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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
In short, we identified the type of compounds and assigned appropriate names as follows: (a) \(\mathrm{TiCl}_{4}\): Titanium(IV) Chloride (ionic) and \(\mathrm{CaF}_{2}\): Calcium Fluoride (ionic) (b) \(\mathrm{ClF}_{3}\): Chlorine Trifluoride (molecular) and \(\mathrm{VF}_{3}\): Vanadium(III) Fluoride (ionic) (c) \(\mathrm{SbCl}_{5}\): Antimony Pentachloride (molecular) and \(\mathrm{AlF}_{3}\): Aluminum Fluoride (ionic)

Step by step solution

01

Identify the elements involved in each compound

For \(\mathrm{TiCl}_{4}\), we have Titanium (Ti) and Chlorine (Cl). For \(\mathrm{CaF}_{2}\), we have Calcium (Ca) and Fluorine (F).
02

Determine the type of compound

Referring to the periodic table, we can see that Titanium (Ti) and Calcium (Ca) are metals. Chlorine (Cl) and Fluorine (F) are non-metals. Therefore, both compounds consist of a metal and non-metal combination, which means both substances are ionic compounds.
03

Assign names using the ionic naming convention

Using the ionic naming convention, we have: \(\mathrm{TiCl}_{4}\): Titanium(IV) Chloride \(\mathrm{CaF}_{2}\): Calcium Fluoride (b) \(\mathrm{ClF}_{3}\) and \(\mathrm{VF}_{3}\)
04

Identify the elements involved in each compound

For \(\mathrm{ClF}_{3}\), we have Chlorine (Cl) and Fluorine (F). For \(\mathrm{VF}_{3}\), we have Vanadium (V) and Fluorine (F).
05

Determine the type of compound

Chlorine (Cl) and Fluorine (F) are both non-metals, so \(\mathrm{ClF}_{3}\) is a molecular substance. Vanadium (V) is a metal, and Fluorine (F) is a non-metal, so \(\mathrm{VF}_{3}\) is an ionic substance.
06

Assign names using the appropriate naming conventions

Using the molecular naming convention for \(\mathrm{ClF}_{3}\) and the ionic naming convention for \(\mathrm{VF}_{3}\), we have: \(\mathrm{ClF}_{3}\): Chlorine Trifluoride \(\mathrm{VF}_{3}\): Vanadium(III) Fluoride (c) \(\mathrm{SbCl}_{5}\) and \(\mathrm{AlF}_{3}\)
07

Identify the elements involved in each compound

For \(\mathrm{SbCl}_{5}\), we have Antimony (Sb) and Chlorine (Cl). For \(\mathrm{AlF}_{3}\), we have Aluminum (Al) and Fluorine (F).
08

Determine the type of compound

Antimony (Sb) is a metalloid, while Chlorine (Cl) is a non-metal. Considering the properties of metalloids, for this case, we can treat Antimony (Sb) as a non-metal, thus \(\mathrm{SbCl}_{5}\) is a molecular substance. Aluminum (Al) is a metal, and Fluorine (F) is a non-metal, so \(\mathrm{AlF}_{3}\) is an ionic substance.
09

Assign names using the appropriate naming conventions

Using the molecular naming convention for \(\mathrm{SbCl}_{5}\) and the ionic naming convention for \(\mathrm{AlF}_{3}\), we have: \(\mathrm{SbCl}_{5}\): Antimony Pentachloride \(\mathrm{AlF}_{3}\): Aluminum Fluoride

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Most popular questions from this chapter

A major challenge in implementing the "hydrogen economy" is finding a safe, lightweight, and compact way of storing hydrogen for use as a fuel. The hydrides of light metals are attractive for hydrogen storage because they can store a high weight percentage of hydrogen in a small volume. For example, \(\mathrm{NaAlH}_{4}\) can release \(5.6 \%\) of its mass as \(\mathrm{H}_{2}\) upon decomposing to \(\mathrm{NaH}(s), \mathrm{Al}(s)\), and \(\mathrm{H}_{2}(g) . \mathrm{NaAlH}_{4}\) possesses both covalent bonds, which hold polyatomic anions together, and ionic bonds. (a) Write a balanced equation for the decomposition of \(\mathrm{NaAlH}_{4}\). (b) Which element in \(\mathrm{NaAlH}_{4}\) is the most electronegative? Which one is the least electronegative? (c) Based on electronegativity differences, predict the identity of the polyatomic anion. Draw a Lewis structure for this ion. (d) What is the formal charge on hydrogen in the polyatomic ion?

(a) True or false: The hydrogen atom is most stable when it has a full octet of electrons. (b) How many electrons must a sulfur atom gain to achieve an octet in its valence shell? (c) If an atom has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{3}\), how many electrons must it gain to achieve an octet?

An ionic substance of formula MX has a lattice energy of \(6 \times 10^{3} \mathrm{~kJ} / \mathrm{mol}\). Is the charge on the ion M likely to be \(1+, 2+\), or \(3+\) ? Explain.

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) Draw the dominant Lewis structure for the phosphorus trifluoride molecule, \(\mathrm{PF}_{\mathfrak{3} .}\) (b) Determine the oxidation numbers of the \(P\) and \(F\) atoms. (c) Determine the formal charges of the \(\mathrm{P}\) and \(\mathrm{F}\) atoms.
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