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Since a linear molecule deals with the double bonding of 2 other atoms to the central atom, the central atom must hybridize its orbitals to include the available amount of bonding electrons. For example, CO2 has 2 c double bonded o regions. Since carbon needs 4 electrons to perform this task, it must hybridize its s and p orbitals to use 2 electrons for each bond.
Since linear molecules have two main regions of electron density, the two hybrid orbitals that will arise are SP orbitals. This is a hybridization between the S and the one of the P orbitals.
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