Question

Based on the reactivity of li, na and k. Predict the behavior of rb and cs. Why would we not do these experiments in the freshman chemistry labs?.

Answer 1

Rubidium and caesium are less reactive in comparison to Lithium Sodium and potassium. These experiment should not be performed in freshmen Chemistry lab because Lithium Sodium and potassium are highly reactive elements.

The same group contains the elements lithium, sodium, potassium, rubidium, and cesium. These are all components in group 1.

When we move from top to bottom in the group, lithium is at the top and caesium is at the bottom. The element becomes less reactive. The ionization energy drops, which causes a drop in reactivity.

From top to bottom in the group, the element's size grows. The element becomes less reactive as a result of its larger size since the ionization enthalpy is decreased. Due to the three compounds' extreme reactivity—lithium, sodium, and potassium—when they are left open, they react even with air, making them inappropriate for use in freshman chemistry laboratories.

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