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A neutral molecule XF(3) has a zero dipl...

A neutral molecule `XF_(3)` has a zero diple moment. The element X is most likely :

A

chlorine

B

boron

C

nitrogen

D

carbon

Text Solution

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The correct Answer is:
To determine which element X in the molecule \( XF_3 \) has a zero dipole moment, we will analyze the possible candidates: chlorine (Cl), boron (B), nitrogen (N), and carbon (C). ### Step-by-Step Solution: 1. **Identify the molecular structure of \( XF_3 \)**: - The molecule consists of one atom of element X and three fluorine (F) atoms. 2. **Consider each candidate for X**: - **Candidate 1: Chlorine (Cl)** - Chlorine has 7 valence electrons. In \( ClF_3 \), it will use 3 electrons to bond with 3 fluorine atoms, leaving 2 lone pairs. - The molecular geometry is **T-shaped** due to the presence of lone pairs. - The dipoles from the fluorine atoms do not cancel out completely because of the asymmetrical shape, resulting in a **non-zero dipole moment**. - **Candidate 2: Boron (B)** - Boron has 3 valence electrons and will use all of them to bond with 3 fluorine atoms, resulting in no lone pairs. - The molecular geometry is **trigonal planar**. - The dipoles from the three fluorine atoms will cancel each other out perfectly, leading to a **zero dipole moment**. This makes boron a strong candidate. - **Candidate 3: Nitrogen (N)** - Nitrogen has 5 valence electrons. In \( NF_3 \), it will use 3 electrons to bond with 3 fluorine atoms, leaving 1 lone pair. - The molecular geometry is **trigonal pyramidal** due to the lone pair. - The dipoles do not cancel out completely, resulting in a **non-zero dipole moment**. - **Candidate 4: Carbon (C)** - Carbon has 4 valence electrons. In \( CF_3 \), it will use all 4 electrons to bond with 3 fluorine atoms, leaving 1 lone pair. - The molecular geometry is also **trigonal pyramidal**. - Similar to nitrogen, the dipoles do not cancel out completely, resulting in a **non-zero dipole moment**. 3. **Conclusion**: - After analyzing all candidates, the only element that results in a zero dipole moment for the molecule \( XF_3 \) is **Boron (B)**. ### Final Answer: The element X is most likely **Boron (B)**.
To determine which element X in the molecule \( XF_3 \) has a zero dipole moment, we will analyze the possible candidates: chlorine (Cl), boron (B), nitrogen (N), and carbon (C). ### Step-by-Step Solution: 1. **Identify the molecular structure of \( XF_3 \)**: - The molecule consists of one atom of element X and three fluorine (F) atoms. 2. **Consider each candidate for X**: ...
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Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. Which is a polar molecule?

Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. Which is a polar molecule?