Tell me everything about Periodic classification of elements
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Lavoisier divided elements into two main types known as metals and non-metals.
3. Doberiner’s Law of Triads:
According to this law, “in certain triads (grout) of three elements) the atomic mass of the central element was the arithmetic mean of the atomic masses of the other two elements.” But in some triads all the threc elements possessed nearly the same atomic masses, therefore the law was rejected.
e.g., atomic masses of Li, Na and K are respectively 7, 23 and 39, thus the mean of atomic masses of I St and 3rd element is
Limitations of Doberiner’s Triads: He could identify only a few such triads and so the law could not gain importance. In the triad ofFe, Co, Ni, all the three elements have a nearly equal atomic mass and thus does not follow the above law
4. Newland’s Law of Octaves:
According to this law “the elements are arranged in such a way that the eighth element starting from a given one has properties which are a repetition of those of the first if arranged in order of increasing atomic weight like the. eight note of musical scale.”
Drawback of Newland’s law of Octaves:
(i) According to Newland only 56 elements exists in nature and no more elements would be discovered in the future. But later on several new element were discovered
whose properties did not fit into law of octaves.
(ii) In order to fit new elements into his table Newland adjust two elements in the same column, but put some unlike elements under the same column.
Thus, Newland’s classification was not accepted.
Mendeleev’s Periodic Table :
Mendeleev arranged 63 elements known at that time in the periodic table. According to Mendeleev “the properties of the elements are a periodic function of their atomic masses.” The table consists of eight vertical column called ‘groups’ and horizontal rows called ‘periods’.
Merits of Mendeleev’s Periodic Table:
(i) At some places the order of atomic weight was changed in order to justify the chemical and physical nature.
(ii) Mendeleev left some gap for new elements which were not discovered at that time.
(iii) One of the strengths of Mendeleev’s periodic table was that, when inert gases were discovered they could be placed in a new group without disturbing the existing
order.
Characteristics of the periodic table : Its main characteristics are :
(i) In the periodic table, the elements are arranged in vertical rows called groups and horizontal rows called periods.
(ii) There are eight groups indicated by Roman Numerals I, II, III, IV, V, VI, VII, VIII. The elements belonging to first seven groups have been divided into sub-groups designated as A and B on the basis of similarities. The elements that are present on the left hand side in each group constitute sub-group A while those on the right hand side form sub-group B. Group VIII consists of nine elements arranged in three triads.
(iii) There are six periods (numbered 1, 2, 3, 4, 5 and 6). In order to accomodate more elements, the periods 4, 5, 6 are divided into two halves. The first half ofthe elements are placed in the upper left corners and the second half occupy lower right corners in each box.
Achievements of mendeleev’s periodic table
(i) The arrangement of elements in groups and periods made the study of elements quite systematic in the sense that if properties of one element in a particular group are known, those of the others can be easily predicted.
(ii) Prediction of new elements and their properties : Many gaps were left in this table for undiscovered elements. However, properties of these elements could be predicted in advance from their expected position. This helped in the discovery of these elements. The elements silicon, gallium and germanium were discovered in this manner.
(iii) Correction of doubtful atomic masses :
Mendeleev corrected the atomic masses of certain elements with the help of their expected positions and properties.
Limitations of mendeleev’s classification :
(i) He could not assign a correct position of hydrogen in his periodic table, as the properties of hydrogen resembles both with alkali metals as well as with halogens.
(ii) The isotopes of the same element will be given different position if atomic number is taken as basis, which will disturb the symmetry of the periodic table.
(iii) The atomic masses do not increases in a regular manner in going from one elements to the next.
So it was not possible to predict how many elements could be discovered between two elements.
6. Modern Periodic Law : This law was given by Henry Moseley in 1913. it states, “Properties of the elements are the periodic function of their atomic numbers”.
Cause of periodicity : Periodicity may be defined as the repetition of the similar properties of the elements placed in a group and separated by certain definite gap of atomic numbers.
The cause of periodicity is the resemblance in properties of the elements is the repetition of the same valence shell electronic configuration.
hope it helps
here's your answer
Lavoisier divided elements into two main types known as metals and non-metals.
3. Doberiner’s Law of Triads:
According to this law, “in certain triads (grout) of three elements) the atomic mass of the central element was the arithmetic mean of the atomic masses of the other two elements.” But in some triads all the threc elements possessed nearly the same atomic masses, therefore the law was rejected.
e.g., atomic masses of Li, Na and K are respectively 7, 23 and 39, thus the mean of atomic masses of I St and 3rd element is
Limitations of Doberiner’s Triads: He could identify only a few such triads and so the law could not gain importance. In the triad ofFe, Co, Ni, all the three elements have a nearly equal atomic mass and thus does not follow the above law
4. Newland’s Law of Octaves:
According to this law “the elements are arranged in such a way that the eighth element starting from a given one has properties which are a repetition of those of the first if arranged in order of increasing atomic weight like the. eight note of musical scale.”
Drawback of Newland’s law of Octaves:
(i) According to Newland only 56 elements exists in nature and no more elements would be discovered in the future. But later on several new element were discovered
whose properties did not fit into law of octaves.
(ii) In order to fit new elements into his table Newland adjust two elements in the same column, but put some unlike elements under the same column.
Thus, Newland’s classification was not accepted.
Mendeleev’s Periodic Table :
Mendeleev arranged 63 elements known at that time in the periodic table. According to Mendeleev “the properties of the elements are a periodic function of their atomic masses.” The table consists of eight vertical column called ‘groups’ and horizontal rows called ‘periods’.
Merits of Mendeleev’s Periodic Table:
(i) At some places the order of atomic weight was changed in order to justify the chemical and physical nature.
(ii) Mendeleev left some gap for new elements which were not discovered at that time.
(iii) One of the strengths of Mendeleev’s periodic table was that, when inert gases were discovered they could be placed in a new group without disturbing the existing
order.
Characteristics of the periodic table : Its main characteristics are :
(i) In the periodic table, the elements are arranged in vertical rows called groups and horizontal rows called periods.
(ii) There are eight groups indicated by Roman Numerals I, II, III, IV, V, VI, VII, VIII. The elements belonging to first seven groups have been divided into sub-groups designated as A and B on the basis of similarities. The elements that are present on the left hand side in each group constitute sub-group A while those on the right hand side form sub-group B. Group VIII consists of nine elements arranged in three triads.
(iii) There are six periods (numbered 1, 2, 3, 4, 5 and 6). In order to accomodate more elements, the periods 4, 5, 6 are divided into two halves. The first half ofthe elements are placed in the upper left corners and the second half occupy lower right corners in each box.
Achievements of mendeleev’s periodic table
(i) The arrangement of elements in groups and periods made the study of elements quite systematic in the sense that if properties of one element in a particular group are known, those of the others can be easily predicted.
(ii) Prediction of new elements and their properties : Many gaps were left in this table for undiscovered elements. However, properties of these elements could be predicted in advance from their expected position. This helped in the discovery of these elements. The elements silicon, gallium and germanium were discovered in this manner.
(iii) Correction of doubtful atomic masses :
Mendeleev corrected the atomic masses of certain elements with the help of their expected positions and properties.
Limitations of mendeleev’s classification :
(i) He could not assign a correct position of hydrogen in his periodic table, as the properties of hydrogen resembles both with alkali metals as well as with halogens.
(ii) The isotopes of the same element will be given different position if atomic number is taken as basis, which will disturb the symmetry of the periodic table.
(iii) The atomic masses do not increases in a regular manner in going from one elements to the next.
So it was not possible to predict how many elements could be discovered between two elements.
6. Modern Periodic Law : This law was given by Henry Moseley in 1913. it states, “Properties of the elements are the periodic function of their atomic numbers”.
Cause of periodicity : Periodicity may be defined as the repetition of the similar properties of the elements placed in a group and separated by certain definite gap of atomic numbers.
The cause of periodicity is the resemblance in properties of the elements is the repetition of the same valence shell electronic configuration.
hope it helps
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Periodic Classification in modern periodic table is based on atomic number of an element. Earlier, it was based on atomic mass of an element. There are 7 periods and 18 groups in Modern Periodic Table.
Periods are made such they have same number of shells throughout the period. Groups are made such that each of they possess similar characteristics.
The group 1 elements are called alkali metals.
The group 2 elements are called alkaline earth metals.
The group 3 to 12 are called transition elements.
The group 16 elements are called Chalcogens.
The group 17 elements are called Halogens.
The group 18 elements are called Inert or Nobel gases.
Group 1-2 are called s-block elements, since the last electrons enters in s-orbital.
Group 3-12 are called d-block elements, since the last electron enter in d-orbital.
Group 13-18 are called p-block elements, since the last electron enter in p-orbital.
The elements which are diagonally related to each other have similar properties. This is called diagonal relationship.
Periods are made such they have same number of shells throughout the period. Groups are made such that each of they possess similar characteristics.
The group 1 elements are called alkali metals.
The group 2 elements are called alkaline earth metals.
The group 3 to 12 are called transition elements.
The group 16 elements are called Chalcogens.
The group 17 elements are called Halogens.
The group 18 elements are called Inert or Nobel gases.
Group 1-2 are called s-block elements, since the last electrons enters in s-orbital.
Group 3-12 are called d-block elements, since the last electron enter in d-orbital.
Group 13-18 are called p-block elements, since the last electron enter in p-orbital.
The elements which are diagonally related to each other have similar properties. This is called diagonal relationship.
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