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Statement 1: BF(3) molecules planar whil...

Statement 1: `BF_(3)` molecules planar while `NF_(3)` is pyramidal.
Statement 2: N atom is smaller in size as compared to B atom.

A

Statement-1 is true, Statement-2 is also true, Statement -2 is the correct explanation of statement-1

B

Statement -1 is true , Statement 2 is also true, Statement-2 is not the correct explanation of Statement-1

C

Statement-1 is true, Statement-2 is false.

D

Statement-1 is false, Statement-2 is true.

Text Solution

AI Generated Solution

The correct Answer is:
To analyze the statements given in the question, we will evaluate each statement step by step. ### Step 1: Analyzing Statement 1 **Statement 1:** BF₃ molecules are planar while NF₃ is pyramidal. - **BF₃ (Boron Trifluoride):** - Boron has three valence electrons and forms three bonds with fluorine atoms. - The molecular geometry of BF₃ is trigonal planar because there are no lone pairs on the boron atom, and the three bond pairs are arranged in a plane to minimize repulsion. - **NF₃ (Nitrogen Trifluoride):** - Nitrogen has five valence electrons and forms three bonds with fluorine atoms, leaving one lone pair on the nitrogen atom. - The presence of this lone pair causes the molecular geometry of NF₃ to be trigonal pyramidal, as the lone pair occupies more space and pushes the bond pairs down. **Conclusion for Statement 1:** This statement is true. ### Step 2: Analyzing Statement 2 **Statement 2:** The nitrogen atom is smaller in size as compared to the boron atom. - **Atomic Size Comparison:** - Nitrogen (N) is in Group 15 and Boron (B) is in Group 13 of the periodic table. - As we move from left to right across a period, atomic size decreases due to the increase in effective nuclear charge, which pulls the electrons closer to the nucleus. - Therefore, nitrogen, being to the right of boron in the periodic table, is indeed smaller in size compared to boron. **Conclusion for Statement 2:** This statement is also true. ### Step 3: Evaluating the Relationship Between the Statements - While both statements are true, we need to determine if Statement 2 provides a correct explanation for Statement 1. - The planar shape of BF₃ is due to the absence of lone pairs, while the pyramidal shape of NF₃ is due to the presence of a lone pair on nitrogen. - The size difference between nitrogen and boron does not directly explain the molecular shapes of BF₃ and NF₃. ### Final Conclusion - **Statement 1 is true.** - **Statement 2 is true.** - However, Statement 2 does not serve as a correct explanation for Statement 1. ### Answer: - Statement 1 is true, and Statement 2 is true, but Statement 2 is not the correct explanation for Statement 1. ---
To analyze the statements given in the question, we will evaluate each statement step by step. ### Step 1: Analyzing Statement 1 **Statement 1:** BF₃ molecules are planar while NF₃ is pyramidal. - **BF₃ (Boron Trifluoride):** - Boron has three valence electrons and forms three bonds with fluorine atoms. - The molecular geometry of BF₃ is trigonal planar because there are no lone pairs on the boron atom, and the three bond pairs are arranged in a plane to minimize repulsion. ...
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The BF_3 is a planar molecule where as NF_3 is pyramidal because :

Knowledge Check

  • The BCl_3 is a planar molecule whereas NCl_3 is pyramidal because

    A
    B-Cl bond is more polar than N - Cl bond
    B
    N-Cl bond is more covalent than B- Cl bond
    C
    nitrogen atom is smaller than boron atoms
    D
    `BCl_(3)` has no lone pair but `NCl_(3)` has a lone pair of electrons.

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