
Which of the following species are hypervalent?
1. \[Cl{O_4}^ - \] 2. \[B{F_3}\] 3. \[S{O_4}^{2 - }\] 4. \[C{O_3}^{2 - }\]
A. 1, 2, 3
B. 1, 3
C. 3, 4
D. 1, 2
Answer
154.5k+ views
Hint: A hypervalent molecule or a hypervalent species is a compound in which the given molecule contains one or more main group elements, and have more than eight electrons in their valence shell. This phenomenon is also commonly known as ‘expanded octet’.
Complete Step-by-Step answer:
To determine which of the given molecules are hypervalent, let us first understand the molecular structures of these compounds:
\[Cl{O_4}^ - \]

As we can observe in this structure, chlorine is forming 6 double bonds and 1 single bond. This brings the total number of electrons present in the valence shell of chlorine to be:
\[ = {\text{ }}6{\text{ }}\left( 4 \right){\text{ }} + {\text{ }}1{\text{ }}\left( 2 \right){\text{ }} = {\text{ }}12\] electrons
Hence, the given species is hypervalent
\[B{F_3}\]

As we can observe in this structure, boron is forming 3 single bonds. This brings the total number of atoms present in the valence shell of boron to be:
\[ = {\text{ }}3\left( 2 \right){\text{ }} = {\text{ }}6\] electrons
Hence, the given species is not hypervalent
\[Cl{O_4}^ - \]

As we can observe in this structure, sulphur is forming 2 double bonds and 2 single bonds. This brings the total number of electrons present in the valence shell of sulphur to be:
\[ = {\text{ }}2{\text{ }}\left( 4 \right){\text{ }} + {\text{ }}2{\text{ }}\left( 2 \right){\text{ }} = {\text{ }}10\] electrons
Hence, the given species is hypervalent
\[C{O_3}^{2 - }\]

As we can observe in this structure, carbon is forming 2 single bonds and 1 double bond. This brings the total number of atoms present in the valence shell of carbon to be:
\[ = {\text{ }}2\left( 2 \right){\text{ }} + {\text{ }}1\left( 4 \right){\text{ }} = {\text{ }}8\] electrons
Hence, the given species is not hypervalent
Hence, we can conclude that, the species that are hypervalent are \[Cl{O_4}^ - \] and \[Cl{O_4}^ - \]
Hence, Option B is the correct option.
Note: Early considerations of the geometry of hypervalent molecules returned familiar arrangements that were well explained by the VSEPR model for atomic bonding. In order to account for the observed bond angles, bond lengths and apparent violation of the Lewis octet rule, several alternative models have been proposed.
Complete Step-by-Step answer:
To determine which of the given molecules are hypervalent, let us first understand the molecular structures of these compounds:
\[Cl{O_4}^ - \]

As we can observe in this structure, chlorine is forming 6 double bonds and 1 single bond. This brings the total number of electrons present in the valence shell of chlorine to be:
\[ = {\text{ }}6{\text{ }}\left( 4 \right){\text{ }} + {\text{ }}1{\text{ }}\left( 2 \right){\text{ }} = {\text{ }}12\] electrons
Hence, the given species is hypervalent
\[B{F_3}\]

As we can observe in this structure, boron is forming 3 single bonds. This brings the total number of atoms present in the valence shell of boron to be:
\[ = {\text{ }}3\left( 2 \right){\text{ }} = {\text{ }}6\] electrons
Hence, the given species is not hypervalent
\[Cl{O_4}^ - \]

As we can observe in this structure, sulphur is forming 2 double bonds and 2 single bonds. This brings the total number of electrons present in the valence shell of sulphur to be:
\[ = {\text{ }}2{\text{ }}\left( 4 \right){\text{ }} + {\text{ }}2{\text{ }}\left( 2 \right){\text{ }} = {\text{ }}10\] electrons
Hence, the given species is hypervalent
\[C{O_3}^{2 - }\]

As we can observe in this structure, carbon is forming 2 single bonds and 1 double bond. This brings the total number of atoms present in the valence shell of carbon to be:
\[ = {\text{ }}2\left( 2 \right){\text{ }} + {\text{ }}1\left( 4 \right){\text{ }} = {\text{ }}8\] electrons
Hence, the given species is not hypervalent
Hence, we can conclude that, the species that are hypervalent are \[Cl{O_4}^ - \] and \[Cl{O_4}^ - \]
Hence, Option B is the correct option.
Note: Early considerations of the geometry of hypervalent molecules returned familiar arrangements that were well explained by the VSEPR model for atomic bonding. In order to account for the observed bond angles, bond lengths and apparent violation of the Lewis octet rule, several alternative models have been proposed.
Recently Updated Pages
JEE Atomic Structure and Chemical Bonding important Concepts and Tips

JEE Amino Acids and Peptides Important Concepts and Tips for Exam Preparation

JEE Electricity and Magnetism Important Concepts and Tips for Exam Preparation

Chemical Properties of Hydrogen - Important Concepts for JEE Exam Preparation

JEE Energetics Important Concepts and Tips for Exam Preparation

JEE Isolation, Preparation and Properties of Non-metals Important Concepts and Tips for Exam Preparation

Trending doubts
JEE Main 2025 Session 2: Application Form (Out), Exam Dates (Released), Eligibility, & More

JEE Main 2025: Derivation of Equation of Trajectory in Physics

Electric Field Due to Uniformly Charged Ring for JEE Main 2025 - Formula and Derivation

NH4NO3 and NH4NO2 on heating decomposes in to A NO2 class 11 chemistry JEE_Main

Degree of Dissociation and Its Formula With Solved Example for JEE

Displacement-Time Graph and Velocity-Time Graph for JEE

Other Pages
JEE Advanced Marks vs Ranks 2025: Understanding Category-wise Qualifying Marks and Previous Year Cut-offs

JEE Advanced 2025: Dates, Registration, Syllabus, Eligibility Criteria and More

JEE Advanced Weightage 2025 Chapter-Wise for Physics, Maths and Chemistry

NCERT Solutions for Class 11 Chemistry In Hindi Chapter 1 Some Basic Concepts of Chemistry

JEE Advanced 2025 Notes

Electrical Field of Charged Spherical Shell - JEE
