Fluorine nitrate, \(\mathrm{FONO}_{2}\), is an oxidizing agent used as a rocket propellant. A reference source lists the following data for \(\mathrm{FO}_{\mathrm{a}} \mathrm{NO}_{2}\). (The subscript "a" shows that this O atom is different from the other two.) Bond lengths: \(\mathrm{N}-\mathrm{O}=129 \mathrm{pm}\) $$ \mathrm{N}-\mathrm{O}_{\mathrm{a}}=139 \mathrm{pm} ; \mathrm{O}_{\mathrm{a}}-\mathrm{F}=142 \mathrm{pm} $$ Bond angles: \(\mathrm{O}-\mathrm{N}-\mathrm{O}=125^{\circ}\) $$ \mathrm{F}-\mathrm{O}_{\mathrm{a}}-\mathrm{N}=105^{\circ} $$ \(\mathrm{NO}_{\mathrm{a}} \mathrm{F}\) plane is perpendicular to the \(\mathrm{O}_{2} \mathrm{NO}_{\mathrm{a}}\) plane Use these data to construct a Lewis structure(s), a three-dimensional sketch of the molecule, and a plausible bonding scheme showing hybridization and orbital overlaps.

Step by step solution

01

Lewis Structure

The first step is to draw the Lewis structure for \(\mathrm{FONO}_{2}\). Start with considering the valence electrons for each atom - nitrogen (N) has five, oxygen (O) has six, and fluorine (F) has seven. Connect nitrogen to one oxygen (labelled \(O_a\)) and fluorine, and the nitrogen to two other oxygens. Add double bonds to the two oxygen atoms directly connected to the nitrogen, and single bonds for the \(O_a\) to F, and N to \(O_a\). Fill the remaining electrons to complete the octets of each atom, ensuring that each atom follows the octet rule.

02

Molecular Geometry

With the Lewis structure, we can determine the geometry of the molecule. The molecular geometry around the nitrogen atom is trigonal planar, because there three regions of electron density (three bonds). The geometry around the \(O_a\) atom however, is bent/ angular because it has two bonding pairs of electrons and two lone pairs.

03

Bonding Scheme and Hybridization

In the nitrogen atom, the presence of three electron domains suggests an \(sp^2\) hybridization. We have three \(sp^2\) orbitals forming the bonds with the two oxygens and \(O_a\), and one unhybridized p orbital lying perpendicular to the plane of these three bonds. This p orbital is involved in the formation of \(pi\) bonds with the p orbitals of the two oxygen atoms. The oxygen atom attached to Fluorine has two unshared pairs of electrons (in two \(2p\) orbitals) and two shared pairs of electrons (in \(sp^3\)). Therefore, the \(O_a\) atom is \(sp^3\) hybridized.

04

Sketching

Sketch the molecule keeping in mind the bond lengths, bond angles, and the orientation of the molecules in different planes as stated in the problem. Ensure the \(F-O_a-N\) bond angle is 105 degrees, the \(O-N-O\) bond angle is 125 degrees, and the \(NO_aF\) plane is perpendicular to the \(O_2 NO_a\)

Unlock Step-by-Step Solutions & Ace Your Exams!

• Full Textbook Solutions

  Get detailed explanations and key concepts

• Unlimited Al creation

  Al flashcards, explanations, exams and more...

• Ads-free access

  To over 500 millions flashcards

• Money-back guarantee

  We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!