The degree of polarity of a convalent compound is measured by the dipole moment `(mu_(bond))` of the bond defined as:
`mu_(bond) =`Charge on one of the poles `x` bond length
`mu_(bond)` is a vector quantity. The dipole moment of a molecule is the vector addition of all the bond dipole moments present in it. For a triatomic molecule, containing two bond's like `H_(2)O, mu_("molecule")` is dipole mements present in it. For a triatomic molecule, containing two bond's like `H_(2)O, mu_("molecule")` is given by
`mu_("molcular")^(2) = mu_(bond)^(2) + mu_(bond)^(2) + 2mu_(bond).mu_(bond)costheta`
`theta =` bond angle
The `%` ionic character of a bond is calculated using the equations
`%` ionic character `= (mu_(obs))/(mu_(ionic)) xx 100`
`mu_(ionic) =` dipole moment when the molecule is assumed to be completely ionic.
Which of the follwing is //are nonpolar `(mu = 0)`?

Options

A.
B.
C.
D.

Answer

A, C

Explanation