Zumdahl • DeCoste chemistry world of Chapter 12



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Chem Chap 12 pp

Zumdahl • Zumdahl • DeCoste

  • CHEMISTRY
  • World of

Chapter 12

  • Chemical Bonding

Chapter 12 Overview

  • Ionic & covalent bonds & their formation
  • Polar covalent bonds
  • Bond relationships to electronegativity
  • Bond polarity & its relationship to molecular polarity
  • Ionic structures
  • Ionic size
  • Lewis structures
  • Molecular structures & bond angles
  • VSEPR model

Why are graphite and diamonds so different even though they are both carbon?

  • The carbon atoms are bound differently
  • Structure & shape very important

Types of Chemical Bonds

  • Bond: force that holds groups of 2 or more atoms together and makes them function as a unit
  • Bond Energy: the energy required to break a bond
  • Ionic Bonding: attraction between oppositely charged ions
  • Ionic Compound: result of metal reacting with a nonmetal
  • Covalent Bonding: bonding where atoms share electrons
  • Polar Covalent Bond: covalent bond where electrons are not shared equally because on atom attracts them more strongly than the other

Figure 12.1: The formation of a bond between two atoms.

  • Covalent Bond

Figure 12.2: Probability representations of the electron sharing in HF.

  • Polar Covalent Bond

Electronegativity

  • The relative ability of an atom in a molecule to attract shared electrons to itself
  • Chemists determine by measuring the polarities of bonds between different atoms
  • Higher value = higher attraction of electrons
  • Difference between electronegativity values determines polarity of molecule
    • Larger difference = more polar
    • Smaller difference = more equally shared
    • If difference is greater than 2 – bond is ionic (electrons are transferred)

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