Advertisements
Advertisements
प्रश्न
In which of the following molecule/ion all the bonds are not equal?
पर्याय
\[\ce{XeF4}\]
\[\ce{BF^{-}4}\]
\[\ce{C2H4}\]
\[\ce{SiF4}\]
उत्तर
\[\ce{C2H4}\]
Explanation:
\[\ce{C2H4}\] has one double bond and four single bonds. Bond length of double bond \[\ce{(C = C)}\] is smaller than single bond \[\ce{(C - H)}\].
\[\begin{array}{cc}
\ce{H - C = C - H}\\
\phantom{}|\phantom{....}|\phantom{}\\
\phantom{}\ce{H}\phantom{...}\ce{H}\phantom{}
\end{array}\]
APPEARS IN
संबंधित प्रश्न
Define the bond length.
Which of the following statements are correct about \[\ce{CO^{2-}3}\]?
(i) The hybridisation of central atom is sp3.
(ii) Its resonance structure has one \[\ce{C - O}\] single bond and two \[\ce{C = O}\] double bonds.
(iii) The average formal charge on each oxygen atom is 0.67 units.
(iv) All \[\ce{C - O}\] bond lengths are equal.
All the \[\ce{C - O}\] bonds in carbonate ion \[\ce{(CO^{2-}3)}\] are equal in length. Explain.
Describe hybridisation in the case of \[\ce{PCl5}\] and \[\ce{SF6}\]. The axial bonds are longer as compared to equatorial bonds in \[\ce{PCl5}\] whereas in \[\ce{SF6}\] both axial bonds and equatorial bonds have the same bond length. Explain.
In a covalent bond, ______ the bond length ______ is the energy required to break the bond.
