Chapter 8, The Hard and Soft Acid-Base (HSAB) Principle and Its Applications Video Solutions, Principles of Descriptive Inorganic Chemistry

Problem 1

In each of the following complexes, classify both the metal ions and each ligand as hard, soft, or borderline: $\mathrm{a} .\left(\mathrm{NH}_4\right)_2\left[\mathrm{Pd}(-\mathrm{SCN})_4\right]$;
b. $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_4\left(\mathrm{SeO}_4\right)\right] \mathrm{ClO}_4$.

Shazia Naz

Numerade Educator

01:53

Problem 2

Draw the Lewis dot structures of the following molecules or ions, identify the potential donor atoms in each, and classify the donor atoms as hard, soft, or borderline bases: $\mathrm{a} . \mathrm{NH}_3$;
c. $\mathrm{SO}_4{ }^{2-}$;
d. $\mathrm{SO}_3^{2-}$.
b. $\mathrm{NH}_2-\mathrm{CH}_2-\mathrm{COOH}$ (an amino acid);

Vasu Makani

Numerade Educator

01:08

Problem 3

Classify each Lewis acid and each Lewis base in the following complexes as hard, soft, or borderline. a. $\left[\mathrm{Na}\left(\mathrm{CH}_3-\mathrm{O}-\mathrm{CH}_2-\mathrm{CH}_2-\mathrm{O}-\mathrm{CH}_3\right)_3\right]^{+}$
b. $\left[\mathrm{SnI}_6\right]^{2-}$
c. $\left[\mathrm{HgCl}_2\right]$
d. $\left[\mathrm{Hg}\left(\mathrm{CH}_3\right)_2\right]$

Shazia Naz

Numerade Educator

01:52

Problem 4

Rewrite each of these lists of Lewis acids or bases so that each is in increasing order of softness: $\mathrm{a} . \mathrm{Cu}^{+}, \mathrm{Au}^{+}, \mathrm{Ag}^{+}, \mathrm{K}^{+}$;
b. $\mathrm{Br}^{-}, \mathrm{I}^{-}, \mathrm{F}^{-}, \mathrm{Cl}^{-}$;
c. $\mathrm{Mo}^{2+}, \mathrm{Mo}^{6+}, \mathrm{Mo}^{4+}$;
d. $\mathrm{BF}_3, \mathrm{~B}\left(\mathrm{OCH}_3\right)_3, \mathrm{~B}\left(\mathrm{CH}_3\right)_3$ :
e. $\mathrm{FHg}^{+}, \mathrm{CH}_3 \mathrm{Hg}^{+}, \mathrm{Fe}^{2+}, \mathrm{Fe}^{3+} ; \quad$ f. $\left(\mathrm{CH}_3\right)_2 \mathrm{~S},\left(\mathrm{CH}_3\right)_2 \mathrm{Se},\left(\mathrm{CH}_3\right)_2 \mathrm{O}$.

David Collins

Numerade Educator

05:11

Problem 5

Most oxo anions are hard bases, but some are ambidentate and may also act as soft bases. List some of these.

Pam Owens

Numerade Educator

02:19

Problem 6

Predict whether reactants (left side) or products (right side) will be favored in each of the following equilibria:
6.1 $\mathrm{As}_2 \mathrm{~S}_5+5 \mathrm{HgO} \rightleftharpoons \mathrm{As}_2 \mathrm{O}_5+5 \mathrm{HgS}$
6.2 $\mathrm{ZnI}_2+\mathrm{HgCl}_2 \rightleftharpoons \mathrm{ZnCl}_2+\mathrm{HgI}_2$
$6.3 \mathrm{La}_2\left(\mathrm{CO}_3\right)_3+\mathrm{Bi}_2 \mathrm{~S}_3 \rightleftharpoons \mathrm{La}_2 \mathrm{~S}_3+\mathrm{Bi}_2\left(\mathrm{CO}_3\right)_3$
$6.42 \mathrm{CH}_3 \mathrm{MgF}+\mathrm{HgF}_2 \rightleftharpoons\left(\mathrm{CH}_3\right)_2 \mathrm{Hg}+2 \mathrm{MgF}_2$
6.5 $\mathrm{AgF}+\mathrm{LiI} \rightleftharpoons \mathrm{AgI}+\mathrm{LiF}$
6.6 $\left[\mathrm{Cu}(\text { thiourea })_4\right]^{+}+\left[\mathrm{Cu}(\text { urea })_4\right]^{2+} \rightleftharpoons\left[\mathrm{Cu}(\text { thiourea })_4\right]^{2+}+$ $\left[\mathrm{Cu}(\text { urea })_4\right]^{+}$
$$
\begin{aligned}
& \text { 6.7 } \mathrm{PbSe}+\mathrm{HgS} \rightleftharpoons \mathrm{HgSe}+\mathrm{PbS} \\
& 6.83 \mathrm{FeO}+\mathrm{Fe}_2 \mathrm{~S}_3 \rightleftharpoons \mathrm{Fe}_2 \mathrm{O}_3+3 \mathrm{FeS} \\
& 6.9 \mathrm{CdSO}_4+\mathrm{CaS} \rightleftharpoons \mathrm{CdS}+\mathrm{CaSO}_4 \\
& 6.10 \mathrm{Zn}\left(\mathrm{SCH}_3\right)_2+\mathrm{Hg}\left(\mathrm{SeCH}_3\right)_2 \rightleftharpoons \mathrm{Hg}\left(\mathrm{SCH}_3\right)_2+\mathrm{Zn}\left(\mathrm{SeCH}_3\right)_2 \\
& 6.112 \mathrm{Fe}(\mathrm{SCN})_3+3 \mathrm{Fe}(\mathrm{OCN})_2 \rightleftharpoons 2 \mathrm{Fe}(\mathrm{OCN})_3+3 \mathrm{Fe}(\mathrm{SCN})_2 \\
& 6.12 \mathrm{CaS}+\mathrm{ZnSeO}_4 \rightleftharpoons \mathrm{ZnS}+\mathrm{CaSeO}_4 \\
&
\end{aligned}
$$

Sriparna Bhattacharjee

Numerade Educator

06:55

Problem 7

Give plausible products (or just one product) for each of the following reactions, or tell if no reaction is expected.
$7.1 \mathrm{CdSO}_4+\mathrm{MgS} \rightarrow$
$7.2\left(\mathrm{CH}_3\right)_2 \mathrm{Hg}+\mathrm{CaF}_2 \rightarrow$

Adriano Chikande

Numerade Educator

01:33

Problem 8

Predict any products that will precipitate in each of the following mixtures in water:
8.1 $\mathrm{HgCl}_2+\mathrm{KI}+\mathrm{KF}$
8.2 $\mathrm{PrCl}_3+\mathrm{Na}_2 \mathrm{~S}$
8.3 $\mathrm{TlNO}_3+\mathrm{KI}+\mathrm{KF}$

Ronald Prasad

Numerade Educator

02:17

Problem 9

What do relative electronegativities suggest about the nature of the bond between a hard acid and a hard base? a soft acid and a soft base?

Lottie Adams

Numerade Educator

02:17

Problem 10

Are the ionic radii and charges of hard acids and bases also favorable to the kind of bonding you cited in the previous question? Explain.

Lottie Adams

Numerade Educator

02:58

Problem 11

Hydrogen and boron do not have electronegativities characteristic of hard acids, yet the $\mathrm{H}^{+}$and $\mathrm{B}^{3+}$ ions are classified as hard acids. Which of their properties other than electronegativity might justify such a classification?

Sima Sarker

Numerade Educator

01:52

Problem 12

What other characteristic of acids and bases-besides their hardness and softness-determines whether a reaction will go to the left or to the right?

Shahina -

Numerade Educator

01:28

Problem 13

Circle all insoluble salts: CdTe; AgI; AgF; KI; EuSe; $\mathrm{TiO}_2 ; \mathrm{TiTe}_2 ; \mathrm{PtAs}_2$.

Lottie Adams

Numerade Educator

03:31

Problem 14

Give the symbols for two metal ions that would fall into each of the groups of the qualitative analysis scheme.

Prashant Bana

Numerade Educator

01:55

Problem 15

Into which group of the qualitative analysis scheme will each of the following ions fall? a. $\mathrm{Tl}^{+}$;
b. $\mathrm{Cu}^{+}$:
c. $\mathrm{Rb}^{+}$;
d. $\mathrm{Cr}^{3+}$ :
e. $\mathrm{Sn}^{2+}$

Ronald Prasad

Numerade Educator

03:18

Problem 16

Predict in which group of the qualitative analysis scheme each of the following metal ions would occur. If the metal ion gives a precipitate, write the formula of the precipitate: a. $\mathrm{Sn}^{2+}$;
b. $\mathrm{Pr}^{3+}$;
c. $\mathrm{Cu}^{+}$;
d. $\mathrm{Sr}^{2+}$;
e. $\mathrm{Sb}^{3+}$;
f. $\mathrm{Eu}^{3+}$
g. $\mathrm{Au}^{+}$;
h. $\mathrm{Ra}^{2+}$;
i. $\mathrm{Rb}^{+}$.

Shahina -

Numerade Educator

01:09

Problem 17

Answer the following questions about the following metal ions: $\mathrm{a} . \mathrm{Zr}^{4+}$;
b. $\mathrm{Ag}^{+}$;
c. $\mathrm{Sb}^{3+}$.
17.1 Is its bromide soluble or insoluble?
17.2 Is its selenide soluble or insoluble?
17.3 Is its oxide soluble or insoluble?
17.4 In which group of the qualitative analysis scheme does this metal ion occur?
17.5 Is this metal a lithophile?
17.6 Which is the more likely mineral source: a silicate, a sulfide, or seawater?

Eileen Sullivan

Numerade Educator

00:48

Problem 18

Classify each element as $(A)$ a lithophile or $(B)$ either a chalcophile or a siderophile. Then choose its most likely mineral source.
18.1 $\mathrm{La}$; source: $\mathrm{LaPO}_4, \mathrm{LaAs}^2, \mathrm{Lal}_3$, or $\mathrm{LaCl}_3$.
18.2 Pt; source: $\mathrm{PtAs}_2, \mathrm{PtN}_2, \mathrm{PtSiO}_4$, or $\mathrm{PtF}_2$.
18.3 $\mathrm{Zr}$; source: $\mathrm{ZrSiO}_4, \mathrm{ZrPbS}_4$, or $\mathrm{ZrCl}_4$.
18.4 $\mathrm{Sb}$; source: $\mathrm{Sb}_2\left(\mathrm{SiO}_3\right)_3, \mathrm{Sb}_2 \mathrm{~S}_3, \mathrm{SbF}_3$, or $\mathrm{SbCl}_3$.
18.5 Te; source: $\mathrm{TeF}_4, \mathrm{Na}_2 \mathrm{Te}, \mathrm{PbTe}$, or $\mathrm{TeI}_4$.
$18.6 \mathrm{Be}$; source: $\mathrm{Be}^{2+}$ (aq), $\mathrm{Be}_3 \mathrm{Al}_2 \mathrm{Si}_6 \mathrm{O}_{18}$, or $\mathrm{BeSeS}_2$.
$18.7 \mathrm{~F}$; source: $\mathrm{F}^{-}(\mathrm{aq}), \mathrm{CaF}_2$, or $\mathrm{HgF}_2$.
18.8 Co; source: $\mathrm{CoCO}_3, \mathrm{CoAs}_2$, or $\mathrm{Co}^{2+}$ (aq).
18.9 Th; source: $\mathrm{ThS}_2, \mathrm{ThO}_2$, or $\mathrm{Th}^{4+}(\mathrm{aq})$.

Jorge Villanueva

Numerade Educator

01:50

Problem 19

Which are more generally toxic, soft-acid metal ions or hard-acid metal ions? To which type of biochemical ligand would soft-acid metal ions bind most strongly? a. phosphate groups; b. porphyrin groups (nitrogen donor); c. cysteine groups (sulfur donor).

Marissa Turner

Numerade Educator

01:18

Problem 20

Which of the following medicinal chemicals would be most effective in combating poisoning by a soft-acid metal ion:
FIGURE CANT COPY

Alkendra Singh

Numerade Educator

02:20

Problem 21

Consider the following six ligands. a. List them in order of increasing softness (note that some will be equally soft). b. Which one of these might make the best medicine to combat poisoning by the $\mathrm{Pt}^{2+}$ ion? What principles did you use to choose this ligand?
FIGURE CANT COPY

Marissa Turner

Numerade Educator

01:00

Problem 22

Briefly explain why the element selenium is necessary for life and protects against mercury poisoning but is also highly poisonous itself.

Lena Jake

Numerade Educator

02:23

Problem 23

Which of the following manners of disrupting protein structure would you expect to be most uniquely associated with the heavy-metal ions? a. Hydrolysis of the $\mathrm{CO}-\mathrm{NH}$ (peptide) linkages; $\mathbf{b}$. disruption of hydrogen bonding between different $\mathrm{CO}-\mathrm{NH}$ groups; $\mathrm{c}$. disruption of $\mathrm{S}-\mathrm{S}$ bond formation between different cysteine amino acid S-H groups; d. disruption of the electrostatic attraction of oppositely charged amino acid side chains.

Nimi Das

Numerade Educator

00:59

Problem 24

Compare the compounds $\left(\mathrm{CH}_3\right)_3 \mathrm{SnCl}$ and $\mathrm{F}_3 \mathrm{SnCl}$ : a. Which should show the highest electronegativity for $\mathrm{tin}$ ? b. Which should show the strongest $\mathrm{Sn}-\mathrm{Cl}$ bond?

Lottie Adams

Numerade Educator

03:47

Problem 25

The electronegativity of carbon in $\mathrm{CCl}_4$ is estimated as 2.64; the electronegativity of carbon in $\left(\mathrm{CH}_3\right)_3 \mathrm{CCl}$ is estimated as 2.29 . Compute the expected $\mathrm{C}-\mathrm{Cl}$ bond energy in each compound.

Adriano Chikande

Numerade Educator

01:06

Problem 26

You are given the following bond energies: $\mathrm{Ge}-\mathrm{Ge}=188 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{Cl}-\mathrm{Cl}=$ $240 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{Ge}-\mathrm{Cl}$ (in $\mathrm{GeCl}_2$ ) $=385 \mathrm{~kJ} / \mathrm{mol}$. Calculate the electronegativity of $\mathrm{Ge}$ in $\mathrm{GeCl}_2$. Does your answer differ from the Pauling electronegativity of $\mathrm{Ge}$ in $\mathrm{GeCl}_4$ (2.01) in the expected manner? Explain.

Lottie Adams

Numerade Educator

03:49

Problem 27

For which elements (other than iodine, used in an example) are there appropriate data in Tables 6.5 and 8.3 to 8.6 for the calculation of the effects of changing oxidation numbers on the Pauling electronegativities of elements? Carry out such calculations for two of those elements.

Yongyao Zhou

Numerade Educator

04:48

Problem 28

Some new elements have just been discovered in the author's laboratory. The following atomic parameters have been obtained:
TABLE CANT COPY
28.1 Will products or reactants be favored in the equilibrium Sheltonium Benneride + Coatsium Kamelide $\rightleftharpoons$ Sheltonium Kamelide + Coatsium Benneride?
28.2 Calculate the covalent bond energies expected for the CoatsiumKamelogen bond; for the Sheltonium-Bennerine bond.

Pam Owens

Numerade Educator