9 Class- Periodic Table of Elements

Periodic Table of Elements Class 9th Chemistry Notes

Periodic table of elements is important chapter in many schools' science & chemistry 9th 10th class books. More than 115 elements have been discovered which need to be arranged systematically, first elements were classified as metals and nonmetals. This chemistry notes on periodic table of elements contains all basic information about periodic table for learning purposes.

 

History of classification of elements

•       Prout’s Hypothesis – 1815
•       Dobereiner’s Triads – 1829
•       Newland’s Law of Octaves – 1863
•       Lother Meyer Curves – 1869
•       Mendeleev’s Periodic Table – 1869
•       Modern Periodic Laws of Moseley -1913
•       Modern Periodic Table (of 18 columns) 

 Prout’s Hypothesis

According to this hypothesis atomic mass of elements is multiple of mass of hydrogen atom. So, elements are related to each other on the basis of their atomic masses. 

It fails due to the reason that some elements do not have atomic mass in whole no. (Like chlorine have atomic mass of 35.5).

Dobereiner’s Triads

According to Dobereiner’s triads elements arranged in the group of three elements so that atomic mass of central element is appropriate mean of 1^st and 3^rd element. These groups of three elements are known as Dobereiner’s triads.

Example-

Element                                                           
 Li                Na                  K

Atomic Mass                                              
7                 23                  39

Mean of Atomic Masses of 1^st and 3^rd elements is (7+39)/2  =   46/2   =  23

Drawback of Dobereiner’s triads: All elements are not arranged in triads.

Newland’s Law of Octaves

According to Newland’s Law of Octaves elements arranged in the group of 8 elements and every 8^th element is similar to the 1^st element.

Li         Be         B        C          N         O           F

Na        Mg       Al        Si         P          S          Cl 

Drawback of Newland’s Law of Octaves:

Heavy elements do not follow this law, inert gases disturb the order of octave.

Lother Meyer Curves

In 1869, Lother Meyer derived following conclusion by obtaining information from graph between the atomic weight at x-axis and atomic volume at y-axis.

1.     Elements which have similar properties found on the same position on the graph curves.

2.     All alkali metals like Li, Na, K, Rb, Cs, and Fr found at highest peak of curve.

3.     Halogens like F, Cl, Br and I are found on ascending portion of curve.

4.     Alkaline earth metals like Mg, Ca, Sr, Ba and Ra are found on descending portion of curve.

5.     Elements which do not melt easily like Be, B, C, Al, Si, Cu etc. are found at lowest point of curve.

On the basis of above conclusions Lother Meyer give periodic Law:

                                                                                                  According to Lother Meyer periodic law – “Atomic volume of elements are periodic function of their atomic weights”.

Periodic Table

To classify elements a chart is prepared in which elements are arranged in rows and columns. These elements are arranged in table in such a way that the elements with similar properties are repeat after some intervals; also, elements with similar properties are put in same column below one another. 

In periodic table vertical columns are called group while horizontal rows are called periods. In periodic table this repetition of properties in regular interval is known as periodicity. Read below chemistry notes of periodic table like Mendeleev periodic table, Mosley periodic table, Modern periodic table etc.

Mendeleev’s Periodic Table

In Mendeleev’s Periodic Table, Mendeleev classify elements according to their atomic masses and arranged these elements in table according to their increasing order of atomic masses.

Mendeleev’s Periodic Law

According to Mendeleev’s Periodic Law – “Physical and chemical properties of elements are periodic function of their atomic masses”.

Mendeleev’s Periodic Table contains seven horizontal rows known as periods and nine vertical columns known as groups.

Groups of Mendeleev’s Periodic Table

1.     In original Mendeleev’s Periodic Table only 8 groups present because zero group contains noble gases is added later after discovery of noble gases.

2.     So, total vertical column is 9 including group 1 to 8 and Zero group.

3.     Group 1 to 7 are divided into two subgroups (A and B) each.

4.     In eighth group, three elements found together in each period (from fourth period onward) known as transition triplet.

Periods of Mendeleev’s Periodic Table

1.     Mendeleev’s Periodic Table has seven periods.

2.     First period is known as very short period because contain only two elements.

3.     Second and Third period is known as short period because contain only 8 elements each.

4.     Fourth and Fifth period is known as long period because contain 18 elements each.

5.     Sixth period is known as very long period because contain 32 elements each, 18 elements in table and remaining 14 elements called Lanthanides (from atomic no. 58 to 71)

6.     Seventh period is known as incomplete period because it contains only 24 elements and some places are left vacant for elements as they are not known yet. 10 elements in the table and remaining 14 elements called Actinides (from atomic no. 90 to 103) placed outside at bottom of periodic table.

Demerits of Mendeleev’s Periodic Table

These below points are some Demerits of Mendeleev’s Periodic Table

1.     Position of Hydrogen: Hydrogen is placed in 1^st as well as in 7^th group because its properties are similar to both groups, which is not explained well.

2.     Elements which have similar properties are placed apart in different groups.

Example: Copper and Mercury with similar properties placed in group first and second.

3.     Elements with different properties are placed in one group.

Example: Coin metals like Li, Na, K, Rb, Cs.

4.     Atomic weights are not kept in serial order.

Example: Argon with higher atomic weight 39.948 is placed before potassium, which have lower atomic weight of 39.102

5.     Position of isotope is not proper because all isotopes of elements are placed in one group though the atomic weights of isotopes are different.

6.      Eighth group elements position is not appropriate because elements put in triplet form.

7.     Rare earth elements (Lanthanides and Actinides) position is not proper so they placed outside at bottom of periodic table.

Modern Periodic Law and Modern Periodic Table

Moseley in 1913, after doing many experiments comes to a conclusion that the elements should be arranged as per their atomic no. and not according to atomic masses. As atomic no. is fundamental property of all elements of periodic table. So, Mosley gives a new law which is called is Modern Periodic Law.

Modern Periodic Law

According to Modern Periodic Law- “Physical and Chemical properties of elements are periodic function of their atomic numbers”.

Long Form of Periodic Table

Bohr Bury invented new periodic table, which is called as Long Form of Periodic Table. This Long Form of Periodic Table is also known as Modern Periodic Table.

Special features of Modern or Long Form of Periodic Table

These below are Special features of Modern or Long Form of Periodic Table

1.     18 vertical columns known as groups.

2.     Horizontal rows known as periods.

3.     Light metals – These are elements of periodic table of group 1 and 2.

4.     Heavy metals or Transition metals - These are elements of periodic table of group 3, 4, 5, 6, 7, 8, 9, 10, 11 and 12.

5.     Non-Metals – These are elements of periodic table of group 13, 14, 15, 16 and 17.

6.     Zero group – These are elements of periodic table of group 18.

Properties of periods

1.     All periods start with alkali metal and end with noble gases.

2.     If we see table, it is very clear that from 1^st to 7^th period there is an addition of one shell in each period like n=1,2,3,4,5…

Properties of groups

1.     In any group, outermost shell electrons are known as valance electrons and these electrons are same so main properties of elements of group is similar.

2.     Elements are divided into four blocks, which is s, p, d, f   according to valance electrons.

3.     s-block elements – elements of 1 and 2 group.

4.     p-block elements – elements of 13 to 18 group.

5.     d-block elements – elements of 3 to 12 group.

6.     f-block elements – elements of the Lanthanide and Actinide series.

7.     Representative Elements – elements of s-block and p-block collectively called as Representative elements also known as Normal elements or Typical elements.

8.     Transition Elements – elements of d-block.

9.     Inner Transition Elements – elements of f-block, also known as Rare Earth Elements.

10.                         Alkali Metals – elements of 1^st group.

11.                         Alkaline Earth Metals – elements of 2^nd group.

Solution for the demerits of Mendeleev’s Periodic Table in the Long Form of Periodic Table (or Modern Periodic Table)

1.     Mendeleev’s Periodic Table contains some heavy elements placed before lighter elements, this problem is solved automatically in Modern Periodic Table

2.     All isotopes of an element have same atomic number so no need to place them separate.

3.     All inert gases (or noble gases) got their appropriate place in zero group (or 18^th group).

4.     Mendeleev’s Periodic Table have problem with 8^th group, but it is resolved in Modern Periodic Table as it is divided into three groups.

Drawback of Modern Periodic Table

1.     Position of Hydrogen is still not clear in Modern Periodic Table.

2.     Position of f-block elements (Lanthanides and Actinides) is not proper as these placed at bottom, separately from periodic table that is impractical.

Periodic Properties of the Elements

Periodic properties are the properties of the elements which depend on their electronic configuration and these properties changes on moving down in the group and on moving left to right in the period of the periodic table. Some periodic properties are atomic size, electron affinity, ionization energy, metallic and non-metallic properties etc. are the main periodic properties.

Atomic Size

Size of any atom is explained with the help of atomic radius.

Atomic Radius

The distance between outermost shell electrons and centre of nucleus of isolated atom is called atomic radius.

There are two hypotheses for the calculation of atomic radius i.e.

1.     Van der Waals Radii

It is the one half of the distance between the two adjacent atoms nuclei centres, is known as Van der Waals radii.

Van der Waals radii is calculated as follows, first calculate the distance from the centre of nuclei of one atom to centre of nuclei of another adjacent atom in solid state of same substance. Then divide this distance by two. Van der Waals distance is represented by Angstrom A.

Where, 1 A = 10^-8 cm.

2.     Covalent Radii

It is the one half of the distance between the diatomic molecule nuclei centres, is known as Covalent Radii.

Covalent radii is calculated as follows, first calculate the distance from the centre of nuclei of one atom to centre of nuclei of another atom in diatomic molecule containing covalent single bond. Then divide this distance by two.

 

  Isolated Atom

 Isolated atom is an absolutely alone single atom.

  Periodicity in Atomic Size

  In Period: On moving left to right in any period atomic size decreases because atomic radii decreases, As electrons are attracted towards nucleus due to increasing nuclear charge.

  In Group: On moving down in any group atomic size increases because atomic radii increase, as more electrons shells added.

  An ionic radius of cation is smaller than its normal atom while that of anion is larger than its normal atom.

  Cations are formed by loss of electron or electrons and carry positive charge.

  Anions are formed by gain of electron or electrons and carry negative charge.

  Ionization Energy

The energy required for the removal of one electron from the isolated atom in gaseous state is called ionization energy.

  Ionization Energy is represented by I.E.

  Ionization Energy is expressed in Electron Volts per Atom or Kilo Joules per Mole or Kilo Calorie per Mole. Ionization Energy is also known as Ionization Potential.

  Equation for I.E.

  Atom (g) + Ionization Energy (I.E.) ---> Cation + Electron (e^-) 

  Removal of further electron from cation is difficult so value of Ionization Energy kept on increasing.

  I.E.₁ < I.E.₂ < I.E.₃ < I.E.₄ …………………………………..

  Periodicity in I.E. (Ionisation Energy)

  In Period: On moving left to right in any period ionization energy increases because nuclear charge increases with the increasing atomic number, so more energy required to remove electron. Therefore value of I.E. increases on moving left to right in any period.

  In Group: On moving down in any group ionisation energy decreases because atomic size increase, as more electrons shells added.

  Electron Affinity

                                    The amount of energy release as a result of addition of electron in any atom in gaseous state to form anion is known as Electron Affinity.

  Electron Affinity is represented by E.A.

  Electron Affinity is expressed in Electron Volts per Mole or Kilo Joule per Mole

  Values of all electron affinity are negative except first Electron Affinity which is positive.

  Periodicity in E.A. (Electron Affinity)

  In Period: On moving left to right in any period the value of Electron Affinity increases because atomic size decreases, so amount of energy released is more.

  In Group: On moving down in any group, the value of Electron Affinity decreases with some irregularities.

Metallic and Non-Metallic characters

 In Period: On moving left to right in any period Metallic character decreases and Non-Metallic character increases.

  In Group: On moving down in any group Metallic character increases and Non-Metallic character decreases.

  In Periodic Table: Metallic elements are found on left hand side and Non-Metallic elements are found on right hand side.

Metalloids

The elements which are neither metals nor non-metals are known as metalloids. 

Example of Metalloids: B, Si, As, Te etc.

What is the last element of periodic table?

The last element in the periodic table is called Oganesson (Og). It's element number 118, which means it's the 118th element in the periodic table. Oganesson is a special element because scientists had to create it in a laboratory; it doesn't exist naturally on Earth. It was named after a famous Russian physicist named Yuri Oganessian.

What is the first element of periodic table?

he first element in the periodic table is Hydrogen (H). Hydrogen has the atomic number 1, which means it is the very first element on the periodic table. It is the lightest and most abundant element in the universe.

Hydrogen was discovered as an element by the British scientist Henry Cavendish in 1766. He referred to it as "inflammable air" because of its flammability when it reacts with oxygen. Cavendish's work was essential in identifying and characterising hydrogen as a distinct element.

 

High resolution periodic table of elements

Below is the high-resolution periodic table of elements image for learning purpose for science students.   

Do you know, at room temperature number of liquid elements in periodic table exists?

There are two elements on the periodic table that are usually in liquid form when it's not too hot or not too cold (that is at room temperature and standard atmospheric pressure). These two elements are Mercury (Hg) and Bromine (Br).

1. Mercury (Hg): Mercury is a metal that stays liquid at room temperature. It's the only metal that does this. Think of it like a silvery liquid.
2. Bromine (Br): Bromine is another element that is a liquid at room temperature. It's not metal but belongs to a group called halogens. It looks like a reddish-brown liquid.

Most other elements of periodic table are either solid (like a rock) or gas (like the air that we breathe) at room temperature.

Periodic Table of Elements Image

Below is the image of periodic table of elements.

 

Oxidation number of common elements in periodic table

Below is the table for oxidation no. of common elements in periodic table. These are general oxidation states and may vary for specific compounds. 

Serial No.	Element Name	Element Symbol	Atomic Number	Common Oxidation Numbers
1	Hydrogen	H	1	+1, -1
2	Helium	He	2	0
3	Oxygen	O	8	-2
4	Sodium	Na	11	1
5	Chlorine	Cl	17	-1
6	Iron	Fe	26	+2, +3
7	Copper	Cu	29	+1, +2
8	Zinc	Zn	30	2
9	Silver	Ag	47	1
10	Iodine	I	53	-1, +1, +5, +7

 For oxidation states of all other elements of periodic table visit our chemistry notes on the same, whose link is given below-

Oxidation number of all elements in periodic table (chemistrynotesinfo.com)

    Also Learn From these Basic Chemistry Chapters-

•  Atomic Structure
•  Periodic Table of Elements
•  Chemical Bonding and Reactions
•  Chemical Reactions and Equations
•  Acids, Bases and Salts
•  Metals and Non-Metals
•  Carbon and its Compounds
•  Periodic Classification of Elements

=> 9th 10th Class Science - Periodic Table of Elements Podcast-