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Descriptive Inorganic Chemistry

James House, Kathleen A. House

Chapter 16

Halogens - all with Video Answers

Educators

Chapter Questions

04:03

Problem 1

Explain what differences would exist between the properties of a solution made by dissolving $\mathrm{Cl}_2 \mathrm{O}_7$ in water and dissolving $\mathrm{I}_2 \mathrm{O}_7$ in water. What is the origin of the differences?

Maryam Riaz
Maryam Riaz
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07:04

Problem 2

Draw structures for each of the following species.
(a) $\mathrm{BrF}_4^{+}$
(b) $\mathrm{Cl}_2 \mathrm{O}_7$
(c) $\mathrm{IBr}_2^{-}$
(d) $\mathrm{IF}_5$
(e) Periodic acid
(f) $\mathrm{IOF}_5$

David Collins
David Collins
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02:26

Problem 3

Write balanced equations for each of the following processes.
(a) Reaction of iodine trichloride with water
(b) Preparation of $\mathrm{NaOCl}$
(c) Preparation of $\mathrm{KI}_3$
(d) Disproportionation of $\mathrm{OCl}^{-}$
(e) Electrolysis of a dilute sodium chloride solution

Adriano Chikande
Adriano Chikande
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01:30

Problem 4

On the basis of energy, explain why fluorine is an even more reactive element than might be expected when compared to the reactivity of the other halogens.

Bin Chen
Bin Chen
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03:24

Problem 5

Iodine dissolved in carbon tetrachloride is purple. In acetone, the color is brown. Explain these observations.

Dr. Satish Ingale
Dr. Satish Ingale
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03:19

Problem 6

Discuss the reasons why $\mathrm{HF}$ is a weak acid.

LJ
Lena Jake
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01:04

Problem 7

Draw the molecular orbital energy level diagram for NO. What indication do you see for the observed chemistry of the molecule as it pertains to halogen chemistry?

Crystal Wang
Crystal Wang
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02:46

Problem 8

Write an equation to show how $\mathrm{SbF}_5$ behaves as an acid in liquid $\mathrm{BrF}_3$.

A. Elizabeth Hildreth
A. Elizabeth Hildreth
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Problem 9

Complete and balance the following.
(a) $\mathrm{MnO}_2+\mathrm{HCl} \stackrel{\text { heat }}{\longrightarrow}$
(b) $\mathrm{ClF}+\mathrm{H}_2 \mathrm{O} \rightarrow$
(c) $\mathrm{BrF}_3+\mathrm{AsF}_5 \rightarrow$
(d) $\mathrm{H}_2 \mathrm{O}+\mathrm{OF}_2 \rightarrow$
(e) $\mathrm{HClO}_3+\mathrm{P}_4 \mathrm{O}_{10} \rightarrow$

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00:46

Problem 10

Give formulas for three species that are isoelectronic with $\mathrm{Cl}_2 \mathrm{O}_7$ that do not contain halogen atoms.

Nicole Smina
Nicole Smina
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05:40

Problem 11

Complete and balance the following.
(a) $\mathrm{BrF}_3+\mathrm{H}_2 \mathrm{O} \rightarrow$
(b) $\mathrm{S}+\mathrm{ClF}_3 \rightarrow$
(c) $\mathrm{HI}+\mathrm{H}_2 \mathrm{SO}_4 \rightarrow$
(d) $\mathrm{ONF}+\mathrm{ClF} \rightarrow$

Shaelyn Deal
Shaelyn Deal
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Problem 12

Draw structures for the following species.
(a) $\mathrm{ClF}_2^{+}$
(b) $\mathrm{I}_3{ }^{-}$
(c) $\mathrm{ClO}_2^{-}$
(d) $\mathrm{I}_2 \mathrm{O}_7$
(e) $\mathrm{Br}_3^{+}$

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08:25

Problem 13

Complete and balance the following.
(a) $\mathrm{Ca}(\mathrm{OH})_2+\mathrm{Cl}_2 \rightarrow$
(b) $\mathrm{KMnO}_4+\mathrm{HCl} \rightarrow$
(c) $\mathrm{Cl}_2 \mathrm{O}+\mathrm{H}_2 \mathrm{O} \rightarrow$
(d) $\mathrm{NaOH}+\mathrm{I}_2 \rightarrow$
(e) $\mathrm{SO}_2 \mathrm{Cl}_2+\mathrm{H}_2 \mathrm{O} \rightarrow$

Evelyn Clay
Evelyn Clay
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02:14

Problem 14

Complete and balance the following.
(a) $\mathrm{F}_2+\mathrm{H}_2 \mathrm{O} \rightarrow$
(b) $\mathrm{ICl}+\mathrm{H}_2 \mathrm{O} \rightarrow$
(c) $\mathrm{KF}+\mathrm{IF}_5 \rightarrow$
(d) $\mathrm{SiO}_2+\mathrm{ClF}_3 \rightarrow$
(e) $\mathrm{PI}_3+\mathrm{H}_2 \mathrm{O} \rightarrow$

Niamat Khuda
Niamat Khuda
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01:26

Problem 15

Draw structures for the following.
(a) $\mathrm{IF}_6^{-}$
(b) $\mathrm{ClF}_2^{-}$
(c) $\mathrm{IF}_4^{+}$
(d) $\mathrm{OF}_2$
(e) $\mathrm{BrF}_4^{-}$

Jorge Villanueva
Jorge Villanueva
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01:24

Problem 16

Explain in terms of periodic properties why compounds such as $\mathrm{IClO}_4$ and $\mathrm{I}(\mathrm{py})_2 \mathrm{ClO}_4$ (py = pyridine) are much more stable than those with $\mathrm{Cl}$ replacing $\mathrm{I}$.

Narayan Hari
Narayan Hari
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03:13

Problem 17

For a cation containing two chlorine atoms and one fluorine atom $\left(\mathrm{Cl}_2 \mathrm{~F}^{+}\right)$, two structures are possible. Explain the difference in stability expected for these ions.

Shazia Naz
Shazia Naz
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01:39

Problem 18

Although chlorine is a stronger oxidizing agent than bromine, the following reaction takes place:
$$
2 \mathrm{ClF}_3+\mathrm{Br}_2 \rightarrow 2 \mathrm{BrF}_3+\mathrm{Cl}_2
$$
Explain this observation.

Dan Ni
Dan Ni
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01:14

Problem 19

Although $\mathrm{ClO}_4^{-}$does not coordinate to metal ions strongly, numerous complexes are known in which it is a ligand. Describe ways in which $\mathrm{ClO}_4{ }^{-}$could form coordinate bonds to metal ions.

Aadit Sharma
Aadit Sharma
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02:06

Problem 20

The I-O (the oxygen atom that does not have a hydrogen atom attached) bond length in $\mathrm{H}_5 \mathrm{IO}_6$ is $178 \mathrm{pm}$. Assume that a proton is removed to form the $\mathrm{H}_4 \mathrm{IO}_6{ }^{-}$ion. Which proton would likely be removed? In this ion, the length of the bonds between I and the two oxygen atoms with no hydrogen atom attached is $186 \mathrm{pm}$. Explain why this is different from the value of $178 \mathrm{pm}$ in $\mathrm{H}_5 \mathrm{IO}_6$.

Lottie Adams
Lottie Adams
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