A basic introduction to Organic chemistry
By definition, we know that organic chemistry is the largest branch of chemistry which is all about the study of compounds of carbon. Carbon is a very important element as it alone has millions of compounds.
Carbon results in this high number of compounds due to its ability to make bonds with itself and other elements. Probably it is the major factor for carbon to exhibit multiple bonding. These elements are hydrogen, oxygen-nitrogen.
In this article, we will study how carbon makes bonds with these elements to give a variety of compounds that all the other members of the periodic table collectively cannot compete. For this purpose let us discuss the electronic structure of atoms first.
Electronic structure of the atom
We know that atom is the smallest particle of matter which contains a dense nucleus ( protons & neutrons). The surrounding of the nucleus is attributed to the extranuclear space which contains negatively charged particles called electrons.
The diameter of the nucleus ( 10-14 to 10-15) is smaller than the diameter of the extranuclear space (10-10).
Diagram showing the basic structure of atom
Basic terminologies regarding Atomic structure
Shells
Shell defines the probability of finding an electron in various regions of space relative to the nucleus. The energy of electrons in the shell is quantized which means having discrete values for energy.
We can identify the electronic shells by the principle quantum numbers 1, 2, 3, and so forth by following 2n2 rule. Here n shows the number of shells. For example, the first shell can accommodate only two electrons and the second 8.
Orbital is a region with specific quantized energy that can hold two electrons.For example,1s, 2s, 2p,3d,4f etc.
Aufbau principle
Pauli exclusion principle
It
states that no more than two electrons may accommodate in an orbital. Moreover, the spin of these two electrons must be paired.
The pairing of electron spins
Hund’s rule
It has two parts.
The first part states that when orbitals having equal energy (
called degenerate orbitals )but no electrons to fill all of them completely,
Then one electron fills each orbital before a second electron is added to any.
The second rule states that spins of the
single electron in the degenerate orbitals should be aligned.
This post is written by PrepChemistry.blogspot.com
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