Question

Explain Hybridisation and also give its characteristics...


#⃣50points✔

Answer 1

Introducing Hybridisation

All elements around us, behave in strange yet surprising ways. The electronic configuration of these elements, along with their properties, is a unique concept to study and observe. Owing to the uniqueness of such properties and uses of an element, we are able to derive many practical applications of such elements.

When it comes to the elements around us, we can observe a variety of physical properties that these elements display. The study of hybridization and how it allows the combination of various molecules in an interesting way is a very important study in science.

Understanding the properties of hybridisation lets us dive into the realms of science in a way that is hard to grasp in one go but excellent to study once we get to know more about it. Let us get to know more about the process of hybridization, which will help us understand the properties of different elements.

What is Hybridization?

Scientist Pauling introduced the revolutionary concept of hybridization in the year 1931. He described it as the redistribution of the energy of orbitals of individual atoms to give new orbitals of equivalent energy and named the process as hybridisation. In this process, the new orbitals come into existence and named as the hybrid orbitals.

Rules for Calculating Hybridisation

The following rules are observed to understand the type of hybridisation in a compound or an ion.

Calculate the total number of valence electrons.

Calculate the number of duplex or octet OR

Number of lone pairs of electrons

Number of used orbital = Number of duplex or octet + Number of lone pairs of electrons

If there is no lone pair of electrons then the geometry of orbitals and molecule is different.

Types of Hybridisation

The following are the types of hybridisation:

1) sp – Hybridisation

In such hybridisation one s- and one p-orbital are mixed to form two sp – hybrid orbitals, having a linear structure with bond angle 180 degrees. For example in the formation of BeCl2, first be atom comes in excited state 2s12p1, then hybridized to form two sp – hybrid orbitals. These hybrid orbitals overlap with the two p-orbitals of two chlorine atoms to form BeCl2

2) sp2 – Hybridisation

In such hybridisation one s- and tow p-orbitals are mixed form three sp2– hybrid orbitals, having a planar triangular structure with bond angle 120 degrees.

3) sp3 – Hybridisation

In such hybridisation one s- and three p-orbitals are mixed to form four sp3– hybrid orbitals having a tetrahedral structure with bond angle 109 degrees 28′, that is, 109.5 degrees.

Studying the Formation of Various Molecules

1) Methane

4 equivalent C-H σ bonds can be made by the interactions of C-sp3 with an H-1s

2) Ethane

6 C-H sigma(σ) bonds are made by the interaction of C-sp3 with H-1s orbitals and 1 C-C σ bond is made by the interaction of C-sp3 with another C-sp3 orbital.

3) Formation of NH3 and H2O molecules

In NH2 molecule nitrogen atom is sp3-hybridised and one hybrid orbital contains two electrons. Now three 1s- orbitals of three hydrogen atoms overlap with three sp3 hybrid orbitals to form NH3 molecule. The angle between H-N-H should be 109.50 but due to the presence of one occupied sp3– hybrid orbital the angle decreases to 107.80. Hence, the bond angle in NH3 molecule is 107.80.

4) Formation of C2H4 and C2H2 Molecules

In C2H4 molecule carbon atoms are sp2-hybridised and one 2p-orbital remains out to hybridisation. This forms p-bond while sp2 –hybrid orbitals form sigma- bonds.

5) Formation of NH3 and H2O Molecules by sp2 hybridization

In H2O molecule, the oxygen atom is sp3 – hybridized and has two occupied orbitals. Thus, the bond angle in the water molecule is 105.50.

Answer 2

$\huge\mathfrak{Hola\: Mate}$

$\huge\bold{Hybridisation}$

This process was given by Pauling.

The process of intermixing of the orbitals of slightly different energies so as to redistribute their energies resulting in the formation of new set of orbitals of equivalent energies and shape.

The new orbital formed as a result of hybridisation is called $\small\bold{hybrid\: orbitals}$.

$\huge\bold{Characteristics}$

=>The number of hybrid orbitals formed is equal to the number of the orbitals that gets hybridised.

=>The hybrid orbitals are always equivalent in energy and shapes.

=> The hybrid orbitals are more effective in forming stable bonds than the pure atomic orbitals.

HOPE IT HELPS YOU OUT✔✔ :)