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Covalent Bonding (Molecules)

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Published in: Chemistry
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This PowerPoint presentation provides an in-depth look at covalent bonding, one of the fundamental types of chemical bonds responsible for forming molecules. Covalent bonding occurs when two nonmetal atoms share electrons to achieve a full outer shell, resulting in a more stable electron configuration. The presentation concludes with an emphasis on the significance of covalent bonding in creating the vast variety of molecules found in both biological systems and everyday materials, such as plastics, gases, and organic compounds.

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  1. Covalent Bonding Bonding models for H H methane, CH4. Models are NOT reality. Each has its own strengths and limitations.
  2. CA Standards C] Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds. C] Students know chemical bonds between atoms in molecules such as 1--12, CH4, NH3 H2CCH2, N2, C12, and many large biological molecules are covalent. C) Students know how to draw Lewis dot structures.
  3. The Octet Rule and Covalent Compounds •:• Covalent compounds tend to form so that each atom, by sharing electrons, has an octet of electrons in its highest occupied energy level. •:• Covalent compounds involve atoms of nonmetals onl . The term "molecule" is used exclusively for covalent bonding
  4. The Octet Rule: The Diatomic Fluorine Molecule Is Is Each has seven valence electrons
  5. The Octet Rule: The Diatomic Oxygen Molecule Is Is Each has six valence electrons
  6. The Octet Rule: The Is Is Diatomic Nitrogen Molecule Each has five valence electrons
  7. Lewis Structures CILewis structures show how valence electrons are arranged among atoms in a molecule. QLewis structures Reflect the central idea that stability of a compound relates to noble gas electron configuration. OShared electrons pairs are covalent bonds and can be represented by two dots (:) or by a single line (
  8. The HONC Rule Hydrogen (and Halogens) form one covalent bond • Qxygen (and sulfur) form two covalent bonds One double bond. or two single bonds • Nitrogen (and phosphorus) form three covalent bonds One triple bond, or three single bonds, or one double bond and a single bond • Carbon (and silicon) form four covalent bonds. Two double bonds, or four single bonds, or a triple and a single, or a double and two singles
  9. Completinq a Lewis Structure -CH3Cl Make carbon the central atom (it wants the most bonds, 4) Add up available valence electrons: C = 4, H = Cl = 7 Total = 14 Join peripheral atoms to the central atom with electron pairs. Complete octets on atoms other than hydrogen with remaining electrons Cl
  10. Bond Bond Length and Length (pm) 154 134 120 147 132 116 143 120 113 145 125 Bond Energy Energy (kJ/mol) 346 612 835 305 615 887 358 799 1072 180 418
  11. Resonance • Occurs when more than one valid Lewis structure can be written for a particular molecule. 080 O No • These are resonance structures. The actual structure is an average of the resonance structures.
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