An objectionable component of smoggy air is acetylperoxide, which has the skeleton structure (a) Draw the Lewis structure of this compound. (b) Indicate all the bond angles.

To draw the Lewis structure of acetylperoxide, we will follow these steps: 1. Identify the elements present in the compound and count their total valence electrons. In acetylperoxide, there are three different elements: Carbon (C), Oxygen (O), and Hydrogen (H). - Carbon has 4 valence electrons. - Oxygen has 6 valence electrons. - Hydrogen has 1 valence electron. The molecular formula for acetylperoxide is C4H6O4. Hence, the total number of valence electrons for the entire molecule is: Total valence electrons = (4 C * 4) + (6 H * 1) + (4 O * 6) = 16 + 6 + 24 = 46 2. As mentioned earlier, acetylperoxide consists of two acetate groups linked by a peroxide group. So, first, draw the combined skeleton structures of two acetate groups and a peroxide group. Remember, oxygen atoms will bridge the acetate groups. 3. Now, we need to distribute the valence electrons in order to satisfy the octet rule for each atom. Keep in mind that carbon and oxygen require eight electrons while hydrogen requires two. 4. If there are any leftover electrons, place them on the central atom. However, in this case, we won't need to do this step. 5. Count the electrons around each atom to make sure they now satisfy the octet rule. Following these steps will give you the Lewis structure of acetylperoxide.

To determine the bond angles, you'll need to look at the bonding arrangement of each atom in the acetylperoxide molecule: 1. Carbon (C) - In acetylperoxide, each carbon forms two sigma (single) bonds to oxygen/hydrogen, and one pi (double) bond to oxygen. So, there are three electron domains around each carbon atom. This corresponds to a trigonal planar arrangement, and the bond angle is approximately 120 degrees. 2. Oxygen (O) - In the acetate groups, each oxygen atom forms one sigma (single) bond with carbon, one pi (double) bond with carbon, or one sigma bond with hydrogen. They have two electron domains, so there should be a linear arrangement with a bond angle of 180 degrees. 3. For the peroxide group, each oxygen is connected with a sigma (single) bond to the other oxygen in the peroxide and to one acetate group's carbon. They have two electron domains, so it has a linear arrangement too, with a bond angle of 180 degrees. In summary, the bond angles for acetylperoxide are approximately 120 degrees for carbon atoms, and approximately 180 degrees for oxygen atoms.