Question 1

The Pauling electronegativities of chlorine and iodine are 3.0 and 2.5 respectively. Estimate the dipole moment of iodine monochloride, ICl.

Accepted Answer

A)  0.0 D 
B)  0.5 D 
C)  2.5 D 
D)  3.0 D 
A)  0.0 D 
B)  0.5 D 
C)  2.5 D 
D)  3.0 D B

Question 2

The dipole moment of hydrogen chloride, HCl, is 1.08 D and the bond length is 127 pm. Calculate the fractional charge on the hydrogen and chlorine atoms.

Accepted Answer

A)  8.50 F1F1F1S1F1F1F10 10-3 C 
B)  2.84 F1F1F1S1F1F1F10 10-8 C 
C)  2.84 F1F1F1S1F1F1F10 10-20 C 
D)  2.84 F1F1F1S1F1F1F10 10-20 C
Title: Focus 10 - Question 02 
A)  8.50 F1F1F1S1F1F1F10 10-3 C 
B)  2.84 F1F1F1S1F1F1F10 10-8 C 
C)  2.84 F1F1F1S1F1F1F10 10-20 C 
D)  2.84 F1F1F1S1F1F1F10 10-20 C
Title: Focus 10 - Question 02 C

Question 3

The Lennard-Jones parameters for the interactions between benzene, C6H6, molecules are F1F1F1S1F1F1F10 = 454 kJ mol-1 and r0 = 527 pm. Calculate the separation that corresponds to the minimum in the Lennard-Jones potential.

Accepted Answer

A)  592 pm 
B)  527 pm 
C)  1054 pm 
D)  745 pm 
A)  592 pm 
B)  527 pm 
C)  1054 pm 
D)  745 pm A

Question 4

The atomic coordinates and partial charges for the planar molecule fluoroethene, C2H3F, are
$\begin{array}{lrrrr} 
& x / A & y / A & z / A & \text { Partial charge } \
\mathrm{C} & -0.669 & 0.019 & 0.000 & +0.353 \mathrm{e} \
\mathrm{C} & 0.669 & -0.019 & 0.000 & -0.367 e \
\mathrm{H} & 1.211 & -0.978 & 0.000 & +0.039 \mathrm{e} \
\mathrm{H} & 1.265 & 0.906 & 0.000 & +0.041 e \
\mathrm{H} & -1.257 & -0.913 & 0.000 & 0.008 \mathrm{e} \
\mathrm{F} & -1.306 & 1.178 & 0.000 & -0.075 \mathrm{e}
\end{array}$ Calculate the x and y components of the dipole moment.

Accepted Answer

A)  F1F1F1S1F1F1F10x = -4.72 F1F1F1S1F1F1F10 10-30 C m, F1F1F1S1F1F1F10y = -1.33 F1F1F1S1F1F1F10 10-30 C m 
B)  F1F1F1S1F1F1F10x = -0.295 F1F1F1S1F1F1F10 10-30 C m, F1F1F1S1F1F1F10y = -0.083 F1F1F1S1F1F1F10 10-30 C m 
C)  F1F1F1S1F1F1F10x = -7.27 F1F1F1S1F1F1F10 10-33 C m, F1F1F1S1F1F1F10y = -1.28 F1F1F1S1F1F1F10 10-30 C m 
D)  F1F1F1S1F1F1F10x = 1.10 F1F1F1S1F1F1F10 10-29 C m, F1F1F1S1F1F1F10y = 2.96 F1F1F1S1F1F1F10 10-30 C m 
A)  F1F1F1S1F1F1F10x = -4.72 F1F1F1S1F1F1F10 10-30 C m, F1F1F1S1F1F1F10y = -1.33 F1F1F1S1F1F1F10 10-30 C m 
B)  F1F1F1S1F1F1F10x = -0.295 F1F1F1S1F1F1F10 10-30 C m, F1F1F1S1F1F1F10y = -0.083 F1F1F1S1F1F1F10 10-30 C m 
C)  F1F1F1S1F1F1F10x = -7.27 F1F1F1S1F1F1F10 10-33 C m, F1F1F1S1F1F1F10y = -1.28 F1F1F1S1F1F1F10 10-30 C m 
D)  F1F1F1S1F1F1F10x = 1.10 F1F1F1S1F1F1F10 10-29 C m, F1F1F1S1F1F1F10y = 2.96 F1F1F1S1F1F1F10 10-30 C m

Question 5

The dipole moment of nitrobenzene is 3.99 D. Estimate the magnitude of the dipole moment in meta (1,3-)dinitrobenzene.

Accepted Answer

A)  2.0 D 
B)  3.0 D 
C)  4.0 D 
D)  8.0 D 
A)  2.0 D 
B)  3.0 D 
C)  4.0 D 
D)  8.0 D

Question 6

Calculate the magnitude of the potential energy for the interaction of two co-linear hydrogen fluoride, HF, molecules whose centres are separated by 5.0 Å. The dipole moment of a hydrogen fluoride molecules is 1.91 D.

Accepted Answer

A)  1.9 F1F1F1S1F1F1F10 10-21 J 
B)  12 F1F1F1S1F1F1F10 10-22 J 
C)  5.8 F1F1F1S1F1F1F10 10-21 J 
D)  2.9 F1F1F1S1F1F1F10 10-21 J 
A)  1.9 F1F1F1S1F1F1F10 10-21 J 
B)  12 F1F1F1S1F1F1F10 10-22 J 
C)  5.8 F1F1F1S1F1F1F10 10-21 J 
D)  2.9 F1F1F1S1F1F1F10 10-21 J

Question 7

Estimate the potential energy resulting from the dispersion interaction between two xenon, Xe, atoms at a separation of 4.80 Å. The polarizability volume of a xenon atom is 4.16 Å3 and the ionization energy is 12.1 eV.

Accepted Answer

A)  -1.26 F1F1F1S1F1F1F10 10-22 J 
B)  -5.71 F1F1F1S1F1F1F10 10-3 J 
C)  -3.50 F1F1F1S1F1F1F10 10-22 J 
D)  -9.14 F1F1F1S1F1F1F10 10-22 J 
A)  -1.26 F1F1F1S1F1F1F10 10-22 J 
B)  -5.71 F1F1F1S1F1F1F10 10-3 J 
C)  -3.50 F1F1F1S1F1F1F10 10-22 J 
D)  -9.14 F1F1F1S1F1F1F10 10-22 J

Question 8

The mean separation between chlorine, Cl2, molecules, at a temperature of 298.15 K and a pressure of 1 bar is 3.5 nm. Given the values of the Lennard-Jones parameters are F1F1F1S1F1F1F10 = 368 kJ mol-1 and rF1F1F1S1F1F1F10 = 412 pm, use the Lennard-Jones function to calculate the potential energy between pairs of xenon atoms at this separation.

Accepted Answer

A)  -3.9 J mol-1 
B)  0.0 J mol-1 
C)  -0.98 J mol-1 
D)  -15 J mol-1 
A)  -3.9 J mol-1 
B)  0.0 J mol-1 
C)  -0.98 J mol-1 
D)  -15 J mol-1

Question 9

The dipole moment of an ozone molecule, O3, is 0.53 D. The molecule has a symmetrical bent structure so that, if the molecule is assumed to lie in the yz plane, the terminal atoms have coordinates (F1F1F1S1F1F1F100.678 Å,0,-0.362 Å) and the central atom has coordinates (0,0,0.724 Å). The terminal atoms have a net negative partial charge and the central atom has a net positive partial charge. Determine the magnitude of the partial charges on each of the oxygen atoms.

Accepted Answer

A)  Terminal: -0.051e Central: +0.102e 
B)  Terminal: -0.076e Central: +0.076e 
C)  Terminal: -0.102e Central: +0.102e 
D)  Terminal: -0.108e Central: +0.215e 
A)  Terminal: -0.051e Central: +0.102e 
B)  Terminal: -0.076e Central: +0.076e 
C)  Terminal: -0.102e Central: +0.102e 
D)  Terminal: -0.108e Central: +0.215e

Question 10

Determine the strength of the electric field necessary to induce a dipole moment of1.0 F1F1F1S1F1F1F10D in sulfur hexafluoride, SF6, which has been calculated to have a polarizability volume of 4.00 Å3.

Accepted Answer

A)  1.7 kV m-1 
B)  6.2 kV m-1 
C)  95 kV m-1 
D)  7.5 kV m-1 
A)  1.7 kV m-1 
B)  6.2 kV m-1 
C)  95 kV m-1 
D)  7.5 kV m-1

The Pauling electronegativities of chlorine and iodine are 3.0 and 2.5 respectively. Estimate the dipole moment of iodine monochloride, ICl.

The dipole moment of hydrogen chloride, HCl, is 1.08 D and the bond length is 127 pm. Calculate the fractional charge on the hydrogen and chlorine atoms.

The Lennard-Jones parameters for the interactions between benzene, C₆H₆, molecules are  = 454 kJ mol^-1 and r₀ = 527 pm. Calculate the separation that corresponds to the minimum in the Lennard-Jones potential.

The dipole moment of nitrobenzene is 3.99 D. Estimate the magnitude of the dipole moment in meta (1,3-)dinitrobenzene.

Calculate the magnitude of the potential energy for the interaction of two co-linear hydrogen fluoride, HF, molecules whose centres are separated by 5.0 Å. The dipole moment of a hydrogen fluoride molecules is 1.91 D.

Estimate the potential energy resulting from the dispersion interaction between two xenon, Xe, atoms at a separation of 4.80 Å. The polarizability volume of a xenon atom is 4.16 Å³ and the ionization energy is 12.1 eV.

Determine the strength of the electric field necessary to induce a dipole moment of1.0 D in sulfur hexafluoride, SF₆, which has been calculated to have a polarizability volume of 4.00 Å³.

The Propertiesof Gases

The First Law of Thermodynamics

The Second Law of Thermodynamics

Physical Transformations

Chemical Change

Chemical Kinetics

Quantum Theory

Atomic Structure

The Chemical Bond

Molecular Spectroscopy

Statistical Thermodynamics

Filters

Exam 10: Molecular Interactions

The Pauling electronegativities of chlorine and iodine are 3.0 and 2.5 respectively. Estimate the dipole moment of iodine monochloride, ICl.

The dipole moment of hydrogen chloride, HCl, is 1.08 D and the bond length is 127 pm. Calculate the fractional charge on the hydrogen and chlorine atoms.

The Lennard-Jones parameters for the interactions between benzene, C6H6, molecules are  = 454 kJ mol-1 and r0 = 527 pm. Calculate the separation that corresponds to the minimum in the Lennard-Jones potential.

The dipole moment of nitrobenzene is 3.99 D. Estimate the magnitude of the dipole moment in meta (1,3-)dinitrobenzene.

Calculate the magnitude of the potential energy for the interaction of two co-linear hydrogen fluoride, HF, molecules whose centres are separated by 5.0 Å. The dipole moment of a hydrogen fluoride molecules is 1.91 D.

Estimate the potential energy resulting from the dispersion interaction between two xenon, Xe, atoms at a separation of 4.80 Å. The polarizability volume of a xenon atom is 4.16 Å3 and the ionization energy is 12.1 eV.

Determine the strength of the electric field necessary to induce a dipole moment of1.0 D in sulfur hexafluoride, SF6, which has been calculated to have a polarizability volume of 4.00 Å3.

The Propertiesof Gases

The First Law of Thermodynamics

The Second Law of Thermodynamics

Physical Transformations

Chemical Change

Chemical Kinetics

Quantum Theory

Atomic Structure

The Chemical Bond

Molecular Spectroscopy

Statistical Thermodynamics

Filters

The Lennard-Jones parameters for the interactions between benzene, C₆H₆, molecules are  = 454 kJ mol^-1 and r₀ = 527 pm. Calculate the separation that corresponds to the minimum in the Lennard-Jones potential.

Estimate the potential energy resulting from the dispersion interaction between two xenon, Xe, atoms at a separation of 4.80 Å. The polarizability volume of a xenon atom is 4.16 Å³ and the ionization energy is 12.1 eV.

Determine the strength of the electric field necessary to induce a dipole moment of1.0 D in sulfur hexafluoride, SF₆, which has been calculated to have a polarizability volume of 4.00 Å³.