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Chemical Bonding Theories

Topic Review on "Title":

Atoms bond chemically to form molecules.

Types of bonding
The periodic table is organized in columns, called groups or families, and rows, called periods.  There are several groups or periods that have specific names.

Bond type

Happens between

Electrons are

Ionic

Metal & non-metal

Transferred

Covalent

Non-metals

Shared

Polar Covalent

Non-metals

Shared unevenly

Metallic

Metals

pooled

There are general characteristics of each type of bonding:

  • Ionic: High melting points, most dissolve in water, conduct electricity when dissolved in water, brittle
  • Covalent: Low melting points, most do not dissolve in water, do not conduct electricity when dissolved in water
  • Polar covalent: Medium melting points, some dissolve in water, do not conduct electricity when dissolved in water
  • Metallic:  Soft, conduct heat and electricity, do not dissolve in water

Bond Polarity
When nonmetals bond covalently with a large difference in electronegativity, a polar bond is formed.  A polar bond has a partial separation of charges.  Polar bonds are symbolized with an arrow pointing towards the more electronegative element and a crossed tail by the less electronegative element

Isomers and Resonance
Isomers are compounds with the same chemical formula but different chemical structure.  Resonance occurs when a double bond can be placed in more than one place in a structure without creating isomers.

Bonding theory
The Valence Shell Bonding Theory assumes that bonds are formed when atomic orbitals overlap.  Direct overlap leads to sigma bonds and parallel overlap leads to pi bond.  The Hybridization Theory says that the sigma bonds are all identical around an atom, therefore the orbitals forming them must be identical.  Therefore, any atomic orbitals involved in sigma bonds hybridize into identical orbitals to bond.  The Molecular Orbital Theory says that rather than overlapping atomic orbitals, or hybridized atomic orbitals, new orbitals are formed in the molecule that are separate.  Some of the new orbitals formed pull the two nuclei together and are bonding orbitals.  However, some of them pull the two orbitals apart and are anti-bonding orbitals.  The bond order is the number of bonding orbital electrons – the number of antibonding orbital electrons divided by 2.  The bond order can be used to determine the type of bond (single, double, triple).


Rapid Study Kit for "Title":
Flash Movie Flash Game Flash Card
Core Concept Tutorial Problem Solving Drill Review Cheat Sheet

"Title" Tutorial Summary :

Atoms chemically bond together to form molecules.  This tutorial introduces the types of bonds that occur, and theories on how orbitals in the molecule.


Tutorial Features:

Specific Tutorial Features:

  • Molecular animations of orbitals coming together to bond
  • 3D visualization of hybrid and molecular orbitals
  • Animation of electrons moving from atomic orbitals to molecular orbitals
  • How do these questions look on the AP Exam?

 Series Features:

  • Concept map showing inter-connections of new concepts in this tutorial and those previously introduced.
  • Definition slides introduce terms as they are needed.
  • Visual representation of concepts
  • Animated examples—worked out step by step
  • A concise summary is given at the conclusion of the tutorial.

"Title" Topic List:
  • Bonding
    • Ionic
    • Covalent
    • Polar Covalent
      • Bond polarity
    • Metallic
  • Isomers and resonance
  • Bonding theories
    • Valence shell bonding
    • Hybridization
    • Molecular orbital
      • Bonding and anti-bonding orbitals
      • Bond order


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