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Periodic Table: Groups and Periods:
We use a great number of elements in our daily life without much knowledge of their
properties. Efficient usage of these elements can be made with the knowledge of
their properties. As there are more than hundred elements, it is hard to remember
the properties of each and every element. So, is there an easy way to remember and
understand the properties of elements?
Source: http://en.wikipedia.org/wiki/Periodic_table
A simple solution for this problem was given by a scientist Dmitri Mendeleev in
1869. He grouped all the elements with similar properties in the form of a table.
This table was given the name periodic table. He organized elements in the order
of increasing atomic weight. However, the periodic table we use today is not that
proposed by Mendeleev. There is greater significance for atomic number and can be
found by knowing the number of protons present in the atom. Basing on this fact
Henry Moseley in 1914 reorganized the entire periodic table. He arranged elements
in the increasing order of atomic number. It is the Moseley periodic table that
we use today.
As said earlier, atoms are arranged in the periodic table in rows and columns. The
vertical rows are called groups and the horizontal columns are called periods. There
are 7 periods and 18 groups in a periodic table.
Periods: atomic number of the elements increases as you move from
left to right. The number of elements in a particular period increases as you move
down the periodic table. The period number signifies the highest energy level that
can be attained by the elements in that period. As the number of energy levels increase
as we move down the period there are more number of sub-levels available to accommodate
more number of elements. Thus, the number of elements in a particular period increases
as we move down the periodic table.
Groups: like periods, the atomic number of the elements in a particular
group increases as we move from top to bottom. All the elements in a particular
group have same outer electron configuration i.e. the valence electrons. Due to
the presence of same number of valence electrons, all the elements in a group have
similar properties. All the elements in a periodic table are arranged into two sets
of groups they are Group A elements which are termed as representative elements
and the Group B elements termed as non-representative elements.
As said, all the elements in a group have same outer electronic configuration. So,
all the representative elements i.e. group A elements have s or p sublevels in the
outer orbitals. The non-representative elements have partly filled d-orbitals or
the partly filled f-orbitals. Elements with partly filled d-orbitals are termed
as transition elements and those with partly filled f-orbitals are termed as lanthanides
and actinidies.
The group number given on the top of the periodic table indicates the number of
valence electrons in that group. For example, Group VA will have five electrons
in the outer orbital. As all the A series elements have either s or p sublevels,
we have s2 p3 as their outer configuration.
Solved problems
- What is period table that is being followed now-a-days?
- Mendeleev’s
- Moseley’s
- Both a and b
- Rutherford
- What is the basis for grouping of elements as per the
Moseley’s periodic table?
- Atomic number
- Atomic mass
- Atomic radius
- Ionization energy
- What are vertical rows of a periodic table called?
- Periods
- Groups
- a or b
- None
- The outermost configuration of the elements of group IV
A is
- SP
- S2 P3
- S2 P
- S2 P2
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