Observation Set 3 The concepts of partial atomic charges and relative electroneg
ID: 1047400 • Letter: O
Question
Observation Set 3
The concepts of partial atomic charges and relative electronegativities can be used to predict the acid–base properties of molecules. These partial hydrogen charges (?+) have been calculated based on the electronegativities of the atoms.
12. Why are HCl and HClO4 both strong acids?
Species H's Charge (?+) Species H's Charge (?+) CH4 +0.012 H2PO4– +0.36 HClO +0.34 H2O +0.26 HSO3– +0.28 HSO4– +0.30 H2SO4 +0.53 HClO4 +0.57 CH3COOH +0.35 (OH) CH3OH +0.30 (OH) +0.099 (CH) +0.050 (CH) H3PO4 +0.36 H2S +0.30 Al(OH)3 +0.23 HPO4– +0.26Explanation / Answer
Ans> HCl and HClO4 both are strong acids. Chlorine is highly electronegetive element. Only fluorine, oxygen and nitrogen has higher electronegetivity than Chlorine. The partial hydrogen charge on HClO4 is +0.57 which is highest in the table. This shows the pull effect or the high electronegetivity of chlorine pulling the electron density from hydrogen. So the proton is easily abstracted from HClO4. The conjugate anions are highly stable in Cl- and ClO4- due to the higher electronegetives of the conjugate base species of HCl and HClO4. The high electronegetivity of ClO4 is indicated by the partial hydrogen chargen value from the table. More the electronegetivity and more is the electron density pull and more stable the conjugate base and more the acidity. This is why HCl and HClO4 are both strong acids.
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