What is the electron configuration of V3+? [Ar]4s23d3 [Ar]4s23d0 [Ar]4s03d2 [Ar]4s23d5 What are possible correct quantum numbers for two outer most valence electrons in V3+? 3,3,-2, +1\/2 AND 3,3,-1, + 1\/2 3,2,-2,+ 1\/2 AND 3,2,-1, + 1\/2 4,1,0 + 1\/2 AND 4,1,0, – 1\/2 4,0,0+ 1\/2 AND 4,0,0, – 1\/2 How many unpaired electrons does V3+ have? Three One None Two Is V3+ paramagnetic or diamagnetic? Why? Diamagnetic because it has paired electrons Paramagnetic because it has unpaired electrons Paramagnetic because it has paired electrons Diamagnetic because it has unpaired electrons<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n To determine the electron configuration of ( \\text{V}^{3+} ), we start with the electron configuration of the neutral vanadium (( \\text{V} )) atom, which has an atomic number of 23. The ground state electron configuration for vanadium is:<\/p>\n\n\n\n [ When vanadium loses three electrons to form ( \\text{V}^{3+} ), the electrons are removed first from the 4s subshell and then from the 3d subshell. Therefore, the electron configuration for ( \\text{V}^{3+} ) becomes:<\/p>\n\n\n\n [ So, the correct answer is [ \\text{Ar} 3d^2 ]<\/strong>.<\/p>\n\n\n\n The two outermost electrons in ( \\text{V}^{3+} ) are found in the 3d subshell, where there are two electrons. The possible correct quantum numbers for these electrons can be derived as follows:<\/p>\n\n\n\n From the options provided, the set 3,2,-2,+\\frac{1}{2}<\/strong> and 3,2,-1,+\\frac{1}{2}<\/strong> accurately reflects the quantum numbers for the two valence electrons in ( \\text{V}^{3+} ).<\/p>\n\n\n\n In ( \\text{V}^{3+} ), the 3d subshell contains 2 electrons (( 3d^2 )). When filling the 3d orbitals, the two electrons occupy two different orbitals to minimize repulsion (Hund’s rule), resulting in both electrons being unpaired. Therefore, ( \\text{V}^{3+} ) has two unpaired electrons<\/strong>.<\/p>\n\n\n\n Since ( \\text{V}^{3+} ) has unpaired electrons, it is paramagnetic<\/strong>. Paramagnetic materials are attracted to magnetic fields due to the presence of unpaired electrons, which contribute to a net magnetic moment. In contrast, diamagnetic materials, which have all electrons paired, are weakly repelled by magnetic fields.<\/p>\n\n\n\n In summary:<\/p>\n\n\n\n What is the electron configuration of V3+? [Ar]4s23d3 [Ar]4s23d0 [Ar]4s03d2 [Ar]4s23d5 What are possible correct quantum numbers for two outer most valence electrons in V3+? 3,3,-2, +1\/2 AND 3,3,-1, + 1\/2 3,2,-2,+ 1\/2 AND 3,2,-1, + 1\/2 4,1,0 + 1\/2 AND 4,1,0, – 1\/2 4,0,0+ 1\/2 AND 4,0,0, – 1\/2 How many unpaired electrons does […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"","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-152882","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/152882","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=152882"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/152882\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=152882"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=152882"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=152882"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\\text{V: } [\\text{Ar}] 4s^2 3d^3
]<\/p>\n\n\n\n
\\text{V}^{3+}: [\\text{Ar}] 3d^2
]<\/p>\n\n\n\nQuantum Numbers for Two Outermost Valence Electrons in ( \\text{V}^{3+} )<\/h3>\n\n\n\n
\n
Number of Unpaired Electrons in ( \\text{V}^{3+} )<\/h3>\n\n\n\n
Paramagnetism vs. Diamagnetism<\/h3>\n\n\n\n
\n