Home
Class 12
CHEMISTRY
Fluoride ion has higher hydration enthal...

Fluoride ion has higher hydration enthalpy than chloride ion. Give reasons.

Text Solution

Verified by Experts

Due to smaller size of F over CI, the electron density on the F atom is higher than on CI atom. Therefore, F attracts H of `H_(2)O` molecule more strongly than CI does and hence hydratio energy of F is higher than that of CI.
Promotional Banner

Topper's Solved these Questions

  • P-BLOCK ELEMENTS

    PRADEEP|Exercise NCERT QUESTIONS AND EXERCISES WITH ANSWERS|96 Videos

  • P-BLOCK ELEMENTS

    PRADEEP|Exercise MCQ - I|27 Videos

  • P-BLOCK ELEMENTS

    PRADEEP|Exercise FILL IN THE BLANKS|34 Videos

  • ORGANIC COMPOUNDS CONTAINING NITROGEN

    PRADEEP|Exercise IMPORTANT QUESTIONS FOR BOARD EXAMINATION|27 Videos

  • POLYMERS

    PRADEEP|Exercise IMPORTANT Questions (For Board Examination)|27 Videos

Similar Questions

Explore conceptually related problems

Given reasion: (i) Thermal stability decreases from H_(2)O " to " H_(2)Te (ii) Fluoride ion has higher hydration enthalpy than chloride ion (iii) Nitrogen does not form pentahalide

Write the disproportionation reaction of that oxoacid of nitrogen in which nitrogen is in +3 oxidation state. overset(+3) (3HNO_(2)) to overset(+5)(HNO_(3)) +overset(+2)(2NO_(2))+H_(2)O Give reasons for the following : (i) Fluoride ion has higher hydration enthalpy than chloride ion. (ii) Thermal stability, decreases from H_(2)O " to " H_(2)Te .

Assertion: Nitrogen has higher ionization enthalpy than oxygen. .Reason: Oxygen has stable half filled configuration .

Assertion: F^(-) ion has highest hydrated radius among the other halide ions. Reason: Ionic radius of F^(-) is smallest in the periodic table.

Fluoride has high hydration energy and iodide has least value. Explain.

Beryllium has higher ionisation enthalpy than boron.This can be explained as,

Explain the following (a) Gallium has higher ionisation enthalpy than aluminium (b) Boron does not exist as B^(3+) ion (c) Aluminium forms [AlF_(6)]^(3-) ion but boron does not form [BF_(6)]^(3-) ion.

Alkali metal salts ionic and soluble in water. The solubility of an ionic compound depends on (i) lattic ethalpy and (ii) hydration enthalpy. These two factor oppose each other. If hydration ethalpy is high, the ions will have greater tendency to be hydrated and therefore the solubility will be high. The smaller the cation, the greater is the degree of hydration. The reducing behaviour of alkali metals in solution is also dependent on the hydration enthalpy besides other factors. The ionic mobility of Li^(o+) is less than of the Na^(o+) ion in solution because

PRADEEP-P-BLOCK ELEMENTS -CONCEPTUAL QUESTION
  1. I(2) is more soluble in KI than in water. Why ?

    Text Solution

    |

  2. Why fluorine does not exhibit any positive oxidation state?

    Text Solution

    |

  3. Fluoride ion has higher hydration enthalpy than chloride ion. Give rea...

    Text Solution

    |

  4. Among halogens, F(2) is the strongest oxidising agent. Or F(2) is a ...

    Text Solution

    |

  5. F(2) is a stronger oxidising agent than Cl(2)

    Text Solution

    |

  6. Addition of Cl(2) to KI solution gives it a brown colour but excess of...

    Text Solution

    |

  7. Give chemical reaction in support of the observation that iodide ions ...

    Text Solution

    |

  8. Arrange the following in the decreasing order of their boiling points ...

    Text Solution

    |

  9. (i) Hydrogen fluoride is a weaker acid than hydrogen chloride in aqueo...

    Text Solution

    |

  10. Complete the following reaction equation : NaClO(3) (aq) + SO(2)(g) ra...

    Text Solution

    |

  11. More metal fluorides are ionic in nature than metal chlorides. Assign ...

    Text Solution

    |

  12. Why HF acid is stored in wax coated glass bottle ?

    Text Solution

    |

  13. Name the gas evolved when concentrated HCI is added to powdered potass...

    Text Solution

    |

  14. Complete the following reaction equation : Ca(OCl)(2) + HCl.

    Text Solution

    |

  15. Explain bleaching action of chlorine. Or Cl(2) acts as a bleaching a...

    Text Solution

    |

  16. What happen when Cl(2) is passed through a hot concentrated solution o...

    Text Solution

    |

  17. Arrange HClO, HBrO, HIO decreasing order of acidic strength.

    Text Solution

    |

  18. Arrange HClO(4), HClO(3), HClO(2), HClO in order of (i) decreasing aci...

    Text Solution

    |

  19. The acidic strength decreases in the order : HCl gt H(2)S gt PH(3). Ex...

    Text Solution

    |

  20. Give appropriate reason for each of the following : Perchloric acid ...

    Text Solution

    |