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In which of the following molecule are all the bonds not equal ?
- a)NF3
- b)CIF3
- c)BF3
- d)AlF3
Correct answer is option 'B'. Can you explain this answer?
Verified Answer
In which of the following molecule are all the bonds not equal ?a)NF3b...
In CIF3, all the bonds are not equal due to the presence of a lone pair of electrons on the central chlorine atom. This molecule has a T-shaped molecular geometry, and the presence of the lone pair leads to differences in the bond angles and bond lengths.
The central chlorine atom in this molecule is bonded to three fluorine atoms and has one lone pair of electrons. The VSEPR theory predicts a T-shaped geometry for this molecule. The presence of the lone pair on the chlorine atom causes repulsion, leading to unequal bond angles and bond lengths between the chlorine and fluorine atoms. Therefore, all the bonds in CIF3 are not equal.
The central chlorine atom in this molecule is bonded to three fluorine atoms and has one lone pair of electrons. The VSEPR theory predicts a T-shaped geometry for this molecule. The presence of the lone pair on the chlorine atom causes repulsion, leading to unequal bond angles and bond lengths between the chlorine and fluorine atoms. Therefore, all the bonds in CIF3 are not equal.
Most Upvoted Answer
In which of the following molecule are all the bonds not equal ?a)NF3b...
In CIF3, all the bonds are not equal due to the presence of a lone pair of electrons on the central chlorine atom. This molecule has a T-shaped molecular geometry, and the presence of the lone pair leads to differences in the bond angles and bond lengths.
The central chlorine atom in this molecule is bonded to three fluorine atoms and has one lone pair of electrons. The VSEPR theory predicts a T-shaped geometry for this molecule. The presence of the lone pair on the chlorine atom causes repulsion, leading to unequal bond angles and bond lengths between the chlorine and fluorine atoms. Therefore, all the bonds in CIF3 are not equal.
The central chlorine atom in this molecule is bonded to three fluorine atoms and has one lone pair of electrons. The VSEPR theory predicts a T-shaped geometry for this molecule. The presence of the lone pair on the chlorine atom causes repulsion, leading to unequal bond angles and bond lengths between the chlorine and fluorine atoms. Therefore, all the bonds in CIF3 are not equal.
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Community Answer
In which of the following molecule are all the bonds not equal ?a)NF3b...
Explanation:
The molecule that has all the bonds not equal is CIF3.
Reason:
In CIF3, the central atom is chlorine (Cl) and it is surrounded by three fluorine (F) atoms. The chlorine atom is more electronegative than the fluorine atoms, which means it has a stronger pull on the shared electrons. As a result, the bonds between chlorine and fluorine are polar covalent bonds.
Bond Length:
The bond length between the central chlorine atom and the fluorine atoms is not equal in CIF3. This is because the electronegativity difference between chlorine and fluorine causes an uneven distribution of electron density in the molecule. The bond length is shorter between chlorine and the fluorine atom closest to it, and longer between chlorine and the other two fluorine atoms.
Electron Density:
The uneven distribution of electron density is due to the lone pair of electrons on the chlorine atom. Chlorine has one lone pair of electrons, which repels the bonding electron pairs. As a result, the bond length between chlorine and the fluorine atom closest to it is shorter.
Overall Structure:
The CIF3 molecule has a trigonal bipyramidal structure, with the chlorine atom at the center and the three fluorine atoms arranged in a trigonal planar fashion. The shorter bond length between chlorine and the fluorine atom closest to it gives the molecule a distorted shape, where the bond angles are not equal.
Conclusion:
In CIF3, all the bonds are not equal due to the difference in electronegativity between chlorine and fluorine. The bond length is shorter between chlorine and the fluorine atom closest to it, leading to a distorted shape and unequal bond angles.
The molecule that has all the bonds not equal is CIF3.
Reason:
In CIF3, the central atom is chlorine (Cl) and it is surrounded by three fluorine (F) atoms. The chlorine atom is more electronegative than the fluorine atoms, which means it has a stronger pull on the shared electrons. As a result, the bonds between chlorine and fluorine are polar covalent bonds.
Bond Length:
The bond length between the central chlorine atom and the fluorine atoms is not equal in CIF3. This is because the electronegativity difference between chlorine and fluorine causes an uneven distribution of electron density in the molecule. The bond length is shorter between chlorine and the fluorine atom closest to it, and longer between chlorine and the other two fluorine atoms.
Electron Density:
The uneven distribution of electron density is due to the lone pair of electrons on the chlorine atom. Chlorine has one lone pair of electrons, which repels the bonding electron pairs. As a result, the bond length between chlorine and the fluorine atom closest to it is shorter.
Overall Structure:
The CIF3 molecule has a trigonal bipyramidal structure, with the chlorine atom at the center and the three fluorine atoms arranged in a trigonal planar fashion. The shorter bond length between chlorine and the fluorine atom closest to it gives the molecule a distorted shape, where the bond angles are not equal.
Conclusion:
In CIF3, all the bonds are not equal due to the difference in electronegativity between chlorine and fluorine. The bond length is shorter between chlorine and the fluorine atom closest to it, leading to a distorted shape and unequal bond angles.
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