Chapter 9, The Halides, Nitrides, and Sulfides of the Elements Video Solutions, Principles of Descriptive Inorganic Chemistry

Problem 1

Which of the following hypothetical halides probably do not actually exist? $\mathrm{LaF}_3, \mathrm{SF}_6, \mathrm{CI}_4, \mathrm{BiI}_5, \mathrm{CuBr}_2, \mathrm{XeBr}_4, \mathrm{~S}_2 \mathrm{I}_2, \mathrm{WF}_6, \mathrm{FeI}_3, \mathrm{MnF}_7, \mathrm{AuI}_3, \mathrm{IF}_7$, $\mathrm{FeBr}_3$.

Lottie Adams

Numerade Educator

01:01

Problem 2

Among the halides from the previous list that do exist, pick the ones that are most likely to be intensely colored.

Narayan Hari

Numerade Educator

10:08

Problem 3

Which of the following halides of bismuth is most intensely colored? $\mathrm{BiF}_3$, $\mathrm{BiCl}_3, \mathrm{BiBr}_3$, or $\mathrm{BiI}_3$.

Ronald Prasad

Numerade Educator

Problem 4

For each of the halides listed, choose one of the following four general synthetic routes as the most appropriate (workable yet simple) method of synthesis of the anhydrous halide: Method 1, anhydrous salt results from evaporating the reaction mixture of the metal hydroxide plus the hydrohalic acid; Method 2, the salt precipitates in anhydrous form upon mixing solutions containing the cation and the anion; Method 3, the hydrated halide can be dehydrated by an appropriate chemical dehydrating agent; Method 4 , a strictly anhydrous method of synthesis (halogen exchange or redox) is required. Halides: a. $\mathrm{CF}_4$;
b. AgI;
c. KF;
d. $\mathrm{SiCl}_4$;
e. $\mathrm{BiCl}_3$;
f. $\mathrm{SiI}_4$ :
g. AuI;
h. $\mathrm{RbBr}$;
i. $\mathrm{NiCl}_2$;
j. $\mathrm{BiBr}_3$;
k. $\mathrm{LaF}_3$;
I. $\mathrm{SnCl}_2$;
m. $\mathrm{PrCl}_3$ :
n. $\mathrm{WF}_6$.

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01:29

Problem 5

For any of the above halides assigned, complete and balance an equation showing a plausible synthesis of that halide in anhydrous form.

Lottie Adams

Numerade Educator

01:19

Problem 6

Consider the synthesis of one of the halides listed at the end of this question. (1) Discuss the applicability of each of the seven synthetic methods listed in Section 9.3 to this halide. (2) Look up the synthesis of the halide in an advanced text, such as [3] or Cotton and Wilkinson, Comprehensive Inorganic Chemistry, 4th ed., Wiley-Interscience, New York, 1980. What methods are given there? Do they agree with your prediction? (3) Look up the actual details of the synthesis in the reference cited in the advanced text, in an inorganic lab manual, in Inorganic Syntheses, in [2], or in Chemical Abstracts. Are there important details (such as carrying out the synthesis in a dry or nonoxidizing atmosphere) that you would have expected from the principles of this book? Are there important details that you could not have anticipated? Halides: a. $\mathrm{MoCl}_5$;
b. $\left[\mathrm{Mo}_6 \mathrm{Cl}_8\right] \mathrm{Cl}_4$;
c. $\mathrm{VCl}_4$;
d. $\mathrm{TiBr}_4$.
e. $\mathrm{CrBr}_3$;
f. $\mathrm{CrI}_3$.

Lottie Adams

Numerade Educator

02:55

Problem 7

Choose one of the following thre: siructural classifications (monomeric or dimeric molecular, macromolecular, or ionic) and one of the following four categories of physical state at room temperature (gas, liquid, solid with a low melting point, or solid with a high melting point) for each of the following halides: a. $\mathrm{CF}_4$;
b. AgI;
c. $\mathrm{KF}$;
d. $\mathrm{SiCl}_4$;
e. $\mathrm{BiCl}_3$;
f. $\mathrm{SiI}_4$;
g. AuI;
h. $\mathrm{RbBr}$ :
i. $\mathrm{NiCl}_2$;
j. $\mathrm{BiBr}_3$;
k. $\mathrm{LaF}_3$;
I. $\mathrm{SnCl}_2$;
m. $\mathrm{PrCl}_3$;
n. $\mathrm{WF}_6$.

Natalie Johns

Numerade Educator

01:33

Problem 8

Give actual examples of catenated halides from each of the following groups:
a. $16 /$ VIA;
b. $15 / \mathrm{VA}$;
c. 14/IVA;
d. 13 IIIA.

Ronald Prasad

Numerade Educator

03:39

Problem 9

Give the structural types of the following halides, in all of which the central atom has the group oxidation number minus two: $\mathrm{InI}, \mathrm{SnCl}_2, \mathrm{SbBr}_3, \mathrm{TeCl}_4$, $\mathrm{IF}_5$. Discuss the reasons for the trends in this series.

Crystal Wang

Numerade Educator

03:38

Problem 10

From each of the following series of halides, pick the one that should have the lowest melting point, and explain why:
10.1 IF, BrF, ClF, $\mathrm{F}_2$
10.2 $\mathrm{MgF}_2, \mathrm{MgCl}_2, \mathrm{MgBr}_2, \mathrm{MgI}_2$
10.3 $\operatorname{InI}, \mathrm{SnCl}_2, \mathrm{SbBr}_3, \mathrm{TeCl}_4, \mathrm{IF}_5$
10.4 $\mathrm{SiF}_4, \mathrm{SiCl}_4, \mathrm{SiBr}_4, \mathrm{SiI}_4$

Shazia Naz

Numerade Educator

03:38

Problem 11

$\mathrm{GeCl}_4$ is a liquid with a melting point of $223^{\circ} \mathrm{K} ; \mathrm{GeCl}_2$ is a solid with a melting point of about $400^{\circ} \mathrm{K}$. Is this the normal trend to be expected for two monomeric covalent compounds of these formulas? Is this the normal trend to be expected for two ionic compounds of these stoichiometries? If neither, explain why the melting points fall in this order.

Shazia Naz

Numerade Educator

09:56

Problem 12

On the bench in a professor's laboratory are six bottles containing the products of the syntheses of the six halides $\mathrm{CrCl}_3, \mathrm{HgI}_2, \mathrm{NF}_3, \mathrm{NI}_3, \mathrm{SnCl}_2$, and $\mathrm{SnCl}_4$. Unfortunately the labels have come loose. Examine the bottles, and reattach the labels correctly. Bottle A contains a white solid; bottle B contains an intensely red solid; bottle $\mathrm{C}$ contains a colorless gas; bottle $\mathrm{D}$ contains light violet flakes; bottle E contains a colorless liquid; and bottle F consists of broken glass-all that remains after an explosive attempted preparation of its would-be contents.

Susan Hallstrom

Numerade Educator

01:07

Problem 13

Examine a copy of Table A, the Pauling electronegativity table. Assuming that metal-halogen bonding will be ionic for Pauling electronegativity differences in excess of 1.8 but polar covalent for differences less than 1.8 , identify all metals that you would expect to have ionic fluorides but polar covalent chlorides. Taking into account the likely formulas of these halides, describe how these fluorides and chlorides will differ in terms of structural types, volatility, and solubility in water and in nonaqueous solvents.

Osman Elomda

Numerade Educator

06:28

Problem 14

Classify each of the following halides as: (1) predominantly a Lewis acid; (2) predominantly a Lewis base; (3) neither: $\mathrm{a}$. $\mathrm{CF}_4$;
b. Agl;
c. $\mathrm{KF}_{\text {; }}$
d. $\mathrm{SiCl}_4$;
e. $\mathrm{BiCl}_3$;
f. $\mathrm{SiF}_4$ :
g. $\mathrm{Hgl}_2$;
h. $\mathrm{RbBr}$;
i. $\mathrm{BaCl}_2$;
j. $\mathrm{BiBr}_3$;
k. $\mathrm{CeF}_4$;
1. $\mathrm{PF}_3$;
m. $\mathrm{FeCl}_3$;
n. $\mathrm{SF}_6$;
o. AsF :
p. $\mathrm{IF}_7$ :
q. $\mathrm{XeF}_6$;
r. $\mathrm{PI}_5$.

Bobby Barnes

University of North Texas

01:32

Problem 15

Complete and balance plausible Lewis acid-base reactions between appropriate pairs of halides in the previous question.

Crystal Wang

Numerade Educator

02:17

Problem 16

List four halides that would likely be strong oxidizing agents; four that would likely be useful reducing agents. Complete and balance plausible redox reactions between appropriate pairs of these halides.

Lottie Adams

Numerade Educator

02:56

Problem 17

Complete and balance equations showing the products from the following pairs of reactants, or write "NR" if no reaction will occur: $\mathrm{a}$. $\mathrm{PF}_5+\mathrm{CsF}$;
b. $\mathrm{XeF}_6+\mathrm{CF}_4$ :
c. $\mathrm{RbBr}+\mathrm{BaBr}_2$;
d. $\mathrm{XeF}_6+\mathrm{BF}_3$;
e. $\mathrm{NaF}+\mathrm{AlF}_3$;
f. $\mathrm{SnCl}_2+\mathrm{PbCl}_4$;
g. $\mathrm{GeCl}_3{ }^{-}+\mathrm{IrCl}_6{ }^{3-}$;
h. $\mathrm{ClF}_3+\mathrm{UO}_3$;
i. $\mathrm{PI}_5+\mathrm{ZnI}_2 ; \quad$ j. $\mathrm{CH}_3 \mathrm{I}+\mathrm{NaCl}+$ acetone solvent.

Rajesh Singh

Numerade Educator

00:54

Problem 18

(1) Which of the following lattice types are layer structures? a. fluorite;
b. rock salt:
c. cadmium iodide;
d. chromium chloride;
e. rutile;
f. nickel arsenide;
g. graphite;
h. diamond.
(2) Tell for each of the following types of halide or chalcogenide which of the above lattice types is most likely, assuming an appropriate radius ratio:
a. MO;
b. MS:
c. $\mathrm{MO}_2$;
d. $\mathrm{MS}_2$;
e. MTe;
f. MF;
g. $\mathrm{MF}_2$;
h. $\mathrm{MI}_2$.

Eugene Schneider

University of Minnesota - Twin Cities

01:36

Problem 19

Predict the structure of each of the following halides or derivatives using VSEPR theory, and compare your prediction to the actual structure. Discuss the reasons for any discrepancies: a. $\mathrm{SF}_6$;
b. $\mathrm{XeF}_6$ :
c. $\mathrm{SF}_4$;
d. $\mathrm{TeF}_4$;
e. $\mathrm{TeCl}_4$ :
f. $\mathrm{S}_2 \mathrm{Cl}_2$;
g. $\mathrm{SO}_2 \mathrm{Cl}_2$;
h. $\mathrm{SOCl}_2$;
i. $\mathrm{P}\left(\mathrm{OCH}_3\right)_3$;
j. $\mathrm{PCl}_3$;
k. $\mathrm{SbCl}_3$;
I. IF ;
m. $\mathrm{PI}_5$.

Lottie Adams

Numerade Educator

01:02

Problem 20

Write balanced chemical equations illustrating reasonable methods of preparation of the following compounds: a. $\mathrm{KOC}_2 \mathrm{H}_5$;
b. $\mathrm{As}\left(\mathrm{OCH}_3\right)_3$;
c. VO $\left[\mathrm{N}\left(\mathrm{CH}_3\right)_2\right]_3$ :
d. $\mathrm{B}_3 \mathrm{Cl}_3 \mathrm{~N}_3\left(\mathrm{CH}_3\right)_3$;
e. $S_4 N_4$;
f. $\left[\mathrm{N}=\mathrm{P}\left(\mathrm{OCH}_3\right)_2\right]_3$ :
g. $\mathrm{ZnS}$;
h. CaS.

Lottie Adams

Numerade Educator

10:14

Problem 21

Suggest an inorganic polymer or macromolecule that might be suitable if you needed the following properties: a. a semiconductor that would convert electrical energy to ultraviolet light; $b$. a polymer that would exhibit metallic conduction in one dimension only; $\mathbf{c}$. a macromolecule that would exhibit metallic conduction in two dimensions only; d. a polymer that might slowly hydrolyze to release the anticancer drug cisplatin in the blood; $\mathbf{e}$. a ceramic that would maintain its strength to $1000^{\circ} \mathrm{C} ; \mathbf{f}$. a lubricating oil of low viscosity; g. a solid lubricant.

Shalini Tyagi

Numerade Educator