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Chapter 19: Problem 91

What is the hybridization of the underlined nitrogen atom in each of the following molecules or ions? a. \(\underline{N O}^{+}\) b. \(\mathrm{N}_{2} \mathrm{O}_{3}\left(\mathrm{O}_{2} \mathrm{N} \underline{\mathrm{NO}}\right)\) c. \(\underline{N O}_{2}^{-}\) d. \(\underline{N}_{2}\)

Short Answer

Expert verified
The hybridization states of the underlined nitrogen atoms in the given molecules or ions are: a. \(NO^{+}\): sp b. \(O_2NNO (N_2O_3)\): sp² c. \(NO_2^{-}\): sp² d. \(N_2\): sp²

Step by step solution

01

Finding Steric Number

Determine the steric number for each nitrogen atom (defined as the number of bond pairs and lone pairs around it): a. NO⁺ b. O₂NNO (N₂O₃) c. NO₂⁻ d. N₂
02

Determining Hybridization

Find the hybridization state of the underlined nitrogen atom in each molecule/ion using the steric number calculated from Step 1. a. NO⁺
03

Step 2a: Steric Number for NO⁺

In the case of NO⁺, there are two atoms bonded to the nitrogen (O and N⁺) and no lone pairs. So the steric number of the nitrogen is 2.
04

Step 2b: Hybridization of NO⁺

If the steric number is 2, the hybridization will be sp. Therefore, the hybridization of the underlined nitrogen atom in NO⁺ is sp. b. O₂NNO (N₂O₃)
05

Step 2c: Steric Number for N₂O₃

In the case of N₂O₃, there are three atoms bonded to the nitrogen atom (2 O atoms and 1 N atom) and no lone pairs. So the steric number of the nitrogen is 3.
06

Step 2d: Hybridization of N₂O₃

If the steric number is 3, the hybridization will be sp². Therefore, the hybridization of the underlined nitrogen atom in N₂O₃ (O₂NNO) is sp². c. NO₂⁻
07

Step 2e: Steric Number for NO₂⁻

In the case of NO₂⁻, there are two atoms bonded to the nitrogen atom (2 O atoms) and one lone pair. So the steric number of the nitrogen is 3.
08

Step 2f: Hybridization of NO₂⁻

If the steric number is 3, the hybridization will be sp². Therefore, the hybridization of the underlined nitrogen atom in NO₂⁻ is sp². d. N₂
09

Step 2g: Steric Number for N₂

In the case of N₂, there is one atom bonded to the nitrogen atom (another N atom) and two lone pairs. So the steric number of the nitrogen is 3.
10

Step 2h: Hybridization of N₂

If the steric number is 3, the hybridization will be sp². Therefore, the hybridization of the underlined nitrogen atom in N₂ is sp².

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Most popular questions from this chapter

Many structures of phosphorus-containing compounds are drawn with some \(P=O\) bonds. These bonds are not the typical \(\pi\) bonds we've considered, which involve the overlap of two \(p\) orbitals. Instead, they result from the overlap of a \(d\) orbital on the phosphorus atom with a \(p\) orbital on oxygen. This type of \(\pi\) bonding is sometimes used as an explanation for why \(\mathrm{H}_{3} \mathrm{PO}_{3}\) has the first structure below rather than the second:Draw a picture showing how a \(d\) orbital and a \(p\) orbital overlap to form a \(\pi\) bond.

How could you determine experimentally whether the compound \(\mathrm{Ga}_{2} \mathrm{Cl}_{4}\) contains two gallium(II) ions or one gallium(I) and one gallium(III) ion? (Hint: Consider the electron configurations of the three possible ions.)

Which of the following statement(s) is(are) true? a. The alkali metals are found in the earth's crust in the form of pure elements. b. Gallium has one of the highest melting points known for metals. c. When calcium metal reacts with water, one of the products is \(\mathrm{H}_{2}(\mathrm{~g})\) d. When \(\mathrm{AlCl}_{3}\) is dissolved in water, it produces an acidic solution. e. Lithium reacts in the presence of excess oxygen gas to form lithium superoxide.

Silicon is produced for the chemical and electronics industries by the following reactions. Give the balanced equation for each reaction. a. \(\mathrm{SiO}_{2}(s)+\mathrm{C}(s) \longrightarrow \mathrm{Si}(s)+\mathrm{CO}(g)\). b. Silicon tetrachloride is reacted with very pure magnesium, producing silicon and magnesium chloride. c. \(\mathrm{Na}_{2} \mathrm{SiF}_{6}(s)+\mathrm{Na}(s) \longrightarrow \mathrm{Si}(s)+\mathrm{NaF}(s)\).

Although nitrogen trifluoride (NF \(_{3}\) ) is a thermally stable compound, nitrogen triodide \(\left(\mathrm{NI}_{3}\right)\) is known to be a highly explosive material. \(\mathrm{NI}_{3}\) can be synthesized according to the equation $$\mathrm{BN}(s)+3 \mathrm{IF}(g) \longrightarrow \mathrm{BF}_{3}(g)+\mathrm{NI}_{3}(g)$$. a. What is the enthalpy of formation for \(\mathrm{NI}_{3}(s)\) given the enthalpy of reaction \((-307 \mathrm{kJ})\) and the enthalpies of formation for \(\mathrm{BN}(s)(-254 \mathrm{kJ} / \mathrm{mol}), \operatorname{IF}(g)(-96 \mathrm{kJ} / \mathrm{mol}),\) and \(\mathrm{BF}_{3}(g)(-1136 \mathrm{kJ} / \mathrm{mol}) ?\) b. It is reported that when the synthesis of \(\mathrm{NI}_{3}\) is conducted using 4 moles of IF for every 1 mole of BN, one of the by-products isolated is \(\left[\mathrm{IF}_{2}\right]^{+}\left[\mathrm{BF}_{4}\right]^{-} .\) What are the molecular geometries of the species in this by-product? What are the hybridizations of the central atoms in each species in the by-product?
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