{"id":3657,"date":"2023-01-09T10:11:18","date_gmt":"2023-01-09T10:11:18","guid":{"rendered":"https:\/\/9thclass.deltapublications.in\/?page_id=3657"},"modified":"2025-01-06T17:21:21","modified_gmt":"2025-01-06T17:21:21","slug":"s-4-d-valency","status":"publish","type":"page","link":"https:\/\/9thclass.deltapublications.in\/index.php\/s-4-d-valency\/","title":{"rendered":"S-4.d Valency"},"content":{"rendered":"\n<h2 class=\"wp-block-heading has-text-align-center has-text-color\" style=\"color:#00056d;text-transform:uppercase\"><strong>Valency<\/strong><\/h2>\n\n\n\n<p class=\"has-text-color has-huge-font-size\" style=\"color:#74008b\"><strong>Key Notes:<\/strong><\/p>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-63ede3d11918dd73981c91de577682be\" style=\"color:#000060;background-color:#dfc816\"><strong>Definition of Valency<\/strong>:<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large is-resized\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"576\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-11-1024x576.png\" alt=\"\" class=\"wp-image-15854\" style=\"width:446px;height:auto\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-11-1024x576.png 1024w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-11-300x169.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-11-768x432.png 768w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-11.png 1280w\" sizes=\"auto, (max-width: 1024px) 100vw, 1024px\" \/><\/figure><\/div>\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Valency<\/strong> is the combining capacity of an element, indicating how many atoms of other elements it can combine with to form a compound.<\/li>\n\n\n\n<li>It reflects the number of electrons an atom can lose, gain, or share to achieve a stable electronic configuration (usually that of a noble gas).<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-e069c8843754314304166b813f5cdb45\" style=\"color:#000060;background-color:#dfc816\"><strong>Valence Electrons<\/strong>:<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" width=\"700\" height=\"327\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-44.png\" alt=\"\" class=\"wp-image-15856\" style=\"width:522px;height:auto\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-44.png 700w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/Untitled-design-44-300x140.png 300w\" sizes=\"auto, (max-width: 700px) 100vw, 700px\" \/><\/figure><\/div>\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>The <strong>electrons in the outermost shell<\/strong> of an atom are known as <strong>valence electrons<\/strong>.<\/li>\n\n\n\n<li>These electrons determine the valency of an atom as they participate in chemical bonding.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-243066aef805a18ba3d9eb16a7b67eaa\" style=\"color:#000060;background-color:#dfc816\"><strong>Types of Valency<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Positive Valency<\/strong>: If an atom loses electrons to achieve stability (commonly seen in metals), its valency is <strong>positive<\/strong>.<\/li>\n\n\n\n<li><strong>Negative Valency<\/strong>: If an atom gains electrons to achieve stability (common in non-metals), its valency is <strong>negative<\/strong>.<\/li>\n\n\n\n<li><strong>Zero Valency<\/strong>: Noble gases have a valency of zero since they already have a stable electronic configuration.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-ed0d240c7e3af931a15d77c6b261af63\" style=\"color:#000060;background-color:#dfc816\"><strong>Valency and the Octet Rule<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Atoms strive to have <strong>8 electrons in their outermost shell<\/strong> (octet rule), which is why they either lose, gain, or share electrons during chemical reactions.<\/li>\n\n\n\n<li>For elements with fewer electrons in their outermost shell (like hydrogen, helium, and lithium), achieving a stable configuration often means having <strong>2 electrons<\/strong> (duplet rule).<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-8121a86057b1d757584345927dffb04a\" style=\"color:#000060;background-color:#dfc816\"><strong>Valency of Common Elements<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li><strong>Hydrogen (H)<\/strong>: 1<\/li>\n\n\n\n<li><strong>Oxygen (O)<\/strong>: 2<\/li>\n\n\n\n<li><strong>Nitrogen (N)<\/strong>: 3<\/li>\n\n\n\n<li><strong>Carbon (C)<\/strong>: 4<\/li>\n\n\n\n<li><strong>Sodium (Na)<\/strong>: 1<\/li>\n\n\n\n<li><strong>Chlorine (Cl)<\/strong>: 1<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-e735ebf15d0d1c66c1bd1bf30ab63a8e\" style=\"color:#000060;background-color:#dfc816\"><strong>Determining Valency<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>For elements in <strong>Groups 1, 2, and 13<\/strong> of the periodic table, valency is typically equal to the number of valence electrons.<\/li>\n\n\n\n<li>For elements in <strong>Groups 15, 16, and 17<\/strong>, valency is calculated by subtracting the number of valence electrons from 8.<\/li>\n\n\n\n<li>Example: For sulfur (Group 16), valency = 8 \u2212 6 = 2<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-4721d878fc475c108cb3163e77c51f70\" style=\"color:#000060;background-color:#dfc816\"><strong>Variable Valency<\/strong>:<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large is-resized\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"373\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-12-1024x373.png\" alt=\"\" class=\"wp-image-15857\" style=\"width:511px;height:auto\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-12-1024x373.png 1024w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-12-300x109.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-12-768x280.png 768w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2024\/11\/image-12.png 1189w\" sizes=\"auto, (max-width: 1024px) 100vw, 1024px\" \/><\/figure><\/div>\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Some elements can have more than one valency (e.g., <strong>iron<\/strong> can have a valency of <strong>2 or 3<\/strong>).<\/li>\n\n\n\n<li>This happens because certain elements can lose different numbers of electrons under different conditions.<\/li>\n<\/ul>\n\n\n\n<p class=\"has-text-align-center has-text-color has-background has-link-color has-large-font-size wp-elements-12cfa6009fd1d3fc2c49218e28b71858\" style=\"color:#000060;background-color:#dfc816\"><strong>Applications of Valency<\/strong>:<\/p>\n\n\n\n<ul class=\"has-large-font-size wp-block-list\">\n<li>Understanding valency helps predict the <strong>chemical formulas<\/strong> of compounds.<\/li>\n\n\n\n<li>For example, water (H2O) has 2 atoms of hydrogen (valency 1) combining with 1 atom of oxygen (valency 2).<\/li>\n<\/ul>\n\n\n\n<div class=\"wp-block-group has-large-font-size\"><div class=\"wp-block-group__inner-container is-layout-constrained wp-block-group-is-layout-constrained\">\n<p class=\"has-text-color has-large-font-size\" style=\"color:#d90000\"><strong>Let&#8217;s practice!<\/strong><\/p>\n<\/div><\/div>\n\n\n\n<div class=\"wp-block-columns is-layout-flex wp-container-core-columns-is-layout-9d6595d7 wp-block-columns-is-layout-flex\">\n<div class=\"wp-block-column is-layout-flow wp-block-column-is-layout-flow\">\n<figure class=\"wp-block-image size-full\"><a href=\"https:\/\/wordwall.net\/play\/76018\/613\/340\"><img loading=\"lazy\" decoding=\"async\" width=\"500\" height=\"500\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-2-17.png\" alt=\"\" class=\"wp-image-6388\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-2-17.png 500w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-2-17-300x300.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-2-17-150x150.png 150w\" sizes=\"auto, (max-width: 500px) 100vw, 500px\" \/><\/a><\/figure>\n<\/div>\n\n\n\n<div class=\"wp-block-column is-layout-flow wp-block-column-is-layout-flow\">\n<figure class=\"wp-block-image size-full\"><a href=\"https:\/\/wordwall.net\/play\/76022\/377\/353\"><img loading=\"lazy\" decoding=\"async\" width=\"500\" height=\"500\" src=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-1-1-18.png\" alt=\"\" class=\"wp-image-6389\" srcset=\"https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-1-1-18.png 500w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-1-1-18-300x300.png 300w, https:\/\/9thclass.deltapublications.in\/wp-content\/uploads\/2023\/03\/Worksheet-1-1-1-18-150x150.png 150w\" sizes=\"auto, (max-width: 500px) 100vw, 500px\" \/><\/a><\/figure>\n<\/div>\n<\/div>\n","protected":false},"excerpt":{"rendered":"<p>Valency Key Notes: Definition of Valency: Valence Electrons: Types of Valency: Valency and the Octet Rule: Valency of Common Elements: Determining Valency: Variable Valency: Applications of Valency: Let&#8217;s practice!<\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"om_disable_all_campaigns":false,"_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"footnotes":""},"class_list":["post-3657","page","type-page","status-publish","hentry","entry"],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages\/3657","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/comments?post=3657"}],"version-history":[{"count":19,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages\/3657\/revisions"}],"predecessor-version":[{"id":16349,"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/pages\/3657\/revisions\/16349"}],"wp:attachment":[{"href":"https:\/\/9thclass.deltapublications.in\/index.php\/wp-json\/wp\/v2\/media?parent=3657"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}