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Chapter 2: Problem 54

The most common charge associated with silver in its compounds is \(1+\). Indicate the chemical formulas you would expect for compounds formed between \(\mathrm{Ag}\) and (a) iodine, (b) sulfur, (c) fluorine.

Short Answer

Expert verified
The chemical formulas for the compounds formed between silver (Ag) and the given elements are as follows: (a) AgI: formed between silver and iodine (I), (b) Ag2S: formed between silver and sulfur (S), and (c) AgF: formed between silver and fluorine (F).

Step by step solution

01

(a) Silver and Iodine (Ag and I)

The most common ion of silver is Ag+1, while iodine (I) usually forms the I-1 ion. In order for the compound to be neutral, one positive charge from silver will need to be balanced by one negative charge from iodine. Therefore, the compound formed would require one silver atom and one iodine atom. The chemical formula can be written as AgI.
02

(b) Silver and Sulfur (Ag and S)

Silver forms the Ag+1 ion, while sulfur (S) usually forms the S-2 ion. In this case, we will need two silver ions to balance the charges with one sulfur ion, as +1 + +1 = +2, and the sulfur ion has a charge of -2. This leads to a compound with two silver atoms and one sulfur atom. The chemical formula can be written as Ag2S.
03

(c) Silver and Fluorine (Ag and F)

Silver forms the Ag+1 ion, while fluorine (F) usually forms the F-1 ion. Similar to the case with iodine, a single positive charge from silver can be balanced by a single negative charge from fluorine. Thus, the compound formed would require one silver atom and one fluorine atom. The chemical formula can be written as AgF.

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Key Concepts

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

Ion Charges
Ion charges are crucial in determining how elements combine to form compounds. Each element tends to lose or gain electrons to achieve a full outer electron shell, often resulting in a net positive or negative charge. This charge is known as the ion charge. For metals like silver (Ag), it's common to lose electrons, resulting in a positive charge. Silver typically forms a positive ion with a charge of +1, denoted as Ag鈦�.
Nonmetals, on the other hand, tend to gain electrons and thus acquire a negative charge. For instance:
  • Iodine typically forms I鈦�.
  • Fluorine forms F鈦�.
  • Sulfur forms S虏鈦�.
Understanding these charges helps in predicting the composition of various compounds by balancing the total positive and negative charges to maintain neutrality.
Compound Neutrality
In chemistry, compound neutrality is the principle stating that the overall charge of a compound must be zero. No matter the nature of the elements involved, their charges must sum up to zero in the final compound.
This is achieved by adjusting the ratio of ions in the compound:
  • For Ag鈦� and I鈦�: Both ions have charges that balance each other (+1 and -1, respectively), making the formula AgI neutral.
  • For Ag鈦� and S虏鈦�: Since silver is +1 and sulfur is -2, two silver ions are needed to match sulfur's charge, forming Ag鈧係.
  • For Ag鈦� and F鈦�: Both carry a charge of +1 and -1, resulting in the neutral compound AgF.
The balancing of charges is foundational in chemical formula writing and ensures that compounds have no net charge.
Silver Compounds
Silver is a notable metal used in various compounds, typically carrying a +1 charge. Its ability to form stable compounds makes it versatile and commonly seen in study and industry.
Some common silver compounds include:
  • Silver iodide (AgI), known for applications in photography and weather modification.
  • Silver sulfide (Ag鈧係), which forms naturally and is seen in tarnish on silverware.
  • Silver fluoride (AgF), less common but useful in some high-tech applications.
In each case, the silver ion pairs with another element to achieve a neutral compound, dictated by the ion charges of the partnering element.

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Most popular questions from this chapter

Use Coulomb's law, \(F=k Q_{1} Q_{2} / d^{2}\), to calculate the electric force on an electron \(\left(Q=-1.6 \times 10^{-19} \mathrm{C}\right)\) exerted by a single proton if the particles are \(0.53 \times 10^{-10} \mathrm{~m}\) apart. The constant \(k\) in Coulomb's law is \(9.0 \times 10^{9} \mathrm{~N} \cdot \mathrm{m}^{2} / \mathrm{C}^{2}\). (The unit abbreviated \(\mathrm{N}\) is the Newton, the SI unit of force.)

From the following list of elements \(-\mathrm{Ar}, \mathrm{H}, \mathrm{Ga}, \mathrm{Al}, \mathrm{Ca}\), \(\mathrm{Br}, \mathrm{Ge}, \mathrm{K}, \mathrm{O}-\) pick the one that best fits each description. Use each element only once: (a) an alkali metal, (b) an alkaline earth metal, (c) a noble gas, (d) a halogen, (e) a metalloid, (f) a nonmetal listed in group \(1 \mathrm{~A},(\mathrm{~g})\) a metal that forms a \(3+\) ion, \((h)\) a nonmetal that forms a \(2-\) ion, (i) an element that resembles aluminum.

Name each of the following oxides. Assuming that the compounds are ionic, what charge is associated with the metallic element in each case? (a) \(\mathrm{NiO}\), (b) \(\mathrm{MnO}_{2}\), (c) \(\mathrm{Cr}_{2} \mathrm{O}_{3}\), (d) \(\mathrm{MoO}_{3}\).

Locate each of the following elements in the periodic table; indicate whether it is a metal, metalloid, or nonmetal; and give the name of the element: (a) \(\mathrm{Ca}\), (b) \(\mathrm{Ti}\), (c) \(\mathrm{Ga},(\mathrm{d}) \mathrm{Th},(\mathrm{e}) \mathrm{Pt},(\mathrm{f}) \mathrm{Se},(\mathrm{g}) \mathrm{Kr}\).

Predict the chemical formulas of the compounds formed by the following pairs of ions: (a) \(\mathrm{Cu}^{2+}\) and \(\mathrm{Br}^{-}\), (b) \(\mathrm{Fe}^{3+}\) and \(\mathrm{O}^{2-}\), (c) \(\mathrm{Hg}_{2}^{2+}\) and \(\mathrm{CO}_{3}^{2-}\), (d) \(\mathrm{Ca}^{2+}\) and \(\mathrm{AsO}_{4}{ }^{3-}\), (e) \(\mathrm{NH}_{4}{ }^{+}\) and \(\mathrm{CO}_{3}{ }^{2-}\).
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