Hund’s rule can be stated in a way that every orbital present in the sublevel of an atom is first singly occupied by an electron. When all the orbitals present in the atom are occupied by single electrons, then they are doubly filled. It is because electrons carry a negative charge and hence, repel each other, therefore, they tend to remain in their orbitals to minimize repulsion.
Moreover, the electrons present in the singly occupied orbitals must have the same spin (either clockwise or anti-clockwise). In this way, the total spin is incredibly maximized. The direction of the spin of electrons of all orbitals is dependent on the spin of the first electron. Following is an example given of nitrogen orbitals:
Draw and name four terminal alkynes with the molecular formula C6H10.
Report the result of the following addition to the proper number of
Scorzocreticin (S)-1 was isolated from a plant that is
Write an equation for the proton transfer reaction that occurs when each
87. What is the major product of this reaction?
Propose a stepwise mechanism for the following transformation: /
Identify the sole product of the following reaction: /
Draw the condensation product that is expected when each of the following
Draw a mechanism for each of the following transformations: /
Draw each of the following using condensed formulas and line formulas:
