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Chapter 2: Problem 94

Correct each of the following names: (a) CuI is cobalt(II) iodide. (b) \(\mathrm{Fe}\left(\mathrm{HSO}_{4}\right)_{3}\) is iron(II) sulfate. (c) \(\mathrm{MgCr}_{2} \mathrm{O}_{7}\) is magnesium dichromium heptaoxide. (d) \(\mathrm{CaCl}_{2}\) is calcium(II) dichloride.

Short Answer

Expert verified
(a) copper(I) iodide, (b) iron(III) hydrogen sulfate, (c) magnesium dichromate, (d) calcium chloride

Step by step solution

01

Correct the Name for CuI

Examine the name provided for CuI. Cu (copper) can have a charge of +1 or +2. Since iodine (I) always has a -1 charge, copper must be +1 for the compound to be neutral. Therefore, the correct name for CuI is copper(I) iodide.
02

Correct the Name for \(\mathrm{Fe}(\mathrm{HSO}_{4})_3\)

Examine the name for \(\mathrm{Fe}(\mathrm{HSO}_{4})_3\). Here, \(\mathrm{HSO}_{4}\) (hydrogen sulfate) has a -1 charge and there are three of them, making a total charge of -3. Thus, iron must have a +3 charge to balance. The correct name is iron(III) hydrogen sulfate.
03

Correct the Name for \(\mathrm{MgCr}_{2} \mathrm{O}_{7}\)

Examine the name for \(\mathrm{MgCr}_{2} \mathrm{O}_{7}\). \(\mathrm{Cr}_{2} \mathrm{O}_{7} \) (dichromate) has a -2 charge, and magnesium (Mg) has a +2 charge. Therefore, the correct name is magnesium dichromate.
04

Correct the Name for \(\mathrm{CaCl}_{2}\)

Examine the name for \(\mathrm{CaCl}_{2}\). Calcium (Ca) always has a +2 charge, consistently forming compounds as calcium chloride. The correct name is simply calcium chloride.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

ionic compounds
Ionic compounds are formed when atoms transfer electrons between each other, resulting in the formation of ions. These ions are held together by strong electrostatic forces called ionic bonds. Typically, ionic compounds occur between metals and non-metals. The metal loses electrons to become a positively charged cation, while the non-metal gains electrons to become a negatively charged anion. This transfer leads to the formation of a stable ionic compound with a neutral overall charge.
For instance:
  • NaCl (sodium chloride) - sodium (metal) loses one electron to chlorine (non-metal).
  • MgO (magnesium oxide) - magnesium (metal) loses two electrons to oxygen (non-metal).
Understanding how these bonds form helps in accurately naming the compounds.
copper(I) iodide
Copper(I) iodide, also known as cuprous iodide, is an ionic compound consisting of copper and iodine. Copper can exhibit multiple oxidation states, +1 and +2. In the compound CuI, copper has a +1 charge, and iodine has a -1 charge.
Here's why:
  • Copper (Cu) ion: Cu+
  • Iodine (I) ion: I-
The charges balance each other out, resulting in a neutral compound. The Roman numeral I in the name indicates the +1 oxidation state of copper. It is essential to use this naming convention to distinguish between different copper compounds, like copper(II) iodide (CuI2).
iron(III) hydrogen sulfate
Iron(III) hydrogen sulfate is an ionic compound composed of iron (Fe) and hydrogen sulfate (HSO4). Iron can have multiple oxidation states, such as +2 and +3.
For \(\text{Fe(HSO}_4)_3\), iron has a +3 charge, and hydrogen sulfate has a -1 charge:
Fe - Iron(III) ion: Fe3+
HSO4 - Hydrogen sulfate ion: HSO4-
Since there are three hydrogen sulfate ions (each with -1 charge), they collectively have a -3 charge. This means the iron must have a +3 charge to balance it out, finally making the compound iron(III) hydrogen sulfate.
The Roman numeral III denotes the +3 oxidation state of iron in the compound.
magnesium dichromate
Magnesium dichromate is an ionic compound where magnesium (Mg) and dichromate (Cr2O7) combine. Magnesium always has a +2 charge, while dichromate has a -2 charge:
Mg - Magnesium ion: Mg2+
Cr2O7 - Dichromate ion: Cr2O72-
The charges balance each other, ensuring that the compound remains neutral. The formula for the compound is given as MgCr2O7.
Understanding the charges of the specific ions helps in naming such compounds correctly. In this case, 'magnesium dichromate' clearly states the ions involved and their charges, following standard naming protocol for ionic compounds.
calcium chloride
Calcium chloride is a simple and commonly known ionic compound composed of calcium (Ca) and chlorine (Cl). Calcium typically has a +2 charge, while chlorine has a -1 charge:
Ca - Calcium ion: Ca2+
Cl - Chloride ion: Cl-
To form a neutral compound, one calcium ion bonds with two chloride ions, resulting in the formula CaCl2. Unlike some other metals, calcium has only one common oxidation state (+2), simplifying the naming process. Thus, calcium chloride is a straightforward name without any need for Roman numerals.
This clarity is essential for avoiding confusion and ensuring accurate communication in chemistry.

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Most popular questions from this chapter

How is a structural formula similar to a molecular formula? How is it different?

A compound of copper and sulfur contains \(88.39 \mathrm{~g}\) of metal and 44.61 g of nonmetal. How many grams of copper are in \(5264 \mathrm{~kg}\) of compound? How many grams of sulfur?

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Name the technique(s) and briefly describe the procedure for separating each of the following mixtures into pure components: (a) table salt and pepper; (b) drinking water contaminated with soot; (c) crushed ice and crushed glass; (d) table sugar dissolved in ethanol; (e) two pigments (chlorophyll a and chlorophyll b) from spinach leaves.

Give the systematic names for the formulas or the formulas for the names: (a) \(\mathrm{Na}_{2} \mathrm{HPO}_{4} ;\) (b) ammonium perchlorate; (c) \(\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2} \cdot 3 \mathrm{H}_{2} \mathrm{O} ;\) (d) sodium nitrite.
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