Polarity and Intermolecular Forces Assignment.pdf

# Polarity and Intermolecular Forces Assignment.pdf - Divya...

• Homework Help
• 8

This preview shows page 1 - 3 out of 8 pages.

Divya Dadar Polarity and Intermolecular Forces Assignment 1. Use the VSEPR theory to predict the shape of methane (CH4). Then indicate whether the bonds are polar. Will the molecule be polar? - The methane molecule is tetrahedral since there are four pairs of electrons and has no lone pairs. - CH4 has one carbon atom bonded to 4 hydrogen atoms. The four hydrogen atoms are placed at the vertices of tetrahedron. - There is an equal sharing of electrons and no lone pairs, the EN difference is less than 0.5 therefore, the bonds are nonpolar and the molecule is nonpolar as well - The bond angle is 109.5 - The molecular shape of CH4: (triangular faced pyramid) Figure 1: VSEPR diagram of methane(VibeThemes, 2018) 2. Using electronegativity values, determine bond polarities and the net dipoles in a molecule of PCl3 and indicate if the molecule will be polar. The electronegativity value of phosphorus is 2.1 and the electronegativity value of chlorine is 3.0 The EN difference is greater than 0.5 knowing that has polar bonds It contains one lone pair, four pairs of electrons and three bonding pairs → due to this structure, using VSEPR theory, it is identified with a geometrical arrangement of tetrahedron

Subscribe to view the full document.

Divya Dadar However, due to its one lone pair its molecular shape is trigonal pyramidal, due to the fact that one corner is different from the others As chlorine is electronegative than phosphorus the dipole moment would all be towards chlorine, facing down in the molecule The dipoles do not cancel out as they are all in the same direction meaning the molecule is polar Figure 2:
You've reached the end of this preview.

{[ snackBarMessage ]}

### What students are saying

• As a current student on this bumpy collegiate pathway, I stumbled upon Course Hero, where I can find study resources for nearly all my courses, get online help from tutors 24/7, and even share my old projects, papers, and lecture notes with other students.

Kiran Temple University Fox School of Business ‘17, Course Hero Intern

• I cannot even describe how much Course Hero helped me this summer. It’s truly become something I can always rely on and help me. In the end, I was not only able to survive summer classes, but I was able to thrive thanks to Course Hero.

Dana University of Pennsylvania ‘17, Course Hero Intern

• The ability to access any university’s resources through Course Hero proved invaluable in my case. I was behind on Tulane coursework and actually used UCLA’s materials to help me move forward and get everything together on time.

Jill Tulane University ‘16, Course Hero Intern