Question

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

Answer 1

Q98439

Solution:

1. 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.
2. 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 $S^{2-}=1s^22s^22p^63s^23p^6$ .
3. $SnCl_2$ is an ionic compound. Answer is B.