Diazomethane is a highly poisonous, explosive compound because it readily evolves N2. Diazomethane has the following composition by mass: 28.57% C; 4.80% H; and 66.64% N. The molar mass of diazomethane is 42.04 g/mol. Find the molecular formula of diazomethane, draw its Lewis structure, and assign formal charges to each atom. Why is diazomethane not very stable? Explain.
Solution 92 E Step 1 of 5 The mass percentage can be used to obtain the ratio between the elements involved in forming a compound. Step 2 of 5 Since we know the mass percentages, it is reasonable that in 100 g of compound we have 28.57 g of C 4.80 g of H 66.64 g of N Now we can calculate the number of moles for each element moles of C= Mass of C/(Atomic mass of C)= 28.57 g/ (12.01g/mol)=2.38 moles of H= Mass of H/(Atomic mass of H)= 4.80g/ (1.008g/mol)=4.76 moles of N= Mass of O/(Atomic mass of N)= 66.64 g/ (14.01g/mol)=4.75 Step 3 of 5 Since the C has the lower number of moles, we can use this number as reference to know the ratio between these three elements. We have to divide all the numbers of moles obtained in the step 2 for the lowest value. moles of C/ 2.38= 1 moles of H/2.38= 2 moles of N/2.38= 2 So we obtain a C:H:N ratio that is 1:2:2. Thus we have on atom of C, 2 atoms of H and 2 atoms of N. Thus the empirical formula is CH N 2 2