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Both \( \mathrm{CO}_{2} \) and \( \mathrm{H}_{2} \mathrm{O} \) contain polar covalent bonds
\( \mathrm{P} \) but \( \mathrm{CO}_{2} \) is nonpolar while \( \mathrm{H}_{2} \mathrm{O} \) is polar because:

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(1) \( \mathrm{H} \) atom is smaller than \( \mathrm{C} \) atom
(2) \( \mathrm{CO}_{2} \) is a linear molecule while \( \mathrm{H}_{2} \mathrm{O} \) is an angular molecule
(3) \( \mathrm{O}-\mathrm{H} \) bond is more polar than \( \mathrm{C}-\mathrm{H} \) bond
(4) \( \mathrm{CO}_{2} \) contains multiple bonds while \( \mathrm{H}_{2} \mathrm{O} \) has only single bonds
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