To draw a Lewis structure for a covalent compound, begin by calculating A, the available electrons, and N, the needed electrons. What is N for silicon tetrachloride, SiCl4?

To draw a Lewis structure for a covalent compound, begin by calculating A, the available electrons, and N, the needed electrons.

What is N for silicon tetrachloride, SiCl4?

Explanation:

A covalent compound is formed by the mutual sharing of electrons between two atoms.

According to Lewis octet theory, every atom wants to attain eight electrons around it.

For the given molecule SiCl4

Silicon has four valence electrons.

To attain the nearest inert gas configuration it requires four more electrons.

Each chlorine atom shares an electron and thus silicon attains eight electrons in its valence shell.

The Chlorine atom has seven valence electrons.

To get eight electrons in its valence shell it needs one more electron.

That is shared by the silicon atom.

Thus both Si and Cl attain eight valence electrons by sharing electrons and for the covalent bond.

N value for Si is --- 4.

A the available electrons for Si is ---- 4.

4d^55s^1 ( third choice)