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Chapter 2: Problem 35

Although not a transition element, lead can form two cations: \(\mathrm{Pb}^{2+}\) and \(\mathrm{Pb}^{4+}\). Write the formulas for the compounds of these ions with the chloride ion.

Short Answer

Expert verified
The compounds are \(\mathrm{PbCl}_2\) and \(\mathrm{PbCl}_4\).

Step by step solution

01

Understanding the Problem

We need to find the chemical formulas for compounds formed by lead ions (\(\mathrm{Pb}^{2+}\) and \(\mathrm{Pb}^{4+}\)) when they combine with chloride ions (\(\mathrm{Cl}^{-}\)). Each chloride ion carries a \(-1\) charge.
02

Finding the Formula for \(\mathrm{Pb}^{2+}\) with Chloride

First, consider the \(\mathrm{Pb}^{2+}\) ion, which has a \(+2\) charge. Since each chloride ion has a \(-1\) charge, two chloride ions are needed to balance the charge of one \(\mathrm{Pb}^{2+}\) ion. Thus, the formula for the compound is \(\mathrm{PbCl}_2\).
03

Finding the Formula for \(\mathrm{Pb}^{4+}\) with Chloride

Next, consider the \(\mathrm{Pb}^{4+}\) ion, which has a \(+4\) charge. To balance this, four chloride ions, each with a \(-1\) charge, are needed. Therefore, the chemical formula for this compound is \(\mathrm{PbCl}_4\).

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Key Concepts

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

Understanding Lead Ions
Lead ions are an interesting part of chemistry because they can exist in different forms, notably \(\mathrm{Pb}^{2+}\) and \(\mathrm{Pb}^{4+}\). These ions are derived from lead, which despite not being a transition metal, displays variable oxidation states just like them. This unique feature of lead allows it to form different ions.
  • Lead can lose either two or four electrons resulting in different cations.
  • \(\mathrm{Pb}^{2+}\) and \(\mathrm{Pb}^{4+}\) are both stable forms found in various compounds.
  • The ability of lead to form different ions is key to its capacity to create multiple chemical compounds.
Lead, known by its symbol 'Pb', was historically used in pipes and paints, but due to its toxicity, its use has been minimized.This chemical diversity of lead allows it to combine with other ions such as the chloride ion, forming stable compounds with distinct properties.
Understanding Chloride Ions
The chloride ion, \(\mathrm{Cl}^{-}\), is quite simple compared to lead ions. It is formed when a chlorine atom gains an extra electron. This gives the chloride ion a negative charge of \-1\, making it anionic.
  • Chloride ions are essential in forming many ionic compounds.
  • They often pair with positive ions (cations) to balance charges in a compound.
  • Chloride ions have applications in everyday life, from table salt (NaCl) to disinfectants like bleach.
Because of their simplicity, chloride ions frequently combine with various metal ions including lead. This pairing is important for a wide range of chemical substances present in both nature and manufactured products.
Formation of Ionic Compounds
Ionic compounds are composed of positive and negative ions. The concept is simple: opposites attract. When ions like lead \(\mathrm{Pb}^{2+}\) or \(\mathrm{Pb}^{4+}\) meet chloride ions \(\mathrm{Cl}^{-}\), they form compounds.The main characteristics are:
  • Ionic compounds have high melting and boiling points.
  • They are generally solid due to the strong attraction between opposite charges.
  • These compounds conduct electricity when dissolved in water.
For example, when \(\mathrm{Pb}^{2+}\) combines with chloride ions, two chloride ions are needed to balance it, forming \(\mathrm{PbCl}_2\). Similarly, \(\mathrm{Pb}^{4+}\) needs four chloride ions, resulting in \(\mathrm{PbCl}_4\).Understanding how ions combine to form stable ionic compounds helps in grasping larger chemistry concepts and exploring the diversity of chemical reactions and materials around us.

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Most popular questions from this chapter

The fluoridation of city water supplies has been practiced in the United States for several decades because there is scientific evidence that fluoride prevents tooth decay, especially in young children. Fluoridation is done by continuously adding sodium fluoride to water as it comes from a reservoir. Assume you live in a medium-sized city of 150,000 people and that each person uses 175 gal water per day. Calculate how many tons of sodium fluoride you must add to the water supply each year (365 days) to have the required fluoride concentration of 1 part per million (that is, 1 ton of fluoride per million tons of water). (Sodium fluoride is \(45.0 \%\) fluoride, and U. S. gallon of water has a mass of 8.34 lb.)

Write the chemical formula for calcium nitrate, barium chloride, and ammonium phosphate. What are the names and charges of all the ions in these three compounds?

Solid magnesium oxide melts at \(2800^{\circ} \mathrm{C}\). This property, combined with the fact that magnesium oxide is not an electrical conductor, makes it an ideal heat insulator for electric wires in cooking ovens and toasters. In contrast, solid \(\mathrm{NaCl}\) melts at the relatively low temperature of \(801{ }^{\circ} \mathrm{C}\). What is the formula of magnesium oxide? Suggest a reason that it has a melting temperature so much higher than that of \(\mathrm{NaCl}\).

The alum used in cooking is potassium aluminum sulfate hydrate, \(\mathrm{KAl}\left(\mathrm{SO}_{4}\right)_{2} \cdot x \mathrm{H}_{2} \mathrm{O} .\) To find the value of \(x,\) you can heat a sample of the compound to drive off all the water and leave only \(\mathrm{KAl}\left(\mathrm{SO}_{4}\right)_{2}\). Assume that you heat \(4.74 \mathrm{~g}\) of the hydrated compound and that it loses \(2.16 \mathrm{~g}\) water. Calculate the value of \(x\).

Which of these are the correct formulas of compounds? For those that are not, give the correct formula. (a) \(\mathrm{Ca}_{2} \mathrm{O}\) (b) \(\mathrm{SrCl}_{2}\) (c) \(\mathrm{Fe}_{2} \mathrm{O}_{5}\) (d) \(\mathrm{K}_{2} \mathrm{O}\)
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