The Physics Of Atomic Structure - 963 Words

Lesson 1 1. Increasing current funding for atomic structure would be a fantastic idea which could lead to discoveries beyond our imagination. For instance, in the quantum mechanical model, the fact that it is unable to tell the exact location and speed of the electron and cannot describe the electron as a particle orbiting a fixed path around the nucleus provides evidential support that funding must be placed into this to further our knowledge. This research could potentially result in terminating the use of probability mathematical equations and replacing them with facts. By just looking at the many revised versions of the atomic structure, we are able to see that there is potential in knowing more which could lead to even more†¦show more content†¦Many wait weeks or even months to receive an MRI, thus, making it very difficult to believe that funding needs to go to more research rather than providing more MRI machines to be used. 2. There is a difference in energy between the two lines because the electrons move from higher to lower orbitals. The line within the visible spectrum is an electron that is moving from a 5th orbital to a 2nd and the line within the Ultraviolet area is an electron moving from a 6th orbital to a 2nd, thus meaning that the line within the visible spectrum gives off less energy when releasing light whereas the ultraviolet spectrum gives off more energy. 3. a) b) After reviewing the diagram, you can conclude that the Zr4+ ion exists because in order for the Zr atom to become stable, it gets rid of 4 electrons from the 4d and 5s orbitals. c) The Zr4+ ion is more stable because it outer shell (valance shell) is complete following the octet rule. When this occurs, the atom is less likely to react because it is most stable. Comparing it to the Zr atom, the Zr atom does not have a filled valence shell. Lesson 2 4. NH3 5. a) HCN b) SOC3 -2 S = 6 O = 6 O = 6 O = 6 6 +18 +2 = 26 6. a) NH3 Hybrid orbitals b) HN3 sp3 = sigma bonds (4 bonding) c) Nitrogen has 5 electrons with 4 orbitals and 1 lone pair. The bond is different because Nitrogen has one lone pair and the lone pair results in a more negative pull