Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 30

Give the name of the following binary compounds of transition metals using both the modern and older systems: (a) \(\mathrm{CuCl}\) and \(\mathrm{CuCl}_{2}\) (b) \(\mathrm{Fe}(\mathrm{OH})_{2}\) and \(\mathrm{Fe}(\mathrm{OH})_{3}\)

Short Answer

Expert verified
The binary compounds and their names are: (a) \(\mathrm{CuCl}\): copper(I) chloride (modern) or cuprous chloride (older system) \(\mathrm{CuCl}_{2}\): copper(II) chloride (modern) or cupric chloride (older system) (b) \(\mathrm{Fe}(\mathrm{OH})_{2}\): iron(II) hydroxide (modern) or ferrous hydroxide (older system) \(\mathrm{Fe}(\mathrm{OH})_{3}\): iron(III) hydroxide (modern) or ferric hydroxide (older system)

Step by step solution

01

Identify the transition metals and their oxidation states in each compound

For the given compounds: (a) \(\mathrm{CuCl}\) and \(\mathrm{CuCl}_{2}\). Copper (Cu) is the transition metal, and we need to find its oxidation state in each compound. (b) \(\mathrm{Fe}(\mathrm{OH})_{2}\) and \(\mathrm{Fe}(\mathrm{OH})_{3}\). Iron (Fe) is the transition metal, and we need to find its oxidation state in each compound.
02

Determine the oxidation states of copper in the given compounds

We can determine the oxidation state of a metal in a compound by considering the charges of the other elements in the compound. (a) In \(\mathrm{CuCl}\), chlorine (Cl) has a charge of -1. Therefore, the oxidation state of copper (Cu) must be +1 in order for the compound to be neutral. In \(\mathrm{CuCl}_{2}\), each chlorine (Cl) has a charge of -1, and there are two of them, which makes the total charge -2. Therefore, the oxidation state of copper (Cu) must be +2 in order for the compound to be neutral.
03

Determine the oxidation states of iron in the given compounds

Similarly, we can determine the oxidation state of iron in the compounds: (b) In \(\mathrm{Fe}(\mathrm{OH})_{2}\), each hydroxide (OH) has a charge of -1, and there are two of them, which makes the total charge -2. Therefore, the oxidation state of iron (Fe) must be +2 in order for the compound to be neutral. In \(\mathrm{Fe}(\mathrm{OH})_{3}\), each hydroxide (OH) has a charge of -1, and there are three of them, which makes the total charge -3. Therefore, the oxidation state of iron (Fe) must be +3 in order for the compound to be neutral.
04

Name the compounds using the modern (IUPAC) system

In the modern nomenclature, we use Roman numerals to indicate the oxidation state of the transition metal. (a) \(\mathrm{CuCl}\) is copper(I) chloride, as copper has an oxidation state of +1. \(\mathrm{CuCl}_{2}\) is copper(II) chloride, as copper has an oxidation state of +2. (b) \(\mathrm{Fe}(\mathrm{OH})_{2}\) is iron(II) hydroxide, as iron has an oxidation state of +2. \(\mathrm{Fe}(\mathrm{OH})_{3}\) is iron(III) hydroxide, as iron has an oxidation state of +3.
05

Name the compounds using the older system

In the older nomenclature, we use "-ous" and "-ic" suffixes to indicate the lower and higher oxidation states, respectively. (a) \(\mathrm{CuCl}\) is cuprous chloride, as copper has an oxidation state of +1 (the lower oxidation state). \(\mathrm{CuCl}_{2}\) is cupric chloride, as copper has an oxidation state of +2 (the higher oxidation state). (b) \(\mathrm{Fe}(\mathrm{OH})_{2}\) is ferrous hydroxide, as iron has an oxidation state of +2 (the lower oxidation state). \(\mathrm{Fe}(\mathrm{OH})_{3}\) is ferric hydroxide, as iron has an oxidation state of +3 (the higher oxidation state).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Experiments show that it takes more energy to break the bond between oxygen atoms in the \(\mathrm{O}_{2}\) molecule than in the \(\mathrm{O}_{3}\) molecule. How can you explain this?

Why is the oxygen atom listed first in \(\mathrm{OF}_{2}\) but last in \(\mathrm{Br}_{2} \mathrm{O} ?\)

Why is HF not considered an ionic compound even though its percent ionic character is greater than \(50 \%\) ?

Phosphorus (P) and bromine (Br) form a compound. Predict the formula of this compound starting with dot diagrams for the atoms.

The acetate ion has the formula \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\). Draw a dot diagram for it given the following atomic connections. (Hint: Watch for resonance forms.)
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free