Chapter 1: Problem 118
The oxidation number of sulphur in \(\mathrm{S}_{8}, \mathrm{~S}_{2} \mathrm{~F}_{2}, \mathrm{H}_{2} \mathrm{~S}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) respectively are: (a) \(0,+1,-2\) and 6 (b) \(+2,0,+2\) and 6 (c) \(0,+1,+2\) and 4 (d) \(-2,0,+2\) and 6
Short Answer
Expert verified
The oxidation numbers of sulphur in \(\mathrm{S}_{8}, \mathrm{S}_{2}\mathrm{F}_{2}, \mathrm{H}_{2}\mathrm{S}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\) respectively are 0, +1, -2, and +6.
Step by step solution
01
Understanding Oxidation Numbers
Oxidation numbers are used to keep track of how many electrons are lost or gained by each atom in a compound. In its elemental form, the oxidation number of an atom is always zero. In compounds, the more electronegative element is assigned a negative oxidation number equal to its charge if it were an ion. The less electronegative element is given a positive oxidation number. Hydrogen is usually +1 (except in metal hydrides where it is -1), and oxygen is usually -2.
02
Determining the Oxidation Number of Sulfur in S8
In the molecule \(\mathrm{S}_8\), sulfur is in its elemental form. Therefore, the oxidation number of sulfur in \(\mathrm{S}_8\) is 0.
03
Determining the Oxidation Number of Sulfur in S2F2
In \(\mathrm{S}_2\mathrm{F}_2\), fluorine is more electronegative and will have an oxidation number of -1. There are two fluorine atoms, so the total charge contributed by fluorine is -2. To balance, the total oxidation number for two sulfur atoms must be +2, so each sulfur atom has an oxidation number of +1.
04
Determining the Oxidation Number of Sulfur in H2S
In \(\mathrm{H}_2\mathrm{S}\), hydrogen has an oxidation number of +1 and there are two hydrogen atoms giving a total of +2. To balance the charges, sulfur must have an oxidation number of -2.
05
Determining the Oxidation Number of Sulfur in H2SO4
In \(\mathrm{H}_2\mathrm{SO}_4\), hydrogen has an oxidation number of +1. With two hydrogen atoms, the total is +2. Oxygen has an oxidation number of -2 and there are four oxygen atoms, contributing a total of -8. To balance the charge for sulfate ion \(\mathrm{SO}_4^{2-}\), sulfur must have an oxidation number of +6. The sulfate ion charge doesn't affect the oxidation state as the ion is overall neutral when combined with hydrogen atoms.
Unlock Step-by-Step Solutions & Ace Your Exams!
-
Full Textbook Solutions
Get detailed explanations and key concepts
-
Unlimited Al creation
Al flashcards, explanations, exams and more...
-
Ads-free access
To over 500 millions flashcards
-
Money-back guarantee
We refund you if you fail your exam.
Over 30 million students worldwide already upgrade their learning with Vaia!
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Oxidation State Determination
The oxidation state, also known as oxidation number, is a fundamental concept in chemistry that provides insight into the electron distribution within compounds. It plays a crucial role in understanding the electron transfer process in redox reactions. It is a hypothetical charge that an atom would have if all bonds to atoms of different elements were completely ionic.
Oxidation states are determined by following a set of rules: firstly, the oxidation state of any pure element is zero. Secondly, for a molecule, the sum of the oxidation states must equal the overall charge of the molecule or ion. When dealing with molecular compounds, the most electronegative element is assigned a negative oxidation state. In most cases, hydrogen has an oxidation state of +1 (except when bonded to metals in hydrides, where it is -1), and oxygen has a consistent oxidation state of -2, except in peroxides or when bonded to fluorine. By using these rules, one can deduce the oxidation states of elements in complex compounds and ions, illuminating the underpinnings of the compound's reactivity and chemical behavior.
Oxidation states are determined by following a set of rules: firstly, the oxidation state of any pure element is zero. Secondly, for a molecule, the sum of the oxidation states must equal the overall charge of the molecule or ion. When dealing with molecular compounds, the most electronegative element is assigned a negative oxidation state. In most cases, hydrogen has an oxidation state of +1 (except when bonded to metals in hydrides, where it is -1), and oxygen has a consistent oxidation state of -2, except in peroxides or when bonded to fluorine. By using these rules, one can deduce the oxidation states of elements in complex compounds and ions, illuminating the underpinnings of the compound's reactivity and chemical behavior.
Redox Chemistry
Redox chemistry is centered around the concepts of oxidation and reduction, processes that involve the transfer of electrons between chemical species. The term 'redox' is a portmanteau of reduction-oxidation. An oxidation reaction describes the loss of electrons by a molecule, atom, or ion, while in a reduction reaction, a chemical species gains electrons.
In a redox process, there is always a transfer of electrons from the reducing agent to the oxidizing agent. The oxidation states of atoms change as a result of this electron transfer. The reducing agent increases in oxidation state (loses electrons), and the oxidizing agent decreases in oxidation state (gains electrons). These changes in oxidation state are often the key to identifying redox reactions. Understanding the alteration of oxidation numbers is essential for balancing redox reactions, predicting the direction of electron flow, and determining the energy changes that occur during the process.
In a redox process, there is always a transfer of electrons from the reducing agent to the oxidizing agent. The oxidation states of atoms change as a result of this electron transfer. The reducing agent increases in oxidation state (loses electrons), and the oxidizing agent decreases in oxidation state (gains electrons). These changes in oxidation state are often the key to identifying redox reactions. Understanding the alteration of oxidation numbers is essential for balancing redox reactions, predicting the direction of electron flow, and determining the energy changes that occur during the process.
Chemical Bonding
Chemical bonding refers to the forces that hold atoms together to form compounds and molecules. The distribution of electrons in chemical bonds is related to the concept of oxidation numbers. Atoms form bonds by sharing or transferring valence electrons to achieve stability, often described by the octet rule.
There are three primary types of chemical bonds: ionic, covalent, and metallic. Ionic bonds occur through the transfer of electrons from one atom to another, resulting in positive and negative ions that attract each other. Covalent bonds involve the sharing of electron pairs between atoms, which may not always be equal - in such cases, polar covalent bonds are formed. Metallic bonds involve a 'sea' of delocalized electrons surrounding positively charged metal ions. Understanding the nature of chemical bonds is crucial for deciphering how atoms combine and why they react in certain ways, which in turn affects the determination of oxidation states in various compounds.
There are three primary types of chemical bonds: ionic, covalent, and metallic. Ionic bonds occur through the transfer of electrons from one atom to another, resulting in positive and negative ions that attract each other. Covalent bonds involve the sharing of electron pairs between atoms, which may not always be equal - in such cases, polar covalent bonds are formed. Metallic bonds involve a 'sea' of delocalized electrons surrounding positively charged metal ions. Understanding the nature of chemical bonds is crucial for deciphering how atoms combine and why they react in certain ways, which in turn affects the determination of oxidation states in various compounds.
IUPAC Nomenclature
The International Union of Pure and Applied Chemistry (IUPAC) nomenclature is a systematic way of naming chemical compounds and elements. This nomenclature is used to ensure that each chemical substance has a unique and universally accepted name that describes its composition and structure.
For inorganic compounds, the IUPAC names often reflect their empirical formulas and bonding arrangements, giving clues about their molecular geometry and oxidation states. Common naming conventions include using Greek prefixes to indicate the number of atoms of each element in the compound and naming ions and acids in ways that indicate their composition and oxidation states. Learning the rules of IUPAC nomenclature helps students not only communicate effectively about chemistry but also understand the roles of atoms within a compound and derive information such as oxidation numbers, essential for problem-solving in redox reactions and other areas of chemistry.
For inorganic compounds, the IUPAC names often reflect their empirical formulas and bonding arrangements, giving clues about their molecular geometry and oxidation states. Common naming conventions include using Greek prefixes to indicate the number of atoms of each element in the compound and naming ions and acids in ways that indicate their composition and oxidation states. Learning the rules of IUPAC nomenclature helps students not only communicate effectively about chemistry but also understand the roles of atoms within a compound and derive information such as oxidation numbers, essential for problem-solving in redox reactions and other areas of chemistry.
