Although both \(CO_2\) and \(H_2O\) are triatomic molecules, the shape of \(H_2O\) molecule is bent while that of \(CO_2\) is linear. Explain this on the basis of dipole moment.
Solution and Explanation
According to experimental results, the dipole moment of carbon dioxide is zero. This is possible only if the molecule is linear so that the dipole moments of \(C-O\) bonds are equal and opposite to nullify each other.
Resultant \(\mu\) = \(0 D\)
\(H_2O\), on the other hand, has a dipole moment value of \(1.84 \;D\) (though it is a triatomic molecule as \(CO_2\)). The value of the dipole moment suggests that the structure of \(H_2O\) molecule is bent where the dipole moment of \(O-H\) bonds are unequal.
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Concepts Used:
Chemical Bonding and Molecular Structure
Such a group of atoms is called a molecule. Obviously, there must be some force that holds these constituent atoms together in the molecules. The attractive force which holds various constituents (atoms, ions, etc.) together in different chemical species is called a chemical bond.
Types of Chemical Bonds:
There are 4 types of chemical bonds which are formed by atoms or molecules to yield compounds.
- Ionic Bonds - Ionic bonding is a type of chemical bonding which involves a transfer of electrons from one atom or molecule to another.
- Covalent Bonds - Compounds that contain carbon commonly exhibit this type of chemical bonding.
- Hydrogen Bonds - It is a type of polar covalent bonding between oxygen and hydrogen wherein the hydrogen develops a partial positive charge
- Polar Bonds - In Polar Covalent chemical bonding, electrons are shared unequally since the more electronegative atom pulls the electron pair closer to itself and away from the less electronegative atom.
Factors Affecting Bond Enthalpy in Chemical Bonding:
- Size of the Atom
- Multiplicity of Bonds
- Number of Lone Pair of Electrons Present
- Bond Angle