Import Question JSON

$\text{Hint: See the electronic configuration of given elements.}$\n\n$\text{Explanation:}$\n\n$\text{(1) Phosphorus (P): Atomic number = 15}$\n\n$\text{The electronic configuration of P is: } 1\text{s}^2 2\text{s}^2 2\text{p}^6 3\text{s}^2 3\text{p}^3$\n\n$\text{The orbital picture of P can be represented as:}$\n\n$1\text{s: } \uparrow\downarrow \quad 2\text{s: } \uparrow\downarrow \quad 2\text{p: } \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \quad 3\text{s: } \uparrow\downarrow \quad 3\text{p: } \uparrow \uparrow \uparrow$\n\n$\text{From the orbital picture, phosphorus has three unpaired electrons.}$\n\n$\text{(b) Iron (Fe):}$\n\n$\text{Atomic number = 26}$\n\n$\text{The electronic configuration is: } 1\text{s}^2 2\text{s}^2 2\text{p}^6 3\text{s}^2 3\text{p}^6 4\text{s}^2 3\text{d}^6$\n\n$\text{The orbital picture of iron is:}$\n\n$1\text{s: } \uparrow\downarrow \quad 2\text{s: } \uparrow\downarrow \quad 2\text{p: } \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \quad 3\text{s: } \uparrow\downarrow \quad 3\text{p: } \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \quad 4\text{s: } \uparrow\downarrow \quad 3\text{d: } \uparrow\downarrow \uparrow\downarrow \uparrow \uparrow$\n\n$\text{From the orbital picture, iron has four unpaired electrons.}$\n\n$\text{(c) Krypton (Kr):}$\n\n$\text{Atomic number = 36}$\n\n$\text{The electronic configuration is: } 1\text{s}^2 2\text{s}^2 2\text{p}^6 3\text{s}^2 3\text{p}^6 4\text{s}^2 3\text{d}^{10} 4\text{p}^6$\n\n$\text{The orbital picture of krypton is:}$\n\n$1\text{s: } \uparrow\downarrow \quad 2\text{s: } \uparrow\downarrow \quad 2\text{p: } \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \quad 3\text{s: } \uparrow\downarrow \quad 3\text{p: } \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \quad 4\text{s: } \uparrow\downarrow \quad 3\text{d: } \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \quad 4\text{p: } \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow$\n\n$\text{Since all orbitals are fully occupied, there are no unpaired electrons in}$ $\text{krypton.}$\n\n$\text{(d) Chromium (Cr):}$\n\n$\text{Atomic number = 24}$\n\n$\text{The electronic configuration of Cr is: } 1\text{s}^2 2\text{s}^2 2\text{p}^6 3\text{s}^2 3\text{p}^6 4\text{s}^1 3\text{d}^5$\n\n$\text{The orbital picture of chromium is:}$\n\n$1\text{s: } \uparrow\downarrow \quad 2\text{s: } \uparrow\downarrow \quad 2\text{p: } \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \quad 3\text{s: } \uparrow\downarrow \quad 3\text{p: } \uparrow\downarrow \uparrow\downarrow \uparrow\downarrow \quad 4\text{s: } \uparrow \quad 3\text{d: } \uparrow \uparrow \uparrow \uparrow \uparrow$\n\n$\text{From the orbital picture, chromium has six unpaired electrons. Hence, Cr is}$ $\text{the correct answer.}$