Solid State NEET Questions: Important Solid State Questions For NEET 2025

Solid State NEET Questions: Solid State as a subject of Chemistry is one of the most recognized segments of the NEET syllabus, dealing with properties and solid structure. The subject matter includes crystal lattices, unit cells, nature of solids (ionic, molecular, covalent, metallic), and crystal defects. It also deals with key concepts such as packing efficiency, calculation of density, and electrical conductance of solids. Solid State is the building block of subject matter such as material science and chemical bonding.

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1. Analysis of Previous Year NEET Questions
2. NEET Chapter-Wise Question Breakdown – Detailed Analysis & Weightage
3. Solid State previous year questions in NEET Exam

LiveNEET UG Admit Card 2025 (OUT) LIVE: NTA hall ticket at neet.nta.nic.in; qualifying marks, PYQMay 1, 2025 | 4:23 PM IST

The NTA has revised the tie-breaking procedure for NEET UG 2025. In case two or more candidates secure the same marks or percentile scores, the tie will be resolved in the following order:

• Higher marks/percentile in biology (botany and zoology)
• Higher marks/percentile in chemistry
• Higher marks/percentile in physics
• Fewer incorrect answers across all subjects
• Fewer incorrect answers in biology
• Fewer incorrect answers in chemistry
• Fewer incorrect answers in physics

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This chapter is important for NEET students as it has application-based questions that check concept and problem-solving ability. The practice of Solid State not only enhances Chemistry's scoring but also gives a good base of Physical Chemistry and inorganic compound subjects. Practising the numerical and theoretical concepts of this chapter daily can improve the performance of the NEET exam.

Analysis of Previous Year NEET Questions

Analyzing the previous year’s questions for NEET is very important for identifying exam trends, important topics, and question patterns. Understanding the frequency of questions, chapter-wise distribution, and difficulty levels of the past questions can provide a clear insight for focused preparation.

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NEET Solid State Chapter-Wise Question Distribution (2020-2024)

NEET Chapter-Wise Question Breakdown – Detailed Analysis & Weightage

While preparing for NEET, it becomes important to understand the chapter-wise question distribution as it significantly improves your preparation. Here, we have provided a detailed breakdown of NEET questions from Solid State to give you clear insights into your preparation strategy.

Important topics:

Types of solids, packing efficiency, voids, crystal lattices and unit cells, point defects (Schottky & Frenkel), electrical & magnetic properties, and semiconductors.

Solid State previous year questions in NEET Exam

1. Calculate the density of a solid if the atomic solid is crystallised in body centered cubic lattice, the inner surface of the atom at adjacent corners are separated by 60.3 pm, and the atomic mass of A is.

Option 1) 1.86

Option 2) 1.9

Option 3) 1.3

Option 4) 2.4

Solution -

Hence, the answer is option (2).

2. Calculate the number of unit cells in the atom that lies on the surface of a cubic crystal that is 2.0 cm in length.

Option 1) $0.18\times {10}^{-3}$

Option 2) $1.24\times {10}^{-2}$

Option 3) $1.84\times {10}^{-1}$

Option 4) $0.86\times {10}^{-2}$

Solution - $\begin{array}{rl}\mathrm{AC}:\therefore 4R& =\sqrt{3a}\\ a& =22.17\mathrm{pm}=10.9\times {10}^{-3}{\mathrm{m}}^3\\ (2.0\mathrm{cm}{)}^3=& {\left({20}^{-2}\right)}^3={20}^{-6}{\mathrm{m}}^3\\ \text{ No. of unit cell }& =\frac{{20}^{-6}{\mathrm{m}}^3}{10.9\times {10}^{-3}{\mathrm{m}}^3}\\ & =0.18\times {10}^{-3}\end{array}$

Hence, the answer is option (1).

3. Ammonium chloride crystallizes in a body-centred cubic lattice with an edge length of a unit cell of 480 pm. If the size of the chloride ion is 240 pm, the size of the ammonium ion would be

Option 1) 180.6

Option 2) 182.4

Option 3) 175.2

Option 4) 166.9

Solution -

$\begin{array}{rl}& \frac{\sqrt{3}a}{2}=r^{+}+r^{-}\\ & \frac{\sqrt{3}\times 480}{2}-r^{+}+240\\ & 415.2-240=r^{+}\\ & 175.2=r^{+}\end{array}$

Hence, the answer is option (3).

4. Which of the following statements is not true for the crystal structure of cesium chloride (CsCl)?

Option 1) CsCl has a cubic structure.

Option 2) Cs+ and Cl- ions are arranged in a face-centred cubic lattice.

Option 3) Cs+ and Cl- ions have a coordination number of 8 and 6, respectively.

Option 4) The Cs+ ions are located at the corners of the cube and Cl- ions are at the center of the cube.

Solution - $CsCl$ is an example of a simple cubic crystal lattice, not a face-centred cubic lattice as stated in option
2. In a simple cubic lattice, the unit cell consists of a cube with lattice points located at the corners of the cube. Each lattice point represents one ${\mathrm{Cs}}^{+}$ion. Additionally, there is one ${\mathrm{Cl}}^{-}$ion located at the centre of the cube.

In CsCl , each ${\mathrm{Cs}}^{+}$ion is surrounded by $8{\mathrm{Cl}}^{-}$ions arranged at the corners of a cube around it, resulting in a coordination number of 8 for the ${\mathrm{Cs}}^{+}$ion. On the other hand, each ${\mathrm{Cl}}^{-}$ion is surrounded by $6{\mathrm{Cs}}^{+}$ions arranged at the corners of an octahedron around it, resulting in a coordination number of 6 for the ${\mathrm{Cl}}^{-}$ion. This is stated in option 3 .

Therefore, the correct statement regarding the location of ${\mathrm{Cs}}^{+}$and ${\mathrm{Cl}}^{-}$ions in the CsCl crystal structure is that ${\mathrm{Cs}}^{+}$ions are located at the corners of the cube and ${\mathrm{Cl}}^{-}$ions are located at the centre of the cube.

Option 4) incorrectly describes the location of the ${\mathrm{Cl}}^{-}$ion in the CsCl unit cell.

Hence, the answer is option (4).

5. Which of the following ionic solids has the highest packing efficiency?

Option 1) NaCl

Option 2) CsCl

Option 3) ZnS

Option 4) $Ca{F}_2$

Solution - The correct answer is an option (c) $ZnS$,also known as zinc sulfide, has the highest packing efficiency among the given options. ZnS has a zincblende structure, which has a cubic close-packed (CCP) arrangement of both cations $\left(Z{n}^{2+}\right)$ and anions $\left(S^{2-}\right)\text{in which they occupy alternate positions. This }$ arrangement results in the highest packing efficiency of approximately $74\mathrm{\%}$, which is the maximum possible packing efficiency for ionic solids. NaCl (sodium chloride), ${\mathrm{CsCl}}^{\prime }$ (cesium chloride), and ${\mathrm{CaF}}_{2\text{ (calcium fluoride) have }}$ different crystal structures with lower packing efficiencies compared to $ZnS$. Hence, the correct answer is option (c) $ZnS$.

Hence, the answer is the option (3).

6. A crystal has a face-centered cubic (FCC) structure with an edge length of $4/AA$. The radius of the atoms in the crystal is $1/AA$. What is the packing efficiency of the FCC structure?

Option 1) 33.3%

Option 2) 48.6%

Option 3) 52.4%

Option 4) 74.0%

Solution - The packing efficiency of a face-centered cubic (FCC) structure is 74%. This is a characteristic property of FCC structures, where atoms are arranged in a closely packed manner with atoms located at the corners and the center of each face of the unit cell.

Hence, the answer is the option (4).

7. Assertion: The body-centred cubic lattice has a higher packing efficiency than the simple cubic lattice.

Reasoning: In the body-centred cubic lattice, the atoms are located at the corners and at the centre of the unit cell, which allows for a more efficient packing than the simple cubic lattice.

Option 1) Both assertion and reasoning are true, and the reasoning is the correct explanation of the assertion.

Option 2) Both assertion and reasoning are true, but the reasoning is not the correct explanation of the assertion.

Option 3) The assertion is true, but the reasoning is false.

Option 4) Both assertion and reasoning are false.

Solution - The assertion that the body-centred cubic lattice has a higher packing efficiency than the simple cubic lattice is true. In the body-centred cubic lattice, the constituent particles are located at the corners and the centre of the unit cell. This allows for a more efficient packing than the simple cubic lattice, where the particles are located only at the corners of the unit cell.

The reasoning that the atoms are located at the corners and the centre of the unit cell in the body-centred cubic lattice, allowing for a more efficient packing than the simple cubic lattice, is also correct. The body-centred cubic lattice has a packing efficiency of 68%, while the simple cubic lattice has a packing efficiency of only 52%.

Therefore, both the assertion and reasoning are true, and the reasoning correctly explains the assertion.

Hence, the answer is option (1).

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