Welcome to the project dedicated to the remarkable Periodic Table of Elements! Prepare to embark on an exciting exploration of the building blocks of our universe through our comprehensive presentation. Our presentation offers a captivating visual representation of the Periodic Table, showcasing the elements and their essential properties. Each element is presented with its atomic number, symbol, and atomic mass, providing a clear overview of the entire table. Delve deeper into the presentation and unlock a wealth of knowledge about each element. Discover their unique characteristics, such as their physical and chemical properties, common uses, and even their historical significance. Engaging narratives and captivating illustrations bring the elements to life, making the learning experience both enjoyable and informative. Whether you're a student, a science enthusiast, or simply curious about the elements that shape our world, our presentation on the Periodic Table will enlighten and inspire. Join us on this educational journey as we unravel the mysteries and marvels of the elements that surround us.

1. THE
PERIODIC
TABLE
BY ISHANI
VERONICA

2. SALIENT FEATURES OF THE MODERN PERIODIC
TABLE
● The shortcomings of the Mendeleev’s periodic table were overcome by
Henry Moseley and he put forward the Modern Periodic Table in which
the elements are arranged in the increasing order of their atomic
numbers
● Modern Periodic Law: The physical and chemical properties of all
elements are the periodic functions of their atomic number
● The properties of the elements are repeated after regular intervals
● Periodic table may be defined as the table in which the elements are
arranged in the increasing order of their atomic numbers

3. PERIODS AND GROUPS
P E R I O D S
● The horizontal rows of elements in a periodic table are called periods
● There are seven periods in the long form of the periodic table
● The first period consists of 2 elements called the shortest period
● The second and third periods consist of 8 elements called short periods
● The fourth and fifth periods contain 18 elements each and are called long periods
● In the modern periodic table, period six contains the lanthanide series which are
the rare earth elements, sixth period consists of 32 elements and it is the longest
period.
● Radioactive elements (actinides) present in period seven, seventh period is yet an
incomplete period

4. PERIODS AND GROUPS
G R O U P S
● The modern periodic table has eighteen vertical columns known as groups,
arranged from left to right in the order: IA, IIA, IIIB, IVB, VB, VIB, VIIB, VIII
(three columns), IB, IIB, IIIA, IVA, VA, VIA, VIIA and Zero.
● A group is determined by the number of electrons present in the outermost
shell.
● Elements in groups 1, 2 and 13 to 17 are called normal elements. Reactive
metals are placed in groups 1 and 2.
● Elements in groups 3 to 12 are called transition elements. Transition elements
[metals] are placed in the middle.
● Group 18 at the extreme right contains noble or inert gases.
● Non-metals are placed in the upper right corner of the periodic table.

5. PROPERTY OF ELEMENTS
● The elements can be classified as: Representative/Normal elements, Transition
elements, Inert gases or Noble gases, Inner Transition elements which include
Lanthanides and Actinides
● The properties which reoccur after a regular interval in periodic table are called as
periodic properties and the phenomenon is called as periodicity
● The major cause for the periodicity is the reoccurrence of similar outer electronic
configuration.
● In a particular group the valence electrons remains the same and thus the valency
is also the same. Hence the properties are same.
● According to the Modern Periodic Law the properties of an element depends upon:
Atomic size, Metallic character, Non -metallic character, Ionisation energy, Electro
affinity, Electronegativity.

6. ALKALI METALS
● Highly electropositive in nature
● Good reducing agents
● Valency is +1
● They have low ionization potential
● They form metal halides
● Good conductors of electricity
● They have the largest atomic size in their periods
● They react vigorously with dilute acids and cold water to liberate
hydrogen.
● They’re reactivity increases on moving down the group. Aakanksha sakhare

7. (a) An element Z has atomic number 16. Answer the
following questions on Z: [i]. State the period and
group to which Z belongs. [ii]. Is Z a metal or a non-
metal?
(b) If an element A belongs to Period 3 and Group II,
then it will have
A]. 3 shells and 2 valence electrons
B]. 2 shells and 3 valence electrons
C]. 3 shells and 3 valence electrons
D]. 2 shells and 2 valence electrons[2014]
[2014]

8. (c) Give reasons for the following: Alkali metals
are good reducing agents.
(d) Which one of the following is not true of
metals?
A)Metals are good conductors of electricity.
B)Metals are malleable and ductile.
C) Metals form non-polar covalent compounds.
D)Metals will have 1 or 2 or 3 electrons in their
valence shell.
[2012]
Aakanksha sakhare
[2012]

9. Ionization potential (ionization energy) :
❏ The energy required to remove an electron from a neutral isolated
gaseous atom and convert it into a positively charged gaseous ion.
M(g) + I.E. → M+(g) + e-
❏ Unit of I.P. = eV
❏ Energy required to remove 1st electron - is called first I.P.
M → M+ + e- [ first I.P. is less ]
atom ion electron
❏ Energy required to remove 2nd electron - is called second I.P.
M+ → M++ + e- [second I.P. is more ]
Ishani Ravi Kabbur

10. ★ Atomic Size Increases ----- Ionization Potential Decreases
★ Nuclear Charge Increases ----- Ionization Potential
Increases
Ishani Ravi Kabbur
➢ Factors That Affect I.P.
❖ Trends in I.P.
Across a period: I.P. tends to increase as one moves from left to right
across a period.
Down a group: I.P. tends to decreases as one moves down a group.

11. Electron Affinity [E.A.]
❏ The amount of energy released when an atom in the gaseous state
accepts an electron to form an anion.
X + e- → X- + energy liberated
Atom electron anion [1st electron affinity]
❏ Unit of Electron Affinity = eV
★ Atomic Size Increases ------ Electron Affinity Decreases
A small atom takes up electrons more readily than a large atom.
★ Nuclear Charge Increases ----- Electron Affinity Increases
Increases the tendency of the atom to accept electrons.
Ishani Ravi Kabbur

12. ➢ Variation (trends) in electron affinity:
❏ In a period, i.e., from left to right the electron affinity
increases.
➢ Down a group:
❏ Moving from the top to the bottom in a group, causing a
net decrease in E.A.
❏ Inert gases have zero electron affinity due to their stable
electronic configuration.
Ishani Ravi Kabbur

13. Electronegativity-
★ The tendency of an atom in a molecule to attract the
shared pair of electrons towards itself is called
electronegativity.
Electronegativity values too depend on:
(i) Size of atom: The greater the size of the atom, the lesser the
electronegativity.
(ii) Nuclear charge: The greater the nuclear charge, the greater the
electronegativity.
Ishani Ravi Kabbur

14. Trends in electronegativity-
➢ Across a period:
❏ Electronegativity increases from left to right in a period.
➢ Down a group:
❏ Electronegativity decreases down a group.
★ Generally, metals show lower electronegativity as compared to non-
metals. Thus metals are electropositive and non-metals are
electronegative.
Ishani Ravi Kabbur
★ In periodic table-
★ Fluorine → most electronegative
★ Caesium → least electronegative
★ Noble gases have complete octet and hence do not
attract electrons to itself.

15. Ishani Ravi Kabbur

16. (i) Which element would be expected to have the highest
electronegativity?(2007)
(ii) What happens to the atomic size of elements on moving from top to bottom
of a group?(2008)
(iii) Which of the elements has the greatest electron affinity among the
halogens?(2008)
(iv) If an element has a low ionisation energy then it is likely to be
…………..(metallic / non-metallic). (2008)
(v) 1) Be, Mg, Ca, Sr, Ba are group 2 metals. Which of these metals will form
ions most readily and why?
2) What property of an element is measured by electronegativity?
(2008)
Ishani Ravi Kabbur

17. (vi) Among Period-2 elements --
Lithium Carbon
Fluorine Neon
(2009)
(vii) Down the group, electron affinity……………(increases, decreases,
remains same)(2011)
(viii) Ionisation potential of the element increases across a period. Give
reason.(2012)
(ix) Give one words or phrase for: The amount of energy released when an
atom in the gaseous state accepts an electron to form an anion.(2014)
Ishani Ravi Kabbur

18. (x) Among the elements give below, the element with the least
electronegativity is:
(A)Lithium
(B)Carbon
(C)Boron
(D)Fluorine
(2015)
Ishani Ravi Kabbur

19. Ishani Ravi Kabbur