The molecule of CO_2 has a 180^{circ} bond an | vedclass

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(C) The central carbon atom in $CO_2$ is bonded to two oxygen atoms by double bonds.According to the Valence Shell Electron Pair Repulsion $(VSEPR)$ t

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$sp$ hybridisation

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(C) The central carbon atom in $CO_2$ is bonded to two oxygen atoms by double bonds.According to the Valence Shell Electron Pair Repulsion $(VSEPR)$ theory,the carbon atom has two bond pairs and zero lone pairs,resulting in a linear geometry.In terms of hybridisation,the carbon atom undergoes $sp$ hybridisation,where one $2s$ orbital and one $2p$ orbital mix to form two equivalent $sp$ hybrid orbitals.These two $sp$ hybrid orbitals are oriented at an angle of $180^{\circ}$ to minimize repulsion,which explains the linear shape and $180^{\circ}$ bond angle of the $CO_2$ molecule.

The molecule of $CO_2$ has a $180^{\circ}$ bond angle. It can be explained on the basis of:

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Which of the underlined atoms in the molecules shown below have $sp$-hybridization?
$(u) H_2\underline{C}=CH-CH_3$
$(v) CH_2=\underline{C}=CHCl$
$(w) CH_3-\underline{C}H_2^+$
$(x) H-C \equiv C-H$
$(y) CH_3-\underline{C} \equiv N$
$(z) (CH_3)_2C=\underline{N}-NH_2$

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