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Chapter 22: Problem 79

The amide anion \(\mathrm{NH}_{2}^{-}\) is a very strong base. On the basis of molecular orbital theory, would you expect \(\mathrm{NH}_{2}^{-}\) to be linear or bent?

Short Answer

Expert verified
The \(\mathrm{NH}_{2}^{-}\) anion is expected to have a bent structure.

Step by step solution

01

Understand Molecular Orbitals and Electron Distribution

A molecular orbital is a region in a molecule where there's a high probability of finding an electron. In an \(\mathrm{NH}_{2}^{-}\) molecule, there's a total of 8 valence electrons. Nitrogen atom has 5 valence electrons and each Hydrogen atom contributes one, the extra electron makes it eight.
02

Apply Molecular Orbital Theory to \(\mathrm{NH}_{2}^{-}\) structure

The \(\mathrm{NH}_{2}^{-}\) molecule forms when one extra electron is added to the Nitrogen atom, making it an anion. This extra electron will go to the non-bonding orbital of nitrogen. Nitrogen atom forms two bond pairs with the two Hydrogen atoms, and it has one non-bonding electron pair.
03

Determine the Structure of \(\mathrm{NH}_{2}^{-}\)

Non-bonding electron pairs require more space than bonding pairs. Therefore, the \(\mathrm{NH}_{2}^{-}\) anion prefers a shape that minimizes electron pair repulsion and ensures maximum stability. In this case, it's a 'bent' or 'V-shaped' geometry, not linear.

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Most popular questions from this chapter

The heavier halogens (Cl, Br, and I) form compounds in which the central halogen atom, \(X\), is bonded directly to oxygen and to fluorine. Several examples are known, including those with formulas of the type \(\mathrm{FXO}_{2}, \mathrm{FXO}_{3, \text { and } \mathrm{F}_{3} \mathrm{XO} . \text { The structures of these }}\) molecules are all consistent with the VSEPR model. Draw Lewis structures and predict the geometries of (a) chloryl fluoride, \(\mathrm{FClO}_{2}\); (b) perchloryl fluoride, \(\mathrm{FClO}_{3} ;(\mathrm{c}) \mathrm{F}_{3} \mathrm{ClO}\).

A \(1.100 \mathrm{g}\) sample of copper ore is dissolved, and the \(\mathrm{Cu}^{2+}(\mathrm{aq})\) is treated with excess KI. The liberated \(\mathrm{I}_{3}^{-}\) requires \(12.12 \mathrm{mL}\) of \(0.1000 \mathrm{M} \mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) for its titration. What is the mass percent copper in the ore?

Write balanced equations for the following important commercial reactions involving nitrogen and its compounds. (a) the principal artificial method of fixing atmospheric \(\mathrm{N}_{2}\) (b) oxidation of ammonia to \(\mathrm{NO}\) (c) preparation of nitric acid from \(\mathrm{NO}\).

What is the oxidation state of sulfur in the following compounds? (a) \(\mathrm{SF}_{4} ;\) (b) \(\mathrm{S}_{2} \mathrm{F}_{10} ;\) (c) \(\mathrm{H}_{2} \mathrm{S} ;\) (d) \(\mathrm{CaSO}_{3}\).

The best reducing agent of the following substances is (a) \(\mathrm{H}_{2} \mathrm{S} ;\) (b) \(\mathrm{O}_{3} ;\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4} ;\) (d) \(\mathrm{NaF}\); (e) \(\mathrm{H}_{2} \mathrm{O}\).
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