{"id":7317,"date":"2024-12-29T10:59:57","date_gmt":"2024-12-29T10:59:57","guid":{"rendered":"https:\/\/workhouse.sweetdishy.com\/?p=7317"},"modified":"2024-12-29T11:02:27","modified_gmt":"2024-12-29T11:02:27","slug":"bond-characteristics","status":"publish","type":"post","link":"https:\/\/workhouse.sweetdishy.com\/index.php\/2024\/12\/29\/bond-characteristics\/","title":{"rendered":"Bond Characteristics"},"content":{"rendered":"\n<h3 class=\"wp-block-heading\">Bond Length<\/h3>\n\n\n\n<p>During chemical bonding, when the atoms come closer to each other, the attraction takes place between them, and the potential energy of the system keeps on decreasing till a particular distance at which the potential energy is minimum. If the atoms come closer, repulsion starts, and again, the potential energy of the system begins to increase.<\/p>\n\n\n\n<p>At equilibrium distance, the atoms keep on vibrating about their mean position. The equilibrium distance between the centres of the nuclei of the two bonded atoms is called its&nbsp;<strong>bond length.<\/strong><\/p>\n\n\n\n<p>It is expressed in terms of an angstrom (A<sup>0<\/sup>) or picometer (pm). It is determined experimentally by x-ray diffraction or electron diffraction method, or spectroscopic method. The bond length in chemical bonding is the sum of the ionic radii in an ionic compound. In a\u00a0covalent compound, it is the sum of its covalent radii. For a covalent molecule AB, the bond length is given by d = r<sub>a<\/sub>\u00a0+ r<sub>b<\/sub><\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Factors Affecting the Bond Length<\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Size of the atoms:\u00a0<\/strong>The bond length increases with an increase in the size of the atom. HI > HBr > HCl > HF<\/li>\n\n\n\n<li><strong>The multiplicity of bond:\u00a0<\/strong>The bond length decreases with an increase in bond order.<\/li>\n\n\n\n<li><strong>Type of hybridization:\u00a0<\/strong>A\u2018s\u2019 orbital is smaller in size; the greater the \u2018s\u2019 character, the shorter the bond length.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\">Bond Enthalpy<\/h2>\n\n\n\n<p>When atoms come close together, energy is released due to the chemical bonding between them. The amount of energy required to break one mole of bonds of a type so as to separate the molecule into individual gaseous atoms is called&nbsp;<strong>bond dissociation enthalpy or bond enthalpy.<\/strong>&nbsp;Bond enthalpy is usually expressed in KJ mol<sup>-1.<\/sup><\/p>\n\n\n\n<p>The greater the bond dissociation enthalpy, the greater the bond strength. For\u00a0diatomic molecules, like H<sub>2<\/sub>, Cl<sub>2<\/sub>, O<sub>2<\/sub>, N<sub>2<\/sub>, HCl, HBr and HI, the bond enthalpies are equal to their dissociation enthalpy.<\/p>\n\n\n\n<p>In the case of polyatomic molecules, bond enthalpies are usually the average values because the dissociation energy varies with each type of bond.<\/p>\n\n\n\n<p>In H<sub>2<\/sub>0, first O-H bond enthalpy = 502 KJ\/mol; Second bond enthalpy = 427 KJ\/mol Average bond enthalpy = (502 + 427) \/ 2 = 464.5 KJ\/mol<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Factors Affecting Bond Enthalpy in Chemical Bonding<\/h3>\n\n\n\n<h4 class=\"wp-block-heading\">Size of the Atom<\/h4>\n\n\n\n<p>The greater the size of the atom, the greater the bond length, and the less the\u00a0bond dissociation enthalpy, i.e., less the bond strength during chemical bonding.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Multiplicity of Bonds<\/h4>\n\n\n\n<p>The greater the multiplicity of the bond, the greater the bond dissociation enthalpy.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Number of Lone Pair of Electrons Present<\/h4>\n\n\n\n<p>The more the number of lone pairs of electrons present on the bonded atoms, the greater the repulsion between the atoms, and thus, less is the bond dissociation enthalpy of the chemical bond.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Bond Angle<\/h4>\n\n\n\n<p>A bond is formed by the overlap of atomic orbitals. The direction of overlap gives the direction of the bond. The angle between the lines representing the direction of the bond, i.e., the orbitals containing the bonding electrons, is called the<strong>&nbsp;bond angle.<\/strong><\/p>\n\n\n\n<p>Factors Affecting Bond Enthalpy in Chemical Bonding<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Bond Order<\/h4>\n\n\n\n<p>In Lewis representation, the number of bonds present between two atoms is called the&nbsp;<strong>bond order<\/strong>. The greater the bond order, the greater the stability of the bond during chemical bonding, i.e., the greater the bond enthalpy. The greater the bond order, the shorter the bond length.<br><a><\/a><\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Resonance in Chemical Bonding<\/h2>\n\n\n\n<p>There are molecules and ions for which drawing a single Lewis structure is not possible.&nbsp;For example, we can write two structures of O<sub>3<\/sub>.<\/p>\n\n\n\n<p>In (A), the oxygen-oxygen bond on the left is a double bond, and the oxygen-oxygen bond on the right is a single bond. In B, the situation is just the opposite. The experiment shows, however, that the two bonds are identical.<\/p>\n\n\n\n<p>Therefore, neither structure A nor B can be correct. One of the bonding pairs in ozone is spread over the region of all three atoms rather than localised on a particular oxygen-oxygen bond. This delocalised bonding is a type of chemical bonding in which bonding pair of electrons are spread over a number of atoms rather than localised between two.<\/p>\n\n\n\n<p>Structures (A) and (B) are called\u00a0resonating or canonical structures, and (C) is the resonance hybrid. This phenomenon is called resonance, a situation in which more than one canonical structure can be written for a species. The chemical activity of an atom is determined by the number of electrons in its valence shell. With the help of the concept of chemical bonding, one can define the structure of a compound, which is used in many industries for manufacturing products in which the true structure cannot be written at all.<\/p>\n\n\n\n<p>Here are some other examples.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>CO<sub>3<\/sub><sup>2\u2013<\/sup>\u00a0ion<\/li>\n<\/ul>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Vinyl chloride<\/li>\n<\/ul>\n\n\n\n<p>The difference in the energies of the canonical forms and resonance hybrid is called resonance stabilisation energy.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Resonance in Chemical Bonding<\/h2>\n\n\n\n<h3 class=\"wp-block-heading\">London Dispersion Forces<\/h3>\n\n\n\n<p>Another form of chemical bonding is caused by London dispersion forces. These forces are weak in magnitude.<\/p>\n\n\n\n<p>These forces occur due to a temporary charge imbalance arising in an atom. This imbalance in charge of the atom can induce dipoles in neighbouring atoms. For example, the temporary positive charge on one area of an atom can attract the neighbouring negative charge.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Bond Length During chemical bonding, when the atoms come closer to each other, the attraction takes place between them, and the potential energy of the system keeps on decreasing till a particular distance at which the potential energy is minimum. If the atoms come closer, repulsion starts, and again, the potential energy of the system [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":7309,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[761],"tags":[],"class_list":["post-7317","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-chemical-bonding"],"jetpack_featured_media_url":"https:\/\/workhouse.sweetdishy.com\/wp-content\/uploads\/2024\/12\/molecular.png","_links":{"self":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts\/7317","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/comments?post=7317"}],"version-history":[{"count":1,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts\/7317\/revisions"}],"predecessor-version":[{"id":7318,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/posts\/7317\/revisions\/7318"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/media\/7309"}],"wp:attachment":[{"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/media?parent=7317"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/categories?post=7317"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/workhouse.sweetdishy.com\/index.php\/wp-json\/wp\/v2\/tags?post=7317"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}