{"id":1092,"date":"2025-05-13T13:31:36","date_gmt":"2025-05-13T08:01:36","guid":{"rendered":"https:\/\/www.chemtopper.com\/myblog\/?page_id=1092"},"modified":"2025-07-18T20:24:49","modified_gmt":"2025-07-18T14:54:49","slug":"coulombs-law-ionic-attractions-enthalpy-energy-trends","status":"publish","type":"page","link":"https:\/\/www.chemtopper.com\/myblog\/coulombs-law-ionic-attractions-enthalpy-energy-trends\/","title":{"rendered":"Coulomb\u2019s Law and Periodic trends."},"content":{"rendered":"<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large\"><a href=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/COULOMBS-LAW-1.png\"><img loading=\"lazy\" decoding=\"async\" width=\"819\" height=\"1024\" src=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/COULOMBS-LAW-1-819x1024.png\" alt=\"\" class=\"wp-image-1266\" srcset=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/COULOMBS-LAW-1-819x1024.png 819w, https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/COULOMBS-LAW-1-240x300.png 240w, https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/COULOMBS-LAW-1-768x960.png 768w, https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/COULOMBS-LAW-1.png 1080w\" sizes=\"auto, (max-width: 819px) 100vw, 819px\" \/><\/a><\/figure>\n<\/div>\n\n\n<p><\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><strong>Coulomb\u2019s Law and Periodic trends- Force of attraction between oppositely charged particles<\/strong><\/h2>\n\n\n\n<h4 class=\"wp-block-heading\"><\/h4>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full is-resized\"><a href=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/image.gif\"><img loading=\"lazy\" decoding=\"async\" width=\"89\" height=\"28\" src=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/image.gif\" alt=\"\" class=\"wp-image-1276\" style=\"width:292px;height:auto\"\/><\/a><\/figure>\n<\/div>\n\n\n<p><strong>Coulomb\u2019s law<\/strong> can be used for qualitative comparison of attractions among the charged particles in molecules, ions and within the atom etc. Here <strong>q<sub>1 <\/sub>and q<sub>2<\/sub><\/strong> are the charges on the particles and &nbsp;&nbsp;&nbsp;<strong>r <\/strong>is the distance of separation between the charged particles.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Qualitative meaning of Coulomb\u2019s Law and Periodic trends.<\/h2>\n\n\n\n<ol class=\"wp-block-list\">\n<li>The <strong>electrostatic force of attraction<\/strong> is <strong>directly proportional to the product of the charges<\/strong> on the interacting particles. This means that <strong>the greater the magnitude of the charges<\/strong>, the <strong>stronger the force of attraction<\/strong> between them.\n<ul class=\"wp-block-list\">\n<li><strong>Examples:<\/strong> <strong>NaCl vs MgO:<\/strong><\/li>\n\n\n\n<li><strong>Na\u207a and Cl\u207b<\/strong>: Charges = +1 and \u20131 \u2192 Product = 1<\/li>\n\n\n\n<li><strong>Mg\u00b2\u207a and O\u00b2\u207b<\/strong>: Charges = +2 and \u20132 \u2192 Product = 4<br>\u2192 MgO has <strong>4 times stronger attraction<\/strong> than NaCl (assuming equal distance), leading to <strong>higher lattice enthalpy<\/strong> and <strong>higher melting point<\/strong>.<\/li>\n\n\n\n<li><strong>Ionization Energy <\/strong>Trends: In atoms with a <strong>+2 nucleus (He)<\/strong> vs <strong>+1 nucleus (H)<\/strong>, the attraction to electrons is stronger in He, making it harder to remove an electron despite nearly similar size.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>The <strong>electrostatic force of attraction<\/strong> between charged particles is <strong>inversely proportional to the square of the distance<\/strong> between them. This means that as the distance between the particles increases, the force of attraction decreases rapidly. Therefore, <strong>more energy is required to separate charges that are closer together<\/strong>, because the attractive force between them is stronger.<\/li>\n<\/ol>\n\n\n\n<p><strong>Examples:<\/strong><\/p>\n\n\n\n<p>As the <strong>shell number increases<\/strong>, the <strong>distance of the orbitals (and electrons) from the nucleus<\/strong> also increases. As a result, the <strong>electrostatic attraction between the nucleus and the electron decreases<\/strong>, leading to an <strong>increase in the energy of the electron<\/strong> in higher shells.<br>Electrons in the <strong>first energy level (closer to the nucleus)<\/strong> experience a much stronger attraction to the positively charged nucleus than electrons in outer shells. As a result, <strong>more ionization energy is needed<\/strong> to remove an electron from the first shell than from higher shells.<\/p>\n\n\n\n<p><\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><strong>Electrons in different shells of an atom:<\/strong><\/h2>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><a href=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/Distance-of-the-orbitals-from-the-nucleus.jpg\"><img loading=\"lazy\" decoding=\"async\" width=\"418\" height=\"246\" src=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/Distance-of-the-orbitals-from-the-nucleus.jpg\" alt=\"\" class=\"wp-image-1268\" srcset=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/Distance-of-the-orbitals-from-the-nucleus.jpg 418w, https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/Distance-of-the-orbitals-from-the-nucleus-300x177.jpg 300w\" sizes=\"auto, (max-width: 418px) 100vw, 418px\" \/><\/a><\/figure>\n<\/div>\n\n\n<ul class=\"wp-block-list\">\n<li>In <strong>ionic solids<\/strong> like <strong>NaCl<\/strong>, the positive (Na\u207a) and negative (Cl\u207b) ions are held together by electrostatic forces of attraction in a closely packed lattice. In compounds like <strong>MgO<\/strong>, the ions\u2014Mg\u00b2\u207a and O\u00b2\u207b\u2014carry <strong>higher charges<\/strong> and are <strong>smaller in size<\/strong>, resulting in <strong>even stronger electrostatic attraction<\/strong> and a <strong>more tightly packed lattice<\/strong> compared to NaCl. This leads to a <strong>much higher lattice enthalpy<\/strong> in MgO, making it more thermally stable and requiring significantly more energy to separate the ions.\n<ul class=\"wp-block-list\">\n<li>For example:<\/li>\n\n\n\n<li><strong>MgO<\/strong> has a <strong>much higher melting point<\/strong> (~2852\u202f\u00b0C) than <strong>NaCl<\/strong> (~801\u202f\u00b0C), which correlates with its <strong>higher lattice enthalpy<\/strong>.<\/li>\n\n\n\n<li>In short, <strong>lattice enthalpy is directly related to melting point<\/strong> in ionic compounds\u2014<strong>Higher charges and smaller size =stronger attractions = higher lattice energy = higher m.p.t.<\/strong><br><\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><strong>Mantra in chemistry-Force of attraction \u221e Energy<\/strong><\/h2>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large\"><a href=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/image.png\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"105\" src=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/image-1024x105.png\" alt=\"\" class=\"wp-image-1269\" srcset=\"https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/image-1024x105.png 1024w, https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/image-300x31.png 300w, https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/image-768x79.png 768w, https:\/\/www.chemtopper.com\/myblog\/wp-content\/uploads\/2025\/05\/image.png 1147w\" sizes=\"auto, (max-width: 1024px) 100vw, 1024px\" \/><\/a><\/figure>\n<\/div>\n\n\n<p>Explanation of the Flow:<\/p>\n\n\n\n<ol start=\"1\" class=\"wp-block-list\">\n<li><strong>More force of attraction<\/strong><br>\u2192 Typically due to higher effective nuclear charge or smaller atomic size.<\/li>\n\n\n\n<li>&nbsp;<strong>Exothermic process<\/strong><br>\u2192 When electrons are added or bonds are formed, energy is released.<\/li>\n\n\n\n<li>&nbsp;<strong>Less energy (more negative energy)<\/strong><br>\u2192 Indicates a more stable state (like in electron affinity or bond formation).<\/li>\n\n\n\n<li>&nbsp;<strong>More stability<\/strong><br>\u2192 Atoms reach low-energy configurations, like noble gases.<\/li>\n\n\n\n<li><strong>&nbsp;Less reactivity<br><\/strong>\u2192 Stable atoms (e.g., noble gases) are less likely to react.<\/li>\n<\/ol>\n\n\n\n<h2 class=\"wp-block-heading\">Coulomb\u2019s Law and Periodic trends-Where This Applies:<\/h2>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron Affinity<\/strong>: More attraction \u2192 more energy released (exothermic) \u2192 more stable anion \u2192 less likely to gain another electron.<\/li>\n\n\n\n<li><strong>Ionization Energy:<\/strong> Opposite\u2014more attraction means more energy is required to remove an electron.<\/li>\n\n\n\n<li><strong>Covalent Bond Formation:<\/strong> Atoms bond to reach lower energy (stability)\u2192 Small atoms means small bonds \u2192 more attraction \u2192stronger bond \u2192more energy needed to break it \u2192High bond energy.<\/li>\n\n\n\n<li><strong>Hydration enthalpy<\/strong> &#8211; more charge and small size means more stronger hydration by water molecules and more negative hydration enthalpy. (Look at the picture in flash card)<\/li>\n\n\n\n<li><strong>Lattice enthalpy and melting points<\/strong>-more charge and small size means more stronger attraction \u2192stronger lattice and higher melting point\u2192 stable compound.<\/li>\n<\/ul>\n\n\n\n<div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-3\" class=\"h5p-iframe\" data-content-id=\"3\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Coulomb&#039;s Law\"><\/iframe><\/div>\n","protected":false},"excerpt":{"rendered":"<p>Coulomb\u2019s Law and Periodic trends- Force of attraction between oppositely charged particles Coulomb\u2019s law can be used for qualitative comparison of attractions among the charged particles in molecules, ions and within the atom etc. Here q1 and q2 are the charges on the particles and &nbsp;&nbsp;&nbsp;r is the distance of separation between the charged particles. &hellip;<\/p>\n<p class=\"read-more\"> <a class=\"\" href=\"https:\/\/www.chemtopper.com\/myblog\/coulombs-law-ionic-attractions-enthalpy-energy-trends\/\"> <span class=\"screen-reader-text\">Coulomb\u2019s Law and Periodic trends.<\/span> Read More &raquo;<\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":"[]"},"categories":[13,44],"class_list":["post-1092","page","type-page","status-publish","hentry","category-ap-chemistry-exam","category-periodic-trends-of-elements"],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v27.5 - https:\/\/yoast.com\/product\/yoast-seo-wordpress\/ -->\n<title>Coulomb\u2019s Law and Periodic trends.<\/title>\n<meta name=\"description\" content=\"Learn &amp; practice how Coulomb\u2019s Law explains periodic trends such as atomic size, ionization energy, and lattice enthalpy.\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, 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