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Corrosion is the degradation of material properties caused by interactions between a material and its environment. It occurs via various chemical and electrochemical processes involving electron and ion transport. Factors like oxygen, water, temperature, pressure, other metals, bacteria and cells influence the corrosion rate. Passivation and anodic protection are two common methods used to prevent corrosion. Passivation creates a protective oxide layer barrier while anodic protection coats a more active metal with a less active one. Corrosion can be classified as chemical or electrochemical depending on the mechanism.
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Corrosion is an electrochemical process where a metal oxidizes and dissolves into its environment. There are several types of corrosion including uniform corrosion, galvanic corrosion, pitting corrosion, and crevice corrosion. Uniform corrosion proceeds uniformly over the entire metal surface. Galvanic corrosion occurs when two dissimilar metals are electrically coupled in a corrosive electrolyte. Pitting and crevice corrosion are localized forms of attack that can cause perforation. Cathodic protection is a technique to control the corrosion of a metal by making it the cathode of an electrochemical cell.
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Presentation (1)-1.pptx
- 1. Corrosion • Introduction 1. Corrosion is a general term used to describe various interactions between a material and it’s environment leading to a degradation in the material properties. 2. Interaction with ambient oxygen can cause the formation of oxide layers via diffusion controlled growth. These may passivate the material against further oxidation 3. In a wet environment, aqueous corrosion can occur due to electrochemical processes which depend upon metal ion transport and reaction. Gradients of metallic and electrolytic ion concentrations, temperature, ambient pressure, and the presence of other metals bacteria, or active cells, all influence the corrosion rate. 4. Electric fields applied to corroding systems can accelerate or inhibit the rate of corrosion or material deposition. Galvanic corrosion between different metals in am aqueous environment is due to the electric field arising from the different electrode potential of the two materials. External fields may enhance or supress this corrosion. 5. In all of these reactions, electrons and ionic transport occurs. The following sections will be concerned with these processes and the effort of conditions on the corrosion rates.
- 2. Corrosion CERTIFICATE This is to certify that “ SYEDA NURIN HAQUE “ Student of class 10 has successfully completed her Chemistry Project on “CORROSION “ Under the guidance of teacher “MAINUL HAQUE” Guardian‘s signature: Syed Amanul Haque
- 3. Corrosion • Methods of prevention for corrosion • 1. Passivation : • In passivation a light coat of a protective material, such as metal oxide, creates a protective layer over the metal which acts as a barrier against corrosion. • The formation of a passivation layer is affected by environmental pH , temperature, and chemical conditions.
- 4. Corrosion • 2. Anodic Protection: • Anodic protection involves in coating the iron alloy steel with less a active metal, such as tin. • Anodic protection is often applied to carbon steel storage tanks used to store sulfuric acid and 50% caustic soda.
- 5. Corrosion • Definition: • Chemical or electrochemical Process in which a solid, usually a metal, is attacked by an environmental agent, resulting in portial or complete dissolution
- 6. Corrosion • Fundam Basis of Corrosion : • Corrosion occurs because most commonly used metal and alloys not in Locioest energy state. • Aluminium is extracted from Aluminium oxide and copper from copper sulphate
- 7. Corrosion • Classification of corrosion: • 1. Chemical corrosion • 2. Electrochemical corrosion
- 8. Corrosion • Chemical Corrosion: • Chemical corrosion is the direct combination of metallic and non-metallic elements to yield a chemical compound through oxidation reactions • It can also be a corrosion product of dental gold alloys that contains silver.