Question

Among the following, electron deficient compound is:
A.$CC{l_4}$
B.$PC{l_5}$
C.$Si{F_4}$
D.$BC{l_3}$

Answer 1

Hint: In organic chemistry, the phrase electron-deficient has historically been used to describe a pi-system, such as an alkene or arene, that has electron-withdrawing groups attached, such as nitrobenzene or acrylonitrile. Electrophilic and sensitive to nucleophilic assault, as shown in the Michael addition and nucleophilic aromatic substitution, electron-deficient pi-systems may be electrophilic and vulnerable to nucleophilic attack instead of the nucleated feature found with simple C=C bonds.

Complete answer:
Electron deficit refers to atoms or molecules that have less electrons than are necessary for optimum stability. Main group atoms with less than 8 electrons and transition metal atoms with less than 18 electrons are defined as electron-deficient for each atom in a molecule. Molecules with an incompletely full set of bonding molecular orbitals are termed electron-deficient for the entire molecule.
In the creation of a compound, electrons play a crucial function. Both electron-rich and electron-deficient cells play different roles. Please inform us of any electron-deficient substances. An electron-deficient compound is one in which the number of electrons required to complete the octet of the central atom is inadequate. There aren't enough electrons in these compounds to create conventional electron-pair bonds between each pair of linked atoms. Electron-deficient compounds, such as \[{\text{B}}{{\text{H}}_{\text{3}}}{\text{, }}{{\text{B}}_{\text{2}}}{{\text{F}}_{\text{6}}}{\text{, A}}{{\text{l}}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{6}}}\], and others, have less than 8 electrons in their valence shells.

For example, boron, with the electronic configuration \[\left[ {He} \right]2{s^2}2{p^1}\], generates compounds that are classified as electron-deficient.
Boron only has three valence electrons, but it has four accessible orbitals to accept them.
Aluminium, gallium, indium, and thallium, all members of the boron family, have a tendency to lose their valence electrons and produce ionic \[{M^{3 + }}\] species in their compounds.

Note:
Traditionally, the term "electron deficit" has been applied to boron hydrides and other compounds that lack enough valence electrons to form localised (2-centre 2-electron) bonds that connect all atoms. The B-H groups in this molecule, on the other hand, have a comparatively high electron density and show no electrophilic activity.