hypervalent molecule

Examples of hypervalent molecule in the following topics:

• The Expanded Octet

  • A hypervalent molecule is a molecule that contains one or more main group elements that bear more than eight electrons in their valence levels as a result of bonding.
  • Phosphorus pentachloride (PCl5), sulfur hexafluoride (SF6), chlorine trifluoride (ClF3), and the triiodide ion (I3−) are examples of hypervalent molecules.
  • In the SF6 molecule, the central sulfur atom is bonded to six fluorine atoms, so sulfur has 12 bonding electrons around it.
  • The overall geometry of the molecule is depicted (tetragonal bipyramidal, or octahedral), and bond angles and lengths are highlighted.
  • The overall geometry of the molecule is depicted (trigonal bipyramidal), and bond angles and lengths are highlighted.

• Bonding in Coordination Compounds: Valence Bond Theory

  • Valence bond theory is used to explain covalent bond formation in many molecules.
  • In 1927, physicist Walter Heitler and collaborator Fritz London developed the Heitler-London theory, which enabled the calculation of bonding properties of the covalently bonded diatomic hydrogen molecule (H2) based on quantum mechanical considerations.
  • Valence bond theory is used to explain covalent bond formation in many molecules, as it operates under the condition of maximum overlap, which leads to the formation of the strongest possible bonds.

• The Nonclassical Carbocation Hypothesis

  • One of the best criteria for evaluating candidate ions is to establish whether one or more of the participating carbon atoms is hypervalent (has more than four coordinating groups).
  • In the first diagram below, the simplest hypervalent carbocation, methanonium, is drawn on the left in the gray shaded box.

• 1,2-Group Shifts

  • When alkoxide base is added to silyl ketones, hypervalent silicon intermediates may be formed prior to rearrangement, shown in the fourth diagram above.

• Homonuclear Diatomic Molecules

  • Diatomic molecules are composed of only two atoms, of either the same or different chemical elements.
  • Common diatomic molecules include hydrogen (H2), nitrogen (N2), oxygen (O2), and carbon monoxide (CO).
  • All diatomic molecules are linear, which is the simplest spatial arrangement of atoms.
  • Translational energies (the molecule moving from point A to point B)
  • A space-filling model of the homonuclear diatomic molecule nitrogen.

• Molecules

  • Most often, the term "molecules" refers to multiple atoms; a molecule may be composed of a single chemical element, as with oxygen (O2), or of multiple elements, such as water (H2O).
  • Most molecules are too small to be seen with the naked eye.
  • The full elemental composition of a molecule can be precisely represented by its molecular formula, which indicates the exact number of atoms that are in the molecule.
  • Isomers are molecules with the same atoms in different geometric arrangements.
  • Each molecule is a structural isomer of the other.

• Polyatomic Molecules

  • A polyatomic molecule is a single entity composed of at least three covalently-bonded atoms.
  • Molecules are distinguished from ions by their lack of electrical charge.
  • The science of molecules is called molecular chemistry or molecular physics, depending on the focus.
  • A pure substance is composed of molecules with the same average geometrical structure.
  • Molecules with the same atoms in different arrangements are called isomers.

• Dipole-Dipole Force

  • Molecules that contain dipoles are called polar molecules and are very abundant in nature.
  • A dipole is a molecule that has split charge.
  • The negatively charged oxygen atom of one molecule attracts the positively charged hydrogen of another molecule.
  • Attractions between polar molecules vary.
  • Choose a pair of molecules from the drop-down menu and "pull" on the star to separate the molecules.

• Introduction to Intermolecular Forces

  • Our chief focus up to this point has been to discover and describe the ways in which atoms bond together to form molecules.
  • Since all observable samples of compounds and mixtures contain a very large number of molecules (ca. !
  • 020), we must also concern ourselves with interactions between molecules, as well as with their individual structures.
  • All atoms and molecules have a weak attraction for one another, known as van der Waals attraction.
  • This attractive force has its origin in the electrostatic attraction of the electrons of one molecule or atom for the nuclei of another.

• Ion-Dipole Force

  • The ion-dipole force is an intermolecular attraction between an ion and a polar molecule.
  • However, ion-dipole forces involve ions instead of solely polar molecules.
  • An ion-induced dipole force occurs when an ion interacts with a non-polar molecule.
  • Ion-dipole forces are generated between polar water molecules and a sodium ion.
  • The oxygen atom in the water molecule has a slight negative charge and is attracted to the positive sodium ion.