If a molecule possess 4 bonds and 2 lone pairs the Structure it can adopt is A. Octahedral B. See-saw C. Square planer D. Square pyramidal<\/p>\n\n\n\n
The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n Correct Answer: C. Square planar<\/strong><\/p>\n\n\n\n When determining the molecular structure of a molecule based on the number of bonding and lone pairs, we use the Valence Shell Electron Pair Repulsion (VSEPR) theory. This theory helps predict the geometry of a molecule by considering how electron pairs repel each other.<\/p>\n\n\n\n In the given case, the molecule has 4 bonds<\/strong> and 2 lone pairs<\/strong>, which means there are 6 regions of electron density<\/strong> around the central atom. These 6 regions (4 bonding pairs + 2 lone pairs) correspond to an electron geometry<\/strong> of octahedral<\/strong>. This is because 6 electron regions are arranged around a central atom in an octahedral shape to minimize repulsion.<\/p>\n\n\n\n However, VSEPR theory distinguishes between electron geometry and molecular geometry<\/strong>. While the electron geometry is octahedral due to six electron regions, the molecular geometry<\/strong> depends only on the position of atoms, not the lone pairs.<\/p>\n\n\n\n When two of the positions in the octahedral arrangement are occupied by lone pairs and the other four by bonding atoms, the atoms arrange themselves in a square planar<\/strong> geometry. The lone pairs take up positions opposite each other (usually the axial positions) to reduce electron pair repulsion, leaving the four bonded atoms in a square plane.<\/p>\n\n\n\n This kind of structure is common in certain metal complexes, such as [PtCl\u2084]\u00b2\u207b<\/strong>, where platinum is the central atom surrounded by four chlorine atoms and two lone pairs.<\/p>\n\n\n\n Therefore, a molecule with 4 bonds and 2 lone pairs will have a square planar<\/strong> molecular geometry due to the arrangement of atoms around a central atom that minimizes repulsion among all electron regions.<\/p>\n\n\n\n So, the correct answer is C. Square planar<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":" If a molecule possess 4 bonds and 2 lone pairs the Structure it can adopt is A. Octahedral B. See-saw C. Square planer D. Square pyramidal The correct answer and explanation is: Correct Answer: C. Square planar When determining the molecular structure of a molecule based on the number of bonding and lone pairs, we […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-31019","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/31019","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=31019"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/31019\/revisions"}],"predecessor-version":[{"id":31024,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/31019\/revisions\/31024"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=31019"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=31019"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=31019"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}