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As the s-character of hybridisation orbi...

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

A

Increase

B

Decreases

C

Becomes zero

D

Does not change

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question, "As the s-character of hybridization orbital increases, the bond angle...", we can follow these steps: ### Step 1: Understand Hybridization Hybridization is the concept used to explain the shape of molecules. It involves the mixing of atomic orbitals to form new hybrid orbitals that can form bonds. ### Step 2: Identify the Types of Hybridization The common types of hybridization are: - **sp³ hybridization**: 25% s-character, 75% p-character - **sp² hybridization**: 33.33% s-character, 66.67% p-character - **sp hybridization**: 50% s-character, 50% p-character ### Step 3: Analyze Bond Angles The bond angles associated with these hybridizations are: - **sp³**: 109.5 degrees - **sp²**: 120 degrees - **sp**: 180 degrees ### Step 4: Observe the Trend As we move from sp³ to sp² to sp hybridization, the s-character increases: - sp³ (25% s-character) has a bond angle of 109.5 degrees. - sp² (33.33% s-character) has a bond angle of 120 degrees. - sp (50% s-character) has a bond angle of 180 degrees. ### Step 5: Conclusion From the analysis, we can conclude that as the s-character of hybridization increases, the bond angle also increases. ### Final Answer Therefore, the correct answer to the question is that as the s-character of hybridization increases, the bond angle **increases**. ---
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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 .

Which is correct statement ? As the s-character of a hybrid orbital decreases (I) The bond angle decreases (II) The bond strength increases (III) The bond length increases (IV) Size of orbitals increases

Knowledge Check

  • 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.
  • Similar Questions

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    As the s character of the hybrid orbital decreases, the EN increases.

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

    In which of the following , the theory of hybridisation does not help to predict the bond angle ?

    The percentage s-character of the hybrid orbitals in methane , ethene are respectively

    Angle between two hybridised orbital is 105^(@) and hence the percentage of s-character in the hybridised orbital would be in the range .

    According to hybridisation theory, the % s-character in sp, sp^(2) and sp^(3) hybrid orbitals is 50, 33.3 and 25 respectively, but this is not true for all the species. When theta is the bond angle between equivalent hybrid orbitals then % s and p-character in hybrid orbitals (when only s and p-orbitals are involved in hybridisation) can be calculated by the following formula : costheta=(S)/(S-1)=(P-1)/(P) Q. Smallest Ohat(S)O bond angle is found in :

    According to hybridisation theory, the % s-character in sp, sp^(2) and sp^(3) hybrid orbitals is 50, 33.3 and 25 respectively, but this is not true for all the species. When theta is the bond angle between equivalent hybrid orbitals then % s and p-character in hybrid orbitals (when only s and p-orbitals are involved in hybridisation) can be calculated by the following formula : costheta=(S)/(S-1)=(P-1)/(P) Q. Correct order of P-P bond length in the following compound is :