Chemistry Regents Practice Test 2025 - Free Chemistry Regents Practice Questions and Study Guide

Electronegativity values for elements are determined based on their ability to attract electrons within a chemical bond. Metallic elements generally possess lower electronegativity values compared to nonmetals because they tend to lose electrons and form positive ions rather than attracting electrons.

The most likely range for electronegativity values of metallic elements typically falls between 0.5 and 2.0 on the Pauling scale. A value of 1.3 fits comfortably within this range and is indicative of the tendency of metals to exhibit lower electronegativity. Elements with this electronegativity tend to be able to participate in bonding while still demonstrating their metallic character, where they can lose electrons rather than compete for them aggressively.

In contrast, values like 0.9 are also low but may represent less electronegative metals that have a weaker capacity to attract electrons in bonds. Higher values such as 2.5 and 3.0 are characteristic of nonmetals, which have a much stronger affinity for electrons and are more likely to engage in covalent bonding by drawing electrons from other atoms.

Thus, an electronegativity value of 1.3 for a metallic element is reasonable, suggesting a moderate ability to attract electrons compared to the