# Three resonance structures are possible for the thiocyanate ion, SCN − . (a) Draw the three resonance structures. (b) Calculate the formal charge on each atom in each resonance structure. (c) Based on formal charges and electronegativity, predict which resonance structure most closely approximates the bonding in this ion? (d) What are the similarities and differences of bonding in SCN − compared to the bonding in OCN − (page 382). ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 8, Problem 34PS
Textbook Problem
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## Three resonance structures are possible for the thiocyanate ion, SCN−. (a) Draw the three resonance structures. (b) Calculate the formal charge on each atom in each resonance structure. (c) Based on formal charges and electronegativity, predict which resonance structure most closely approximates the bonding in this ion? (d) What are the similarities and differences of bonding in SCN− compared to the bonding in OCN− (page 382).

(a)

Interpretation Introduction

Interpretation: The resonance structures for SCN- molecule should be determined.

Concept Introduction:

Resonance stabilization: Due to the delocalization of electrons within the molecule the overall energy becomes lower and makes that molecule more stable.

### Explanation of Solution

Lewis structure for any molecule is drawn by using the following steps,

First the skeletal structure for the given molecule is drawn then the total number of valence electrons for all atoms present in the molecule is determined

The next step is to subtract the electrons present in the total number of bonds present in the skeletal structure of the molecule with the total valence electrons such that considering each bond contains two electrons with it...

(b)

Interpretation Introduction

Interpretation: The formal charge of the SCN- molecule should be determined.

Concept Introduction:

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

(c)

Interpretation Introduction

Interpretation: The resonance structure that closely approximates the bonding in the given ion should be identified.

Concept Introduction:

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

(d)

Interpretation Introduction

Interpretation: The similarities and differences of bonding in SCN-andOCN- should be determined.

Concept Introduction:

Molecular geometry: It is defined as unique three dimensional arrangement of atoms around the central metal present in the molecule which is determined by using spectroscopic techniques and also by using Lewis structure or the valence shell electron pair repulsion theory (VSEPR).

VSEPR Theory:

As the name itself indicate that the basis for this theory is the electron pair that is bonded electron present in either single or double bonds or lone pair electrons, present in the valence shell tend to repel each other which then tends to be in position in order to minimize the repulsions. The steps involved in the theory in describing the geometry is as follows,

• The first step is to draw the correct Lewis structure for the molecule.
• Then, the electron domain around the central atom should be counted and the geometry that matches with that type of domain in VSEPR should be determined.
• Finally, the geometry is predicted by using the orientation of atoms.

The molecules with domains of type AB2 tend to have shape like linear, type AB2 with lone pair electrons will have bent shape, type AB3 will have shape like trigonal planar, type AB4 will have shape like tetrahedral or square planar, type AB5 will have trigonal bipyramidal and AB6 will have shape like octahedral respectively.

Electron Domain: In VSEPR theory, both the lone pair and the bonded pair are together considered as electron domain regardless of the type of bond in which the bonded pair presents.

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