Basic characters of hydride of these element decreases
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The discussion of this topic is made under the following heads.
(a) Hydracids of the elements of the same period. We can consider the hydracids of the elements of 2nd period viz. CH4, NH3, H2O and HF. These hydrides become increasingly acidic as we move from CH4 to HF.
Thus CH4 has negligible acidic properties, but NH3 donates a proton (H+) to strong bases to form , H2O loses a proton even more readily and HF is a fairly strongly acid. The increase in the acidic properties of these hydrides is due to the fact that as we move from CH4 to HF, the stability of their conjugate base viz , , OH– and F– increases in the order:
CH3– < NH3– < OH– < F–
the increase in acidic properties is supported by the successive increase in the dissociation constant values of these hydrides as shown.
CH4(=10-58) < NH3(=10-35) < H2O(= 10-14) < HF (= 10-4)
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(a) Hydracids of the elements of the same period. We can consider the hydracids of the elements of 2nd period viz. CH4, NH3, H2O and HF. These hydrides become increasingly acidic as we move from CH4 to HF.
Thus CH4 has negligible acidic properties, but NH3 donates a proton (H+) to strong bases to form , H2O loses a proton even more readily and HF is a fairly strongly acid. The increase in the acidic properties of these hydrides is due to the fact that as we move from CH4 to HF, the stability of their conjugate base viz , , OH– and F– increases in the order:
CH3– < NH3– < OH– < F–
the increase in acidic properties is supported by the successive increase in the dissociation constant values of these hydrides as shown.
CH4(=10-58) < NH3(=10-35) < H2O(= 10-14) < HF (= 10-4)
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