Describe what makes a bond polar or nonpolar.

CO2 Molecular Shape: Hybridization of the central atom write in normal characters sp, sp2, sp3 Name: Number of sigma bonds: Number of pi bonds:

CO2 Draw the Lewis structure on a separate piece of paper. Show your work and label the question number clearly. You will upload a photo of your response at the end of the test.

Upload your work. It is allowed to use your phone to upload your work to your exam.   Work not posted to the exam will not be accepted. You must complete the upload of your work before time ends (3 hours total). It is easier to save all of your work in one file, either as a .pdf or .doc. Don’t use .heic files! Turn off the Live feature of your iPhone and this will save your pictures as .jpg instead of .heic. Save your file with your last name in the file name. Completing this process is worth points if completed correctly.

Determine whether a bond in the compound is polar or nonpolar and whether the molecule as a whole is polar or nonpolar. Place your answers in the table below. Electronegativity of C is 2.5, H is 2.1, and Cl is 3.5. Compound Nonpolar Bond Y/N Polar Bond Y/N Molecule Polar Y/N CH4       CH3Cl       CH2Cl2       CHCl3       CCl4        

O2 Draw the Lewis structure on a separate piece of paper. Show your work and label the question number clearly. You will upload a photo of your response at the end of the test.

For one of the ions shown above, write out all of the possible resonance structures. Work out the problem on a separate piece of paper and upload a photo of your response at the end of the test. Please mark the problem clearly and show your work.

Using the electronegativity table and the rules (which suggest that a difference in electronegativity below 0.4 is equally shared, 0.5–1.7 is polar covalent, and greater than 1.8 is ionic), the bonds in BeBr2 (electronegativity of Be is 1.5 and Br is 2.8) would be classified as ________.

Double Bonds A double bond between two carbon atoms consists of one sigma-type bond and one pi-type bond. Draw a diagram of the double bond orbitals. Briefly describe how a pi bond differs from a sigma bond. Enter the text of your answer in the box below. A diagram with a brief description can be recorded on a separate piece of paper, labeled and numbered clearly, and uploaded as a photo at the end of the exam.

At the end of “Barn Burning,”