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Covalent Bonds & Lewis Dot Structure: Understanding Molecular Formulas and Bonding

Learn about covalent bonds and the Lewis Dot Structure, molecular formulas, single, double, and triple bonds, resonance structures, bond dissociation energy, and real-world applications. Practice problems and quiz included.

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Covalent Bonds & Lewis Dot Structure: Understanding Molecular Formulas and Bonding

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  1. Section 1: Covalent Bonds and the Lewis Dot Structure Chapter 8 in text

  2. Covalent Bonds: Bond formed when valence electrons are shared between atoms. Molecular Formula: Chemical formula that represents how many and the types of atoms that make up the molecule. Example: Methane Molecule CH4

  3. Lewis Dot Structure: Draw the Lewis Dot Structure for each: Li Be B C N O F Ne

  4. Single Bond: atoms in bonding share one set of electronsLewis Dot structure with single bonds Ex) Cl2 Ex) H2O Ex) CH4

  5. More single bond practice Ex) C2H6 Ex) CH2Cl2 Ex) NH4+Ex) C5H12

  6. Lewis Dot Structures for double bonds Ex) O2 Ex) C2H4

  7. Ex) N2F2 Ex) C3H6O

  8. Lewis Dot Structure for Triple Bonds Ex) C2H2 Ex) N2

  9. Resonance Structure: Single bond and double bond switch with each other.

  10. Bond strength listed from least to greatest: Bond Dissociation Energy: Energy required to break the bond. 1) Single Bond 2) Resonance 3) Double Bond 4) Triple Bond Real world Application: Why does our body need oxygen not nitrogen?

  11. Lewis Dot Structure Practice Problems: • C4H10 2) HCN 3) CO2 4) H2O2 5) N2Cl2 6) C2H6

  12. Lewis Dot Structure Quiz 1) C7H16 2) SiH4 3) CH2O 4) CH4O

  13. Warm-up: • What is the difference between ionic and covalent bonds? • Is Calcium Sulfide ionic or covalently bonded and why? • What are valence electrons? • How many valence electrons does nitrogen have?

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