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Chemical Bonds

Chemical Bonds. Metallic Ionic Covalent. Background Information. Most atoms are not found uncombined in nature. Atoms combine to become stable (“stable 8”). Chemical bonds are the forces that hold atoms/ions together.

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Chemical Bonds

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  1. Chemical Bonds Metallic Ionic Covalent

  2. Background Information • Most atoms are not found uncombined in nature. • Atoms combine to become stable (“stable 8”). • Chemical bonds are the forces that hold atoms/ions together. • The properties of elements are different from the properties of their compounds.

  3. Periodic Patterns • Column number=number of valence (outer electrons) • Atoms lose, gain, or share electrons to have a stable octet (8 valence electrons) • Oxidation numbers are + or – numbers that indicate whether an atom loses/gains electrons to become stable He N Ne B C O F Li Be Gains 2 Gains 1 Gains 3 Loses 2 Loses 3 Loses 1 -1 -2 -3 +3 +2 +1

  4. Types of Bonds Covalent Nonmetal+Nonmetal Electrons are Shared Form network of molecules Do not conduct when dissolved in water Low melting & boiling points Ionic Metal+Nonmetal Electrons are Transferred Form Crystals Conduct when dissolved in water High melting & boiling points Metallic Metal+Metal Equal Sharing of Electrons Conduct electricity & heat Easily shaped

  5. Bonding & Valence Electrons • Elements try to have 8 valence electrons (except H, He, Li, Be, B) • Elements will lose, gain, or share electrons • If elements have less than 4 electrons, they will lose electrons; these acquire a positive charge • If elements have more than 4 electrons, they will gain electrons; these acquire a negative charge

  6. Formation of NaClIonic Bond

  7. Formation of Water H2OCovalent Bond

  8. Now You Try:Use Bohr Models or Lewis Dot Diagrams to Show Bonding for 1) Ionic Bonding Between Mg & O 2) Covalent Bonding for CO2

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