Name the following ionic compounds: (a) Li 2 O (b) FeCl 3 (c) NaClO (d) CaSO 3 (e) Cu(OH) 2

Hey everyone, let's go ahead and practice naming the following compound And identifying the formula for Iron three phosphate. Starting off with a we have C. U. Two S. 043. So we know that we have copper. Now before we name this, let's go ahead and determine the charge of copper since copper can have more than one possible charge. And that's because it's a transition metal. And the reason why this is important is because its charge is going to affect the way we name it. So to determine this we're going to need to look a bit more closely at our sulfate. So we know that sulfate is one of our poly atomic ions and sulfate has a minus to charge. And we can see right here that we needed three of sulfate and two of copper in order to balance out this whole compound. So reversing our criss cross method, we can see that we have that subscript of two written as the minus to charge for sulfate. So that must mean copper has a plus three charge. So when we named this, we're going to name this as copper three sulfate And we're going to denote its charge with that Roman numeral three and that's going to be our final answer. Now moving on to be we have iron three phosphate. So we know that iron is F. E. And we know that it's going to have a plus three charge and that's because we have that roman numeral three written right here and we know that phosphate is are poly atomic ion which has a charge of three minus. So doing our criss cross method, we're going to end up with a formula of f e p Since we have a 1-1 ratio between our charges. So this is going to be our final answers for both questions. So I hope this made sense and let us know if you have any other questions.

Ch.2 - Atoms, Molecules, and Ions

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.2 - Atoms, Molecules, and Ions

Problem 71a,b,c,d,e

Chapter 2, Problem 71a,b,c,d,e

Name the following ionic compounds: (a) Li₂O (b) FeCl₃ (c) NaClO (d) CaSO₃ (e) Cu(OH)₂

Verified step by step guidance

Identify the cation and anion in the compound. Here, Cu represents copper and OH represents the hydroxide ion.

Determine the charge of the hydroxide ion, which is -1.

Recognize that the subscript '2' next to OH indicates there are two hydroxide ions, giving a total charge of -2.

Since the compound is neutral, the copper cation must balance the -2 charge from the hydroxide ions. Therefore, copper must have a +2 charge.

Name the compound by combining the name of the cation with its oxidation state in Roman numerals and the name of the anion. The compound is named Copper(II) hydroxide.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively charged cations and negatively charged anions. These oppositely charged ions attract each other, creating a stable compound. Understanding the nature of ionic bonds is essential for naming and writing formulas for these compounds.

Nomenclature of Ionic Compounds

The nomenclature of ionic compounds involves specific rules for naming the cations and anions. Typically, the cation retains its elemental name, while the anion's name is derived from its elemental name, often modified to end in '-ide' for simple anions. For transition metals, the oxidation state is indicated using Roman numerals.

Hydroxide Ion

The hydroxide ion (OH⁻) is a polyatomic ion consisting of one oxygen atom covalently bonded to one hydrogen atom, carrying a negative charge. It is commonly found in bases and plays a crucial role in the naming of compounds that contain it, such as hydroxides. Recognizing hydroxide's presence is vital for accurately naming compounds like Cu(OH)₂.

Name the following ionic compounds: (a) Li2O (b) FeCl3 (c) NaClO (d) CaSO3 (e) Cu(OH)2