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Chapter 9: Problem 110

Write Lewis structures for the following four isoelectronic species: (a) \(\mathrm{CO},(\mathrm{b}) \mathrm{NO}^{+},(\mathrm{c}) \mathrm{CN}^{-}\) (d) \(\mathrm{N}_{2}\). Show formal charges.

Short Answer

Expert verified
The Lewis structures with formal charges will be as follows: For (a) CO: :O=C: , (b) NO+: [O=N+] , (c) CN-: [C≡N-] , (d) N2: N≡N.

Step by step solution

01

Compute Total Number of Valence Electrons

Determine the number of valence electrons using the atomic numbers: Carbon(C) has 4, Oxygen(O) has 6, Nitrogen(N) has 5.
02

Determine Central Atom and Draw Skeletal Structure

The least electronegative element is usually the central atom, except for hydrogen. In CO and N2, it's C and N, respectively. For NO+ and CN-, the positive charge is usually on the less electronegative atom and the negative charge on the more electronegative. Thus, for NO+ it's N-O, and for CN- it's C≡N.
03

Distribute Electrons

Arrange the remaining electrons as lone pairs on the atoms. Every atom (except H) should have an octet. For CO: O=C.; For NO+: O=N+; For CN- : C≡N-; For N2: N≡N.
04

Indicate Formal Charges

The formal charge (FC) can be determined using the formula: FC = (number of valence electrons) - 0.5 * (number of bonding electrons) - (number of nonbonding electrons). Apply this formula to each atom and indicate in the structures.

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Most popular questions from this chapter

Because fluorine has seven valence electrons \(\left(2 s^{2} 2 p^{5}\right),\) seven covalent bonds in principle could form around the atom. Such a compound might be \(\mathrm{FH}_{7}\) or \(\mathrm{FCl}_{7}\). These compounds have never been prepared. Why?

When irradiated with light of wavelength \(471.7 \mathrm{nm}\) the chlorine molecule dissociates into chlorine atoms. One \(\mathrm{Cl}\) atom is formed in its ground electronic state while the other is in an excited state that is \(10.5 \mathrm{~kJ} / \mathrm{mol}\) above the ground state. What is the bond enthalpy of the \(\mathrm{Cl}_{2}\), molecule?

The amide ion, \(\mathrm{NH}_{2}^{-},\) is a Bronsted base. Represent the reaction between the amide ion and water.

Draw Lewis structures for the following organic molecules. In each there is one \(\mathrm{C}=\mathrm{C}\) bond, and the rest of the carbon atoms are joined by \(\mathrm{C}-\mathrm{C}\) bonds. \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{~F}, \mathrm{C}_{3} \mathrm{H}_{6}, \mathrm{C}_{4} \mathrm{H}_{8}\)

What is Lewis's contribution to our understanding of the covalent bond?
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