What do the electron structures of the alkali metals have in common?
The electron structures of the alkali metals (Group 1 elements) have the following common features:
1. They all have a single valence electron in their outermost shell. This electron is in the s-orbital.
2. The energy level of the outermost electron increases as you move down the group. For example, lithium (Li) has its valence electron in the second energy level, sodium (Na) in the third energy level, and potassium (K) in the fourth energy level.
3. All the alkali metals have a relatively low ionization energy, which means it takes very little energy to remove the valence electron and form a positively charged ion.
4. All the alkali metals react vigorously with water to form hydroxides and release hydrogen gas.
Overall, the electron structure of alkali metals makes them highly reactive and ready to donate their valence electron to form positive ions.