Write the condensed ground state electron configuration for the following ions.
ID: 500084 • Letter: W
Question
Write the condensed ground state electron configuration for the following ions. Identify the paramagnetic and diamagnetic species. V^5+ Cd^2+ Co^3+ Ag^+ What is the lowest principal energy level in which g orbitals could exist? How many g orbitals are there in that energy level? How many electrons could the g sublevel hold? Could (40, 5, -5, + 1/2) and (4, 4, 0, -1/2) be valid sets of quantum numbers for a hydrogen atom? Explain Write equations that represent a. 1st ionization energy of Al b. 2nd ionization energy of Al c. electron affinity of Al What is a node? How do you determine the number of nodes in an s orbital? How many nodal planes does a 2p orbital have?Explanation / Answer
V5+ - The atomic number of V is 23 but with a 3+ charge, it lost 3 electrons so now it has the electron configuration of element 20
The condensed ground-state electron configurations of V5+ is [Ar] 4s0 3d0
It is diamagnetic, because there are no singly-occupied orbitals
Cd2+- The atomic number of Cd is 48 but with a 2+ charge, it lost 2 electrons so now it has the electron configuration of element 46.
So the condensed ground-state electron configurations of Cd2+ is (Kr) 4d10
There are no singly-occupied orbitals, so Cd2+ is diamagnetic
Co3+- The atomic number of Co is 27 but with a 3+ charge, it lost 3 electrons so now it has the electron configuration of element 24
In condensed phase, ground-state electron configurations of Co3+is [Ar] 3d6
It is diamagnetic, because there are no singly-occupied orbitals
Ag+- Ag has atomic number 47, Ag+ has one less electron than does Ag. The one that it loses is the single 5s1 electron. Consequently,
The condensed ground-state electron configuration of Ag+ is [Kr] 4d10
Diamagnetic (Its outermost orbitals are completely occupied and thus have no unpaired electrons)
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