For acids of the same general structure but differing electronegativities of the central atoms, acid strength decreases with increasing electronegativity of the central atom. True or false
To determine the accuracy of the statement, let's break it down and explain the concepts involved.
In general, acid strength refers to the ability of an acid to donate protons (H+ ions) in a chemical reaction. The strength of an acid depends on various factors, such as the stability of the resulting conjugate base after donating a proton.
Electronegativity is a measure of the tendency of an atom to attract electrons towards itself in a chemical bond. It increases as we move across a period in the periodic table and decreases as we move down a group.
In the context of acid strength, the electronegativity of the central atom can influence the stability of the conjugate base. Higher electronegativity of the central atom can result in stronger bonds between the central atom and the remaining atoms of the molecule.
Now, let's analyze the statement: "For acids of the same general structure but differing electronegativities of the central atoms, acid strength decreases with increasing electronegativity of the central atom."
This statement is FALSE. In general, higher electronegativity of the central atom leads to stronger acid strength, rather than weaker acid strength.
Why is this the case? When the central atom has a higher electronegativity, it tends to attract electron density towards itself. As a result, it can more effectively stabilize the negative charge on the conjugate base formed after donating a proton. The greater stability of the conjugate base increases the tendency of the acid to donate protons, thus enhancing the acid's strength.
In summary, higher electronegativity of the central atom is usually associated with stronger acid strength, contradicting the statement provided.
False.
Acid strength generally increases with increasing electronegativity of the central atom. This is because a more electronegative central atom can more effectively withdraw electron density from the acidic hydrogen, making it easier for the hydrogen to dissociate and therefore increasing the acidity of the compound.