17. Which of the following have the lowest first ionization energies of the groups listed.1 pointTransition metalsAlkali metalsAlkaline earth metalsNoble gasesHalogens

The group with the lowest first ionization energies among the ones listed is the Alkali metals.

Here's why:

1. Ionization energy is the energy required to remove an electron from an atom or ion.

2. Alkali metals (Group 1 elements on the periodic table) have only one electron in their outermost shell. This electron is relatively easy to remove because it is not strongly attracted to the nucleus of the atom.

3. In contrast, transition metals, alkaline earth metals, noble gases, and halogens have more electrons in their outermost shell, and these electrons are more strongly attracted to the nucleus. Therefore, it requires more energy to remove an electron from these atoms.

4. Among these, noble gases have the highest first ionization energies because they have full electron shells, which makes them very stable and resistant to losing an electron.

5. Therefore, alkali metals have the lowest first ionization energies of the groups listed.