The chapter chemical bonding deals with the study of attraction between two or more atoms is called chemical bond. The chapter contains important topics like Lewis Theory, Kossel’s theory, Hydrogen Bonding, etc. The average weightage of this chapter in NEET is 12.50%.
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The formation of chemical bonds were successfully explained by Albrecht kossel and Gilbert lewis in the year of 1916.Both of them explained the basis of the inertness of noble gases in chemical bonding.
Lewis symbols for lithium (1 electron), oxygen (6 electrons), neon (8 electrons)
The stability of the resulting compound in the chemical bonding is gauged by the substances and yield compounds that present in that chemical bonding.Due to strength and properties Chemical bonds vary from its type.There are four types of chemical bonds which are formed by atoms and molecules to yield compounds.
There are three types of chemical bonding which are listed below.
Each and every bonding has its own structure here we attach the structure of the bonding.
The transfer of electrons from one atom or molecules to another is a type of chemical bonding that is called Ionic bonding.In this form atom loses an electron which is in turn gained by another atom.The atom develops a negative charge when an electron transfer takes place and this is called anion,and the remaining atom develops a positive charge and that is called the cation.this difference in charge between the two atoms gives the strength to the ionic bond.
If an atom shares its electron to another atom that indicates a covalent bond. When a compound contains its carbon that exhibits this type of chemical bonding.When an atom shares its pair of electrons around the nuclei of atom that leads to the creation of a molecule.
Pink color indicates electron from Hydrogen
Violet color indicates electron from carbon
In nature covalent bonds can either be polar or nonpolar.the more electrons are shared unequally in the covalent chemical bonding and the more electronegative atom pulls the electron pair towards itself and aways from the less electronegative atom. Example for polar covalent bonding is water.
Due to the uneven spacing of the electrons between the atoms there is a difference in charge that arises in different areas of the atom.Both end of the molecule tends to be different one end will be positively charged and another end will be negatively charged.
Comparatively Hydrogen bonding is the weaker form of chemical bonding then ionic and covalent bonding.Where in the hydrogen develops a particle positive charge when the polar covalent bonding between oxygen and hydrogen.This indicates that the electrons attract closer to the more electronegative oxygen atom.this bond gives the tendency for the hydrogen to be pulled towards the negative charges of any neighbouring atom.Hydrogen bond is responsible for the properties of exhibited by water.
By Hess law,
Ionic | covalent |
low positive charge | high positive charge |
large cation | small cation |
small anion | large anion |
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Correct Answer: b
Solution
[b] BF3:|planar(sp2),|120 degree| bond angle (maximum),Higher the electronegativity of central atom (in sp3| hybridized) larger the bond angle but presence of lone pair of electrons decreases the bond angle. Greater the no. of lone pair of electrons, lower the bond angle.
Correct Answer:B
Solution
Correct Answer:B
Solution:
Correct Answer: A
Solution:
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