Across the periodic table, atomic radius continues to decrease through Group 17. How does this fact help explain why the metals in Groups 3 through 13 are less reactive than the me... Across the periodic table, atomic radius continues to decrease through Group 17. How does this fact help explain why the metals in Groups 3 through 13 are less reactive than the metals in Group 1 and 2?

Understand the Problem

The question explores the relationship between atomic radius, periodic table position, and reactivity of metals. It asks you to explain why metals in Groups 3-13 are less reactive than metals in Groups 1 and 2, using the fact that atomic radius decreases across the periodic table to Group 17.

Answer

Metals in groups 1 and 2 have larger atomic radii and lose electrons easier. Groups 3-13 have a stronger attraction and are less likely to react.

The atomic radius decreases across the periodic table, the metals present in group 1 and 2 have larger atomic radii, which allows them to lose electrons easily. Due to the stronger attraction in groups 3 through 13, they are less likely to react.

More Information

Reactivity in metals is related to how easily they lose electrons. Larger atoms lose electrons easier than smaller atoms because of the distance of the valence electrons from the nucleus.

Tips

Remember the trend: Atomic radius decreases from left to right across the periodic table. This is due to increasing nuclear charge.

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