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Chapter 2: Problem 61

Many ionic compounds contain either aluminum (a Group \(3 \mathrm{~A}\) metal) or a metal from Group \(1 \mathrm{~A}\) or Group \(2 \mathrm{~A}\) and a nonmetal - oxygen, nitrogen, or a halogen (Group \(7 \mathrm{~A}\) ). Write the chemical formulas and names of all the binary compounds that can result from such combinations.

Short Answer

Expert verified
The possible binary compounds that can be formed from the given metals and nonmetals include: Sodium Oxide (\( \mathrm{Na_2O} \)), Sodium Nitride (\( \mathrm{Na_3N} \)), Sodium Halides (\( \mathrm{NaX} \)), Magnesium Oxide (\( \mathrm{MgO} \)), Magnesium Nitride (\( \mathrm{Mg_3N_2} \)), Magnesium Halides (\( \mathrm{MgX_2} \)), Aluminum Oxide (\( \mathrm{Al_2O_3} \)), Aluminum Nitride (\( \mathrm{AlN} \)), and Aluminum Halides (\( \mathrm{AlX_3} \)). Note that \( X \) represents a halide.

Step by step solution

01

Identify the elements and their charges

The metals listed in the question (Group 1A, 2A and Aluminum from Group 3A) are all considered to be cations — they lose electrons and have positive charges. Nonmetals (Oxygen, Nitrogen, and Halogens from Group 7A) are anions — they gain electrons and have negative charges. Group 1A metals have +1 charge, Group 2A metals have +2 charge, and Aluminum has +3 charge. Oxygen and Nitrogen commonly have -2 and -3 charges respectively, while Halogens usually have -1 charge.
02

Write down all possible combinations

Combine each metal with each non-metal to form a binary compound. Make sure the total charge is neutral. For instance, Aluminum (Al, +3) and Oxygen (O, -2) can combine to form \( \mathrm{Al_2O_3} \). Applying this method, get all possible combinations of given metals and non-metals.
03

Naming the compounds

The names for binary ionic compounds typically follow the pattern of: Name of cation (metal) + Base name of anion (nonmetal) + 'ide'. Therefore, \( \mathrm{Al_2O_3} \) is called Aluminum Oxide.

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Most popular questions from this chapter

Of the 114 -elements known, only two are liquids at room temperature \(\left(25^{\circ} \mathrm{C}\right)\). What are they? (Hint: One element is a familiar metal and the other element is in Group 7A.)

Identify the following as elements or compounds: \(\mathrm{NH}_{3}, \mathrm{~N}_{2}, \mathrm{~S}_{8}, \mathrm{NO}, \mathrm{CO}, \mathrm{CO}_{2}, \mathrm{H}_{2}, \mathrm{SO}_{2}\)

Name these compounds: (a) \(\mathrm{Na}_{2} \mathrm{CrO}_{4},\) (b) \(\mathrm{K}_{2} \mathrm{HPO}_{4}\) (c) HBr (gas), (d) HBr (in water), (e) \(\mathrm{Li}_{2} \mathrm{CO}_{3},\) (f) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7},(\mathrm{~g}) \mathrm{NH}_{4} \mathrm{NO}_{2}\) (h) \(\mathrm{PF}_{3}\) (i) \(\mathrm{PF}_{5},\) (j) \(\mathrm{P}_{4} \mathrm{O}_{6}\) (k) \(\mathrm{CdI}_{2}\) - (I) \(\mathrm{SrSO}_{4},(\mathrm{~m}) \mathrm{Al}(\mathrm{OH})_{3},(\mathrm{n}) \mathrm{Na}_{2} \mathrm{CO}_{3} \cdot 10 \mathrm{H}_{2} \mathrm{O} .\)

List the types of radiation that are known to be emitted by radioactive elements.

Write the formulas for these compounds: (a) copper(I) cyanide, (b) strontium chlorite, (c) perchloric acid, (d) hydroiodic acid, (e) disodium ammonium phosphate, (f) lead(II) carbonate, (g) tin(II) fluoride, (h) tetraphosphorus decasulfide, (i) mercury(II) oxide, (j) mercury(I) iodide, (k) cobalt(II) chloride hexahydrate.
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