Question

Can you explain how and why?

cular Models Pre-Lab Questions ) Lewis Structures are used to represent covalently bonded molecules and polyatomic ions. a. Answer the following to draw the Lewis Structure of the molecule of OF i. How many valence electrons (total) are you working with? ii. Which atom is the central atom? What criteria must you use to decide this? Do the atoms in the molecule all obey the octet rule? Are there any lone pairs on the central atom in your final structure? If iv. so, how many? v. What types of bonds (single, double, triple) exist between the central and outer atoms in your final structure. vi. Sketch.

Answer 1

(i) Total Valence Electrons = Valence electrons on O + (2* valence electrons on F) = 6+(2*7) = 20

(ii) Central atom is O.

Criteria:

Least electronegative element is the central atom.

Here F is more electronegative than O.

(iii) yes, Oxygen will combine with 2 F atoms and thus will be having 8 valence electrons. Similarly, F requires only 1 electron to complete its octet. Thus, it will form 1 bond with O to complete its octet and hence both follow octet rule.

(iv) Yes. there are lone pairs on the central atom. Oxygen has 6 valence electrons. 2 of its electrons are utilized in forming bond with 2 F atoms. Thus, we are left with 4 electrons resulting in 2 lone pairs.

(v) Single bonds only. Oxygen atom forms 2 single bond, one with each F atom to complete its octet.

(vi)

FOF