Final answer:
The cation with a +1 charge and electron configuration 1s2 2s2 2p6 is Sodium (Na+), having 10 total electrons and 6 electrons in the 2p subshell.
Step-by-step explanation:
The atomic cation in question with a charge of +1 and the electron configuration of 1s2 2s2 2p6 is the chemical element with atomic number 11. The chemical symbol for this ion is Sodium, or Na+. Since the cation has a +1 charge, it implies that one electron has been removed from the neutral sodium atom, which usually has 11 electrons. Consequently, the ion now possesses 10 electrons. When considering its subshell distribution, it has 6 electrons specifically located in the 2p subshell, this is because the full configuration of the 2p subshell is represented by 2p6, indicating it is fully occupied.
The atomic cation with a charge of +1 and the electron configuration of 1s22s22p6 is the chemical element with atomic number 11, which is Sodium (Na+). Since this cation has lost one electron to achieve a +1 charge, it now has 10 electrons in total (11 protons – 1 electron = 10 electrons). Specifically, this cation has 6 2p electrons because the 2p subshell is full (2p6).