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:
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 Lewis Dot Structure: Formal Charge concept. If you need more Lewis Dot Structure: Formal Charge practice, you can also practice Lewis Dot Structure: Formal Charge practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Julian's class at UCR.