Step-by-step analysis:

1. Analyze Statement 1: "Boron always forms covalent bond."

   • Boron (B) has an atomic number of 5, and its electronic configuration is 1s² 2s² 2p¹. It has three valence electrons.
   • To form an ionic bond, Boron would need to lose its three valence electrons to form a cation, B³⁺.
   • The energy required to remove these three electrons is the sum of the first three ionization enthalpies (IE). For Boron, these values are:
     • IE₁ = 801 kJ/mol
     • IE₂ = 2427 kJ/mol
     • IE₃ = 3660 kJ/mol
   • The sum of these ionization enthalpies (IE₁ + IE₂ + IE₃) is 6888 kJ/mol, which is a very large amount of energy. This high energy requirement makes the formation of the B³⁺ ion energetically unfavorable.
   • Instead of losing electrons, Boron readily shares its three valence electrons with other atoms to form three covalent bonds, as seen in compounds like BF₃, BCl₃, and B₂H₆.
   • Therefore, Statement 1 is considered true in the context of general chemistry, as Boron compounds are predominantly covalent.

2. Analyze Statement 2: "The small size of B³⁺ favours formation of covalent bond."

   • This statement can be explained using Fajan's Rules, which predict the degree of covalent character in an ionic bond.
   • According to Fajan's Rules, covalent character is favored by:
     • A small, highly charged cation (high polarizing power).
     • A large, highly charged anion (high polarizability).
   • Let's consider the hypothetical B³⁺ ion. It would have a very small ionic radius (approximately 27 pm) and a high positive charge (+3).
   • A cation with a small size and high charge has a very high charge density. This gives it a strong ability to polarize (distort) the electron cloud of a nearby anion.
   • This strong polarization leads to a significant sharing of electron density between the cation and anion, resulting in a bond with high covalent character rather than a purely ionic bond.
   • Thus, the small size and high charge of the hypothetical B³⁺ ion strongly favor the formation of covalent bonds. Statement 2 is true.

3. Relate Statement 1 and Statement 2:

   • Statement 1 makes an observation: Boron forms covalent bonds.
   • Statement 2 provides a reason for this observation based on the properties of the potential cation, B³⁺.
   • The underlying reason for both the high ionization energy and the high polarizing power of B³⁺ is the same: the three valence electrons are held very tightly by the nucleus due to the small size and high effective nuclear charge of the boron atom. This makes it difficult to remove the electrons (high IE) and makes the resulting cation (if it were to form) highly polarizing.
   • Therefore, the high polarizing power of the B³⁺ ion, due to its small size and high charge, is a correct explanation for why boron compounds are covalent in nature.

Conclusion:

Both statements are true, and Statement 2 provides a correct explanation for Statement 1.

• Statement 1: True.
• Statement 2: True.
• Explanation: Statement 2 correctly explains Statement 1.