And I will discuss these below,
periodic table by electronegativity, periodic table with electronegativity, the periodic table of electronegativity, periodic table for electronegativity, periodic table electronegativity trend, periodic table electronegativity values, periodic table with charges And a periodic table with mass … So Read More Fully Carefully …
What is the Periodic Table?
The periodic table is an arrangement of all the elements known to man in accordance with their increasing atomic number and recurring chemical properties. They are assorted in a tabular arrangement wherein a row is a period and a column is a group.
PERIODIC TABLE OF ELEMENTS
Periodic table ( English: Periodic Table) is a system of representing chemical elements as a table with their corresponding characteristics.
In the periodic table, the chemical elements are decorated in increasing order of atomic number and the periodic, elementary group, Is classified into a secondary group.
The current periodic table contains 118 known elements. The first Russian chemist Mendeleev (correctly pronounced – Mendeleyev) introduced the periodic rule in 1869 and presented the elements as a table.
A few months later, the German scientist Lothar Meyer (1830–1895) also independently created the periodic table.
Alfred Werner created the current form of the periodic table from Mendeleyev’s table. In 1952, scientist Gil Chaverri of Costa Rica introduced a new form of the periodic table that was based on the electronic structure of elements.
The periodic table is very important and useful for chemists. Mozale created the modern Arvat table according to-
- The chemical and physical properties of the elements placed in the Arviat table are a recurring function of their atomic numbers.
- In the Arviat table, vertical lines are called groups and horizontal lines are called periods.
- Based on the electronic configurations of these elements, they are divided into four blocks.
- The last electrons of the elements of S Block are in the S subcellular.
- The last electrons of the elements of P Block are in the P subfamily.
- Similarly, the last electrons of the elements in the d and f blocks are in the subfields d and f. Elements of d and f blocks exhibit variable valency.
This modern Arvat table consists of seven horizontal rows known as Arviat. The numbers in the arvat represent the number of the outermost orbit of the element.
The Arvat table has 9 vertical fields called groups. Again 8 groups are divided into two subgroups. These are called A and B subgroups.
The last electron of an element in subgroup A is in the subfamily S or P. Elements of d and f blocks fall under subgroup B. All the 9 elements have been given suitable space by dividing the 8th group into 3 parts.
Thus the total number of groups is 16 which are as follows – IA, IIA, IIIB, IVB, VB, VIB, VIIB, VIIIB, IB, IIB, IIIA, IVA, VA, VIA, VIIA, Zero.
The periodic table is a table in which classification of elements into ordered groups and elements of similar properties are found at places corresponding to the horizontal or vertical sequence.
Apart from the unknown properties of known elements from this table, the properties of unknown elements can also be explained by looking at their position in the table.
History – In the same old countries as India, Arabia, and Yunnan, four or five elements were considered – Chiti-jal-pavak-Gagan-Samira (Tulsi), that is, earth, water, light, air, and sky. But Boyle (1627–91) gave a new definition of the elements, which helped chemists to understand chemical changes and reactions.
At the same time, Boyle also stated that the number of elements cannot be considered limited. As a result of this, new elements were soon discovered and by the end of the 18th century, the number of elements reached more than 60. Most of the elements were solid;
Some elements similar to bromine and mercury were also found to be liquid at ordinary heat and hydrogen, oxygen, etc. were in the gas state.
All these elements could also be divided into two classes of metals and non-metals, but some elements, such as bismuth and antimony, were difficult to say whether they were metals or non-metals.
The periodic table of the elements was created by Julius Tamsen and is given here in some revised form. Each column displays a period. Elements of the same property are related to lines.
As the chemists studied these elements more and more, it became clear that some elements were very similar to each other in properties, and they tried to classify them based on these similarities.
Atomic charges of these elements were also extracted at the same time as Dalton’s nuclear suit was presented. In 1820, Dobreiner noticed that elements of similar quality were found in groups of three called triads.
These triads were of two types – in the first type of triads, the atomic weights of the three elements were almost mutually equal, such as in iron (55.84), cobalt (58.94) and nickel (58.69) or in osmium (190.2), iridium (193.1) and platinum ( 195.25) in.
In the second type of triangles, the atomic weight of the middle element was the mean or average of the atomic bases of the first and third elements, such as chlorine (35.5),
Periodic Table Of Chemistry
A new attempt at classification of elements was made by Newlands around 1861. He started classifying the elements according to the order of the atomic mass.
He was surprised to see that when placed in the order of atomic weight, the properties of the elements increase gradually some inequalities, but after the seven elements, there comes the eighth element whose properties are very similar to the first element.
This was called the principle of the octave (Law of Octaves), as if the sound of the harmonium had a vowel sound in the form of a’ in a ‘g’, in which the frequency of the vowel after seven vowels. it occurs. The three lines of Newlands classification were of the following type:
Ha li bunl bo ka na au 1 7 9 11 12 14 16 fl so magni ai sif gan 19 23 24 27 28 31 32 Chloe po cai kro ty i lo 35.5 39 40 52 48 55 56
As the octave rule was further pursued, its success began to be doubted and the chemists were not satisfied with Newlands’ classification. In Newlands time, even around 1862, Dichacarto also tried to decorate elements like serpentines in order of atomic weight.
This effort also expressed that the order of atomic mass and the rotation of the properties of elements are related.
In 1869, the Russian chemist Mendeleev (Dmitry Einovich Mendelef) first declared the periodic rule in clear terms. He said that the physical and chemical properties of elements are the recurrence of their atoms.
The term period or frequency means to return or to come again and again. Everyone is introduced to the periodic numbers of arithmetic, such as 1 = .076923076923 … or .076923, ie, 076923. Similarly, if we decorate elements in the order of atomic weight, then again and again the elements of the same property will be found at the same places.
This is what we say in the language of mathematics that the properties of elements are periodic of atoms.
While Mendeleev was attempting this type of classification of elements in Russia, Lotharmeyer also (in 1870) expressed another way of the periodic rule.
He derived the atomic volumes of various elements, that is, by dividing the atoms of the elements by their densities, he drew a curve according to the atomic volume of the elements. By doing this, he got a periodic cycle and saw that elements of similar properties are at the same position on this curve.
Not all elements had been discovered by the time of Mendeleeff, yet Mendeleeff composed his periodic table so carefully that on the basis of it he predicted the properties of many unknown elements, now called scandium, gallium, and germanium.
The possible element he named Eka-boron was discovered in 1879 and was called Scandium. What he called Eka-aluminum was named Gallium in 1876, and Mendeleeff’s Eka-Silicon became known as Germanium when it was invented in 1876.
Mendleaf also modified the atomic bases of many elements on the basis of his periodic law, and later experiments confirmed Mendeleeff’s modifications.
Since the time of Mendeleeff, his periodic table underwent many changes and improvements. In 1913, Moseley stated that each element has a definite atomic number.
This atomic number is more important than the atomic mass, because the same element may belong to many different atoms, but the atomic number of the element is constant.
From Moseley’s time, the periodic law began to be expressed not by the expectation of the atomic mass, but rather by the expectation of the atomic number presented. It is now, not in the order of atoms.
There were sometimes faults in the classification to fit the sequence of atomic loads and Mendeleev was also aware of these defects.
He has neglected the order of atoms in his table at several places, such as tellurium to be the first of iodine, Although the atomic mass of tellurium is higher than iodine.
Similarly, by disregarding the order of atomic weight, nickel is placed after cobalt. These defects disappear when the atom is ordered.
Helium, neon, argon, krypton, etc. gases of the atmosphere were not known at the time of Mendeleev. When Ramze invented them and the chemists saw that the compounds of these elements did not form and were inert in that sense, they were placed in a separate group in the table.
It was named Zero Group. There should have been a group of zero electromagnets combining the groups of elements of electronegative and electronegative trends.
Mendeleev’s Periodic Table – Mendeleev’s Periodic Table has nine groups called the zero, first, second … the eighth group respectively. These groups also reflect the valencies of those elements. Each group has two subgroups — A and B.
There are ten lines from left to right, which is called Kaal. Actually the tenses are seven, but there are two categories in each of the fourth, fifth, and sixth periods. Thus, the total rows were ten. These seven periods are also evident in Lotharmeyer’s curve.
When the electron configuration of the atoms of the elements was discovered, the importance of the periodic law became even more pronounced. The atomic number of the elements also tells how many electrons are circulating in different elements in that element (dr. ‘Atom’).
The configuration of elements has many orbits and the number of electrons in these orbits or peripheries is also certain. These classes or peripheries can have maximum electrons of 2, 8, 18, 32, … respectively. At the same time, it is also a rule that no more than eight will remain on the outermost perimeter and no more than 18 electrons on the back.
This rule made it clear why some periods have 18 and some why 32 elements. It also expressed why vicious earth elements (atomic numbers 58 to 71 after lanthanum) could only be 14.
The periodic classification that Julius Tamsen gave according to the electron configuration is also important. This classification suggests that rotations occur at 2, 8, 18, 32, … atomic numbers (pictogram).
The atomic number of uranium is 92. The first element in the periodic classification is now considered to be a neutron, not hydrogen, whose atomic number is zero (0). 92 elements ranging from hydrogen to uranium are found in nature on the ground, not the rest; But now, by artificial means, even seven elements can be made after uranium – Neptunium (93), Plutonium (94), Americium (95), Curium (96), Berkelium (97), California (98), Einstium. (99), Shazam (100), etc. These are called actinides.
Just as there are 14 sparse earth elements after lanthanum (57), similarly 14 elements after actinium (89), which are not yet known, are not impossible. The existence of these new elements is completely compatible with the periodic law. 
The Russian chemist Mandlef arranged the known elements until his time (1869) as a table in the order of atoms growing. This is called the periodic table of the mandrel. The modern periodic table includes many elements found after mandrelif and the location of elements in this classification is based on their atomic number (d diagram).
The modern periodic table is sometimes called the bore table. Following are the main points of this table:
(1) It has 16 vertical fields called subclasses. The various subclasses are denoted by IA, IB, IIA, IIB … VIIA, VIIB, VIII and 0 numbers.
(2) Its horizontal mines are called periodic. The study of chemistry becomes very simple with the help of the periodic table. The study of 114 elements so far known as authentic turns into a study of only nine classes.
Since the properties of all the elements of a group are similar, one gets a simple knowledge of the properties of one element and the properties of the other elements of that group are also studied. Like, if you study the properties of Na, then the properties of other elements of subclass IA are studied equally.
Periodic Table Group Names
- Alkali metals (rarely ‘Hydrogen and the alkali metals’)
- Alkaline earth metals (in old chemistry this name applied only to Ca and its congeners)
- Icosagens (unofficial name; aka Boron group; rarely Earth metals)
- Crystallogens (unofficial name; aka Carbon group; rarely Adamantogens[a] or Merylides[b])
- Noble gases (rarely Aerogens). The Group name may have to be changed to the “Helium group” since oganesson is not expected to be noble.
Periodic Table Atomic Number
In the modern periodic table, the elements are listed in order of increasing atomic number. The atomic number is the number of protons in the nucleus of an atom.
The number of protons defines the identity of an element (i.e., an element with 6 protons is a carbon atom, no matter how many neutrons may be present). The number of protons determines how many electrons surround the nucleus, and it is the arrangement of these electrons that determines most of the chemical behavior of an element.
In a periodic table arranged in order of increasing atomic number, elements having similar chemical properties naturally line up in the same column (group).
For instance, all of the elements in Group 1A are relatively soft metals, react violently with water, and form 1+ charges; all of the elements in Group 8A are unreactive, monatomic gases at room temperature, etc. In other words, there is a periodic repetition of the properties of the chemical elements with increasing mass.
In the original periodic table published by Dimitri Mendeleev in 1869, the elements were arranged according to increasing atomic mass — at that time, the nucleus had not yet been discovered, and there was no understanding at all of the interior structure of the atom, so atomic mass was the only guide to use.
Once the structure of the nucleus was understood, it became clear that it was the atomic number that governed the properties of the elements.
The Elements, sorted by Atomic Number
Periodic Table With Names
Periodic Table Electron Configuration
Periodic Table Metals And Nonmetals
Periodic Table Atomic Radius
Atomic Mass Periodic Table
Given below is a table that lists the first 30 elements based on atomic number and their corresponding atomic mass.
|ATOMIC NUMBER||ELEMENT||ATOMIC MASS|
Periodic Table Of Chemistry And Periodic Table Atomic Radius…, Friends This Post End Here – If you have benefited from this post ( Periodic Table Of Chemistry ), Please let everyone see this post and stay with us.