
In the sigma bond
A. Sidewise, as well as end-to-end overlapping of orbitals take place
B. Sidewise overlap of orbitals takes place
C. End-to-end overlap of orbitals takes place
D. None of the above
Answer
163.5k+ views
Hint: The overlap of orbitals is essential for the formation of covalent chemical bonds. It is defined as the combining of orbitals of adjacent atoms in the same parts of an area or space. This combination leads to the formation of a hybridised orbital.
Complete Step by Step Answer:
Partial linking or interpenetration of atomic orbitals is defined as overlapping due to which the pairing of electrons happens.
When two atoms become near to each other, the merging of orbitals to form a hybridized orbital encloses the bonding pair of electrons.
This stability of the hybridized orbital is due to its lower energy than the atomic orbital.
The magnitude of overlap decides the strength of a covalent bond.
Greater overlapping ensures higher stability of the covalent bond.
The covalent bond is categorised into two types relying on the overlap of orbitals.
Sigma bond
This is created by the end-to-end or head-on overlapping of bonding orbitals along the internuclear axis.
This is also known as head-on overlap or axial overlap.
In this case, a higher degree of overlapping happens.
So, it is a stronger bond than a pi-bond.
In the pi bond, the atomic orbitals coincide and their axes stay parallel to each other and perpendicular to the internuclear axis.
The orbitals constituted by side-wise overlapping have two saucer-type charge clouds above and below the plane of the bonded atoms.
Here we have been asked in the sigma bond which type of overlapping happens.
In a sigma bond, end-to-end overlapping happens.
So, option C is correct.
Note: Covalent bond is a chemical bond constituted by the sharing of electron pairs between atoms. These electron pairs are named shared pairs or bonding pairs. We know that single bonds comprise one sigma bond. Double bonds comprise one sigma and one pi-bond, and triple bonds have one sigma and two pi-bonds. Double bonds are less stable than a single bond due to their greater reactivity. This is because double bonds are electron rich and the weak pi-bond can be shared by another electron acceptor like halogens.
Complete Step by Step Answer:
Partial linking or interpenetration of atomic orbitals is defined as overlapping due to which the pairing of electrons happens.
When two atoms become near to each other, the merging of orbitals to form a hybridized orbital encloses the bonding pair of electrons.
This stability of the hybridized orbital is due to its lower energy than the atomic orbital.
The magnitude of overlap decides the strength of a covalent bond.
Greater overlapping ensures higher stability of the covalent bond.
The covalent bond is categorised into two types relying on the overlap of orbitals.
Sigma bond
This is created by the end-to-end or head-on overlapping of bonding orbitals along the internuclear axis.
This is also known as head-on overlap or axial overlap.
In this case, a higher degree of overlapping happens.
So, it is a stronger bond than a pi-bond.
In the pi bond, the atomic orbitals coincide and their axes stay parallel to each other and perpendicular to the internuclear axis.
The orbitals constituted by side-wise overlapping have two saucer-type charge clouds above and below the plane of the bonded atoms.
Here we have been asked in the sigma bond which type of overlapping happens.
In a sigma bond, end-to-end overlapping happens.
So, option C is correct.
Note: Covalent bond is a chemical bond constituted by the sharing of electron pairs between atoms. These electron pairs are named shared pairs or bonding pairs. We know that single bonds comprise one sigma bond. Double bonds comprise one sigma and one pi-bond, and triple bonds have one sigma and two pi-bonds. Double bonds are less stable than a single bond due to their greater reactivity. This is because double bonds are electron rich and the weak pi-bond can be shared by another electron acceptor like halogens.
Recently Updated Pages
JEE Main 2021 July 25 Shift 1 Question Paper with Answer Key

JEE Main 2021 July 22 Shift 2 Question Paper with Answer Key

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

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

Atomic Structure - Electrons, Protons, Neutrons and Atomic Models

Displacement-Time Graph and Velocity-Time Graph for JEE

JEE Main 2025: Derivation of Equation of Trajectory in Physics

Learn About Angle Of Deviation In Prism: JEE Main Physics 2025

Types of Solutions

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

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

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

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

Degree of Dissociation and Its Formula With Solved Example for JEE

NCERT Solutions for Class 11 Chemistry Chapter 7 Redox Reaction
