Final answer:
The electron configurations correspond to a halogen, transition metals, an inert gas, an alkali metal, and an alkaline earth metal, identified by their completed electron orbitals and the presence of electrons in specific orbitals such as d or p.
Step-by-step explanation:
- To determine whether an electron configuration corresponds to an inert gas, a halogen, an alkali metal, an alkaline earth metal, or a transition metal, you must look at the position that the electron configuration would occupy on the periodic table.
- (a) 1s2 2s2 2p6 3s2 3p5: This is a halogen because it is one electron short of a noble gas configuration, indicating it is in group 17.
- (b) 1s2 2s2 2p6 3s2 3p6 3d7 4s2: This is a transition metal due to the partially filled d orbital.
- (c) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6: This is an inert gas because all orbitals are filled, indicating that it is in group 18.
- (d) 1s2 2s2 2p6 3s2 3p6 4s1: This is an alkali metal, in group 1, with a single electron in the outermost s orbital.
- (e) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d5 5s2: This configuration belongs to a transition metal because of the partially filled d orbital (4d5).
- (f) 1s2 2s2 2p6 3s2: This is an alkaline earth metal with two electrons in the outermost s orbital, indicating it is in group 2.