314221
When sodium metal is dropped in liquid \(\mathrm{\mathrm{NH}_{3}}\), it forms \(\mathrm{\mathrm{Na}^{+}}\)and gets ammoniated. Which of the following forces are responsible for the formation of ammoniated sodium ion?
1 Ion - induced dipole
2 Dipole-dipole
3 Ion-dipole
4 Dipole-induced dipole
Explanation:
Between \(\mathrm{\mathrm{Na}^{+}}\)and \(\mathrm{\mathrm{NH}_{3}}\), ion dipole attractions are present in ammoniated sodium ion.
CHXI06:STATES OF MATTER
314222
The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles but their magnitude depends upon
1 Charge of interacting particles
2 Mass of interacting particles
3 Polarisablility of interacting particles
4 Strength of permanent dipoles in the particles
Explanation:
London forces operate only over very short distance. The energy of interaction varies as \(\mathrm{1 / r^{6}}\). Larger or more complex are the molecules, greater is the magnitude of London forces. This is obviously due to the fact that the large electron clouds are easily distorted or polarised. Hence, greater the polarisability of the interacting particles, greater is the magnitude of the interaction energy.
NCERT Exemplar
CHXI06:STATES OF MATTER
314223
Dipole-Induced dipole interactions are present in which of the following pairs?
1 \(\mathrm{\mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{CCl}_{4}}\)
2 \(\mathrm{\mathrm{HCl}}\) and \(\mathrm{\mathrm{He}}\) atoms
3 \(\mathrm{\mathrm{SiF}_{4}}\) and He atoms
4 \(\mathrm{\mathrm{H}_{2} \mathrm{O}}\) and alcohol
Explanation:
Dipole-induced dipole interactions are present in the pair in which the first species is polar and the other is non-polar. Both \(\mathrm{\mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{CCl}_{4}}\) are non-polar so there exists induced dipole-induced dipole interaction in between them. The same is true for \(\mathrm{\mathrm{SiF}_{4}}\) and He atoms pair. In \(\mathrm{\mathrm{H}_{2} \mathrm{O}}\) and alcohol, both are polar molecule, so there exists dipole-dipole interaction in between them. \(\mathrm{\mathrm{HCl}}\) is a polar molecule, whereas \(\mathrm{\mathrm{He}}\) atoms are non-polar, so in between them dipole-induced dipole interactions exist.
CHXI06:STATES OF MATTER
314224
Dipole-dipole forces act between the molecules possessing permanent dipole. Ends of dipoles possess partial charges. The partial charge is
1 more than unit electronic charge
2 equal to unit electronic charge
3 less than unit electronic charge
4 double the unit electronic charge
Explanation:
Partial charge is small charge developed by displacement of electrons. It is less than unit electric charge.
314221
When sodium metal is dropped in liquid \(\mathrm{\mathrm{NH}_{3}}\), it forms \(\mathrm{\mathrm{Na}^{+}}\)and gets ammoniated. Which of the following forces are responsible for the formation of ammoniated sodium ion?
1 Ion - induced dipole
2 Dipole-dipole
3 Ion-dipole
4 Dipole-induced dipole
Explanation:
Between \(\mathrm{\mathrm{Na}^{+}}\)and \(\mathrm{\mathrm{NH}_{3}}\), ion dipole attractions are present in ammoniated sodium ion.
CHXI06:STATES OF MATTER
314222
The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles but their magnitude depends upon
1 Charge of interacting particles
2 Mass of interacting particles
3 Polarisablility of interacting particles
4 Strength of permanent dipoles in the particles
Explanation:
London forces operate only over very short distance. The energy of interaction varies as \(\mathrm{1 / r^{6}}\). Larger or more complex are the molecules, greater is the magnitude of London forces. This is obviously due to the fact that the large electron clouds are easily distorted or polarised. Hence, greater the polarisability of the interacting particles, greater is the magnitude of the interaction energy.
NCERT Exemplar
CHXI06:STATES OF MATTER
314223
Dipole-Induced dipole interactions are present in which of the following pairs?
1 \(\mathrm{\mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{CCl}_{4}}\)
2 \(\mathrm{\mathrm{HCl}}\) and \(\mathrm{\mathrm{He}}\) atoms
3 \(\mathrm{\mathrm{SiF}_{4}}\) and He atoms
4 \(\mathrm{\mathrm{H}_{2} \mathrm{O}}\) and alcohol
Explanation:
Dipole-induced dipole interactions are present in the pair in which the first species is polar and the other is non-polar. Both \(\mathrm{\mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{CCl}_{4}}\) are non-polar so there exists induced dipole-induced dipole interaction in between them. The same is true for \(\mathrm{\mathrm{SiF}_{4}}\) and He atoms pair. In \(\mathrm{\mathrm{H}_{2} \mathrm{O}}\) and alcohol, both are polar molecule, so there exists dipole-dipole interaction in between them. \(\mathrm{\mathrm{HCl}}\) is a polar molecule, whereas \(\mathrm{\mathrm{He}}\) atoms are non-polar, so in between them dipole-induced dipole interactions exist.
CHXI06:STATES OF MATTER
314224
Dipole-dipole forces act between the molecules possessing permanent dipole. Ends of dipoles possess partial charges. The partial charge is
1 more than unit electronic charge
2 equal to unit electronic charge
3 less than unit electronic charge
4 double the unit electronic charge
Explanation:
Partial charge is small charge developed by displacement of electrons. It is less than unit electric charge.
314221
When sodium metal is dropped in liquid \(\mathrm{\mathrm{NH}_{3}}\), it forms \(\mathrm{\mathrm{Na}^{+}}\)and gets ammoniated. Which of the following forces are responsible for the formation of ammoniated sodium ion?
1 Ion - induced dipole
2 Dipole-dipole
3 Ion-dipole
4 Dipole-induced dipole
Explanation:
Between \(\mathrm{\mathrm{Na}^{+}}\)and \(\mathrm{\mathrm{NH}_{3}}\), ion dipole attractions are present in ammoniated sodium ion.
CHXI06:STATES OF MATTER
314222
The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles but their magnitude depends upon
1 Charge of interacting particles
2 Mass of interacting particles
3 Polarisablility of interacting particles
4 Strength of permanent dipoles in the particles
Explanation:
London forces operate only over very short distance. The energy of interaction varies as \(\mathrm{1 / r^{6}}\). Larger or more complex are the molecules, greater is the magnitude of London forces. This is obviously due to the fact that the large electron clouds are easily distorted or polarised. Hence, greater the polarisability of the interacting particles, greater is the magnitude of the interaction energy.
NCERT Exemplar
CHXI06:STATES OF MATTER
314223
Dipole-Induced dipole interactions are present in which of the following pairs?
1 \(\mathrm{\mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{CCl}_{4}}\)
2 \(\mathrm{\mathrm{HCl}}\) and \(\mathrm{\mathrm{He}}\) atoms
3 \(\mathrm{\mathrm{SiF}_{4}}\) and He atoms
4 \(\mathrm{\mathrm{H}_{2} \mathrm{O}}\) and alcohol
Explanation:
Dipole-induced dipole interactions are present in the pair in which the first species is polar and the other is non-polar. Both \(\mathrm{\mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{CCl}_{4}}\) are non-polar so there exists induced dipole-induced dipole interaction in between them. The same is true for \(\mathrm{\mathrm{SiF}_{4}}\) and He atoms pair. In \(\mathrm{\mathrm{H}_{2} \mathrm{O}}\) and alcohol, both are polar molecule, so there exists dipole-dipole interaction in between them. \(\mathrm{\mathrm{HCl}}\) is a polar molecule, whereas \(\mathrm{\mathrm{He}}\) atoms are non-polar, so in between them dipole-induced dipole interactions exist.
CHXI06:STATES OF MATTER
314224
Dipole-dipole forces act between the molecules possessing permanent dipole. Ends of dipoles possess partial charges. The partial charge is
1 more than unit electronic charge
2 equal to unit electronic charge
3 less than unit electronic charge
4 double the unit electronic charge
Explanation:
Partial charge is small charge developed by displacement of electrons. It is less than unit electric charge.
314221
When sodium metal is dropped in liquid \(\mathrm{\mathrm{NH}_{3}}\), it forms \(\mathrm{\mathrm{Na}^{+}}\)and gets ammoniated. Which of the following forces are responsible for the formation of ammoniated sodium ion?
1 Ion - induced dipole
2 Dipole-dipole
3 Ion-dipole
4 Dipole-induced dipole
Explanation:
Between \(\mathrm{\mathrm{Na}^{+}}\)and \(\mathrm{\mathrm{NH}_{3}}\), ion dipole attractions are present in ammoniated sodium ion.
CHXI06:STATES OF MATTER
314222
The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles but their magnitude depends upon
1 Charge of interacting particles
2 Mass of interacting particles
3 Polarisablility of interacting particles
4 Strength of permanent dipoles in the particles
Explanation:
London forces operate only over very short distance. The energy of interaction varies as \(\mathrm{1 / r^{6}}\). Larger or more complex are the molecules, greater is the magnitude of London forces. This is obviously due to the fact that the large electron clouds are easily distorted or polarised. Hence, greater the polarisability of the interacting particles, greater is the magnitude of the interaction energy.
NCERT Exemplar
CHXI06:STATES OF MATTER
314223
Dipole-Induced dipole interactions are present in which of the following pairs?
1 \(\mathrm{\mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{CCl}_{4}}\)
2 \(\mathrm{\mathrm{HCl}}\) and \(\mathrm{\mathrm{He}}\) atoms
3 \(\mathrm{\mathrm{SiF}_{4}}\) and He atoms
4 \(\mathrm{\mathrm{H}_{2} \mathrm{O}}\) and alcohol
Explanation:
Dipole-induced dipole interactions are present in the pair in which the first species is polar and the other is non-polar. Both \(\mathrm{\mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{CCl}_{4}}\) are non-polar so there exists induced dipole-induced dipole interaction in between them. The same is true for \(\mathrm{\mathrm{SiF}_{4}}\) and He atoms pair. In \(\mathrm{\mathrm{H}_{2} \mathrm{O}}\) and alcohol, both are polar molecule, so there exists dipole-dipole interaction in between them. \(\mathrm{\mathrm{HCl}}\) is a polar molecule, whereas \(\mathrm{\mathrm{He}}\) atoms are non-polar, so in between them dipole-induced dipole interactions exist.
CHXI06:STATES OF MATTER
314224
Dipole-dipole forces act between the molecules possessing permanent dipole. Ends of dipoles possess partial charges. The partial charge is
1 more than unit electronic charge
2 equal to unit electronic charge
3 less than unit electronic charge
4 double the unit electronic charge
Explanation:
Partial charge is small charge developed by displacement of electrons. It is less than unit electric charge.
