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Periodic Table Of Chemistry And Periodic Table Atomic Radius

Hey Chemistry Lovers,  Today I Will Show You, Periodic Table Of Chemistry, Periodic Table Atomic Radius, Periodic Table Group Names, Periodic Table With Names, the atomic mass periodic table, periodic table electronegativity

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.
  1. The last electrons of the elements of S Block are in the S subcellular.
  2. The last electrons of the elements of P Block are in the P subfamily.
  3. 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. [1]

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

  1. Alkali metals (rarely ‘Hydrogen and the alkali metals’)
  2. Alkaline earth metals (in old chemistry this name applied only to Ca and its congeners)
  3. Icosagens (unofficial name; aka Boron group; rarely Earth metals)
  4. Crystallogens (unofficial name; aka Carbon group; rarely Adamantogens[a] or Merylides[b])
  5. Pnictogens
  6. Chalcogens
  7. Halogens
  8. 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

 

Atomic
Number
SymbolNameAtomic Mass
(amu, g/mol)
1HHydrogen1.00797
2HeHelium4.00260
3LiLithium6.941
4BeBeryllium9.01218
5BBoron10.81
6CCarbon12.011
7NNitrogen14.0067
8OOxygen15.9994
9FFluorine18.998403
10NeNeon20.179
11NaSodium22.98977
12MgMagnesium24.305
13AlAluminum26.98154
14SiSilicon28.0855
15PPhosphorus30.97376
16SSulfur32.06
17ClChlorine35.453
18ArArgon39.948
19KPotassium39.0983
20CaCalcium40.08
21ScScandium44.9559
22TiTitanium47.90
23VVanadium50.9415
24CrChromium51.996
25MnManganese54.9380
26FeIron55.847
27CoCobalt58.9332
28NiNickel58.70
29CuCopper63.546
30ZnZinc65.38
31GaGallium69.72
32GeGermanium72.59
33AsArsenic74.9216
34SeSelenium78.96
35BrBromine79.904
36KrKrypton83.80
37RbRubidium85.4678
38SrStrontium87.62
39YYttrium88.9059
40ZrZirconium91.22
41NbNiobium92.9064
42MoMolybdenum95.94
43TcTechnetium(98)
44RuRuthenium101.07
45RhRhodium102.9055
46PdPalladium106.4
47AgSilver107.868
48CdCadmium112.41
49InIndium114.82
50SnTin118.69
51SbAntimony121.75
52TeTellurium127.60
53IIodine126.9045
54XeXenon131.30
55CsCesium132.9054
56BaBarium137.33
57LaLanthanum138.9055
58CeCerium140.12
59PrPraseodymium140.9077
60NdNeodymium144.24
61PmPromethium(145)
62SmSamarium150.4
63EuEuropium151.96
64GdGadolinium157.25
65TbTerbium158.9254
66DyDysprosium162.50
67HoHolmium164.9304
68ErErbium167.26
69TmThulium168.9342
70YbYtterbium173.04
71LuLutetium174.967
72HfHafnium178.49
73TaTantalum180.9479
74WTungsten183.85
75ReRhenium186.207
76OsOsmium190.2
77IrIridium192.22
78PtPlatinum195.09
79AuGold196.9665
80HgMercury200.59
81TlThallium204.37
82PbLead207.2
83BiBismuth208.9804
84PoPolonium(209)
85AtAstatine(210)
86RnRadon(222)
87FrFrancium(223)
88RaRadium226.0254
89AcActinium227.0278
90ThThorium232.0381
91PaProtactinium231.0359
92UUranium238.029
93NpNeptunium237.0482
94PuPlutonium(242)
95AmAmericium(243)
96CmCurium(247)
97BkBerkelium(247)
98CfCalifornium(251)
99EsEinsteinium(252)
100FmFermium(257)
101MdMendelevium(258)
102NoNobelium(250)
103LrLawrencium(260)
104RfRutherfordium(261)
105DbDubnium(262)
106SgSeaborgium(263)
107BhBohrium(262)
108HsHassium(255)
109MtMeitnerium(256)
110DsDarmstadtium(269)
111RgRoentgenium(272)
112UubUnunbiium(277)
113—————
114UuqUnunquadium

 

Periodic Table With Names

Name With Periodic Table – 118 Elements Of Periodic Table:
Element 1: H-Hydrogen
Element 2: He-Helium
Element 3: Li-Lithium
Element 4: Be-Beryllium
Element 5: B-Boron
Element 6: C-Carbon
Element 7: N-Nitrogen
Element 8: O-Oxygen
Element 9: F-Fluorine
Element 10: Ne-Neon
Element 11: Na-Sodium
Element 12: Mg-Magnesium
Element 13 : Al-Aluminum
Element 14 : Si-Silicon
Element 15 : P-Phosphorus
Element 16 : S-Sulfur
Element 17 : Cl-Chlorine
Element 18 : Ar-Argon
Element 19 : K-Potassium
Element 20 : Ca-Calcium
Element 21 : Sc-Scandium
Element 22 : Ti-Titanium
Element 23 : V-Vanadium
Element 24 : Cr-Chromium
Element 25 : Mn-Manganese
Element 26 : Fe-Iron
Element 27 : Co-Cobalt
Element 28 : Ni-Nickel
Element 29 : Cu-Copper
Element 30 : Zn-Zinc
Element 31 : Ga-Gallium
Element 32 : Ge-Germanium
Element 33 : As-Arsenic
Element 34 : Se-Selenium
Element 35 : Br-Bromine
Element 36 : Kr-Krypton
Element 37 : Rb-Rubidium
Element 38 : Sr-Strontium
Element 39 : Y-Yttrium
Element 40 : Zr-Zirconium
Element 41 : Nb-Niobium
Element 42 : Mo-Molybdenum
Element 43 : Tc-Technetium
Element 44 : Ru-Ruthenium
Element 45 : Rh-Rhodium
Element 46 : Pd-Palladium
Element 47 : Ag-Silver
Element 48 : Cd-Cadmium
Element 49 : In-Indium
Element 50 : Sn-Tin
Element 51 : Sb-Antimony
Element 52 : Te-Tellurium
Element 53 : I-Iodine
Element 54 : Xe-Xenon
Element 55 : Cs-Cesium
Element 56 : Ba-Barium
Element 57 : La-Lanthanum
Element 58 : Ce-Cerium
Element 59 : Pr-Praseodymium
Element 60 : Nd-Neodymium
Element 61 : Pm-Promethium
Element 62 : Sm-Samarium
Element 63 : Eu-Europium
Element 64 : Gd-Gadolinium
Element 65 : Tb-Terbium
Element 66 : Dy-Dysprosium
Element 67 : Ho-Holmium
Element 68 : Er-Erbium
Element 69 : Tm-Thulium
Element 70 : Yb-Ytterbium
Element 71 : Lu-Lutetium
Element 72 : Hf-Hafnium
Element 73 : Ta-Tantalum
Element 74 : W-Tungsten
Element 75 : Re-Rhenium
Element 76 : Os-Osmium
Element 77 : Ir-Iridium
Element 78 : Pt-Platinum
Element 79 : Au-Gold
Element 80 : Hg-Mercury
Element 81 : Tl-Thallium
Element 82 : Pb-Lead
Element 83 : Bi-Bismuth
Element 84 : Po-Polonium
Element 85 : At-Astatine
Element 86 : Rn-Radon
Element 87 : Fr-Francium
Element 88 : Ra-Radium
Element 89 : Ac-Actinium
Element 90 : Th-Thorium
Element 91 : Pa-Protactinium
Element 92 : U-Uranium
Element 93 : Np-Neptunium
Element 94 : Pu-Plutonium
Element 95 : Am-Americium
Element 96 : Cm-Curium
Element 97 : Bk-Berkelium
Element 98 : Cf-Californium
Element 99 : Es-Ensteinium
Element 100 : Fm-Fermium
Element 101 : Md-Mendelevium
Element 102 : No-Nobelium
Element 103 : Lr-Lawrencium
Element 104 : Rf-Rutherfordium
Element 105 : Db-Dubnium
Element 106 : Sg-Seaborgium
Element 107 : Bh-Bohrium
Element 108 : Hs-Hassium
Element 109 : Mt-Meitnerium
Element 110 : Ds-Darmstadtium
Element 111 : Rg-Roentgenium
Element 112 : Cn-Copernicium
Element 113 : Nh-Nihonium
Element 114 : Fl-Flerovium
Element 115 : Mc-Moscovium
Element 116 : Lv-Livermorium
Element 117 : Ts-Tennessine
Element 118 : Og-Oganesson

Periodic Table Electron Configuration

periodic table electron configuration
Source – Google

Periodic Table Metals And Nonmetals

periodic table metals and nonmetals
Source – Google

Periodic Table Atomic Radius

periodic table atomic radius
Source – Google

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 NUMBERELEMENTATOMIC MASS
1Hydrogen1.008
2Helium4.0026
3Lithium6.94
4Beryllium9.0122
5Boron10.81
6Carbon12.011
7Nitrogen14.007
8Oxygen15.999
9Fluorine18.998
10Neon20.180
11Sodium22.990
12Magnesium24.305
13Aluminium26.982
14Silicon28.085
15Phosphorus30.974
16Sulfur32.06
17Chlorine35.45
18Argon39.948
19Potassium39.098
20Calcium40.078
21Scandium44.956
22Titanium47.867
23Vanadium50.942
24Chromium51.996
25Manganese54.938
26Iron55.845
27Cobalt58.933
28Nickel58.693
29Copper63.546
30Zinc65.38
Periodic Table Electronegativity
Periodic Table Electronegativity
Periodic Table Electronegativity
Periodic Table Of Chemistry Last Quote:

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