SOLVED: Consider the PF5 molecule: a) Draw a lewis structure for this molecule. b) Does the molecule follow the octet rule? c) Are the P-F bonds polar? If so, which atom in the bond will have a partia

Molecular Geometry of PF5 (phosphorus pentafluoride)
Molecular Geometry of PF5 (phosphorus pentafluoride)

Get 5 free video unlocks on our app with code GOMOBILE

Snapsolve any problem by taking a picture.
Try it in the Numerade app?

Solved step-by-step

Consider the PF5 molecule:
a) Draw a lewis structure for this molecule.
b) Does the molecule follow the octet rule?
c) Are the P-F bonds polar? If so, which atom in the bond will
have a partial positive (O+) charge?

Solved by verified expert

This problem has been solved!

Try Numerade free for 7 days

01:19

Draw a Lewis structure of a covalent compound in which oxygen has:(a) Two single bonds and two unshared pairs of electrons(b) One double bond and two unshared pairs of electrons

01:20

Draw a Lewis structure of a covalent compound in which nitrogen has:(a) Three single bonds and one unshared pair of electrons(b) One single bond, one double bond, and one unshared pair of electrons(c) One triple bond and one unshared pair of electrons

03:47

Write the Lewis structure for each molecule (octet rule notfollowed).a. BCl3 b. NO2 c. BH3

01:06

Draw Lewis structures that obey the octet rule for the following species. Assign the formal charge to each central atom.a. $\mathrm{POCl}_{3}$b. $\mathrm{SO}_4{^2}{^-}$c. $\mathrm{ClO}$${4}^{-}$d. $\mathrm{PO}_{4}{^3}{^-}$e. $\mathrm{SO}_{2} \mathrm{Cl}_{2}$f. $\mathrm{XeO}_{4}$g. $\mathrm{ClO}$$3^{-}$h. $$\mathrm{NO}_{4}{^3}{^-}$$

Transcript

To draw the Lewis structure for PF five we need to first count the total number of valence electrons phosphorus has five. Flooring has seven and there are five of them. So that gives us a total of 40 valence electrons. If we put phosphorus in the middle and bond all five florins to it, We will have used up 10 valence electrons two per bond. And then if we give each flooring and octet by adding three lone pairs, three Lone pairs at two apiece gives us six valence electrons per floor Een six times five Gives us the 30 electrons that we had left. So now we’ve used up all of our valence electrons. All the…

Enter your parent or guardian’s email address:

Already have an account? Log in

An exclusive promotional rate that’s yours to keep forever

or

EMAIL

PASSWORD

You are watching: SOLVED: Consider the PF5 molecule: a) Draw a lewis structure for this molecule. b) Does the molecule follow the octet rule? c) Are the P-F bonds polar? If so, which atom in the bond will have a partia. Info created by THVinhTuy selection and synthesis along with other related topics.

Rate this post

Related Posts