This document discusses the classification and periodic trends of chemical elements. It begins with early classification systems developed by Döbereiner, Newlands, and Lother-Meyer. It then covers Mendeleev's periodic table and its strengths and limitations. The modern periodic table is based on Henry Moseley's discovery that atomic number, not atomic mass, is fundamental. The document outlines the key features and groups of the long form periodic table. It concludes by examining periodic trends in physical and chemical properties, including ionization energy, atomic radius, and oxidation states.
Classification of elements periodicity properties IUPAC names 100 to 118SURI BABU JOGA
This document discusses the classification of elements and periodic trends in their physical and chemical properties. It begins with an overview of how elements have historically been classified from Dobereiner's triads to Mendeleev's periodic table. Key periodic properties discussed include atomic radius, ionization energy, and electronegativity. Periodic trends in these properties are explained in terms of the periodic variation in the effective nuclear charge experienced by outer shell electrons due to shielding effects. Chemical properties also vary periodically, including oxidation states and reactivity. The document aims to explain these periodic trends using concepts of electronic configuration.
This document discusses the classification and periodic trends of chemical elements. It begins by outlining early classification systems developed by Dobereiner, Newlands, Meyer and Mendeleev that organized elements by their increasing atomic masses and recognized periodic trends in their properties. Mendeleev organized the elements into the first periodic table. Later, Moseley determined that atomic number, not atomic mass, was fundamental in organizing elements. This led to the modern periodic table arranged by increasing atomic number. The document then discusses the organization and features of the long form periodic table, including grouping elements by their electronic configurations and periodic trends in physical and chemical properties.
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIESniralipatil
The document discusses the classification of elements and the development of the periodic table over time. It describes early attempts at classification by Dobereiner, Newlands, and Mendeleev. Mendeleev organized the elements into the first periodic table based on increasing atomic mass. Later, Moseley established the modern periodic table based on increasing atomic number. The document outlines the structural features and characteristics of the main blocks (s, p, d, f) of the periodic table. It also defines atomic properties like atomic radius, covalent radius, and metallic radius, and how they vary within the periodic table.
Mendeleev arranged elements in increasing order of atomic mass and placed those with similar properties in the same group, forming the first periodic table. This allowed for accurate prediction of undiscovered elements and correction of atomic masses. The modern periodic table is arranged by atomic number, with elements in periods by electron shell and groups by valence electrons. Trends across periods include decreasing atomic size and metallic character from left to right as nuclear charge increases, while trends down groups include increasing size and metallic character as shells are added.
This document discusses the periodic table and classification of elements. It explains that elements are arranged in the periodic table in order of increasing atomic number. The table is divided into blocks based on the subshell where electrons are located (s, p, d, f blocks). Elements are also classified into groups based on their physical and chemical properties. The modern periodic table improved upon earlier versions by being based on the fundamental property of atomic number, better correlating an element's position with its electronic configuration.
Commonly know as The Copper State, Arizona is the largest copper producing state in the United States. The copper-colored star in the center of its flag symbolizes the metal’s importance to the state.
The document discusses the periodic table and periodic trends in properties of elements. It defines key periodic table terms like groups, periods, atomic radius, ionization energy, and provides examples of how properties change within periods and groups. It also discusses Mendeleev's original periodic table and the modern periodic law.
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
Classification of elements periodicity properties IUPAC names 100 to 118SURI BABU JOGA
This document discusses the classification of elements and periodic trends in their physical and chemical properties. It begins with an overview of how elements have historically been classified from Dobereiner's triads to Mendeleev's periodic table. Key periodic properties discussed include atomic radius, ionization energy, and electronegativity. Periodic trends in these properties are explained in terms of the periodic variation in the effective nuclear charge experienced by outer shell electrons due to shielding effects. Chemical properties also vary periodically, including oxidation states and reactivity. The document aims to explain these periodic trends using concepts of electronic configuration.
This document discusses the classification and periodic trends of chemical elements. It begins by outlining early classification systems developed by Dobereiner, Newlands, Meyer and Mendeleev that organized elements by their increasing atomic masses and recognized periodic trends in their properties. Mendeleev organized the elements into the first periodic table. Later, Moseley determined that atomic number, not atomic mass, was fundamental in organizing elements. This led to the modern periodic table arranged by increasing atomic number. The document then discusses the organization and features of the long form periodic table, including grouping elements by their electronic configurations and periodic trends in physical and chemical properties.
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIESniralipatil
The document discusses the classification of elements and the development of the periodic table over time. It describes early attempts at classification by Dobereiner, Newlands, and Mendeleev. Mendeleev organized the elements into the first periodic table based on increasing atomic mass. Later, Moseley established the modern periodic table based on increasing atomic number. The document outlines the structural features and characteristics of the main blocks (s, p, d, f) of the periodic table. It also defines atomic properties like atomic radius, covalent radius, and metallic radius, and how they vary within the periodic table.
Mendeleev arranged elements in increasing order of atomic mass and placed those with similar properties in the same group, forming the first periodic table. This allowed for accurate prediction of undiscovered elements and correction of atomic masses. The modern periodic table is arranged by atomic number, with elements in periods by electron shell and groups by valence electrons. Trends across periods include decreasing atomic size and metallic character from left to right as nuclear charge increases, while trends down groups include increasing size and metallic character as shells are added.
This document discusses the periodic table and classification of elements. It explains that elements are arranged in the periodic table in order of increasing atomic number. The table is divided into blocks based on the subshell where electrons are located (s, p, d, f blocks). Elements are also classified into groups based on their physical and chemical properties. The modern periodic table improved upon earlier versions by being based on the fundamental property of atomic number, better correlating an element's position with its electronic configuration.
Commonly know as The Copper State, Arizona is the largest copper producing state in the United States. The copper-colored star in the center of its flag symbolizes the metal’s importance to the state.
The document discusses the periodic table and periodic trends in properties of elements. It defines key periodic table terms like groups, periods, atomic radius, ionization energy, and provides examples of how properties change within periods and groups. It also discusses Mendeleev's original periodic table and the modern periodic law.
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
Periodic Table (Classification of elements) MANIKImran Nur Manik
Electronic structure of atoms, modern periodic table and periodic law, variation of periodic properties within periods and groups, ionization potential, electron affinity, electronegativity, usefulness and limitation of periodic table.
The periodic table is arranged based on atomic number and properties repeat periodically. Early forms grouped elements based on atomic mass but Moseley found atomic number was key. The table is divided into periods and groups with trends in properties like atomic size decreasing left to right across periods and ionization energy increasing. Metallic character increases down groups and nonmetallic character increases right across periods. The periodic table organizes the elements and allows prediction of properties.
During the 19th century, chemists began categorizing elements based on their properties, leading to modern periodic tables. Johann Dobereiner observed that some elements formed triads with similar properties. John Newlands proposed an early periodic law in which properties repeated every eighth element, though this failed with new discoveries. Dmitri Mendeleev and Lothar Meyer independently created early periodic tables arranging elements by atomic mass, with Mendeleev accurately predicting unknown elements. Henry Moseley determined elements' ordering by atomic number, establishing the modern periodic table.
1. The document provides a summary of the periodic classification of elements, including the theories of Dobereiner, Newlands, and Mendeleev, and the modern periodic law.
2. It describes the achievements and limitations of their classifications, and how the modern periodic table addresses the limitations by arranging elements by atomic number instead of atomic mass.
3. The document also summarizes key trends in the modern periodic table such as how properties change from period to period and group to group.
This document discusses the development of the periodic table from early classification attempts to the modern periodic table. It describes Dobereiner's discovery of triads of elements with similar properties in the 1810s. It then discusses Newlands' law of octaves from the 1860s which noted patterns every eighth element. Mendeleev developed the first periodic table in 1869, arranging elements by atomic mass and leaving gaps for undiscovered elements. The modern periodic table is arranged by atomic number instead of mass and helped resolve limitations of earlier classifications. It describes trends in properties like valency and size across periods and groups in the modern periodic table.
The document discusses the history and development of the periodic table. It describes early classification systems developed by Dobereiner, Newlands, and Mendeleev. Mendeleev arranged elements in order of atomic mass and left gaps for undiscovered elements, correctly predicting their properties. The modern periodic table is arranged by atomic number instead of mass. The 7th period is now complete with the discovery of elements 113, 115, 117, and 118 as announced by IUPAC. The periodic table is divided into periods and groups based on electron configuration and properties repeat periodically.
This document contains the scheme of work and lesson plans for teaching chemistry to SS2 students. It covers topics on the periodic table over two weeks, including properties of elements, groups and periods. It then covers chemical reactions over one week, discussing concepts like reactants and products, and factors that affect reaction rates such as concentration, temperature, and catalysts. The lessons include content, examples, evaluations, and assignments.
The document discusses the history and development of the periodic table. It describes Dobereiner's triads and Newlands' law of octaves as early attempts to classify elements. Mendeleev created the first periodic table by arranging elements by atomic mass and predicted properties of undiscovered elements. The modern periodic table is arranged by atomic number, completing the 7th period with the discoveries of elements 113, 115, 117, and 118. Elements are classified into blocks based on their electronic configuration. The periodic table shows periodic trends in properties and groups elements with the same number of valence electrons.
Periodic classification of elements gr10, 2020-21MhdAfz
For more such informative content, go to https://scifitechify.blogspot.com/. This video will tell you about the history of periodic classification of elements. HOPE YOU ENJOY IT. NEXT POST ON: WHY DO WE WEIGH LESS ON THE MOON ?
The document summarizes key concepts from Chapter 4 of the textbook, including:
1) Elements are organized in the periodic table based on their atomic number, with elements in the same group sharing similar chemical properties due to having the same number of valence electrons.
2) Early scientists like Newlands and Mendeleev noticed repeating patterns in element properties and developed the first periodic tables, with Mendeleev arranging elements by atomic mass and predicting missing elements.
3) Moseley later determined that atomic number, not atomic mass, is the fundamental basis for the periodic table's organization.
4) The periodic table is divided into blocks like s-block main group elements and d-block transition metals that have
Classification of Elements: The electronic structure of the atom and the Modern Periodic Table
and Periodic Law. Variation of properties within period and groups. Usefulness and limitations of
Periodic Table.
Periodic table and periodic properties discusses the development and features of the periodic table. It describes how early scientists like Dobereiner, Newlands, and Mendeleev organized elements and recognized periodic trends before the modern periodic table. The document then outlines the structure and classifications of the modern periodic table, including periods, groups, blocks, and representative and transition metals. It also explains important periodic properties such as atomic and ionic radii, ionization energy, and effective nuclear charge and how they vary predictably across the table.
The document discusses the development of the periodic table. It describes early attempts by scientists like Dobereiner, de Chancourtois, and Newlands to classify and organize the known chemical elements. It then focuses on the key contributions of Dmitri Mendeleev and Lothar Meyer, who independently proposed the periodic law stating that properties of elements are periodic functions of their atomic weights. Mendeleev is credited with publishing the first recognizable version of the modern periodic table in 1869, arranging elements by property groups and leaving gaps for undiscovered elements, some of which he accurately predicted properties for like gallium and germanium. His work established the periodic table as essential for classifying and understanding the elements.
Chemistry notes class 11 chapter 3 classification of elements and periodicity...AMARJEET KUMAR
This document provides an overview of the history of classifying elements and the development of the periodic table. It discusses early classification systems proposed by Prout, Dobereiner, Newlands and others. Meyer proposed classifying elements based on an atomic volume curve. Mendeleev created the first recognizable periodic table in 1869, which was improved upon over time. Key periodic properties like atomic radius, ionization energy, electronegativity and valency are explained in relation to an element's position on the periodic table. The modern periodic table is based on atomic number and has 18 groups and 7 periods.
The periodic table evolved over time as scientists discovered more useful ways to organize the elements. Elements are organized into blocks according to their electron configurations, with trends in properties like atomic radius occurring from period to period and group to group. Atomic radius generally decreases left to right as nuclear charge increases, and increases down a group as the outer orbital size increases. Ionic radius follows similar trends but is smaller for positive ions and larger for negative ions due to electron gain or loss.
The document provides biographical information about Dmitri Mendeleyev, the discoverer of the periodic table. It notes that he was a Russian chemist born in 1834 who served as a professor of chemistry. In 1869, he announced the principle of periodicity of properties in chemical elements and created the first periodic table. His table arranged elements in order of atomic weight and grouped them by similar properties, allowing him to predict properties of undiscovered elements. The periodic table organized the known chemical elements and reflected recurring trends in their properties based on atomic structure.
The document discusses the organization and structure of the periodic table. It describes how elements are arranged based on their atomic structure and properties. Elements are organized by increasing atomic number and grouped according to similar characteristics. The periodic table displays the symbols, names, atomic numbers and masses of each element.
The document discusses the organization and structure of the periodic table. It describes how elements are arranged based on their atomic structure and properties. Elements are organized by increasing atomic number and grouped according to similar characteristics. The periodic table displays the symbols, names, atomic numbers and masses of each element.
The document summarizes key concepts about the periodic table, including its history and development. It describes how Mendeleev organized the elements and made predictions that were later confirmed, establishing the periodic law. Over time, the periodic table was refined as new elements were discovered and atomic number was established as the basis for organization. The document also outlines periodic trends in properties like atomic radius, ionization energy, and electronegativity.
Periodic Table (Classification of elements) MANIKImran Nur Manik
Electronic structure of atoms, modern periodic table and periodic law, variation of periodic properties within periods and groups, ionization potential, electron affinity, electronegativity, usefulness and limitation of periodic table.
The periodic table is arranged based on atomic number and properties repeat periodically. Early forms grouped elements based on atomic mass but Moseley found atomic number was key. The table is divided into periods and groups with trends in properties like atomic size decreasing left to right across periods and ionization energy increasing. Metallic character increases down groups and nonmetallic character increases right across periods. The periodic table organizes the elements and allows prediction of properties.
During the 19th century, chemists began categorizing elements based on their properties, leading to modern periodic tables. Johann Dobereiner observed that some elements formed triads with similar properties. John Newlands proposed an early periodic law in which properties repeated every eighth element, though this failed with new discoveries. Dmitri Mendeleev and Lothar Meyer independently created early periodic tables arranging elements by atomic mass, with Mendeleev accurately predicting unknown elements. Henry Moseley determined elements' ordering by atomic number, establishing the modern periodic table.
1. The document provides a summary of the periodic classification of elements, including the theories of Dobereiner, Newlands, and Mendeleev, and the modern periodic law.
2. It describes the achievements and limitations of their classifications, and how the modern periodic table addresses the limitations by arranging elements by atomic number instead of atomic mass.
3. The document also summarizes key trends in the modern periodic table such as how properties change from period to period and group to group.
This document discusses the development of the periodic table from early classification attempts to the modern periodic table. It describes Dobereiner's discovery of triads of elements with similar properties in the 1810s. It then discusses Newlands' law of octaves from the 1860s which noted patterns every eighth element. Mendeleev developed the first periodic table in 1869, arranging elements by atomic mass and leaving gaps for undiscovered elements. The modern periodic table is arranged by atomic number instead of mass and helped resolve limitations of earlier classifications. It describes trends in properties like valency and size across periods and groups in the modern periodic table.
The document discusses the history and development of the periodic table. It describes early classification systems developed by Dobereiner, Newlands, and Mendeleev. Mendeleev arranged elements in order of atomic mass and left gaps for undiscovered elements, correctly predicting their properties. The modern periodic table is arranged by atomic number instead of mass. The 7th period is now complete with the discovery of elements 113, 115, 117, and 118 as announced by IUPAC. The periodic table is divided into periods and groups based on electron configuration and properties repeat periodically.
This document contains the scheme of work and lesson plans for teaching chemistry to SS2 students. It covers topics on the periodic table over two weeks, including properties of elements, groups and periods. It then covers chemical reactions over one week, discussing concepts like reactants and products, and factors that affect reaction rates such as concentration, temperature, and catalysts. The lessons include content, examples, evaluations, and assignments.
The document discusses the history and development of the periodic table. It describes Dobereiner's triads and Newlands' law of octaves as early attempts to classify elements. Mendeleev created the first periodic table by arranging elements by atomic mass and predicted properties of undiscovered elements. The modern periodic table is arranged by atomic number, completing the 7th period with the discoveries of elements 113, 115, 117, and 118. Elements are classified into blocks based on their electronic configuration. The periodic table shows periodic trends in properties and groups elements with the same number of valence electrons.
Periodic classification of elements gr10, 2020-21MhdAfz
For more such informative content, go to https://scifitechify.blogspot.com/. This video will tell you about the history of periodic classification of elements. HOPE YOU ENJOY IT. NEXT POST ON: WHY DO WE WEIGH LESS ON THE MOON ?
The document summarizes key concepts from Chapter 4 of the textbook, including:
1) Elements are organized in the periodic table based on their atomic number, with elements in the same group sharing similar chemical properties due to having the same number of valence electrons.
2) Early scientists like Newlands and Mendeleev noticed repeating patterns in element properties and developed the first periodic tables, with Mendeleev arranging elements by atomic mass and predicting missing elements.
3) Moseley later determined that atomic number, not atomic mass, is the fundamental basis for the periodic table's organization.
4) The periodic table is divided into blocks like s-block main group elements and d-block transition metals that have
Classification of Elements: The electronic structure of the atom and the Modern Periodic Table
and Periodic Law. Variation of properties within period and groups. Usefulness and limitations of
Periodic Table.
Periodic table and periodic properties discusses the development and features of the periodic table. It describes how early scientists like Dobereiner, Newlands, and Mendeleev organized elements and recognized periodic trends before the modern periodic table. The document then outlines the structure and classifications of the modern periodic table, including periods, groups, blocks, and representative and transition metals. It also explains important periodic properties such as atomic and ionic radii, ionization energy, and effective nuclear charge and how they vary predictably across the table.
The document discusses the development of the periodic table. It describes early attempts by scientists like Dobereiner, de Chancourtois, and Newlands to classify and organize the known chemical elements. It then focuses on the key contributions of Dmitri Mendeleev and Lothar Meyer, who independently proposed the periodic law stating that properties of elements are periodic functions of their atomic weights. Mendeleev is credited with publishing the first recognizable version of the modern periodic table in 1869, arranging elements by property groups and leaving gaps for undiscovered elements, some of which he accurately predicted properties for like gallium and germanium. His work established the periodic table as essential for classifying and understanding the elements.
Chemistry notes class 11 chapter 3 classification of elements and periodicity...AMARJEET KUMAR
This document provides an overview of the history of classifying elements and the development of the periodic table. It discusses early classification systems proposed by Prout, Dobereiner, Newlands and others. Meyer proposed classifying elements based on an atomic volume curve. Mendeleev created the first recognizable periodic table in 1869, which was improved upon over time. Key periodic properties like atomic radius, ionization energy, electronegativity and valency are explained in relation to an element's position on the periodic table. The modern periodic table is based on atomic number and has 18 groups and 7 periods.
The periodic table evolved over time as scientists discovered more useful ways to organize the elements. Elements are organized into blocks according to their electron configurations, with trends in properties like atomic radius occurring from period to period and group to group. Atomic radius generally decreases left to right as nuclear charge increases, and increases down a group as the outer orbital size increases. Ionic radius follows similar trends but is smaller for positive ions and larger for negative ions due to electron gain or loss.
The document provides biographical information about Dmitri Mendeleyev, the discoverer of the periodic table. It notes that he was a Russian chemist born in 1834 who served as a professor of chemistry. In 1869, he announced the principle of periodicity of properties in chemical elements and created the first periodic table. His table arranged elements in order of atomic weight and grouped them by similar properties, allowing him to predict properties of undiscovered elements. The periodic table organized the known chemical elements and reflected recurring trends in their properties based on atomic structure.
The document discusses the organization and structure of the periodic table. It describes how elements are arranged based on their atomic structure and properties. Elements are organized by increasing atomic number and grouped according to similar characteristics. The periodic table displays the symbols, names, atomic numbers and masses of each element.
The document discusses the organization and structure of the periodic table. It describes how elements are arranged based on their atomic structure and properties. Elements are organized by increasing atomic number and grouped according to similar characteristics. The periodic table displays the symbols, names, atomic numbers and masses of each element.
The document summarizes key concepts about the periodic table, including its history and development. It describes how Mendeleev organized the elements and made predictions that were later confirmed, establishing the periodic law. Over time, the periodic table was refined as new elements were discovered and atomic number was established as the basis for organization. The document also outlines periodic trends in properties like atomic radius, ionization energy, and electronegativity.
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1. CLASSIFICATION OF ELEMENTS AND
PERIODICITY IN PROPERTIES OF
ELEMENTS
BY-
A.P.S. BHADOURIYA
M.Sc. , B.Ed., NET
PGT-CHEMISTRY
K.V. BARABANKI
2. 1. Why do we need
classification.?
2. Dobereniner’s triads
3. Newlands law of octave
4. Lother Meyer volume curve
5. Mendeleev’s periodic table
6. Modern periodic table
7. IUPAC nomenculature for
elements Z >100
8. Periodic Trends in Physical
Properties
Shielding effect & Effective
Nuclear Charge
Atomic Radius
Ionic Radius
Ionization Enthalpy
Electron Gain Enthalpy
Electronegativity
9. Periodic Trends in Chemical
Properties
Periodicity of Valence or
Oxidation States
Anomalous Properties of
Second Period Elements
Chemical Reactivity
SESSIONOBJECTIVES
3. Lavoisier (1789) classified elements into
metals, non-metals, gases and earths.
During the nineteenth century, chemists
began to categorize the elements according
to similarities in their physical and chemical
properties. The end result of these studies
was our modern periodic table.
4. DOBEREINER’S TRIADS [ JOHN DOBEREINER (1817)]
In 1829, he classified some elements into groups of
three, which he called triads.
The elements in a triad had similar chemical
properties and orderly physical properties.
Model of triads
S.N
o
Triad
Atomic masses of
elements of triad
Arithmetic mean of
atomic masses of first
and third element
1 Cl,Br,I 35.5, 80, 127 35.5 + 127
2
= 81.25
3 Ca,Sr,Ba 40,87.5,137 40+137
2
= 88.5
2 Li,Na,K 7, 23, 39 7 + 39
2 = 23
5. In 1866, he suggested that elements be arranged in
“octaves” because he noticed (after arranging the
elements in order of increasing atomic mass) that
certain properties repeated every 8th element.
NEWLAND’S LAW OF OCTAVES [JOHN NEWLAND (1866)]
6. NEWLAND’S LAW OF OCTAVES [JOHN NEWLAND (1863)]
Element
Atomic mass
Element
Atomic mass
Element
Atomic mass
I II III IV V VI VII
Li Be B C N O F
7 9 11 12 14 16 19
Na Mg Al Si p S Cl
23 24 27 28 31 32 35.5
K Ca
39 40
Newland was first to publish the list of elements in
increasing order of atomic masses.
11. Groups
•8 vertical rows.
•7 groups were subdivided in A and B.
•8th group has 9 elements in the group of
3 each.
Periods
•7 horizontal rows.
Only 63 elements were known.
MENDELEEV’S PERIODIC TABLE
12. MERITS OF MENDELEEV’S PERIODIC TABLE
Prediction of new
elements
(Ge, Ga, Sc)
1
Systematic study
of elements
2
Correction of
atomic mass
(Be, Au, Pt)
3
13. Mendeleev
•stated that if the atomic weight of an element
caused it to be placed in the wrong group, then
the weight must be wrong.
(He corrected the atomic masses of Be, In, and
U)
•was so confident in his table that he used it to
predict the physical properties of three elements
that were yet unknown.
After the discovery of these unknown elements
between 1874 and 1885, and the fact that
Mendeleev’s predictions for Sc, Ga, and Ge were
amazingly close to the actual values, his table
was generally accepted.
14. DEFECTS OF MENDELEEV’S PERIODIC TABLE
Position of
hydrogen.
Anomalous pairs.
(Ar and K, Co and
Ni, Te and I)
Position of
isotopes
e.g. 1H1,
1H2,
1H3
16. Mendeleev’s periodic table was published in 1905 when
no one had an idea of the structure of an atom.
DO YOU KNOW?
Mendeleev’s name has been immortalized by naming
the element with atomic number 101, as Mendelevium.
This name was proposed by American scientist Glenn
T. Seaborg, the discoverer of this element, “in
recognition of the pioneering role of the great Russian
Chemist who was the first to use the periodic system
of elements to predict the chemical properties of
undiscovered elements, a principle which has been the
key to the discovery of nearly all the transuranium
elements
17. English physicist, Henry Moseley observed regularities
in the characteristic X-ray spectra. A plot of f against
atomic number (Z ) of the elements gave a straight line
and not the plot of f vs atomic mass
He thereby showed that the atomic number is a more
fundamental property of an element than its atomic
mass.
MODERN PERIODIC LAW AND THE MODERN
PERIODIC TABLE
18.
19. Mendeleev’s Periodic Law was,
therefore, accordingly modified.
This is known as the Modern Periodic
Law and can be stated as :
The physical and chemical properties of
the elements are periodic functions of
their atomic numbers.
20. HENRY MOSELEY
In 1913, through his work with X-rays, he determined the actual
nuclear charge (atomic number) of the elements*. He rearranged
the elements in order of increasing atomic number.
*“There is in the atom a fundamental
quantity which increases by regular
steps as we pass from each element to
the next. This quantity can only be the
charge on the central positive nucleus.”
His research was halted when the British government sent him to
serve as a foot soldier in WWI. He was killed in the fighting in
Gallipoli by a sniper’s bullet, at the age of 28. Because of this loss,
the British government later restricted its scientists to noncombatant
duties during WWII.
25. FEATURES OF LONG FORM OF PERIODIC
TABLE
•Contains elements arranged in
increasing order of atomic numbers.
•Explains the position of an element in
relation to other elements.
•Consists of groups and periods.
26. FEATURES OF LONG FORM OF PERIODIC TABLE
Groups Vertical column
Total 18. Numbered 1-18 or
IA to VII A, IB to VII B, VIII and zero.
Periods Horizontal column
Total 7 numbered from 1 to 7.
Elements in a group have similar but not
identical electronic configuration and properties
Contains 2,8,8,18,18,32 and 28 elements
respectively.
27. ELECTRONIC CONFIGURATIONS AND TYPES OF
ELEMENTS:
On the basis of the nature of sub-shell in which
last electron of atom enters, elements are
divided into 4 blocks
s-Block Element
p-Block Element
d-Block Element
f- Block Element
s-,p-,d-,f- Block Elements
28. • Electronic configuration:
• Groups:
• All are metal, low ionisation energy and low
melting and boiling points, electropositive
elements.
• compounds are mostly ionic & colourless.
IA (alkali metals )and
IIA(alkaline earth metals
ns1 or ns2
In these elements last electron enters the s-orbital
s-Block Elements
29. • Electronic configuration:
• Groups:
• Non-metals, electronegative.
• Form covalent compounds.
ns2,np1 -6
III A to VII A and zero group (group 13-18).
In these elements last electron enters the p-orbital
p-Block Elements
30. • Electronic configuration:
• Groups:
• Variable valency high melting and boiling point.
• Coloured compounds and catalytic property.
(n-1)d1-10 ns1or2
I B to VII B and VIII groups (Gr- 3-12).
In these elements last electron enters the d-orbital,
Also known as transition metals.
d-Block Elements
31. • Electronic configuration:
• Have high melting and boiling point.
(n-2)f1-14(n-1)d0-1ns2
•Present below the periodic
table in two rows
•Lanthanides-elements after
lanthanum(Gr.-3, Pd.-6)
•Actinides-elements after
actinium. (Gr.-3, Pd.-7)
In these elements last electron enters the f-orbital,
Also known as Inner-Transition Elements
f-Block Elements
32. Representative elements
Transition elements
s and p block elements .
d-block elements. Valence shell and penultimate
Shell both are incomplete.
Inner Transition elements
f-block elements. Valence shell, penultimate shell
antipenultimate shell are incomplete.
FEATURES OF LONG FORM OF PERIODIC TABLE
33. Metals
•Present on left hand side of periodic
table.
•Solid,malleable,ductile and conductors .
Non-metals
•Present on right hand side of periodic
table.
•Solid or liquid or gas.
Metalloids
•Present on zig-zag between metals and non-metals.
e.g. B,Si,Ge,As,Sb and Te.
FEATURES OF LONG FORM OF PERIODIC TABLE
34. • Based on a more fundamental basis
- the atomic number
• Position of an element is related to the electronic
configuration of its atom.
• Due to separation of elements into groups, dissimilar
elements (e.g. alkali metals I A and coinage metals I B)
do not fall together.
MERITS OF LONG FORM OF PERIODIC TABLE
35. DEFECTS OF LONG FORM OF
PERIODIC TABLE
The problem of the position of hydrogen in
the table has not been solved completely
Configuration of Helium(1s2 ) is different
from inert gases (ns2,np6) but are placed in
the same group.
It is unable to include lanthanides and
actinides in its main body.
36. e.g. atomic number 115
Will be named as
un+un+pent+ium
=ununpentium
and symbol is Uup
Name
=digits name + ium
NOMENCLATURE OF THE ELEMENTS
WITH ATOMIC NUMBER >100
Digit Name Abbrevia
tion
0 nil n
1 un u
2 bi b
3 tri t
4 quad q
5 pent p
6 hex h
7 sept s
8 oct o
9 enn e
39. Periodic Trends in Chemical Properties
Periodicity of Valence or Oxidation States
Anomalous Properties of Second Period
Elements
Chemical Reactivity
Periodic Properties
40. Shielding effect & Effective Nuclear Charge
The decrease in nuclear charge ( nuclear
force of attraction) on outermost shell
electrons due to repulsion caused by inner
shell electron is known as shielding effect of
inner shell or intervening electrons on outer
shell electron.
41. Shielding effect & Effective Nuclear Charge
Due to shielding effect the nuclear charge is lowered
on outermost shell electrons, the net nuclear
charge acting on outermost shell electrons is known
as Effective Nuclear Charge. It is denoted by Z* or
Zeff.
Z* or Zeff. = Z - σ
where Z = nuclear charge( = atomic No.) &
σ = shielding constant or screening constant , it is a
measure of shielding effect
42. Determination of ENC (Z*)
If the electron resides in s or p orbital
1. Electrons in principal shell higher than the e- in
question contribute 0 to σ .
2. Each electron in the same principal shell contribute
0.35 to σ (0.30 if it is 1S shell).
3. Electrons in (n-1) shell each contribute 0.85 to σ .
4. Eelectrons in deeper shell each contribute 1.00 to σ
Shielding effect & Effective Nuclear Charge
43. Determination of ENC (Z*)
If the electron resides in d or f orbital
1. All e-s in higher principal shell contribute 0 to σ
2. Each e- in same shell contribute 0.35 to σ
3. All inner shells in (n-1) and lower contribute
1.00 to σ
Shielding effect & Effective Nuclear Charge
44. Determination of ENC (Z*)
e.g. Calculate the Z* for the 2p electron Fluorine
(Z = 9) 1s2, 2s 2p5.
Soln. Screening constant for one of the outer electron
6 (six) (two 2s e- and four 2p e-) = 6 X 0.35 = 2.10
2 (two)1s e- = 2 X 0.85 = 1.70
σ = 1.70+2.10 = 3.80
Z* = 9 - 3.80 = 5.20
Shielding effect & Effective Nuclear Charge
45. Trend of ENC in Periodic Table
In a Period - Effective nuclear charge Z*
increases increases rapidly along a
period(0.65 per next group)
e.g.
Shielding effect & Effective Nuclear Charge
Li Be B C N O F Ne
1.3 1.95 2.6 3.3 3.9 4.6 5.2 5.9
46. Shielding effect & Effective Nuclear Charge
Trend of ENC in Periodic Table
In a Group - Effective nuclear charge Z* increases
slowly along a group.
e.g.
Gr-1 H Li Na K Rb Cs
Z* 1.0 1.3 2.2 2.2 2.2 2.2
47.
48.
49. PERIODIC TREND OF ATOMIC RADIUS
In A Period-
atomic radius decreases with increase in atomic number
(in a period left to right)
BECAUSE in a period left to right-
1. n (number of shells) remain constant.
2. Z increases (by one unit)
3. Z* increases (by 0.65 unit)
4. Electrons are pulled close to the nucleus by the increased
Z*
50. In a group-
Atomic radius increases moving down the group
Because, along a group top to bottom
1. n increases
2. Z increases
3. No dramatic increase in Z* - almost remains
constant
51. IONIC RADII
All anions are larger than their parent atoms.
because the addition of one or more electrons would result
in increased repulsion among the electrons and a decrease
in ENC.
The cations are smaller than their parent atoms
because it has fewer electrons while its nuclear charge
remains the same & hence ENC is greater in cation than its
parent atom
52.
53.
54. ISOELECTRONIC SPECIES
Atoms and ions which contain the same number of
electrons, are called as isoelectronic species.
For example, F–, Na+ and Mg2+ have the same number of
electrons(=10).
The size of isoelectronic species decreases with increase in
nuclear charge. e.g.-
o2->F- >Ne>Na+>Mg2+>Al3+
---------SIZE DECREASING------
58. NOTE:
Metallic radii in the third row d-block are similar to
the second row d-block, but not larger as one
would expect given their larger number of
electrons.
This is due to Lanthanide Contraction as f-orbitals
have poor shielding properties.
59. Ionisation Energy (IE) or
Ionisation Enthalpy (ΔiH )
Ionization: removing an electron from an atom or ion
Ionization energy: energy required to remove an electron
from an isolated, gaseous atom or ion is called as Ionization
energy or ionisation enthalpy.
If the atom is neutral the above defined ionisation energy
is called as first ionisation enthalpy.
Energy required to remove an electron from an isolated,
monovalent cation is called as second Ionization energy.
The ionization enthalpy is expressed in units of kJ /mol
60. X(g) + energy → X+(g) + e–.
1st ionisation enthalpy
X+(g) + energy → X++(g) + e–.
2nd ionisation enthalpy
Ionisation Energy (IE) or
Ionisation Enthalpy (ΔiH )
61. The second ionization enthalpy will be higher than
the first ionization enthalpy because it is more
difficult to remove an electron from a positively
charged ion than from a neutral atom because a
cation has greater ENC than a neutral atom.
In the same way the third ionization enthalpy will
be higher than the second and so on.
Ionisation Energy (IE) or
Ionisation Enthalpy (ΔiH )
62. (a) Size of the atom - IE decreases as the size of the
atom increases
(b) Nuclear Charge - IE increases with increase in
nuclear charge
(c) The type of electron - Shielding effect, Penetration
effect
(e)Electronic configuration: e.g. noble gases passes
very high value of IE due to stable octet
configuration
Factors affecting Ionisation Enthalpy (ΔiH )
63. On moving down a group
1. nuclear charge increases
2. Z* due to screening is almost constant
3. number of shells increases, hence atomic size
increases.
4. there is a increase in the number of inner electrons
which shield the valence electrons from the nucleus
Thus IE decreases down the group
Periodic Trend of Ionisation Enthalpy (ΔiH )
64. On moving across a period(L--->R)
1. the atomic size decreases
2. Effective nuclear charge increases
Thus IE increases along a period
However there are some exceptions also e.g.
IE of Be is higher than that of B.
IE of N is higher than that of O.
Periodic Trend of Ionisation Enthalpy
65.
66. Explain why- (a). IE of Be is higher than that of B.
Ans. - In beryllium(1s2,2s2 ), the electron removed during the
ionization is an s-electron whereas the electron removed
during ionization of boron(1s2,2s2,2p1) is a p-electron. The
penetration of a 2s-electron to the nucleus is more than
that of a 2p-electron; hence the 2p electron of boron is more
shielded from the nucleus by the inner core of electrons
than the 2s electrons of beryllium.
Therefore, it is easier to remove the 2p-electron from boron
compared to the removal of a 2s- electron from beryllium.
Thus, boron has a smaller first ionization.
Periodic Trend of Ionisation Enthalpy (ΔiH )
67. (b) Why IE of N is higher than that of O.
Ans. The first ionization enthalpy of oxygen compared to
nitrogen is smaller. This arises because in the nitrogen
atom(1s2,2s2,2p3) three 2p-electrons reside in different
atomic orbitals (Hund’s rule) whereas in the oxygen atom
(1s2,2s2,2p4), two of the four 2p-electrons must occupy the
same 2p-orbital resulting in an increased electron-electron
repulsion. Consequently, it is easier to remove the fourth
2p-electron from oxygen than it is, to remove one of the
three 2p-electrons from nitrogen.
Periodic Trend of Ionisation Enthalpy (ΔiH )
68. Electron Gain Enthalpy (ΔegH)
When an electron is added to a neutral gaseous atom (X) to
convert it into a negative ion, the enthalpy change
accompanying the process is defined as the Electron
GainEnthalpy (ΔegH) or Electron Affinity.
Electron gain enthalpy provides a measure of the ease
with which an atom adds an electron to form anion as
represented by equation –
X(g) + e --- X- (g)+energy
(electrongainenthalpy)
69. Depending on the element, the process of
adding an electron to the atom can be either
endothermic or exothermic.
For many elements energy is released when an
electron is added to the atom and the electron gain
enthalpy is negative.
Electron Gain Enthalpy (ΔegH)
70. ENC- With increase in ENC, the force of attraction exerted by
the nucleus on the electrons increases. Consequently, the
atom has a greater tendency to attract additional electron
i.e., its EGE increases i.e. become more negative.
ATOMIC SIZE-
With decrease in size ENC increases & hence EGE
increases.
ELECTRONIC CONFIGURATION-
The value of EGE depends effectively upon electronic
configuration of elements, elements with stable electronic
configuration posses lower (less -ve) value of EGE, e.g.-
Factors Affecting E G E (ΔegH)
71. A. Noble gases have practically zero or +ve EGEs. This
is because they have no tendency to gain an
additional electron as they already have the stable
ns2np6 configuration
B. Halogens have high electron affinities. This is due
to their strong tendency to gain an additional
electron to change into the stable ns2np6
configuration.
Factors Affecting E G E (ΔegH)
72. IN A PERIOD-
The EGE increases i.e. become more negative as we move
across a period because the atomic size decreases and hence
the force of attraction exerted by the nucleus on the
electrons increases. Consequently, the atom has a greater
tendency to attract additional electron i.e., its electron
affinity increases
IN A GROUP-
The EGE decreases (-)vely because the atomic size increases
and therefore, the effective nuclear attraction decreases and
thus electron affinity decreases
PERIODIC TREND OF EGE (ΔegH)
73.
74. Explain why –
(a). electron gain enthalpy of O is less than that of the S.
(b). electron gain enthalpy of F is less than that of the Cl.
Ans:- The electron gain enthalpy of O or F is less than that
of the succeeding element. This is because when an electron
is added to O or F, the added electron goes to the smaller n
= 2 quantum level and suffers significant repulsion from the
other electrons present in this level. For the n = 3 quantum
level (S or Cl ), the added electron occupies a larger region
of space and the electron-electron repulsion is much less.
Electron Gain Enthalpy (ΔegH)
75. The tendency of an element in a molecule
to attract the shared pair of electrons
towards itself is known as electronegativity.
It is measured on Pauling scale in which F
(most EN element)is attributed to a value of
4 .
Electronegativity
76. Periodic trend of EN
In a Group- on moving down the group,
Z increases but Z* almost remains constant
number of shells (n) increases
atomic radius increases
force of attraction between added electron and
nucleus decreases
Therefore EN decreases moving down the group
77. In a Period- On moving across a period left to right
Z and Z* increases
number of shells remains constant
atomic radius decreases
force of attraction between shared electron and
nucleus increases
Hence EN increases along a period
Periodic trend of EN
78.
79. Periodicity of Valence or Oxidation States
Anomalous Properties of Second Period
Elements
Chemical Reactivity
Periodic Trends in Chemical Properties
80. The valence of representative elements is usually (though
not necessarily) equal to the number of electrons in the
outer most orbitals and / or equal to eight minus the
number of outermost Electrons(w.r.t. H)
Some periodic trends observed in the valence of elements
(hydrides and oxides) are shown in Table
Periodicity of Valence or Oxidation States
Group 1 2 13 14 15 16 17
Number of
valence
electron
1 2 3 3 5 6 7
Valence 1 2 3 4 3,5 2,6 1,7
81. The oxidation state of an element in a particular
compound can be defined as the charge acquired by
its atom on the basis of electronegative
consideration from other atoms in the molecule.
Each group has a common (+)ve or (-)ve oxidation state
And it show gradual change in oxidation state in a
period
Periodicity of Valence or Oxidation States