Arrange the following compounds in order of increasing molar conductivity .
`(i) K[Co(NH_(3))_(2)(NO_(2))_(4)]" " (ii) [Cr(NH_(3))_(3)(NO_(2))_(3)]`
`(iii) [Cr(NH_(3))_(5)(NO_(2))]_(3)[Co(NO_(2))_(6)]_(2)" " (iv) [Cr(NH_(3))_(6)]Cl_(3)`
Correct Answer - (i)Bond dissociation enthalpy should decrease as the bond distance increases from `F_(2)` to `I_(2)` due to the corresponding increase in the size of the atom as we...
Correct Answer - (i)`HCIOltHCIO_(2)ltHCIO_(3)ltHCIO_(4)`
(ii)`HCIOltHCIO_(2)ltHCIO_(3)ltHCIO_(4)`
(iii)`F^(-)ltCl^(-)ltBr^(-)ltI^(-)`
(iv)`HIltI_(2)ltIclltHIO_(4)`
(v)`HOIltHOBrltHOClltHOF`
(vi)`I_(2)ltBr_(2)ltCl_(2)ltF_(2)`
(vii)`HFltHClltHBrltHI` (On the basis of their bond dissociation energies)
(viii)`IltBrltClltF`
Compounds having cations with higher charge have large lattice enthalpy (higher positive value) than compounds having cations with lower charge.
Hence,
The correct order is NaCl < CaCl2 < AlCl3.
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