Question

Using Lewis symbols and Lewis structures, diagram the formation of \(\mathrm{SiCl}_{4}\) from \(\mathrm{Si}\) and \(\mathrm{Cl}\) atoms.

Short answer

In the formation of SiCl4, Silicon (Si) has 4 valence electrons, and Chlorine (Cl) has 7 valence electrons. The Lewis symbols are represented as ⋅:Si:⋅ and ⋅:Cl:. In the Lewis structure, Si forms 4 bonds with 4 chlorine atoms, creating a single bond by sharing one valence electron from each Cl atom. The resulting Lewis structure is: :Cl: | :Cl: — Si — :Cl: | :Cl: Si is the central atom, and there are 4 single bonds in the SiCl4 molecule.

Step-by-step solution

Determine the Valence Electrons of Si and Cl atoms

First, we need to figure out the number of valence electrons for Si and Cl atoms. Silicon (Si) belongs to Group 14, which means it has 4 valence electrons. Chlorine (Cl) belongs to Group 17, with 7 valence electrons for each atom.

Draw the Lewis Symbols for Si and Cl atoms

Now we'll draw the Lewis symbols for Si and Cl atoms using dots to represent their valence electrons: Si:⋅:Si:⋅ Cl:⋅:Cl: In Lewis symbols, we place dots around the elements that represent their valence electrons.

Draw the Lewis Structure for the Formation of SiCl4

Now, we will draw the Lewis structure for the formation of SiCl4. Since Si has 4 valence electrons, it can form 4 bonds with 4 chlorine atoms. Each Cl atom will share one of its valence electrons with Si to form a single bond. To do this, move one electron from each Cl atom towards the Si atom to create a bond between them: :Cl: | :Cl: — Si — :Cl: | :Cl: Great! Now we've got the Lewis structure for the formation of SiCl4, where the Si atom is the central atom bonded to four Cl atoms, making a total of 4 single bonds.