There are two rules we'll take into consideration in this exercise. First is that acidity increases with an increase in oxidation state. Second is that when we have two oxides in which the central atom is in the same oxidation state, the oxide in which the central atom is more electronegative will be more acidic. As we know electronegativity decreases down the group, therefore:
Bi2O3<Sb2O3<Sb2O5<P4O10
Electronegativity is the tendency for an atom of a given chemical element to attract shared electrons (or electron density) when forming a chemical bond. An atom's electronegativity is affected by both its atomic number and the distance at which its valence electrons reside from the charged nucleus. The higher the associated electronegativity, the more an atom or a substituent group attracts electrons. Electronegativity serves as a simple way to quantitatively estimate the bond energy, and the sign and magnitude of a bond's chemical polarity, which characterizes a bond along the continuous scale from covalent to ionic bonding.
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