![]() In the same way, when H is 4, the molecule will show Sp3 hybridizationĪnd, when H is 6, the molecule will show Sp3d2 hybridization. Likewise, if H= 3, it indicates Sp2 hybridization. Now if H is 2, then it’s Sp hybridization H represents the hybridization, V represents the number of valence electrons, M represents the number of the monovalent atom, C represents the charge of the cation, and A represents the charge of the anion The formula to find the hybridization of any compound is, H = ½ Now let’s come to the exciting part! The formula!! This explains the theory of hybridization in CO2. The p orbitals of oxygen combine with the hybrid orbitals formed and a sigma bond is formed. This leads to the formation of 2 Sp orbital involving one electron of 2s and 1 electron of 2p orbital of the carbon atom. Thus new configuration becomes – 1s2 2s1 2p3 Now when the atoms reach their excited state, 1 electron from the 2s orbital of carbon jumps to vacant orbital 2p. ![]() The ground state configuration of C = 1s2 2s2 2p2Īnd ground state configuration of O = 1s2 2s2 2p4 Let’s understand the theory first and then we can use the formula easily! Hybridization can be understood by 2 methods, one by understanding the combination of the orbitals and 2nd by using a simple formula. The carbon atom is Sp hybridized and oxygen atoms are Sp2, making the overall molecule Sp hybridized. Thus the lewis structure of CO2 is formed using 4-5 simple steps! Also, both are having the lowest possible formal charge. In the end, check that carbon and oxygen both are having 8 electrons. These 8 electrons are distributed among the surrounding atoms. Thus according to the rule, changing the lone pairs into double bonds is necessary. Still, 12 electrons are remaining.īut, looking at the octet of atoms, observe that carbon’s octet is not fulfilled. Thus carbon is the central atom of this molecule.įollowing up the step and after drawing the skeletal diagram, we see that 4 electrons are used so far. Now, while deciding the central atom, notice that carbon has the highest bonding sites. Number of valence electrons for 2 oxygen atoms = 6*2 = 12 Number of valence electrons of oxygen = 6 Number of valence electrons of carbon = 4 Now let’s move on to the lewis structure of CO2, The calculation for formal charge can be done using the formula given below:. Step 6 – At the end ensure all the atoms are in their lowest possible formal charge. Step 5 – After that, we need to ensure if there is a requirement of multiple bonds for fulfilling the octet rule of all atoms. It’s advisable, to begin with, the electronegative atoms and then the electropositive ones. Step 4 – Then we need to complete the octet of the atoms with the electrons left. Step 3 – Next step will be, creating a skeleton containing only single bonds. Mostly the atom with the highest bonding sites is the central atom. Step 2 – Next we need to figure out the central atom of the molecule. A ‘+’ sign means losing electrons and ‘-‘ means gaining. ![]() Care should be taken regarding +, – signs. Step 1 – First and foremost we need to calculate the total valence electrons present in the molecule. Now, let us quickly go through the steps for creating a lewis structure of any compound. According to the octet rule, an atom attains stability by fulfilling its octet.įor example, in CO2, carbon needs 6 electrons to fulfill the octet, whereas oxygen needs only 2 electrons. So lewis structure generally gives us an idea about the nature of bonding and octet fulfillment of the atoms. The lewis structure of CO2 can be with some simple steps, but before that, it is important to understand lewis structure properly. ![]()
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