Draw the Lewis structure for each organic compound from its condensed structural formula.
Solution 99E Step 1 of 6 The compounds in this exercise are all organic molecules. We have to assume that exists a chain of atoms of Carbon that can be bonded each other by single, double or triple bonds. Moreover, we have to remember that every atom of Carbon has the possibility to form four bond maximum because it has only 4 electrons of valence.; Oxygen instead, has six electons of valence that are organized as two lone pairs and 2 single electrons that can be used to form two single bonds or a double bond. Nitrogen has 5 electrons of valence organized as a lone pair and 3 unpaired electrons that can be used to form single, double or triple bonds. Step 2 of 6 C24s a molecule belonging to the family of alkanes (general formula C H n n+2). In Lewis structure we have a chain formed by two atoms of Carbon (each of them is bonded to the other by a single covalent bond). Both of them are bonded with three atoms of Carbon . We can see the molecule in the figure below or better Since we have 2 carbons and six Oxygens we have Total electrons= 2(Valence number of C) + 6(valence number of H)= 2(4) + 6(1)= 14 We use all 14 electrons to form single covalent bonds Step 3 of 6 CH NH is a primary amine. In this case a NH is linked to a carbon chain. Nitrogen carries lone 3 2 2 pair and forms two single covalent bonds with two atoms of H. The third bond Nitrogen can form is with the Carbon chain. We have to remember that CH means that Carbon forms three 3 single covalent bonds with three atoms of H. For what we’ve said, the structure is Since we have one carbon, one N and 5 Hydrogens we have Total electrons= (Valence number of C) + 5(valence number of H) + (valence electrons of N)= 4 + 4(1) + 5= 14. In the Lewis structure above, every connecting line counts as a couple of bonding electrons. Thus in this molecule we can confirm we are using 14 electrons of valence.