one drawback of valency theory
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Postulates of Valence Bond Theory
The Valence Bond Theory postulatescertain assumptions and facts that go on to establish certain premises and facts which lead to the conclusion and assertion of the Theory to be true.The overlapping of two half-filled valence orbitals of two different atoms results in the formation of the covalent bond. Due to overlapping, the electron density between two bonded atoms increases and this gives stability to the molecule.In case the atomic orbitals possess more than one unpaired electron, more than one bond can be formed and electrons paired in the valence shell cannot take part in such a bond formation.A covalent bond is directional and it is parallel to the region of overlapping atomic orbitals.Based on the pattern of overlapping, there are two types of covalent bonds: sigma bond and a pi bond. The covalent bond formed by sideways overlapping of atomic orbitals is known as pi bond whereas the bond formed by overlapping of atomic orbital along the inter nucleus axis is known as a sigma bond.
Limitations of Valence Bond Theory
The theories and laws that came before this also had certain limitations on them resulting in their failure. However, the theory is also not perfect and does have its shortcomings. The Limitations of Valence Bond Theory are:
It fails to explain the tetravalency of carbon.This theory does not discuss the energies of electrons.The assumptions about the electrons being localized to specific locations.
To follow more on this, Check Valence Bond Theory in Coordination Compound.
Practise This Question
Which of the following represents s - s, s - p and p - p overlap respectively?

I, II, III
III, II, I
I, III, II
II, III, I
Submit
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Practise This Question
Which of the following compounds does not have molecular plane as nodal plane for its π - electron cloud?
CH2 = CH2
C6H6
CH2 = C = CH2
All of the above
Submit


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The Valence Bond Theory postulatescertain assumptions and facts that go on to establish certain premises and facts which lead to the conclusion and assertion of the Theory to be true.The overlapping of two half-filled valence orbitals of two different atoms results in the formation of the covalent bond. Due to overlapping, the electron density between two bonded atoms increases and this gives stability to the molecule.In case the atomic orbitals possess more than one unpaired electron, more than one bond can be formed and electrons paired in the valence shell cannot take part in such a bond formation.A covalent bond is directional and it is parallel to the region of overlapping atomic orbitals.Based on the pattern of overlapping, there are two types of covalent bonds: sigma bond and a pi bond. The covalent bond formed by sideways overlapping of atomic orbitals is known as pi bond whereas the bond formed by overlapping of atomic orbital along the inter nucleus axis is known as a sigma bond.
Limitations of Valence Bond Theory
The theories and laws that came before this also had certain limitations on them resulting in their failure. However, the theory is also not perfect and does have its shortcomings. The Limitations of Valence Bond Theory are:
It fails to explain the tetravalency of carbon.This theory does not discuss the energies of electrons.The assumptions about the electrons being localized to specific locations.
To follow more on this, Check Valence Bond Theory in Coordination Compound.
Practise This Question
Which of the following represents s - s, s - p and p - p overlap respectively?

I, II, III
III, II, I
I, III, II
II, III, I
Submit
CHEMISTRY Related Links100 Examples Of Chemical EquationsProperties MagnesiumWhat Is Iron Used ForWhat Are IsotopesAtomic ConfigurationRutherford TheoryReactivity Series Of ElementsDefine ElectronegativityHow Many States Of Matter Are ThereChromium Uses
NCERT Related ArticlesNCERT Solutions Maths Class 8NCERT Ebook PdfPhysics Class 10 NCERT SolutionsNCERT Solutions Science Class 9NCERT 10 MathsNCERT Solutions For Class 7NCERT Class 9ThNCERT App Free DownloadNCERT Books Of Class 6Exemplar NCERT
Practise This Question
Which of the following compounds does not have molecular plane as nodal plane for its π - electron cloud?
CH2 = CH2
C6H6
CH2 = C = CH2
All of the above
Submit


Join BYJU'S Chemistry Learning Program
Submit
COURSESCBSEICSECATIASJEENEETGREGMATCommerce
EXAMSCAT ExamIAS ExamUPSC SyllabusUPSC 2018
RESOURCESBlogVideosCBSE Sample PapersCBSE Question Papers
EXAM PREPARATIONFree CAT PrepFree IAS PrepFree GRE PrepFree GMAT PrepMathsPhysicsChemistryBiology
COMPANYAbout UsContact UsInvestorsCareersBYJU'S in MediaStudents Stories - The Learning TreeFaces of BYJU'S Life at BYJU'S
FOLLOW US
Free ResourcesNCERT SolutionsNCERT Solutions for Class 6NCERT Solutions for Class 7NCERT Solutions for Class 8NCERT Solutions for Class 9NCERT Solutions for Class 10NCERT Solutions for Class 11NCERT Solutions for Class 12RD Sharma SolutionsRS Aggarwal Solutions
Disclaimer | Privacy Policy | Terms of Services | Sitemap
© 2019, BYJU'S. All rights reserved.
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