CBSE Class 12 Chemistry HOTs The Solid State

Please refer to CBSE Class 12 Chemistry HOTs The Solid State. Download HOTS questions and answers for Class 12 Chemistry. Read CBSE Class 12 Chemistry HOTs for Unit 1 The Solid State below and download in pdf. High Order Thinking Skills questions come in exams for Chemistry in Class 12 and if prepared properly can help you to score more marks. You can refer to more chapter wise Class 12 Chemistry HOTS Questions with solutions and also get latest topic wise important study material as per NCERT book for Class 12 Chemistry and all other subjects for free on Studiestoday designed as per latest CBSE, NCERT and KVS syllabus and pattern for Class 12

Unit 1 The Solid State Class 12 Chemistry HOTS

Class 12 Chemistry students should refer to the following high order thinking skills questions with answers for Unit 1 The Solid State in Class 12. These HOTS questions with answers for Class 12 Chemistry will come in exams and help you to score good marks

HOTS Questions Unit 1 The Solid State Class 12 Chemistry with Answers

Question. Value of heat of fusion of NaCl is:
a. Very low
b. Very high
c. Not very low and not very high
d. None of the above
Answer : B

Question. NaCl is an example of:
a. Covalent solid
b. Ionic solid
c. Molecular solid
d. Metallic solid
Answer : B

Question. Under which category iodine crystals are placed among the following?
a. Ionic crystal
b. Metallic crystal
c. Molecular crystal
d. Covalent crystal
Answer : C

Question. Crystalline solids are:
a. Glass
b. Rubber
c. Plastic
d. Sugar
Answer : D

Question. The solid NaCl is a bad conductor of electricity since:
a. In solid NaCl there are no ions
b. Solid NaCl is covalent
c. In solid NaCl there is no velocity of ions
d. In solid NaCl there are no electrons
Answer : C

Question. Which solid will have the weakest intermolecular forces?
a. Ice
b. Phosphorus
c. Naphthalene
d. Sodium fluoride
Answer : A

Question. Example of unit cell with crystallographic dimensions a ≠ b ≠ c α = γ = 90^o, β ≠ 90^ois:
a. Calcite
b. Graphite
c. Rhombic sulphur
d. Monoclinic sulphur
Answer : D

Question. For tetrahedral coordination number, the radius ratio r_c+/r_a-is:
a. 0.732 −1.000
b. 0.414 − 0.732
c. 0.225 − 0.414
d. 0.155 − 0.225
Answer : C

Question. If ‘Z’ is the number of atoms in the unit cell that represents the closest packing sequence − − −A B C A B C − − −, the number of tetrahedral voids in the unit cell is equal to:
a. Z
b. 2 Z
c. Z/2
d. Z/4
Answer : B

Question. Which of the following is an example of ionic crystal solid?
a. Diamond
b. LiF
c. Li
d. Silicon
Answer : B

Question. Which of the following is a molecular crystal?
a. SiC
b. NaCl
c. Graphite
d. Ice
Answer : D

Question. Amorphous substances show:
a. Short and long range order
b. Short range order
c. Long range order
d. Have no sharp M.P.
a. A and C are correct
b. B and C are correct
c. C and D are correct
d. B and D are correct
Answer : D

Question. A crystalline solid:
a. Changes abruptly from solid to liquid when heated
b. Has no definite melting point
c. Undergoes deformation of its geometry easily
d. Has an irregular 3-dimensional arrangements
Answer : A

Question. Glass is:
a. Supercooled liquid
b. Crystalline solid
c. Amorphous solid
d. Liquid crystal
Answer : A,C

Question. Na and Mg crystallize in BCC and FCC type crystals respectively, then the number of atoms of Na and Mg present in the unit cell of their respective crystal is:
a. 4 and 2
b. 9 and 14
c. 14 and 9
d. 2 and 4
Answer : D

Question. The total number of lattice arrangements in different crystal systems is:
a. 3
b. 7
c. 8
d. 14
Answer : B

Question. Bravais lattices are of:
a. 8 types
b. 12 types
c. 14 types
d. 9 types
Answer : C

Question. The correct statement in the following is:
a. The ionic crystal of AgBr has Schottky defect
b. The unit cell having crystal parameters, a = b ≠ c, 90 , 120 α = β = o γ = o is hexagonal
c. In ionic compounds having Frenkel defect the ratio γ₊/γ_-is high
d. The coordination number of Na⁺ ion in NaCl is 4
Answer : B

Question. For cubic coordination the value of radius ratio is:
a. 0.732 −1.000
b. 0.225 − 0.414
c. 0.000 − 0.225
d. 0.414 − 0.732
Answer : A

Question. Monoclinic crystal has dimension:
a. a ≠ b ≠ c,α = γ = 90°,β ≠ 90°
b. a = b = c,α = β = γ = 90°
c. a = b ≠ c,α = β = γ = 90°
d. a ≠ b ≠ c,α ≠ β ≠ γ ≠ 90°
Answer : A

Question. The structure of TlCl is similar to CsCl. What would be the radius ratio in TlCl?
a. 0.155 – 0.225
b. 0.225–0.414
c. 0.414–0.732
d. 0.732–1.000
Answer : D

Question. The number of octahedral sites per sphere in a fcc structure is:
a. 8
b. 4
c. 2
d. 1
Answer : D

Question. The ratio of close-packed atoms to tetrahedral holes in cubic close packing is:
a. 1 : 1
b. 1 : 2
c. 1 : 3
d. 2 : 1
Answer : B

Question. For tetrahedral coordination number, the radius ratio r_c+/r_a– is:
a. 0.732 −1.000
b. 0.414 − 0.732
c. 0.225 − 0.414
d. 0.155 − 0.225
Answer : C

Question. The unit cell of a NaCl lattice:
a. Is body centred cube
b. Has 3Na+ions
c. Has 4 NaCl units
d. Is electrically charged
Answer : C

Question. Ferrous oxide has a cubic structure and each edge of the unit cell is 5.0Å. Assuming density of the oxide as 4.0 g-cm–3, then the number of Fe²⁺ and O^2– ions present in each unit cell will be
a. Four Fe²⁺and four O^2–
b. Two Fe²⁺ and four O^2–
c. Four Fe²⁺ and two O^2–
d. Three Fe²⁺ and three O^2–
Answer : A

Question. The number of octahedral voids in a unit cell of a cubical closest packed structure is:
a. 1
b. 2
c. 4
d. 8
Answer : C

Question. Which ion has the largest radius from the following ions?
a. Na⁺
b. Mg²⁺
c. Al³⁺
d. Si⁴⁺
Answer : A

Question. The number of equidistant oppositely charged ions in a sodium chloride crystal is:
a. 8
b. 6
c. 4
d. 2
Answer : B

Question. Structure of ZnS is:
a. Body centred cubic
b. Face centred cubic
c. Simple cube
d. Fluorite structure
Answer : B

Question. An fcc unit cell of aluminium contains the equivalent of how many atoms:
a. 1
b. 2
c. 3
d. 4
Answer : D

Question. The number of atoms in 100g of an fcc crystal with density d=10 g/cm³ and cell edge equal to 100 pm, is equal to:
a. 4×10²⁵
b. 3×10²⁵
c. 2×10²⁵
d. 1×10²⁵
Answer : A

Question. A solid has a structure in which 'W' atoms are located at the corners of a cubic lattice 'O' atoms at the centre of edges and 'Na' atoms at the centre of the cube. The formula for the compound is:
a. NaWO₂
b. NaWO₃
c. Na₂WO₃
d. NaWO₄
Answer : B

Question. In a cubic structure of compound which is made from X and Y, where X atoms are at the corners of the cube and Y at the face centres of the cube. The molecular formula of the compound is
a. X₂Y
b. X₃Y
c. XY₂
d. XY₂
Answer : D

Question. Sodium metal crystallizes as a body centred cubic lattice with the cell edge 4.29Å. What is the radius of sodium atom?
a. 8 1.857x10⁻⁸ cm
b. 2.371x10⁻⁷ cm
c. 3.817x10⁻⁸ cm
d. 9.312x10⁻⁷ cm
Answer : A

Question. Potassium has a bcc structure with nearest neighbour distance 4.52Å. Its atomic weight is 39. Its density (in kg m^–3) will be:
a. 454
b. 804
c. 852
d. 908
Answer : D

Question. How many unit cells are present in a cube-shaped ideal crystal of NaCl of mass 1.00 g:
[Atomic masses: Na = 23, Cl = 35.5]
a. 2.57×10²¹ unit cells
b. 5.14×10²¹ unit cells
c. 1.28×10²¹ unit cells
d. 1.71×10²¹ unit cells
Answer : A

Question. An element occurring in the bcc structure has 12.08×10²³ unit cells. The total number of atoms of the element in these cells will be
a. 24.16×10²³
b. 36.18×10²³
c. 6.04×10²³
d. 12.08×10²³
Answer : A

Question. For an ionic crystal of the general formula AX and coordination number 6, the value of radius ratio will be:
a. Greater than 0.73
b. In between 0.73 and 0.41
c. In between 0.41 and 0.22
d. Less than 0.22
Answer : B

Question. CsBr crystal has bcc structure. It has an edge length of 4.3Å. The shortest interionic distance between Cs⁺ and Br^– ions is:
a. 1.86 Å
b. 3.72 Å
c. 4.3 Å
d. 7.44 Å
Answer : B

Question. In the crystal of CsCl, the nearest neighbours of each Cs ion are:
a. Six chloride ions
b. Eight chloride ions
c. Six Cs ions
d. Eight Cs ions
Answer : B

Question. In a cubic structure of compound which is made from X and Y, where X atoms are at the corners of the cube and Y at the face centres of the cube. The molecular formula of the compound is:
a. X₂Y
b. X₃Y
c. XY₂
d. XY₃
Answer : D

Question. The low solubility of BaSO₄ in water can be attributed to:
a. High lattice energy
b. Dissociation energy
c. Low lattice energy
d. Ionic bond
Answer : A

Question. Brava is lattices are of:
a. 8 types
b. 12 types
c. 14 types
d. 9 types
Answer : C

Question. In orthorhombic, the value of a,b and c are respectively 4.2Å,8.6Å and8.3Å. given the molecular mass of the solute is 155 gm mol–1 and that of density is 3.3 gm/cc, the number of formula units per unit cell is:
a. 2
b. 3
c. 4
d. 6
Answer : C

Question. In face centred cubic unit cell edge length is

""CBSE-Class-12-Chemistry-HOTs-The-Solid-State

Answer : B

Question. In a solid ‘AB’ having the NaCl structure, ‘A’ atoms occupy the corners of the cubic unit cell. If all the facecentered atoms along one of the axes are removed, then the resultant stoichiometry of the solid is:
a. AB₂
b. A₂B
c. A₄B₃
d. A₃B₄
Answer : D

Case Based Questions :

Crystalline solids have a sharp melting point and sharp boiling when it reaches a particular temperature.The shape of crystalline solids are definite and having typical arrangements of particles. They show cleavage property i.e. when they are cut with the edge of a sharp tool they split into two pieces and the newly generated surfaces are smooth and plain. They have definite heat of fusion (amount of energy needed to melt a given mass of solid at its melting point).Crystalline solids are anisotropic which means their physical properties like electrical resistance or refractive index show different values when they are measured along with different directions in the same crystal . Crystalline solids are true solids. Crystalline solids are of different types : Ionic solids, Covalent solids , Molecular solids and Metallic Solids.
Amorphous solids are gradually softened over a range of temperature and they can be moulded into different shapes on heating.Amorphous solids are pseudo solids or super cooled liquids which means they have a tendency to flow very slowly. If you observe that the glass panes which is fixed to windows of old buildings they are found to be slightly thicker from the bottom than at the top. Amorphous solids have irregular shape i.e. their constituent particles do not have definite geometry of arrangements. When amorphous solids are cut with a sharp edge tool they form pieces with irregular surfaces. Amorphous solids do not have definite heat of fusion due to its irregular arrangement of the particles. Amorphous solids are isotropic in nature which means the value of any physical property would be same along any direction because of the irregular arrangement of particles.

Question. Why some glass objects from the ancient civilizations are found to become milky
(a) Glass is a crystalline solid, milky appearance is due to its crystalline nature
(b) Glass is amorphous but on heating it become crystalline at some temperature
(c) Glass reacts with the impurities present in air
(d) None of these

Answer: B

Question. Silicon carbide is an example of
(a) Molecular solid
(b) covalent solid
(c) Metallic solid
(d) ionic solid

Answer: B

Question. Which of the following statement is not a characteristic property of amorphous solids
(a) Irregular shape
(b) Gradually soften over a range of temperature
(c) When cut with a sharp edged tool, they cut into two pieces with irregular surfaces
(d) They have a definite and characteristic heat of fusion

Answer: D

Question. Which one of the following is non-crystalline or amorphous?
(a) Diamond
(b) Graphite
(c) Glass
(d) Common Salt

Answer: C

Question. A crystalline solid
(a) has no definite melting point
(b) undergoes deformation of its geometry easily
(c) has irregular three dimensional arrangements
(d) changes abruptly from solid to liquid when heated

Answer: D

The adjective, ‘crystalline’ when applied to solids, implies an ideal crystal in which the structural units, termed as unit cells, are repeated regularly and indefinitely in three dimensions in space. The unit cell, containing at least one molecule has definite orientation and shape defined by the translational vectors, a, b and c. The unit cell therefore has a definite volume, V that contains the atoms and molecules necessary for generating the crystal. Every crystal can be classified as a member of one of the seven possible crystal systems or crystal classes that are defined by the relationships between the individual dimensions, a, b and c of the unit cell and between the individual angles, α, β, and γ of the unit cell. The structure of the given crystal may be assigned to one of the 7 crystal systems, to one of the 14 Bravais lattices, and to one of the 230 space groups. These uniquely define the possible ways of rearranging atoms in a three dimensional solid. Based on these observations, seven crystal systems were identified: triclinic, monoclinic, trigonal or rhombohedral, tetragonal, hexagonal, rhombic or orthorhombic and cubic

Question. The following unit cell with the structure given below represents ............ crystal system
CBSE Class 12 Chemistry HOTs The Solid State Set A
(a) Tetragonal
(b) Orthorombic
(c) Hexagonal
(d) trigonal

Answer: A

Question. The crystal system of compound with unit cell dimensions a= 10.48, b= 12.92, c= 24.55 Ao and α=β=γ=90ois
(a) Monoclinic
(b) Orthorombic
(c) Hexagonal
(d) Rhombohedral

Answer: B

The discovery of imperfections in an other wise ideally perfect crystal is one of the most fascinating aspects of solid state science. An ideally perfect crystal is one which has the same unit cell and contains the same lattice points throughout the crystal. The term imperfection or defect is generally used to describe any deviation of the ideally perfect crystal from the periodic arrangement of its constituents. If the deviation occurs because of missing atoms, displaced atoms or extra atoms, the imperfection is named as a point defect. Such defects can be the result of imperfect packing during the original crystallisation or they may arise from thermal vibrations of atoms at elevated temperatures because with increase in thermal energy there is increased probability of individual atoms jumping out of their positions of lowest energy. Following diagram show the imperfections :

CBSE Class 12 Chemistry HOTs The Solid State Set A

Question. Which among the following statement is true about the Schottky defect?
(a) In the defect cation and anion are lacking in stoichiometric proportion
(b) Formation of metal alloy is example of this defect
(c) In this regular cation is replaced by different cation
(d) In this cation or anion moves from regular site to place between lattice site

Answer: A

Question. Which of the following compounds does not show metal deficiency defect?
(a) FeO
(b) FeS
(c) NaCl
(d) NiO

Answer: C

Question. A perfect crystal of silicon is doped with some elements as given in the options.

Which of these options show n- type semiconductors.

Answer: A

Question. The appearance of colour in solid alkali metal halides is generally due to
(a) Schottky defect
(b) Frenkel defect
(c) Interstitial position
(d) F- centres

Answer: D

1 - MARK QUESTIONS

1.What is the number of unit cells in 936 u of sodium chloride ? 1

2. MgO has NaCl structure , what is the coordination number of both ions. 1

3. What type of substances would make better permanent magnets, Ferromagnetic or Ferrimagnetic. 1

4. In corundum, oxide ions are arranged in hcp arrangement and the aluminium ions occupy 2/3 of the octahedral voids. What is the formula of corundum ? 1

5. A compound contains two types of atoms - X and Y. It crytallises in a cubic lattice with atom X at the corners of the unit cell and atoms Y at the body centre. What is the simplest possible formula of this compound? 1

6. Name the type of point defect that occurs in a crystal of zinc sulphide. 1

7. How many octahedral voids are there in 0.5 mole of a compound having cubic close packed structure? 1

2 MARKS QUESTION

8. If the atoms of an element have the radius r, then in a primitive cubic unit cell, Calculate

(a) the length of the face diagonal.

(b) the length of the body diagonal. 2

9. A metal crystallises into two cubic phases, face-centerd cubic(FCC) and bodycentred cubic(BCC) whose unit cell lengths are 3.5 and 3.0 A^o respectively. Calculate the ratio of the densities of FCC and BCC. 2

10. What happens when

a) CsCl crystal is heated b) Pressure is applied on NaCl crystal. 2

11. ZnO crystal appears yellow on heating. Discuss. 2

12. Crystals containing F-centres are generally paramagnetic. Discuss. 2

13.. Examine the illustration of a portion of the defective crystal given below and answer the following questions.

(i) What are these type of vacancy defects called?

(ii) How is the density of a crystal affected by these defects?

(iii) Name one ionic compound which can show this type of defect in the crystalline state

(iv) How is the stoichiometry of the compound affected? 2

14. In an ionic compound the anion (N¯) form cubic close type of packing. While the cation (M⁺) ions occupy one third of the tetrahedral voids. Deduce the empirical formula of the compound and the coordination number of (M⁺) ions. 2.

15. Iron crystallizes in bcc structure. Calculate the radius of Fe atom if edge length of unit cell is 286pm. 2

16.. Xe crystallizes in fcc structure and edge of the unit cell is 620pm calculate nearest neighbour distance. 2

17. A metal (atomic mass=50) has a bcc structure. The density of metal is 5.96 g cm³.Find the volume of the cell. 2

18. In Chromium (III) Chloride, CrCl₃, chloride ions have cubic close packed arrangement and Cr (III) ions are present in the octahedral holes. What is the fraction of octahedral holes occupied? What is the fraction of total number of holes occupied? 2

a. What are the types of close packing shown in figure 1 and 2?

b. Write one example for each type of close packing in metals. 2

20. Cation vacancies in some crystals make them good catalysts. Explain 2

21. Noble Gases and metals crystallize with closed packed structure, yet the melting point of noble gas crystals are very low. Explain. 2

22. In a face centred cubic(fcc) crystal lattice, edge length is 4.0pm.find the diameter of the largest sphere which can be filled into the interstitial void without distortion of the lattice. 2

23.A metallic element crystallizes into a lattice containing sequence of layers of ABABAB……..(Any packing of spheres leaves out voids in the lattice). What percentage by volume of this lattice has empty space? 2

3 - MARKS QUESTIONS

24. In a face-centred cubic (fcc) crystal lattice, edge length is 400pm. Find the diameter of the greatest sphere which can be fitted into the interstitial void without distortion of the lattice. 3

25. KF has NaCl structure. What is the distance between K+and F- in KF if density is 2.48 gm/c.c 3

26. The density of CsBr is 4.4gm/c.c. the unit cell edge length is 400pm.calculate inter ionic distance in CsBr. 3

27..An element X with an atomic mass of 60g/mol has density of 6.23g cm^-3. If the edge length of its cubic unit cell is 400 pm, identify the type of cubic unit cell. Calculate the radius of an atom of this element.

28. The metal calcium crystallizes in a fcc unit cell with cell edge 0.556 nm. Calculate the density of metal if

i) it contains 0.2% of Frenkel defects

ii) it contains 0.1% of Schottky defects.

1-Mark Questions

1) In the normal spinel structure, the oxide ions are arranged in CCP pattern. The Zn2+ ions occupy one eighth of the tetrahedral holes and one half of the octahedral voids are occupied by Al3+. Give the formula of the spinel.

2) Metallic gold crystallizes in FCC lattice. How many nearest neighbours do each gold atom has?

3) When a crystal of NaCl is heated in sodium vapour, it acquires a yellow colour. The yellow colour is due to non stoichiometric defect. Name the defect.

4) In the face centered cubic arrangement of A and B atoms where A atoms are at the corner of the unit cell and B atoms at the face centres. One of the A atom is missing from one corner in the unit cell. What is the simplest formula of the compound

5) For the structure given below identify the site marked as S.

6) In BCC lattice, what are the numbers of the nearest and next nearest neighbours?

7) What type of magnetism is shown by the substance whose magnetic moments are aligned as given below:

8) A solid ‘X’ conducts electricity in solid state as well as in molten state. Its conductance decreases with increase in temperature. Identify the solid X.

9) In Chromium(III) Chloride, CrCl3, chloride ions have cubic close packed arrangement and Cr(III) ions are present in the octahedral holes. What is the fraction of octahedral holes occupied? What is the fraction of total number of holes occupied?

2 Marks Questions

10) A compound AB crystallizes in BCC lattice with unit cell edge length of 480Pm If the radius of B is 225Pm. Calculate the radius of A⁺.

Hint:

For BCC structure: 2(r_A+r_B) = ¥3 a

11) In the close packing arrangement of atoms does a face centred atom touch the face centred atom of an adjacent face? Give reason for your answer.

12) Identify the crystal systems which have the following crystallographic dimensions:

a. What are the types of close packing shown in figure 1 and 2?

b. Write one example for each type of close packing in metals.

15) The composition of a sample of wustite is Fe_0.93O_1.00. What percentage of Fe is present as Fe(III)?

16) Iron changes its crystal structure from body centred to cubic close packed structure when heated to 916°C. Calculate the ratio of the density of the BCC crystal to that of CCP crystal. Assume that the metallic radius of the atom does not change.

Hint:

Volume same, so ratio of density is also same

i.e. d(bcc)/d(ccp)

17) A compound forms hexagonal close packed structure. What is the total number of voids in 0.5 mol of it? How many of these are tetrahedral voids?

18) The electrical conductivity of Zinc oxide increases on heating. Give reason.

19) Both the ionic solids NaF and MgO have the same number of electrons and about the same inter nuclear distances. But the melting point of NaF is 992°C and that of MgO is 2642°C. Give plausible reason for this observation.

Hint:- charge of ions and lattice enthalpy.

20) The concentration of cation vacancies in NaCl crystal doped with CdCl₂ is found to be 6.02x10¹⁶ mol^-1. What is the concentration of CdCl₂ added to it?

3 Marks Questions

21) Calcium crystallizes in a face centred cubic unit cell with a=0.556nm. Calculate the density if

i. It contains 0.1% Frenkel defects.

ii. It contains 0.1% Schottky defects.

Hint:

Frenkel defect does not affect density.

d=zM/a³NA

Schottky defect reduces the density by 0.1%, assuming that volume remains constant.

d’=d( 1- 0.1/100)

d’=0.999d

22) You are given marbles of diameter 10mm. They are to be placed such that their centres are lying in a square bound by four lines each of length 40mm. What will be the arrangements of the marbles in a plane so that maximum number of marbles can be placed inside the area? Sketch the diagram and calculate the number of spheres per unit area.

23)

i. Name the defect shown in the figure.

ii. How does it affects the density of the solid

iii. Name a solid which shows this defect.

24) In the mineral, spinel, having the formula MgAl₂O₄, oxide irons are arranged in the cubic close packing. Mg²⁺ions occupy the tetrahedral voids while Al³⁺ions occupy the octahedral voids.

(i) What is the percentage of tetrahedral voids occupied by Mg²⁺ions?

(ii) What is the percentage of octahedral voids occupied by Al³⁺ions?

25) Metallic magnesium has a hexagonal close packed structure and has a density 1.74g cm^-3. Assuming magnesium atoms to be spherical, calculate the radius of magnesium atom. (Atomic mass of Magnesium= 24.3).

Hints: Consider 1cm³ Mg and calculate mass of 1cm³ of Mg. Then calculate the No: of atoms in that much mass of Mg. Calculate the volume occupied by the Mg Atoms and that occupied by 1 Mg atom.Then using the formula 4/3Πr³ radius of Mg, r can be calculated.

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Regular revision of HOTS given on studiestoday for Class 12 subject Chemistry Unit 1 The Solid State can help you to score better marks in exams

Are HOTS questions important for Unit 1 The Solid State Class 12 Chemistry exams

Yes, HOTS questions are important for Unit 1 The Solid State Class 12 Chemistry exams as it helps to assess your ability to think critically, apply concepts, and display understanding of the subject.