Subject: Periodic classification of elements
Introduction:-
Matter around us is present in the form of elements, compounds and mixtures.
Elements contain atoms of only one type .
Till now 114 elements are known to us.
Around 1800, only 30 elements were known.
All these had different properties.
More elements discovered with time ,so scientist gather more and more information about the properties of these elements.
Making order out of chaos - early attempts at the classification of elements.
Dobereiner's Triads:-
In 1817, Johann Wolfgang Dobereine, tried to arrange elements with similar properties into groups.
He identified some groups having three elements each.
So he called these groups 'traids'.
He showed that when three elements in a triad were written in order of increasing atomic masses; the atomic mass of the middle element was roughly average of the atomic masses of the other two elements.
For example:-
Atomic mass of Li =6.9
Atomic mass of Na = 23.0
Atomic mass of K = 39.0
Average of atomic masses Li and K = mass of Na
6.9+39.0/2 =mass of Na
45.9/2=mass of Na
22.95= 23.0(approx)=mass of Na
Limitations of Dobereiner's classification=
At that time 30 elements are known to exist but only 9 were classified in the form of 3 triads.
Newlands' law of octaves:-
In 1866, John Newlands' arranged the then known elements in order of increasing atomic masses.
He started with the element having he lowest atomic mass (Hydrogen) and ended at thorium which as the 56th element.
He found that every eighth element had the properties similar to that of the first .
He compared this to the octaves found in music.
Therefore, he called it the 'law of octaves'.
It is known as 'Newlands Law of Octaves'.
At that time 56 elements elements were known.
Limitations of Newlands'law of octaves:-
It is found that the Law of octaves was applicable only upto calcium as after Calcium every eighth element didn't possess properties similar to that of the first.
It is assumed by Newlands' that only 56 elements existed in nature and no more elements would be discovered in the future. But , later on , several new elements were discovered, whose properties didn't fir into the law of octaves.
In order to fit elements into his table, Newlands'adjust two elements in the same slot, but also put some unlike elements under the same note.
Example:- Cobalt and nickel are in the same slot and these are placed in the same column as fluorine, chlorine and bromine which have different properties then these elements.
Iron which resembles cobalt and nickel in properties has been placed far away from these elements.
Thus Newlands' Law of octaves worked well with lighter elements only.
Making order out of choas- Mendeleev's Periodic table :-
Dmitri Ivanovich Mendeleev was the most important contributor to the early development of a periodic table of elements where in the elements were arranged on the basis of their fundamental property, the atomic mass and also on the similarity of chemical properties.
When Mendeleev started his work , 63 elements were known.
He examined the relationship between the atomic masses of the elements and their Physical and chemical properties.
Among chemical properties, Mendeleev concentrated on the compounds formed by elements with oxygen and hydrogen.
He selected Hydrogen and oxygen as they are very reactive and formed compounds with most elements.
The formulae of hydride and oxides formed by an element were
treated as one of the basic properties of an element for its classification.
How he classify??
He took 63 cards and on each card he wrote down the properties of one element.
He sores out the elements with similar properties and pinned the cards together on a wall
He observed that most of the elements got a place in a periodic table and were arranged in order of their increasing atomic masses.
It was also observed that there occurs a periodic recurrence of elements with similar physical and chemical properties.
On this basis, Mendeleev formulated a periodic law, which states that' 'properties of elements are the periodic function of their atomic masses.
Mendeleev's Periodic Table contains vertical columns called 'groups' and horizon rows called 'periods'.
Achievements of Mendeleev's Periodic table:-
While developing the Periodic Table, there were a few instances where Mendeleev had to place n element with slightly greater atomic mass before an element with a slightly lower atomic mass.
The sequence was Invented so that elements with similar properties could be grouped together.
For example, Cobalt appeared before nickel.
Atomic mass of cobalt = 58.9
Atomic mass of nickel = 58.7
He left some gaps in his periodic table and predicted the existence of some elements that had not been discovered at that time.
He named them by prefixing a Sanskrit numeral, Eka (one) to the name of preceding element in the same group.
Example:- scandium , gallium and germanium , discovered later, have properties similar to Eka-boron , eka aluminium and eka silicon, respectively. The properties of Eka aluminium predicted by Mendeleev and those of element , gallium which was discovered later and replaced eka aluminium.
Noble gases such as helium(He), neon(Ne) and argon(Ar) have been discovered very late because they are inert and present in low concentrations in our atmosphere. these could placed in a new group without disturbing the existing order.
Limitations of Mendeleev's classification:-
Electronic configuration of Hydrogen resemble that of alkali metal.
Like alkali metals Hydrogen combine with halogen, sulphur and oxygen to form compounds having similar formulae.
On the other hand like halogens, Hydrogen also exists as diatomic molecules and it combines with metals and non-metals to form covalent compounds.
So , no fixed position can be given to Hydrogen in the periodic table. This was the first limitation of Mendeleev's Periodic table.
Isotopes were not considered.
Atomic mass donot increase in regular manner in going from one element to next.
So it was not possible to predict how many elements could be discovered between two elements.
Making order out of chaos – The modern periodic table:-
In 1913 , Henry Moseley showed that thr atomic number of an element is a more fundamental property than its atomic mass.
Modern periodic law:- property of an element is the periodic function of their atomic number
Position of elements in the modern periodic table:-
Modern periodic table has 18 vertical columns known as "groups" and
7 horizontal rows known as period s.
Elements present in one group have same number of valance electrons.
For example :- Fluorine and chlorine belong to group 17 , so have 7 electrons in outermost shell.
Number of shells increase as we go down the group.
Atomic number increases by one unit on moving from left to right
Trends in modern periodic table:-
Valency :- the combining capacity of the element.
Example:- sodium:- 2,8,1
Valency :- 1
Chlorine :- 2,8,7
Valency:- 7
Carbon :- 2,8,4
Valency :- 4
Atomic size:- It refers to radius of an atom.
It refers to distance between the centre of nucleus and outermost shell of an isolated atom.
Atomic radius of Hydrogen atom is 37pm.
Atomic radius decrease along the period.
Reason:- this is due to increase in nuclear charge which tends to pull the electrons closer to the nucleus and reduces the size of the atom.
Atomic radius increase along the group.
Reason:- this is because the distance between the nucleus and the outermost shell increase due to increase in number of shell.
Metallic and non-metallic properties:-
Metals tend to lose electrons while forming bonds . So they are electropositive in nature.
Down the group electron loosing tendency increase and so metallic character increase.
Along the period effective nuclear charge increase and so metallic character decrease.
Non-metals are electronegative.
They tend to form bond by gaining electron.
Along the period non-metallic character increase.
Metal oxides are basic in nature.
Non-metal oxide are acidic in nature.