Y. A. EL‐TANTAWY

Kuwait University

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A. I. Abu-Shady

Public Authority for Applied Education and Training

F. Al-Kharafi

Kuwait University

Inas I. Ezzat

Alexandria University

G. A. Rechnitz

University of Hawaiʻi at Mānoa

D.D. Macdonald

University of California, Berkeley

Romeu C. Rocha‐Filho

Universidade Federal de São Carlos

M. Urquidi‐Macdonald

Pennsylvania State University

Ayman E. Elkholy

Swinburne University of Technology

A. M. Shams El-Din

National Research Centre

Fayza M. Al-Kharafi

Kuwait University

Cooperative Institutions

Alexandria University

Kuwait University

SRI International

Menlo School

Cairo University

Centre National de la Recherche Scientifique

National Research Centre

King Fahd University of Petroleum and Minerals

Pennsylvania State University

Qatar University

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The passivation of dilute Cu(Hg) in alkaline solutions

Corrosion Science (1978)

Y. A. EL‐TANTAWY Ayman E. Elkholy Taher S. Kasem

Passivation

Mole fraction

10.1016/0010-938x(78)90042-2

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Citations (7)

The anodic oxidation of dilute Cu(Hg) in carbonate solutions

Corrosion Science (1971)

Y. A. EL‐TANTAWY F. M. ABD EL‐HALIM F. R. EL‐EZIRI

Passivation

10.1016/s0010-938x(71)80037-9

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Citations (4)

ChemInform Abstract: THE KINETICS AND MECHANISM OF THE CE(IV)‐U(IV) REACTION IN ACIDIC SULPHATE MEDIA

Chemischer Informationsdienst (1973)

Y. A. EL‐TANTAWY A. I. Abu-Shady

Abstract Kinetik und Mechanismus der Reaktion A werden im sauren Sulfatmedium untersucht, dessen Verhältnis der HSO; ‐ Konzentration zu der des Redoxsystems die maximale Koordinationszahl jeder der reagierenden Spezies überschreitet.

10.1002/chin.197337050

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ChemInform Abstract: ROLE OF CHLORIDE IN BREAKDOWN OF NICKEL PASSIVITY IN AQUEOUS SODIUM HYDROXIDE SOLUTIONS

Chemischer Informationsdienst (1982)

Y. A. EL‐TANTAWY F. Al-Kharafi

Abstract Potentio‐ und galvanokinetische Untersuchungen an Ni‐Stäben ( u.a. im Hinblick auf Ni‐Cd‐Batterien) zeigten anodische Maxima, die der wahrscheinlichen Bildung von α‐ und β‐Ni(OH 2 ) und NiO(OH) vor der O 2 ‐Entwicklung entsprechen.

Passivity

Sodium hydroxide

Non-blocking I/O

10.1002/chin.198238022

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Passivation of molybdenum in aqueous hydroxide solutions

British Corrosion Journal (1989)

Y. A. EL‐TANTAWY

AbstractAbstractThe electrochemical oxidation of molybdenum rod electrodes has been investigated in a range of dilute sodium hydroxide solutions. The experimental technique involved potentiokinetic, potentiostatic, and open circuit potential decay measurements of oxidised and cleaned electrode surfaces. In the concentration range O·Ol–lM NaOH, the cyclic voltammogram exhibited three anodic peaks on the anodic half cycle. On reversing the scan direction, two anodic peaks in addition to a reduction peak were again obtained. Splitting of the initial peak is observed. The oxidation states of molybdenum corresponding to the anodic peaks were identified in the light of previous studies employing XPS analysis. It is proposed that the initial oxidation results in reversible formation of highly hydrated, surface bound Mo(III) oxy or hydroxy species. Theformation of Mo(IV) and Mo(VI) is thought to result principally from oxidation of metal, rather than from that of the initially formed Mo(III). It is proposed that the electrochemical formation of M 0 (IV) occurs by a diffusion controlled mechanism. None of the products of oxidation produced effective protection of the metal surface against corrosion.

Passivation

Sodium hydroxide

10.1179/000705989798269966

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Citations (6)

The mechanism of Os(VIII)-catalyzed Ce(IV)As(III) reaction

Journal of Inorganic and Nuclear Chemistry (1978)

Y. A. EL‐TANTAWY A. I. Abu-Shady Inas I. Ezzat

10.1016/0022-1902(78)80353-4

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Citations (6)

ChemInform Abstract: THE PASSIVATION OF DILUTE COPPER AMALGAM IN ALKALINE SOLUTIONS

Chemischer Informationsdienst (1979)

Y. A. EL‐TANTAWY Ayman E. Elkholy Taher S. Kasem

Abstract Die anodische Oxidation verdünnter Cu(Hg)‐Poolelektroden (maximaler Molenbruch des Cu: 0.031) in wäßrige Lösungen von Na 3 PO 4 und NaOH (pH‐Bereich l0.5‐12.2) bewirkt eine Reihe von Potential‐Zeit‐Transienten entsprechend der Bildung von Cu 2 O, CuO und Cu(OH) 2 beim höheren pH‐Wert und von Cu 2 O sowie 2 löslichen Spezies (wahrscheinlich CuO 2‐ und HCuO2 ‐ ) beim niedrigeren pH‐Wert.

Amalgam (chemistry)

10.1002/chin.197917025

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Determination of the Polarization Resistance of Rebar in Reinforced Concrete

CORROSION (1991)

D.D. Macdonald M. Urquidi‐Macdonald Romeu C. Rocha‐Filho Y. A. EL‐TANTAWY

The problem of determining the polarization resistance of rebar in reinforced concrete is addressed by modeling the electrical properties of the rebar/concrete system as a bifurcated transmission line. The polarization resistance, concrete resistance, and the interfacial capacitance are obtained by fitting the model to experimental impedance data using nonlinear regression analysis. Although the efficiency of this procedure depends on the quality of the initial estimates for the model variables, we show that the final values obtained are independent of the initial values used in the analysis. Finally, we explore the distribution of the current along the rebar as a function of the polarization resistance, concrete resistance per unit length of the rebar, and the frequency of the applied alternating voltage perturbation. We show that the current distribution becomes a particular problem at low frequencies when the concrete resistance is low and/or the polarization resistance is high.

Rebar

10.5006/1.3585261

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Citations (23)

Studies on the Anodic and Cathodic Polarization of Amalgams. Part II. Mercury in Ammonium Hydroxide Solution

The Journal of Physical Chemistry (1959)

A. M. Shams El-Din S. E. Khalafalla Y. A. EL‐TANTAWY

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTStudies on the Anodic and Cathodic Polarization of Amalgams. Part II. Mercury in Ammonium Hydroxide SolutionA. M. Shams El-Din, S. E. Khalafalla, and Y. A. El-TantawyCite this: J. Phys. Chem. 1959, 63, 8, 1224–1227Publication Date (Print):August 1, 1959Publication History Published online1 May 2002Published inissue 1 August 1959https://pubs.acs.org/doi/10.1021/j150578a002https://doi.org/10.1021/j150578a002research-articleACS PublicationsRequest reuse permissionsArticle Views31Altmetric-Citations1LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InRedditEmail Other access options Get e-Alerts

Mercury

Citation database

10.1021/j150578a002

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Citations (1)

Competitive Role of Chloride and Phosphate Ions in the Electrochemical Passivation of Co in NaOH Solutions

British Corrosion Journal (1984)

Y. A. EL‐TANTAWY F. Al-Kharafi Z. Al-Fahd

AbstractAbstractThe electrochemical oxidation of Co in NaOH solutions containing chloride, phosphate or mixtures of both ions has been studied. The experimental technique involved cyclic potentiodynamic, potentiostatic and open circuit potential decay measurements. The anodic peaks are interpreted in the light of previous reports in which surface analysis methods were employed for the identification of oxidation states. Co(II)-oxide is believed to form via an instantaneous nucleation mechanism. The formation of Co(III)-oxides follows a diffusion controlled mechanism, and phosphate additions inhibited the Co(II) peak. Additions of Cl− had no effect on the Co(II) process, and it is proposed that the role of Cl− in the breakdown of Co passivity resides in a post-oxide-crystallisation mechanism. In NaOH solution colltaining a mixture of Cl− and phosphate, the role of the latter in promoting passivity protection overcomes completely the Cl− breakdown effect. A mechanism explaining the competitive roles of cl− and phosphate in the breakdown and promotionof Co passivation is discussed.

Passivation

10.1179/000705984798273434

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Citations (4)