The bond length of $HCl$ molecule is $1.275\,?$ and its dipole moment is $1.03\, D$. The ionic character of the molecule (in percent) (charge of the electron $= 4.8 \times 10^{-10}$ esu) is
- 100
- 67.3
- 33.66
- 16.83
The Correct Option is D
Solution and Explanation
observed dipole moment $=1.03\, D$
Bond length of $HCl$ molecule,
$d=1.275\,?$
$=1.275 \times 10^{-8} cm$
Charge of electrons, $e^{-}=4.8 \times 10^{-10}$ esu
Percentage ionic character $=?$
Theoretical value of dipole moment $=e \times d$
$=4.8 \times 10^{-10} \times 1.275 \times 10^{-8}$ esu $- cm$
$=6.12 \times 10^{-18}$ esu $- cm$
$=6.12\, D$
Percentage ionic character
$=\frac{\text { observed dipole moment }}{\text { theoretical value of dipole moment }} \times 100$
$=\frac{1.03}{6.12} \times 100$
$=16.83 \%$
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Concepts Used:
Polarity of bonds
Polarity, in chemical bonding, distribution of electrical charge over the atoms joined by the bond. Specifically, while bonds between identical atoms, as in H2, are electrically uniform in the sense that both hydrogen atoms are electrically neutral, bonds between atoms of different elements are electrically inequivalent.
Non-polar Covalent Bond:
A non-polar covalent bond is a type of chemical bond that is formed when electrons are shared equally between two atoms. Thus, in an atom, the number of electrons shared by the adjacent atoms will be the same.
The covalent bond is also termed as nonpolar because the difference in electronegativity is mostly negligible.
Polar Covalent Bond:
A polar covalent bond exists when atoms with different electronegativities share electrons in a covalent bond. Consider the hydrogen chloride (HCl) molecule. Each atom in HCl requires one more electron to form an inert gas electron configuration.
Dipole Moment
Dipole moment is defined as the product of the magnitude of charge and the distance of separation between the centres of positive and negative charge.
Dipole moment is a vector quantity and it is denoted by µ.
µ = charge (Q) * Distance of separation(r)
The dipole moment is expressed in Debye units (D).