Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O 3 Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH 3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.
Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O 3 Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH 3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.
Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles.
(a) Sketch the bond dipoles and molecular dipole (if any) for
O
3
Explain your observations.
(b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative.
(c) Predict whether there should be a molecular dipole for
NH
3
and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.
3. How many valence electrons are in a C atom?
an Cl atom?
(a) Write the full Lewis structure for the CH2C2 molecule. Show all lone pairs.
Pert
(b) Write the geometric structure for the CH2CI2 molecule and name the geometry.
(c) Determine if the CH2CI2 molecule has polar or nonpolar bonds using the
following electronegativity: C = 2.5, H = 2.1, CI = 3.0. Re-draw the geometric
structure below, but this time include partial charges and dipole arrows for any
polar bonds present. Justify your assignments for polar or nonpolar bonds.
3. The following are some molecules:H2, HF, CO2, H2O, Cl2, NH3, CH4, CHCl3
(a) Which of the above molecules do/does not contain polar bond? Explain your answer.
(b) Which covalent bond has the highest bond polarity among the eight molecules?
(c) (i) Which of the above molecules are non-polar molecules?
(ii) Explain why these molecules are non-polar. 4. (d) Draw a diagram to illustrate the formation of hydrogen bonds in H2O.
Based on Linus Pauling's electronegativity scale, would H2S be considered a polar molecule?
Pick the best answer.
(a) No. It would technically be considered a non-polar molecule.
(b) No. Even though it contains polar bonds they are symmetrical and therefore H2S is non-polar.
(c) No. The electronegativity difference between H and S is so great that it would be considered an ionic compound.
(d) H2S violates the octet rule and therefore would not even exist
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell