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Chapter 9: Problem 9

Name one ionic compound that contains only nonmetallic elements.

Short Answer

Expert verified
One example of an ionic compound that contains only nonmetallic elements is Nitrogen Trifluoride (NF3).

Step by step solution

01

Understand Ionic Compounds

Ionic compounds are usually formed by the combination of metals with nonmetals. The metals lose electrons to become positively charged ions, and the nonmetals accept those electrons to become negatively charged ions. The compound is held together by the electrostatic attraction between these ions.
02

Identify Non-Metallic Elements Which Can Form Ionic Bonds

When it comes to ionic compounds involving only nonmetals, some halogens, specifically elements like Fluorine (F), can exhibit properties akin to metals due to their high electronegativity. They can attract electrons from other nonmetals to form ionic bonds.
03

Combine Non-Metallic Elements to Form Ionic Compounds

One example of such compounds can be Nitrogen Trifluoride (NF3), where Fluorine (F) behaves like a metal due to its high electronegativity, and Nitrogen (N), being less electronegative in this scenario, behaves like the nonmetal.

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Most popular questions from this chapter

Define bond enthalpy. Bond enthalpies of polyatomic molecules are average values. Why?

Four atoms are arbitrarily labeled \(\mathrm{D}, \mathrm{E}, \mathrm{F},\) and \(\mathrm{G}\). Their electronegativities are: \(\mathrm{D}=3.8, \mathrm{E}=3.3, \mathrm{~F}=\) \(2.8,\) and \(\mathrm{G}=1.3\). If the atoms of these elements form the molecules DE, DG, EG, and DF, how would you arrange these molecules in order of increasing covalent bond character?

Write Lewis structures for the reaction $$ \mathrm{AlCl}_{3}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AlCl}_{4}^{-} $$ What kind of bond is between \(\mathrm{Al}\) and \(\mathrm{Cl}\) in the product?

Is it possible to "trap" a resonance structure of a compound for study? Explain.

The triiodide ion \(\left(\mathrm{I}_{3}^{-}\right)\) in which the \(\mathrm{I}\) atoms are arranged as III is stable, but the corresponding \(\mathrm{F}_{3}^{-}\) ion does not exist. Explain.
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