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Chapter 4: Problem 3

Which chemical formulas are consistent with the guidelines for creating ionic compounds? Explain your thinking. a. LiCI \(\quad\) b. \(\operatorname{LiCl}_{2} \quad\) c. \(\mathrm{MgCl}\) d. \(\mathrm{MgCl}_{2} \quad\) e. \(\mathrm{AlCl}_{3}\)

Short Answer

Expert verified
Correct formulas are (a) LiCl, (d) MgCl鈧�, (e) AlCl鈧�.

Step by step solution

01

Understanding Ionic Compounds

Ionic compounds are formed when metals transfer electrons to nonmetals, resulting in positive and negative ions that attract each other. The total charge in an ionic compound must be neutral, meaning the positive and negative charges must balance each other.
02

Analyzing Each Compound

The compounds need to be analyzed based on the charges of the ions that make them up: (a) LiCl - Lithium (Li) has a charge of +1 and chlorine (Cl) has a charge of -1. The charges are balanced, so this is correct. (b) LiCl鈧� - The charge of Li is +1, whereas Cl is -1, thus Li would require two Cl atoms to balance, making LiCl鈧� incorrect. (c) MgCl - Magnesium (Mg) has a charge of +2 and Cl has a charge of -1, these charges do not balance, so this is incorrect. (d) MgCl鈧� - Mg is +2 and each Cl is -1, thus two Cl balances one Mg, making it correct. (e) AlCl鈧� - Aluminum (Al) is +3 and each Cl is -1, thus three Cl atoms balance one Al, making it correct.

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Key Concepts

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

Chemical Formulas
Chemical formulas represent the types and numbers of atoms in a compound and are crucial in understanding ionic compounds. For ionic compounds, a chemical formula must show the ratio of ions where the total charges balance out to zero. This means that the positive charges of the metal ions must equal the negative charges of the nonmetal ions.

When forming ionic compounds:
  • The metal is always written first, followed by the nonmetal.
  • The subscripts in the formula indicate the number of each ion needed to balance the total charge.
  • An accurate chemical formula is necessary because it provides a blueprint of the compound's identity and structure.
For example, in the compound MgCl\(_2\), the subscript "2" beside Cl indicates that two chlorine ions are needed for every magnesium ion to ensure charge neutrality.
Charge Balance
Charge balance is a fundamental rule for the composition of ionic compounds. Every ionic compound must be electrically neutral. This means that the total positive charge from metal ions must offset the total negative charge from nonmetal ions.

To achieve this balance:
  • Identify the charges of the ions involved. For example, Mg has a charge of +2 and Cl has a charge of -1.
  • Calculate how many ions are needed to neutralize the charge. In MgCl\(_2\), two Cl\(^-\) ions (totaling -2 charge) are needed to balance the +2 charge of one Mg ion.
  • Make sure the overall charge of the formula is zero by adjusting the ratios of the ions accordingly.
Understanding charge balance ensures the correct formulation of ionic compounds, keeping them stable and predictable.
Electron Transfer
Electron transfer is the key process in the formation of ionic compounds. Metals lose electrons, while nonmetals gain those electrons. This transfer results in the formation of positive and negative ions, which then attract each other to form a stable ionic bond.

Here's how it works:
  • Metals have a tendency to lose electrons because of their low ionization energy, resulting in positively charged ions (cations).
  • Nonmetals tend to gain electrons due to their high electron affinity, resulting in negatively charged ions (anions).
  • For instance, a lithium atom loses one electron to become Li\(^+\), and a chlorine atom gains this electron to become Cl\(^-\). They attract each other to form LiCl.
This electron exchange is what solidifies the formation of ionic compounds, making them essential to the structure of many minerals and materials.
Metal and Nonmetal Ions
Ionic compounds are typically composed of metal and nonmetal ions. Understanding the properties of these ions is crucial to predicting the structure and behavior of ionic compounds.

**Metal Ions:**
  • Generally located on the left side of the periodic table, metals tend to lose electrons easily.
  • Examples include lithium (Li\(^+\)), magnesium (Mg\(^{2+}\)), and aluminum (Al\(^{3+}\)).
**Nonmetal Ions:**
  • Generally found on the right side of the periodic table, nonmetals tend to gain electrons.
  • Examples include chlorine (Cl\(^-\)), oxygen (O\(^{2-}\)), and nitrogen (N\(^{3-}\)).
The interaction between these metal cations and nonmetal anions forms the foundation of ionic compounds. This interaction results in compounds with high melting and boiling points and the ability to conduct electricity when dissolved.

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Most popular questions from this chapter

For each of these compounds, show that the charges on the ions add up to zero. a. \({KBr}\) b. \({CaO}\) \({c} . {Li}_{2} {O}\) \({d} . {CaCl}_{2}\) e. AlCl_ \(_{3}\)

What evidence supports the claim that chloride, \(C 1^{-},\) does not cause the flame to have a color? (A) Lithium chloride, LiCl, and sodium chloride, NaCl, have different colors. (B) Ammonium chloride, \(\mathrm{NH}_{4}\),Cl, does not cause the flame to have a color. (C) Sodium chloride, NaCl, and sodium nitrate, \( NaNO_{3}\) both produce flames with a yellow-orange color. (D) All of the above.

How does the rule of zero charge help you predict the formula of an ionic compound?

List four ions that have the same number of electrons as argon, Ar.

If an element is located in Group 4A of the periodic table, what can you conclude about atoms of this element? (A) It has four valence electrons. (B) It has four electron shells. (C) It has four core electrons. (D) It has properties similar to carbon. (E) Both A and D.
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