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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

A rule for drawing plausible Lewis structures is that the central atom is invariably less electronegative than the surrounding atoms. Explain why this is so.

Of the noble gases, only \(\mathrm{Kr}, \mathrm{Xe},\) and \(\mathrm{Rn}\) are known to form a few compounds with \(\mathrm{O}\) and/or \(\mathrm{F}\). Write Lewis structures for these molecules: (a) \(\mathrm{XeF}_{2},\) (b) \(\mathrm{XeF}_{4}\) (c) \(\mathrm{XeF}_{6},\) (d) \(\mathrm{XeOF}_{4},\) (e) \(\mathrm{XeO}_{2} \mathrm{~F}_{2}\). In each case Xe is the central atom.

For each of the following pairs of elements, state whether the binary compound they form is likely to be ionic or covalent. Write the empirical formula and name of the compound: (a) I and \(\mathrm{Cl}\), (b) \(\mathrm{Mg}\) and \(\mathrm{F}\).

Give three examples of compounds that do not satisfy the octet rule. Write a Lewis structure for each.

Write three resonance structures for the isocyanate ion (CNO \(^{-}\) ). Rank them in importance.
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