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Chapter 9: Problem 86

Give an example of an ion or molecule containing Al that (a) obeys the octet rule, (b) has an expanded octet, and (c) has an incomplete octet.

Short Answer

Expert verified
An example of a molecule that obeys the octet rule containing aluminum would be Aluminum chloride (AlCl3), given that the aluminum atom achieves a full set of eight valence electrons. It is important to note that due to Aluminum's placement in the periodic table, it cannot form an expanded octet. For an ion containing aluminum with an incomplete octet, an example is Aluminum monochloride (AlCl), where the aluminum atom has only seven valence electrons.

Step by step solution

01

Identifying a Molecule with Octet Rule

Remembering the octet rule, one needs to think about a molecule which contains the element aluminum and obeys the said rule. A suitable candidate for this is aluminum chloride (AlCl3). In each AlCl3 molecule, Aluminum (Al) loses three electrons, and each of the three chlorine (Cl) atoms gain one electron. Consequently, Aluminum (Al) achieves a full set of eight valence electrons (an octet).
02

Identifying a Molecule with Expanded Octet

In the case of an expanded octet, it's important to note that Aluminum due to its placement in the periodic table (Period 3), cannot form an expanded octet as this phenomenon typically occurs in heavier elements (from Period 3 and beyond). So, it is not a viable option to find a molecule consists of Aluminum that follows the expanded octet rule.
03

Identifying a Molecule with Incomplete Octet

In terms of incomplete octet molecules, one needs to identify a molecule where the aluminum atom has less than eight valence electrons. A potential candidate for this is Aluminium monochloride (AlCl). In this case, the Aluminum atom loses one electron and the Chlorine atom gains one electron, leaving the Aluminium atom with only seven valence electrons, hence an incomplete octet.

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Most popular questions from this chapter

Write Lewis structures for the following molecules: (a) ICl, (b) \(\mathrm{PH}_{3}\), (c) \(\mathrm{P}_{4}\) (each \(\mathrm{P}\) is bonded to three other \(\mathrm{P}\) atoms (d) \(\mathrm{H}_{2} \mathrm{~S}\), (e) \(\mathrm{N}_{2} \mathrm{H}_{4}\), (f) \(\mathrm{HClO}_{3}\), (g) \(\mathrm{COBr}_{2}\) (C is bonded to \(\mathrm{O}\) and \(\mathrm{Br}\) atoms).

Write the Lewis dot symbols of the reactants and products in the following reactions. (First balance the equations.) (a) \(\mathrm{Sr}+\mathrm{Se} \longrightarrow \mathrm{SrSe}\) (b) \(\mathrm{Ca}+\mathrm{H}_{2} \longrightarrow \mathrm{CaH}_{2}\) (c) \(\mathrm{Li}+\mathrm{N}_{2} \longrightarrow \mathrm{Li}_{3} \mathrm{~N}\) (d) \(\mathrm{Al}+\mathrm{S} \longrightarrow \mathrm{Al}_{2} \mathrm{~S}_{3}\)

Hydrazine borane, \(\mathrm{NH}_{2} \mathrm{NH}_{2} \mathrm{BH}_{3}\), has been proposed as a hydrogen storage material. When reacted with lithium hydride (LiH), hydrogen gas is released: $$ \mathrm{NH}_{2} \mathrm{NH}_{2} \mathrm{BH}_{3}+\mathrm{LiH} \longrightarrow \mathrm{LiNH}_{2} \mathrm{NHBH}_{3}+\mathrm{H}_{2} $$ Write Lewis structures for \(\mathrm{NH}_{2} \mathrm{NH}_{2} \mathrm{BH}_{3}\) and \(\mathrm{NH}_{2} \mathrm{NHBH}_{3}^{-}\) and assign all formal charges.

What is the difference between a Lewis dot symbol and a Lewis structure?

From the lattice energy of \(\mathrm{KCl}\) in Table 9.1 and the ionization energy of \(\mathrm{K}\) and electron affinity of \(\mathrm{Cl}\) in Tables 8.2 and \(8.3,\) calculate the \(\Delta H^{\circ}\) for the reaction $$ \mathrm{K}(g)+\mathrm{Cl}(g) \longrightarrow \mathrm{KCl}(s) $$
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