S2-
Cu+
Sn2+
O2-
A 1s22s22p63s23p63d10
B. 2s2
C. 1s22s22p63s23p4
D. 1s22s22p63s23p63d104s1
E. 1s2
F. 1s22s22p63s23p64s23d104p65s24d10
G. 1s22s22p63s23p64s23d104p64d105s25p2
H. 1s22s22p4
I. 1s22s22p6
J. none of the above
Choose from the list the correct electron configurations for the following ions.
I thought the answers were J D F I but its showing online as incorrect
A. 1s2 2s2 2p6 3s2 3p6 3d10 28e
B. 2s2 ?e
C. 1s2 2s2 2p6 3s2 3p4 16e
D. 1s2 2s2 2p6 3s2 3p6 3d10 4s1 29e
E. 1s2 2e
F. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 48e
G. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10 5s2 5p2 50e
H. 1s2 2s2 2p4 8e
I. 1s2 2s2 2p6 10
S^2- must have 16+2=18e. None listed so J.
Cu^+ must have 29-1 = 28e. So A.
Sn^2+ must have 50-2 = 48. So ?
O^2- must have 8+2 = 10. So ?
1s22s22p63s23p4
The correct electron configurations for the ions mentioned are as follows:
Cu+: [Ar] 3d10 4s1
Sn2+: [Kr] 4d10
O2-: [He] 2s2 2p6
Therefore, the correct options are:
D. 1s22s22p63s23p63d104s1
G. 1s22s22p63s23p64s23d104p64d105s25p2
I. 1s22s22p6
To determine the correct electron configurations for the given ions, we need to consider the number of electrons and their arrangement within the atom.
1. S2-: This ion has gained two electrons, which means it now has a total of 18 electrons. The electron configuration of Argon (Ar) is 1s^2 2s^2 2p^6 3s^2 3p^6, so to represent S2-, we add two more electrons to the outermost shell: 1s^2 2s^2 2p^6 3s^2 3p^6. The correct answer is I.
2. Cu+: Copper loses one electron to become Cu+. The electron configuration of neutral copper (Cu) is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^9. After losing one electron, the configuration becomes 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10. The correct answer is D.
3. Sn2+: Tin gains two electrons to become Sn2+. The electron configuration of neutral tin (Sn) is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^2. After gaining two electrons, the configuration becomes 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^4. The correct answer is C.
4. O2-: Oxygen gains two electrons to become O2-. The electron configuration of neutral oxygen (O) is 1s^2 2s^2 2p^4. After gaining two electrons, the configuration becomes 1s^2 2s^2 2p^6. The correct answer is E.
Therefore, the correct answers are C, D, E, and I.