Home
Class 11
CHEMISTRY
Assertion: Hybridisation influences the ...

Assertion: Hybridisation influences the bond length and bond enthalpy in organic compound.
Reason: More the s character of hybrid orbital, shorter and stornger will be the bond.

A

If both assertion and reason are true and reason is the correct explanation of assertion

B

If both assertion and reason are true but reason is not the correct explanation of assertion

C

If assertion is true but reason is false.

D

If both assertion and reason are false.

Text Solution

Verified by Experts

The correct Answer is:
A
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • ORGANIC CHEMISTRY-SOME BASIC PRINCIPLES AND TECHNIQUES

    NCERT FINGERTIPS ENGLISH|Exercise Tetravalence Of Carbon : Shape Of Organic Compounds|5 Videos

  • ORGANIC CHEMISTRY-SOME BASIC PRINCIPLES AND TECHNIQUES

    NCERT FINGERTIPS ENGLISH|Exercise Nomenclature Of Organic Compounds|12 Videos

  • ORGANIC CHEMISTRY-SOME BASIC PRINCIPLES AND TECHNIQUES

    NCERT FINGERTIPS ENGLISH|Exercise Exemplar Problems|12 Videos

  • HYDROGEN

    NCERT FINGERTIPS ENGLISH|Exercise Assertion And Reason|15 Videos

  • PRACTICE PAPER 1

    NCERT FINGERTIPS ENGLISH|Exercise Practice Paper 1|44 Videos

Similar Questions

Explore conceptually related problems

As the s-character of hybridisation orbital increase, the bond angle

The change in bond angle as the s - character of hybridized orbital decreases is ,

Knowledge Check

  • Bond X is made by the overlap of which type of hybridized orbitals ?

    A
    `sp and sp^3`
    B
    `sp and sp^2`
    C
    `sp^2 and sp^3`
    D
    none of these

    • Similar Questions

    Explore conceptually related problems

    The longest C-N bond length in the given compound is :

    In which compound C–Cl bond length is shortest

    The bond angle between two hybrid orbitals is 180^(@) The percentage s-character of hybrid orbital is between .

    The decreasing order of bond length of C=C bond in the following compounds is :

    Most of the polyatomic molecules except a few such as CO_(2) and CS_(2) are linear or angular with a bond angle generally somewhat greater than 90^(@) A bond angle is defined as the angle between the direction of two covalent bonds Since the atoms in molecules are in constant motion with respect to each other they are not expected to have a fixed value of bond angle Repulsion between non-bonded atoms alone does not provide an adequate explanation Hybridisation of bonding orbitals an adequate explanation Hybridisation of bonding orbitals also plays a very important role in detrmining the value of bond angle It has been observed that in hybridisation as the s-character of hybrid orbital increases the bond angle increases In P_(4) molecule phosphorous atoms are tetrahedrally arranged The angle P-P-P in the molecule is .

    The bond angle formed by different hybrid orbitals are in the order

    The compounds in which C uses its sp^(3) - hybrid orbitals for bond formation are:

    Home
    Profile