Question

What is the general electronic configuration of Group-14 or IVA elements:
A. $n{s^2}n{p^4}$
B. $n{s^2}n{p^2}$
C. $n{s^2}n{p^6}$
D. $n{s^2}$

Answer 1

The distribution of electrons in an element's atomic orbitals is described by its electron configuration. Atomic electron configurations follow a standard nomenclature in which all electron-containing atomic subshells are arranged in a sequence. By assisting in the determination of an atom's valence electrons, electron configurations provide insight into its chemical behaviour. It also aids in the categorization of elements into several groups (such as the s-block elements, the p-block elements, the d-block elements, and the f-block elements). This makes studying the properties of the components more accessible to a group.

Complete Step By Step Answer:
Carbon $\left( C \right)$ , silicon $\left( {Si} \right)$ , germanium $\left( {Ge} \right)$ , tin $\left( {Sn} \right)$ , lead $\left( {Pb} \right)$ , and flerovium $\left( {Fl} \right)$ make up Group 14 of the p-carbon block's family. Each of these elements only possesses two electrons in its outermost p orbital: $n{s^2}n{p^2}$ . The inert pair effect causes the Group-14 elements to assume oxidation states of $+ 4$ and $+ 2$ for the heavier elements.
Hence, we can conclude from the above information that general electronic configuration of group 14 or IVA elements is $n{s^2}n{p^2}$ .
So, the correct option is: (B) $n{s^2}n{p^2}$ .

Additional Information:
This group's members follow general periodic patterns well. Ionization energies drop as atomic radii increase down the group. Metallic qualities become more prevalent as you progress through the group. Tin and lead are poor metals, while carbon is a non-metal and silicon and germanium are metalloids (they conduct heat and electricity less effectively than other metals such as copper).

Note:
The properties of the carbon family vary widely, despite their adherence to periodic trends. Carbon, for example, is a non-metal that behaves as such, but tin and lead are both metals. The Group-14 metalloids silicon and germanium act as electrical semiconductors in their elemental solid states, despite the fact that silicon is largely non-metallic; their electrical conductivity can be affected to varying degrees by doping, or the addition of Group-13 or Group-15 elements in varying concentrations to the Group-14 solid matrix. These semiconductor qualities are used in circuitry components such as diodes, transistors, and integrated circuit (IC) chips in the electronics industry.