Relative Acidity

[Jamie2002]

When determining relative acidity, do we consider bond length first or electronegativity? Which one is more important?

[Steph Du 1H]

If the bond being broken for the compounds you are comparing is different, you compare bond length (ex. HCl and HBr). If the bond being broken is the same, then you compare electronegativity (ex. CCl3COOH and CH3COOH).

[Brianne Conway 1D]

If the bond being broken for the compounds you are comparing is different, you compare bond length (ex. HCl and HBr). If the bond being broken is the same, then you compare electronegativity (ex. CCl3COOH and CH3COOH).

Thanks for that explanation, it really clears everything up nicely.

[Rose_Malki_3G]

First compare bond length. If bonds are the same in the compounds you are comparing then compare stability of the anions (so compare electronegativity)

[Nathan Chu 3H]

Bond length is mainly considered when comparing binary acids, such as HF, HCl, and HI. In this case, the acids with longer bonds will be stronger acids, as they have weaker bonds and can deprotonate easier.

Electronegativity and how well the conjugate base anion dilutes the negative charge is used when considering oxoacids, such as HOBrO2 and HOClO2. In this example, the HOClO2 acid is stronger because chlorine is more electronegative than Bromine. Because chlorine is more electronegative, it is able pull the electron density away from the O-H bond and allow it to deprotonate easier.

[Jamie2002]

Bond length is mainly considered when comparing binary acids, such as HF, HCl, and HI. In this case, the acids with longer bonds will be stronger acids, as they have weaker bonds and can deprotonate easier.

Electronegativity and how well the conjugate base anion dilutes the negative charge is used when considering oxoacids, such as HOBrO2 and HOClO2. In this example, the HOClO2 acid is stronger because chlorine is more electronegative than Bromine. Because chlorine is more electronegative, it is able pull the electron density away from the O-H bond and allow it to deprotonate easier.

Thankyou so much! It's a lot clearer now :)

[Jamie2002]

First compare bond length. If bonds are the same in the compounds you are comparing then compare stability of the anions (so compare electronegativity)

Thank you!

[Jamie2002]

If the bond being broken for the compounds you are comparing is different, you compare bond length (ex. HCl and HBr). If the bond being broken is the same, then you compare electronegativity (ex. CCl3COOH and CH3COOH).

Thank you!