ECAT Entry Test Chemistry Liquids and Solids MCQs

Liquids and Solids, Matter, Liquid Definition, Gas Definition, Plasma. 

Chemistry is another area that helps in understanding states of matter, especially liquids and solids. These two states have different properties to the familiar gas and plasma states. Solids hold their shape and have a fixed volume because intermolecular forces are strong; liquids have a fixed volume but take the shape of their container. In this article, we are going to discuss the basic properties, types, and nature of chemistry rocks and Fashion and will end this deliver with the example MCQs(multiple choice questions) to ease the understanding of chemistry liquids and solids.

Understanding Matter: Solids and Liquids

Matter exists in different states, primarily solids, liquids, gases, and plasma. Each state has distinct characteristics:

• Solids: Have a fixed shape and volume with tightly packed molecules.
• Liquids: Adapt the shape of their container but retain a definite volume.
• Gases: Have neither a definite shape nor volume and expand to fill their container.
• Plasma: An ionized state of matter found in high-energy environments like stars.

Properties of Liquids

Liquids possess unique properties that differentiate them from solids and gases. Some of these properties include:

• Viscosity: A measure of a liquid’s resistance to flow.
• Surface Tension: The cohesive force at the liquid’s surface.
• Capillary Action: The ability of a liquid to flow in narrow spaces without external force.
• Evaporation and Boiling: Processes by which a liquid turns into gas.

Properties of Solids

Solids are classified based on their internal structure and bonding. Some key properties include:

• Crystalline and Amorphous Solids: Crystalline solids have an ordered structure (e.g., diamond), whereas amorphous solids lack a definite shape (e.g., glass).
• Melting Point: The temperature at which a solid turns into a liquid.
• Electrical Conductivity: Some solids, like metals, conduct electricity, while others, like non-metals, do not.

Classification of Solids

Solids can be classified based on the nature of bonding between their particles:

1. Ionic Solids: Composed of positive and negative ions (e.g., NaCl).
2. Covalent Solids: Held together by covalent bonds (e.g., diamond).
3. Metallic Solids: Consist of a sea of electrons that allow conductivity (e.g., copper).
4. Molecular Solids: Held by weak intermolecular forces (e.g., ice).

Conclusion

Chemistry liquids and solids are really important concepts to understand when trying to master the basics of chemistry. Solids have fixed structures, and liquids take shape to accommodate their containers, demonstrating characteristics such as viscosity and surface tension. There are many kinds of solids — ionic solids, metallic solids, molecular solids, covalent solids. These chemistry notes and MCQ will assist students in ECAT entry test chemistry section preparation.

Sample MCQs on Chemistry Liquids and Solids

1. Which one of the following is not a form of chemical bonding?

• Metallic bonding
• Hydrogen bonding
  correct
• Ionic bonding
• Covalent bonding

2. Which one of the following statement about positive ions is incorrect?

• They are smaller than the atom from which they were formed
• They are larger than the atom from which hey were formed
  correct
• They are formed when electrons are removed from atoms
• They are also known as cations

3. NH3 show a maximum boiling point among the hydrides of V-A group elements due to

• Very small size of nitrogen
• Pyramidal structure of NH3
• Lone pair of electrons present on nitrogen
• Enhanced electromotive character of nitrogen
  correct

4. A chemist was able to measure the value of lattice energy of KCI to be 690 kj/mol from this experiment, he concluded that:

• Lattice energy of KBr is mol and thatr of KI 665 kJ/mol
• Lattice energy of KBr is 730 kJ/mol and that of KI 765 kJ/mol
• Lattice energy of KBr is 765 kJ/mol and that of KI 730 kJ/mol
• Lattice energy of KBr is 665 kJ/mol and that of KI is 360 kJ/mol
  correct

5. All of following acids have hydrogen bond in liquid state except

• Nitric acid
• Hydrochloric acid
  correct
• Hydrofluoric acid
• Sulphuric acid

6. Aluminum is in a Group III .Its oxide will have the formula:

• ALO₂
• AL₃O₂
• AL₂O₃
  correct
• ALO

7. Which one of the following statement about negative ions is incorrect?

• They are formed when atoms gain electrons
• They are larger than the atom from which they were formed
• They are also known as anions
• They are smaller than the atom from which they were formed
  correct

8. when water freezes at 0°Cits density decreases dues to:

• Cubic structure of ice
• Change of bond angles
• Change of bond lengths
• Empty spaces present in the structure
  correct

9. Acetone and chloroform are soluble in each other due to

• Dipole-dipole interaction
• All of these
• Intermolecular hydrogen bonding
  correct
• Instantaneous dipoles

10. which one of the following pair of atoms is most likely to from an ionic bond?

• Na and F
  correct
• O and F
• C and F
• N and F

11. Which of the following successive ionization energies belong to a Group II element?

• 320,600,1110,1700,5650
• 736,1451,7741,10500,13600correct
• 428,3070,4600,5860,7990
• 577,1820,2740,11600,14800

12. Which of the following statements is incorrect?

• The layers in graphite are held together by van der Waals forces
• The greater the number of electrons in a molecule , the greater the van der Waals forces
• 
  The boiling point of noble gases increases down the group
• H₂O has higher than expected b.p. because of inter molecular Van der Waals forcescorrect

13. A student put two eggs A and B in HCI solution. After five minutes, he took them out for weighing but egg dropped in water accidentally. The student was able to take it out after 30 minutes. He weighed it. Its weight was 40.33g. Weight of egg B was also 40.33g. Teacher told him told him that if both eggs have been dropped in water, the weight of egg B would have been.

• Unaffected instead
• Less than that of egg A
• Greater than that of egg A
  correct
• Equal to that of egg A

14. In order to mention boiling point of water at 110°C, the external pressure should be:

• 765 torr
• Between 200 torr and 760 torr
• Between 760 torr an 1200 torr
  correct
• Any value of pressure

15. Which one of the following equation represents the 2st ionization energy of Na?

• Na⁺ (g)….> Na²⁺(g)+e¯correct
• Na(g)….> Na²⁺(g)+2e¯
• Na(s)….> Na²⁺(g)+2e¯
• Na⁺ (s)….> Na²⁺(g)+e¯

16. Ionic solids are characterized by?

• High vapour pressures
• Good conductivity in solid state
• Low melting points
• Solubility in polar solventscorrect

17. Which one of the following equation represents the 1st ionization energy of Na?

• Na(s)….> Na⁺(s)+e¯
• Na(s) + e¯….> Na⁺(g)
• Na(s)….> Na⁺(g)+e¯
• Na(g)….> Na⁺(g)+e¯
  correct

18. Covalent bonds are least likely to be formed

• Between atoms of different elements on the right of the periodic table
• Between an element in group I and an element in Group VII
  correct
• By head of the group elements with high ionization energies
• Between atoms of the same element

19. London dispersion forces are the only present among the

• Molecules of water in liquid state
• Molecules of solid iodine
• Atoms of helium in gaseous state at high temperature
  correct
• Molecules of hydrogen chloride gas

20. The structure normally associated with ionic bonding is:

• A simple molecule
• A regular arrangement of ions surrounded by a sea, or cloud, of electrons
• A giant molecule
• A giant lattice
  correct

21. Instantaneous dipole-induced dipole forces are also known as

• Dipole-dipole interactions
• Van Der Waals forces
  correct
• Covalent bonds
• Hydrogen bonds

22. Why is it difficult to cook food at high as compared to at sea level?

• Boiling point of water decreases at the mountain
  correct
• Density of water decreases at the mountain
• H-bonding in H₂O changes with height
• Temperature at the top of mountain is low

23. London forces are more effective at

• Low temperature
• Low pressure
  correct
• High temperature
• High pressure

24. In which one of the following does the central atom not possess an ‘octet’ in its outer shell?

• H₂O
• BH₃
  correct
• NH₃
• CH₄

25. Which one of the following statements about sodium chloride is incorrect?

• It has a high melting point
• It conducts electricity at room temperature
  correct
• It is brittle
• It is soluble in water

Chemistry

• Basic Concepts
• Experimental Techniques
• Gases
• Liquids and Solids
• Atomic Structure
• Chemical Bonding
• Alcohols, Phenols And Ethers
• Solutions
• Chemical Equilibrium
• Electro Chemistry
• Periodic Classification Of Elements & Periodicity
• The Halogens and Noble Gases
• Group III A And IV A Elements
• S-Block Elements
• Fundamental Principles of Organic Chemistry