Which of the following has the correct order in terms of increasing acidity?
Correct answer: B. CH4 < NH3 < H2O < HF
- A. HI < HBr < HCl < HF
- B. CH4 < NH3 < H2O < HF
- C. Both of the above options
- D. Cannot be determined
Explanation
HI < HBr < HCl < HF is wrong. HI is the most acidic of all because iodine is the least electronegative among all halogen in the choices. In short, the distance between H+ and I- compared to others is bigger resulting in longer bond length. The longer the bond length means it can easily dissociate because it requires less energy to break the bond. Thus, the trend of acidity in Group VII is increasing from top to bottom. CH4 < NH3 < H2O < HF is correct. The trend of acidity is increasing from the left to right. That is because the electronegativity is increasing from left to right.
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About Periodic Properties and Trends
Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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