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Chapter 9: Problem 78

Which of the following are ionic compounds? Which are covalent compounds? \(\mathrm{RbCl}, \mathrm{PF}_{5}, \mathrm{BrF}_{3},\) \(\mathrm{KO}_{2}, \mathrm{CI}_{4}\)

Short Answer

Expert verified
\(\mathrm{RbCl}\) and \(\mathrm{KO}_{2}\) are ionic compounds, while \(\mathrm{PF}_{5}, \mathrm{BrF}_{3},\) and \(\mathrm{CI}_{4}\) are covalent compounds.

Step by step solution

01

Understanding Compound Properties

Remember that ionic compounds form when a metal and nonmetal exchange electrons, whereas covalent compounds form when two or more nonmetals share electrons. In an elemental context, metals tend to occupy the left-hand side of the periodic table, while nonmetals occupy the right.
02

Identifying Ionic Compounds

\(\mathrm{RbCl}\) and \(\mathrm{KO}_{2}\) are both ionic compounds. They form when the metal atoms Rb and K lose electrons and the nonmetal atoms Cl and O gain them.
03

Identifying Covalent Compounds

\(\mathrm{PF}_{5}, \mathrm{BrF}_{3},\) and \(\mathrm{CI}_{4}\) are covalent compounds. These compounds form when the nonmetal atoms P, F, Br, and Cl share electrons.

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Most popular questions from this chapter

The following species have been detected in interstellar space: (a) \(\mathrm{CH},(\mathrm{b}) \mathrm{OH},(\mathrm{c}) \mathrm{C}_{2},(\mathrm{~d}) \mathrm{HNC},(\mathrm{e}) \mathrm{HCO} .\) Draw Lewis structures for these species and indicate whether they are diamagnetic or paramagnetic.

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) \(\mathrm{B}\) and \(\mathrm{F},\) (b) \(\mathrm{K}\) and \(\mathrm{Br}\)

What is a polar covalent bond? Name two compounds that contain one or more polar covalent bonds.

Most organic acids can be represented as \(\mathrm{RCOOH}\) where \(\mathrm{COOH}\) is the carboxyl group and \(\mathrm{R}\) is the rest of the molecule. (For example, \(\mathrm{R}\) is \(\mathrm{CH}_{3}\) in acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH} .\) ) (a) Draw a Lewis structure for the carboxyl group. (b) Upon ionization, the carboxyl group is converted to the carboxylate group, \(\mathrm{COO}^{-}\). Draw resonance structures for the carboxylate group.

List the following bonds in order of increasing ionic character: cesium to fluorine, chlorine to chlorine, bromine to chlorine, silicon to carbon.
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