Question

Draw a Lewis structure for (a) ${\mathbf{SiF}}_4$; (b)${\mathbf{SeCl}}_2$ ; (c)${\mathbf{COF}}_2$(C is central).

Short answer

The Lewis structure of

a.

b.

C.

Step-by-step solution

Lewis Structure

A Lewis structure can be defined as the basic structure of a molecule which used the valence electron of each atom involved. In Lewis’s structure, the least electronegative atom will be the central atom.

Part (a) Explanation

Si belongs to group 14 having 4 electrons in the valence shell and F belongs to group 17 having 7 electrons in valence and required 1 electron to fulfil its octet.

In the Lewis structure, the Si forms a bond with 4 fluorine atoms by sharing a pair of electrons to fulfil the octet configuration.

${\mathbf{SiF}}_4$ is a Tetrahedral structure

Part (b) Explanation

In this molecule, the Se has 6 electrons in the valence orbital and needs 2 electrons to fulfil octet which is given by 2 Cl-atom having 1 electron each.

The Se-atom forms a single bond by sharing one electron with each Cl-atom.

${\mathrm{SeCl}}_2$is a Tetrahedral structure.

The two bond pair electrons and two lone pair of electrons make it a tetrahedral structure.

Part (c) Explanation

C belongs to group 14 having 4 electrons in the valence shell requires 4 electrons for octet, O belongs to group 16 having 6 electrons in the valence shell requires 2 electrons for octet and F belongs to group 17 having 7 electrons in the valence shell requires 1 electron to fulfil the octet.

C needs four electrons for octet configuration which is fulfilled by 2 electrons from O-atom and 2 electrons from 2 F-atom.

${\mathrm{COF}}_2$is a Trigonal Planar