313877
Statement A : \({\rm{B}}{{\rm{F}}_{\rm{3}}}\) molecule has zero dipole moment. Statement B : F is electronegative and B-F bonds are polar in nature.
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
\({\rm{B}}{{\rm{F}}_{\rm{3}}}\) is \({\rm{s}}{{\rm{p}}^{\rm{2}}}\) hybridized. Dipole moment is a vector quantity. The three bond moments give a net sum of zero, as the resultant of any two is equal andopposite to the third. So, the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313878
The total number of pairs from the following having both compounds with net non-zero dipole moment is
Dipole moment of \({\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}\) is +1.60 D and that of \({\rm{CHC}}{{\rm{l}}_3}\) is +1.80 D .
JEE - 2023
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313879
Which of the possible molecule/species is having maximum value for dipole moment (where " \({\text{A}}\) " is the central atom)?
1 \(\mathrm{AX}_{3}\) (having one lone pair on central atom)
2 \(\mathrm{AX}_{4}\) (Tetrahedral)
3 \(\mathrm{AX}_{3} \mathrm{Y}\) (having no lone pair on central atom)
4 Can't be predicted
Explanation:
Dipole moment will be more when lone pair of electrons are present on central atom.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313880
Which of the following is polar?
1 \(\mathrm{I}^{-}{ }_{3}\)
2 \(\mathrm{CO}^{2-}{ }_{3}\)
3 \(\mathrm{XeF}_{4}\)
4 \(\mathrm{PF}_{3}\)
Explanation:
\(\mathrm{PF}_{3}\) is triangular pyramidal, so its net dipole moment is not zero. \(\therefore \mathrm{PF}_{3}\) is polar. Rest of the compounds have symmetrical shape. Thus, they are non-polar.
313877
Statement A : \({\rm{B}}{{\rm{F}}_{\rm{3}}}\) molecule has zero dipole moment. Statement B : F is electronegative and B-F bonds are polar in nature.
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
\({\rm{B}}{{\rm{F}}_{\rm{3}}}\) is \({\rm{s}}{{\rm{p}}^{\rm{2}}}\) hybridized. Dipole moment is a vector quantity. The three bond moments give a net sum of zero, as the resultant of any two is equal andopposite to the third. So, the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313878
The total number of pairs from the following having both compounds with net non-zero dipole moment is
Dipole moment of \({\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}\) is +1.60 D and that of \({\rm{CHC}}{{\rm{l}}_3}\) is +1.80 D .
JEE - 2023
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313879
Which of the possible molecule/species is having maximum value for dipole moment (where " \({\text{A}}\) " is the central atom)?
1 \(\mathrm{AX}_{3}\) (having one lone pair on central atom)
2 \(\mathrm{AX}_{4}\) (Tetrahedral)
3 \(\mathrm{AX}_{3} \mathrm{Y}\) (having no lone pair on central atom)
4 Can't be predicted
Explanation:
Dipole moment will be more when lone pair of electrons are present on central atom.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313880
Which of the following is polar?
1 \(\mathrm{I}^{-}{ }_{3}\)
2 \(\mathrm{CO}^{2-}{ }_{3}\)
3 \(\mathrm{XeF}_{4}\)
4 \(\mathrm{PF}_{3}\)
Explanation:
\(\mathrm{PF}_{3}\) is triangular pyramidal, so its net dipole moment is not zero. \(\therefore \mathrm{PF}_{3}\) is polar. Rest of the compounds have symmetrical shape. Thus, they are non-polar.
313877
Statement A : \({\rm{B}}{{\rm{F}}_{\rm{3}}}\) molecule has zero dipole moment. Statement B : F is electronegative and B-F bonds are polar in nature.
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
\({\rm{B}}{{\rm{F}}_{\rm{3}}}\) is \({\rm{s}}{{\rm{p}}^{\rm{2}}}\) hybridized. Dipole moment is a vector quantity. The three bond moments give a net sum of zero, as the resultant of any two is equal andopposite to the third. So, the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313878
The total number of pairs from the following having both compounds with net non-zero dipole moment is
Dipole moment of \({\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}\) is +1.60 D and that of \({\rm{CHC}}{{\rm{l}}_3}\) is +1.80 D .
JEE - 2023
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313879
Which of the possible molecule/species is having maximum value for dipole moment (where " \({\text{A}}\) " is the central atom)?
1 \(\mathrm{AX}_{3}\) (having one lone pair on central atom)
2 \(\mathrm{AX}_{4}\) (Tetrahedral)
3 \(\mathrm{AX}_{3} \mathrm{Y}\) (having no lone pair on central atom)
4 Can't be predicted
Explanation:
Dipole moment will be more when lone pair of electrons are present on central atom.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313880
Which of the following is polar?
1 \(\mathrm{I}^{-}{ }_{3}\)
2 \(\mathrm{CO}^{2-}{ }_{3}\)
3 \(\mathrm{XeF}_{4}\)
4 \(\mathrm{PF}_{3}\)
Explanation:
\(\mathrm{PF}_{3}\) is triangular pyramidal, so its net dipole moment is not zero. \(\therefore \mathrm{PF}_{3}\) is polar. Rest of the compounds have symmetrical shape. Thus, they are non-polar.
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313877
Statement A : \({\rm{B}}{{\rm{F}}_{\rm{3}}}\) molecule has zero dipole moment. Statement B : F is electronegative and B-F bonds are polar in nature.
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
\({\rm{B}}{{\rm{F}}_{\rm{3}}}\) is \({\rm{s}}{{\rm{p}}^{\rm{2}}}\) hybridized. Dipole moment is a vector quantity. The three bond moments give a net sum of zero, as the resultant of any two is equal andopposite to the third. So, the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313878
The total number of pairs from the following having both compounds with net non-zero dipole moment is
Dipole moment of \({\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}\) is +1.60 D and that of \({\rm{CHC}}{{\rm{l}}_3}\) is +1.80 D .
JEE - 2023
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313879
Which of the possible molecule/species is having maximum value for dipole moment (where " \({\text{A}}\) " is the central atom)?
1 \(\mathrm{AX}_{3}\) (having one lone pair on central atom)
2 \(\mathrm{AX}_{4}\) (Tetrahedral)
3 \(\mathrm{AX}_{3} \mathrm{Y}\) (having no lone pair on central atom)
4 Can't be predicted
Explanation:
Dipole moment will be more when lone pair of electrons are present on central atom.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313880
Which of the following is polar?
1 \(\mathrm{I}^{-}{ }_{3}\)
2 \(\mathrm{CO}^{2-}{ }_{3}\)
3 \(\mathrm{XeF}_{4}\)
4 \(\mathrm{PF}_{3}\)
Explanation:
\(\mathrm{PF}_{3}\) is triangular pyramidal, so its net dipole moment is not zero. \(\therefore \mathrm{PF}_{3}\) is polar. Rest of the compounds have symmetrical shape. Thus, they are non-polar.
