{"id":1276,"date":"2024-08-12T11:00:25","date_gmt":"2024-08-12T11:00:25","guid":{"rendered":"https:\/\/www.meniit.com\/study-material\/?p=1276"},"modified":"2024-08-17T09:35:22","modified_gmt":"2024-08-17T09:35:22","slug":"modern-periodic-table-laws","status":"publish","type":"post","link":"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/modern-periodic-table-laws","title":{"rendered":"Modern Periodic Table Laws"},"content":{"rendered":"<h2 style=\"text-align: justify;\">Mendeleev\u2019s Periodic Table<\/h2>\n<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_69_1 counter-hierarchy ez-toc-counter ez-toc-light-blue ez-toc-container-direction\">\n<div class=\"ez-toc-title-container\">\n<p class=\"ez-toc-title\" style=\"cursor:inherit\">Table of Contents<\/p>\n<span class=\"ez-toc-title-toggle\"><a href=\"#\" class=\"ez-toc-pull-right ez-toc-btn ez-toc-btn-xs ez-toc-btn-default ez-toc-toggle\" aria-label=\"Toggle Table of Content\"><span class=\"ez-toc-js-icon-con\"><span class=\"\"><span class=\"eztoc-hide\" style=\"display:none;\">Toggle<\/span><span class=\"ez-toc-icon-toggle-span\"><svg style=\"fill: #999;color:#999\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" class=\"list-377408\" width=\"20px\" height=\"20px\" viewBox=\"0 0 24 24\" fill=\"none\"><path d=\"M6 6H4v2h2V6zm14 0H8v2h12V6zM4 11h2v2H4v-2zm16 0H8v2h12v-2zM4 16h2v2H4v-2zm16 0H8v2h12v-2z\" fill=\"currentColor\"><\/path><\/svg><svg style=\"fill: #999;color:#999\" class=\"arrow-unsorted-368013\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" width=\"10px\" height=\"10px\" viewBox=\"0 0 24 24\" version=\"1.2\" baseProfile=\"tiny\"><path d=\"M18.2 9.3l-6.2-6.3-6.2 6.3c-.2.2-.3.4-.3.7s.1.5.3.7c.2.2.4.3.7.3h11c.3 0 .5-.1.7-.3.2-.2.3-.5.3-.7s-.1-.5-.3-.7zM5.8 14.7l6.2 6.3 6.2-6.3c.2-.2.3-.5.3-.7s-.1-.5-.3-.7c-.2-.2-.4-.3-.7-.3h-11c-.3 0-.5.1-.7.3-.2.2-.3.5-.3.7s.1.5.3.7z\"\/><\/svg><\/span><\/span><\/span><\/a><\/span><\/div>\n<nav><ul class='ez-toc-list ez-toc-list-level-1 ' ><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/modern-periodic-table-laws\/#Periodic-Law\" title=\"Periodic Law\">Periodic Law<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-2\" href=\"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/modern-periodic-table-laws\/#Modern-Periodic-Law-And-Modern-Periodic-Table\" title=\"Modern Periodic Law And Modern Periodic Table\">Modern Periodic Law And Modern Periodic Table<\/a><\/li><\/ul><\/nav><\/div>\n<h3 style=\"text-align: justify;\"><span class=\"ez-toc-section\" id=\"Periodic-Law\"><\/span>Periodic Law<span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p style=\"text-align: justify;\"><strong>&#8220;The physical and chemical properties of elements are a\u00a0periodic function of their atomic masses.&#8221;<\/strong><\/p>\n<p style=\"text-align: justify;\">On the basis of this law he arranged all the elements in order of increasing atomic mass and he found that <strong>after certain regular intervals repetition in properties occur.<\/strong><\/p>\n<ol style=\"list-style-type: upper-alpha; text-align: justify;\">\n<li>\n<h4><strong>Merits of Mendeleev\u2019s Table<\/strong><\/h4>\n<\/li>\n<\/ol>\n<ol style=\"list-style-type: lower-roman; text-align: justify;\">\n<li>First systematic classification of elements by forming a table. Mendeleev\u2019s periodic table has <strong>8 groups<\/strong> and <strong>7 periods.<\/strong><\/li>\n<li>Correction of Atomic Masses of the elements was done.<\/li>\n<li>He left a certain <strong>gap<\/strong> in the periodic table for <strong>undiscovered elements<\/strong> and he predicted the properties of those elements correctly. For instance, what he called <strong>Eka-Aluminium<\/strong> is now a days <strong>Gallium<\/strong> and what he called <strong>Eka-Silicon<\/strong> is now a days <strong>Germanium<\/strong>.<\/li>\n<\/ol>\n<ol style=\"list-style-type: upper-alpha; text-align: justify;\" start=\"2\">\n<li>\n<h4><strong>Demerits of Mendeleev\u2019s Table<\/strong><\/h4>\n<\/li>\n<\/ol>\n<ol style=\"list-style-type: lower-roman; text-align: justify;\">\n<li>Anomalous position of <strong>Hydrogen.\u00a0<\/strong>He failed to justify the position of Hydrogen because some properties of hydrogen were <strong>similar to alkali metals<\/strong> and some other properties were similar to <strong>halogens<\/strong>.<\/li>\n<li><strong>Cause of periodicity<\/strong>: He failed to explain<strong> why the repetition<\/strong> in properties occur after certain regular intervals.<\/li>\n<li>He failed to accommodate Lanthanides &amp; Actinides in the main body of the periodic table.<\/li>\n<li>Some pairs did not obey the rule of increasing atomic masses. For instance <strong>Tellurium with atomic number 52 had a mass of 127.60u but lodine with atomic number 53 had a mass of 126.90<\/strong> which was less than that of Tellurium.<\/li>\n<li>He failed to justify the <strong>position of isotopes<\/strong> in the periodic table.<\/li>\n<\/ol>\n<h3 style=\"text-align: justify;\"><span class=\"ez-toc-section\" id=\"Modern-Periodic-Law-And-Modern-Periodic-Table\"><\/span>Modern Periodic Law And Modern Periodic Table<span class=\"ez-toc-section-end\"><\/span><\/h3>\n<ol style=\"list-style-type: lower-roman; text-align: justify;\">\n<li><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-1278 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/modern-periodic-table.png\" alt=\"modern periodic table\" width=\"865\" height=\"163\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/modern-periodic-table.png 865w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/modern-periodic-table-300x57.png 300w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/modern-periodic-table-768x145.png 768w\" sizes=\"auto, (max-width: 865px) 100vw, 865px\" \/><\/li>\n<\/ol>\n<p style=\"text-align: justify;\">where Z is the atomic number of the target element and (a) and (b) are Moseley\u2019s constants.<\/p>\n<ol style=\"list-style-type: lower-roman; text-align: justify;\" start=\"2\">\n<li>The results of this experiment led to the <strong>re-framing of the periodic law<\/strong>. The modern periodic lav was hence propounded as, <strong>&#8220;The physical and chemical properties of elements are a periodic functions of their atomic numbers&#8221;.<\/strong><\/li>\n<\/ol>\n<p style=\"text-align: justify;\"><strong>Long Form of the Modern Periodic Table :<\/strong><\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-1285 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/bhors-table.png\" alt=\"bhors table\" width=\"928\" height=\"538\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/bhors-table.png 928w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/bhors-table-300x174.png 300w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/bhors-table-768x445.png 768w\" sizes=\"auto, (max-width: 928px) 100vw, 928px\" \/><\/p>\n<p style=\"text-align: justify;\"><strong>Some Important Points about the Modern Periodic Table :<\/strong><\/p>\n<ol style=\"list-style-type: lower-alpha; text-align: justify;\">\n<li>It consist of <strong>eighteen groups<\/strong>. Each group consists of a number of elements having the <strong>same outer electronic configuration.<\/strong><\/li>\n<li>The elements of <strong>18th group<\/strong> are called inert gases or noble gases.<\/li>\n<li>The elements of groups 3, 4, 5, 6, 7, 8, 9, 10, 11 and 12 are called <strong>transition elements.<\/strong><\/li>\n<li>Two series each of <strong>14 elements<\/strong> are placed at the bottom of the periodic table, known as <strong>Lanthanides and Actinides<\/strong> (Inner Transition Elements)<\/li>\n<li>There are 7 known periods (horizontal rows) in this table. Distribution of element in different periods are as below:<\/li>\n<\/ol>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-1317 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/Periodic-table.png\" alt=\"Periodic table\" width=\"332\" height=\"160\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/Periodic-table.png 332w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/Periodic-table-300x145.png 300w\" sizes=\"auto, (max-width: 332px) 100vw, 332px\" \/><\/p>\n<h4 style=\"text-align: justify;\">Atomic Size<\/h4>\n<ol style=\"list-style-type: lower-roman; text-align: justify;\">\n<li><strong>Atomic Radius<\/strong>: It is the <strong>distance from the centre of the nucleus to the outer most shell containing electron<\/strong>. It is impossible to isolate the atom and determine its radius precisely because its radius on is affected by its association with its neighbourhood. On the basis of the bond formed between atoms we can estimate the radius of the atom with great precision. Some of the radii are mentioned here:<\/li>\n<\/ol>\n<ol style=\"list-style-type: lower-alpha; text-align: justify;\" start=\"4\">\n<li><strong>Ionic Radius<\/strong>: The lonic radius may be defined as the effective <strong>distance from the centre of the nucleus of the ion upto which it exerts its influence on the electron cloud.<\/strong><\/li>\n<\/ol>\n<ol style=\"text-align: justify;\">\n<li style=\"list-style-type: none;\">\n<ol>\n<li style=\"list-style-type: none;\">\n<ol style=\"list-style-type: lower-roman;\">\n<li>The <strong>radius of cation is always smaller than that of its parent atom due to higher effective nuclear charge<\/strong> after removal of electron.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-1291\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/cation-1.png\" alt=\"cation\" width=\"469\" height=\"72\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/cation-1.png 469w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/cation-1-300x46.png 300w\" sizes=\"auto, (max-width: 469px) 100vw, 469px\" \/><br \/>\nDue to removal of a valence electron, the number of electrons decrease. Each electron now experiences greater nuclear pull. As a result, the size of cation is smaller than that of the parent atom.<\/li>\n<li>The <strong>radius of anion is always larger than that of its parent atom<\/strong>.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-1292\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/anion.png\" alt=\"anion\" width=\"460\" height=\"82\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/anion.png 460w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/anion-300x53.png 300w\" sizes=\"auto, (max-width: 460px) 100vw, 460px\" \/><br \/>\nAn anion is formed by <strong>gain of electron<\/strong>, which increases the number of electrons in the same shell. The <strong>effective nuclear charge now decreases<\/strong> and each electron <strong>experiences reduced nuclear pull.<\/strong> Repulsions between valence electrons now cause the cloud to expand making the anion larger in size than the neutral atom.<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<ul style=\"text-align: justify;\">\n<li><strong>Iso-electronicions<\/strong>: lons of different elements which have the same number of electrons but different magnitude of nuclear charge are called isoelectronic ions.<\/li>\n<li><strong>Variation of size:<\/strong> The <strong>ionic radius of iso-electronic ions decreases with the increase in the magnitude of nuclear charge.<\/strong><br \/>\ne.g., among isoelectronic ions of the second period the order of radius should be<br \/>\nC4&gt; N3-&gt; 02-&gt; F-&gt; Na+ &gt; Mg2+ &gt; Al3+<br \/>\nand among those of the third period:<br \/>\nSi4-&gt; P3-&gt; S2-&gt; CI &gt; K+ &gt; Ca2+<\/li>\n<\/ul>\n<ol style=\"list-style-type: lower-roman; text-align: justify;\" start=\"2\">\n<li><strong>Factors affecting the Atomic Radii :<\/strong><\/li>\n<\/ol>\n<ol style=\"list-style-type: lower-alpha; text-align: justify;\">\n<li><strong>Number of Shell:<\/strong> More the <strong>number of the shells<\/strong> filled with electrons, <strong>larger will be size.<\/strong><\/li>\n<li><strong>Nuclear Charge:<\/strong> Nuclear charge attracts the electrons toward itself and attempts to decrease the size. This is <strong>nuclear charge effect.<\/strong><br \/>\nGenerally, <strong>across the period size decreases<\/strong> because <strong>with increase in atomic number effective nuclear charge increases<\/strong>. As electrons are filled in the same shell they contract towards the nucleus causing size to decrease.<br \/>\n<strong>Down the group size generally increases, addition of an extra shell causes effective nuclear charge to decrease on the valence electron.<\/strong><\/li>\n<li><strong>Screening Effect or Shielding Effect<\/strong>: The inner layer of the electron act as shield between nucleus and valence electron. This is known as shielding effect or screening effect as discussed earlier.<br \/>\nEffective screening therefore attempts to increase the size and ineffective screening causes a decrease in atomic radius.<\/li>\n<\/ol>\n<ol style=\"list-style-type: lower-roman; text-align: justify;\" start=\"3\">\n<li><strong>Periodicity in Atomic Radius<\/strong><\/li>\n<\/ol>\n<ol style=\"list-style-type: lower-alpha; text-align: justify;\">\n<li><strong>In a Period:<\/strong> The number of orbit remains same on going from left to right in a period while effective nuclear charge increases. So, <strong>atomic radius decreases across the period<\/strong>.<\/li>\n<li><strong>In a Group:<\/strong> The <strong>atomic radius increases on going down a group<\/strong> due to addition of an extra shell.<\/li>\n<\/ol>\n<h4 style=\"text-align: justify;\">Ionization Energy (Enthalpy)<\/h4>\n<p style=\"text-align: justify;\">It is the amount of energy required to <strong>remove the outer most electron<\/strong> from an <strong>isolated atom in gaseous state.<\/strong><\/p>\n<p style=\"text-align: justify;\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-1307 aligncenter\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/Ionization.png\" alt=\"Ionization\" width=\"369\" height=\"133\" srcset=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/Ionization.png 369w, https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/Ionization-300x108.png 300w\" sizes=\"auto, (max-width: 369px) 100vw, 369px\" \/><\/p>\n<p style=\"text-align: justify;\">Neutral isolated gaseous atom is produced by firstly subliming the metal atom from its solid state. Further on, the energy needed to <strong>knock off the first outermost electron<\/strong> is called the<strong> first ionization enthalpy<\/strong>. As this is the energy required, so <strong>value of ionization enthalpy is always positive.<\/strong><\/p>\n<p style=\"text-align: justify;\">Unit wise, ionization enthalpy is expressed in kJ\/mole or kCal\/mol, however for an atom if the energy unit is in terms of eV then ionization enthalpy can also be refrred to as <strong>lonisation potential.<\/strong><\/p>\n<p style=\"text-align: justify;\"><strong>Successive lonisation Energy<\/strong><\/p>\n<ol style=\"list-style-type: lower-alpha; text-align: justify;\">\n<li><strong>lonisation Energy (First):<\/strong> It is the amount of energy required to remove the outer most e from an atom in gaseous state.<\/li>\n<li><strong>lonisation Energy (Second):<\/strong> It is the amount of energy required to remove the 2nd e- from same atom in gaseous state.<\/li>\n<\/ol>\n<p style=\"text-align: justify;\"><strong>Important Fact:\u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/strong> I.E<sub>2<\/sub> &gt; I.E<sub>1<\/sub><\/p>\n<p style=\"text-align: justify;\">Because 2<sup>nd<\/sup> electron has to be removed from a cation which has <strong>high effective nuclear charge<\/strong> and <strong>smaller size<\/strong> than the neutral atom.<\/p>\n<p style=\"text-align: justify;\">Ionisation energy generally<strong> increases across a period<\/strong> and <strong>decreases down the group.<\/strong><\/p>\n<p style=\"text-align: justify;\"><strong>Successive ionization energies are always larger. There is no exception to this rule.<\/strong><\/p>\n<h4 style=\"text-align: justify;\">Electron Gain Enthalpy<\/h4>\n<p style=\"text-align: justify;\">It is the <strong>enthalpy change<\/strong> when an <strong>electron is added to the gaseous neutral atom.<\/strong><\/p>\n<p style=\"text-align: justify;\">Electron gain enthalpy provides a measure of the ease with which an atom adds an electron to form anion.<\/p>\n<p style=\"text-align: center;\">X(g) + e<sup>&#8211;<\/sup> \u2192 X<sup>&#8211;<\/sup>(g); \u2206H = A<sub>eg<\/sub>H\u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 ..(i)<\/p>\n<p style=\"text-align: justify;\"><strong>The negative of the enthalpy change for the process shown in equation is defined as electron affinity of the atom undergoing the change for formation of anion.<\/strong><\/p>\n<p style=\"text-align: justify;\">Depending on the element, enthalpy change in process may be <strong>endothermic <\/strong>or <strong>exothermic.<\/strong><\/p>\n<p style=\"text-align: justify;\">When electron is added to gaseous neutral atom that has a <strong>natural tendency to accept an electron then energy is released, electron gain enthalpy is negative and electron affinity is positive.<\/strong><\/p>\n<p style=\"text-align: justify;\">When an electron is added to an element that <strong>does not have a natural tendency to accept an electron then energy will be absorbed electron gain enthalpy will be positive and electron affinity will be negative.<\/strong><\/p>\n<h4 style=\"text-align: justify;\">Electronegativity<\/h4>\n<p style=\"text-align: justify;\">Electronegativity is a <strong>measure of the tendency of an element to attract bonded electron pair<\/strong> towards (itself) in a covalent bonded molecule.<\/p>\n<ol style=\"list-style-type: lower-roman; text-align: justify;\">\n<li><strong>Factors on which electronegativity depend:<\/strong><\/li>\n<\/ol>\n<ol style=\"list-style-type: lower-alpha; text-align: justify;\">\n<li><strong>Atomic Size<\/strong>: <strong>Electronegativity is inversely proportional to the size.<\/strong> Small sized elements generally have higher electronegativity.<\/li>\n<li><strong>Effective Nuclear Charge:<\/strong> Electronegativity is <strong>directly proportional<\/strong> to the effective nuclear charge. Elements such as fluorine have highest effective nuclear charge in the second period and hence have the highest electronegativity.<\/li>\n<li><strong>Hybridization:<\/strong> More is the s-character in hybridization, higher will be electronegativity. The order of electronegativity among different hybridizations is:<br \/>\n<strong>sp hybrid carbon &gt;sp<sup>2<\/sup> hybrid carbon &gt; sp<sup>3<\/sup> hybrid carbon<\/strong><\/li>\n<\/ol>\n<ol style=\"list-style-type: lower-roman; text-align: justify;\" start=\"2\">\n<li><strong>Electronegativity Scales:<\/strong><\/li>\n<\/ol>\n<ol style=\"list-style-type: lower-alpha; text-align: justify;\">\n<li><strong>Mulliken Scale:<\/strong> According to Mulliken, <img decoding=\"async\" class=\"alignnone size-full wp-image-1211\" src=\"https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/electronegativity.png\" alt=\"NEET Chemistry Class XI Module\" \/><br \/>\nBoth ionization energy and electron affinity are taken in eV\/atom.<\/li>\n<li><strong>Pauling Scale<\/strong>: Linus Pauling developed a method for the calculation of relative electronegativity of element.<br \/>\n<img decoding=\"async\" class=\"alignnone size-full wp-image-1211\" src=\" https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/Pauling.png\" alt=\"NEET Chemistry Class XI Module\" \/><strong>Relation between Mulliken and Pauling Scale<\/strong>: The value of electronegativity for an element in <strong>Mulliken scale is 2.8 times higher than Pauling\u2019s value.<\/strong><\/li>\n<li><strong>Allred Rochow&#8217;s Electronegativity<\/strong>: Allred and Rochow defined electronegativity as the force exerted by the nucleus of an atom on its valence electrons:<\/li>\n<\/ol>\n<p style=\"text-align: justify;\"><img decoding=\"async\" class=\"size-full wp-image-1211 aligncenter\" src=\" https:\/\/www.meniit.com\/study-material\/wp-content\/uploads\/2024\/08\/Rochows-Electronegativity.png \" alt=\"NEET Chemistry Class XI Module\" \/>Here, Z<sub>eff<\/sub> is effective nuclear charge and r is the radius of the atom.<\/p>\n<p style=\"text-align: justify;\">On the Pauling Scale: <strong>Fluorine is most electronegative element<\/strong> with an electronegativity value of <strong>4.0<\/strong> followed by <strong>oxygen with a value of 3.5.<\/strong><\/p>\n<div class=\"newspaper-x-tags\"><strong>TAGS: <\/strong><span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/anion\" rel=\"tag\">anion<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/atomic-size\" rel=\"tag\">Atomic Size<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/classification-of-elements\" rel=\"tag\">Classification of Elements<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/electron-gain-enthalpy\" rel=\"tag\">Electron Gain Enthalpy<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/electronegativity\" rel=\"tag\">Electronegativity<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/hybridization\" rel=\"tag\">Hybridization<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/ionization-energy\" rel=\"tag\">Ionization Energy<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/mendeleevs-periodic-table\" rel=\"tag\">Mendeleev\u2019s periodic table<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/modern-periodic-law\" rel=\"tag\">Modern Periodic Law<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/modern-periodic-table\" rel=\"tag\">Modern Periodic Table<\/a><\/span><a href=\"https:\/\/www.meniit.com\/study-material\/tag\/nuclear-charge\" rel=\"tag\">Nuclear Charge<\/a> <\/div>\n","protected":false},"excerpt":{"rendered":"<p>Mendeleev\u2019s Periodic Table Periodic Law &#8220;The physical and chemical properties of elements are a\u00a0periodic function of their atomic masses.&#8221; On&nbsp;&nbsp;&#8230;.<a class=\"read_more\" href=\"https:\/\/www.meniit.com\/study-material\/neet\/class-11th\/chemistry\/modern-periodic-table-laws\" rel=\"nofollow\">Read More >><\/a><\/p>\n","protected":false},"author":6,"featured_media":1381,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"om_disable_all_campaigns":false,"rank_math_lock_modified_date":false,"footnotes":""},"categories":[268,241,240],"tags":[443,439,436,441,442,444,440,435,438,437,445],"class_list":["post-1276","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-chemistry","category-class-11th","category-neet","tag-anion","tag-atomic-size","tag-classification-of-elements","tag-electron-gain-enthalpy","tag-electronegativity","tag-hybridization","tag-ionization-energy","tag-mendeleevs-periodic-table","tag-modern-periodic-law","tag-modern-periodic-table","tag-nuclear-charge"],"acf":[],"_links":{"self":[{"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/posts\/1276","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/users\/6"}],"replies":[{"embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/comments?post=1276"}],"version-history":[{"count":16,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/posts\/1276\/revisions"}],"predecessor-version":[{"id":1463,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/posts\/1276\/revisions\/1463"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/media\/1381"}],"wp:attachment":[{"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/media?parent=1276"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/categories?post=1276"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.meniit.com\/study-material\/wp-json\/wp\/v2\/tags?post=1276"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}