In The Compound C1H2 C2 C3H C4H3 The Hybridization Class 12 ...

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• In the compound C1H2 C2 C3H C4...

AnswerQuestion Answers for Class 12Class 12 BiologyClass 12 ChemistryClass 12 EnglishClass 12 MathsClass 12 PhysicsClass 12 Social ScienceClass 12 Business StudiesClass 12 EconomicsQuestion Answers for Class 11Class 11 EconomicsClass 11 Computer ScienceClass 11 BiologyClass 11 ChemistryClass 11 EnglishClass 11 MathsClass 11 PhysicsClass 11 Social ScienceClass 11 AccountancyClass 11 Business StudiesQuestion Answers for Class 10Class 10 ScienceClass 10 EnglishClass 10 MathsClass 10 Social ScienceClass 10 General KnowledgeQuestion Answers for Class 9Class 9 General KnowledgeClass 9 ScienceClass 9 EnglishClass 9 MathsClass 9 Social ScienceQuestion Answers for Class 8Class 8 ScienceClass 8 EnglishClass 8 MathsClass 8 Social ScienceQuestion Answers for Class 7Class 7 ScienceClass 7 EnglishClass 7 MathsClass 7 Social ScienceQuestion Answers for Class 6Class 6 ScienceClass 6 EnglishClass 6 MathsClass 6 Social ScienceQuestion Answers for Class 5Class 5 ScienceClass 5 EnglishClass 5 MathsClass 5 Social ScienceQuestion Answers for Class 4Class 4 ScienceClass 4 EnglishClass 4 MathsIn the compound ${C^1}{H_2} = {C^2} = {C^3}H = {C^4}{H_3}$, the hybridization of first, second carbon atom is:A)$s{p^3} - sp$B) $s{p^2} - s{p^3}$ C) $s{p^2} - sp$ D) $s{p^2} - s{p^2}$AnswerVerified567k+ viewsHint:We know that,Hybridization:Hybridization is the idea that atomic orbitals combine to form new hybridized orbitals which in turn, influences molecular geometry and bonding properties.We know that the electrons which are present at the outermost shell of an atom are called valence electrons and valency of an electron is the number of electrons in which atom accepts or donate to form a bond.Complete step by step answer:Given,The molecular formula of the compound is,${C^1}{H_2} = {C^2} = {C^3}H = {C^4}{H_3}$In this compound each of two electrons of the central atom forms collinear $sp$ sigma bonds to the terminal $s{p^2}$ hybridized carbons. The two remaining electrons of the central carbon occupy p orbitals and form pi bonds through an overlap of these p orbitals and the p orbitals of the terminal carbons.Thus the First carbon is $s{p^2}$ hybridized and second carbon is \[sp\] hybridized.Therefore option C is correct.Note: The \[sp\] Hybridization:The \[sp\] hybridization is practical when one s and one p orbital in the same shell of an atom mix to form two new equivalent orbitals. The new orbitals formed are called \[sp\] hybridized orbitals. It forms linear molecules with an angle of \[180^\circ \]. This hybridization is also called diagonal hybridization. Each \[sp\]hybridized orbital has an equal amount of s and p character, i.e., \[50\% \] s and p character.The \[s{p^2}\] Hybridization:This hybridization is possible when one s and two p orbitals of the same shell of an atom mix to form three equivalent orbits. The new orbitals formed are called \[s{p^2}\] hybrid orbitals. It is also called trigonal hybridization. Each of the hybrid orbitals formed has \[33.33\% \] s character and \[66.66\% \] ‘p’ character.Recently Updated PagesMaster Class 12 Business Studies: Engaging Questions & Answers for SuccessMaster Class 12 Economics: Engaging Questions & Answers for SuccessMaster Class 12 English: Engaging Questions & Answers for SuccessMaster Class 12 Maths: Engaging Questions & Answers for SuccessMaster Class 12 Social Science: Engaging Questions & Answers for SuccessMaster Class 12 Chemistry: Engaging Questions & Answers for SuccessMaster Class 12 Business Studies: Engaging Questions & Answers for SuccessMaster Class 12 Economics: Engaging Questions & Answers for SuccessMaster Class 12 English: Engaging Questions & Answers for SuccessMaster Class 12 Maths: Engaging Questions & Answers for SuccessMaster Class 12 Social Science: Engaging Questions & Answers for SuccessMaster Class 12 Chemistry: Engaging Questions & Answers for Success

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