Identify the correct Lewis structure of CF4. Ensure that all charges and lone pairs are shown.Group of answer choices

To draw the Lewis structure for CF4 (Carbon Tetrafluoride), follow these steps:

1. Count the total number of valence electrons. Carbon has 4 valence electrons and each Fluorine atom has 7 valence electrons, so the total is 4+(4*7)=32 valence electrons.

2. Draw a skeleton structure of the molecule. Carbon is less electronegative than Fluorine, so it goes in the center. Draw a single bond (representing 2 electrons) between the Carbon and each Fluorine atom.

3. Distribute the remaining electrons as lone pairs on the surrounding atoms (in this case, the Fluorine atoms) to fulfill the octet rule. Each Fluorine atom will have 3 lone pairs (6 electrons) and one single bond (2 electrons) with Carbon, making a total of 8 electrons for each Fluorine atom.

4. Check that you have used the total number of valence electrons calculated in step 1. In this case, you should have used all 32 electrons.

5. Check that each atom satisfies the octet rule (2 for Hydrogen, 8 for all other atoms). In this case, Carbon has 8 electrons (4 bonds * 2 electrons/bond) and each Fluorine has 8 electrons (1 bond * 2 electrons/bond + 6 lone electrons), so the octet rule is satisfied.

6. If any atom does not satisfy the octet rule, and there are no more lone pairs to move to make a double or triple bond, then the molecule does not follow the octet rule. This is not the case for CF4.

So, the correct Lewis structure for CF4 is a Carbon atom in the center with single bonds to four Fluorine atoms. Each Fluorine atom has three lone pairs of electrons. There are no charges because all of the atoms are neutral.