Which group in the periodic table exhibits the greatest metallic character?

• A. Group 2 (alkaline earth metals)
• B. Group 17 (halogens)
• C. Group 1 (alkali metals)
• D. Group 18 (noble gases)

Answer: (C)

Verified step by step guidance

1. Understand that metallic character refers to how readily an element can lose electrons to form positive ions, which is related to properties like conductivity, malleability, and luster.
2. Recall that metallic character increases as you move down a group in the periodic table because atoms have more electron shells, making it easier to lose outer electrons.
3. Recall that metallic character decreases as you move from left to right across a period because atoms have more protons, increasing the effective nuclear charge and holding onto electrons more tightly.
4. Identify the groups given: Group 1 (alkali metals), Group 2 (alkaline earth metals), Group 17 (halogens), and Group 18 (noble gases). Group 1 elements are located at the far left of the periodic table and have the lowest ionization energies, making them the most metallic.
5. Conclude that Group 1 exhibits the greatest metallic character because they are the most reactive metals, easily losing their single valence electron compared to the other groups listed.