Advertisements
Advertisements
Question
Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF3.
Advertisements
Solution
The ionic character in a molecule is dependent upon the electronegativity difference between the constituting atoms. The greater the difference, the greater will be the ionic character of the molecule.
On this basis, the order of increasing ionic character in the given molecules is
N2 < SO2 < ClF3 < K2O < LiF.
RELATED QUESTIONS
Although both CO2 and H2O are triatomic molecules, the shape of H2O molecule is bent while that of CO2 is linear. Explain this on the basis of dipole moment.
Write the significance/applications of dipole moment.
Define electronegativity.
How does electronegativity differ from electron gain enthalpy?
Explain with the help of suitable example polar covalent bond.
Which out of NH3 and NF3 has higher dipole moment and why?
Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment?
Arrange the following bonds in order of increasing ionic character giving reason.
\[\ce{N - H, F - H, C - H}\] and \[\ce{O - H}\]
If AB4 molecule is a polar molecule, a possible geometry of AB4 is ______.
Dipole moment of HX is 2.59 × 10−30 coulomb-metre. Bond length of HX is 1.39 Å. The ionic character of molecule is ______%.
The dipole moments of the given molecules are such that ______.
The observed dipole-moment of HCl molecule is 1.03 D. If \[\ce{H - Cl}\] bond distance is 1.275 Å and electronic charge is 4.8 × 10-10 esu. What is the percent polarity of HCl?
The dipole moments of CCl4, CHCl3 and CH4 are in the order:
