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Chapter 2: Problem 66

Write the formula for each of the following compounds: a. zinc chloride d. aluminum sulfide b. \(\operatorname{tin}(\mathrm{IV})\) fluoride e. mercury(I) selenide c. calcium nitride f. silver iodide

Short Answer

Expert verified
ZnCl\(_2\), SnF\(_4\), Ca\(_3\)N\(_2\), Al\(_2\)S\(_3\), Hg\(_2\)Se, AgI

Step by step solution

01

a. zinc chloride

: In zinc chloride, the cation is zinc (Zn) with a charge of +2, and the anion is chloride (Cl) with a charge of -1. To form a neutral compound, you will need two chloride ions for every zinc ion. The chemical formula for zinc chloride is ZnCl\(_2\).
02

b. tin(IV) fluoride

: In tin(IV) fluoride, the cation is tin with a Roman numeral (IV) which indicates an oxidation state of +4. The symbol for tin is Sn. The anion is fluoride (F) with a charge of -1. To form a neutral compound, you will need four fluoride ions for every tin ion. The chemical formula for tin(IV) fluoride is SnF\(_4\).
03

c. calcium nitride

: In calcium nitride, the cation is calcium (Ca) with a charge of +2, and the anion is nitride (N) with a charge of -3. To form a neutral compound, you will need three calcium ions for every two nitride ions. The chemical formula for calcium nitride is Ca\(_3\)N\(_2\).
04

d. aluminum sulfide

: In aluminum sulfide, the cation is aluminum (Al) with a charge of +3, and the anion is sulfide (S) with a charge of -2. To form a neutral compound, you will need two aluminum ions for every three sulfide ions. The chemical formula for aluminum sulfide is Al\(_2\)S\(_3\).
05

e. mercury(I) selenide

: In mercury(I) selenide, the cation is mercury with a Roman numeral (I) which indicates an oxidation state of +1. The symbol for mercury is Hg. The anion is selenide (Se) with a charge of -2. As mercury(I) forms a diatomic ion (Hg\(_2\)) with a combined charge of +2, one diatomic mercury(I) ion will combine with one selenide ion. The chemical formula for mercury(I) selenide is Hg\(_2\)Se.
06

f. silver iodide

: In silver iodide, the cation is silver (Ag) with a charge of +1, and the anion is iodide (I) with a charge of -1. They combine in a 1:1 ratio to form a neutral compound. The chemical formula for silver iodide is AgI.

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Most popular questions from this chapter

You have gone back in time and are working with Dalton on a table of relative masses. Following are his data. \(0.602 \mathrm{~g}\) gas A reacts with \(0.295 \mathrm{~g}\) gas \(\mathrm{B}\) \(0.172 \mathrm{~g}\) gas \(\mathrm{B}\) reacts with \(0.401 \mathrm{~g}\) gas \(\mathrm{C}\) \(0.320 \mathrm{~g}\) gas \(\mathrm{A}\) reacts with \(0.374 \mathrm{~g}\) gas \(\mathrm{C}\) a. Assuming simplest formulas \((\mathrm{AB}, \mathrm{BC}\), and \(\mathrm{AC}\) ), construct a table of relative masses for Dalton. b. Knowing some history of chemistry, you tell Dalton that if he determines the volumes of the gases reacted at constant temperature and pressure, he need not assume simplest formulas. You collect the following data: 6 volumes gas \(A+1\) volume gas \(B \rightarrow 4\) volumes product 1 volume gas \(\mathrm{B}+4\) volumes gas \(\mathrm{C} \rightarrow 4\) volumes product 3 volumes gas \(\mathrm{A}+2\) volumes gas \(\mathrm{C} \rightarrow 6\) volumes product Write the simplest balanced equations, and find the actual relative masses of the elements. Explain your reasoning.

Which of the following statements are true? For the false statements, correct them. a. Most of the known elements are metals. b. Element 118 should be a nonmetal. c. Hydrogen has mostly metallic properties. d. A family of elements is also known as a period of elements. e. When an alkaline earth metal, A, reacts with a halogen, X. the formula of the covalent compound formed should be \(\mathrm{A}_{2} \mathrm{X}\).

Write the formula for each of the following compounds: a. chromium(VI) oxide b. disulfur dichloride c. nickel(II) fluoride d. potassium hydrogen phosphate e. aluminum nitride f. ammonia g. manganese(IV) sulfide h. sodium dichromate i. ammonium sulfite j. carbon tetraiodide

By analogy with phosphorus compounds, name the following: \(\mathrm{Na}_{3} \mathrm{AsO}_{4}, \mathrm{H}_{3} \mathrm{AsO}_{4}, \mathrm{Mg}_{3}\left(\mathrm{SbO}_{4}\right)_{2}\)

A reaction of 1 liter of chlorine gas \(\left(\mathrm{Cl}_{2}\right)\) with 3 liters of fluorine gas \(\left(\mathrm{F}_{2}\right)\) yields 2 liters of a gaseous product. All gas volumes are at the same temperature and pressure. What is the formula of the gaseous product?
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