313881
A diatomic molecule has a dipole moment of 1.2 D. If its bond distance is \({\rm{1}}{\rm{.0}}{\mkern 1mu} {\rm{A^\circ }}\), what fraction of an electronic charge exists on each atom?
1 0.85
2 0.65
3 0.45
4 0.25
Explanation:
For a diatomic molecule dipole moment \({\rm{\mu = e \times d}}\) \(\therefore \) electronic charge \({\rm{ = }}\frac{{\rm{\mu }}}{{\rm{d}}}{\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 18}}}}\,\,{\rm{esu}}\,\,{\rm{cm}}}}{{{\rm{1}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{ - 8}}}}\,\,{\rm{cm}}}}\) \({\rm{ = }}\,\,{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}\) Actual value of electronic charge \({\rm{ = 4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}{\rm{.}}\) \(\therefore \) Fraction of the electronic charge \({\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{{{\rm{4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{\rm{ = 0}}{\rm{.25}}{\rm{.}}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313882
The correct order of decreasing bond polarity is
As the EN difference decreases, the bond polarity decreases accordingly.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313883
Bond polarity of diatomic molecule is because of
1 Difference in electron affinities of two atoms
2 Difference in electronegativities of two atoms
3 Difference in ionisation potentials
4 All of the above
Explanation:
In case of diatomic molecule, the greater difference of electronegativities of the two atoms leads to greater polarity.
AIIMS - 2013
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313884
The electronegativity of O, F, N, Cl and H are 3.5, 4.0, 3.0, 3.0 and 2.1 respectively. The strongest bond will be :
1 F – O
2 O – Cl
3 N – H
4 O – H
Explanation:
Bond strength \( \propto \) Difference in electronegativity of atoms.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313885
Assertion : \(\mathrm{NaCl}\) is more ionic than \(\mathrm{LiCl}\). Reason : Greater the size of cation, greater is the polarising power.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
In the case of \(\mathrm{LiCl}\), the smaller \(\mathrm{Li}^{+}\)cation can polarize the electron cloud of the larger \(\mathrm{Cl}^{-}\)anion more effectively, leading to a stronger partial covalent character in the \(\mathrm{Li}-\mathrm{Cl}\) bond. On the other hand, in \(\mathrm{NaCl}\), the larger size of the \(\mathrm{Na}^{+}\)cation results in less effective polarization, and the ionic bond is primarily ionic in nature. So the option (3) is correct.
313881
A diatomic molecule has a dipole moment of 1.2 D. If its bond distance is \({\rm{1}}{\rm{.0}}{\mkern 1mu} {\rm{A^\circ }}\), what fraction of an electronic charge exists on each atom?
1 0.85
2 0.65
3 0.45
4 0.25
Explanation:
For a diatomic molecule dipole moment \({\rm{\mu = e \times d}}\) \(\therefore \) electronic charge \({\rm{ = }}\frac{{\rm{\mu }}}{{\rm{d}}}{\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 18}}}}\,\,{\rm{esu}}\,\,{\rm{cm}}}}{{{\rm{1}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{ - 8}}}}\,\,{\rm{cm}}}}\) \({\rm{ = }}\,\,{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}\) Actual value of electronic charge \({\rm{ = 4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}{\rm{.}}\) \(\therefore \) Fraction of the electronic charge \({\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{{{\rm{4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{\rm{ = 0}}{\rm{.25}}{\rm{.}}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313882
The correct order of decreasing bond polarity is
As the EN difference decreases, the bond polarity decreases accordingly.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313883
Bond polarity of diatomic molecule is because of
1 Difference in electron affinities of two atoms
2 Difference in electronegativities of two atoms
3 Difference in ionisation potentials
4 All of the above
Explanation:
In case of diatomic molecule, the greater difference of electronegativities of the two atoms leads to greater polarity.
AIIMS - 2013
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313884
The electronegativity of O, F, N, Cl and H are 3.5, 4.0, 3.0, 3.0 and 2.1 respectively. The strongest bond will be :
1 F – O
2 O – Cl
3 N – H
4 O – H
Explanation:
Bond strength \( \propto \) Difference in electronegativity of atoms.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313885
Assertion : \(\mathrm{NaCl}\) is more ionic than \(\mathrm{LiCl}\). Reason : Greater the size of cation, greater is the polarising power.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
In the case of \(\mathrm{LiCl}\), the smaller \(\mathrm{Li}^{+}\)cation can polarize the electron cloud of the larger \(\mathrm{Cl}^{-}\)anion more effectively, leading to a stronger partial covalent character in the \(\mathrm{Li}-\mathrm{Cl}\) bond. On the other hand, in \(\mathrm{NaCl}\), the larger size of the \(\mathrm{Na}^{+}\)cation results in less effective polarization, and the ionic bond is primarily ionic in nature. So the option (3) is correct.
313881
A diatomic molecule has a dipole moment of 1.2 D. If its bond distance is \({\rm{1}}{\rm{.0}}{\mkern 1mu} {\rm{A^\circ }}\), what fraction of an electronic charge exists on each atom?
1 0.85
2 0.65
3 0.45
4 0.25
Explanation:
For a diatomic molecule dipole moment \({\rm{\mu = e \times d}}\) \(\therefore \) electronic charge \({\rm{ = }}\frac{{\rm{\mu }}}{{\rm{d}}}{\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 18}}}}\,\,{\rm{esu}}\,\,{\rm{cm}}}}{{{\rm{1}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{ - 8}}}}\,\,{\rm{cm}}}}\) \({\rm{ = }}\,\,{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}\) Actual value of electronic charge \({\rm{ = 4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}{\rm{.}}\) \(\therefore \) Fraction of the electronic charge \({\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{{{\rm{4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{\rm{ = 0}}{\rm{.25}}{\rm{.}}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313882
The correct order of decreasing bond polarity is
As the EN difference decreases, the bond polarity decreases accordingly.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313883
Bond polarity of diatomic molecule is because of
1 Difference in electron affinities of two atoms
2 Difference in electronegativities of two atoms
3 Difference in ionisation potentials
4 All of the above
Explanation:
In case of diatomic molecule, the greater difference of electronegativities of the two atoms leads to greater polarity.
AIIMS - 2013
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313884
The electronegativity of O, F, N, Cl and H are 3.5, 4.0, 3.0, 3.0 and 2.1 respectively. The strongest bond will be :
1 F – O
2 O – Cl
3 N – H
4 O – H
Explanation:
Bond strength \( \propto \) Difference in electronegativity of atoms.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313885
Assertion : \(\mathrm{NaCl}\) is more ionic than \(\mathrm{LiCl}\). Reason : Greater the size of cation, greater is the polarising power.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
In the case of \(\mathrm{LiCl}\), the smaller \(\mathrm{Li}^{+}\)cation can polarize the electron cloud of the larger \(\mathrm{Cl}^{-}\)anion more effectively, leading to a stronger partial covalent character in the \(\mathrm{Li}-\mathrm{Cl}\) bond. On the other hand, in \(\mathrm{NaCl}\), the larger size of the \(\mathrm{Na}^{+}\)cation results in less effective polarization, and the ionic bond is primarily ionic in nature. So the option (3) is correct.
313881
A diatomic molecule has a dipole moment of 1.2 D. If its bond distance is \({\rm{1}}{\rm{.0}}{\mkern 1mu} {\rm{A^\circ }}\), what fraction of an electronic charge exists on each atom?
1 0.85
2 0.65
3 0.45
4 0.25
Explanation:
For a diatomic molecule dipole moment \({\rm{\mu = e \times d}}\) \(\therefore \) electronic charge \({\rm{ = }}\frac{{\rm{\mu }}}{{\rm{d}}}{\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 18}}}}\,\,{\rm{esu}}\,\,{\rm{cm}}}}{{{\rm{1}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{ - 8}}}}\,\,{\rm{cm}}}}\) \({\rm{ = }}\,\,{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}\) Actual value of electronic charge \({\rm{ = 4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}{\rm{.}}\) \(\therefore \) Fraction of the electronic charge \({\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{{{\rm{4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{\rm{ = 0}}{\rm{.25}}{\rm{.}}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313882
The correct order of decreasing bond polarity is
As the EN difference decreases, the bond polarity decreases accordingly.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313883
Bond polarity of diatomic molecule is because of
1 Difference in electron affinities of two atoms
2 Difference in electronegativities of two atoms
3 Difference in ionisation potentials
4 All of the above
Explanation:
In case of diatomic molecule, the greater difference of electronegativities of the two atoms leads to greater polarity.
AIIMS - 2013
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313884
The electronegativity of O, F, N, Cl and H are 3.5, 4.0, 3.0, 3.0 and 2.1 respectively. The strongest bond will be :
1 F – O
2 O – Cl
3 N – H
4 O – H
Explanation:
Bond strength \( \propto \) Difference in electronegativity of atoms.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313885
Assertion : \(\mathrm{NaCl}\) is more ionic than \(\mathrm{LiCl}\). Reason : Greater the size of cation, greater is the polarising power.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
In the case of \(\mathrm{LiCl}\), the smaller \(\mathrm{Li}^{+}\)cation can polarize the electron cloud of the larger \(\mathrm{Cl}^{-}\)anion more effectively, leading to a stronger partial covalent character in the \(\mathrm{Li}-\mathrm{Cl}\) bond. On the other hand, in \(\mathrm{NaCl}\), the larger size of the \(\mathrm{Na}^{+}\)cation results in less effective polarization, and the ionic bond is primarily ionic in nature. So the option (3) is correct.
313881
A diatomic molecule has a dipole moment of 1.2 D. If its bond distance is \({\rm{1}}{\rm{.0}}{\mkern 1mu} {\rm{A^\circ }}\), what fraction of an electronic charge exists on each atom?
1 0.85
2 0.65
3 0.45
4 0.25
Explanation:
For a diatomic molecule dipole moment \({\rm{\mu = e \times d}}\) \(\therefore \) electronic charge \({\rm{ = }}\frac{{\rm{\mu }}}{{\rm{d}}}{\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 18}}}}\,\,{\rm{esu}}\,\,{\rm{cm}}}}{{{\rm{1}}{\rm{.0 \times 1}}{{\rm{0}}^{{\rm{ - 8}}}}\,\,{\rm{cm}}}}\) \({\rm{ = }}\,\,{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}\) Actual value of electronic charge \({\rm{ = 4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}\,\,{\rm{esu}}{\rm{.}}\) \(\therefore \) Fraction of the electronic charge \({\rm{ = }}\frac{{{\rm{1}}{\rm{.2 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{{{\rm{4}}{\rm{.8 \times 1}}{{\rm{0}}^{{\rm{ - 10}}}}}}{\rm{ = 0}}{\rm{.25}}{\rm{.}}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313882
The correct order of decreasing bond polarity is
As the EN difference decreases, the bond polarity decreases accordingly.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313883
Bond polarity of diatomic molecule is because of
1 Difference in electron affinities of two atoms
2 Difference in electronegativities of two atoms
3 Difference in ionisation potentials
4 All of the above
Explanation:
In case of diatomic molecule, the greater difference of electronegativities of the two atoms leads to greater polarity.
AIIMS - 2013
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313884
The electronegativity of O, F, N, Cl and H are 3.5, 4.0, 3.0, 3.0 and 2.1 respectively. The strongest bond will be :
1 F – O
2 O – Cl
3 N – H
4 O – H
Explanation:
Bond strength \( \propto \) Difference in electronegativity of atoms.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313885
Assertion : \(\mathrm{NaCl}\) is more ionic than \(\mathrm{LiCl}\). Reason : Greater the size of cation, greater is the polarising power.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
In the case of \(\mathrm{LiCl}\), the smaller \(\mathrm{Li}^{+}\)cation can polarize the electron cloud of the larger \(\mathrm{Cl}^{-}\)anion more effectively, leading to a stronger partial covalent character in the \(\mathrm{Li}-\mathrm{Cl}\) bond. On the other hand, in \(\mathrm{NaCl}\), the larger size of the \(\mathrm{Na}^{+}\)cation results in less effective polarization, and the ionic bond is primarily ionic in nature. So the option (3) is correct.
