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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

Summarize the essential features of the Lewis octet rule. The octet rule applies mainly to the second period elements. Explain.

Methyl isocyanate, \(\mathrm{CH}_{3} \mathrm{NCO},\) is used to make certain pesticides. In December \(1984,\) water leaked into a tank containing this substance at a chemical plant to produce a toxic cloud that killed thousands of people in Bhopal, India. Draw Lewis structures for this compound, showing formal charges.

The formulas for the fluorides of the third-period elements are \(\mathrm{NaF}, \mathrm{MgF}_{2}, \mathrm{AlF}_{3}, \mathrm{SiF}_{4}, \mathrm{PF}_{5}, \mathrm{SF}_{6},\) and \(\mathrm{ClF}_{3}\). Classify these compounds as covalent or ionic.

What is Lewis's contribution to our understanding of the covalent bond?

Write Lewis structures for these four isoelectronic species: (a) CO, (b) \(\mathrm{NO}^{+},\) (c) \(\mathrm{CN}^{-},\) (d) \(\mathrm{N}_{2}\). Show formal charges.
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