Question:
In which of the following pairs, both molecules possess dipole moment?
In which of the following pairs, both molecules possess dipole moment?
Show Hint
Molecules with symmetric geometry (linear, trigonal planar) usually have zero dipole moment.
Updated On: May 18, 2025
- \( CO_2, BCl_3 \)
- \( BCl_3, NF_3 \)
- \( CO_2, SO_2 \)
- \( SO_2, NF_3 \)
Show Solution
Verified By Collegedunia
The Correct Option is D
Approach Solution - 1
Step 1: Identify Molecular Geometry and Dipole Moments
- \( CO_2 \) and \( BCl_3 \) are symmetric → No dipole moment.
- \( SO_2 \) (bent) and \( NF_3 \) (pyramidal) → Have dipole moment.
Step 2: Correct Pair \[ SO_2, NF_3 \]
Was this answer helpful?
0
0
Show Solution
Verified By Collegedunia
Approach Solution -2
To determine whether molecules possess a dipole moment, we need to consider their molecular geometry and the electronegativity difference between atoms.
1. \( SO_2 \) (Sulfur dioxide):
- Molecular shape: Bent (angular)
- The S–O bonds are polar due to electronegativity difference.
- The bent shape means the bond dipoles do not cancel out.
- Hence, \( SO_2 \) has a net dipole moment.
2. \( NF_3 \) (Nitrogen trifluoride):
- Molecular shape: Trigonal pyramidal (like ammonia)
- N–F bonds are polar.
- The lone pair on nitrogen causes the bond dipoles to not cancel completely.
- Therefore, \( NF_3 \) has a net dipole moment, though smaller than ammonia.
Therefore, in the pair \( SO_2 \) and \( NF_3 \), both molecules possess dipole moments.
Hence, the correct answer is:
\( SO_2, NF_3 \)
1. \( SO_2 \) (Sulfur dioxide):
- Molecular shape: Bent (angular)
- The S–O bonds are polar due to electronegativity difference.
- The bent shape means the bond dipoles do not cancel out.
- Hence, \( SO_2 \) has a net dipole moment.
2. \( NF_3 \) (Nitrogen trifluoride):
- Molecular shape: Trigonal pyramidal (like ammonia)
- N–F bonds are polar.
- The lone pair on nitrogen causes the bond dipoles to not cancel completely.
- Therefore, \( NF_3 \) has a net dipole moment, though smaller than ammonia.
Therefore, in the pair \( SO_2 \) and \( NF_3 \), both molecules possess dipole moments.
Hence, the correct answer is:
\( SO_2, NF_3 \)
Was this answer helpful?
0
0
Top AP EAPCET Chemistry Questions
- The four quantum numbers of the valence electron of potassium are :
- The volume of $0.02\, M$ acidified permanganate solution required for complete reaction of $60\, mL$ of $0.01\, MI^{-}$ ion solution to form $I_2$ in $mL$ is
- In which of the following the election gain enthalpy of elements is correctly arranged?
- The radii of $ \text{F,}{{\text{F}}^{-}}\text{O} $ and $ {{\text{O}}^{2-}} $ are in the order
- Which of the following has the highest first ionization potential?
View More Questions
Top AP EAPCET Questions
- A body is projected from the ground at an angle of $\tan^{-1} \left( \frac{8}{7}\right)$ with the horizontal. The ratio of the maximum height attained by it to its range is
- The four quantum numbers of the valence electron of potassium are :
- A lens forms real and virtual images of an object, when the object is at $u_{1}$ and $u_{2}$ distances respectively. If the size of the virtual image is double that of the real image, then the focal length of the lens is (take, the magnification of the real image as $m$ )
- Two spheres $P$ and $Q$, each of mass $200\, g$ are attached to a string of length one metre as shown in the figure. The string and the spheres are then whirled in a horizontal circle about $O$ at a constant angular speed. The ratio of the tension in the string between $P$ and $Q$ to that of between $P$ and $O$ is $(P$ is at mid-point of the line joining $O$ and $Q$ )
- The volume of $0.02\, M$ acidified permanganate solution required for complete reaction of $60\, mL$ of $0.01\, MI^{-}$ ion solution to form $I_2$ in $mL$ is
View More Questions