Chapter 1, Inorganic Chemistry: The Periodic Table and the World We Live In Video Solutions, Principles of Descriptive Inorganic Chemistry

Problem 1

Write the characteristic valence electron configurations of the following atoms or ions: a. Fr;
b. As;
c. Pt;
d. Dy;
e. $\mathrm{Bi}^{3-}$;
f. $\mathrm{Bi}^{3+}$;
g. $\mathrm{Ba}^{2+}$;
h. $\mathrm{Pt}^{2+}$;
i. $\mathrm{Dy}^{3+}$;
j. Ge;
k. $\mathrm{Ge}^{2+}$;
1. Ge ${ }^{4-}$.

Nicole Smina

Numerade Educator

05:35

Problem 2

Write the characteristic valence electron configurations of the following atoms or ions: a. $\mathrm{Sr}$;
b. At;
c. W;
d. $\mathrm{Bk}$;
e. $\mathrm{S}^{2-}$;
f. $\mathrm{Tl}^{+}$;
g. $\mathrm{Cs}^{+}$;
h. $\mathrm{W}^{4+}$;
i. $\mathrm{Bk}^{3+}$;
j. Mn;
k. $\mathrm{Mn}^{4+}$;
l. Pa.

Susan Hallstrom

Numerade Educator

07:23

Problem 3

Write the Lewis dot structures of the following molecules or ions:
a. $\mathrm{CO}_2$;
b. $\mathrm{NO}_2^{-}$;
c. $\mathrm{NO}^{+}$;
d. $\mathrm{H}_2 \mathrm{O}_2$;
e. $\mathrm{CH}_4$;
f. $\mathrm{H}_2 \mathrm{SiBr}_2$;
g. $\mathrm{IF}_5$;
h. $\mathrm{OsO}_4$.

Nicholas Sacco

Numerade Educator

View

Problem 4

Write the Lewis dot structures of the following molecules or ions:
a. HCN;
b. $\mathrm{SO}_3^{2-}$
c. $\mathrm{NO}_2{ }^{+}$;
d. $\mathrm{XeF}_4$;
e. $\mathrm{H}_2 \mathrm{~N}-\mathrm{NH}_2$;
f. $\mathrm{SiH}_4$;
g. $\mathrm{ICl}_4^{-}$.

Tom Comey

Numerade Educator

13:00

Problem 5

Assign oxidation numbers to each atom in the molecules and ions of
a. question 3;
b. question 4 .

Sarah Bennett

Numerade Educator

02:10

Problem 6

Working from Lewis structures, assign oxidation numbers in the following molecules or ions: a. $\mathrm{HCCl}_3$;
b. $\mathrm{NSF}_3$;
c. $\mathrm{C}_2 \mathrm{H}_6$;
d. $\mathrm{C}_3 \mathrm{H}_7 \mathrm{Cl}$;
e. $\mathrm{Fe}(\mathrm{CO})_5 ; \quad$ f. $\mathrm{TeO}_6{ }^{6-}$.

Lottie Adams

Numerade Educator

13:00

Problem 7

Working from Lewis structures, assign oxidation numbers in the following molecules or ions: a. HOF;
b. $\mathrm{Si}_2 \mathrm{H}_6$;
c. $\mathrm{Si}_3 \mathrm{H}_8$;
d. $\mathrm{CSe}_2$;
e. $\mathrm{V}(\mathrm{CO})_6{ }^{-}$;
f. cyclo-(HN-BH) ;
g. $\mathrm{ClCH}_2-\mathrm{CH}_2 \mathrm{Cl}$.

Sarah Bennett

Numerade Educator

00:40

Problem 8

Without referring to Table B, describe the most common positive oxidation numbers to be expected in the following regions of the periodic table: a. $s$-block; b. left side of the $p$-block; $c$. right side of the $p$-block; d. left side of the $d$-block; e. right side of the $d$-block; $\mathrm{f}$. left side of the $f$-block; g. right side of the $f$-block.

David Collins

Numerade Educator

06:47

Problem 9

List all the known chemical elements that have six valence electrons (and no more). Then, without referring to Tables B or $\mathrm{C}$, circle those elements that commonly give up or share all six of those valence electrons with more electronegative elements to achieve an oxidation number of six. Give the atomic numbers of the next five elements that can be expected to have six valence electrons.

Shazia Naz

Numerade Educator

00:43

Problem 10

Without referring to Table C, arrange the following sets of atoms and ions in order of increasing radii:
$10.1 \mathrm{Cr}^{6+} ; \mathrm{Cr}^{4+} ; \mathrm{Cr}^{2+} ; \mathrm{Cr}^{3+}$.
$10.2 \mathrm{Ra}^{2+} ; \mathrm{Mg}^{2+} ; \mathrm{Be}^{2+} ; \mathrm{Sr}^{2+}$.
10.3 The ions of valence electron configuration $6 s^{\circ}$ between $\mathrm{Cs}$ and $\mathrm{Re}$.
10.4 The $f$-block +3 ions of Period 7 .

Lottie Adams

Numerade Educator

10:47

Problem 11

Without looking at the relevant tables, describe: a. the main horizontal trends in Pauling electronegativities; b, the main horizontal trends in ionic radii; c. the main horizontal trends in common oxidation numbers; d. the main vertical trends in Pauling electronegativities; e. the main vertical trends in ionic radii; $\mathrm{f}$. the main vertical trends in common oxidation numbers.

Tianyu Li

Numerade Educator

03:49

Problem 12

In what regions of the periodic table are there anomalous vertical trends in Pauling electronegativities? Are there corresponding anomalous vertical trends in these regions in ionic radii? Common positive oxidation numbers?

Yongyao Zhou

Numerade Educator

09:53

Problem 13

Make reasonable predictions of the following:
13.1 The valence electron configurations of the elements of atomic number 126,144 , and 162 .
13.2 The Pauling electronegativities of the elements directly below
a. U;
b. $\mathrm{Au}$;
c. At.
13.3 The common positive oxidation number for $\mathrm{Rn}$; the element number 121; the elements directly below $\mathrm{Np}$, No, $\mathrm{Os}, \mathrm{Pb}$.
13.4 Using Table 1.4, the ionic radii for the cations corresponding to the common positive oxidation numbers and the elements in the previous question.

Ren Jie Tuieng

Numerade Educator