how and why does relative atomic size of element lithium (atomic number =3)and oxygen (atomic number =8) present in period 2 of modern periodic table Vary?
Answers
In the Periodic Table, there are a number of physical properties that are not really "similar" as it was previously defined, but are more trend-like. This means is that as you move down a group or across a period, you will see a trend-like variation in the properties. There are three specific periodic trends that we will discuss. The first lesson of this chapter is devoted to the trend in atomic size in the Periodic Table. The two following this lesson will discuss ionization energy and electron affinity. Each of these trends can be understood in terms of the electron configuration of the atoms.
The actual trends that are observed with atomic size have to do with three factors. These factors are:
The number of protons in the nucleus (called the nuclear charge).
The number of energy levels holding electrons (and the number of electrons in the outer energy level).
The number of electrons held between the nucleus and its outermost electrons (called the shielding effect)
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A period 2 element is one of the chemical elements in the second row (or period) of the periodic table of the chemical elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behavior of the elements as their atomic number increases; a new row is started when chemical behavior begins to repeat, creating columns of elements with similar properties.
The second period contains the elements lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, and neon. This situation can be explained by modern theories of atomic structure. In a quantum mechanical description of atomic structure, this period corresponds to the filling of the 2s and 2p orbitals. Period 2 elements obey the octet rule in that they need eight electrons to complete their valence shell.
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