Elements are organized on the periodic table based on their properties. Which statement correctly predicts and explains the chemical reactivity of two metals?

The correct statement about the chemical reactivity of the metals provided is:

Rubidium (Rb) is more reactive than strontium (Sr) because strontium atoms must lose more electrons.

However, let's clarify the explanation to ensure accuracy:

1. Rubidium (Rb) is in Group 1 (the alkali metals) of the periodic table, which consists of highly reactive metals. Alkali metals tend to lose one electron to achieve a stable electron configuration.

2. Strontium (Sr) is in Group 2 (the alkaline earth metals), which means it typically loses two electrons to become stable.

Since rubidium only needs to lose one electron to become stable, it is more reactive than strontium, which must lose two.

The other statements are incorrect because they misinterpret the process of gaining or losing electrons in relation to reactivity. For example, sodium is more reactive than magnesium not because it gains electrons but because it loses electrons more readily. Similarly, potassium is more reactive than calcium because it loses one electron more easily, and beryllium is less reactive than lithium because it requires energy to lose two electrons instead of one.