How Many Electrons are Unpaired in the Orbitals of Carbon

carbon unpaired electrons

Carbon has a electron configuration of 1s2 2s2 2p2.

How Many Electrons are Unpaired in the Orbitals of Carbon? There are 2 unpaired electrons in the orbitals of carbon in its ground state. There are 4 unpaired electrons in the orbitals of carbon in its bonding state.

Carbon ground state: 1s2 2s2 2p1 2p1

Carbon bonding state: 1s2 2s1 2s1 2p1 2p1

In this article we will try to find an answer for ” How Many Electrons are Unpaired in the Orbitals of Carbon “.

Unpaired Electrons of Carbon

The first condition for a good understanding of organic chemistry is to know the carbon atom, which is in the second row of the periodic table and has atomic number 6. In addition to the simple hydrogen atom found in almost all of them, nitrogen, oxygen, phosphorus, sulfur and halogens are indispensable atoms of an organic chemist. The most important feature of carbon, which makes it so important and creates a science in its name, is its ability to form various (single-double-triple) and long-chain compounds between carbon and carbon. These issues will be discussed in more detail in the following lessons.

Atom: Atoms are the smallest building blocks of the elements, which have a positive charge in their nuclei and negatively charged electrons in a relatively large area around them compared to the nucleus. Atoms contain positively charged protons as well as uncharged neutrons in their nuclei.

Protons and neutrons determine the weight of an atom and its properties are determined by protons. For example, the number of protons and electrons determines the charge of an atom. In an element, the number of protons is constant, and the number of protons and electrons is equal for an atom in a neutral (uncharged) state. The charge of the atom can change positively or negatively according to the changing number of electrons. A negatively charged atom has gained electrons, while a positively charged atom has lost electrons.

While the proton determines the properties of an element, its chemical reaction properties are determined by how it uses electrons.

Electrons in motion around atoms do not move randomly, but in a certain geometric pattern. These regions are called electron clouds (orbitals).

These orbitals (orbitals) around the atom have their own unique shapes, and some of them that are very important for organic chemistry are given below.

S and P

The angles between the p-orbitals are 90° and the orbitals are arranged in accordance with the three-dimensional space geometry. They are named Px, Py and Pz depending on the direction they are in. The d- orbitals have five and can hold 10 electrons and are more complex than the S and P orbitals. The d-orbital structure will not be covered in this course, since it is not widely used in organic chemistry.

As it can be understood from the number of electrons that their orbitals can hold, each orbital can have a maximum of two electrons.

If an atom’s orbitals are full, they are not prone to chemical reactions (bond formation). If they have half-filled (single-electron) orbitals, they are prone to bond formation.

Recognizing the most frequently used atoms in organic chemistry from these perspectives greatly facilitates the understanding of organic chemistry. Possible elements in organic molecules are Hydrogen (H), Halogens (X=F, Cl, Br, I), Oxygen (O), Nitrogen (N), Phosphorus (P), sulfur (S) and carbon (C). .

One of these elements is hydrogen, the first atom of the periodic table. Hydrogen is the smallest known atom, with only one proton and one electron. Because it has only one electron, it has a half-filled orbital and tends to form a single bond.

Carbon Unpaired Electrons

Carbon (C): The carbon atom, which led to the emergence of organic chemistry and is a little more complicated to understand than other elements, has 4 valence electrons and naturally makes four bonds. The carbon atom cannot arrange all four of these four bonds to be attached to the same atom.

While the carbon atom cannot share its four bonds with the same element, it can bond to four different atoms separately. The best example of a molecule in which carbon bonds to four different atoms is methane CH4, the smallest of the hydrocarbons. Methane is formed by the bonding of four hydrogen atoms to the four unpaired electrons of a hybridized carbon atom.

Although the carbon atom has 4 valence electrons, electron configuration of Carbon is 1S2 2S2 2P2.

It should be in shape and have two unpaired electrons so that it makes two bonds. How can it be explained that the carbon atom has four bonds instead of two?

As shown above, the 2S and 2P orbitals differ in energy levels, but are very close to each other, and one of the paired electrons in the 2S orbital can move to the vacant orbital in 2P with very little energy transfer.

This transformation (hybridization) puts all orbitals in a structure with four unpaired electrons of equal energy, in which case the carbon atom now has the familiar four bonding properties. This property of methane was examined for four different bonds, and it was announced that it could not share all four bonds with the same element.

The feature of the carbon atom that enriches organic chemistry is its ability to form double triple bonds with two carbon atoms or other suitable heteroatoms (other electronegative atoms in organic molecules, N, O, S, etc.).


How Many Electrons are Unpaired in the Orbitals of Carbon?

Carbon’s ground state electron configuration is 1s2 2s2 2p1 2p1. So, there are 2 unpaired electrons in the orbitals of carbon in ground state.

Carbon’s bonding state electron configuration is 1s2 2s1 2s1 2p1 2p1. So, there are 4 unpaired electrons in the orbitals of carbon in bonding state.

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