XI Chemistry State Of Matter: Solids Online Test Mdcat-2024

Instructions for Chapter State Of Matter: Solids Online Test Mdcat-2024:

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Test Details:

Subject: Chemistry
Class: 1st year or 11
Chapter name: State Of Matter: Solids
Test: MDCAT 2024
Book: Sindh Textbook
Total No. Of MCQS: 50
Time Allowed: 50 Minutes
Price : Free

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Created on June 29, 2024 By

medicoengineer.com

XI Chemistry States Of Matter: Solid Online Test Mdcat-2024

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NameEmailPhone Number

1 / 50

1. Which statement best describes the kinetic molecular theory as it applies to solids?

a) Particles in solids are in constant, random motion with high kinetic energy.

b) Particles in solids are fixed in position and do not move at all.

c) Particles in solids vibrate around fixed positions with relatively low kinetic energy.

d) Particles in solids move freely and are far apart from each other.

2 / 50

2. Why do solids maintain a definite shape and volume according to the kinetic molecular theory?

a) The particles in solids have enough energy to overcome intermolecular forces and move freely.

b) The particles in solids are held in place by strong intermolecular forces, allowing only vibrational motion.

c) The particles in solids are arranged in a regular, repeating pattern that can change shape easily.

d) The particles in solids are not affected by temperature changes, maintaining their shape and volume.

3 / 50

3. What type of molecular motion is predominant in solids?

a) Rotational

b) Translational

c) Vibrational

d) Free motion

4 / 50

4. Why are solids generally incompressible?

a) The particles are loosely packed.

b) The particles are in constant motion.

c) The particles are tightly packed with strong intermolecular forces.

d) The particles can easily change position.

5 / 50

5. Which of the following best explains why solids have a definite shape?

a) The particles are free to move past each other.

b) The particles are held in place by strong intermolecular forces.

c) The particles are in a state of constant, random motion.

d) The particles can expand to fill their container.

6 / 50

6. Which process describes the transition of a solid directly into a gas?

a) Melting

b) Freezing

c) Sublimation

d) Condensation

7 / 50

7. Which of the following is not a sublime?

a) Naphthalene

b) Camphor

c) Solid CO₂

d) none

8 / 50

8. Select the correct statement regarding crystalline solids:

a) They don't have definite shape

b) They are isotropic in nature

c) They can be cut down at fixed cleavage plane

d) They melt over a wide range of temperature

9 / 50

9. Regular repetition of edges and faces in a crystal is known as.

a) asymmetry

b) Isotropy

c) Symmetry

d) Both B And C

10 / 50

10. A phenomenon in which crystal solids show a variation in their certain physical properties along different directions in crystal lattice :

a) Isotropy

b) Anisotropy

c) Allotropy

d) Crystal growth

11 / 50

11. The phenomenon in which different solid substances exist in the same crystalline structure is called as.

a) Polymorphism

b) Isomorphism

c) Allotropy

d) All of these

12 / 50

12. Calcite and Aragonite are __ to each other

a) Isomorph

b) Polymorph

c) Allotrope

d) None

13 / 50

13. Select the correct statement

a) Isomorphous substances have same chemical properties but.different physical properties

b) Polymorphous substances have different chemical and physical properties

c) Allotropes have same chemical nature but different physical properties

d) All of these

14 / 50

14. Which type of crystalline solid has a three-dimensional network of covalently bonded atoms?

a) Ionic solids

b) Molecular solids

c) Metallic solids

d) Network covalent solids

15 / 50

15. What is the primary bonding mechanism in metallic solids?

a) Covalent bonds

b) Ionic bonds

c) Metallic bonds

d) Hydrogen bonds

16 / 50

16. Which type of crystalline solid is typically held together by London dispersion forces and dipole-dipole interactions?

a) Ionic solids

b) Molecular solids

c) Metallic solids

d) Network covalent solids

17 / 50

17. Which type of crystalline solid conducts electricity in the molten state or in aqueous solution but not in the solid state?

a) Ionic solids

b) Molecular solids

c) Metallic solids

d) Network covalent solids

18 / 50

18. Which type of crystalline solid is characterized by a regular arrangement of positive and negative ions?

a) Ionic solids

b) Molecular solids

c) Metallic solids

d) Network covalent solids

19 / 50

19. Which type of crystalline solid has delocalized electrons that allow it to conduct electricity well?

a) Ionic solids

b) Molecular solids

c) Metallic solids

d) Network covalent solids

20 / 50

20. Which type of crystalline solid is held together by strong electrostatic forces between oppositely charged ions?

a) Ionic solids

b) Molecular solids

c) Metallic solids

d) Network covalent solids

21 / 50

21. Which type of crystalline solid can be malleable and ductile due to the ability of atoms to slide past each other?

a) Ionic solids

b) Molecular solids

c) Metallic solids

d) Network covalent solids

22 / 50

22. Select the incorrect statement

a) Ionic solids are brittle and can be shattered easily by hammering

b) Covalent solids are identified by their malleability and ductility

c) Layers of hexagons in graphite are held together by vander Waal forces

d) CaCl serves as a best dehumidifier

23 / 50

23. If the limiting radius ratio of ionic solids is 0.15 to 0.22 then coordination no and it's shape will be, respectively.

a) 4,Tetrahedral

b) 3,Cubic

c) 3,Triangular planar

d) 4,Octahedral

24 / 50

24. In terms of coordination number, a larger radius ratio (r+/r-) generally leads to:

a) A lower coordination number

b) A higher coordination number

c) No change in coordination number

d) A change in crystal color

25 / 50

25. Which of the following is correct for radius ratio of ionic solids?

a) r+/r-

b) r-/r+

c) r+ × r-/2

d) A and C

26 / 50

26. If the radius of Zn+² ion is 0.74A° and S־² ion is 1.84 A°.then its radius ratio and the geometry will be respectively

a) 0.402,Triangular

b) 0.402, Tetrahedral

c) 0.732,Tetrahedral

d) 0.22,Triangular

27 / 50

27. Covalent solids :

a) Good conductors of electricity

b) are insoluble in water

c) Possess Low melting point

d) Possess Low density

28 / 50

28. Ice, Iodine, Dry Ice are the examples of

a) Ionic Solids

b) Covalent Solids

c) Metallic solids

d) Molecular Solids

29 / 50

29. Silicon carbide is:

a) Ionic solid

b) Molecular Solid

c) Covalent Solid

d) Metallic Solid

30 / 50

30. The smallest structural part of a crystal lattice is known as

a) Lattice

b) Unit cell

c) Cube

d) Edge

31 / 50

31. Select the correct statement

a) Diamond is sp³ hybridized

b) The greasy nature of graphite is due to inter layer space.

c) Metals are good conductor of heat

d) All of these

32 / 50

32. NaCl is a :

a) Cubic Crystal

b) Tetragonal Crystal

c) Metallic Solid

d) Hexagonal Crystal

33 / 50

33. Number of chloride ions at the eight corners of cube

a) 4

b) 6

c) 8

d) 12

34 / 50

34. Number of chloride ions at the corner of one unit cell

a) 8

b) 1

c) 1/8

d) 6

35 / 50

35. Total number of chloride ions in each unit cell

a) 1

b) 3

c) 4

d) 6

36 / 50

36. Number of sodium ions on each edge of cube

a) 12

b) 8

c) 4

d) 3

37 / 50

37. Total no of sodium ions in each unit cell:

a) 4

b) 6

c) 8

d) 12

38 / 50

38. In Hexagonal close packing which type of arrangement of atoms is developed

a) ABC

b) ABA

c) ABCA

d) ABAC

39 / 50

39. Space used by ABCA layer arrangement

a) 74%

b) 68%

c) 26%

d) 36%

40 / 50

40. Coordination number in ABA and ABCA layer arrangement respectively

a) 12,8

b) 8,12

c) 8,8

d) 12,12

41 / 50

41. ABAC type of layer arrangement is developed in

a) Hexagonal close packing

b) Face Centered Cubic close packing

c) Body centered cubic

d) All of these

42 / 50

42. What factor primarily determines the magnitude of lattice energy in an ionic compound?

a) Atomic radius of the cations and anions

b) Charge of the ions

c) Density of the crystal lattice

d) Electron affinity of the ions

43 / 50

43. As the charge on the ions in an ionic compound increases, what happens to the lattice energy?

a) It decreases

b) It remains unchanged

c) It increases

d) It becomes zero

44 / 50

44. Which factor does NOT influence the lattice energy of an ionic compound?

a) Size of the ions

b) Charge of the ions

c) Crystal structure

d) Oxidation state of the cation

45 / 50

45. Lattice energy is indirectly determined by the use of?

a) Born-Haber cycle

b) Contact process

c) Hess Law

d) None

46 / 50

46. Lattice energy values are important for predicting. ?

a) Density

b) Solubility

c) Melting point

d) All of these

47 / 50

47. If all three axes in unit cell are different length but all angles are of 90° then it is identified as:

a) Orthorhombic System

b) Cubic System

c) Tetragonal System

d) Hexagonal System

48 / 50

48. The temperature at which two allotropic forms co-exist in equilibrium is called as:

a) Melting temperature

b) Fusion Temperature

c) Transition temperature

d) Critical temperature

49 / 50

49. Graphite can conduct electricity in one direction only. With this behavior, it is said to be:

a) Amorphous

b) Symmetrical

c) Anisotropic

d) Polymorphous

50 / 50

50. Select the incorrect

a) Solids do not bear vibrational kinetic energy

b) Solids are less compressible

c) Solids diffuse very slowly

d) All of these

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