SBH3 Lewis Structure: Drawings, Hybridization, Shape, Charges, Pair And Detailed Facts


In this article, we look into the sbh3 lewis structure, shape, formal charge and its hybridization.

SbH3 has three single bonds between the Antimony atom and each Hydrogen atom in its Lewis structure. The Antimony (Sb) atom is in the centre, surrounded by three Hydrogen atoms (H). The antimony atom have a one electron pair.

SbH3 is a colourless, flammable gas that smells like rotten eggs. It is a severely hazardous heavy antimony counterpart of ammonia. Because SbH3 is extremely unstable, it is seldom found outside of labs.

1. How to draw Lewis structure for SbH3?

Steps to Draw the Lewis Structure of SbH3 as follows:

Step 1: Determine how many valence electrons there are in total

To draw the Lewis structure of SbH3, you must first figure out how many valence electrons there are in the molecule.

Valence electron calculations in SbH3:

Antimony is a periodic table group 15 element. As a result, antimony has 5 valence electrons.

On the periodic chart, hydrogen belongs to group 1.

As a result, the valence electron in hydrogen is 1.

In the SbH3 molecule, the total amount of Valence electrons is 5 + 1(3) = 8.

Step 2: Select the centre atom and keep H always outside

Always place the least electronegative atom in the centre when choosing the centre atom.

The hydrogen in the SbH3 molecule is less electronegative than antimony. We must, however, keep hydrogen outdoors due to legal requirements. As a result, antimony should be positioned in the centre, surrounded by the remaining three hydrogen atoms.

Step 3: Place the two electrons between the atoms to illustrate the chemical bond

Place two electrons between each antimony atom and hydrogen atom to show a chemical bond.

Step 4: Complete the octet on each atoms

Each hydrogen and antimony atom should have eight electrons around it. As a result, the construction must be stable.

Step 5: Check the stability of Lewis structure by calculating the formal charge on each atom

The formula for the calculation of the formal charge as follows:

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

Antimony contains five Valence electrons, two Nonbonding electrons and six Bonding electrons

Hydrogen contains one Valence electron, zero Nonbonding electrons and two Bonding electrons.

The formal charge on antimony is found to be zero.

The formal charge on hydrogen is zero.

sbh3 lewis structure
Lewis Structure of Stibine

2. SbH3 Lewis structure shape:

In order to find out Shape, consider only bond pair of electrons but for Geometry, need to consider lone pair of electrons along with bond pairs. The shape of the SbH3 molecule is Trigonal pyramidal.

Shape of SbH3 molecule from wikipedia

3. SbH3 Lewis structure formal charges:

The formula for the calculation of the formal charge as follows:

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

Antimony contains five Valence electrons, two Nonbonding electrons and six Bonding electrons

Hydrogen contains one Valence electron, zero Nonbonding electrons and two Bonding electrons.

The formal charge on antimony is found to be zero.

The formal charge on hydrogen is zero.

4. SbH3 Lewis structure lone pairs:

In SbH3 Lewis structure, antimony has 5 valence electrons and each hydrogen has one valence electron. The central atom antimony has one lone pair of electrons.

5. SbH3 hybridization:

The hybridization of SbH3 molecule is found to be sp3.

6. SbH3 Lewis structure octet rule:

The octet rule asserts that atoms gain, lose, or share electrons to establish a stable electron configuration with eight valence electrons while producing compounds. In the Lewis structure of SbH3, all of the atoms have fulfilled their octet number of electrons.

Conclusion:

In the above article, we studied about Lewis structure of Stibine molecule and its shape, hybridization, lone pairs, octet rule, formal charge calculation.

Madhusudan DN

Hi....Myself D N Madhusudan, I have completed my Masters in General Chemistry at University of Mysore. Mysore. Apart from this, I like to read, and listen to Music. Let's connect through LinkedIn:https://www.linkedin.com/in/madhusudan-d-n-b83a05156

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