{"id":1123,"date":"2020-12-03T05:08:27","date_gmt":"2020-12-02T23:38:27","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=1123"},"modified":"2020-12-03T17:07:52","modified_gmt":"2020-12-03T11:37:52","slug":"sp3-hybridized-carbon-atom","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/sp3-hybridized-carbon-atom\/","title":{"rendered":"What is an sp3 Hybridized Carbon atom"},"content":{"rendered":"

What is an\u00a0sp3\u00a0<\/sup>Hybridized Carbon atom
\n<\/span><\/strong><\/span><\/h2>\n

sp<\/strong>3<\/strong>\u00a0<\/sup>Hybridisation<\/b><\/span><\/p>\n

In the excited carbon atom its one s-orbital (2s) and three p-orbitals\u00a0(2px<\/sub> , 2py<\/sub>, 2pz<\/sub>) intermix and reshuffle into four identical orbitals known as\u00a0sp3\u00a0<\/sup>orbitals. Thus, carbon atom undergoes \u00a0sp3<\/sup>\u00a0<\/b>hybridisation.
\nThe four electrons enter into the new four identical hybrid orbitals\u00a0known as sp3<\/sup> hybrid orbitals one each as per Hund\u2019s rule. (because they\u00a0are made from one \u2018s-orbital\u2019 and three \u2018p-orbitals\u2019 they are called sp3<\/sup> orbitals).
\n\"What
\nThe hybridisation enables the carbon to have four identical sp3<\/sup> hybrid\u00a0orbitals and these have one electron each. Since carbon has four unpaired\u00a0electrons, it is capable of forming bonds with four other atoms may be\u00a0carbon or atoms of some other monovalent element. When carbon reacts\u00a0with hydrogen, four hydrogen atoms allow their \u2018s\u2019 orbitals containing one\u00a0electron each to overlap the four sp3\u00a0<\/sup>orbitals of carbon atom which are\u00a0orieted at an angle of 109\u00b028′. (Four orbitals of an atom in the outer shell\u00a0orient along the four corners of a tetrahedron to have minimum repulsion\u00a0between their electrons). The nucleus of the atom is at the centre of the\u00a0tetrahedron. See figures below:
\n\"What
\nThis leads to form four sp3<\/sup> \u2013 s sigma bonds between carbon atom and\u00a0four hydrogen atoms. All these bonds are of equal energy.<\/p>\n

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