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Chapter 8: Problem 46

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) \(\mathrm{TiCl}_{4}\) and \(\mathrm{CaF}_{2}\), (b) \(\mathrm{ClF}_{3}\) and \(\mathrm{VF}_{3}\), (c) \(\mathrm{SbCl}_{5}\) and \(\mathrm{AlF}_{3}\).

Short Answer

Expert verified
(a) \(\mathrm{TiCl}_{4}\): ionic, titanium tetrachloride; \(\mathrm{CaF}_{2}\): ionic, calcium fluoride. (b) \(\mathrm{ClF}_{3}\): molecular, chlorine trifluoride; \(\mathrm{VF}_{3}\): ionic, vanadium(III) fluoride. (c) \(\mathrm{SbCl}_{5}\): molecular, antimony pentachloride; \(\mathrm{AlF}_{3}\): ionic, aluminum fluoride.

Step by step solution

01

(a) Identify the type of bond in \(\mathrm{TiCl}_{4}\) and \(\mathrm{CaF}_{2}\)

To identify the bond type, we need to look at the elements involved in the compounds: - \(\mathrm{TiCl}_{4}\) consists of \(\mathrm{Ti}\) (a metal, titanium) and \(\mathrm{Cl}\) (a non-metal, chlorine). - \(\mathrm{CaF}_{2}\) consists of \(\mathrm{Ca}\) (a metal, calcium) and \(\mathrm{F}\) (a non-metal, fluorine). Since both compounds consist of a metal and a non-metal, they both exhibit ionic bonding.
02

(a) Name \(\mathrm{TiCl}_{4}\) and \(\mathrm{CaF}_{2}\) using ionic conventions

Ionic compounds are named by stating the cation (metal) first, followed by the anion (non-metal) with an "-ide" ending. - \(\mathrm{TiCl}_{4}\): titanium tetrachloride - \(\mathrm{CaF}_{2}\): calcium fluoride
03

(b) Identify the type of bond in \(\mathrm{ClF}_{3}\) and \(\mathrm{VF}_{3}\)

Again, let's look at the elements in each compound: - \(\mathrm{ClF}_{3}\) consists of \(\mathrm{Cl}\) (a non-metal, chlorine) and \(\mathrm{F}\) (a non-metal, fluorine). - \(\mathrm{VF}_{3}\) consists of \(\mathrm{V}\) (a metal, vanadium) and \(\mathrm{F}\) (a non-metal, fluorine). \(\mathrm{ClF}_{3}\) consists of only non-metals, indicating a covalent bond; \(\mathrm{VF}_{3}\) has both a metal and a non-metal, indicating an ionic bond.
04

(b) Name \(\mathrm{ClF}_{3}\) and \(\mathrm{VF}_{3}\) using relevant conventions

- \(\mathrm{ClF}_{3}\) (molecular): Use the standard covalent naming with prefixes: chlorine trifluoride. - \(\mathrm{VF}_{3}\) (ionic): vanadium(III) fluoride. (The (III) indicates a +3 charge on the vanadium ion).
05

(c) Identify the type of bond in \(\mathrm{SbCl}_{5}\) and \(\mathrm{AlF}_{3}\)

Once more, look at the elements in each compound: - \(\mathrm{SbCl}_{5}\) consists of \(\mathrm{Sb}\) (a metalloid, antimony) and \(\mathrm{Cl}\) (a non-metal, chlorine). - \(\mathrm{AlF}_{3}\) consists of \(\mathrm{Al}\) (a metal, aluminum) and \(\mathrm{F}\) (a non-metal, fluorine). \(\mathrm{SbCl}_{5}\) has a metalloid and a non-metal, indicating a molecular bond; \(\mathrm{AlF}_{3}\) has a metal and a non-metal, indicating an ionic bond.
06

(c) Name \(\mathrm{SbCl}_{5}\) and \(\mathrm{AlF}_{3}\) using relevant conventions

- \(\mathrm{SbCl}_{5}\) (molecular): antimony pentachloride. - \(\mathrm{AlF}_{3}\) (ionic): aluminum fluoride.

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Most popular questions from this chapter

Which of the following bonds are polar? (a) \(\mathrm{C}-\mathrm{O}\) (b) \(\mathrm{Sl}-\mathrm{F},(\mathbf{c}) \mathrm{N}-\mathrm{Cl}\) (d) \(\mathrm{C}-\mathrm{Cl}\). Which is the more electronegative atom in each polar bond?

(a) What is the trend in electronegativity going from left to right in a row of the periodic table? (b) How do electronegativity values generally vary going down a column in the periodic table? (c) True or false: The most easily ionizable elements are the most electronegative.

(a) Draw the best Lewis structure(s) for the nitrite ion, \(\mathrm{NO}_{2}^{-}\). (b) With what allotrope of oxygen is it isoelectronic? (c) What would you predict for the lengths of the bonds in \(\mathrm{NO}_{2}^{-}\) relative to \(\mathrm{N}-\mathrm{O}\) single bonds and double bonds?

Draw Lewis structures for the following: $(\mathbf{a}) \mathrm{CH}_{2} \mathrm{Cl}_{2},(\mathbf{b}) \mathrm{ClCN},\( (c) \)\mathrm{AsF}_{5}$ (d) \(\mathrm{CH}_{2} \mathrm{O}\) (C the central atom), (e) \(\mathrm{OF}_{2}\) (f) \(\mathrm{NO}_{3}^{-}\).

We can define average bond enthalpies and bond lengths for ionic bonds, just like we have for covalent bonds. Which ionic bond is predicted to be stronger, \(\mathrm{Na}-\mathrm{Cl}\) or \(\mathrm{Ca}-\mathrm{O}\) ?
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