Answer: Parapagnetism and Diamagnetism.
Explanation:
Alkali metals exhibit interesting properties due to their unique electronic configurations. Let’s explore their magnetic behavior:
Paramagnetism:
All alkali metals (lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr)) are paramagnetic.
This means that they have unpaired electrons in their valence shells, which makes them attracted to an external magnetic field.
The presence of one valence electron in the outermost shell contributes to their paramagnetic behavior.
Diamagnetism:
Alkali metal cations (such as Li⁺, Na⁺, K⁺, Rb⁺, and Cs⁺) are diamagnetic.
Diamagnetic substances are repelled by an external magnetic field.
In alkali metal cations, all valence electrons are paired, resulting in diamagnetic behavior.
In summary, alkali metals are paramagnetic due to their unpaired valence electrons, while alkali metal cations are diamagnetic because of the absence of unpaired electrons. These properties contribute to their fascinating behavior in various chemical and physical contexts!