Table of Contents
How do you determine the hybridization of a species?
Here’s what you do: Look at the atom. Count the number of atoms connected to it (atoms – not bonds!) Count the number of lone pairs attached to it….Add these two numbers together.
- If it’s 4, your atom is sp3.
- If it’s 3, your atom is sp2.
- If it’s 2, your atom is sp.
How do you identify an odd electron species?
In some compounds, the number of electrons surrounding the central atom in a stable molecule is fewer than eight; this indicates an incomplete octet. There are a number of molecules whose total number of valence electrons is an odd number; this indicates an odd-electron molecule.
In which of the following odd electron bond is present?
The chlorine has one unpaired electron. So, it has an odd electron bond. Hence all the options are odd electron bonds. So, the correct answer is “Option D”.
Which of the following is an odd electron species?
The most commonly encountered stable species that exist with an odd number of electrons are nitrogen oxides, such as nitric oxide (NO) and nitrogen dioxide (NO2), both of which are free radicals and disobey the octet rule.
Which of the following are odd electron molecules?
NO2.
How do you determine the hybridization of a steric number?
One way to determine the hybridization of an atom is to calculate its steric number, which is equal to the number of sigma bonds surrounding the atom plus the number of lone pairs on the atoms. In this video, we focus on atoms with a steric number of 4, which corresponds to sp³ hybridization.
How do you find the hybridization of NO2?
NO2 involves an sp2 type of hybridization. The most simple way to determine the hybridization of NO2 is by drawing the Lewis structure and counting the number of bonds and lone electron pairs around the nitrogen atom. You will find that in nitrogen dioxide there are 2 sigma bonds and 1 lone electron pair.
What do you mean by odd electron compounds explain giving two examples?
These molecules are quite stable and paramagnetic in nature. They do not follow the octet rule because the rule requires eight electrons (or two for hydrogen) around each atom. Example: Nitrogen dioxide is a stable molecule that disobeys the octet rule. It is an odd electron molecule.
Which one of the following is not an odd electron molecule?
Nitrogen dioxide is the chemical compound with the formula NO2 . Again, nitrogen dioxide does not follow the octet rule for one of its atoms, namely nitrogen. There is the persistent radical character on nitrogen because it has an unpaired electron.
What is the hybrid orbital of an odd electron species?
Odd electron species contain an unpaired electron which can either be placed in hybrid orbital or in pure orbital. Example: In the case of ⋅ C F X 3 radical, the unpaired electron is placed in s p 3 hybrid orbital of carbon.
Which electron does not participate in hybridization?
If lone pair is present with odd electron on central atom then odd electron will not participate in hybridization irrespective of oxidation state of central atom. (1) NO2 is an example of case- (I) with positive oxidation state of central atom, so odd electron will participate in hybridization.
How many electron groups are involved in sp3d2 hybridization?
Octahedral: Six electron groups involved resulting in sp3d2 hybridization, the angle between the orbitals is 90°. Explain sp3 Hybridization in Methane? The 2s and all the three (3p) orbitals of carbon hybridize to form four sp3 orbitals.
What is the angle between the orbitals in sp2 hybridization?
The geometry of the orbital arrangement: Linear: Two electron groups involved resulting in sp hybridization, the angle between the orbitals is 180°. Trigonal planar: Three electron groups involved resulting in sp2 hybridization, the angle between the orbitals is 120°.