Atomic Structure & Bonding

⚗️ Atomic Structure Bonding

Part 1 of 7 — Atomic Orbitals & Electron Configuration

1. Electron configuration determines bonding

Electron configuration determines bonding

2. Valence electrons

outermost shell electrons

3. Octet rule

atoms tend to have 8 valence electrons

4. Carbon has 4 valence electrons → forms 4 bonds

Carbon has 4 valence electrons → forms 4 bonds

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Key Concepts Summary

• Electron configuration determines bonding
• Valence electrons: outermost shell electrons
• Octet rule: atoms tend to have 8 valence electrons
• Carbon has 4 valence electrons → forms 4 bonds

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Lewis Structures & Formal Charge

Part 2 of 7 — Lewis Structures & Formal Charge

1. Lewis structures show bonding and lone pairs

Lewis structures show bonding and lone pairs

2. Formal charge = valence e⁻ - lone pair e⁻ - ½ bonding e⁻

Formal charge = valence e⁻ - lone pair e⁻ - ½ bonding e⁻

3. Minimize formal charges for best structure

Minimize formal charges for best structure

4. Resonance structures

delocalized electrons

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Key Concepts Summary

• Lewis structures show bonding and lone pairs
• Formal charge = valence e⁻ - lone pair e⁻ - ½ bonding e⁻
• Minimize formal charges for best structure
• Resonance structures: delocalized electrons

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Hybridization

Part 3 of 7 — Hybridization

1. sp³ hybridization

4 bonds, tetrahedral (109.5°)

2. sp² hybridization

3 bonds, trigonal planar (120°)

3. sp hybridization

2 bonds, linear (180°)

4. Hybridization determines molecular geometry

Hybridization determines molecular geometry

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Key Concepts Summary

• sp³ hybridization: 4 bonds, tetrahedral (109.5°)
• sp² hybridization: 3 bonds, trigonal planar (120°)
• sp hybridization: 2 bonds, linear (180°)
• Hybridization determines molecular geometry

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Molecular Orbital Theory

Part 4 of 7 — Molecular Orbital Theory

1. Bonding MOs

lower energy, constructive overlap

2. Antibonding MOs

higher energy, destructive overlap

3. Bond order = (bonding e⁻ - antibonding e⁻) / 2

Bond order = (bonding e⁻ - antibonding e⁻) / 2

4. MO theory explains paramagnetism of O₂

MO theory explains paramagnetism of O₂

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Key Concepts Summary

• Bonding MOs: lower energy, constructive overlap
• Antibonding MOs: higher energy, destructive overlap
• Bond order = (bonding e⁻ - antibonding e⁻) / 2
• MO theory explains paramagnetism of O₂

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Bond Polarity & Dipole Moments

Part 5 of 7 — Bond Polarity & Dipole Moments

1. Electronegativity difference determines polarity

Electronegativity difference determines polarity

2. Dipole moment

μ = q × d

3. Polar bonds in symmetric molecules can cancel

Polar bonds in symmetric molecules can cancel

4. Molecular polarity affects physical properties

Molecular polarity affects physical properties

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Key Concepts Summary

• Electronegativity difference determines polarity
• Dipole moment: μ = q × d
• Polar bonds in symmetric molecules can cancel
• Molecular polarity affects physical properties

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Problem-Solving Workshop

Part 6 of 7 — Problem-Solving Workshop

1. Drawing Lewis structures and assigning formal charges

Drawing Lewis structures and assigning formal charges

2. Determining hybridization from structure

Determining hybridization from structure

3. Predicting molecular geometry

Predicting molecular geometry

4. Calculating bond order from MO diagrams

Calculating bond order from MO diagrams

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Key Concepts Summary

• Drawing Lewis structures and assigning formal charges
• Determining hybridization from structure
• Predicting molecular geometry
• Calculating bond order from MO diagrams

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Synthesis & Review

Part 7 of 7 — Synthesis & Review

1. Bonding fundamentals underpin all organic chemistry

Bonding fundamentals underpin all organic chemistry

2. Hybridization determines geometry and reactivity

Hybridization determines geometry and reactivity

3. Polarity influences intermolecular forces

Polarity influences intermolecular forces

4. Review

structure determines properties

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Key Concepts Summary

• Bonding fundamentals underpin all organic chemistry
• Hybridization determines geometry and reactivity
• Polarity influences intermolecular forces
• Review: structure determines properties

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