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Chapter 3: Problem 67

Name the following compounds and specify which ones are best described as ionic: (a) \(\mathrm{OF}_{2} ;\) (b) \(\mathrm{XeF}_{2}\) (c) \(\operatorname{CuSO}_{3} ;\) (d) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\)

Short Answer

Expert verified
The compounds are named as: (a) Oxygen difluoride, (b) Xenon difluoride, (c) Copper(II) Sulfate and (d) Diammonium hydrogen phosphate. Copper(II) Sulfate and Diammonium hydrogen phosphate are ionic compounds.

Step by step solution

01

Naming \( \mathrm{OF}_{2} \)

The compound \( \mathrm{OF}_{2} \) is a molecule formed from oxygen (O) and fluorine (F). Since it is formed from non-metals, we can suggest it's not an ionic compound. Oxygen difluoride is the correct IUPAC name for this compound.
02

Naming \( \mathrm{XeF}_{2} \)

The compound \( \mathrm{XeF}_{2} \) is formed from Xenon (Xe) and Fluorine (F), both Non-Metals, thus it's probably not ionic. The naming of compounds of noble gases usually involve their full name and the non-metal they bond with. Hence, the name of \( \mathrm{XeF}_{2} \) is Xenon difluoride.
03

Naming \( \operatorname{CuSO}_{3} \)

The compound \( \operatorname{CuSO}_{3} \) is formed by copper (Cu, a Metal) and Sulfate (SO3, an ion), thus likely an ionic compound. Copper has variable oxidation states, and in this case it is in the 2+ state, leading to the name: Copper(II) sulfate.
04

Naming \( \left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4} \)

The compound \( \left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4} \) is formed by the ammonium ion (\( (NH_4)^+ \)) and the hydrogen phosphate ion (\( HPO_4^- \)). As it involves ions, it's an ionic compound. The IUPAC name would be: Diammonium hydrogen phosphate.

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Most popular questions from this chapter

In an experiment, \(244 \mathrm{mL}\) of chlorine gas \(\left(\mathrm{Cl}_{2}, d=2.898 \mathrm{g} / \mathrm{L}\right)\) combines with iodine to give \(1.553 \mathrm{g}\) of a binary compound. In a separate experiment, the molar mass of the compound is found to be about \(467 \mathrm{g} / \mathrm{mol} .\) What is the molecular formula of this compound?

Name these compounds: (a) \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2} ;\) (b) \(\mathrm{HNO}_{2}\); (c) \(\operatorname{Cr} \mathrm{O}_{2} ;\) (d) \(\mathrm{KIO}_{3} ;\) (e) \(\mathrm{LiCN} ;\) (f) \(\mathrm{KIO} ;\) (g) \(\mathrm{Fe}(\mathrm{OH})_{2}\) (h) \(\mathrm{Ca}\left(\mathrm{H}_{2} \mathrm{PO}_{4}\right)_{2} ;\) (i) \(\mathrm{H}_{3} \mathrm{PO}_{4} ;\) (j) \(\mathrm{NaHSO}_{4} ;\) (k) \(\mathrm{Na}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\); (l) \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2} ;(\mathrm{m}) \mathrm{MgC}_{2} \mathrm{O}_{4} ;\) (n) \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\)

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