Advertisements
Advertisements
प्रश्न
In Ammonia molecule the bond angle is 107° and in water molecule it is 104°35', although in both the central atoms are sp3 hybridized Explain.
Advertisements
उत्तर
- The ammonia molecule has sp3 hybridization. The expected bond angle is 109°28′. But the actual bond angle is 107°18′. It is due to the following reasons:
- One lone pair and three bond pairs are present in the ammonia molecule.
- The strength of lone pair-bond pair repulsion is much higher than that of bond pair-bond pair repulsion.
- Due to these repulsions, there is a small decrease in bond angle (∼2°) from 109°28′ to 107°18′.
- The water molecule has sp3 hybridization. The expected bond angle is 109°28′. But the actual bond angle is 104°35′. It is due to the following reasons:
- Two lone pairs and two bond pairs are present in the water molecules.
- The decreasing order of the repulsion is Lone pair-Lone pair > Lone pair-Bond pair > Bond pair-Bond pair.
- Due to these repulsions, there is a small decrease in bond angle (∼5°) from 109°28′ to 104°35′.
APPEARS IN
संबंधित प्रश्न
Select and write the most appropriate alternatives from the given choices.
The angle between the two covalent bonds is minimum in:
Give a reason for HF is a polar molecule
Which type of hybridization is present in the ammonia molecule?
Write the geometry and bond angle present in ammonia.
F-Be-F is a liner molecule but H-O-H is angular. Explain.
In the case of bond formation in Acetylene molecule: How many covalent bonds are formed?
In the case of bond formation in Acetylene molecule: State number of sigma and pi bonds formed.
In the case of bond formation in Acetylene molecule: Name the type of Hybridization.
Define Bond Enthalpy
Define Bond Length
Predict the shape and bond angles in the following molecule:
NF3
Predict the shape and bond angles in the following molecule:
HCN
Using data from the Table, answer the following:
| Examples | C2H6 Ethane | C2H4 Ethene | C2H2 Ethyne |
| Structure |
\[\begin{array}{cc} \backslash \phantom{......}/\phantom{.}\\ \ce{—C – C —}\\ /\phantom{......}\backslash\phantom{.}\end{array}\] |
\[\begin{array}{cc} \backslash \phantom{......}/\\ \ce{C \text{=} C}\\ /\phantom{......}\backslash\end{array}\] |
\[\ce{- C ≡ C -}\] |
| Type of bond between carbons | single | double | triple |
| Bond length (nm) | 0.154 | 0.134 | 0.120 |
| Bond Enthalpy kJ mol-1 | 348 | 612 | 837 |
- What happens to the bond length when unsaturation increases?
- Which is the most stable compound?
- Indicate the relationship between bond strength and Bond enthalpy.
- Comment on the overall relation between Bond length, Bond Enthalpy, and Bond strength and stability.
Write the formula to calculate the bond order of molecule.
The CORRECT order of C-X bond polarity is ____________.
In gas phase H-O-O-H bond angle in H2O2 is ______.
What is the value of C-O-H bond angle in CH3_OH?
What is the H-S-H bond angle in H2S?
The hybridization and bond angle in BeCl2 molecule are ____________ respectively.
Consider the reactions.
\[\ce{C_{(s)} + 2H2_{(g)} -> CH4_{(g)}}\], ΔH = −x kcal
\[\ce{C_{(g)} + 4H_{(g)} -> CH4_{(g)}}\], ΔH = −x1 kcal
\[\ce{CH4_{(g)} -> CH3_{(g)} + H_{(g)}}\], ΔH = +y kcal
The average C-H bond enthalpy is:
Which of the following pairs have identical bond order?
Identify the CORRECT option.
What is the bond order of B2 molecule?
What is the bond order of Be2 molecule?
Consider the ions/molecule:
\[\ce{O^+_2, O_2, O^-_2, O^{2-}_2}\]
For increasing bond order the correct option is:
What is the bona order of O2 molecules?
