This chapter introduces electrochemistry, focusing on the conversion between chemical and electrical energy through oxidation-reduction reactions. It begins with a spontaneous redox reaction between zinc and copper sulfate, leading to the concept of galvanic cells, exemplified by the Daniell cell. The role of the salt bridge, measurement of electrode potentials using the standard hydrogen electrode, and the electromotive series are explained. The chapter then covers different types of galvanic cells (primary and secondary), including mercury, fuel, lead-acid, and lithium-ion batteries, with their reactions and applications. Corrosion of metals, particularly iron, is discussed, including its mechanism and protection methods such as galvanization and sacrificial electrodes. Electrolytic cells are introduced, where electrical energy drives nonspontaneous reactions, and Faraday's laws of electrolysis are presented with calculations. Applications of electrolysis include electroplating, extraction of aluminum, and purification of copper. By the end, students should be able to explain galvanic and electrolytic cell reactions, calculate electromotive force and deposited mass using Faraday's laws, and describe corrosion and protection methods.
Multiple choice questions on this lesson in Chemistry for 3rd secondary, First Term, with practice exercises for revision and exam preparation.
عند استخدام قطب تضحية لحماية أنابيب الحديد المدفونة في الأرض، ما الشرط الواجب توافره في معدن القطب التضحية؟
ما الذي يميز بطارية الليثيوم أيون عن بطارية الرصاص الحمضية؟
في خلية الوقود، ما مصدر الطاقة الذي يتحول إلى طاقة كهربائية؟
أي مما يلي يُعد تطبيقاً صناعياً للتحليل الكهربائي في استخلاص الفلزات؟
ما المصطلح الذي يُطلق على كتلة المادة التي يترسبها واحد فاراداي من الكهرباء؟
في قانون فاراداي الأول للتحليل الكهربائي، ما الذي يتناسب معه كتلة المادة المترسبة؟
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