{"id":1901,"date":"2025-05-09T12:46:15","date_gmt":"2025-05-09T12:46:15","guid":{"rendered":"https:\/\/yaveni.com\/blog\/?p=1901"},"modified":"2025-05-09T12:46:16","modified_gmt":"2025-05-09T12:46:16","slug":"what-is-the-hybridization-of-cunh342","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/what-is-the-hybridization-of-cunh342\/","title":{"rendered":"What is the hybridization of [Cu(NH3)4]2+"},"content":{"rendered":"\n

What is the hybridization of [Cu(NH3)4]2+?<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The hybridization of the central copper ion in the complex $[Cu(NH_3)_4]^{2+}$ is d^2sp^3<\/strong>.<\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

The complex $[Cu(NH_3)_4]^{2+}$ involves a copper ion (Cu\u00b2\u207a) coordinated to four ammonia (NH\u2083) ligands. To determine the hybridization of the central metal ion (Cu\u00b2\u207a), we need to consider its electronic configuration, the nature of the ligands, and the coordination number of the complex.<\/p>\n\n\n\n

    \n
  1. Oxidation State of Copper<\/strong>: In $[Cu(NH_3)_4]^{2+}$, the copper ion is in the +2 oxidation state. The electronic configuration of copper (Cu) in its ground state is [Ar] 3d\u00b9\u2070 4s\u00b9. Upon losing two electrons to form Cu\u00b2\u207a, the electron configuration becomes [Ar] 3d\u2079. This means that Cu\u00b2\u207a has a partially filled d-orbital, which is available for bonding with ligands.<\/li>\n\n\n\n
  2. Ligands and Coordination Number<\/strong>: Ammonia (NH\u2083) is a neutral ligand that donates a lone pair of electrons to the metal ion. In this complex, there are four NH\u2083 ligands, which means the coordination number of copper is 4. A coordination number of 4 generally results in a square planar or tetrahedral geometry, depending on the metal’s electronic structure.<\/li>\n\n\n\n
  3. Geometry and Hybridization<\/strong>: Copper(II) typically prefers a square planar<\/strong> geometry when coordinated by four ligands, especially for d\u2078 metal ions, such as Cu\u00b2\u207a. This is because the d-orbitals of Cu\u00b2\u207a will interact with the ligands in such a way that the hybridization leads to a square planar arrangement. In the square planar geometry, the copper ion undergoes d^2sp^3 hybridization<\/strong>, where two d-orbitals, one s-orbital, and one p-orbital mix to form six hybrid orbitals. Four of these hybrid orbitals are used to form bonds with the four NH\u2083 ligands, while the remaining two hybrid orbitals can accommodate lone pairs if necessary.<\/li>\n<\/ol>\n\n\n\n

    Therefore, the hybridization of Cu\u00b2\u207a in $[Cu(NH_3)_4]^{2+}$ is d^2sp^3<\/strong>, leading to a square planar geometry.<\/p>\n","protected":false},"excerpt":{"rendered":"

    What is the hybridization of [Cu(NH3)4]2+? The correct answer and explanation is : The hybridization of the central copper ion in the complex $[Cu(NH_3)_4]^{2+}$ is d^2sp^3. Explanation: The complex $[Cu(NH_3)_4]^{2+}$ involves a copper ion (Cu\u00b2\u207a) coordinated to four ammonia (NH\u2083) ligands. To determine the hybridization of the central metal ion (Cu\u00b2\u207a), we need to consider […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[],"tags":[],"class_list":["post-1901","post","type-post","status-publish","format-standard","hentry"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/1901","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=1901"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/1901\/revisions"}],"predecessor-version":[{"id":1902,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/1901\/revisions\/1902"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=1901"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=1901"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=1901"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}