Periodic Classification of Elements

Periodic Classification of Elements
Periodic Classification of Elements


 1. Did Dรถbereiner’s triads also exist in the columns of Newlands’ Octaves? Compare
and find out.

Solution:

Dรถbereiner’s triads did exist in the columns of Newlands’ Octaves; For example, the

elements

Lithium (Li), Potassium (K) and Sodium (Na) constitute a Dobereiner’s Triad but are also

found in the second column of Newland’s Octaves.

2. What were the limitations of Dรถbereiner’s classification?

Solution:

(i) They were not applicable for very low mass or very high mass elements.

(ii) All the elements couldn’t fit into Dobereiner’s triads.

(iii) As the methods to calculate atomic mass improved, Dobereiner’s triads validity

began to decrease. For example, in the triad of F, Cl and Br, the arithmetic mean of

atomic masses of F and Br are not equal to the atomic mass of CI.

3. What were the limitations of Newlands’ Law of Octaves?

Solution:

 Limitations of Newlands’ Law of Octaves are as follows

 Newlands’ Law of Octaves applicable to elements up to Calcium

 Newland assumed there are 56 elements in the nature and no more elements would

be discovered in the future.

 To fit elements into table Newland put two elements into one slot. Newland

introduced unlike elements with different properties into one column.

 Iron (Fe) was placed away from elements that resembles in properties. Ex: Nickel

and cobalt

Questions Page number 85



1. Use Mendeleev’s Periodic Table to predict the formulae for the oxides of the
following elements: K, C, AI, Si, Ba.

Solution:

K- K2O

C-C2O4 or CO2

Al- Al2O3

Si-Si2O4 or SiO2

Ba2O2 or BaO

Oxygen is a member of group VI A in Mendeleev's periodic table. Its valency is 2.

Similarly. The valencies of all the elements listed can be predicted from their respective

groups. This will help in writing the formulae of their oxides.

(i) Potassium (K) is a member of group IA. Its valency is 1. Therefore, the formula of it is

K2O.

(ii) Carbon (C) is a member of group IV A. Its valency is 4. Therefore, the formula of it is

C2O4 or CO2.

(iii) Aluminium (Al) belongs to groups III A and its valency is 3. The formula of its oxide

is Al2O3.

(iv) Silicon (Si) is present in group IV A after carbon. Its valency is also 4. The formula

oxide is Si2O4 or SiO2.

(v) Barium (Ba) belongs to group II A and the valency of the element is 2. The formula

of oxide of the element is Ba2O2 or BaO.

2. Besides gallium, which other elements have since been discovered that were left
by Mendeleev in his Periodic Table? (Any two)

Solution:

Germanium and Scandium are the element that are left by Mendeleev in his Periodic

Table since its discovery.

3. What were the criteria used by Mendeleev in creating his Periodic Table?

Solution:

NCERT Solution for Class 10 Science Chapter 5 -

Periodic Classification of Elements

Mendeleev concentrated on various compounds formed by the elements with Hydrogen

and

Oxygen. Among physical properties, he observed the relationship between the atomic

masses

of various elements while creating his periodic table.

4. Why do you think the noble gases are placed in a separate group?

Solution:

Noble gases are placed in a separate group because of their inert nature and low

concentration in our atmosphere. They are kept in a separate group called Zero group so

that they don’t disturb the existing order.

NCERT Solution for Class 10 Science Chapter 5 -

Periodic Classification of Elements

Questions Page number 90

1. How could the Modern Periodic Table remove various anomalies of Mendeleev’s
Periodic Table?

Solution:

(a) In the Modern Periodic table elements are arranged in the increasing order of their

atomic number. This removes the anomaly regarding certain pairs of elements in

Mendeleev’s periodic table.

(b) Atomic number of cobalt is 27 and nickel is 28. Hence cobalt will come before nickel

even though its atomic mass is greater.

c) All isotopes of the same elements have different atomic masses, but same atomic

number; therefore they are placed in the same position in the modern periodic table.

2. Name two elements you would expect to show chemical reactions similar to
magnesium. What is the basis for your choice?

Solution:

Calcium and Beryllium are similar to Magnesium because all the three elements belong

to the same group and have 2 valence electrons in their outer shell.

3. Name
(a) Three elements that have a single electron in their outermost shells.
(b) Two elements that have two electrons in their outermost shells.
(c) Three elements with filled outermost shells

Solution:

(a) Lithium (Li), Sodium (Na) and potassium (k) have a single electron in their

outermost shells.

(b)Magnesium (Mg) and Calcium (Ca) have two electrons in their outermost shells

(c) Neon (Ne), Argon (Ar and Xenon (Xe) filled outermost shells

4. a) Lithium, sodium, potassium are all metals that react with water to liberate
hydrogen gas. Is there any similarity in the atoms of these elements?
(b) Helium is an unreactive gas and neon is a gas of extremely low reactivity. What,
if anything, do their atoms have in common?


Solution:

They’ve one valence electron in their outermost shells and as a result of this, they are

very unstable. So, they readily react with water to liberate hydrogen. They are also called

alkali metals.

Their outermost shells are full leading to high stability. They react only in extreme

circumstances and hence are called noble gases.

5. In the Modern Periodic Table, which are the metals among the first ten elements?

Solution:

Lithium and Beryllium are the metals among the first ten elements in Modern Periodic

Table.

6. By considering their position in the Periodic Table, which one of the following
elements would you expect to have maximum metallic characteristic? Ga Ge As Se
Be

Solution:

Among the elements listed in the question. Be and Ga are expected to be most

metallic. Out of Be and Ga, Ga is bigger in size and hence has greater tendency to

lose electrons than Be. Therefore, Ga is more metallic than Be. 

Periodic Classification of Elements

Exercise questions Page number 91-92

1. Which of the following statements is not a correct statement about the trends
when going from left to right across the periods of periodic Table.

(a) The elements become less metallic in nature.

(b) The number of valence electrons increases.

(c) The atoms lose their electrons more easily.

(d) The oxides become more acidic

Solution:

Correct answer is c .The atoms lose their electrons more easily.

The atoms lose their electrons more easily is a wrong statement because as we move from

left to right across the periods of the periodic table, the non-metallic character increases.

Therefore tendency to lose an electron decreases.

2. Element X forms a chloride with the formula XCl2, which is a solid with a high
melting point. X would most likely be in the same group of the Periodic Table as (a)
Na (b) Mg (c) AI (d) Si

Solution:

Answer is Magnesium because Mg has the valency 2 which is same as the group (a) Na

(b) Mg (c) AI (d) Si

Also Mg when combines chloride forms MgCl2.

3. Which element has?
(a) Two shells, both of which are completely filled with electrons?
(b) The electronic configuration 2, 8, 2?
(c) A total of three shells, with four electrons in its valence shell?
(d) A total of two shells, with three electrons in its valence shell?
(e) twice as many electrons in its second shell as in its first shell?

Solution:

a) Neon has two shells which are completely filled.

b) Silicon has the electronic configuration 2, 8, 2

c) Carbon has a total of three shells, with four electrons in its valence shell

d) Boron a total of two shells, with three electrons in its valence shell

e) Magnesium has twice as many electrons in its second shell as in its first shell


4. (a) What property do all elements in the same column of the Periodic Table as
boron have in common?
(b) What property do all elements in the same column of the Periodic Table as
fluorine have in common?

Solution:

(a)All the elements which lie in me same column as that of boron belong to group 13.

Therefore, they have three electrons in their respective valence shells. Except, boron

which is a non-metal, all other elements (i.e., aluminum, gallium, indium and thallium) in

this group are metals.

(b) All elements in the same column of the Periodic Table as fluorine have in common

three electrons in their valence shell and they all are belong to group thirteen.

5. An atom has electronic configuration 2, 8, 7.
(a) What is the atomic number of this element?
(b) To which of the following elements would it be chemically similar? (Atomic
numbers are given in parentheses.) N(7), F(9), P(15), Ar(18)

Solution:

(a)The element with electronic configuration (2+8+7) 17 is chlorine.

The no. of atomic number = no. of electrons

Therefore, atomic number is 17.

(b) An atom with electronic configuration 2, 8, 7 would be chemically similar to F (9)

6. The position of three elements A, B and C in the Periodic Table are shown below–
Group 16 Group 17

 - -

 - A

 - -

 B C

(a) State whether A is a metal or non-metal.

(b) State whether C is more reactive or less reactive than A.

(c) Will C be larger or smaller in size than B?

(d) Which type of ion, cation or anion, will be formed by element A?

Solution:

(a) Element A is a non-metal

(b)Element C is less reactive than Element A

(c) C is smaller in size than B

(d)A will form anion

7. Nitrogen (atomic number 7) and phosphorus (atomic number 15) belong to group
15 of the Periodic Table. Write the electronic configuration of these two elements.
Which of these will be more electronegative? Why?

Solution:

Atomic number of Nitrogen is 7 hence Electronic configuration of Nitrogen is 1s2 2s2 2p3

Atomic number of Nitrogen is 15 hence Electronic configuration of Phosphorous is 1s2

2s2 2p6 3s2 3p3

On moving down a group in the periodic table, the number of shell increases. Because of

which valence electrons move away from the electrons and the effective nuclear charge

decreases. This causes the decrease in the tendency to attract electron and hence electro

negativity decreases. Because of all these reasons Nitrogen is more electronegative than

phosphorus.

8. How does the electronic configuration of an atom relate to its position in the
Modern Periodic Table?

Solution:

The number of valence electrons decides an atom’s position in the periodic table while

the electronic configuration decides the number of valence electrons.

9. In the Modern Periodic Table, calcium (atomic number 20) is surrounded by
elements with atomic numbers 12, 19, 21 and 38. Which of these have physical and
chemical properties resembling calcium?

Solution:

Calcium has an atomic number of 20, and thus has an electronic configuration of 2, 8, 8,

2. Thus, calcium has 2 valence electrons. The electronic configuration of the element

having atomic number 12 is 2, 8.2. Thus, this element with 2 valence electrons resemble

calcium the most.