Orbitals

Orbitals

1. Chemical bonds= overlap of an atoms' individual electron clouds, rather than the sharing of specific electrons

   • Atoms are ball-like with a electrons in a spherical cloud around the nucleus

2. Molecules form from overlapping electron clouds flowing around the nuclei of bonding atoms

   • Un-bonded atoms within a molecule generally like to be as far away from eachother as possible, especially if they have the same partial charge
     • Electrons are both particles and waves

3. KEY VOCAB TERMS

   • Wave Function
     • a mathematical function that describes the probability that an electron is in a certain place at any given moment
   • Standing Waves
     • Electrons function the same way; they exist as excitations in the electron field around the nucleus in a standing wave
       • Can have different numbers of nodes drawing pattern to repeat themselves when there are more electrons around the nucleus
   • Periodic Table
     • Map of orbitals as they fill
       • Elements in the s block are filling their s orbitals
       • Elements in the p block are filling their p orbitals
   • Hybridization
     • the s and p orbitals can merge into sp orbitals and become 4 identical orbitals trying not to overlap
       • When the s orbital hybridizes with all 3p orbitals its called Sp3 Hybridization and it forms a tetrahedral shape

4. S orbital

   • Contains 2 electrons and is a spherical pattern of standing waves around the nucleus
     • Every orbital is at its lowest energy when it contains 2 electrons

5. P orbital

   • After we fill the first and second s orbitals, we move on to filling the p orbital
     • There can be one on the x axis, there can be one on the y axis, and there can be one on the z-axis
       • Each of these contain two electrons for a total of 8 with 2 in the s orbital and 6 in the 3p orbital

6. Example

   • In water, oxygen's 8 electrons are arranged with 2 in each SP3 orbital. 2 are from hydrogen and 6 are from oxygen including 2 lone pairs. (LONE PAIRS STILL HAVE ORBITALS)

7. WHY IMPORTANT?

   • These orbital configurations determine the shape of molecules, and the shape of molecules determine how they behave and what forms they take, and what properties they have