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In non-aqueous solution, the trend in acid strength is observed to be: Ka (HI) > Ka (HBr) > Ka (HCl). Which periodic trend best explains this observed pattern? (A) Atomic radius: as the bond between H and the halogen becomes shorter, acid strength decreases. (B) Electron affinity: as the halogen becomes more attracted to electrons, acid strength increases (C) Electronegativity: as the bond between the two atoms becomes less polar, acid strength decreases (D) Ionization energy: as it becomes harder to remove an electron from the halogen, acid strength increases