Draw the Line Bond Structure for Acetone (C3H\u00c3\u00a2\u00e2\u20ac\u0161\u00e2\u20ac\u0161O) Step 2: Step 1A: (ADD HYDROGENS UNTIL EACH CARBON HAS 4 BONDS = OCTET) Use the skeleton structure from step 1A to find: O || C C C Step 1B: Count the total number of valence electrons from all the atoms in the molecule. Chemical formula of molecule Atom # of atoms X X X # of valence electrons = = Total # of electrons in structure = totals Step 3: Subtract the number of electrons used to make the skeleton structure from the total number of valence electrons. Total # of electrons in structure (from step 1 above) # of electrons used in skeleton (from step 2 above) Remaining # electrons to be added= Step 5: Check for Octets Check the structure in step 4 for octets (4 pairs) of electrons around each atom. If octet rule is satisfied, you are done. If octet rule is not satisfied, go to Step 6. # of electrons used in skeleton = (multiply # of bonds in skeleton by 2) Step 4: Add the remaining electrons (if any remain) to the skeletal structure above as lone pairs as evenly as possible on all atoms except hydrogen. Step 6: Use existing lone pairs to make double or triple bonds until the octet rule is satisfied for all atoms<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n Acetone (C\u2083H\u2086O), also known as propan-2-one, is the simplest ketone with a central carbonyl group (C=O) flanked by two methyl groups (CH\u2083). To draw its Lewis structure, follow these steps:<\/p>\n\n\n\n Step 1A: Skeleton Structure<\/strong><\/p>\n\n\n\n Arrange the atoms to reflect the molecular formula:<\/p>\n\n\n\n Here, the central carbon (C\u2082) is double-bonded to oxygen (O) and single-bonded to two other carbons (C\u2081 and C\u2083), each bonded to three hydrogens.<\/p>\n\n\n\n Step 1B: Count Valence Electrons<\/strong><\/p>\n\n\n\n Total valence electrons:<\/strong> 12 (C) + 6 (H) + 6 (O) = 24 electrons.<\/p>\n\n\n\n Step 2: Add Hydrogens to Satisfy Carbon’s Octet<\/strong><\/p>\n\n\n\n Each carbon atom needs four bonds to satisfy the octet rule:<\/p>\n\n\n\n Step 3: Subtract Electrons Used in Skeleton from Total Valence Electrons<\/strong><\/p>\n\n\n\n Remaining electrons:<\/strong> 24 total electrons \u2013 18 used electrons = 6 electrons.<\/p>\n\n\n\n Step 4: Add Remaining Electrons as Lone Pairs<\/strong><\/p>\n\n\n\n Distribute the remaining 6 electrons as lone pairs:<\/p>\n\n\n\n Step 5: Check for Octets<\/strong><\/p>\n\n\n\n All atoms have complete octets, confirming the structure is correct.<\/p>\n\n\n\n For a visual demonstration, you can refer to the following video:<\/p>\n\n\n\n H3C\u2014C\u2014C\u2014H3\n ||\n O<\/code><\/pre>\n\n\n\n\n
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