Lewis Structure of SiH3- (With 6 Simple Steps to Draw!)

I’m super excited to teach you the lewis structure of SiH3- ion in just 6 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of SiH3- ion.

So, if you are ready to go with these 6 simple steps, then let’s dive right into it!

Lewis structure of SiH3- ion contains three single bonds between each Silicon (Si) and Hydrogen (H) atoms. The Silicon atom (Si) is at the center and it is surrounded by 3 Hydrogen atoms (H). The silicon atom has 1 lone pair and it has -1 formal charge.

Let’s draw and understand this lewis dot structure step by step.

(Note: Take a pen and paper with you and try to draw this lewis structure along with me. I am sure you will definitely learn how to draw lewis structure of SiH3- ion).

6 Steps to Draw the Lewis Structure of SiH3-

Step #1: Calculate the total number of valence electrons

Here, the given ion is SiH3- ion. In order to draw the lewis structure of SiH3- ion, first of all you have to find the total number of valence electrons present in the SiH3- ion.
(Valence electrons are the number of electrons present in the outermost shell of an atom).

So, let’s calculate this first.

Calculation of valence electrons in SiH3-

• For Silicon: 

Silicon is a group 14 element on the periodic table. ^[1]

Hence, the valence electrons present in silicon is 4 (see below image).

• For Hydrogen: 

Hydrogen is a group 1 element on the periodic table. ^[2]

Hence, the valence electron present in hydrogen is 1 (see below image).

Hence in a SiH3- ion, 

Valence electrons given by Silicon (Si) atom = 4
Valence electron given by each Hydrogen (H) atom = 1
Electron due to -1 charge, 1 more electron is added
So, total number of Valence electrons in SiH3- ion = 4 + 1(3) + 1 = 8

Step #2: Select the center atom (H is always outside)

While selecting the center atom, always put the least electronegative atom at the center.

(Remember: Fluorine is the most electronegative element on the periodic table and the electronegativity decreases as we move right to left in the periodic table as well as top to bottom in the periodic table). ^[1]

Here in the SiH3- ion, if we compare the silicon atom (Si) and hydrogen atom (H), then hydrogen is less electronegative than silicon. But as per the rule, we have to keep hydrogen outside.

So, silicon should be placed in the center and the remaining 3 hydrogen atoms will surround it.

Step #3: Put two electrons between the atoms to represent a chemical bond

Now in the above sketch of SiH3 molecule, put the two electrons (i.e electron pair) between each silicon atom and hydrogen atom to represent a chemical bond between them.

These pairs of electrons present between the Silicon (Si) and Hydrogen (H) atoms form a chemical bond, which bonds the silicon and hydrogen atoms with each other in a SiH3 molecule.

Step #4: Complete the octet (or duplet) on outside atoms. If the valence electrons are left, then put the valence electrons pair on the central atom

Don’t worry, I’ll explain!

In the Lewis structure of SiH3, the outer atoms are hydrogen atoms.

So now, you have to check whether these hydrogen atoms are forming a duplet or not! (because hydrogen requires only 2 electrons to have a complete outer shell).

You can see in the above image that all the hydrogen atoms form a duplet.

Also, only 6 valence electrons of SiH3- ion are used in the above structure.

But there are total 8 valence electrons in SiH3- ion (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 8 – 6 = 2.

So let’s keep these two electrons (i.e electron pair) on the central atom.

Now, let’s move to the next step.

Step #5: Check whether the central atom has octet or not

In this step, we have to check whether the central atom (i.e silicon) has an octet or not. 

In simple words, we have to check whether the central Silicon (Si) atom is having 8 electrons or not.

As you can see from the above image, the central atom (i.e silicon), is having 8 electrons. So it fulfills the octet rule and the silicon atom is stable.

Step #6: Final step – Check the stability of lewis structure by calculating the formal charge on each atom

Now, you have come to the final step and here you have to check the formal charge on silicon atom (Si) as well as each hydrogen atom (H).

For that, you need to remember the formula of formal charge;

Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2

• For Silicon:
  Valence electrons = 4 (as it is in group 14)
  Nonbonding electrons = 2
  Bonding electrons = 6
• For Hydrogen:
  Valence electron = 1 (as it is in group 1)
  Nonbonding electrons = 0
  Bonding electrons = 2

Formal charge	=	Valence electrons	–	Nonbonding electrons	–	(Bonding electrons)/2
Si	=	4	–	2	–	6/2	=	-1
H	=	1	–	0	–	2/2	=	0

So you can see above that the formal charges on silicon is -1 and the formal charge on the hydrogen atoms is 0.

Let’s keep these charges on the atoms in the above lewis structure of SiH3.

As you can see in the above sketch, there is one -ve charge on the silicon atom, which indicates the -1 formal charge on the SiH3 molecule.

Hence, the above lewis structure of SiH3- ion is the stable lewis structure.

Each electron pair (:) in the lewis dot structure of SiH3- ion represents the single bond ( | ). So the above lewis dot structure of SiH3- ion can also be represented as shown below.

Related lewis structures for your practice:
Lewis Structure of AsBr3
Lewis Structure of TeO3
Lewis Structure of TeO2
Lewis Structure of SbH3
Lewis Structure of KrCl4 

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