Question

Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign.

a) HF, HCl, HBr, HI (increasing acidity)
b) NH₃, H₂O, H₂S, H₂Se (increasing basicity)

Answer 1

To rank the compounds in order of increasing acidity or basicity, we need to consider the factors that determine their relative strengths as acids or bases. Acidity is determined by the ability to donate a proton (H+) to a solution, while basicity is determined by the ability to accept a proton.

Step-by-step explanation:

To rank the compounds in order of increasing acidity or basicity, we need to consider the factors that determine their relative strengths as acids or bases. Acidity is determined by the ability to donate a proton (H+) to a solution, while basicity is determined by the ability to accept a proton. In the case of the compounds listed:

a) HF, HCl, HBr, and HI, the acidity increases as we move from HF to HI. This is because the strength of the H-X bond decreases, making it easier to donate a proton. HF is the weakest acid in this series and HI is the strongest acid.

b) NH3, H2O, H2S, and H2Se, the basicity increases as we move from NH3 to H2Se. This is because as you go down the group, the size of the atom increases and the electronegativity decreases, making it easier to accept a proton. NH3 is the weakest base in this series and H2Se is the strongest base.