Question

Two statements are given below:
Statement I: Nitrogen has more ionization enthalpy and electronegativity than beryllium.
Statement II:\( CrO_3 \), \( B_2O_3 \) are acidic oxides.
Correct answer is:

• A. \(\text{Both statements I and II are correct} \)
• B. \(\text{Both statements I and II are not correct} \)
• C. \(\text{Statement I is correct, but statement II is not correct} \)
• D. \(\text{Statement I is not correct, but statement II is correct} \)

Hint:

Elements in the right side of the periodic table generally have higher ionization enthalpies and electronegativity. Transition metal oxides and non-metal oxides tend to be acidic.

Answer 1

The Correct Option is A

Step 1: Verifying Statement I 
- Ionization enthalpy is the energy required to remove an electron from an atom.
- Electronegativity is the tendency of an atom to attract electrons in a bond.
- In the periodic table, ionization enthalpy and electronegativity generally increase from left to right.
- Nitrogen (group 15) is to the right of Beryllium (group 2), meaning Nitrogen has a higher ionization enthalpy and electronegativity than Beryllium.
Conclusion: Statement I is correct.
Step 2: Verifying Statement II 
- \( CrO_3 \) (Chromium trioxide) is an acidic oxide. It reacts with water to form chromic acid (\( H_2CrO_4 \)).
- \( B_2O_3 \) (Boron trioxide) is also an acidic oxide, forming boric acid (\( H_3BO_3 \)) when dissolved in water.
- Acidic oxides typically react with bases to form salts.
Conclusion: Statement II is also correct.
Final Answer: Since both statements are correct, the correct option is (1) Both statements I and II are correct.