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Electrons • closer to nucleus - lower energy • further from nucleus – higher energy

Learn about the significance of electrons in chemical bonding, the Octet Rule, types of bonds (ionic, covalent, hydrogen, metallic), and how electrons form bonds based on energy levels. Discover why atoms gain, lose, or share electrons to achieve stability and explore examples of different bond formations.

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Electrons • closer to nucleus - lower energy • further from nucleus – higher energy

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  1. Electrons •closer to nucleus - lower energy •further from nucleus – higher energy

  2. Chemical bond is an attempt to fill an electron shell. Valence – outer shell 4 Energy Levels: 1. Holds just 2 electrons 2. Holds just 8 electrons 3. Maximum of 18 electrons 4. Maximum of 32 electrons

  3. Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons C would like to N would like to O would like to Gain 2 electrons Gain 4 electrons Gain 3 electrons

  4. Bonding (an attempt to fill electron shell) • Forces that hold the atoms together in compounds are called chemical bonds • The bonds form when atoms share or exchange electrons • Only those electrons having highest energies can form bonds (valence electrons)

  5. Why are electrons important? • different electron configurations mean different type of bonding

  6. Types of Bonds: 1. Ionic bonds 2. Covalent bonds 3. Hydrogen bonds 4. Metallic bonds

  7. IONIC BOND bond formed between two ions by the transfer of electrons

  8. Ionic Bonds: One Big Greedy Thief Dog!

  9. COVALENT BOND bond formed by the sharing of electrons

  10. 2. Covalent bonds- Two atoms share one or more pairs of outer-shell electrons. Oxygen Atom Oxygen Atom Oxygen Molecule (O2)

  11. Covalent Bonds: Unevenly matched, but willing to share.

  12. Metallic Bond • Formed between atoms of metallic elements • electrons are free to move • Good conductors of electric currents, very high melting points • Examples: Fe, Al, Au, Co

  13. Metallic Bonds: Mellow dogs with plenty of bones to go around.

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