classification of elements

1. Home
Presented By
PRAMOD ANANDRAO
KONDALKAR
ASST. TEACHER
ADARSH KISAN
VIDYALAYA, NARANDA
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2. Back
Moseley showed that the atomic number of an
element is equal to the number of protons in the
nucleus of the atom.
1)
Moseley’s contribution to the classification of elements.
He suggested that atomic number should be
considered as a more fundamental property of an
elements rather than its atomic weight.
2)
In modern periodic table, on the basis of Moseley’s
work, elements were arranged in the increasing
order of their atomic number (Z) in a more
systematic way.
3)
Electronic configuration of an element is directly
related to its atomic number (Z).
4)
Modern periodic law
Law : The properties of the element are the periodic function of their atomic numbers.
(Atomic No (Z) is the number of protons in the nucleus or the number of extra nuclear
electrons present in the neutral atoms of the elements. )
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3. Modern Periodic Table
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4. Number of Energy Levels: 3
First Energy Level: 2
Second Energy Level: 8
Third Energy Level: 1
Isotopes
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Remember
The position of an element in the periodic table is generally determined
by its electronic configuration.
e.g. electronic configuration of sodium is 2, 8, 1 i.e., it has three shells and one
electron in the outermost shell.
Hence, it is placed in period number 3 and group number 1. However,
in the case of transition elements this pattern is not followed.

5. Sketch of the Modern Periodic Table.
IIIB – VI PERIOD
IA
IIA
IIIB IVB VB VIB VIIB ----VIIIB--- - IB IIB
IIIA IVA VA VIA
VIIA
VIII
A/
0
GR
OU
P
IIIB – VII PERIOD
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6. Normal elements
Classification of Element
1) The elements of the atoms of which only the
outermost shell incompletely filled are called
normal elements.
2) The elements of s-block and p-block together,
except zero group constitute normal elements.
3) They are reactive elements.
4) They are solids, liquids and gases.
5) Alkali metals, alkaline earth metals and
halogensare some of normal elements.
Examples : 1) Typical elements : Li, Be, B, C, N, O, F.
2) Representative elements : Na, Mg, Al, Si, P, S, Cl.
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7. Transition Elements
1) The elements of the atoms of which the last two shells
incompletely filled are called Transition elements.
2) They are placed in between elements of s-block and p-block. They
are also called d-block elements.
3) They belong to group IB to VIIB and VIII.
4) These elements are solid metals at room temperature.
Exemple : Cu, Ag, Au, Fe etc.
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8. Inner transition elements
1) The elements of the atoms of which the last three shells
incompletely filled are called inner transition elements.
2) They are placed into two separate series at the bottom of periodic
table. That series are called Lanthanides series and Actinides series.
Each series contain 14 elements.
3) They are also called f-block elements.
4) The elements belonging to each series have quite similar
properties.
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9. Inert gases
1) The elements of the atoms of which all shells completely filled are called
inert gases or noble gases or rare gases.
2) In the modern periodic table they are placed in zero group.
3) Under ordinary condition these elements are chemically inert due to
their stable electronic configuration.
4) They all are gases elements.
Example : Helium(He), Neon(Ne), Argon(Ar), Krypton(Kr), Xenon(Xe) and
Radon(Rn) are inert gases.
Helium (He)
Atom
Neon (Ne)
Atom
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10. Main Features of the Long form of the Periodic Table.
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1) The position of an element in the longform of the periodic table is related
to its electronic configuration.
2) The number of electronic shells present in the atoms of elements in
each period is equal to the number of the period.
3) The number of electrons in the outermost shell of an atom of an element is
equal to the group number of the element.
4) Each period begins with an alkali metal element with only one electron
is the outermost shell and ends with an inert gas elements having
stable electronic configuration i.e. 8 electron in outermost shell.
5) Systematic classification of elements into s-block, p-block, d-block and f-
block is achieve in the table.
6) Elements belonging to the same group have the same characteristic
electronic configuration in their outermost shell. Hence they show
similar chemical properties.
7) Properties of the elements belonging to the same period change gradually
from left to right.
8) Metals and non-metals are properly separated in the periodic table.
9) On the basis of electronic configuration elements are classified into inert
gases, normal elements, transition elements and inner transition
elements. content

11. The elements first period/ second period/ third period of the
modern periodic table and their electronic configuration.
Elements in first period Electronic Configuration
Hydrogen (H)
Helium (He)
(1)
(2)
The elements in the first period and their electronic
configuration are as follows :
Dmitri Mendeleev, father
of the periodic tableHydrogen (H)
Atom
Helium (He)
Atom
Proton (+)
Neutron (no charge)
Electron (-) Home
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12. The elements in the Second period and their
electronic configuration are as follows :
Elements in Second
period
Electronic
Configuration
Lithium (Li) (2,1)
Beryllium (Be) (2, 2)
Boron (B) (2, 3)
Carbon (C) (2, 4)
Nitrogen (N) (2, 5)
Oxygen (O) (2, 6)
Fluorine (F) (2, 7)
Neon (Ne) (2, 8)
Lithuum (Li)
Atom
Beryllium (Be)
Atom
Proton (+)
Neutron (no charge)
Electron (-)
Boron (B)
Atom
Caron (C)
Atom
Atomic Structure
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13. The elements in the Third period and their electronic
configuration are as follows :
Elements in Third
period
Electronic
Configuration
Sodium (Na) (2,8, 1)
Magnesium (Mg) (2, 8, 2)
Aluminium (Al) (2, 8, 3)
Silicon (Si) (2, 8, 4)
Phosphorus (P) (2, 8, 5)
Sulphur (S) (2, 8, 6)
Chlorine (Cl) (2, 8, 7)
Argon (Ar) (2, 8, 8)
Proton (+)
Neutron (no charge)
Electron
(-)
Magnesium
(Mg) Atom
Sodium (Na)
Atom
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14. The periods in the modern periodic table.
There are 7 periods in the modern periodic table, they are described below.
1) First period is the shortest period containing only two elements hydrogen and
helium.
2) Second and third periods known as short periods consist of eight elements
each. Second period start lithium and ends with neon and third period start with
sodium and ends with argon. Both period contain normal elements.
3) Fourth and fifth periods are long periods containing 18 elements. Fourth period
starts with Potassium and ends with krypton. Fifth period start with rubidium and
ends with xenon. Each of these periods contains one set of eight normal elements
and a set of 10 transition elements.
4) Sixth period is the longest period containing 32 elements from caesium to
radon. This period contains 14 lanthanide elements. It includes eight normal
elements, 10 transition elements and 14 inner transition elements
5) Seventh period is an incomplete period containing 30 elements (Fr-87 to
element-116).It contains 14 inner transition series of actinide elements. Elements
coming after uranium are known as transuranic elements. All actinides are
radioactive. The elements up to atomic number 92 occur in nature and elements
after this are all prepared artificially.
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15. The trends in the valences of the elements in a period.
The valency of an elements is the number of hydrogen atoms it can
combine with or replace. It related to the number of valence electrons in the
atoms of an elements.
Group IA IIA IIIA IVA VA VIA VIIA Zero Group
Element Li Be B C N O F Ne
Chloride LiCl BeCl2 BCl3 CCl4 NCl3 Cl2O ClF No chloride
Oxide Li2O BeO B2O3 CO2 N2O3 O2 OF2 No Oxide
Hydride LiH BeH2 B2H6 CH4 NH3 H2O HF No Hydride
Valency 1 2 3 4 3 2 1 0
2) In a second period, the valency of elements increases from 1 for alkali metals to 4 for
the group IVA(14) elements and then decreases to 1 for Halogens VIIA (17), and zero of
zero group.
Q1) What is the valency of the atom shown in figure?
Q2) In which period and which group the atom shown
in figure is placed?
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16. Groups of the modern periodic table with reference to the
properties of the Elements.
There are 18 vertical columns constitute 16 group. These groups are IA - VIIA (1, 2 and
13 - 17), IB - VIIB and the group VIII (3 to 12).
1)
2) Elements belonging to same group have the same numbers of electron in outermost
orbit (valence electron). Hence show similar chemical properties.
In a group, as atomic number increases new shell are successively added. The atomic
size (atomic radius) thus increases and hence shows gradation of properties of the
element down the group.
3)
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17. Elements and their Electronic Configuration of the Group IA and
their valency.
In the atoms of elements of Group IA, only the outermost shell is incomplete with
one electron.
The elements of group IA (1), have one electron in the valence shell. They are
mono valent.
Valency
:
Valency
:
Group IA (1) elements known as alkali metalsGroup IA (1) elements known as alkali metals
Group IA (1) elements are called alkali metals because their oxides
are water soluble and they form strong bases, when dissolved in
water.
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Element Atomic Electronic configuration Valency Formula of oxide Formula of
number hydroxide
Lithium 3 2, 1 +1 Li2O LiOH
Sodium 11 2, 8, 1 +1 Na2O NaOH
Potassium 19 2, 8, 8, 1 +1 K2O KOH
Rubidium 37 2, 8, 18, 8, 1 +1 Rb2O RbOH
Caesium 55 2, 8, 18, 18, 8, 1 +1 Cs2O CsOH
Francium 87 2, 8, 18, 32, 18, 8, 1 +1 - -
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18. The similarities in the chemical properties of the compounds of alkali metals.
1) The similarities in the chemical properties of (Group IA) alkali metals can be seen from
similarity of the molecular formulae of their compounds, and the reaction of water on their
chlorides and oxides.
Alkali metalsAlkali metals ChloridesChlorides OxideOxide
Lithium (Li)
Sodium (Na)
Potassium (K)
LiCl
NaCl
KCl
Li2O
Na2O
K2O
2) The chlorides and oxides of alkali metal are
water soluble and they form strong bases.
Exp.
NaCl + H2O NaOH + HCl
Na2O + H2O 2NaOH
Comparison of the reactivity's of sodium (Na), Lithium (Li) and Potassium (K)
with respect to reaction with water.
Comparison of the reactivity's of sodium (Na), Lithium (Li) and Potassium (K)
with respect to reaction with water.
As the atomic number increases from Lithium (Li) to Potassium (K), the reactivity also
increases. Thus, Lithium (Li) reacts quietly with water, while sodium reacts vigorously with
water and the amount of energy released in the reaction is also high that the liberated
hydrogen catches fire.
2Na(s) + 2H2O(l) 2NaOH (aq) + H2 + energy
2K(s) + 2H2O(l) 2KOH (aq) + H2 + energy
Thus, sodium is more reactive than
lithium, while potassium is more
reactive than sodium.
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19. Elements of group IIA and their atomic numbers and electronic configuration.
Group IIA consists of alkaline earth metals, they are as follows with their atomic
numbers and their electronic configuration.
Group IIA
Elements
Z Electronic
configuration
Beryllium (Be)
Magnesium (Mg)
Calcium (Ca)
Strontium (Sr)
Barium (Ba)
Radium (Ra)
4
12
20
38
56
88
2,2
2, 8, 2
2, 8, 8, 2
2, 8, 18, 8, 2
2, 8, 18, 18, 8, 2
2, 8, 18, 32, 18, 8, 2
In the atoms of elements of Group
IIA, only the outermost shell is
incomplete with two electron.
Beryllium (Be)
Atom
Magnesium
(Mg) Atom
Valency : In the elements of Group IIA , have
2 electrons in their valence shell, hence they
are divalent.
Exp. MgH2, CaH2
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20. CaCl2 + 2H2O Ca(OH)2 + 2HClCaCl2 + 2H2O Ca(OH)2 + 2HCl
MgCl2 + 2H2O Mg(OH)2 + 2HClMgCl2 + 2H2O Mg(OH)2 + 2HCl
The similarities in the chemical properties of the compounds of Alkaline earth metals.
1) Similarities in the chemical properties of (Group IIA) alkaline earth metals can be seen
from the similarity of molecular formulae of their compounds.
Chlorides of
alkaline
earth metals
Oxides of
alkaline
earth metals
Carbonates of
alkaline earth
metals
BeCl2
MgCl2
CaCl2
BeO
MgO
CaO
BeCO3
MgCO3
CaCO3
2) The chlorides and oxides of
alkaline earth metals react with water
to give hydroxides.
Examples :
MgO + 2H2O Mg(OH)2
MgO + 2H2O Mg(OH)2
CaO + 2H2O Ca(OH)2
CaO + 2H2O Ca(OH)2
3) The carbonate of alkaline earth metals lose
carbon dioxide on heating and form
corresponding oxides
Exp:
MgCO3(s) MgO(s) + CO2
MgCO3(s) MgO(s) + CO2
heat
CaCO3(s) CaO(s) + CO2
CaCO3(s) CaO(s) + CO2
heat
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21. The elements placed in group 7 (VIIA) of the periodic table are called
halogens or salt producers. All these elements form salts called halides, e.g.
NaCl, NaI, KCl, KI etc. Halogen is an ancient Greek word meaning 'salt
producer'. Halogens have seven electrons in their valence shell and so are
monovalent.
Halogens
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Element Atomic number Electronic configuration Valency State Colour
Fluorine 9 2, 7 -1 Gas Greenish
but more
yellow
Chlorine 17 2, 8, 7 -1 Gas Greenish
yellow
Bromine 35 2, 8, 18, 7 -1 Liquid Dark red
liquid
Iodine 53 2, 8, 18, 18, 7 -1 Solid Dark
purple
Astatine 85 2, 8, 18, 32, 18, 7 -1 - -

22. Similarities in the properties of the elements of Group VIIA (17) (Halogens)
considering the following points : (1) Electronic configuration (2) Valences .
1) Electronic configuration : In the atoms of the elements of Group
VIIA (17), only the outermost shell is incomplete with seven
electrons.
Exp :
2) Valency : In the elements of Group
VIIA (17), have 7 electrons in their
valence shell. For complete the octet
they required 1 electron. This makes
the valency of a halogen one. Therefore
they are monovalent.
Exp. HF, HBr, HCl.
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23. Similarities in the chemical properties of the elements of Group VIIA (17) (Halogens).
1) Similarities in the chemical properties of halogens can be seen
from the similarities of the molecular formulae of their
compounds.
Compounds with Hydrogen : HF, HCl, HBr, HI, etc.
Compounds with alkaline earth metals: BeCl2, MgBr2, CaCl2, etc.
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24. Gradation in the properties of the elements of Group VIIA (17)
(Halogens), considering the physical state of the elements.
As the atomic number increases down the
group, the physical state of halogens show
gradation from fluorine to iodine.
At normal temperature fluorine and
chlorine are gaseous, bromine is a liquid while
iodine and astatine are solids.
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25. Zero Group (18) Elements
Names and electronic configuration.
Zero Group
Elements
Zero Group
Elements
ZZ Electronic
configuration
Electronic
configuration
Helium (He)
Neon (Ne)
Argon (Ar)
Krypton (Kr)
Xenon (Xe)
Radon (Rn)
Helium (He)
Neon (Ne)
Argon (Ar)
Krypton (Kr)
Xenon (Xe)
Radon (Rn)
2
10
18
36
54
86
2
2, 8
2, 8, 8
2, 8, 18, 8
2, 8, 18, 18, 8
2, 8, 18, 32, 18, 8
2
2, 8
2, 8, 8
2, 8, 18, 8
2, 8, 18, 18, 8
2, 8, 18, 32, 18, 8
In the atoms of elements of
Zero Group all shells are
completely filled.
Why inert gaseous element not
form ionic or covalent compounds?
1) All the electron shells of atom of inert gaseous element are
completely filled. Hence they have stable electronic configuration.
2) Due to stable electronic configuration they do not lose, gain or
share electron with other atoms. Therefore they do not form ionic
or covalent compounds
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26. FOUR BLOCKS OF PERIODIC TABLE BASED ON THE ELECTRONIC CONFIGURATION.
Based on electronic configuration of elements the four blocks are,
s-block, p-block, d-block and f block.
1) The group IA(1) and IIA(2) together with hydrogen form the s-block elements.
The elements in IA are called alkali metals and elements in IIA are called the
alkaline earth metals.
2) The elements of s-block except hydrogen are all metals.
3) The group of IIIA to VIIA and Zero group together form the p-block elements.
They have 3 to 8 electron in their outermost shell. In the Zero group all the
shells are completely filled.
4) In the p-block all three types of elements are present. i.e. a few metals, all
metalloids and all non-metals.
5) The group IB to VIIB and the group VIII together form the d-block elements.
These elements are also called transition elements. The block is placed
between s- and p- block. There last two shells are incompletely filled. The
elements of d-block are all metals.
6) The two series lanthanides and the actinides place at the bottom of the table
together form the f-block elements. These elements are also called inner
transition elements. There last three shells are incompletely filled. The elements
of f-block are all metals. Home
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28. Give three examples of each of the following.
1) alkali metals 2) alkaline earth metals 3) metals 4) non-metals 5) metalloids.
Give three examples of each of the following.
1) alkali metals 2) alkaline earth metals 3) metals 4) non-metals 5) metalloids.
1) akali metals - Li, Na, K etc.
2) alkaline earth metals - Mg, Ca, Sr etc.
3) metals - Cu, Ag, Au etc.
4) non-metals - F, Cl, Br ect.
5) metalloids - B, Si, Ge, As, Sb, Te, Po.
Metalloids or Zig-zag line in the modern periodic table
1) Elements which have properties intermediate between metallic elements and
non-metallic elements are called metalloid.
2) The bordering elements along the zig-zag line in the modern periodic table are
the metalloids. They are place in IIIA to VIIA group in modern periodic table.
3) All metalloids are p-block elements.
Exp. : Boran (B), Silicon (Si), Germanium (Ge),
Arsenic (As), Antimony (Sb), Tellurium (Te),
Polonium (Po) and Astatine (At).
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29. Give scientific reasons :
1) Valency of elements of group IA is one.
1) Combining power of an atom of element is called valency. It is related with the
number of valance electron i.e. electron present in outermost shell of an atom.
2) The number of valence electron present in atom is equal to the group number. Hence
elements of group IA contain one valence electron.
3) Therefore atoms of elements in Group IA, can lose, gain or share one electron to
complete the outermost shell for stable electronic configuration.
4) Therefore valency of elements of group IA is one.
2) All halogens are monovalent with respect to hydrogen.
1) All halogens contain seven electron in the outermost shell of their atoms.
2) So they can form stable octet by accepting or sharing one electron. All halogens show
common valency of one.
3) Hence all halogens are monovalent with respect to hydrogen.
3) The family of noble gases is named as zero group.
1) The number of electron present in outermost shell of an atom of an elements is equal
to the group number of the elements.
2) In the atoms of inert gas elements (noble gases), all the shells are completely filled.
3) Due to the stable electronic configuration atoms of elements don't lose, accept or
share electrons. Hence valences of noble gases elements is zero.
4) Hence family of noble gases is named as zero group.
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30. 4) Inert gases exit in the form of free atom.
Give scientific reasons :
1) All the shells including outermost shell are completely filled in atoms of Inert gases.
2) Due to stable electronic configuration these elements do not lose, accept or share
electrons and do not form ionic or covalent bonds under normal conditions.
3) Hence, they are monoatomic gases and exist in smallest independent unit in the form
of free atoms.
5) Valency varies gradually along a period.
1) Valency of an elements is fundamental chemical property. i.e. it is directly related to
chemical properties of the elements.
2) The variation of valency along a period follows from the electronic configuration of the
elements.
3) In a second period, the valency varies gradually from 1 for group IA, alkali metals to 4
for Group IVA elements and then decrease to 1 for halogens VIIA and 0 for 0 group.
Thus, valency varies gradually along a period.
6) In the periodic table, iodine is placed in Group VIIA (17).
1) Iodine has seven electrons in the outermost shell.
2) In the modern periodic table, group number indicates the number of electrons in the
valence shell of the atom.
Hence Iodine is placed in Group VIIA (17) of the periodic table.
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31. 7) Actinides are placed at the bottom of the Long form of the Periodic Table.
Give scientific reasons :
1) Actinides are inner transition elements.
2) In the atoms of these elements, the last three shells are incomplete.
3) All of them contain two electrons in the outermost shell. All of them show similar
chemical properties. Hence, all of these elements should be placed in the same group. As it
is not possible the actinides are placed at the bottom of the Long form of the periodic
table.
8) Molecular formulae of chlorides of sodium and potassium are similar while those of
sodium and magnesium are different.
1) Elements belonging to the same group have the same valence electrons and show
similarity in the molecular formulae of their compounds.
2) Sodium (Na) and Potassium (K) belonging to the same group IA (1) of the periodic table.
They have one valence electron in their outermost shell. In the formation of chlorides of
sodium and potassium, sodium and potassium combines with one chlorine atom each to
form sodium chloride (NaCl) and potassium chloride (KCl). Therefore, the molecular
formulae of chlorides of sodium and potassium are similar.
3) magnesium belongs to group IIA (2) of periodic table. It has two valence electrons in the
outermost shell. In the formation of magnesium chloride, magnesium combines with two
chlorine atoms to form magnesium chloride (MgCl2).
Molecular formulae of chlorides of sodium and magnesium are different.
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32. 9) Fluorine is the most reactive among the halogens.
Give scientific reasons :
1) Fluorine has the electronic configuration (2,7).
2) It requires only one electron to complete the octet.
3) The atomic size of fluorine is the smallest among the all halogens. Hence, the nuclear
attraction on the outermost electrons is maximum. Hence, fluorine is the most reactive
among the halogens.
10) Sodium is more metallic than Aluminium.
1) Metals give electrons. Sodium has electronic configuration(2,8,1). It has only one
electron in the outermost shell.
2) It can easily give the single electron in the outermost shell. Hence, sodium is a strong
metal.
3) Aluminium has electronic configuration (2,8,3). It has three electrons in the
outermost shell.
4) Donation of three electrons is more difficult than the donation of one electron. Hence,
sodium is more metallic than aluminium.
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33. 11) All the elements belonging to groups IB to VIIB, VIII are known as transition
elements.
1) The last two shells of the atoms of the elements belonging to groups IB to VIIB and VIII,
are incompletely filled. These elements shows variable valency.
Give scientific reasons :
2) These elements are placed between the most reactive metals on the left and non-
metals of the right. Hence all the elements belonging to B groups are known as transition
elements.
A summary of periodic properties and their variation in groups and periods is given below:
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34. Distinguish between :
1) Inert gases and Normal elements.
Inert gases Normal elements
1) The elements of zero group are
called inert gases or noble gases.
1) The elements of s-block and p-block
except zero group together are
called normal element.
2) The outermost shell of an atom of
an inert gas is saturated.
2) The outermost shell of an atom of a
normal element is incomplete.
3) Under normal conditions, these
elements do not take part in chemical
reactions.
3) Under normal conditions, these
elements take part in chemical
reactions.
4) These elements are gaseous at
room them premature.
4) These elements are solid, liquid or
gaseous at room temperature.
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35. Distinguish between :
2) Inert gases and transition elements.
1) Inert gases belong in to zero
Group. (18)
Inert gasesInert gases Transition elementsTransition elements
1) Transition elements belong to
Group IB to VIIB and VIII group.(Group
3 to 12)
2) The outermost shell of an atom of
an inert gas is saturated, in the case of
helium with 2 electron and in the case
of other gases with 8 electron.
2) The last two shells of an atom of a
transition element are incomplete.
3) Under normal conditions, these
elements do not take part in chemical
reactions.
3) Under normal conditions, these
elements take part in chemical
reactions.
4) These elements are gaseous at
room temperature.
4) These elements are solid metals at
room temperature.
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36. Back
Distinguish between :
3) Transition elements and inner transition
elements.
Transition elementsTransition elements Inner transition elementsInner transition elements
1) The last two shell of the atoms of
transition elements are incompletely
filled.
1) The last three shells of an atom of
inner transition element are
incompletely filled.
2) They belong to groups IB to VIIB,
and VIII (group 3 to 12) and they are
placed between s- and p- block.
2) They are placed in two separate
series (rows) at the bottom of the
periodic table.
3) They belong to d- block of the
periodic table.
3) They belong to f-block of the
periodic table.
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37. Distinguish between :
4) s-block elements and p-block elements.
s-block elementss-block elements p-block elementsp-block elements
1) The groups IA (1) and IIA (2)
together with hydrogen constitute
the s- block.
1) The group IIIA (13) to VIIA (17) and
the Zero group (18) constitute the
p- block.
2) They have one or two electrons in
the outermost shell.
2) They have three to eight electrons in
the outermost shell.
3) The elements of s-block (except
hydrogen) are all metals.
3) The elements of p-block include a
few metals, all non-metals and all
metalloids.
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38. CONTENT
1) Moseley’s contribution to the classification of elements. 2
2) Modern Periodic Table 3
3) Isotopes of Na 4
4) Sketch of the Modern Periodic Table. 5
5) Normal elements 6
6) Transition Elements 7
7) Inner transition elements 8
8) Inert gases 9
9) Main Features of the Long form of the Periodic Table. 10
10) Elements in first period 11
11) Elements in Second period 12
12) Elements in Third period 13
13) The periods in the modern periodic table. 14
14) The trends in the valences of the elements in a period. 15
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39. 15) Groups of the modern periodic table with reference to the
properties of the Elements.
16
CONTEST
16) Elements and their Electronic Configuration of the
Group IA and their valency.
17
17) The similarities in the chemical properties of the compounds
of alkali metals.
18
18) Elements of group IIA and their atomic numbers and
electronic configuration.
19
19) The similarities in the chemical properties of the compounds
of Alkaline earth metals.
20
20) Halogens 21
21) Similarities in the properties of the elements of Group VIIA
(Halogens) considering electronic configuration and valances.
22
22) Similarities in the chemical properties of the elements of
Group VIIA (17) (Halogens).
23
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40. 23) Gradation in the properties of the elements of Group VIIA (17)
(Halogens), considering the physical state of the elements.
24
CONTEST
24) Zero Group (18) Elements-Names and electronic
configuration.
25
25) FOUR BLOCKS OF PERIODIC TABLE BASED ON THE ELECTRONIC
CONFIGURATION.
26
26) PERIODIC TABLE – SHOWING 4-BLOCKS OF ELEMENTS 27
27) Metalloids or Zig-zag line in the modern periodic table 28
28) Scientific reasons : 1 to 3 29
29) Scientific reasons : 4 to 6 30
30) Scientific reasons : 7 and 8 31
31) Scientific reasons : 9 and 10 32
32) Scientific reasons : 11 and summary of properties of elements 33
33) Distinguish between : 1) Inert gases and Normal elements. 34
34) Distinguish between : 2) Inert gases and transition elements. 35
35) Distinguish between : 3) Transition elements and inner
transition elements.
36
36) Distinguish between : 4) s-block elements and p-block
elements. First Page Back Page Back
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