Question

Question: SF₆, CIF₅ , and XeF₄ are three compounds whose central atoms do not follow the octet rule. Draw Lewis structures for these compounds.

Short answer

Answer

Lewis structure of SF₆, CIF₅ , and XeF₄

Step-by-step solution

Definition of Lewis structure

The Lewis structure of a molecule is used to represent the arrangement of valence electrons among the atoms in the molecule

Fluorine and octet rule:

12 electrons are employed to form the S-F bonds, leaving 36 electrons. Since fluorine follows the octet rule, we complete the six fluorine octets to give the structure.

Xenon and octet rule:

The xenon atom in this molecule is surrounded by six pairs of electrons, requiring an octahedral arrangement.

Petafluoride chloride and octet ruel:

Chlorine pentafluoride, CIF₅ , has 42 valence electrons in total, 7 from the chlorine atom and 7 from each of the five fluorine atoms. Single bonds will connect the five fluorine atoms to the centre chlorine atom. Ten of the 42 valence electrons will be accounted for by this.