Order the bond angles of the molecules or ions from smallest to largest: O3+, O3, O3-

The bond angles of the molecules or ions from smallest to largest:

O3-, O3, O3+

Explanation:

O3 - has the smallest bond angle because the added electron makes two places for electron repulsion as it allocates time on the central O.

O3 has lowering bond angle because at O3 appearance of alone pair over oxygen it will experience contracting so it may cause lowering bond angle.

O3 + has a lower electronegativity so it has a higher bond angle. Electronegativity is the tendency of an atom to attract a shared pair of the electron. so electronegativity decreases than bond angle increase so O3 has higher electronegativity so it has lowering bond angle than O3+.

O3+, O3, O3-

Explanation:

O3 - has the highest bond angle because it has the highest electro negative value. Increase in electronegativity leads to increase in bond angles so as to minimize interelectronic repulsion between the electrons. Decrease in electronegativity leads to decrease in bond angle because the repulsion is minimized.

In general, the more electronegative an ion is, the larger the bond angle. The more electropositive an ion is, the smaller the bond angle. Hence cations are smaller than anions.