For the given molecule the presence of formal charge of nitrogen atom should be identified. Concept Introduction : Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom. Valence electrons represent the electrons present in the outermost shell of an atom. Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons. Each atom has a specific number of valence electrons. If the valence electrons in that atom are reduced by one number, it gets positive charge. If the valence electrons in that atom are increased by one number, it gets negative charge. Formal charge of an atom can be identified by drawing the molecules in Lewis structures. The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound. Formal charge of an atom can be calculated by using the formula given below. Formal charge ( FC ) = [ number of valence electrons on atom ] - [ non bonded electrons+ number of bonds ] To find: Get the formal charge of nitrogen atom in the given molecule

Question

Want to see the full answer?

Answer 1

Question

Chapter 1.4, Problem 4LTS

Interpretation Introduction

Interpretation: For the given molecule the presence of formal charge of nitrogen atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons. If the valence electrons in that atom are reduced by one number, it gets positive charge. If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

Formal charge (FC) = [number of valence electrons on atom] - [non bonded electrons+ number of bonds]

To find: Get the formal charge of nitrogen atom in the given molecule

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Photochemical smog is formed in part by the action of light on nitrogen dioxide. The wavelength of radiation absorbed by NO2 in this reaction is 197 nm.(a) Draw the Lewis structure of NO2 and sketch its π molecular orbitals.(b) When 1.56 mJ of energy is absorbed by 3.0 L of air at 20 °C and 0.91 atm, all the NO2 molecules in this sample dissociate by the reaction shown. Assume that each absorbed photon leads to the dissociation (into NO and O) of one NO2 molecule. What is the proportion, in parts per million, of NO2 molecules in this sample? Assume that the sample behaves ideally.

Correct each molecule in the drawing area below so that it has the skeletal ("line") structure it would have if it were dissolved in a 0.1 M aqueous solution of HCI. If there are no changes to be made, check the No changes box under the drawing area. No changes. HO Explanation Check NH, 2 W O :□ G ©2025 M unter Accessibility

An expression for the root mean square velocity, vrms, of a gas was derived. Using Maxwell’s velocity distribution, one can also calculate the mean velocity and the most probable velocity (mp) of a collection of molecules. The equations used for these two quantities are vmean=(8RT/πM)1/2 and vmp=(2RT/M)1/2 These values have a fixed relationship to each other.(a) Arrange these three quantities in order of increasing magnitude.(b) Show that the relative magnitudes are independent of the molar mass of the gas.(c) Use the smallest velocity as a reference for establishing the order of magnitude and determine the relationship between the larger and smaller values.