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3-Phase Servo AVR (AC Voltage Stabilizer) — Parts, Tests, Repair & Maintenance

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3-Phase Servo AVR (AC Voltage Stabilizer) — Troubleshooting, Repair & Maintenance By Edwin Ogie • December 18, 2025 • -- AC Voltage Stabilizer — 3-phase servo control type (example from user photo) A practical, step-by-step guide to diagnose, repair and maintain 3-phase servo Automatic Voltage Regulators (AVR) / servo voltage stabilizers. Written in simple terms for technicians and maintenance teams working with generators, UPS rooms and factories. Includes videos, spare-parts list, safety checklist, troubleshooting flow and links to internal/external resources. Contents Why this matters In environments with unstable mains (frequent sags, surges or phase imbalance) a servo AVR protects sensitive equipment by continuously adjusting an autotransformer tap via a small servo motor. A well-maintained stabilizer saves equipment, reduces downtime and prevents costly damage. ...

Oxidation and Reduction

Edwin Ogie Library: Oxidation & Reduction (Redox) E‑Book

Edwin Ogie Library — Oxidation & Reduction (Redox)

Clear, school‑friendly notes on redox reactions: definitions, oxidation numbers, balancing redox equations, tests and nomenclature.

Page 1 — What is a Redox Reaction?

A redox (oxidation–reduction) reaction is any chemical change where electrons are transferred between species. One species loses electrons (oxidation) while another gains electrons (reduction).

  • Redox can be described by addition/removal of oxygen or hydrogen, by electron transfer, or by a change in oxidation numbers.
  • Every redox reaction has an oxidizing agent (accepts electrons) and a reducing agent (donates electrons).
Redox illustration

Page 2 — Oxidation (Simple Definitions)

Oxidation is when a substance loses electrons. Other easy ways to spot oxidation are when a substance gains oxygen or loses hydrogen.

  • Electron view: Loss of electrons (e⁻). Example: Zn → Zn²⁺ + 2e⁻ (Zn is oxidized).
  • Oxygen/hydrogen view: Addition of oxygen or removal of hydrogen counts as oxidation.
Quick check: In 2Fe + O₂ → 2FeO, iron is oxidized (it gains oxygen).

Page 3 — Reduction (Simple Definitions)

Reduction is when a substance gains electrons. It can also be seen as loss of oxygen or gain of hydrogen.

  • Electron view: Gain of electrons (e⁻). Example: Cu²⁺ + 2e⁻ → Cu (copper is reduced).
  • Oxygen/hydrogen view: Removal of oxygen or addition of hydrogen counts as reduction.
Tip: The species that is reduced is the oxidizing agent because it causes another species to lose electrons.

Page 4 — Oxidation Numbers (How to Assign)

Oxidation numbers help us track electron transfer. Use these simple rules:

  • Free elements have oxidation number 0 (e.g., H₂, O₂, Fe).
  • For simple ions, the oxidation number equals the charge (Na⁺ → +1, Cl⁻ → -1).
  • Oxygen is usually -2 (except in peroxides where it is -1).
  • Hydrogen is usually +1 (except in metal hydrides where it is -1).
  • The sum of oxidation numbers in a neutral compound is 0; in a polyatomic ion it equals the ion charge.
Example: In H₂O, H is +1 and O is -2 → total = 2(+1)+(-2)=0.

Page 5 — Balancing Redox Equations (Simple Steps)

  1. Write the two half-reactions (oxidation & reduction).
  2. Balance atoms other than O and H.
  3. Balance O by adding H₂O; balance H by adding H⁺ (in acidic) or H₂O/OH⁻ (in basic).
  4. Balance charge by adding electrons (e⁻).
  5. Multiply half-reactions to equalize electrons and add them together.
  6. Cancel species that appear on both sides and simplify.
Short worked form: Zn + 2HCl → ZnCl₂ + H₂ (Zn → Zn²⁺ + 2e⁻; 2H⁺ + 2e⁻ → H₂) → combine and balance.

Page 6 — Balancing in Acidic and Basic Media

For reactions in acidic solution use H⁺ and H₂O to balance oxygen and hydrogen. For basic solutions, after balancing in acid, neutralize H⁺ with OH⁻ to form water.

Remember: Acid → use H⁺; Basic → use OH⁻ (after initial acid balance).

Page 7 — Identifying Oxidizing and Reducing Agents

The oxidizing agent is the species reduced (gains electrons). The reducing agent is the species oxidized (loses electrons).

  • Example: In 2Ag⁺ + Cu → 2Ag + Cu²⁺, Ag⁺ is reduced so it is the oxidizing agent; Cu is oxidized and is the reducing agent.

Page 8 — Tests for Oxidizing & Reducing Agents

  • KMnO₄ test: Purple KMnO₄ is decolorized by reducing agents in acidic medium.
  • Iodine-starch test: Iodine gives a blue color with starch; reducing agents remove iodine, fading the color.
  • Dilute HNO₃ test: Strong oxidizing agents may produce brown NO₂ gas.

Page 9 — IUPAC Naming Using Oxidation Numbers

When a metal has variable oxidation states, indicate the state in Roman numerals in brackets after the metal name.

  • Fe₂O₃ → iron(III) oxide (each Fe is +3).
  • CuO → copper(II) oxide (Cu is +2).

Page 10 — Worked Examples (Short)

Example 1

Balance: Fe²⁺ + MnO₄⁻ → Fe³⁺ + Mn²⁺ in acidic medium.\p>

Balanced: 5Fe²⁺ + MnO₄⁻ + 8H⁺ → 5Fe³⁺ + Mn²⁺ + 4H₂O (electrons balanced: 5e⁻).

Example 2

Identify oxidizing and reducing agents: Cu + 2Ag⁺ → Cu²⁺ + 2Ag

Ag⁺ is reduced (oxidizing agent); Cu is oxidized (reducing agent).

Edwin Ogie Library: Oxidation & Reduction (Redox) E‑Book

Edwin Ogie Library — Oxidation & Reduction (Redox)

Clear, school‑friendly notes on redox reactions with a timed practice quiz.

Practice: 20‑Question JAMB CBT Quiz (Timed)

Click the Start Quiz button to reveal questions. The timer will begin (5 seconds). You may submit early using the Submit button. When time expires the quiz auto-submits.

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