Question

using hybridisation and Valents hell electron pair
- Electron theory explain the Hybridisation and
Shape of NH3 H2o molecule​

Answer 1

HELLO THERE! Here's your answer!

If you understand the full concept behind understanding the geometry/shape of a molecule, you can just rock!  Here, I'm giving a detailed explanation on how to find the geometry (shape) of any molecule using VSEPR.

 

Let’s now get down to the point:

I’m telling you systematically:

 

For sp² Hybridization:

AB₃ Type, where there are three bond pairs and zero lone pairs. Such type of molecule has Trigonal Planar Shape (Bond angle= 120⁰. Example: BH₃.

AB₂L Type, where there are two bond pairs and one lone pair. Such type of molecule has V-shape/Bent-shape.  

For sp³ Hybridisation:

AB₄ Type, where there are four bond pairs and zero lone pair. Such type of molecule has Tetrahedral shape (Example, CH₄).

Your answer here:

AB₃L Type, where there are three bond pairs and one lone pair. Such type of molecule has Pyramidal shape (Example NH₃).

AB₂L₂ Type, where there are two bond pairs and two lone pairs. Such type of molecule has V-shape/Bent-shape (Example H2O).

For sp³d Hybridisation:

AB₅ Type, where there are five bond pairs and zero lone pair. Such type of molecule has Trigonal Bipyramidal shape (Example, PCl₅).

AB₄L Type, where there are four bond pairs and one lone pair. Such type of molecule has Seesaw shape (Example SF₄).

AB₃L₂ Type, where there are three bond pairs and two lone pairs. Such type of molecule is T-shaped (Example ClF₃).

AB₂L₃ Type, where there are two bond pairs and three lone pairs. Such type of molecule has Linear shape (Example I₃⁻).

For sp³d² Hybridisation:

AB₆ Type, where there are six bond pairs and zero lone pairs. Such type of molecule has Octahedral shape. (Example SF6).

I hope this will be enough, and you've got your answer. To find hybridization, you need to find the steric number H, which is found by the formula:

$H = \frac{1}{2}(V+X-C+A)$

Where,

V = Number of valence electrons of the centre atom.

X = Number of monovalent atoms surrounding the centre atom.

C = Positive charge present in the molecule.

A = Negative charge present in the molecule.

In case, the molecule is neutral, then C and A = 0.

Now once you have found out the steric number, here's how to find the hybridisation:

If steric number is:

2, hybridisation = sp

3, hybridisation = sp²

4, hybridisation = sp³

5, hybridisation = sp³d

6, hybridisation = sp³d²

7, hybridisation = sp³d³

HOPE MY ANSWER IS SATISFACTORY.

Thanks!

Answer 2

Answer:

If you understand the full concept behind understanding the geometry/shape of a molecule, you can just rock! Here, I'm giving a detailed explanation on how to find the geometry (shape) of any molecule using VSEPR.

Let’s now get down to the point:

I’m telling you systematically:

For sp² Hybridization:

AB₃ Type, where there are three bond pairs and zero lone pairs. Such type of molecule has Trigonal Planar Shape (Bond angle= 120⁰. Example: BH₃.

AB₂L Type, where there are two bond pairs and one lone pair. Such type of molecule has V-shape/Bent-shape.

For sp³ Hybridisation:

AB₄ Type, where there are four bond pairs and zero lone pair. Such type of molecule has Tetrahedral shape (Example, CH₄).

Your answer here:

AB₃L Type, where there are three bond pairs and one lone pair. Such type of molecule has Pyramidal shape (Example NH₃).

AB₂L₂ Type, where there are two bond pairs and two lone pairs. Such type of molecule has V-shape/Bent-shape (Example H2O).

For sp³d Hybridisation:

AB₅ Type, where there are five bond pairs and zero lone pair. Such type of molecule has Trigonal Bipyramidal shape (Example, PCl₅).

AB₄L Type, where there are four bond pairs and one lone pair. Such type of molecule has Seesaw shape (Example SF₄).

AB₃L₂ Type, where there are three bond pairs and two lone pairs. Such type of molecule is T-shaped (Example ClF₃).

AB₂L₃ Type, where there are two bond pairs and three lone pairs. Such type of molecule has Linear shape (Example I₃⁻).

For sp³d² Hybridisation:

AB₆ Type, where there are six bond pairs and zero lone pairs. Such type of molecule has Octahedral shape. (Example SF6).

I hope this will be enough, and you've got your answer. To find hybridization, you need to find the steric number H, which is found by the formula:

H = \frac{1}{2}(V+X-C+A)H=

2

1

(V+X−C+A)

Where,

V = Number of valence electrons of the centre atom.

X = Number of monovalent atoms surrounding the centre atom.

C = Positive charge present in the molecule.

A = Negative charge present in the molecule.

In case, the molecule is neutral, then C and A = 0.

Now once you have found out the steric number, here's how to find the hybridisation:

If steric number is:

2, hybridisation = sp

3, hybridisation = sp²

4, hybridisation = sp³

5, hybridisation = sp³d

6, hybridisation = sp³d²

7, hybridisation = sp³d³

HOPE MY ANSWER IS SATISFACTORY.

Thanks!