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Chapter 18: Problem 4

State the oxidation number for each of the following monoatomic ions: (a) \(\mathrm{Ag}^{+}\) (b) \(\mathrm{Mg}^{2+}\) (c) \(\mathrm{S}^{2-}\) (d) \(\mathrm{F}^{-}\)

Short Answer

Expert verified
(a) +1, (b) +2, (c) -2, (d) -1

Step by step solution

01

Understanding Oxidation Numbers

Oxidation numbers for monoatomic ions correspond directly to the charge of the ion. The oxidation number indicates how many electrons are lost or gained by an atom in the ion.
02

Determine Oxidation Number for Ag鈦�

For the ion \( \mathrm{Ag}^{+} \), the oxidation number is the same as the charge. Here, silver (Ag) has a charge of +1, so its oxidation number is +1.
03

Determine Oxidation Number for Mg虏鈦�

For \( \mathrm{Mg}^{2+} \), magnesium has a charge of +2, so its oxidation number is +2, which reflects the loss of two electrons.
04

Determine Oxidation Number for S虏鈦�

For \( \mathrm{S}^{2-} \), sulfur has a charge of -2, meaning it has gained two electrons. Therefore, the oxidation number is -2.
05

Determine Oxidation Number for F鈦�

For \( \mathrm{F}^{-} \), fluorine has a charge of -1, with one electron gained, giving it an oxidation number of -1.

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Key Concepts

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

Monoatomic Ions
Monoatomic ions are single atoms that carry an electrical charge. These ions are crucial in understanding chemical reactions and processes. They form when an atom either loses or gains electrons, resulting in a net electrical charge.
  • If an atom loses electrons, it becomes positively charged and is known as a cation.
  • If an atom gains electrons, it becomes negatively charged and is called an anion.
For example, in the cases listed:
  • Ag鈦� is a cation, having lost one electron, making it positively charged.
  • On the other hand, ions like S虏鈦� and F鈦� are anions, having gained electrons to be negatively charged.
Understanding monoatomic ions is essential to grasping how different substances interact and form compounds in chemistry.
Electron Transfer
Electron transfer is a fundamental concept in chemistry, involving the movement of electrons from one atom to another. This process is responsible for the formation of ions and the creation of new chemical bonds.
When atoms interact, electrons may be transferred to achieve a more stable configuration, often mimicking the structure of noble gases with full outer shells.
  • Cations, like Mg虏鈦�, form when an atom loses electrons. Magnesium (Mg) loses two electrons, thus becoming positively charged.
  • Anions, such as F鈦�, form when an atom gains electrons. For instance, fluorine gains one electron to become negatively charged.
Electron transfer not only results in ion formation but is also central to oxidation-reduction reactions, where oxidation involves losing electrons and reduction involves gaining them. This dynamic movement of electrons drives many chemical processes.
Chemical Charge
Chemical charge refers to the net electric charge of an ion, determined by the gain or loss of electrons compared to the neutral atom. This charge is a direct reflection of the oxidation number in monoatomic ions.
For each of the ions given:
  • The oxidation number for Ag鈦� is +1, showing it has lost one electron.
  • Mg虏鈦� has an oxidation number of +2, reflecting the loss of two electrons.
  • Conversely, S虏鈦� and F鈦� have oxidation numbers of -2 and -1, respectively, indicating they have gained electrons.
The chemical charge is essential in predicting how ions form compounds and react with each other. Understanding these charges helps chemists determine the stoichiometry of reactions and the structure of compounds formed.

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Most popular questions from this chapter

Supply the term that corresponds to each of the following: (a) a redox process characterized by electron loss (b) a substance causing oxidation in a redox reaction

The nonspontaneous redox reaction of chlorine gas and aqueous sodium fluoride is an electrolytic process according to the following equation: $$ \mathrm{Cl}_{2}(g)+2 \mathrm{NaF}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{F}_{2}(g) $$ The half-reactions are separated into two compartments. A \(\mathrm{Pt}\) electrode is placed in \(1.00 \mathrm{M} \mathrm{NaCl},\) and a second \(\mathrm{Pt}\) electrode in \(1.00 \mathrm{M}\) NaF. Indicate each of the following for the electrolytic cell: (a) oxidation half-cell reaction (b) reduction half-cell reaction (c) anode and cathode (d) direction of electron flow (e) direction of \(\mathrm{Na}^{+}\) in the salt bridge

The nonspontaneous redox reaction of nickel and aqueous iron(II) sulfate is an electrolytic process according to the following equation: $$ \mathrm{Ni}(s)+\mathrm{FeSO}_{4}(a q) \longrightarrow \mathrm{Fe}(s)+\mathrm{NiSO}_{4}(a q) $$ The half-reactions are separated into two compartments. A Ni electrode is placed in \(1.00 \mathrm{M} \mathrm{NiSO}_{4},\) and an Fe electrode in \(1.00 \mathrm{M} \mathrm{FeSO}_{4}\). Indicate each of the following for the electrolytic cell: (a) oxidation half-cell reaction (b) reduction half-cell reaction (c) anode and cathode (d) direction of electron flow (e) direction of \(\mathrm{SO}_{4}^{2-}\) in the salt bridge

Calculate the oxidation number for nitrogen in the following compounds: (a) \(\mathrm{NH}_{3}\) (b) \(\mathrm{N}_{2} \mathrm{O}_{4}\) (c) \(\mathrm{Li}_{3} \mathrm{~N}\) (d) \(\mathrm{KNO}_{3}\)

Supply the term that corresponds to each of the following: (a) a redox process characterized by electron gain (b) a substance causing reduction in a redox reaction
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