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Semiconductors

Topic Tree (Ignore Deleted Portions)

Semiconductor Devices

├── Semiconductors
│ ├── Intrinsic
│ │ └── Pure Semiconductor
│ ├── Extrinsic
│ │ └── p-type and n-type Semiconductor
│ ├── Valence Band
│ ├── Conduction Band
│ ├── Energy Gap
│ ├── PNP
│ │ └── CE mode
│ └── NPN
│ ├── CB mode
│ └── CC mode

├── Transistors
│ (linked from Semiconductor → PNP/NPN structure)

├── Junction Diodes
│ ├── PN-Junction Diode
│ │ ├── Potential Barrier and Field
│ │ ├── Depletion Region
│ │ └── Rectifier (Half Wave & Full Wave)
│ │ └── Filter
│ ├── Zener Diode
│ │ ├── I–V Characteristics
│ │ └── Voltage Regulator
│ ├── Photo Diode
│ └── LED

└── Logic Gates
├── NAND
├── AND
├── OR
├── NOR
└── NOT

SaitechAI • Electronics Lecture Cards (Compact)

SaitechAI • Electronics Lecture Cards

Energy Bands → Semiconductors → PN Junction → Biasing → Rectifiers

EB

Energy Band Theory

VB • CB • Forbidden gap (Eg)
Concept
  • In crystals, atomic levels spread into bands.
  • VB: highest filled, CB: next higher; Eg has no states.
  • Fermi level EF: 50% occupancy at equilibrium.
Conductor SemiconductorEg Insulator Conduction requires carriers + empty states near EF
CMP

Conductors vs Semiconductors vs Insulators

σ(T), carriers, EF
PropertyConductorSemiconductorInsulator
Band pictureVB overlaps CBSmall Eg (~0.7–3 eV)Large Eg (>~5 eV)
CarriersElectronse⁻ & h⁺Bound
σ vs T↓ with T↑ with T≈0
Why σ↑ with temperature in semiconductors? Thermal energy generates e⁻–h⁺ pairs (VB→CB), increasing carrier density.
SC

Intrinsic & Extrinsic Semiconductors

Fermi level shift • Majority carriers
  • Intrinsic: n = p = ni, EF ≈ mid-gap; σ = q(nμn+pμp).
  • n-type: donors → electrons majority; EF ↑ toward CB.
  • p-type: acceptors → holes majority; EF ↓ toward VB.
  • Mass action: np=ni2.
Intrinsic EF n-type EF
PN

PN Junction • Equilibrium

Depletion region • Vbi
  • Diffusion leaves fixed ions → depletion with built-in potential Vbi.
  • Equilibrium: drift current = diffusion current.
Vbi = (kT/q) ln(NaNd/ni2)
pn Depletion
FB

Forward Bias

Diode equation & knee
  • p→+, n→− lowers barrier, width ↓, large I after threshold.
  • I = Is(e^{VD/(nVT)} − 1)
  • VT≈25.9 mV @ 300 K; n≈1–2.
+
RB

Reverse Bias

Leakage • Breakdown
  • p→−, n→+ raises barrier; I ≈ Is (tiny) till breakdown.
  • Zener/avalanche at high |VR|.
HWR

Half-Wave Rectifier

Single diode • High ripple
  • Average DC: Vdc=Vm; Ripple factor ≈1.21; η ≈40.6%; PIV =Vm.
R
FWR

Full-Wave Rectifier

Bridge • Low ripple
  • Average DC: Vdc=2Vm; Ripple ≈0.482; η ≈81.2%.
  • PIV: bridge Vm, centre-tap 2Vm.
R
QP

Quick Practice

Check-your-understanding
  1. Why do insulators show negligible conductivity at room temperature?
  2. In B-doped Si, identify majority/minority carriers.
  3. Write diode I–V equation and define symbols.
  4. Bridge FWR with Vm=12 V → Vdc?
  5. Define PIV; give values for HWR and centre-tap FWR.
Answers
  • Large Eg, no states near EF, no free carriers.
  • p-type: holes majority; electrons minority.
  • I = Is(e^{VD/(nVT)}−1); Is: saturation, n: ideality, VT=kT/q.
  • Vdc=2Vm/π≈7.64 V.
  • HWR: Vm; centre-tap FWR: 2Vm.
SUM

One-Page Summary

From bands to rectifiers
  • Metals: band overlap; Semis: small Eg; Insulators: large Eg.
  • Doping shifts EF, sets majority carriers.
  • PN junction: depletion + Vbi; bias controls barrier/current.
  • Rectifiers: HWR (simple, high ripple) vs FWR (better DC, lower ripple).
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Covalent Bond

Chapter: Chemical Bonding, Class 11

Study Notes

Covalent Bond

Covalent Bond – SaitechAI Topic Card
SaitechAI

Covalent Bond – Lecture Notes

Class 11 | Chemistry

Definition
A covalent bond is sharing of electrons between atoms to achieve stable electronic configuration.
Types
Single, Double, Triple, Coordinate covalent bond.
Characteristics
Usually low melting and boiling points (except network solids), poor electrical conductivity, often soluble in non-polar solvents.
Classification based on Electronegativity
Non-polar covalent bond → negligible ΔEN (e.g., H₂, Cl₂, O₂).
Polar covalent bond → moderate ΔEN with partial charges (e.g., HCl, H₂O, NH₃).
Lewis Representation of Simple Molecules
Dot-and-cross structures for shared pairs (e.g., H₂O: two bonding pairs + two lone pairs on O).

Variable Covalency and Its Reason
Elements with vacant d-orbitals (P, S, Cl) can expand their octet and show multiple valencies (PCl₃ vs PCl₅, SF₆).
Formal Charge
FC = (Valence e⁻) − (Nonbonding e⁻ + ½ × Bonding e⁻); helps identify the most stable resonance structure.
Bond Parameters
Bond length → Triple < Double < Single.
Bond angle → CH₄ (109.5°) > NH₃ (107°) > H₂O (104.5°).
Bond enthalpy → Triple > Double > Single.
Bond order → Higher order means stronger, shorter bonds; resonance gives fractional.
Limitations of Octet Rule / Deviations
Incomplete octet (BeCl₂, BF₃).
Expanded octet (SF₆, PCl₅).
Odd-electron species (NO, NO₂).
Hypervalent / hypovalent molecules.
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