Predict the acid strengths of the following compounds: H2O, H2S, and H2Se.
H2S > H2Se > H2O
H2O > H2Se > H2S
H2Se > H2S > H2O
H2Se > H2O > H2S
H2S > H2O > H2Se
H2O > H2S > H2Se<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n The correct order of acid strengths for the compounds H\u2082O, H\u2082S, and H\u2082Se is: H\u2082Se > H\u2082S > H\u2082O.<\/p>\n\n\n\n This trend can be explained by examining the periodic properties of the elements involved, particularly focusing on bond strength and atomic size.<\/p>\n\n\n\n Bond Strength and Atomic Size:<\/strong><\/p>\n\n\n\n As we move down Group 16 in the periodic table from oxygen (O) to sulfur (S) to selenium (Se), the atomic radius increases. This increase in atomic size leads to longer and weaker bonds between hydrogen and the central atom in each molecule. Specifically, the H\u2013O bond in H\u2082O is stronger than the H\u2013S bond in H\u2082S, which in turn is stronger than the H\u2013Se bond in H\u2082Se. Weaker bonds are more easily broken, facilitating the release of a proton (H\u207a), which is the defining characteristic of acid strength. Therefore, H\u2082Se, with the weakest H\u2013Se bond, is the strongest acid among the three, followed by H\u2082S, and then H\u2082O.<\/p>\n\n\n\n Electronegativity Considerations:<\/strong><\/p>\n\n\n\n While electronegativity generally decreases down a group, which might suggest a decrease in acidity, in this case, the bond strength factor predominates. The decreasing bond dissociation energy down the group has a more significant impact on the acid strength than the electronegativity differences. Thus, the trend of increasing acid strength from H\u2082O to H\u2082Se is primarily due to the weakening H\u2013X bonds as the central atom’s size increases.<\/p>\n\n\n\n Conjugate Base Stability:<\/strong><\/p>\n\n\n\n Another factor influencing acid strength is the stability of the conjugate base formed after deprotonation. Larger atoms like selenium can better stabilize the negative charge due to their larger electron cloud, making the conjugate base more stable. This increased stability of the conjugate base further contributes to the higher acidity of H\u2082Se compared to H\u2082S and H\u2082O.<\/p>\n\n\n\n In summary, the increasing acid strength from H\u2082O to H\u2082Se is primarily attributed to the decreasing bond strength between hydrogen and the central atom as we move down Group 16, coupled with the enhanced stability of the conjugate bases formed.<\/p>\n","protected":false},"excerpt":{"rendered":" Predict the acid strengths of the following compounds: H2O, H2S, and H2Se.H2S > H2Se > H2OH2O > H2Se > H2SH2Se > H2S > H2OH2Se > H2O > H2SH2S > H2O > H2SeH2O > H2S > H2Se The Correct Answer and Explanation is : The correct order of acid strengths for the compounds H\u2082O, H\u2082S, and […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-183755","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183755","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=183755"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183755\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=183755"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=183755"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=183755"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}