Types of Bonds and Orbitals in Molecules: NO3-, CS2, CH2O, FNO, C2F4

[MysticDude]

Hello PFers, a chemistry question that I need help with awaits!

Homework Statement

10.42 Describe the types of bonds and orbitals in the following: (a) NO₃^-; (b) CS₂; (c) CH₂O; (d) FNO; (e) C₂F₄.

Homework Equations

The Attempt at a Solution

I tried to visualize the kind of arrangement and what not for these but I did not know where to go from there.

(a).I think that there have to be sigma bonds and in the p-orbital. I'm not sure how to get the orbital though. I'm guessing for the orbital.

I don't know how to do the other ones though :(

 

[MysticDude]

Is there anyone that can help?

 

[Borek]

Googling for "orbitals in nitrate ion" gave this as a first hit:

http://www.chem1.com/acad/webtext/chembond/cb07.html

 

[nobahar]

Determine the Lewis structure and then use VSEPR theory. As far as I am aware...

 

[DeeNos]

Hello! Let's break down each molecule and discuss the types of bonds and orbitals present.

(a) NO3-: This molecule has a trigonal planar geometry, with a central nitrogen atom bonded to three oxygen atoms. The bonds in this molecule are all sigma bonds, formed by the overlap of atomic orbitals. The nitrogen atom has a sp2 hybridization, meaning it has one s orbital and two p orbitals that have combined to form three sp2 hybrid orbitals. These orbitals overlap with the p orbitals of the oxygen atoms to form the sigma bonds. Additionally, the nitrogen atom has a lone pair of electrons in a p orbital.

(b) CS2: This molecule has a linear geometry, with a central carbon atom bonded to two sulfur atoms. The bonds in this molecule are all sigma bonds, formed by the overlap of atomic orbitals. The carbon atom has a sp hybridization, meaning it has one s orbital and one p orbital that have combined to form two sp hybrid orbitals. These orbitals overlap with the p orbitals of the sulfur atoms to form the sigma bonds.

(c) CH2O: This molecule has a trigonal planar geometry, with a central carbon atom bonded to two hydrogen atoms and one oxygen atom. The bonds in this molecule are all sigma bonds, formed by the overlap of atomic orbitals. The carbon atom has a sp2 hybridization, meaning it has one s orbital and two p orbitals that have combined to form three sp2 hybrid orbitals. These orbitals overlap with the s orbitals of the hydrogen atoms and the p orbital of the oxygen atom to form the sigma bonds.

(d) FNO: This molecule has a linear geometry, with a central nitrogen atom bonded to a fluorine atom and an oxygen atom. The bonds in this molecule are all sigma bonds, formed by the overlap of atomic orbitals. The nitrogen atom has a sp hybridization, meaning it has one s orbital and one p orbital that have combined to form two sp hybrid orbitals. These orbitals overlap with the p orbitals of the fluorine and oxygen atoms to form the sigma bonds.

(e) C2F4: This molecule has a planar geometry, with two carbon atoms each bonded to two fluorine atoms. The bonds in this molecule are a combination of sigma and pi bonds. The carbon atoms have a sp2 hybridization, meaning they have one s orbital and two p orbitals that have