THIS PRESENTATION IS BASED ON THE CONTRIBUTION OF DIFFERENT CHEMIST IN CREATING THE PERIODIC TABLE .IT WILL HELP THE LEARN THE VARIOUS MERITS AND DEMERITS OF VARIOUS METHODS OF CLASSIFYING ELEMENTS
Periodic classification of elements 10 CHM(5)VeenuGupta8
THIS PRESENTATION IS BASED ON THE PERIODIC CLASSIFICATION OF ELEMENTS AND THE VARIATION OF THE PERIODIC PROPERTIES IN THE PERIODIC TABLE.IT IS EASY TO GET KNOWLEDGE ABOUT THE PERIODIC PROPERTIES.
Periodic classification of elements 10 CHM(5)VeenuGupta8
THIS PRESENTATION IS BASED ON THE PERIODIC CLASSIFICATION OF ELEMENTS AND THE VARIATION OF THE PERIODIC PROPERTIES IN THE PERIODIC TABLE.IT IS EASY TO GET KNOWLEDGE ABOUT THE PERIODIC PROPERTIES.
The periodic table, also known as the periodic table of elements, is a tabular display of the chemical elements, which are arranged by atomic number, electron configuration, and recurring chemical properties. The structure of the table shows periodic trends.
Periodic Classification Of Elements Class 10thNehaRohtagi1
PowerPoint Presentation on the topic - 'Periodic Classification Of Elements'.
For Class:- 10th
Created By - 'Neha Rohtagi'.
I hope that you will found this presentation useful and it will help you out for your concept understanding.
Thank You!
Please give feedbacks and suggestions to get presentations on more interesting topics.
classification of elements and periodicity in properties class 11
classification of elements and periodicity in properties class 11 pdf classification of elements and periodicity in properties exercise classification of elements and periodicity in properties ncert classification of elements and periodicity in properties class 11 ppt classification of elements and periodicity in properties mind map what is periodic classification of elements classification of elements and periodicity in properties question answer classification of elements and periodicity in properties questions classification of elements and periodicity in properties in hindi chapter 3 classification of elements and periodicity in properties notes what is meant by periodic classification of elements classification of elements and periodicity in properties formulas classification of elements and periodicity in properties mcq pdf
Similar to Historical development of periodic table (20)
This presentation will help students to understand the concept of Alcohols ,Phenols and Ethers.It will help students to revise the chapter in a short time. It will also help the students preparing for various competitive exams based on the subject Chemistry.
Some Basic Concepts of Chemistry(CHAPTER-1)VeenuGupta8
This presentation will help students to understand the importance of chemistry in our daily life.It will help students to revise the chapter of class 11th chemistry in a short time. It will also the students preparing for various competitive exams based on the subject Chemistry.
This presentation will help students to understand the importance of chemistry in our daily life'It will students familiar with the role of chemistry and chemical products in our daily life.
This presentation will help students to understand the various topics related with halogen compounds in a very short time.it also help teachers during the recapitulation of the chapter content.it will also help students to revise the content in short time especially by those students who r preparing for various competitive exams after class 12th.
this presentation is based on the first chapter of chemistry dealing with class 10 .it contain all the necessary informations which are required for solving the HOTS and reasoning problems . this presentation can be used easily in the present teaching learning process. it can be easily accessible by anyone
Chemical reactions and equations 10 chm(1)VeenuGupta8
This presentation is based on the chapter 1 of chemistry .this presentation includes the basic informations related with the chemical Reactions and equations . it will help students and teachers in the teaching learning process
Chemical reactions and their characteristicsVeenuGupta8
This presentation is based on the chapter 1 of chemistry .this presentation includes the basic informations related with the chemical Reactions and their characteristics. it will help students and teachers in the teaching learning process.
This presentation is based on the chapter 1 of chemistry .this presentation includes the basic informations related with the chemical equations and their types. it will help students and teachers in the teaching learning process.
This presentation is based on the main topics dealing with chapter no 14.of chemistry.this chapter deals with the introduction ,classification,properties and functions of carbohydrates,proteins, Enzymes,vitamins,nucleic acids,lipid etc. this presentation will help students as well as teachers in the teaching learning process
This presentation is based on the main topics dealing with chapter no 14.of chemistry.this chapter deals with the introduction ,classification,properties and functions of carbohydrates,proteins, Enzymes,vitamins,nucleic acids,lipid etc. this presentation will help students as well as teachers in the teaching learning process
Acids , Bases & Salts (Some Important chemical compounds)VeenuGupta8
This presentation is based on the some important salts and their uses which are dealing with the syllabus of class 10 chemistry. this presentation will help the students and teachers during the teaching learning process. .It contains all the necessary informations about baking soda,baking powder,sodium hydroxide, POP,Gypsum,bleaching powder,water of crystallisation and hydrated salts
THIS PRESENTATION IS FOR THE STUDENTS STUDYING IN SENIOR CLASSES .IT WILL HELP THE CHILD TO RECALL THE CONTENT IN SHORT TIME IT WILL HELP TO BUILD THE STRONG AND CLEAR CONCEPT KNOWLEDGE.
THIS PRESENTATION IS FOR THE STUDENTS STUDYING IN SENIOR CLASSES .IT WILL HELP THE CHILD TO RECALL THE CONTENT IN SHORT TIME IT WILL HELP TO BUILD THE STRONG AND CLEAR CONCEPT KNOWLEDGE.
Determination of strength of acids and bases by using pH scaleVeenuGupta8
THIS PRESENTATION IS FOR THE STUDENTS STUDYING IN SENIOR CLASSES .IT WILL HELP THE CHILD TO RECALL THE CONTENT IN SHORT TIME IT WILL HELP TO BUILD THE STRONG AND CLEAR CONCEPT KNOWLEDGE.
THIS PRESENTATION IS FOR THE STUDENTS STUDYING IN SENIOR CLASSES .IT WILL HELP THE CHILD TO RECALL THE CONTENT IN SHORT TIME IT WILL HELP TO BUILD THE STRONG AND CLEAR CONCEPT KNOWLEDGE.
Operation “Blue Star” is the only event in the history of Independent India where the state went into war with its own people. Even after about 40 years it is not clear if it was culmination of states anger over people of the region, a political game of power or start of dictatorial chapter in the democratic setup.
The people of Punjab felt alienated from main stream due to denial of their just demands during a long democratic struggle since independence. As it happen all over the word, it led to militant struggle with great loss of lives of military, police and civilian personnel. Killing of Indira Gandhi and massacre of innocent Sikhs in Delhi and other India cities was also associated with this movement.
How to Create Map Views in the Odoo 17 ERPCeline George
The map views are useful for providing a geographical representation of data. They allow users to visualize and analyze the data in a more intuitive manner.
Ethnobotany and Ethnopharmacology:
Ethnobotany in herbal drug evaluation,
Impact of Ethnobotany in traditional medicine,
New development in herbals,
Bio-prospecting tools for drug discovery,
Role of Ethnopharmacology in drug evaluation,
Reverse Pharmacology.
The Roman Empire A Historical Colossus.pdfkaushalkr1407
The Roman Empire, a vast and enduring power, stands as one of history's most remarkable civilizations, leaving an indelible imprint on the world. It emerged from the Roman Republic, transitioning into an imperial powerhouse under the leadership of Augustus Caesar in 27 BCE. This transformation marked the beginning of an era defined by unprecedented territorial expansion, architectural marvels, and profound cultural influence.
The empire's roots lie in the city of Rome, founded, according to legend, by Romulus in 753 BCE. Over centuries, Rome evolved from a small settlement to a formidable republic, characterized by a complex political system with elected officials and checks on power. However, internal strife, class conflicts, and military ambitions paved the way for the end of the Republic. Julius Caesar’s dictatorship and subsequent assassination in 44 BCE created a power vacuum, leading to a civil war. Octavian, later Augustus, emerged victorious, heralding the Roman Empire’s birth.
Under Augustus, the empire experienced the Pax Romana, a 200-year period of relative peace and stability. Augustus reformed the military, established efficient administrative systems, and initiated grand construction projects. The empire's borders expanded, encompassing territories from Britain to Egypt and from Spain to the Euphrates. Roman legions, renowned for their discipline and engineering prowess, secured and maintained these vast territories, building roads, fortifications, and cities that facilitated control and integration.
The Roman Empire’s society was hierarchical, with a rigid class system. At the top were the patricians, wealthy elites who held significant political power. Below them were the plebeians, free citizens with limited political influence, and the vast numbers of slaves who formed the backbone of the economy. The family unit was central, governed by the paterfamilias, the male head who held absolute authority.
Culturally, the Romans were eclectic, absorbing and adapting elements from the civilizations they encountered, particularly the Greeks. Roman art, literature, and philosophy reflected this synthesis, creating a rich cultural tapestry. Latin, the Roman language, became the lingua franca of the Western world, influencing numerous modern languages.
Roman architecture and engineering achievements were monumental. They perfected the arch, vault, and dome, constructing enduring structures like the Colosseum, Pantheon, and aqueducts. These engineering marvels not only showcased Roman ingenuity but also served practical purposes, from public entertainment to water supply.
Students, digital devices and success - Andreas Schleicher - 27 May 2024..pptxEduSkills OECD
Andreas Schleicher presents at the OECD webinar ‘Digital devices in schools: detrimental distraction or secret to success?’ on 27 May 2024. The presentation was based on findings from PISA 2022 results and the webinar helped launch the PISA in Focus ‘Managing screen time: How to protect and equip students against distraction’ https://www.oecd-ilibrary.org/education/managing-screen-time_7c225af4-en and the OECD Education Policy Perspective ‘Students, digital devices and success’ can be found here - https://oe.cd/il/5yV
The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
For more information, visit-www.vavaclasses.com
2. “The periodic table is a tabular
method of displaying the
elements in such a way, that the
elements having similar
properties occur in the same
vertical column or group”.
3. Increase in the discovery of different
elements made it difficult to organise all that
was known about the elements.
To study a large number of elements with
ease, various attempts were made. The
attempts resulted in the classification of
elements into metals and non-metals.
5. Johann Wolfgang Dobereiner, a German chemist, classified
the known elements in groups of three elements on the basis
of similarities in their properties. These groups were called
triads.This classification is based on the atomic mass.
According to this, when elements are arranged in order of
increasing atomic masses, groups of three elements, having
similar properties are obtained. The atomic mass of middle
element of the triad being nearly equal to the average of the
atomic masses of the other two elements.
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 equal to the average of the atomic masses of the
other two elements.
6. Element Atomi
c
mass
Element Atomic
mass
Element Atomic
mass
Lithium(Li) 6.9 Calcium (Ca) 40.1 Chlorine(Cl) 35.5
Sodium(Na) 23 Strontium(Sr) 87.6 Bromine (Br) 79.9
Potassium (K) 39 Barium(Ba) 137.3 Iodine (I) 126.9
7. It fails to arrange all the known elements in the
form of triads, even having similar properties.
He could identify only a few such triads and
so the law could not gain importance.
In the triad of Fe, Co, Ni, all the three elements
have a nearly equal atomic mass and thus does not
follow the above law
9. ‘John Newlands’, an English scientist, arranged the
known elements in the order of increasing atomic
masses and called it the ‘Law of Octaves’. It is known
as ‘Newlands’ Law of Octaves’.
According to this law “when elements are placed in
order of increasing atomic masses, the physical and
chemical properties of every 8th element are a
repetition of the properties of the first element
weight like the eight note of musical scale.”
10. It contained the elements from hydrogen to thorium.
Properties of every eighth element were similar to that of the first element.
Seeing the word octave applied to this table may lead one to think that Newlands
recognised periods of eight elements with repeating properties, as we do with the modern
periodic table, for example: Li Be B C N O F Ne.
However, each sequence of Newlands' octaves contain only seven elements. Count the
elements in the columns! In Newlands' day the group 8 (18) rare gas elements, He, Ne, Ar,
Kr & Xe, had not yet been discovered.
To Newlands, H to F & F to Cl are octaves of eight elements, the eighth element repeating
the properties of the first.
There are seven notes in a musical octave: A B C D E F G, after which you start again with
A'; similarly for Newlands, seven elements H Li G Bo C N O, then the 8th is F and you start
again. [Note that Newlands treated H as a halogen.]
12. sa
(do)
H 1 F 8 Cl 15 Co &
Ni 22
Br 29 Pd 36 I 42 Pt & Ir
50
re
(re)
Li 2 Na 9 K 16 Cu 23 Rb 30 Ag 37 Cs 44 Os 51
ga
(mi)
Be 3 Mg 10 Ca 17 Zn 24 Sr 31 Cd 38 Ba & V
45
Hg 52
ma
(fa)
B 4 Al 11 Cr 19 Y 25 Ce & La
33
U 40 Ta 46 Tl 53
pa
(so)
C 5 Si 12 Ti 18 In 26 Zr 32 Sn 39 W 47 Pb 54
da
(la)
N 6 P 13 Mn 20 As 27 Di & Mo
34
Sb 41 Nb 48 Bi 55
ni
(ti)
O 7 S 14 Fe 21 Se 28 Ro & Ru
35
Te 43 Au 49 Th 56
13. This classification worked well for lighter
elements only up to Ca.
This classification gave us a relation between
the properties of the elements and their
atomic masses.
It was shown by this classification for the first
time that there exists a periodicity in the
properties of the elements.
14. Law of octaves was applicable only upto calcium (only
for lighter elements). After calcium every eighth
element did not possess the properties similar to that
of the first element.
This classification failed when the heavier elements
beyond Ca were arranged according to Newland’s law
of octaves.
Newlands assumed that only 56 elements existed 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.
15. (iv) At the time of this law, noble gases were unknown. When
noble gases were discovered, neon (Ne) between F and Na, and
argon (Ar) between Cl and K, it becomes the ninth element and
not the eighth which has the similar properties.
v) In order to fit elements into his table, Newlands put even two
elements together in one slot and that too in the column of unlike
elements having very different properties.
For example, the two elements cobalt (Co) and nickel (Ni) were
put together in just one slot and that too in the column of
elements like fluorine, chlorine and bromine which have very
different properties from these elements.
(vi) Iron (Fe) element which resemble elements like cobalt and
nickel in properties, was placed far away from these elements.
Thus, Newland‟s classification was not accepted.
17. He was one of the pioneers in developing the first periodic
table of chemical elements. Both Mendeleev and Meyer worked
with Robert Bunsen. He never used his first given name, and was
known throughout his life simply as Lothar Meyer.
Meyer is best known for his part in the periodic classification of
the elements. He noted, as J. A. R. Newlands did in England, if
each element is arranged in the order of their atomic weights,
they fall into groups of similar chemical and physical properties
repeated at periodic intervals.
According to him, if the atomic weights were plotted as ordinates
and the atomic volumes as abscissae—the curve obtained a series
of maxima and minima—the most electro-positive elements
appearing at the peaks of the curve in the order of their atomic
weights
18. I II III IV V VI VII VIII IX
B Al In(?) Tl
C Si
Ti Zr
Sn Pb
N P
V
As
Nb
Sb
Ta
Bi
O S
Cr
Se
Mo
Те
W
F Cl
Mn
Fe
Co
Ni
Br
Ru
Rh
Pd
I
Os
Ir
Pt
Li Na K
Cu
Rb
Ag
Cs
Au
Be Mg Ca
Zn
Sr
Cd
Ba
19. According to this “The physical
and chemical properties of the
elements are the periodic
function of their atomic masses.”
20. The repetition of properties
of elements after certain
regular intervals is known
as Periodicity of Properties.
22. Dmitri Ivanovich – 5 ’ Mendeleev, a Russian
demist, was the most important contributor
to the early development of a periodic table
of elements wherein the elements were
arranged on the basis of their atomic mass
and chemical properties.
23. 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 elements with similar physical and
chemical properties came under the same groups.
In the periodic table, the elements are arranged in vertical rows called
groups and horizontal rows called periods.
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.
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
of the elements are placed in the upper left corners and the second half
occupy lower right corners in each box.
24. Systematic Study Of Elements: 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.
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.
Correction of doubtful atomic masses : Mendeleev corrected the
atomic masses of certain elements with the help of their expected
positions and properties.
25. 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.
No place could be assigned to isotopes of an element.
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.
The atomic masses do not increases in a regular manner in going from
one elements to the next.
The properties of elements are periodic functions of their atomic mass.
It has 8 groups.
Elements with same properties are placed in different groups like
platinum and Gold
There were three gaps left by Mendeleev in his Periodic Table.
No distinction was made between metals and non-metals.
Transition elements are placed together in Group VIII.
Inert gases were not known at the time of Mendeleev
27. Moseley's experiments in X-ray spectroscopy showed directly
from their physics that cobalt and nickel have the different
atomic numbers, 27 and 28, and that they are placed in the
Periodic Table correctly by Moseley's objective measurements
of their atomic numbers. Using atomic number instead
of atomic mass as the organizing principle was first proposed
by the British chemist Henry Moseley in 1913, and it solved
anomalies like this one. Iodine has a higher atomic number
than tellurium - so, even though he didn't know
why, Mendeleev was right to place it after tellurium after all!
28. When World War I broke out in Western Europe, Moseley left his
research work at the University of Oxford behind to volunteer for the
Royal Engineers of the British Army. Moseley was assigned to the force
of British Empire soldiers that invaded the region of Gallipoli, Turkey, in
April 1915, as a telecommunications officer. Moseley was shot and killed
during the Battle of Gallipoli on 10 August 1915, at the age of 27. Experts
have speculated that Moseley could have been awarded the Nobel Prize
in Physics in 1916, if he had not been killed. As a consequence, the
British government instituted new policies for eligibility for combat duty.
29. This law was given by Henry Moseley in
1913. It states, “The physical and
chemical properties of the elements are
the periodic function of their atomic
numbers”.
Modern periodic table is based on
atomic number of elements.
30. 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
31. Moseley proposed this modern periodic table and according to which
“the physical and chemical properties of elements are periodic
function of their atomic number and not atomic mass.“
Group: The vertical columns in Mendeleev’s, as well as in Modern
Periodic Table, are called groups.
Period: The horizontal rows in the Modern Periodic Table and
Mendeleev’s Periodic Table are called periods.
There are 18 groups and 7 (seven) periods in the Modern Periodic
Table.
The elements belonging to a particular group make a family and
usually named after the first member. In a group all the elements
contain the same number of valence electrons.
In a period all the elements contain the same number of shells, but
as we move from left to right the number of valence shell electrons
increases by one unit. The maximum number of electrons that can be
accommodated in a shell can be calculated by the formula 2n2 where
n is the number of the given shell from the nucleus.
32.
33. Name of the
Element
Symbol of
the Element
Atomic
Number
Name of the
Element
Symbol of
the Element
Atomic
Number
Hydrogen H 1 Aluminium Al 13
Helium He 2 Silicon Si 14
Lithium Li 3 Phosphorus P 15
Beryllium Be 4 Sulfur S 16
Boron B 5 Chlorine Cl 17
Carbon C 6 Argon Ar 18
Nitrogen N 7 Potassium K 19
Oxygen O 8 Calcium Ca 20
Fluorine F 9 Scandium Sc 21
Neon Ne 10 Titanium Ti 22
Sodium Na 11 Vanadium V 23
Magnesium Mg 12 Chromium Cr 24
34. Name of
the Element
Symbol of
the Element
Atomic
Number
Name of
the Element
Symbol of
the Element
Atomic
Number
Manganese Mn 25 Strontium Sr 38
Iron Fe 26 Yttrium Y 39
Cobalt Co 27 Zirconium Zr 40
Nickel Ni 28 Niobium Nb 41
Copper Cu 29 Molybdenum Mo 42
Zinc Zn 30 Technetium Tc 43
Gallium Ga 31 Ruthenium Ru 44
Germanium Ge 32 Rhodium Rh 45
Arsenic As 33 Palladium Pd 46
Selenium Se 34 Silver Ag 47
Bromine Br 35 Cadmium Cd 48
Krypton Kr 36 Indium In 49
Rubidium Rb 37 Tin Sn 50
35. Name of the
Element
Symbol of
the Element
Atomic
Number
Name of the
Element
Symbol of
the Element
Atomic
Number
Antimony Sb 51 Gadolinium Gd 64
Tellurium Te 52 Terbium Tb 65
Iodine I 53 Dysprosium Dy 66
Xenon Xe 54 Holmium Ho 67
Cesium Cs 55 Erbium Er 68
Barium Ba 56 Thulium Tm 69
Lanthanum La 57 Ytterbium Yb 70
Cerium Ce 58 Lutetium Lu 71
Praseodymium Pr 59 Hafnium Hf 72
Neodymium Nd 60 Tantalum Ta 73
Promethium Pm 61 Tungsten W 74
Samarium Sm 62 Rhenium Re 75
Europium Eu 63 Osmium Os 76
36. Name of
the Element
Symbol of
the Element
Atomic
Number
Name of
the Element
Symbol of
the Element
Atomic
Number
Iridium Ir 77 Actinium Ac 89
Platinum Pt 78 Thorium Th 90
Gold Au 79 Protactinium Pa 91
Mercury Hg 80 Uranium U 92
Thallium Tl 81 Neptunium Np 93
Lead Pb 82 Plutonium Pu 94
Bismuth Bi 83 Americium Am 95
Polonium Po 84 Curium Cm 96
Astatine At 85 Berkelium Bk 97
Radon Rn 86 Californium Cf 98
Francium Fr 87 Einsteinium Es 99
Radium Ra 88 Fermium Fm 100
37. Name of the
Element
Symbol of
the Element
Atomic
Number
Name of the
Element
Symbol of
the Element
Atomic
Number
Mendelevium Md 101 Darmstadtium Ds 110
Nobelium No 102 Roentgenium Rg 111
Lawrencium Lr 103 Copernicium Cn 112
Rutherfordium Rf 104 Nihonium Nh 113
Dubnium Db 105 Flerovium Fl 114
Seaborgium Sg 106 Moscovium Mc 115
Bohrium Bh 107 Livermorium Lv 116
Hassium Hs 108 Tennessine Ts 117
Meitnerium Mt 109 Oganesson Og 118