Final answer:
The electron configurations that represent transition metal atoms are Option D (1s²2s²2p⁶3s²3p⁶4s²3d⁷) and Option E (1s²2s²2p⁶3s²3p⁶4s²3d²104p¹), with Option D typical of fourth period transition metals and Option E corresponding to elements in the first transition series at the end.
Step-by-step explanation:
The question is asking which of the provided electron configurations represents a transition metal atom. Transition metals are elements found in the d-block of the periodic table and they typically have an incomplete d subshell in one or more of their oxidation states.
Option A (1s²2s²2p⁶) corresponds to the noble gas neon and is not a transition metal. Option B (1s²2s²2p⁶3s²3p⁴) is the configuration for the non-metal sulfur. Option C (1s²2s²2p⁶3s²3p⁶4s²) corresponds to the alkaline earth metal calcium. Option D (1s²2s²2p⁶3s²3p⁶4s²3d⁷) represents a transition metal atom with seven d electrons. Option E (1s²2s²2p⁶3s²3p⁶4s²3d²104p¹) also represents a transition metal but with a d²10 configuration, indicating it is at the end of a transition series, specifically group 11.
Therefore, the electron configurations that represent transition metal atoms are Option D and Option E. Option D is typical for a transition metal in the fourth period of the periodic table, which would include elements like cobalt or manganese. Option E can be associated with elements like copper. Each of these elements is part of the first transition series.