The oxidation states of the elements and their potentials in aqueous solutions. by Wendell M. Latimer

Cover of: The oxidation states of the elements and their potentials in aqueous solutions. | Wendell M. Latimer

Published by Prentice-Hall in New York .

Written in English

Read online

Subjects:

  • Electrolysis,
  • Oxidation,
  • Chemical elements

Edition Notes

Book details

SeriesPrentice-Hall chemistry series
Classifications
LC ClassificationsQD561 .L35 1952
The Physical Object
Pagination392 p.
Number of Pages392
ID Numbers
Open LibraryOL6113391M
LC Control Number52010791

Download The oxidation states of the elements and their potentials in aqueous solutions.

The Oxidation States of the Elements and Their Potentials in Aqueous Solutions (Latimer, Wendell M.). The Oxidation States of the Elements and Their Potentials in Aqueous Solutions (Latimer, Wendell M.) Robert Livingston Cite this: J.

Chem. Educ.17, 7, The oxidation states of the elements and their potentials in aqueous solutions The oxidation states of the elements and their potentials in aqueous solutions by Latimer, Wendell M.

(Wendell Mitchell), Publication date Internet Archive : Oxidation states of the elements and their potentials in aqueous solutions. New York, Prentice-Hall, Inc., (OCoLC) Online version: Latimer, Wendell M.

(Wendell Mitchell), Oxidation states of the elements and their potentials in aqueous solutions. New York, Prentice-Hall, Inc., (OCoLC) Document Type: Book.

The oxidation states of the elements and their potentials in aqueous solutions, ([Prentice-Hall chemistry series; W.M. Latimer, editor]) [Latimer, Wendell M] on *FREE* shipping on qualifying offers. The oxidation states of the elements and their potentials in aqueous solutions, ([Prentice-Hall chemistry series; W.M.

LatimerAuthor: Wendell M Latimer. The oxidation states of the elements and their potentials in aqueous solutions, ([Prentice-Hall chemistry series; W.M. Latimer, editor]) by Latimer, Wendell M and a great selection of related books, art and collectibles available now at Add tags for "The oxidation states of the elements and their potentials in aqueous solutions.".

Be the first. Start Page: 1 l., p.: diagrs, 24 cm. Publisher: Prentice-Hall, inc. All titles: " oxidation states of the elements and their potentials in aqueous solutions "Cited by:   The oxidation states of the elements and their potentials in aqueous solutions by Wendell M.

Latimer,Prentice-Hall edition, in English - 2d : The Oxidation States of the Elements & Their Potentials in Aqueous Solution S, [Latimer, Wendell, ] on *FREE* shipping on qualifying offers.

The Oxidation States of the Elements & Their Potentials in Aqueous Solution SAuthor: Latimer, Wendell. The oxidation states of the elements and their potentials in aqueous solutions by Wendell M.

Latimer; 5 editions; First published in ; Subjects: Oxidation, Chemical elements, Electrolysis, Électrolyse, Oxidatie, Reductie (scheikunde), Éléments chimiques, Tabelas Periodicas, Oxydation, Redoxpotential, Oxidationszahl, Oxidation-Reduction.

Wendell Mitchell Latimer (Ap – July 6, ) was a prominent [peacock term] chemist notable for his description of oxidation states in his book "The Oxidation States of the Elements and Their Potentials in Aqueous Solution" (ASIN BGRXLSA, first published ). He received his Ph.D from the University of California, Berkeley for the work with George Ernest.

Start studying Chemistry: Chapter 4: Reactions in Aqueous Solution. Learn vocabulary, terms, and more with flashcards, games, and other study tools. Although Antoine Lavoisier first began the idea of oxidation as a concept, it was Wendell Latimer ( - ) who gave us the modern concept of oxidation numbers.

His book The Oxidation States of the Elements and Their Potentials in Aqueous Solution laid out the concept in detail. Latimer was a well-known chemist who later became a.

Uses of Lanthanides in Devices. Lanthanides (elements 57–71) are fairly abundant in the earth’s crust, despite their historic characterization as rare earth m, the rarest naturally occurring lanthanoid, is more common in the earth’s crust than silver ( × 10 −5 % versus × 10 −5 % by mass).

There are 17 rare earth elements, consisting of the 15 lanthanoids plus Author: OpenStax. Stability in the aqueous medium depends on the hydration energy of ions when they attract to water to water molecules.

In aqueous solution, Cu+ ion undergoes oxidises and reduces simultaneously in aqueous to give Cu and Cu2+ ion. The relative stability of different oxidation states can be seen from their Electrode potentials Due to more reduction electrode potential. NucL Chem. 12, (). Oxidation-reduction potential of UO.,~-Ua+ system in perchloric acid where: J~i1+ is activity coefficient of H+ ions in solution containing uranium ions, f~2+ is activity coefficient of H+ ions in solution of reference electrode, ED is liquid junction potential between both by: 7.

Potential diagrams are given for the various oxidation states of the elements, and these provide a useful shorthand way of summarising information on the relative stabilities in solution of their various oxidation states.

In short, this review provides at least a foundation for the more quantitative aspects of platinum metal chemistry. Oxidation state explained. The oxidation state, sometimes referred to as oxidation number, describes the degree of oxidation (loss of electrons) of an atom in a chemical tually, the oxidation state, which may be positive, negative or zero, is the hypothetical charge that an atom would have if all bonds to atoms of different elements were.

Although Antoine Lavoisier first began the idea off oxidation as a concept, it was Wendell Latimer () who gave us the modern concept of oxidation numbers. His book The Oxidation States of the Elements and Their Potentials in Aqueous Solution laid out the concept in detail. Latimer was a well-known chemist who later became a member.

Latimer used low-temperature data in conjunction with the third law of thermodynamics to determine the entropies and free energies of aqueous ions.

This work supplied much of the material included in his outstanding book, The Oxidation States of the Elements and Their Potentials in Aqueous Solutions (, ). Oxidation states of vanadium in acidic solution. From left to right the oxidation state goes from +5 to +2. These four oxidation states form the basis of the vanadium flow battery, a storage device for electricity generated from sunlight and wind.

In redox reactions, one element or compound is reduced (gains electrons) and another is oxidized. Each element exhibits several different oxidation states, and the discussion of their compounds is organized by the oxidation states of the elements.

The chapter describes several important industrial chemicals, namely, ammonia, nitric acid, phosphoric acid, and sulfuric acid. The d-block elements are divided into the first transition series (the elements Sc through Cu), the second transition series (the elements Y through Ag), and the third transition series (the element La and the elements Hf through Au).

Actinium, Ac, is the first member of the fourth transition series, which also includes Rf through Rg. The f-block elements are the elements Ce through. Consider, for example, the reaction of Cr 2+ (aq) with manganese dioxide (MnO 2) to make Cr 3+ (aq) and Mn 2+ (aq)in the presence of dilute acid.

Equation is a representation of the reaction before applying our balancing routine. Notice that chromium is oxidized from the +2 to the +3 oxidation state, while manganese is reduced from the +4 to the +2 oxidation state. How can we determine the standard potential of oxidation from a cyclic voltammogram.

states of the elements and their potentials in aqueous solutions"). references which may be. Inorganic Chemistry in Aqueous Solution reviews the chemistry of the elements in all their oxidation states in an aqueous environment. The nature of ions in solution is described in some detail and enthalpies and entropies of hydration of many ions are defined and recalculated from the best data available.

Compounds of elements in high oxidation states (such as ClO 4 −, NO 3 −, MnO 4 −, Cr 2 O 7 2−, and UF 6) tend to act as oxidants and become reduced in chemical reactions. Compounds of elements in low oxidation states (such as CH 4, NH 3, H 2 S, and HI) tend to act as reductants and become oxidized in chemical reactions.

At least two elements must change their oxidation numbers. When an oxidation number of an atom is increased in the course of a redox reaction, that atom is being oxidized. When an oxidation number of an atom is decreased in the course of a redox reaction, that atom is being reduced.

Thus oxidation and reduction can also be defined in terms of. Lanthanides (elements 57–71) are fairly abundant in the earth’s crust, despite their historic characterization as rare earth m, the rarest naturally occurring lanthanoid, is more common in the earth’s crust than silver ( \(×\) 10 −5 % versus \(×\) 10 −5 % by mass).

There are 17 rare earth elements, consisting of the 15 lanthanoids plus scandium and Author: OpenStaxCollege. All of the elements form chemical species that have different oxidation states. Oxidation is the removal of electrons whereas reduction is the addition of electrons to a chemical : George W Luther.

The half-reaction method splits oxidation-reduction reactions into their oxidation “half” and reduction “half” to make finding the overall equation easier. Electrochemical reactions frequently occur in solutions, which could be acidic, basic, or neutral. When balancing oxidation-reduction reactions, the nature of the solution may be Author: OpenStax.

Start studying AQA A Level Chemistry Unit 5. Learn vocabulary, terms, and more with flashcards, games, and other study tools. The enthalpy change when 1 mole of a compound in its standard state is made from its constituent elements in their standard states under standard conditions.

in reactions between 2 aqueous solutions. aqueous solution, a very common reaction for aqueous solutions is the redox reaction. And we can characterize a redox reaction as a reaction in which the oxidation state changes—in other words, reactions where electrons are transferred from one species to another.

Or (i) In aqueous solution, Cu+ ion undergoes oxidation to Cu2+ ion. The relative stability of different oxidation states can be seen from their electrode potentials. Cu+(aq) + e- --> Cu(s), E0red = V Cu2+(aq) + 2e­- > Cu(s), E0red = V Thus overall reaction is: 2Cu+ (aq) > Cu2+ (aq) + Cu(s) Due to more reduction electrode potential value of Cu+, it undergoes.

Further, when the standard electrode potentials of the elements are arranged in order of the most negative [Li+e = Li V, at the top] to the to the most positive [F2 + 2e- = 2F +V, at the bottom] constitutes the electrochemical series of the elements which may be used to interpret and also predict the reactivity of the elements.

Latimer, W.M. () The Oxidation States of the Elements and their Potentials in Aqueous Solutions. Prentice-Hall, Englewood Cliffs, N.J. pp Google Scholar Leary, K. and Bartlett, N.

A new oxidation state of gold: The preparation and some properties of [AuF6] by: Abstract This chapter is intended to provide a unified view of selected aspects of the physical, chemical, and biological properties of the actinide elements, their typical compounds, and their ions in aqueous solutions.

Abstract. Because of their multiple oxidation states, the chalcogens, particularly sulfur, can engage in numerous redox couples participating in acid–base, oxidation–reduction, precipitation, and complexation by: tion.

Electrochemical studies of redox potentials have been more recent. Most of the redox potentials in non-aqueous solutions discussed by us long ago [7] and now reproduced in this paper were gleaned from chemical equilibrium studies (at fixed oxygen pressure established by bubbling gases), e.g., [9–12], rather than the inverse process where.

Materials discovery by chemical analogy: role of oxidation states in structure prediction Oxidation states of all elements can be determined automatically using a bond valence analysis algorithm W.

M. Latimer The Oxidation States of the Elements and their Potentials in Aqueous Solutions, Prentice Hall, some higher oxidation states observed in the secoðd and third series, as in Ru04 and Os It is more important for you to know the behavior of the first transition series than to remember the exceptions in the heavier metals.

Oxidation Potentials The oxidation potentials for the production of ions from neutral atoms areFile Size: 6MB.Lanthanide oxidation states All of the lanthanide elements are commonly known to have the +3 oxidation state and it was thought that only samarium, europium, and ytterbium had the +2 oxidation readily accessible in solution.

Now, it is known that all of the lanthanides can form +2 complexes in solution.

35613 views Sunday, November 29, 2020