Solid State MCQ For NEET | Pdf
Struggling with Solid State MCQ for NEET? You’re not alone! This chapter is a high-weightage topic in NEET Chemistry, covering unit cells, crystal lattices, packing efficiency, and defects. Our free Solid State MCQ for NEET PDF download gives you 100+ practice questions with detailed answers—perfect for quick revision.
These MCQs are curated by experts to match the latest NEET syllabus, focusing on frequently asked concepts like FCC/BCC structures, Schottky defects, and Bragg’s Law. Whether you’re targeting NEET 2026 or need last-minute practice, this PDF helps you identify weak areas, avoid common traps, and build speed. Answers include clear explanations to solidify concepts, not just rote learning. Best of all? Ace your exam with confidence!
Solid State MCQ For NEET | Pdf
Solid state is a very important chapter for NEET Aspirants. NEET exam is important in your life, because your future career depends upon your score in NEET exam Solid State MCQ for NEET test your knowledge, intelligence, memory and quick response. Your speed and accuracy is the essence of this NEET MCQ. For this you have to cultivate a different frame of mind. For this first solve the different Solid State MCQ for NEET given in this page and then try to complete each Chapter of chemistry NEET MCQs given on ybstudy.com.
With Our solid state MCQ for NEET Find out where you stand, your strong points and weak points and try to take corrective steps immediately. In this process your subconscious mind will be thinking about the correct answers of solid state mcq for those questions and in the second round, you will be getting most of the answers. Remember before starting to solve Solid State MCQ for NEET online test all the important notes and the meaning of all definitions should be understood.
1. Solids are characterised by their properties……
(1) incompressibility
(2) crystalline nature
(3) mechanical strength
(4) all of the above
Answer: (4) all of the above
Explanation: Solids exhibit incompressibility because of closely packed particles, crystalline nature due to ordered particle arrangement, and mechanical strength due to strong intermolecular or atomic bonding. Hence, all these properties are correct.
Chapter 2: Solutions
2. Which of the following solids is soft
(1) Fe
(2) diamond
(3) Na
(4) SiO₂
Answer: (3) Na
Explanation: Sodium (Na), being an alkali metal, has a large atomic size and weak metallic bonds, making it soft and easily cut with a knife. The other options are much harder due to strong bonding.
3. Intermolecular distance in liquid is
(1) more than solids
(2) more than gases
(3) less than solids
(4) equal to gases
Answer: (1) more than solids
Explanation: In liquids, particles are not as closely packed as in solids, so the intermolecular distance is more than in solids but less than in gases.
Chapter 3: Electro chemistry
4. Which among the following solids is not soft?
(1) sodium
(2) potassium
(3) copper
(4) phosphorus
Answer: (3) copper
Explanation: Copper is a transition metal with strong metallic bonds and a dense structure, making it much harder than alkali metals like sodium and potassium or nonmetals like phosphorus.
Chapter 4: Chemical Kinetics
5. Which one of the following is a molecular crystal?
(1) Quartz
(2) Rock salt
(3) Dry ice
(4) Diamond
Answer: (3) Dry ice
Explanation: Dry ice is solid CO₂ and consists of molecules held together by weak van der Waals forces. Quartz and diamond are covalent crystals, while rock salt is ionic.
Chapter 5: Surface Chemistry
6. Which of the following is an amorphous solid?
(1) CaF₂
(2) NaCl
(3) CsCl
(4) glass
Answer: (4) glass
Explanation: Glass lacks a long-range orderly arrangement of atoms, making it an amorphous solid. The other options are all crystalline ionic compounds.
Chapter 6: General Principles and Processes of Isolation of Elements
7. Graphite is not…..
(1) sp hybridised
(2) a good conductor
(3) an amorphous solid
(4) a covalent crystal
Answer: (3) an amorphous solid
Explanation: Graphite has a layered crystalline structure with sp² hybridised carbon atoms. It conducts electricity and is a covalent crystal, not amorphous.
Chapter 7: The p Block Elements
8. Diamond is…..
(1) a conductor
(2) an ionic solid
(3) sp³ hybridized
(4) a lubricant
Answer: (3) sp³ hybridized
Explanation: In diamond, each carbon atom is bonded to four others in a tetrahedral geometry using sp³ hybrid orbitals, forming a very hard covalent crystal structure.
Chapter 8: The d and f Block Elements
9. Which of the following is /are covalent solids?
(1) He
(2) Fe
(3) NaCl
(4) graphite
Answer: (4) graphite
Explanation: Graphite is a covalent solid with carbon atoms bonded in hexagonal sheets. Helium is atomic, Fe is metallic, and NaCl is ionic.
Chapter 9: Coordination Compounds
10. Which is/are not amorphous solid(s)
(1) graphite
(2) plastics
(3) rubber
(4) glass
Answer: (1) graphite
Explanation: Graphite has a well-ordered crystalline structure with layers of carbon atoms, unlike plastics, rubber, and glass which lack long-range order and are amorphous.
Chapter 10: Haloalkanes and Haloarenes
11. Ionic solids are characterised by…..
(1) good conductivity in solid state
(2) high vapour pressure
(3) low melting point
(4) solubility in polar solvents
Answer: (4) solubility in polar solvents
Explanation: Ionic solids are composed of ions held by strong electrostatic forces. They dissolve well in polar solvents like water due to ion-dipole interactions but do not conduct electricity in solid state and have high melting points and low vapour pressures.
Chapter 11: Alcohols Phenols and Ethers
12. Crystals which are good conductor of electricity are known as
(1) ionic crystal
(2) covalent crystals
(3) molecular crystal
(4) metallic crystal
Answer: (4) metallic crystal
Explanation: Metallic crystals have free electrons (delocalised) that move throughout the crystal, making them excellent conductors of electricity, unlike ionic, covalent, or molecular crystals.
Chapter 12: Aldehydes Ketones and Carboxylic Acids
13. Which pairs shows isomorphism
(1) KNO₃, NaNO₃
(2) Cr₂O₃, Fe₂O₃
(3) both (1) and (2)
(4) none of these
Answer: (3) both (1) and (2)
Explanation: Isomorphs are compounds with similar crystal structures and compositions. Both KNO₃ with NaNO₃ and Cr₂O₃ with Fe₂O₃ have similar shapes and lattice structures, hence show isomorphism.
Chapter 13: Amines
14. Which of the following are not isomorphous?
(1) NaNO₃ and CaCO₃
(2) H₂SO₄ and Na₂SO₄
(3) K₂SO₄ and K₂SeO₄
(4) Cr₂O₃ and Fe₂O₃
Answer: (2) H₂SO₄ and Na₂SO₄
Explanation: Isomorphous compounds must be similar in structure and form. H₂SO₄ is a covalent liquid while Na₂SO₄ is an ionic solid, so they cannot be isomorphous.
Chapter 14: Biomolecules
15. Isomorphs have……
(1) same atomic ratio
(2) similar molecular formulae
(3) similar chemical properties
(4) all (1), (2) and (3)
Answer: (4) all (1), (2) and (3)
Explanation: Isomorphs have same atomic ratio, similar molecular formulae, and tend to have similar chemical and physical properties due to similar crystalline structures.
Chapter 15: Polymers
16. Different crystalline forms of same substance are called…
(1) isomorphs
(2) isotopes
(3) polymorphs
(4) isobars
Answer: (3) polymorphs
Explanation: Polymorphs are different crystalline forms of the same compound that exist due to different arrangements of atoms or molecules in the solid state.
Chapter 16: Chemistry in Everyday Life
17. Which of the following exhibit anisotropy…..
(1) NaCl
(2) glass
(3) rubber
(4) butter
Answer: (1) NaCl
Explanation: NaCl is a crystalline solid that shows anisotropy—its properties like refractive index or conductivity vary with direction. Glass, rubber, and butter are isotropic.
18. Glass…..
(1) has sharp melting point
(2) is anisotropic
(3) behaves like fluid
(4) is true solid
Answer: (3) behaves like fluid
Explanation: Glass is an amorphous solid that behaves like a supercooled liquid; it does not have a sharp melting point and lacks a long-range ordered structure.
19. Which of the following is mismatched?
(1) Quartz glass → 100% silica
(2) Pyrex glass → 60–80% silica, 10–25% B₂O₃ and Al₂O₃
(3) Soda lime glass → 80% silica, 20% CaO
(4) Soda lime glass → 75% silica, 15% Na₂O, 10% CaO
Answer: (3) Soda lime glass → 80% silica, 20% CaO
Explanation: The correct composition of soda lime glass is about 75% silica, 15% Na₂O, and 10% CaO. The statement in option (3) is incorrect and mismatched.
20. To impart red colour to glass … is used.
(1) Fe₂O₃
(2) VO₂
(3) CoO
(4) Cu
Answer: (4) Cu
Explanation: Trace amounts of copper (Cu) or gold are used to impart red color to glass due to their ability to absorb specific wavelengths of light, producing a red hue.
21. Intermolecular force of attraction present in polar molecular solids is……
(1) dipole-dipole interaction
(2) dispersion force
(3) hydrogen bonding
(4) polar covalent bond
Answer: (1) dipole-dipole interaction
Explanation: Polar molecular solids consist of molecules having permanent dipoles. The main force of attraction between them is dipole-dipole interaction, which is stronger than dispersion forces but weaker than covalent or ionic bonds.
22. Actual arrangement of ions depends upon all….
(1) sizes of cation and anion
(2) the charges of ions
(3) the ease with which anion can be polarised
(4) weight of iron
Answer: (4) weight of iron
Explanation: The actual arrangement of ions in a crystal depends on factors like size and charge of ions and polarisation ability of anions—not on the weight of iron. Hence, option (4) is incorrect.
23. Ionic solids are………
(1) good conductor of electricity
(2) hard and brittle
(3) malleable and ductile
(4) solids with low melting point
Answer: (2) hard and brittle
Explanation: Ionic solids are hard due to strong electrostatic forces but brittle because distortion of lattice causes repulsion between like charges. They do not conduct electricity in solid state and have high melting points.
24. The force of attraction between positively charged and negatively charged delocalized electrons is called……..
(1) dipole–dipole interaction
(2) ionic bond
(3) covalent bond
(4) metallic bond
Answer: (4) metallic bond
Explanation: In metallic solids, positively charged metal ions are surrounded by a ‘sea’ of delocalized electrons. The electrostatic attraction between them is known as a metallic bond, responsible for metallic properties.
25. Metals…..
(1) can be alloyed
(2) bad conductor of electricity
(3) have lustre
(4) are hard but brittle
Answer: (2) and (4)
Explanation: The statement is mismatched. Metals are actually good conductors of electricity and are usually malleable and ductile, not brittle. Hence, options (2) and (4) are incorrect together.
26. Which of the following is not covalent solid…
(1) Diamond
(2) Silicon carbide
(3) Zinc sulphide
(4) Fullerene
Answer: (3) Zinc sulphide
Explanation: Zinc sulphide is an ionic compound made up of Zn²⁺ and S²⁻ ions. Diamond, silicon carbide, and fullerene are all covalent solids, where atoms are held together by covalent bonds.
27. Diamond is not…..
(1) allotropic form of carbon
(2) good conductor of electricity
(3) giant solid
(4) all of the above
Answer: (2) good conductor of electricity
Explanation: Diamond is an allotrope of carbon and forms a giant covalent structure. However, it does not conduct electricity due to absence of free electrons or ions.
28. Which of the following is wrong about graphite?
(1) all carbon atoms are sp hybridised
(2) good conductor of electricity
(3) it is used as lubricant
(4) C–C bond length is 154 pm
Answer: (4) C–C bond length is 154 pm
Explanation: In graphite, the C–C bond length is about 141.5 pm due to partial double-bond character from delocalized π-electrons. Option (4) gives bond length of diamond, hence it is incorrect.
29. Which of the following is not use as fullerene ?
(1) It is used in superconductor
(2) It is used in nanotubes
(3) It is used in jewellery
(4) It is used in catalyst
Answer: (3) It is used in jewellery
Explanation: Fullerenes are used in applications like superconductors, drug delivery, catalysts, and nanotechnology. They are not used in jewellery, unlike diamond or gold.
30. Red glass contains trace amount of….
(1) Al₂O₃ and Fe₂O₃
(2) zinc and aluminum
(3) boron oxide
(4) gold and copper
Answer: (4) gold and copper
Explanation: Red-colored glass is produced by adding trace amounts of gold or copper, which create colloidal particles that absorb and reflect specific wavelengths of light to give a red appearance.
31. Yellow glass contains…..
(1) CuO
(2) UO₂
(3) CoO
(4) Fe₂O₃
Answer: (2) UO₂
Explanation: Yellow color in glass is typically achieved by adding uranium oxide (UO₂). It gives a fluorescent yellow-green appearance. Other oxides give different colors (e.g., CoO → blue, CuO → green).
32. The inter particle forces in solid hydrogen are…
(1) hydrogen bonds
(2) covalent bonds
(3) coordinate bonds
(4) van der Waals forces
Answer: (4) van der Waals forces
Explanation: In solid hydrogen, weak van der Waals forces exist between H₂ molecules, as there are no hydrogen bonds (no polar H–F, H–O, or H–N) or covalent bonds between molecules.
33. In which of the following substances, the carbon atom is arranged in a regular tetrahedral structure?
(1) benzene
(2) diamond
(3) graphite
(4) carbon black
Answer: (2) diamond
Explanation: In diamond, each carbon atom is sp³ hybridized and forms four sigma bonds arranged in a tetrahedral geometry, giving it extreme hardness and symmetry.
34. K₃C₆₀ is a compound of potassium and fullerene. It is….. at 18 K.
(1) a superconductor of electricity
(2) a conductor of electricity
(3) a semi-conductor
(4) an insulator
Answer: (1) a superconductor of electricity
Explanation: K₃C₆₀ (a potassium-doped fullerene) shows superconducting behavior at low temperatures such as 18 K due to the presence of delocalized electrons and special bonding.
35. The existence of a substance in more than one solid modification is known as…
(1) polymorphism
(2) anisotropy
(3) isomorphism
(4) enantiomorphism
Answer: (1) polymorphism
Explanation: Polymorphism refers to the ability of a solid substance to exist in more than one form or crystal structure, like carbon existing as diamond and graphite.
36. Which of the following is true for diamond?
(1) diamond is a good conductor of electricity
(2) diamond is soft
(3) diamond is a bad conductor of heat
(4) diamond is made up of C, H and O
Answer: (3) diamond is a bad conductor of heat
Explanation: Diamond is an excellent conductor of heat due to its tightly bonded lattice, but it is a poor conductor of electricity because it lacks free electrons.
37. In graphite, carbon atoms are joined together due to……
(1) ionic bonding
(2) metallic bonding
(3) van der Waals forces
(4) covalent bonding
Answer: (4) covalent bonding
Explanation: In graphite, each carbon atom is covalently bonded to three others in a hexagonal layer. These layers are held together by weak van der Waals forces, allowing easy slippage.
38. The number of carbon atoms per unit cell of diamond unit cell is……
(1) 8
(2) 4
(3) 1
(4) 6
Answer: (1) 8
Explanation: The diamond unit cell has a face-centered cubic (FCC) structure with 8 atoms per unit cell: 4 atoms from FCC points and 4 additional atoms inside the cell.
39. A molecule contains atoms X and Y so that X occurs at the corners of the cube while Y at the face centres. The formula of the molecule can be…..
(1) XY₃
(2) X₁Y
(3) X₂Y
(4) XY₂
Answer: (1) XY₃
Explanation: In a cube, atoms at corners contribute 1/8 each × 8 = 1 atom of X; atoms at face centres contribute 1/2 each × 6 = 3 atoms of Y. So, the formula is XY₃.
40. Percentage of free space in body centred cubic unit cell…
(1) 34%
(2) 28%
(3) 30%
(4) 32%
Answer: (4) 32%
Explanation: In a BCC unit cell, packing efficiency is approximately 68%, so the free (empty) space is 100% – 68% = 32%.
41. The packing efficiency of the two-dimensional square unit cell as shown is…..
(1) 68.02%
(2) 78.54%
(3) 39.279%
(4) 74.05%
Answer: (2) 78.54%
Explanation: In a two-dimensional square close packing of circles (as in a hexagonal arrangement), the maximum packing efficiency is π/√12 ≈ 78.54%, which represents the most efficient arrangement in 2D.
42. The number of atoms in a body-centred cubic unit cell of a monatomic elementary substance is equal to……
(1) three
(2) two
(3) one
(4) four
Answer: (2) two
Explanation: A BCC unit cell has one atom at each corner (1/8 × 8 = 1 atom) and one atom at the centre (1 atom). Total atoms = 1 + 1 = 2.
43. An atom at the edge centre of a unit cell makes… contribution to a particular unit cell
(1) 1/4
(2) 1/2
(3) 1/8
(4) 1
Answer: (1) 1/4
Explanation: An edge-centered atom is shared between 4 unit cells, so its contribution to a single unit cell is 1/4.
44. The percentage of the available space occupied in a hexagonal close packing of spheres in three dimensions is…
(1) 26%
(2) 76%
(3) 52%
(4) 74%
Answer: (4) 74%
Explanation: Hexagonal close packing (hcp) has a packing efficiency of 74%, meaning 74% of the space is filled by atoms, and 26% is void.
45. How many kinds of space lattices are possible in a crystal?
(1) 23
(2) 7
(3) 230
(4) 14
Answer: (4) 14
Explanation: There are 14 distinct space lattices known as Bravais lattices, derived from 7 crystal systems with different lattice point arrangements.
46. The crystal system of a compound with unit cell dimensions a = 0.387, b = 0.387, and c = 0.504 nm and α = β = 90°, γ = 120° is…….
(1) Cubic
(2) Hexagonal
(3) Rhombohedral
(4) Orthorhombic
Answer: (2) Hexagonal
Explanation: In the hexagonal system, a = b ≠ c and angles α = β = 90°, γ = 120°, which matches the given dimensions and angles.
47. In a face-centred cubic lattice, a unit cell is shared equally by how many unit cells?
(1) 2
(2) 4
(3) 8
(4) 6
Answer: (4) 6
Explanation: Each face-centred atom lies on one of the six faces of a cube and is shared between 2 adjacent unit cells, hence shared by 6 unit cells.
48. The number of atoms present in FCC unit cell is……..
(1) 1
(2) 2
(3) 3
(4) 4
Answer: (4) 4
Explanation: In an FCC unit cell, there are 8 corner atoms (1/8 × 8 = 1 atom) and 6 face atoms (1/2 × 6 = 3 atoms). Total = 1 + 3 = 4 atoms.
49. Na and Mg crystallize in BCC and FCC-type crystals respectively. The ratio of number of atoms present in the unit cell of respective crystal is……..
(1) 1
(2) 3
(3) 0.5
(4) 4
Answer: (3) 0.5
Explanation: Na (BCC) has 2 atoms/unit cell; Mg (FCC) has 4 atoms/unit cell. Ratio (Na:Mg) = 2:4 = 0.5.
50. TiO₂ is a well-known example of…..
(1) triclinic system
(2) tetragonal system
(3) none of these
(4) monoclinic system
Answer: (2) tetragonal system
Explanation: TiO₂ (Rutile form) crystallizes in the tetragonal system, where two sides are equal (a = b ≠ c) and all angles are 90°.
51. The unit cell with the structure below refers to crystal system…
(1) cubic
(2) orthorhombic
(3) tetragonal
(4) trigonal
Answer: (2) orthorhombic
Explanation: The orthorhombic crystal system has all three axes of different lengths (a ≠ b ≠ c) but all angles are 90°. The structure mentioned fits this description.
52. A metal of density 7.5 × 10³ kg/m³ has an FCC crystal structure with lattice parameter a = 400 pm. Calculate the number of unit cells present in 0.0015 kg of the metal.
(1) 3.125 × 10²³
(2) 1.563 × 10²²
(3) 6.250 × 10²³
(4) 3.125 × 10²²
Answer: (4) 3.125 × 10²²
Explanation: Using density = mass/volume and volume of one FCC unit cell = a³, the number of unit cells = (given mass)/(mass of one unit cell). The correct calculated value is 3.125 × 10²².
53. How many octahedral and tetrahedral holes are per unit cell in a face-centred cubic arrangement of atoms?
(1) 1, 2
(2) 2, 1
(3) 8, 4
(4) 4, 8
Answer: (4) 4, 8
Explanation: In FCC unit cells, the number of octahedral voids per unit cell is equal to the number of atoms (4), and tetrahedral voids are twice that number (8).
54. A compound alloy of gold and Cu crystallises in a cubic lattice in which the gold atoms occupy the lattice points at the corners of a cube and the copper atoms occupy the centres of each of the cube faces. What is the empirical formula of this compound?
(1) AuCu₃
(2) Au₃Cu
(3) Au₂Cu₃
(4) AuCu
Answer: (1) AuCu₃
Explanation: Gold atoms at 8 corners contribute 1 atom (1/8 × 8), and copper atoms on 6 faces contribute 3 atoms (1/2 × 6). The ratio of Au : Cu = 1 : 3 → AuCu₃.
55. Which of the following types of cubic lattice has maximum number of atoms per unit cell?
(1) body-centred cubic
(2) simple cubic
(3) face-centred cubic
(4) all of the above
Answer: (3) face-centred cubic
Explanation: FCC has 4 atoms per unit cell, BCC has 2, and simple cubic has only 1. Therefore, FCC has the maximum atoms per unit cell.
56. A metal crystallises in BCC lattice with the cell edge a = 4.229 Å. What is the radius of the metal atom?
(1) 1.86 Å
(2) 1.90 Å
(3) 18.3 Å
(4) 1.12 Å
Answer: (2) 1.90 Å
Explanation: For BCC, the body diagonal = 4r = √3a → r = (√3 × a)/4. Substituting a = 4.229 Å gives r ≈ 1.90 Å.
57. In the closest packing of atoms…
(1) The size of tetrahedral void is greater than that of octahedral void
(2) The size of tetrahedral void is smaller than that of octahedral void
(3) The size of tetrahedral void is equal to that of octahedral void
(4) The size of tetrahedral void may be greater or smaller or equal to that of octahedral void depending upon the size of atoms
Answer: (2) The size of tetrahedral void is smaller than that of octahedral void
Explanation: Octahedral voids are formed by 6 surrounding atoms while tetrahedral voids are formed by 4 atoms. Thus, octahedral voids are larger.
58. The number of atoms in 100 g of an FCC crystal with density 10.0 g/cm³ and cell edge equal to 200 pm is equal to
(1) 5 × 10⁴
(2) 6 × 10³
(3) 5 × 10²⁵
(4) 2 × 10²⁵
Answer: (1) 5 × 10⁴
Explanation: Using volume = mass/density, then using volume of unit cell (a³), we get number of unit cells. Multiply by 4 (atoms per FCC cell) to get total atoms, which evaluates to 5 × 10⁴.
59. NaCl-type ionic structure. If the edge length of cell is 508 pm and the radius of anion is 144 pm, the radius of cation is….
(1) 110 pm
(2) 220 pm
(3) 364 pm
(4) 288 pm
Answer: (1) 110 pm
Explanation: For NaCl structure, the edge length a = 2(r₊ + r₋). Substituting a = 508 pm and r₋ = 144 pm, we solve:
r₊ = (508/2) − 144 = 254 − 144 = 110 pm.
60. The density of an ionic compound (M = 58.5) is 2.165 kg/m³ and the edge length of unit cell is 562 pm, then the number of formula units (Z) of unit cell is….
(1) 4
(2) 1
(3) 3
(4) 2
Answer: (1) 4
Explanation: Using the formula:
ρ=Z×MNA×a3\rho = \frac{Z \times M}{N_A \times a^3}ρ=NA×a3Z×M
Substitute all values and solve for Z, which gives Z = 4, the number of formula units per unit cell in NaCl-type structure.
Solid state mcq for neet with answers pdf, Solid state mcq for neet with answers, Solid state mcq for neet pdf, Solid state mcq for neet pdf free download, Solid state mcq for neet pdf download, 100 MCQ on Solid State, Solid State NEET questions and Answers PDF, Solid State question bank with answers, Class 12 Solid State MCQ for NEET