Electron Configuration Of Carbon

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Carbon is a very common element on Earth, in our atmosphere and even in many of the foods we eat. Carbon makes up about 85% of the human body! Very simply, carbon has 4 electrons in its outermost shell.

What Is The Electron Configuration Of Carbon?

Electron Configuration Of Carbon

The electron configuration of carbon is 1s2 2s2 2p2. This means that there are two electrons in the first shell, four electron in the second shell in which 2 electron in S orbital while 2 electron in P orbital which is unpaired.

It is important to note that electrons in an atom occupy orbitals in a specific order based on the energy level they occupy. The order is determined by the Aufbau principle that states that electrons occupy the lowest energy level orbitals first. In this case if the 1s orbital is the lowest energy level then it is followed by the 2s and 2p orbitals.

The electron configuration of carbon also plays a crucial role in its chemical behavior. For example, the 2p electrons are more reactive than the 1s or 2s electrons that makes carbon capable of forming strong covalent bonds with other elements. This is why carbon is the basis of organic chemistry and is present in all living organisms.

Carbon Electron Configuration Tabular Form

Atomic Number 6
Atomic Mass 12
Ground State  1s2 2s2 2p2
Excited State  1s2 2s1 2p3
Abbreviated Form [He] 2s2 2p2
Block category P block
Group  14
State Solid
Allotropes Diamond, Graphite, Fullerene
Color  black, brown, red, blue, green and teal

 

Excited State configuration of carbon

When sufficient energy is given to carbon atom by means of light and energy then the electron of carbon atom of lower energy level jumps to higher energy level. So, in carbon atom, in 2s2 orbitals the one electron jumps and goes to higher energy level means P orbitals, Thus, the electron configuration of carbon in excited state is 1s2 2s1 2p3.

Properties Of Carbon

Carbon is a non-metallic element that has an atomic number of six and is represented by the symbol C. It is the sixth element in the periodic table and is located in period 2, between boron and nitrogen. Carbon is a member of group 14 on the periodic table. The carbon atom has four valence electrons in its outermost shell, making it capable of forming four covalent bonds.

The element carbon is found in all known life forms and is one of the few elements that can be found in almost every imaginable environment on Earth. Carbon can exist in different forms, known as allotropes, including graphite, diamond, and fullerenes. The different allotropes of carbon have different properties and uses. For example, graphite is used as a lubricant while diamond is the hardest naturally occurring material.

The study of carbon’s properties and reactivity is known as organic chemistry. Organic molecules are those that contain carbon atoms bonded to hydrogen atoms. Because of the vast variety of possible combinations of these atoms, organic molecules can have a wide range of properties and uses. Some common examples include methane (CH4), which is the main component of natural gas, and ethanol (C2H5OH), which is used as a fuel and in alcoholic beverages.

How Does Electron Configuration Relate To Carbon?

Electron configuration is the distribution of electrons among the orbitals of an atom. The ground state of carbon is 1s2 2s2 2p2. 

Valence electron of carbon atom

Carbon has four valence electrons (the outermost electrons in the atom). This means that it can form four covalent bonds with other atoms. Carbon is also known for its ability to form long chains and complex molecules. This is because each carbon atom can form up to four covalent bonds, which allows it to bond with other carbon atoms to create long chains or complex structures.

 

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