A chemist is analyzing a new element discovered in Group 1 of the periodic table. They note its high reactivity, especially with water, and predict its metallic character. Given the trends of periodic properties, which of the following statements best explains the expected behavior of this element compared to elements in Group 17 (halogens)?

The new Group 1 element will have a very low ionization energy and a low electronegativity, so it will readily lose its single valence electron and form a +1 ion, unlike halogens that gain an electron to reach a stable octet. Because it is metallic, it will react violently with water, producing hydrogen gas and a hydroxide, whereas halogens react with metals to produce halide salts. The metal’s tendency to donate rather than accept electrons explains its high reactivity with water, while halogens’ high electronegativity makes them eager to accept electrons. Thus, the Group 1 element behaves as a highly reactive, electron‑donating metal, in contrast to the electron‑accepting, nonmetallic halogens.