Question

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

Answer 1

Answer:

A = 32

Explanation:

We are given that A is the number of electrons available and N is the needed electrons. These " available electrons " would act as the valence electrons, provided they are the only available electrons to participate in this chemical bonding.

Take a look at the placement of Silicon in the periodic table. It is positioned so that it has 4 valence electrons. Respectively Chlorine is positioned to have 7 valence electrons. There are 4 Chlorine, so determine the available electrons take a look at the math below;

$4 + 7 * ( 4 ) =\\4 + 28 =\\32\\\\Solution = 32 electrons$

Answer 2

The compound silicon chloride contains a total of 32 valence electrons.

A Lewis structure is a representation of a molecule using dots to show the valence electrons on atoms in the molecule.

Usually, we begin by determining the number of available electrons on the valence shell of each molecule and them determining the number of electrons that each atom requires to achieve a complete octet.

Silicon has four valence electrons and chlorine has seven valence electrons. Each chlorine atom shares two electrons with silicon making a total of 32 valence electrons in the molecule.

Learn more: https://brainly.com/question/19953404