Please help answer A, b and c. Please explain the answer. Choose the symbol of an atomic ion for each of thefollowing electron configurations:1s 2s²2p°3s²3p®а.OLL+OGe+Ni³+O Ni³+O Ge²+OF-OCI-b.1s 2s²2p°3s²3p°ОнOB²-O Ca+OBr¯ON³-Ca?2+С.1g2OI-C4ONI²+Oc²+C4+ON²+

Electronic configurations are used to explain the distribution of electrons in different energy levels. When an electron is removed from the system, a positive charge is generated while when an electron is added to the system an anion is formed i.e. it acquires a negative charge, the amount of charge is equal to the amount of exchange of electrons.a) 1s22s22p63s23p6 The easiest way to determine that which ion belongs to the given configuration is that first count the total electrons in the system, then recognize that the given configuration belongs to which atom, and finally search for the nearest atoms to that configuration. As in the given configuration we have 18 electrons which belongs to Ar configuration, since Cl is closest to it, by taking up one more electron it will have the same configuration to that of argon. Therefore, the electronic configuration belongs to an Cl- ion, since we know Cl has 17 electrons in its orbital and by adding one more electron it will acquire the noble configuration of argon atom. So, the correct option would be Cl-. b) 1s22s22p63s23p6 Among the given options, the configuration belongs to Ca2+ ion as Ca has 20 electrons and on losing two electrons it will have the same configuration as given. Thus the correct option would be Ca2+. c) 1s2 The configuration belongs to a Helium atom. Among the given options, the nearest atoms will be C, N and we also know C has 6 electrons while N has 7 electrons originally present in the atom. C can have the 1s2 configuration if it loses 4 electrons while N can the configuration if it will lose 5 electrons. Since, we are given with C4+ ion in the option, so it would be the correct one.