Problem: Write the Lewis structure and chemical formula of the compound with a molar mass of about 70 g/mol that contains 19.7% nitrogen and 80.3% fluorine by mass, and determine the formal charge of the atoms in this compound.

FREE Expert Solution

We’re being asked to determine the Lewis structure and chemical formula of a compound in which the molar mass and the mass percent of the elements present are given. 

Furthermore, we are also asked to determine the formal charge of the atoms in this compound.


To solve this problem, we shall follow these steps:

Step 1: Convert the mass percent to mass.

Step 2: Convert mass to moles of the element.

Step 3: Get the empirical formula and obtain the chemical formula from the given molar mass.

Step 4: Determine the central atom in the molecule.

Step 5: Calculate the total number of valence electrons present.

Step 6: Draw the Lewis structure for the molecule.

Step 7: Calculate the formal charge for the indicated atom. 


Recall that the formula for the formal charge is:


F.C.=Group No. -Bonds+Nonbonding electrons


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Problem Details

Write the Lewis structure and chemical formula of the compound with a molar mass of about 70 g/mol that contains 19.7% nitrogen and 80.3% fluorine by mass, and determine the formal charge of the atoms in this compound.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Formal Charge concept. You can view video lessons to learn Formal Charge. Or if you need more Formal Charge practice, you can also practice Formal Charge practice problems.