Chapter 6 Chemistry

Chapter 6 Section 5 Part 2: Hybridization

by Abby Fancsali

​Hybridization

• ​VSEPR Theory is useful for explaining the shapes of molecules, but doesn't explain the relationship between the geometry and shared electrons

• ​Hybridization: the mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies

• ​Hybrid Orbitals: Orbitals of equal energy produced by the combination of two or more orbitals in the same atom

​What does this even mean?

• ​Let's look at the molecule BeF_2, Specifically, its electron configuration

  • ​Fluorine is in good shape, its notation is 1s²2s²2p⁵

    • ​Has unpaired electrons

  • ​Beryllium has a configuration of 1s¹2s²

    • ​no unpaired electrons, but still wants to bond to try and get 8

    • ​To bond, Beryllium will move one of its electrons to the p-orbital

      • ​One Fluorine bonds with the s-orbital electron, one bonds with the p-orbital, making a new shape

• ​The Geometry of some molecules are only possible to do hybridization

Multiple Choice

What is the mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies?

• Hybridization

• atomic collision

• Orbital growth

• Energy Bonding

Multiple Choice

what type of geometry does an sp hybrid have

• Trigonal planar

• Linear

• Tetrahedral

​Intermolecular Forces

• ​Intermolecular Forces: The forces of attraction between molecules

  • ​Vary in strength, but a generally weaker than bonds

    • ​A good way to measure is to look at boiling points

      • ​Higher boiling point=stronger bond of attraction

​Molecular Polarity and Dipole-Dipole Forces

• ​The strongest intermolecular forces exist between polar molecules, which create dipoles

  • ​Dipole: a force created by equal but opposite charges that are separated by a short distance

    • ​direction moves from positive end to negative end

    • ​Negative end of one attracts positive end of another, creating dipole-dipole force

    • ​How they act depends on molecule shape

      • ​See figure 26 on page 205

​Hydrogen Bonding

• ​Hydrogen bonds tend to have a large electronegativity difference, making them more polar

  • ​Hydrogen has a high positive charge and is small enough to get close to electrons of adjacent molecules

• ​Hydrogen Bonding: the intermolecular force in which a hydrogen atom is that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom

​London Dispersion Forces

• ​In any atom, molecules are in constant motion

  • ​at any instant, charge may be uneven, creating a temporary dipole that can attract other atoms

• ​London Dispersion Forces: the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles

  • ​Act between all atoms and molecules

  • ​the only forces that act on the Noble Gases

  • ​Increase with the number of electrons/ increasing atomic number

Multiple Choice

What are the forces of attraction between molecules

• Intermolecular forces

• polar bonds

• ionic bonds

• the atomic force

Multiple Choice

What is the strongest intermolecular force

• Dipole-Dipole Forces

• Ionic force

• boiling force

• covalent force

Multiple Choice

What type of bonding is responsible for the high boiling point of water

• Hydrogen Bonding

• Ionic Bond

• Metallic Bonding

• London Bonding

Multiple Choice

Which force acts on all molecules, including the noble gases

• Hydrogen forces

• No Force

• London Dispersion Force