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Part 02 Covalent Bonding and Covalent Compounds

Part 02 Covalent Bonding and Covalent Compounds. 1. Covalent Bonding - two or more non metals - two or more semi metals - share at least one pair of valence electrons - all the atoms get a stable octet or in the case of hydrogen, a duet

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Part 02 Covalent Bonding and Covalent Compounds

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  1. Part 02Covalent BondingandCovalent Compounds

  2. 1. Covalent Bonding - two or more nonmetals - two or more semimetals - share at least one pair of valence electrons - all the atoms get a stable octet or in the case of hydrogen, a duet - a molecule is formed. The sharing of valence electrons holds the atoms together

  3. 2. Covalent Bonding Between Like Atoms: The Diatomic Molecules H H Lewis Dot Diagram - shared pair belongs to both atoms - each atom has a stable duet

  4. H H Structural Diagram - dash represents one shared pair of valence electrons - a single covalent bond - formula, H20 - no charges, no electrons lost or gained - name, dihydrogen, or just hydrogen - shape or molecular geometry, linear

  5. Lewis Dot Diagram F F - shared pair belongs to both atoms - each atom has a stable octet

  6. Nonbonding electrons F F Structural Diagram Bonding electrons - a single covalent bond - formula, F20 - no charges, no electrons lost or gained - name, difluorine, or just fluorine - shape or molecular geometry, linear

  7. Nonbonding electrons I I Structural Diagram Bonding electrons - all the other halogens bond the same way - Cl2, Br2, I2 all with no charge

  8. O O O O No octets! Unpaired electrons! O O Lewis Dot Diagram

  9. O O Structural Diagram - two dashes are two shared pairs of electrons, i.e., four electrons - a double covalent bond - all the other electrons are nonbonding electrons

  10. O O Structural Diagram - formula, O20 - no charge, no electrons lost or gained - name, dioxygen or just oxygen - shape or molecular geometry, linear

  11. N N N N N N No octets! Unpaired electrons! N N No octets! Unpaired electrons! Lewis Dot Diagram

  12. N N Structural Diagram - three dashes are three shared pairs of electrons, i.e., six electrons - a triple covalent bond - all the other electrons are nonbonding electrons

  13. N N Structural Diagram - formula, N20 - no charge, no electrons lost or gained - name, dinitrogen or nitrogen - shape or molecular geometry, linear

  14. 3. Summary: The Diatomic Molecules a. Single Covalent Bonds 1) Hydrogen, H2 2) Fluorine, F2 3) Chlorine, Cl2 4) Bromine, Br2 4) Iodine, I2 b. Double Bond, Oxygen, O2 c. Triple Bond, Nitrogen N2 Assignment: Read p236-240

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