1. At what step in the ionization process would nitrogen display a sudden increase in its ionization energy?
A. sixth
B. third
C. fourth
D. fifth
E. second
2. How many electrons must a sulfur atom gain to achieve a noble gas structure?
3. Which one of the following compounds is ionic?
a. SeCl2
b. SnCl2
c. PCl3
d. SiCl4
e. None of the Above
1
Expert's answer
2019-11-12T12:02:04-0500
Q98439
Solution:
Nitrogen has an electronic configuration of "N(7)=1s^22s^22p^3" . Thus, after removing 3 electrons from the "2p" orbital, "4^{th}" ionization would mean removal of electron from the fully filled "2s" orbital, thus displaying a sudden increase in its ionization energy. Answer is C.
Sulfur has an electronic configuration of "S(16)=1s^22s^22p^63s^23p^4" and the nearest noble gas Argon has an electronic configuration of "Ar(18)=1s^22s^22p^63s^23p^6" . Thus, on gaining 2 electrons (Answer) Sulfur would attain a noble gas configuration as "S^{2-}=1s^22s^22p^63s^23p^6" .
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