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Chapter 8: Problem 45

In the following pairs of binary compounds determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) \(\mathrm{SiF}_{4}\) and \(\mathrm{LaF}_{3}\), (b) \(\mathrm{FeCl}_{2}\) and \(\mathrm{ReCl}_{6}\) (c) \(\mathrm{PbCl}_{4}\) and \(\mathrm{RbCl}\).

Short Answer

Expert verified
The identified compounds with their names are: (a) silicon tetrafluoride (molecular) and lanthanum fluoride (ionic), (b) iron(II) chloride (ionic) and rhenium hexachloride (molecular), (c) lead(IV) chloride (ionic) and rubidium chloride (ionic).

Step by step solution

01

Identify Metals and Nonmetals

First, we'll identify the metals and nonmetals in each pair of compounds: (a) \(\mathrm{SiF}_{4}\) and \(\mathrm{LaF}_{3}\) Silicon (Si) is a metalloid and Fluorine (F) is a nonmetal. Lanthanum (La) is a metal and Fluorine (F) is a nonmetal. (b) \(\mathrm{FeCl}_{2}\) and \(\mathrm{ReCl}_{6}\) Iron (Fe) is a metal, and Chlorine (Cl) is a nonmetal. Rhenium (Re) is a metal, and Chlorine (Cl) is a nonmetal. (c) \(\mathrm{PbCl}_{4}\) and \(\mathrm{RbCl}\) Lead (Pb) is a metal, and Chlorine (Cl) is a nonmetal. Rubidium (Rb) is a metal, and Chlorine (Cl) is a nonmetal.
02

Determine Molecular and Ionic Compounds

Now, we'll determine whether each compound is molecular or ionic based on the types of elements involved. (a) \(\mathrm{SiF}_{4}\) and \(\mathrm{LaF}_{3}\) \(\mathrm{SiF}_{4}\) is a molecular compound (metalloid and nonmetal). \(\mathrm{LaF}_{3}\) is an ionic compound (metal and nonmetal). (b) \(\mathrm{FeCl}_{2}\) and \(\mathrm{ReCl}_{6}\) \(\mathrm{FeCl}_{2}\) is an ionic compound (metal and nonmetal). \(\mathrm{ReCl}_{6}\) is a molecular compound (metal and nonmetal, but Re is an exception due to its covalent bonding nature). (c) \(\mathrm{PbCl}_{4}\) and \(\mathrm{RbCl}\) \(\mathrm{PbCl}_{4}\) is an ionic compound (metal and nonmetal). \(\mathrm{RbCl}\) is an ionic compound (metal and nonmetal).
03

Apply Naming Conventions

Finally, we will apply the naming conventions for each compound: (a) \(\mathrm{SiF}_{4}\) and \(\mathrm{LaF}_{3}\) \(\mathrm{SiF}_{4}\) (molecular) - silicon tetrafluoride \(\mathrm{LaF}_{3}\) (ionic) - lanthanum fluoride (b) \(\mathrm{FeCl}_{2}\) and \(\mathrm{ReCl}_{6}\) \(\mathrm{FeCl}_{2}\) (ionic) - iron(II) chloride \(\mathrm{ReCl}_{6}\) (molecular) - rhenium hexachloride (c) \(\mathrm{PbCl}_{4}\) and \(\mathrm{RbCl}\) \(\mathrm{PbCl}_{4}\) (ionic) - lead(IV) chloride \(\mathrm{RbCl}\) (ionic) - rubidium chloride

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Most popular questions from this chapter

Use Lewis symbols and Lewis structures to diagram the formation of \(\mathrm{PF}_{3}\) from \(\mathrm{P}\) and \(\mathrm{F}\) atoms.

(a) Determine the formal charge on the chlorine atom in the hypochlorite ion, \(\mathrm{ClO}^{-},\) and the perchlorate ion, \(\mathrm{ClO}_{4}^{-},\) using resonance structures where the \(\mathrm{Cl}\) atom has an octet. (b) What are the oxidation numbers of chlorine in \(\mathrm{ClO}^{-}\) and in \(\mathrm{ClO}_{4}^{-} ?\) (c) Is it uncommon for the formal charge and the oxidation state to be different? Explain. (d) Perchlorate is a much stronger oxidizing agent than hypochlorite. Would you expect there to be any relationship between the oxidizing power of the oxyanion and either the oxidation state or the formal charge of chlorine?

Which ionic compound is expected to form from combining the following pairs of elements: (a) barium and fluorine, (b) cesium and chlorine, (c) lithium and nitrogen, (d) aluminum and oxygen?

(a) Using average bond enthalpies, predict which of the following reactions will be most exothermic: (i) \(\mathrm{C}(g)+2 \mathrm{~F}_{2}(g) \longrightarrow \mathrm{CF}_{4}(g)\) (ii) \(\mathrm{CO}(g)+3 \mathrm{~F}_{2} \longrightarrow \mathrm{CF}_{4}(g)+\mathrm{OF}_{2}(g)\) (iii) \(\mathrm{CO}_{2}(g)+4 \mathrm{~F}_{2} \longrightarrow \mathrm{CF}_{4}(g)+2 \mathrm{OF}_{2}(g)\) (b) Explain the trend, if any, that exists between reaction exothermicity and the extent to which the carbon atom is bonded to oxygen.

(a) When talking about atoms in a Lewis structure, what is meant by the term formal charge? (b) Does the formal charge of an atom represent the actual charge on that atom? Explain. (c) How does the formal charge of an atom in a Lewis structure differ from the oxidation number of the atom?
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