Which generalization applies to non-metals regarding acidic oxides?

Non-metals are characterized by their high electronegativity, which allows them to attract electrons more strongly than metals. This property is fundamental to understanding why they tend to form acidic oxides. Acidic oxides are typically oxides that can react with water to form acids, and this tendency is directly correlated to the non-metals' ability to hold onto oxygen atoms and bond with them effectively due to their high electronegativity.

When non-metals form oxides, these compounds generally exhibit acidic behavior when dissolved in water, releasing hydrogen ions (H+) and thereby leading to acidic solutions. For example, sulfur dioxide (SO₂) and nitrogen dioxide (NO₂) are oxides of non-metals that react with water to yield sulfurous acid (H₂SO₃) and nitric acid (HNO₃), respectively.

The other options do not accurately describe the behavior of non-metals and their oxides. They are not typically associated with basic oxides, as these are predominantly the characteristic of metals. Additionally, non-metals usually exhibit high, rather than low, electronegativity. Lastly, while neutral oxides do exist (for example, CO), they do not represent the primary behavior of non-metals