charges on cation and anion\n                (Fajan&#8217;s Rule)<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Covalent bond is formed by sharing\n                of electrons by two atoms to complete their octet\n                or duplet<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>b)\n        <\/strong><strong><u>Properties:<\/u><\/strong> <\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Compounds containing covalent bonds\n                under normal condition of pressure and\n                temperature exist as gases or liquids of low\n                boiling point due to weak Vander Wall&#8217;s force<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Relatively low melting point and\n                boiling point, generally non-conductor, and\n                soluble in non-polar solvent<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">As the bond is rigid and\n                directional, compounds with covalent bond show\n                isomerism<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Covalency of the atom is equal to\n                the number of covalent bonds formed by the atom<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Bond\n        Length:<\/u><\/strong><\/font><font color=\"#004080\"\n        face=\"Arial\"> It is the average distance between the\n        nuclei of two bonded atoms. It depends upon:<\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Size of the atom: Bond length\n                increases with increase in the size of atom (HI\n                &gt; HBr &gt; HCl &gt; HF)<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Multiplicity of bond: Bond length\n                decreases with multiplicity of bond (C-C &gt; C=C\n                )<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Type of hybridisation: More\n                s-character, shorter is the bond length, greater\n                is the acidity with comparable compound<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Bond\n        Energy:<\/u><\/strong> <\/font><font color=\"#004080\"\n        face=\"Arial\">It is the energy required to break one mole\n        of bonds of a particular type of substance in gaseous\n        state. <\/font><\/p>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Bond\n        Angle:<\/u><\/strong><\/font><font color=\"#004080\"\n        face=\"Arial\"> It is the internal angle between the\n        orbitals containing electron pairs in the valence shell\n        of the central atom in a molecule:<\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">More the lone pairs on the central\n                atom, smaller is the bond angle due to bp\n                repulsion<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">More electronegative the central\n                atom, more is the bond angle<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">More electronegative the surrounding\n                atoms, lesser is the bond angle<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Valence Bond Theory (VBT):<\/u><\/strong><\/font><font\n        color=\"#004080\" face=\"Arial\"> Proposed by Heitler and\n        London and extended by Pauling and State. The postulates\n        are:<\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Overlapping of atomic orbitals of\n                valence shells of two atoms leads to the\n                formation of a covalent bond<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Half filled orbital and opposite\n                spin electrons are used<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><img loading=\"lazy\" decoding=\"async\" src=\"\/wp-content\/uploads\/2024\/03\/symbolsigma.jpg\"\n                width=\"12\" height=\"13\">&#8211;<font face=\"Arial\"> <\/font><font\n                color=\"#004080\" face=\"Arial\">bond is formed by\n                head on overlapping, <img loading=\"lazy\" decoding=\"async\" src=\"\/wp-content\/uploads\/2024\/03\/symbolpie.jpg\"\n                width=\"9\" height=\"10\"> &#8211; bond is formed by\n                lateral overlapping<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Greater the overlapping, stronger is\n                the bond<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><img loading=\"lazy\" decoding=\"async\" src=\"\/wp-content\/uploads\/2024\/03\/symbolsigma.jpg\"\n                width=\"12\" height=\"13\">&#8211;<font face=\"Arial\"> <\/font><font\n                color=\"#004080\" face=\"Arial\">bond is stronger\n                than <img loading=\"lazy\" decoding=\"async\" src=\"\/wp-content\/uploads\/2024\/03\/symbolpie.jpg\" width=\"9\"\n                height=\"10\"> &#8211; bond and <\/font><img loading=\"lazy\" decoding=\"async\"\n                src=\"\/wp-content\/uploads\/2024\/03\/symbolsigma.jpg\" width=\"12\" height=\"13\">&#8211;<font\n                face=\"Arial\"> <\/font><font color=\"#004080\"\n                face=\"Arial\">bond is directional while <img loading=\"lazy\" decoding=\"async\"\n                src=\"\/wp-content\/uploads\/2024\/03\/symbolpie.jpg\" width=\"9\" height=\"10\"> &#8211; bond\n                is non-directional<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">The directon of the bond is the same\n                as the direction of overlapping of orbitals<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">The strength of <\/font><img loading=\"lazy\" decoding=\"async\"\n                src=\"\/wp-content\/uploads\/2024\/03\/symbolsigma.jpg\" width=\"12\" height=\"13\">&#8211;<font\n                face=\"Arial\"> <\/font><font color=\"#004080\"\n                face=\"Arial\">bond follows the order s -s &lt; s &#8211;\n                p &lt; p &#8211; p<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Paired electrons are shifted to\n                higher energy levels while forming a bond<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">VBT cannot explain paramagnetic\n                behaviour of O<sub>2<\/sub> <\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Hybridization:<\/u><\/strong>\n        <\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Number of hybrid orbitals = number\n                of atomic orbitals intermixed<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Hybrid orbitals form <\/font><img loading=\"lazy\" decoding=\"async\"\n                src=\"\/wp-content\/uploads\/2024\/03\/symbolsigma.jpg\" width=\"12\" height=\"13\"><font\n                color=\"#004080\" face=\"Arial\">-bond on overlapping<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">It does not take place in and\n                isolated atom. It occurs only during bond\n                formation<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Hybrid orbitals tend to remain far\n                apart therefore repulsion order is\n                lp-lp&gt;lp-bp&gt;bp-bp<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Total number of hybrid orbitals of\n                central atom = Number of its <\/font><img loading=\"lazy\" decoding=\"async\"\n                src=\"\/wp-content\/uploads\/2024\/03\/symbolsigma.jpg\" width=\"12\" height=\"13\">&#8211;<font\n                face=\"Arial\"> <\/font><font color=\"#004080\"\n                face=\"Arial\">bond pairs + Number of lone pair of\n                electrons around the central atom<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Different types of hybridization are\n                sp, sp<sup>2<\/sup> , sp<sup>3<\/sup> , sp<sup>3<\/sup>d\n                ,sp<sup>3<\/sup> d<sup>2<\/sup> ,sp<sup>3<\/sup> d<sup>3<\/sup><\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Molecular Orbital Theory (MOT):<\/u><\/strong><\/font><font\n        color=\"#004080\" face=\"Arial\"> The theory was developed by\n        Hund &amp; Mulliken. The basic postulates are:<\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">All atomic orbitals are mixed up to\n                form molecular orbitals<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Total M.O = Total A.O<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Two A.O. combine to form tow M.Os.\n                One is anti bonding M.O. and the other is bonding\n                M.O.<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">The filling up of electrons must\n                follow Aufbau&#8217;s principle., Pauli exclusion\n                principle and Hund&#8217;s rule.<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Bond order = (N<sub>b<\/sub> &#8211; N<sub>a<\/sub>\n                )\/2 where N<sub>b<\/sub> = Number of electrons in\n                bonding M.O and N<sub>b<\/sub> = Number of\n                electrons in antibonding M.O<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Bond order <img loading=\"lazy\" decoding=\"async\" src=\"\/wp-content\/uploads\/2024\/03\/sybolalpha.jpg\"\n                width=\"12\" height=\"13\"> Bond energy <img loading=\"lazy\" decoding=\"async\"\n                src=\"\/wp-content\/uploads\/2024\/03\/sybolalpha.jpg\" width=\"12\" height=\"13\">\n                1\/Bond length<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Dipole\n        Moment<\/u><\/strong><strong>:<\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Common in covalent compounds when\n                formed between two dissimilar atoms<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Used to predict the extent of\n                polarity in a molecule<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">A vector quantity so follows vector\n                addition or subtraction rule in predicting net\n                dipole moment of a molecule<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Can predict the shape of molecules,\n                H<sub>2<\/sub> O &#8211; bent, BeF<sub>2<\/sub> &#8211; linear<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Metallic\n        Bond:<\/u><\/strong><\/font><font color=\"#004080\"\n        face=\"Arial\"> <\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>a)\n        <\/strong><strong><u>Favourable conditions to form\n        Metallic Bond:<\/u><\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Formed between Electro positive ions\n                packed in one of the 3 arrangements (1.CCP(or\n                FCC), 2.HCP, 3 BCC)<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>b)\n        <\/strong><strong><u>Properties:<\/u><\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Negatively charged electrons hold\n                the ion together<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Highly conducting becauls the\n                mobility of these electrons through the lattice<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">High m.p and b.p<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">If soluble, then soluble only in\n                polar solvents of high dielectric constant<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Co-ordinate\n        Bond:<\/u><\/strong><\/font><font color=\"#004080\"\n        face=\"Arial\"> <\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>a)\n        <\/strong><strong><u>Favourable conditions to form\n        Metallic Bond:<\/u><\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">One of the group or or atom must\n                have a lone pair of electrons whereas the other\n                must have the incomplete octet or duplet.<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Also known as dative bond<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>b)\n        <\/strong><strong><u>Properties:<\/u><\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Intermediate between ionic and\n                covalent compounds<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Sparingly soluble in water, not\n                forming ions, largely soluble in non-polar\n                solvents<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Melting and boiling points are\n                higher than purely covalent compounds but less\n                than purely ionic compounds<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Stable as covalent compounds,\n                addition compounds are very stable<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Non conductor<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Bond is rigid and directional<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">High value of dielectric constant<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#FF0000\" face=\"Arial\"><strong><u>Other\n        Bonds:<\/u><\/strong><\/font><\/p>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>a)\n        H-bonding: <\/strong>When H is attached to N, O, F<\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">It&#8217;s strength is about one tenth of\n                a covalent bond<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Small size and high\n                electronegativity of atoms forms a strong H-bond<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">They are of twor types;\n                intermolecular (between two molecules) and\n                intramolecular (within a molecule)<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Used to predict boiling point and\n                density of water, solubility of alcohols and\n                carboxylic acids in water.<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>b)\n        Dipole-dipole interactions:<\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">These exist between molecules having\n                permanent dipoles e.g. H-Cl, I-F etc<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>c)\n        Ion-dipole interactions:<\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Between and ion and a polar molecule\n                eg hydration of ions like Na<sup>+<\/sup> , Mg<sup>2+<\/sup>\n                etc<\/font><\/p>\n            <\/li>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Smaller the ion, more the dipole\n                moment, stronger will be these interactions<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>d)\n        Ion-induced dipole interactions:<\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Between an Ion and a dipole induced\n                by the ion in a nonpolar molecule<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>e)\n        Dipole-induced dipole interactions:<\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Between a dipole and and induced\n                dipole in a non polar molecule<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>f)\n        Dispersion forces:<\/strong><\/font><\/p>\n        <ul>\n            <li><p align=\"left\"><font color=\"#004080\"\n                face=\"Arial\">Between two nonpolar substances. The\n                forces are between an instantaneous dipole and\n                and induced dipole eg in O<sub>2<\/sub> , N<sub>2<\/sub>\n                , He, Ne, Ar etc<\/font><\/p>\n            <\/li>\n        <\/ul>\n        <p align=\"left\"><font color=\"#004080\" face=\"Arial\"><strong>Note:<\/strong>\n        Dipole-dipole, dipole-induced dipole and dispersion\n        forces are called Van der Wall&#8217;s forces<\/font><\/p>\n\t\t<\/div>\n\t\n","protected":false},"excerpt":{"rendered":"<p>Chemical Bond: It is the force which keeps atoms together in a molecule. The causes of formation of a chemical bond are: Tendency of atoms to complete their octets or duplets by rearrangement of their valence electrons (octed theory). The system acquires minimum energy when atoms are at some equilibrium distance where attractive forces dominate [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-307","page","type-page","status-publish","hentry"],"blocksy_meta":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v25.9 - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Chemical Bonding and Molecular Structure - Tutors 4 You<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/tutors4you.com\/index.php\/chemical-bonding-and-molecular-structure\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Chemical Bonding and Molecular Structure - Tutors 4 You\" \/>\n<meta property=\"og:description\" content=\"Chemical Bond: It is the force which keeps atoms together in a molecule. The causes of formation of a chemical bond are: Tendency of atoms to complete their octets or duplets by rearrangement of their valence electrons (octed theory). 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The causes of formation of a chemical bond are: Tendency of atoms to complete their octets or duplets by rearrangement of their valence electrons (octed theory). 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