Chemical Bonding (SAQs)

Physical Science | 8. Chemical Bonding – SAQs:
Welcome to SAQs in Chapter 8: Chemical Bonding. This page contains the most Important FAQs for Short Answer Questions in this Chapter. Each answer is provided in simple English, with a Telugu explanation, and formatted according to the exam style. This will support your preparation and help you secure top marks in your exams.

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SAQ-1 : Explain why ionic compounds have high boiling and melting points.

Introduction

Grasping why ionic compounds have high boiling and melting points is crucial for understanding their properties and behavior, primarily due to the strong electrostatic forces binding the ions.

Ionic Compounds and Their High Boiling and Melting Points

1. Strong Electrostatic Force of Attraction:
   • Ionic compounds result from the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions).
   • This ionic bond is incredibly strong, securely holding the ionic compounds together.
2. Energy Requirement:
   • Significant energy is needed to break these strong ionic bonds.
   • Upon heating, this energy tries to break the bonds between the oppositely charged ions, leading to high melting and boiling points.
3. Stability of Ionic Compounds:
   • The high melting and boiling points indicate the stability of ionic compounds.
   • The strength of the bond correlates with the energy required to dissociate them, resulting in high melting and boiling points.
4. Example:
   • Sodium chloride (NaCl): The strong attraction between Na⁺ and Cl⁻ ions contributes to its high melting and boiling points.

Summary

In conclusion, the high boiling and melting points of ionic compounds are due to the strong electrostatic force of attraction in the ionic bonds. This force requires a substantial amount of energy to break, resulting in higher temperatures for melting and boiling processes. Understanding this phenomenon is key to comprehending the nature and applications of ionic compounds in scientific and industrial fields.

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SAQ-2 : Explain ionic bond with suitable example.

Introduction

An ionic bond is a type of chemical bond formed through the transfer of electrons between atoms, leading to the formation of positively and negatively charged ions. This bond is key to understanding the structure and properties of ionic compounds.

Explanation of Ionic Bond

1. Electrostatic Force of Attraction: An ionic bond is the result of the electrostatic force between a cation (positively charged ion) and an anion (negatively charged ion).
2. Transfer of Electrons: The bond forms when one atom loses electrons (becoming a cation) and another atom gains these electrons (becoming an anion).

Example: Formation of Sodium Chloride (NaCl)

1. Sodium Atom (Na):
   • Sodium has one electron in its outermost shell.
   • It loses one electron to become a positively charged ion (Na⁺).
   • Equation:
     $$\text{Na} \rightarrow \text{Na}^+ + 1e^-$$
2. Chlorine Atom (Cl):
   • Chlorine requires one more electron to complete its outer shell.
   • It gains an electron and becomes a negatively charged ion (Cl⁻).
   • Equation:
     $$\text{Cl} + 1e^- \rightarrow \text{Cl}^-$$
3. Formation of Sodium Chloride (NaCl):
   • The sodium cation (Na+Na+) and the chloride anion (Cl−Cl−) attract each other due to their opposite charges.
   • This electrostatic attraction forms an ionic bond, leading to the formation of sodium chloride (NaCl).
   • Equation:
     $$\text{Na}^+ + \text{Cl}^- \rightarrow \text{NaCl}$$

Summary

In conclusion, an ionic bond involves the attraction between oppositely charged ions created by the electron transfer from one atom to another. The formation of sodium chloride (NaCl) is a prime example, illustrating how a sodium atom becomes a cation and a chlorine atom becomes an anion, leading to the creation of an ionic compound. This understanding is essential for comprehending the properties and behaviors of various ionic compounds in chemistry.