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1. Inorganic Chemistry
Periodic Table
By- Deepak Sharma (Assistant Professor, HVPGR- Kadi)

2. Contents-
 History & Introduction
 Mendeleev’s Periodic Law
 Modern Periodic table
 Classification Of Elements
 Periodicity of Elements
 Valency
 Atomic Radius
 Ionization Potential (IP)
 Electron Affinity (EA)
 Electronegativity(EN)

3. History & Introduction
 Similar Properties Are Grouped Together In A Tabular Form
DOBEREINER
TRIADRULE [1817]
• Atomic weight of middle
element is equal to the
average atomic weight of
first and Third element.
NEWLANDOCTAVERULE
[1865]
• Properties Of Every 8th
Element was Similar To The
1st One
LOTHERMEYER’S
CURVE [1869]
• curve between atomic
weight and atomic volume
MENDELEEV’S
Periodic Table
[1869]
•The physical and chemical
properties of elements are the
periodic function of their atomic
weight

4. MENDELEEV’S
PERIODICTABLE
Physical And Chemical Properties Of Elements Are The
Periodic Function Of Their Atomic Weight

5. Characteristic
 It is based on atomic weight
 63 elements were known, noble gases were not discovered.
 12 Horizontal rows are called periods.
 Vertical columns are called groups and there were 8 groups in Mendeleev’s Periodic table.
 Each group up to VIIth is divided into A & B subgroups. “A” sub groups element are called normal
elements and “B” sub groups elements are called transition elements.
 The VIIIth group was consists of 9 elements in three rows (Transition metals group).
 The elements belonging to same group exhibit similar properties. Third bullet point here

6. Advantages
 Study of elements become easier.
 Some elements were discovered after Mendeleev periodic table.
 Eka aluminum-Gallium(Ga) Eka Boron - Scandium(Sc)
 Eka Silicon -Germanium(Ge) Eka Manganese -Technetium(Tc)
 Correction of doubtful atomic weights
e.g U, Be, In, Au, Pt.

7. Disadvantages
 Position of hydrogen
 Position of isotopes
 Anomalous pairs of elements – Ar-39.9, K-39
 Like elements were placed in different groups- Pt & Au
 Unlike elements were placed in same group.- Cu, Ag and Au placed in Ist group along
with Na, K

8. MODERN
PERIODICTABLE
The physical & chemical properties of elements are a
periodic function of the atomic number

9. Do You Have A Mobile?
Yes?
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10. Characteristic
 It was Modified Mendeleev periodic table
 Modern periodic table is based on atomic number
 9 vertical columns called groups- Ist to VIIth + VIIIth group + 0 group of inert gases.
 Inert gases were introduced in periodic table by Ramsay.
 7 horizontal series called periods.
 From this Bohr-Burry gave long form of periodic table.

11. Important points
 It consist of 7 horizontal rows (periods) and 18 vertical columns (groups)
 According to I.U.P.A.C. 18 vertical columns are named as 1st to 18th group.
 2nd period elements (Li, Be, B) Shows diagonal relationship with 3rd period elements (Mg, Al, Si),
so (Li, Be, B) are called Bridge elements.
 3rd period are called typical elements because they represent the properties of other element of
their respective group.
 In 6th period all types of elements are included (s, p, d & f)
 No inert gas in 7th period.
 Atomic No. of last inert gas element is 86.

12. Important points
 The group containing most electro positive elements - IA GROUP
 The group containing most electro negative elements - VIIA GROUP
 The group containing maximum number of gaseous elements - ZERO GROUP (18thGROUP)
 The group in which elements have zero valency - ZERO GROUP (18th GROUP)
 Number of Gaseous elements - 11 (H, N, O, F, Cl + Noble gases)
 Number of Liquid elements - 6 (Cs, Fr, Ga, Hg, Br, Uub)
 Bromine is the only non-metal which exists in liquid form.

13. Important points
 1st period has all the elements in gaseous form(H, He)
 Zero group (18th group) have all the elements in gaseous form.
 Number of Solid elements - 89 (if discovered elements are 105) - 95 (if discovered elements are 112)
 No p-block elements in 1st and 7th periods.
 2nd period contains maximum total number of four gases which are : N,O, F, Ne elements.
 Elements of 3rd period (Na, Mg, Al, Si, P, S and Cl) are called typical elements. These are 7 in
numbers.
 Coin Metals – Cu, Ag, Au

14. CLASSIFICATION OF
ELEMENTS
Elements can be divided in four parts on the basis of
electronic configuration.

15. Bohr classification
Inert gas elements
Normal or Representative elements
Transition elements
Inner transition elements

16. Inert gas elements
 The elements in which ultimate orbit is completely filled up are called inert gas
elements.
 General electronic configuration is ns2np6 (Except He = 1s2)
 Because of most stable configuration, they are very less reactive. Hence known as
noble gas or inert gas.
 These elements are present in .0. group or 18th group and 1st to 6th period of
periodic table.
 Number of inert gas elements are 6 (One in each period up to 6th) He, Ne, Ar, Kr,
Xe, Rn

17. Normal Or Representative Elements
 The elements in which ultimate orbit is incomplete, while penultimate orbits are
complete are called normal elements.
 These elements lies in group IA to VIIA and period 1st to 7th
 Elements of 2nd period known as bridge elements.
 Elements of 3rd period (Na, Mg, Al, Si, P, S and Cl) are called typical elements.
These are 7 in numbers.

18. Transition Elements
 The elements in which both ultimate (n) as well as penultimate shells (n - 1) are
incomplete either in atomic state or in some oxidation state are called transition
elements.
 Group - IIIB to VIIB + VIII + IB
 Periods - 4th to 7th
 Electronic configuration (n - 1)d1-10 ns1 or 2
 Total number of d-block elements = 40
 Total number of transition elements = 36 (Except Zn, Cd, Hg and Uub)

19. Inner Transition Elements
 The elements in which all the three shells that is ultimate(n) penultimate(n-1) and pre
or antepenultimate (n - 2) shell are incomplete are called inner transition elements.
 58Ce = [Xe] 6s2, 5d1, 4f1
 Electronic configuration - (n - 2)f1-14 (n-1)d0 or 1 ns2
 These are 28 in number.
 Group - IIIB
 Period - 6th & 7th
 Inner transition elements are divided into two series.

20. Classification on the Basis Of Subshell
s- block elements
b- block elements
d- block elements
f- block elements

21. S-block Elements
 In these elements last electron enters in s-subshell.
 Groups - IA, IIA + 0 group (He only)
 Period - 1st to 7th
 Electronic configuration - ns1 – 2
IA group n = 1 to 7 IIA group n = 2 to 7
 Total s-block elements are (14) (including H and He)
 Total s-block metals are (12) (excluding H), H is non-metal

22. p-block Elements
 Last electron enters in p-sub shell
 Group - IIIA (13) to VIIA(17) + 0 group (18) (except He)
 Period - 2nd to 6th
 Electronic configuration - ns2 np1 - 6
 Total p-block elements - (30)
 All type of elements are classified in it- Metal, Non- Metal and Metalloids

23. d-block Elements
 Last electron enters in (n - 1)d subshell
 Group - IIIB . VIIB, VIII, IB, IIB or group 3 to 12 (IUPAC)
 Period - 4th to 7th
 Electronic configuration - (n - 1)d1 - 10 ns1 or 2
 Total d-block elements . (40)
 Total transition elements - (36), If 112 elements are included in periodic table.
 IIB elements (Zn, Cd, Hg, Uub) are d-block elements but not transition elements.

24. f-block Elements
 Differentiating electron enters in (n - 2)f subshell.
 Group - IIIB
 Period - 6th and 7th
 From atomic number 58 - 71, 6th period ; Lanthanide series 4f1 - 14 5d0 or 1 6s2
 90 - 103, 7th period; Actinide series 5f1 - 14 6d0 or 1 7s2
 Total number of f-block elements - (28)
 All the actinides are radioactive elements.
 Transuranic actinides are man made elements (Np93 - Lw103)
 Lanthanides are found rarely on earth so these are called rare earth metals.

25. PERIODICITY OF
ELEMENTS
The regular gradation in properties from top to bottom
in a group and from left to right in a period is called
periodicity in properties.

26. Why Periodicity ?
 To study variations among elements.
 In a period, the ultimate orbit remain same, but the no. of electron gradually
increases.
 In a group, the no. of electron in the ultimate orbit remains same, but the values of n
increases.
 The cause of periodicity in properties is due to the same outermost shell electronic
configuration coming at regular intervals.
 In the periodic table, elements with similar properties occur at intervals of 2, 8, 8, 18,
18 and 32. These numbers are called as magic numbers.

27. Periodic Properties
Valency
Atomic Size
Ionization Potential
Electron Affinity
ELECTRON Negativity

28. VALENCY
It is defined as the combining capacity of the
elements.

29. Concept
 The word valency is derived from an Italian word “Valentia” which means combining capacity
Valency
Old
Based on H &
O
New
Based on e-
Configuration

30. Old Concept - Based on H & O
 Valency with respect to Hydrogen- It is defined as the number of hydrogen or Chlorine atoms
attached with a particular element.
 IA IIA IIIA IVA VA VIA VIIA
NaH MgH2 AlH3 SiH4 PH3 H2S H-Cl
1 2 3 4 3 2 1
 Valency with respect to oxygen- It is defined as twice the number of oxygen atoms attached with
a particular atom.
 IA IIA IIIA IVA VA VIA VIIA
 Na2O MgO Al2O3 SiO2 P2O5 SO3 Cl2O7
1 2 3 4 5 6 7

31. New concept- Based on e- Configuration
 Valency for IA to IVA group elements is equal to number of valence shell electron and
 from VA to zero group, it is [8 - (number of valence electron)].
 IA IIA IIIA IVA VA VIA VIIA 0
ns1 ns2 ns2np1 ns2np2 ns2np3 ns2np4 ns2np5 ns2np6
1 2 3 4 3 2 1 0
 Note: All the elements of a group have same valencies because they have same number of
valence shell electrons.

32. ATOMIC RADIUS
It is distance between outermost electron and
nucleus.

33. Concept
 Atomic radius depends on the type of chemical bond between atoms in a molecule
Radius
Covalent Ionic Metallic
Vander
Waal's

34. Factors Affecting Atomic Radius
 Vander’s Waal radius > Metallic radius > Covalent radius
 Atomic Radius α
𝟏
Effective nuclear charge
Ex- Li > Be > B > C > N > O > F
 Atomic radius α No. of shells Ex- Li < Na < K < Rb < Cs
 Atomic radius α Screening effect
 Atomic Radius α
𝟏
Magnitude of positive charge
Ex- Mn > Mn+2 > Mn+3 > Mn+4
 Atomic size α Magnitude of negative charge Ex- O < O- < O-2
 Atomic Radius α
𝟏
Bond order
Ex- > N - N < > -N = N- > -N ≡ N-

35. IONIZATION POTENTIAL
Minimum energy required to remove most loosely
held outermost shell electron in ground state from an
isolated gaseous atom is known as ionization
Potential.

36. Concept
 For an atom M, successive ionization energies are as follows -
 M + E1 → M+ + e- E1 = IP1
 M+ + E2 → M+2 + e- E2 = IP2
 M+2 + E3 → M+3 + e- E3 = IP3
 IP is always an endothermic process (ΔH= +ve)
 IP α
𝟏
Atomic Radius
Ex- Li > Na > K > Rb > Cs
 IP α
𝟏
Screening Effect
 (Penetration power) is - s > p > d > f Ex- IP of Be > IP of B
 IP of Half filled orbital is higher. Ex- IP1 order is C < O < N
IP3 > IP2 > IP1

37. ELECTRON AFFINITY
The amount of energy released or absorbed when
electron is added to the valence shell of an isolated
gaseous atom

38. Concept
 Mostly energy is released in the process of first E.A.
 EA of neutral atom is equal to I.P. of its anion.
 EA α
𝟏
Atomic Radius
Ex- Li > Na > K > Rb > Cs
 EA α
𝟏
Screening Effect
 EA α Zeff
 EA of full filled orbitals is less then Half filled orbital.
 Due to small size of fluorine, electron density around the nucleus increases. The incoming electron
Suffers more repulsion. So EA of Halogen Cl > F >Br > I

39. ELECTRO NEGATIVITY
The tendency of an atom to attract shared electrons
towards itself is called electronegativity

40. Concept
 EN and EA both have tendency to attract electrons but electron affinity is for isolated atoms.
Where as electron negativity is for bonded atoms.
 A polar covalent or ionic bond of A-B may be broken
as (a) A-B → A- + B+ (EN A > EN B)
or (b) A-B → A+ + B- (EN A < EN B)
 There is no unit of electronegativity as EN is tendency of a bonded atom not an energy.

41. Concept

42. Examples
 Out of following, which has the highest electronegativity?
(1) H (2) Li (3) Na (4) Be Sol. Answer (1)
 Which of the following has highest electron affinity?
(1) Na (2) Li (3) K (4) Rb Sol. Answer (2)
 The element which has highest 2nd ionization energy is
(1) Na (2) Mg (3) Ca (4) Ar Sol. Answer (1)
 The first ionization potentials of Na, Mg, Al and Si are in the order
(1) Na < Mg > Al < Si (2) Na < Mg < Al > Si (3) Na > Mg > Al > Si (4) Na > Mg > Al < Si
Sol. Answer (1)

43. Examples
 Which of the following has largest size?
(1) H– (2) He (3) Li+ (4) Be+ 2 Answer (1)
 If the atomic number of an element is 33, it will be placed in the periodic table in the
(1) 1st group (2) 3rd group (3) 15th group (4) 17th group Sol. Answer (3)
 Which of the following elements do not belong to the family indicated?
(1) Cu – Coinage metal (2) Ba – Alkaline earth metal
(3) Zn – Alkaline earth metal (4) Xe – Noble gas Sol. Answer (3)

44. Examples
 Which among the following elements has the highest value for third ionization energy?
(1) Mg (2) Al (3) Na (4) Ar Sol. Answer (1)
 The first electron affinity values of ‘O’, S & Se are given correctly as
(1) O > S > Se (2) S > Se > O (3) Se > O > S (4) Se > S > O Sol. Answer (2)
 The element which has highest IInd I.E.?
(1) Li (2) Be (3) K (4) B Sol. Answer (1)
 The element which has highest electron affinity?
(1) Oxygen (2) Sulphur (3) Nitrogen (4) Phosphorus Sol. Answer (2)

45. Examples
 Which one of the following order is correct?
(1) I > I+ > I– (radii)
(2) I– > I > I+ (radii)
(3) I– > I > I+ (Ionization energy)
(4) I+5 < I+ < I+7 (Ionization energy) Sol. Answer (2)
 Which of the following configuration is associated with the biggest jump between first and
second ionization energy?
(1) 1s22s22p5 (2) 1s22s22p63s1 (3) 1s22s22p4 (4) 1s22s1 Sol. Answer (4)

46. Thank You