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The modern long form of periodic table was constructed by Neils Bohr based on modern periodic law proposed by Moseley.

Modern Periodic Table Chart
Modern periodic law
Salient features
Atomic radius
Ionization energy

LONG FORM OF MODERN PERIODIC TABLE
		GROUPS
		s-block		d-block										p-block
		1	2	3	4	5	6	7	8	9	10	11	12	13	14	15	16	17	18
		IA	IIA	IIIB	IVB	VB	VIB	VIIB	VIII			IB	IIB	IIIA	IVA	VA	VIA	VIIA	0
		ns¹																	ns²np⁶
P E R I O D S	1	₁H	ns²											ns²np¹	ns²np²	ns²np³	ns²np⁴	ns²np⁵	₂He
	2	₃Li	₄Be											₅B	₆C	₇N	₈O	₉F	₁₀Ne
	3	₁₁Na	₁₂Mg	(n-1)d^1-10 ns^1-2										₁₃Al	₁₄Si	₁₅P	₁₆S	₁₇Cl	₁₈Ar
	4	₁₉K	₂₀Ca	₂₁Sc	₂₂Ti	₂₃V	₂₄Cr	₂₅Mn	₂₆Fe	₂₇Co	₂₈Ni	₂₉Cu	₃₀Zn	₃₁Ga	₃₂Ge	₃₃As	₃₄Se	₃₅Br	₃₆Kr
	5	₃₇Rb	₃₈Sr	₃₉Y	₄₀Zr	₄₁Nb	₄₂Mo	₄₃Tc	₄₄Ru	₄₅Rh	₄₆Pd	₄₇Ag	₄₈Cd	₄₉In	₅₀Sn	₅₁Sb	₅₂Te	₅₃I	₅₄Xe
	6	₅₅Cs	₅₆Ba	57-71	₇₂Hf	₇₃Ta	₇₄W	₇₅Re	₇₆Os	₇₇Ir	₇₈Pt	₇₉Au	₈₀Hg	₈₁Tl	₈₂Pb	₈₃Bi	₈₄Po	₈₅At	₈₆Rn
	7	₈₇Fr	₈₈Ra	89-103	₁₀₄Rf	₁₀₅Db	₁₀₆Sg	₁₀₇Bh	₁₀₈Hs	₁₀₉Mt	₁₁₀Ds	₁₁₁Rg	₁₁₂Cn	₁₁₃Uut	₁₁₄Fl	₁₁₅Uup	₁₁₆Lv	₁₁₇Uus	₁₁₈Uuo
				f-block
		Lanthanoids		₅₇La	₅₈Ce	₅₉Pr	₆₀Nd	₆₁Pm	₆₂Sm	₆₃Eu	₆₄Gd	₆₅Tb	₆₆Dy	₆₇Ho	₆₈Er	₆₉Tm	₇₀Yb	₇₁Lu
		Actinoids		₈₉Ac	₉₀Th	₉₁Pa	₉₂U	₉₃Np	₉₄Pu	₉₅Am	₉₆Cm	₉₇Bk	₉₈Cf	₉₉Es	₁₀₀Fm	₁₀₁Md	₁₀₂No	₁₀₃Lr

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MODERN PERIODIC LAW

The modern periodic law was proposed by Moseley. He found the relation between atomic numbers (Z) and the frequencies (ν) of X-rays produced when the atoms of different elements are bombarded with cathode rays. The relation between the square root of frequency (√ν) of highest energy emission line, called K_α line, with the atomic number, Z was found to be linear.

The mathematical relation can be presented as:

√ν = a(Z-b)

Where a & b are constants, characteristic of elements.

Later on it was clearly established that an element can be characterized by its atomic number, Z and not by the atomic weight. It was also found that there is a relation between electronic configuration and properties of elements. The number of electrons in an atom and its electronic configuration are in turn are related to the atomic number.

Thus the modern periodic law can be stated as:

"The chemical and physical properties of elements are the periodic functions of their atomic numbers and electronic configurations."

The modern long form of periodic table was constructed based on above law. The following points are considered while constructing the periodic table.

* The elements in the periodic table are arranged in the increasing order of the atomic number.

* Every row, also called as period, in the periodic table starts with the filling up of differentiating electron into a new quantum shell.

* The elements in a vertical column called as group should get similar outer electronic configuration since it is observed that the elements with similar outer electronic configuration show similar chemical properties.

SALIENT FEATURES OF LONG FORM OF MODERN PERIODIC TABLE

The long form of modern periodic table consists of seven rows called periods and eighteen columns called groups.

Periods:

* Each period starts with an alkali metal and ends with an inert gas element.

* The first period is a very short period with only two elements i.e., Hydrogen (H) & Helium (He). In this period, the 1s orbital is being filled up.

₁H

₂He

* The second period starts with Lithium (Li) and ends with Neon (Ne) and contains 8 elements. It is called first short period. In this group, the 2s & 2p orbitals are being filled up.

₃Li

₄Be

₅B

₆C

₇N

₈O

₉F

₁₀Ne

* The third period also contain 8 elements i.e., from Sodium (Na) to Argon (Ar). It is called second short period. The 3s & 3p orbitals are being filled up in this period.

₁₁Na

₁₂Mg

₁₃Al

₁₄Si

₁₅P

₁₆S

₁₇Cl

₁₈Ar

* The fourth period is the first long period with 18 elements, it starts with Potassium (K) and ends with Krypton (Kr). It also includes 10 elements belonging to 3d series i.e., from Scandium (Sc) to Zinc (Zn). In this period, not only 4s & 4p and also the 3d orbitals are being filled up by electrons.

₁₉K

₂₀Ca

₂₁Sc

₂₂Ti

₂₃V

₂₄Cr

₂₅Mn

₂₆Fe

₂₇Co

₂₈Ni

₂₉Cu

₃₀Zn

₃₁Ga

₃₂Ge

₃₃As

₃₄Se

₃₅Br

₃₆Kr

* The fifth period is the second long period with 18 elements, it starts with Rubidium (Rb) and ends with Xenon (Xe). It also includes 10 elements belonging to 4d series i.e. from Yttrium (Y) to Cadmium (Cd). The 5s & 5p along with 4d orbitals are filled up by electrons.

₃₇Rb

₃₈Sr

₃₉Y

₄₀Zr

₄₁Nb

₄₂Mo

₄₃Tc

₄₄Ru

₄₅Rh

₄₆Pd

₄₇Ag

₄₈Cd

₄₉In

₅₀Sn

₅₁Sb

₅₂Te

₅₃I

₅₄Xe

* The sixth period is the longest period with 32 elements. It not only includes 10 elements belonging to 5d series i.e., Lanthanum (La), Hafnium (Hf) to Mercury (Hg) but also contains 14 elements belonging the 4f series called lanthanides (Cerium (Ce) to Lutetium (Lu)).

In this period, the 6s & 6p along with 4f & 5d orbitals are being filled up.

₅₅Cs

₅₆Ba

57-71

₇₂Hf

₇₃Ta

₇₄W

₇₅Re

₇₆Os

₇₇Ir

₇₈Pt

₇₉Au

₈₀Hg

₈₁Tl

₈₂Pb

₈₃Bi

₈₄Po

₈₅At

₈₆Rn

Lanthanoids

₅₇La

₅₈Ce

₅₉Pr

₆₀Nd

₆₁Pm

₆₂Sm

₆₃Eu

₆₄Gd

₆₅Tb

₆₆Dy

₆₇Ho

₆₈Er

₆₉Tm

₇₀Yb

₇₁Lu

Note: Lanthanum is also considered to be the part of f-block since its properties resemble more to lanthanoids.

* The seventh period is an incomplete period. It starts with Fr. It also includes the 14 elements belonging to 5f series called actinides (Thorium (Th) to Lawrencium (Lr)).

In this period, the 7s & 5f orbitals are filled up. Until recently this period is considered to be incomplete. The names of some of its elements are not yet finalized (like Uut, Uup etc.)

₈₇Fr

₈₈Ra

89-103

₁₀₄Rf

₁₀₅Db

₁₀₆Sg

₁₀₇Bh

₁₀₈Hs

₁₀₉Mt

₁₁₀Ds

₁₁₁Rg

₁₁₂Cn

₁₁₃Uut

₁₁₄Fl

₁₁₅Uup

₁₁₆Lv

₁₁₇Uus

₁₁₈Uuo

Actinoids

₈₉Ac

₉₀Th

₉₁Pa

₉₂U

₉₃Np

₉₄Pu

₉₅Am

₉₆Cm

₉₇Bk

₉₈Cf

₉₉Es

₁₀₀Fm

₁₀₁Md

₁₀₂No

₁₀₃Lr

Note: Actinium is also considered to be the part of f-block since its properties resemble more to actinoids.

* The Lanthanides and actinides are placed below the periodic table separately.

Groups:

* The 18 groups in the periodic table are numbered from 1 to 18 according to IUPAC convention.

However, according to American convention, these are also denoted by IA , IIA, IIIB, IVB, VB, VIB, VIIB, VIII (which actually includes 3 groups), IB ,IIB, IIIA, IVA, VA, VIA, VIIA and 0 (zero). This is based on maximum valency shown by elements in the group.

1	2	3	4	5	6	7	8	9	10	11	12	13	14	15	16	17	18
IA	IIA	IIIB	IVB	VB	VIB	VIIB	VIII			IB	IIB	IIIA	IVA	VA	VIA	VIIA	0

* The elements of IA to VII A groups i.e., 1, 2, 13, 14, 15, 16 & 17 groups are called as representative elements.

* The zero group (or 18th group) elements are called as inert gases or noble gases. This group includes He, Ne, Ar, Kr, Xe and Rn.

* The elements of IIIB to IIB i.e., from groups 3 to 12 are called as transition elements.

* However the Lanthanoids and Actinoids are also considered to be the part of IIIB group (i.e., group 3). These are usually called as inner transition elements.

* The elements present in a group show similar physical & chemical properties since they have similar outer electronic configurations.