Chemical Bonding NEET Previous Year Questions (PYQ): PDF Download

Download Chemical Bonding NEET PYQs PDF

Access the Chemical Bonding NEET previous year questions PDF from the table below to strengthen your preparation with real exam-level questions. These PYQs with solutions will help you revise key concepts, practise important questions, and improve your accuracy for NEET 2026.

Important Chemical Bonding Questions for NEET 2026

Some of the most important questions from Chemical bonding based on concepts that are frequently asked in the NEET Exam are given below. These questions help students to score better in the Chemistry section of NEET.

Question 1: Given below are two statements:

Statement I : A hypothetical diatomic molecule with bond order zero is quite stable. Statement II : As bond order increases, the bond length increases.

In the light of the above statements, choose the most appropriate answer from the options given below :

(1) Statement 1 is false but Statement II is true

(2) Both Statement I and Statement II are true

(3) Both Statement I and Statement II are false

(4) Statement 1 is true but Statement II is false

Solution:

A bond order of zero means no net bonding between the atoms, indicating the molecule cannot exist or is highly unstable. so the first statement is false

As bond order increases, bond length decreases because stronger bonding pulls the atoms closer together. and also the second statement is false

So the correct answer is (3) Both Statement I and Statement II are false

Hence, the correct answer is option (3).

Question 2: Which of the following molecules cannot be explained by valence bond theory?

(1) $\mathrm{H}_2$

(2) $\mathrm{Cl}_2$

(3) $\mathrm{CO}_2$

(4) $\mathrm{O}_3$

Solution:

$\mathrm{O}_3$ is a molecule with a trigonal planar structure. Valence bond theory cannot explain the structure of $\mathrm{O}_3$ because it assumes that electrons are localized in atomic orbitals. However, the electrons in $\mathrm{O}_3$ are delocalized over three different atomic orbitals, which is why the molecule has a trigonal planar structure.

Hence, the answer is the option (4).

Question 3: Which of the following is the most important factor in determining the most appropriate resonance structure?

(1) The formal charges on the atoms in the molecule.

(2) The number of unpaired and paired electrons in the molecule.

(3) The energy of the contributing structures.

(4) The relative position of the atoms in the molecule.

Solution:

The formal charges on the atoms in the molecule are the most important factor in determining the most appropriate resonance structure.

Hence, the answer is the option (1).

Question 4: Which of the following statements is correct about hybrid orbitals?

(1) Hybrid orbitals are always stronger than non-hybrid orbitals.

(2) Hybrid orbitals always form sigma bonds.

(3) Hybridization increases the stability and decreases the reactivity of a molecule.

(4) All of the above.

Solution:

Hybrid orbitals are always stronger than non-hybrid orbitals, they always form sigma bonds, and they increase the stability and decrease the reactivity of a molecule.

Hence, the answer is the option (4).

Question 5: Which of the following statements is NOT correct about valence bond theory?

(1) Valence bond theory assumes that electrons are delocalized in atomic orbitals.

(2) Valence bond theory can be used to explain the formation of both ionic and covalent bonds.

(3) Valence bond theory can be used to predict the shape of molecules.

(4) Valence bond theory can be used to explain the magnetic properties of molecules.

Solution:

Valence bond theory does not assume that electrons are delocalized in atomic orbitals. Instead, it assumes that electrons can be localised over multiple atomic orbitals.

Hence, the answer is the option (1).

Important Concepts of Chemical Bonding for NEET

This section covers the key concepts of Chemical Bonding for NEET, including VSEPR theory, hybridisation, bond order, molecular orbital theory, and polarity, which are essential for scoring well in the exam.

Lewis Structures

• Lewis structures show bonding in molecules and ions using dots to represent electrons.

• They are based on the octet rule and shared pairs of electrons.

• Valence electrons are the electrons present in the outermost shell of an atom.

• Example: Sodium (Na) has a configuration 2, 8, 1, so it has 1 valence electron.

• In representative elements, the group number = number of valence electrons.

• Lewis symbols represent atoms with dots around the element symbol.

• The number of dots equals the number of valence electrons.

• Both paired and unpaired electrons can be shown in Lewis structures.

Resonance Structures

Resonance is a concept wherein, whenever a single Lewis structure cannot describe the structure of a molecule, then various possible canonical structures are used to accurately describe the molecule, which are called Resonance Structures.

Polarity of Bonds

In heteronuclear bonds, the shared electron pair shifts towards the more electronegative atom, resulting in polarity between the atoms, and the molecule is said to be a polar molecule.

Due to polarity, the molecule develops a Dipole Moment, which is defined as the product of charge and distance of separation between the two bonded atoms.

Fazan’s Rule and Covalent Character in Ionic Bond

The covalent character in ionic bonds is determined by Fajan’s Rule. It simply says that no ionic bond is completely ionic, there is always some covalent character in ionic bond. When a cation approaches an anion, then the electron cloud of the anion is distorted and shifted towards the cation, this distortion is known as the polarisation of the anion.

VSEPR Theory

The VSEPR Theory predicts the shape of the covalent molecules.

Below are the postulates of this theory:

1. The number of valence shell electron pairs decides the shape of a molecule around the central atom.

2. Pairs of electrons in the valence shell repel one another because of the negatively charged electron clouds.

3. The pairs of electrons occupy such positions in space where there is minimum repulsion so it maximises the distance between them.

4. The valence shell is assumed as a sphere with the electron pairs present on the spherical surface at a maximum distance from one another.

5. Multiple bonds are considered as a single electron pair and the two/three electron pairs of multiple bonds are taken as a single super pair.

6. When two or more resonance structures represent a molecule, the VSEPR theory is applied to any such structure.

Valence Bond Theory

When two atoms approach each other, at a large distance there is no force; however, as the molecule starts approaching closer, they experience a force of attraction, and after a certain distance, when the two atoms come close enough, they experience a repulsive force.

So, when two atoms approach each other and form a bond, energy is released, and this energy is called bond enthalpy.

Orbital Overlap Concept

Two hydrogen atoms come close enough that their atomic orbitals partially merge during the formation of a hydrogen molecule. This process is known as orbital overlapping. This allows the electrons from each atom to pair up with opposite spins, resulting in the formation of a covalent bond. The strength of this bond depends on the extent of overlap — the greater the overlap, the stronger the bond.

Directional Properties of Bonds

Covalent bonds are formed through the overlap of atomic orbitals, as we have seen in the hydrogen molecule, where two hydrogen atoms bond by overlapping their 1s orbitals. In polyatomic molecules like $\mathrm{CH}_4, \mathrm{NH}_3$, and $\mathrm{H}_2 \mathrm{O}$, understanding the molecular shape becomes equally important. For example, why does methane ($\mathrm{CH}_4$) adopt a tetrahedral structure, and why does ammonia (NH3) have a pyramidal shape? These questions are explained by Valence Bond Theory. VBT describes how atomic orbitals not only overlap but also undergo hybridisation.

Overlapping of Atomic Orbitals

When two atomic orbitals come close to form a bond, the nature of their overlap depends on the phase (sign) and spatial orientation of their wave functions, whether it is positive, negative, or zero. To form an effective bond, the orbitals must have the same phase and be properly aligned in space.

Hybridization

The features of hybridisation are:

1. The number of hybrid orbitals is equal to the number of atomic orbitals that hybridize.

2. The hybridized orbitals are always the same in energy and shape.

3. The hybrid orbitals form more stable bonds than pure atomic orbitals.

4. The hybrid orbitals are directed in a minimum repulsion space, giving a stable arrangement.

Molecular Orbital Theory

• In molecules, electrons are present in molecular orbitals (MOs), similar to atomic orbitals in atoms.

• Molecular orbitals are formed by the combination of atomic orbitals with similar energy and proper symmetry.

• Atomic orbitals are monocentric (influenced by one nucleus), while molecular orbitals are polycentric (influenced by multiple nuclei).

• When two atomic orbitals combine, they form:

• Bonding orbital (lower energy, more stable)

• Antibonding orbital (higher energy, less stable)

• The number of molecular orbitals = number of atomic orbitals combined.

• Electrons fill molecular orbitals according to Aufbau principle, Pauli exclusion principle, and Hund’s rule.

• Molecular orbitals are formed using LCAO (Linear Combination of Atomic Orbitals) for effective overlap.

Hydrogen Bonding

Hydrogen bonds are strong forces which occur when a hydrogen atom bonded to an electronegative atom approaches a nearby electronegative atom, such as O, N, F, etc. A greater electronegativity of the atom will result in an increase in hydrogen-bond strength. The hydrogen bond is a stronger intermolecular force, but it is weaker than a covalent or an ionic bond. Hydrogen Bonding is responsible for holding together DNA, proteins, and other macromolecules.

Formation of Hydrogen Bond

A hydrogen bond is an electromagnetic attraction that occurs between a partially positively charged hydrogen atom attached to a highly electronegative atom and another nearby electronegative atom. A hydrogen bond is a type of dipole-dipole interaction; it is not a true chemical bond. This hydrogen bond attraction can occur between different molecules (intermolecularly) or within different parts of a single molecule (intramolecularly).

Most Repeated Chemical Bonding Topics Asked in NEET

Refer to the topics given below that are asked most repeatedly in the NEET exam. Many NEET chemistry important questions are based on these topics. Prepare these topics effectively to score good marks:

• Bond order Calculation

• Shape of molecules using VSEPR theory

• Hybridisation of central atom

• Polarity of molecules

• Magnetic nature

Year-wise Number of Questions Asked from Chemical Bonding in NEET

The table given below provides data on the number of questions asked on Chemical Bonding in NEET.

Best Strategy to Prepare for Chemical Bonding for NEET

Refer to the points given below to prepare for Chemical Bonding and molecular structure effectively:

• Read the NCERT thoroughly

• Solve NEET previous year questions from chemical bonding and molecular structure

• Understand basic concepts

• Focus more on topics like shapes, NEET chemistry formulas, and exceptions

• Solve mock tests and NEET previous year questions