CBSE Class 10 Science Periodic Table VBQs

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VBQ for Class 10 Science Chapter 5 Periodic Classification of Elements

Class 10 Science students should refer to the following value based questions with answers for Chapter 5 Periodic Classification of Elements in Class 10. These VBQ questions with answers for Class 10 Science will come in exams and help you to score good marks

Chapter 5 Periodic Classification of Elements VBQ Questions Class 10 Science with Answers

VALUE BASED QUESTIONS

Unit - Periodic Classification of Elements

Std – X

Question. Aashish is a student of Class V. His class teacher gave him an assignment to write a review of any of the books written by Enid Blyton. He goes to the library but he was unable to locate anyone. He approaches the librarian for help. The librarian took him to one of the sections of the library and showed him many books of Enid Blyton.

CONTEXTUAL QUESTION : 

   (i) What helped the librarian to locate the book easily ?

VALUE BASED QUESTION :

   (ii) Mention any two values that Aashish learnt 

(i) Value Points

     1. awareness about classification

     2. Application of knowledge.

     3. orderliness

Question. Tanvi was reading the morning newspaper. She came across a new word. She wanted to know its meaning and the way it is pronounced. She refers the dictionary and was thrilled when her attempt was successful.

CONTEXTUAL QUESTION :

Which property of the dictionary helped her in locating the word easily? 

VALUE BASED QUESTION :

     (i) What values do you think that Tanvi has? 

Value Points

     1. Awareness about classification

     2. Application of knowledge.

Question. A particular school has house matches after the assembly on every Wednesday . There would be utter chaos before the matches since each class is divided into different houses. The P.T.Master approached the Principal and got permission to allow the students to assemble housewise on Wednesdays.

CONTEXTUAL QUESTION :

What is the reason for chaos before the matches? Relate this to any one method of periodic classification of elements. 

VALUE BASED QUESTION:

What values can be imbibed from the P.T.Master’s  suggestion ? 

Value Points (any two)

    1. Need for change with time

    2. Capability to find alternative solution.

    3. Simplifying work

Question. Mendeleev left some gaps in his periodic table and predicted the discovery of new elements. Even though it was a drawback he boldly presented his table.

CONTEXTUAL QUESTION :

What is your view about Mendleev’s decision? 

VALUE BASED QUESTION :

List any any two values learnt from Mendleev ‘s decision 

Value Points

1. Self - confidence

2. Courage to face situations.

Question. The teacher was explaining the properties of elements, the types of bonding in the class. After that she asked the children the position they preferred in the periodic table if the choice is given as 14 th group or 18th group. Some chose14th and some18th.

CONTEXTUAL QUESTION :

       (i) Compare the properties of group 14 and group 18 elements.

VALUE BASED QUESTION :

      (ii) Mention the value points for those who chose group 14 and group 18. 

Value Points

Group 14 – sharing and caring, friendliness 

Group 18 - independent, staying calm and composed in all situations.

 

Question. 14 elements after actinium is called
(a) Lanthanides
(b) Actinides
(c) d-block elements
(d) p-block elements
Answer : B

Question. An element belongs to period 2 and group 2 the number of valence electrons in the atoms of this element is
(a) 2
(b) 4
(c) 3
(d) 1
Answer : A

Question. Which of the given elements A, B, C, D, and E with atomic number 3, 11, 15, 18, 19 respectively belong to the same group
(a) A, B, C
(b) B, C, D
(c) A, D, E
(d) A, B, E
Answer : B

Question. In the third period of the Periodic Table the element having smallest size is
(a) Na
(b) Ar
(c) Cl
(d) Si
Answer : B

Question. Element belonging to which of the following atomic numbers 11, 19, 14, 18, 23 belong to the same period?
(a) 11, 14, 23
(b) 11, 18, 20
(c) 11, 14, 18
(d) 14, 19, 23
Answer : C

Question. Electronic configuration of Al+3 is
(a) 2, 8, 3
(b) 2, 8, 8
(c) 2, 8
(d) 2, 8, 8, 3
Answer : C

Question. Which of the following sets does not belong to a group?
(a) Li, Na, K
(b) B, C, N
(c) B, Al, Ga
(d) O, S, Se
Answer : B

Question. Mendeleev predicted the existence of two elements and named them as eka-silicon and eka-aluminium. Identify the elements which took their position at later stage
(a) Si and Ge
(b) Si and Ga
(c) Ge and Ga
(d) Si and Al
Answer : C

Question. An element with atomic number will form a basic oxide _________.
(a) 7
(b) 17
(c) 14
(d) 11
Answer : D

Question. An element has an atomic number of 15 with which of the following elements will it show similar chemical properties?
(a) Be(4)
(b) Ne(10)
(c) N(7)
(d) O(8)
Answer : C

Question. The correct order of the increasing radii of the elements Na, Si, Al and P is
(a) Si, Al, P, Na
(b) P, Si, Al, Na
(c) Al, Si, P, Na
(d) Al, P, Si, Na
Answer : B

Question. Two elements X and Y have —
(i) X has 17 protons 18 neutrons
(ii) Y has 17 protons and 20 neutrons Both X and Y are—

(a) Isobars
(b) Isotopes
(c) Isotones
(d) None of the above
Answer : B

Question. Identify the group which is not a Döbereiner triad
(a) Li, Na, K
(b) Be, Mg, Cr
(c) Ca, Sr, Ba
(d) Cl, Br, I
Answer : B

Question. The group number and period number respectively of an element with atomic number 8 is
(a) 6, 2
(b) 16, 2
(c) 6, 8
(d) 16, 4
Answer : A

Question. The increasing order of the atomic radii of elements Na, Rb, K, Mg is
(a) Na < K < Mg < Rb
(b) K < Na < Mg < Rb
(c) Na < Mg < K < Rb
(d) Mg < Na < K < Rb
Answer : C

Case Study Questions Periodic Classification of Elements Class 10 Science

Read the passage given below and answer the following questions from Study the following table in which positions of six elements A, B, C, D, E and F are shown as they are in the modern periodic table :  

CBSE Class 10 Science Periodic Table VBQs

Question. Element E forms a chloride with formula  
(a) E Cl2
(b) E Cl
(c) E Cl4
(d) ECl

Answer : C

Question. Which of the following elements is a metalloid?  
(a) A
(b) B
(c) C
(d) E

Answer : D

Question. Which element in the given table has same number of electrons as in K+ and Cl–?  
(a) C
(b) F
(c) E
(d) D

Answer : B

Question. The formula of the oxide of element D will be  
(a) DO
(b) D2O
(c) D2O3
(d) D2O5

Answer : C

Question. Which of the following elements has most metallic character?  
(a) F
(b) D
(c) E
(d) B

Answer : B

Read the passage given below and answer the following questions from In 1913, Henry Moseley showed that the atomic number of an element is the more fundamental property than its atomic mass. Accordingly, Mendeleev’s periodic law was modified and atomic number was adopted as the basis of modern periodic table. In this periodic table, the elements are arranged in increasing order of their atomic numbers. There are 18 vertical columns in the periodic table which constitute 18 groups or families. The groups are numbered as 1, 2, 3, ... upto 18. All the members of a particular group have similar outer shell electronic configuration. There are seven horizontal rows of the periodic table which are known as periods.

Question. In the periodic table, the element with atomic number 16 will be placed in the group  
(a) fourteen
(b) sixteen
(c) thirteen
(d) fifteen.

Answer : B

Question. All the elements in a period in the periodic table have the same 
(a) atomic number
(b) electronic configuration
(c) atomic weight
(d) valence shell.

Answer : D

Question. Which of the following combinations of elements belong to the same group?   
(a) N, P, S
(b) Li, Na, K
(c) Na, Mg, Al
(d) O, S, Cl

Answer : B

Question. The atoms of elements belonging to the same group of periodic table have same number of  
(a) protons
(b) electrons
(c) neutrons
(d) electrons in outermost shell.

Answer : D

Read the passage given below and answer the following questions from Maximum number of electrons that can be accommodated in a shell is given by the formula : 2n2, where n is the number of the outermost from the nucleus. For example, K shell – 2 × (1)2 ⇒ 2, hence, K-shell can accommodate maximum 2 electrons. L shell – 2 × (2)2 ⇒ 8, hence, L-shell can accommodate maximum 8 electrons. In the modern periodic table, elements are placed according to their electronic configuration. The elements present in any group have the same number of valence electrons. The elements present in any period contain the same number of shells. The first period of the modern periodic table corresponds to the filling of electrons in the first energy shell, i.e., K-shell, first period has two elements. The second period of the periodic table corresponds to the filling of electrons in the second energy shell, i.e., L-shell, second period contains eight elements. The third, fourth, fifth, sixth and seventh periods have 8, 18, 18, 32 and 32 elements respectively.

Question. The elements A, B, C and D have atomic numbers 4, 12, 17 and 19 respectively. Which pair of elements belong to the same period?  
(a) B and C
(b) A and B
(c) A and D
(d) C and D

Answer : A

Question. Which of the following have the same number of electrons in outermost shell?  
(a) Elements with atomic numbers 3, 11, 19
(b) Elements with atomic numbers 14, 15, 16
(c) Elements with atomic numbers 12, 20, 28
(d) Elements with atomic numbers 10, 18, 26

Answer : A

Question. Electronic configuration of an element ‘X ’ is 2, 1. The number of elements present in the period to which ‘X ’ belongs is  
(a) 8
(b) 32
(c) 18
(d) 2

Answer : A

Question. Among the given elements A, B, C, D and E with atomic numbers 2, 3, 7, 10 and 30 respectively, which of these belong to the same period?  
(a) A, B, C
(b) B, C, D
(c) A, D, E
(d) B, D, E

Answer : B

Question. Which of the following elements has two shells and both are completely filled?  
(a) Helium
(b) Neon
(c) Calcium
(d) Fluorine

Answer : B

Read the passage given below and answer the following questions from Mendeleev arranged the 63 elements known at that time in order of their ascending atomic masses and prepared a periodic table. Mendeleev’s periodic table contains vertical columns called ‘groups’ and horizontal rows called ‘periods’. Elements with similar properties were placed in same groups. The basis of Mendeleev’s classification is his periodic law which states that :
(I) Atomic mass is the fundamental property of elements.
(II) The physical and chemical properties of elements are periodic function of their atomic masses.

Question. The properties of eka-aluminium predicted by Mendeleev were the same as properties of which element that was discovered later?  
(a) Scandium
(b) Germanium
(c) Gallium
(d) Aluminium

Answer : C

Question. Which of the following statements is not correct about Mendeleev’s periodic table?  
(a) In the Mendeleev’s periodic table, some places were left vacant for new elements which were not discovered at that time.
(b) Group VIII like groups I-VII has been divided into two sub-groups A and B.
(c) The group of an element in the periodic table represents its valency.
(d) Li and C belong to same period in Mendeleev’s periodic table.

Answer : B

Question. Which of the following metals is not placed in eighth group of Mendeleev’s periodic table?  
(a) Fe
(b) Na
(c) Co
(d) Ni

Answer : B

Question. In Mendeleev’s periodic table, silver belongs to IB group. The group to which silver belongs in the modern periodic table is  
(a) first
(b) eleventh
(c) tenth
(d) sixteenth.

Answer : B

Question. In Mendeleev’s periodic table, gaps were left for the elements to be discovered later. Which of the following elements found a place in the periodic table later?  
(a) Chlorine
(b) Silicon
(c) Oxygen
(d) Germanium

Answer : D

Read the passage given below and answer the following questions from The distance between the centre of the nucleus and the outermost shell of electrons is known as atomic radius. On moving from left to right along a period, atomic radii decrease because effective nuclear charge increases. For example, the atomic size decreases regularly from Li to F in the second period and from Na to Cl in the third period. It may, however, be noted that in any period, the noble gas has the largest size. On moving down in a group, atomic radii increase. 

CBSE Class 10 Science Periodic Table VBQs

CBSE Class 10 Science Periodic Table VBQs

Question. In the third period of the periodic table, the element having smallest size is  
(a) Na
(b) Ar
(c) Cl
(d) Si

Answer : C

Question. Among O, C, F, Cl, Br, the correct order of increasing atomic radii is   
(a) F, O, C, Cl, Br
(b) F, C, O, Cl, Br
(c) F, Cl, Br, O, C
(d) C, O, F, Cl, Br

Answer : A

Question. Which of the following has the maximum atomic radius?  
(a) Al
(b) Si
(c) P
(d) Mg

Answer : D

Question. The element with the smallest size in group 13 is  
(a) gallium
(b) thallium
(c) aluminium
(d) boron.

Answer : D

Question. The atomic radius decreases as we move across a period because  
(a) atomic mass increases
(b) atomic number decreases
(c) effective nuclear charge increases
(d) electrons are removed.

Answer : C

 

Very Short Answer Type Questions

Question. Besides gallium, which other elements have since been discovered that were left by Mendeleev in his periodic table? (any two)
Answer: Germanium, Scandium.

Question. Write any one difference in the electronic configurations of group 1 and group 2 elements.
Answer: Group 1 elements have one electron in their outermost shell while group 2 elements have two electrons in their outermost shell.

Question. N, O, F cannot be classified as Döbereiner’s triad. Why?
Answer: Although the atomic mass of O (16 u) is approximately an average (16.5 u) of the atomic masses of N (14 u) and F (19 u), i.e., (14 + 19)/2 = 16.5 but they cannot be regarded as a Döbereiner’s triad because their properties are altogether different.

Question. Why does atomic size decrease as we move from left to right along a period in the periodic table?
Answer: Effective nuclear charge increases as we move from left to right in the periodic table so atomic size decreases.

Question. Write the atomic numbers of two elements ‘X’ and ‘Y’ having electronic configurations 2, 8, 2 and 2, 8, 6 respectively.
Answer: Electronic configuration of X = 2, 8, 2
∴ Atomic number is 2 + 8 + 2 = 12
Similarly,
Electronic configuration of Y = 2, 8, 6
∴ Atomic number is 2 + 8 + 6 = 16

Question. Out of Li and K which will have stronger metallic character and why?
Answer: Potassium (K) will have stronger metallic character than lithium (Li) because as we move from top to bottom in a group, the size increases which increases the ease of liberation of electrons.

Question. Name two elements which show same kind of chemical reactivity as sodium.
Answer: Lithium (Li) and potassium (K) both belong to the same group as sodium (Na), So, they will show the same chemical properties as sodium.

Question. What is the valency of silicon with atomic number 14?
Answer: Atomic number of silicon = 14
Electronic configuration = 2, 8, 4
As silicon (Si) contains four electrons in its outermost shell, its valency will be four.

Question. Write the number of horizontal rows in the Modern Periodic Table. What are these rows called?
Answer: There are seven horizontal rows of elements in the Modern periodic table which are known as periods.

Question. State the Modern periodic law of classification of elements.
Answer: Modern periodic law states that the physical and chemical properties of elements are the periodic function of their atomic numbers.

Short Answer Type Questions :

Question. An element X has a total of 31 nucleons, out of which 16 are neutrons.
(a) Write the electronic configuration of an atom of element X.
(b) Determine the group and period number of element X.
(c) Give the formula of the ion formed by element X.
Answer: (a) Number of protons = 31 – 16 = 15
Number of electrons = 15
Electronic configuration = 2,8,5
(b) Element X has five valence electrons.
Hence, element X is from Group V.
Element X has three occupied shells.
Hence, element X is in Period 3.
(c) Formula of the ion formed by X = X 3–

Question. Give reason – While going down in group 1 lithium is least electropositive while caesium is most electropositive.
Answer: As we move down in a group, an electron shell is added after every change of period. For example, lithium has only two electron shells around the nucleus, but caesium has six electron shells around the nucleus. Thus, the positive charge within the nucleus holds the valence electrons of lithium more strongly than caesium. In other words, the valence electrons are held very loosely in case of caesium than lithium. Thus, caesium can lose its valence electrons more easily and hence, is more electropositive as compared to lithium, which is less electropositive. In other words, caesium is more metallic in character than lithium.

Question. In the Modern Periodic Table, the element calcium (atomic number = 20) is surrounded by elements with atomic numbers 12, 19, 21 and 38. Which of these elements have physical and chemical properties resembling those of calcium and why?
Answer: From the given data, the electronic configuration of different elements can be written as :
Calcium (20) = 2, 8, 8, 2
Element with atomic number 12 = 2, 8, 2
Element with atomic number 19 = 2, 8, 8, 1
Element with atomic number 21 = 2, 8, 8, 3
Element with atomic number 38 = 2, 8, 18, 8, 2
It can be easily seen that elements with atomic numbers 12 and 38 have two electrons in their outermost shell thus, they belong to same group as that of calcium. So, they will
show the physical and chemical properties resembling those of calcium.

Question. The electronic configuration of an element is 2, 8, 4. State its
(a) group and period in the Modern Periodic Table.
(b) name and write its one physical property.
Answer: (a) The element belongs to group 14 and 3rd period of the Modern Periodic Table.
(b) The element is silicon. It is non-lustrous.

Question. Choose from the following :
4Be, 9F, 19K, 20Ca
(i) The element having one electron in the outermost shell.
(ii) Two elements of the same group.
Answer: The electronic configurations of the given elements are :
4Be = 2, 2
9F = 2, 7
19K = 2, 8, 8, 1
20Ca = 2, 8, 8, 2
(i) Potassium (K) has one electron in its outermost shell.
(ii) Be and Ca have two electrons in their outermost shells hence, they belong to same group.

Question. Three elements ‘X’, ‘Y’ and ‘Z’ having atomic numbers 11, 7 and 6 respectively react with oxygen to form their oxides.
(a) Arrange these oxides in increasing order of their basic nature.
(b) Give reason for your answer.
Answer: 11X = 2, 8, 1
7Y = 2, 5
6Z = 2, 4
(a) Y < Z < X
(b) X is metallic in nature hence, its oxide is basic in nature.
While Y and Z are non-metals and their oxides are acidic in nature.

Question. Potassium, bromine and krypton are elements in period 4 of the Periodic Table.
(a) In which group of the periodic table can these elements be found?
(i) Potassium (ii) Bromine (iii) Krypton
(b) Bromine exists as a molecule. Draw a ‘dotand- cross’ diagram to show the bonding in a molecule of bromine.
(c) Krypton does not react with either potassium or bromine. Explain the unreactive nature of krypton.
Answer: (a) (i) Group I (ii) Group 17 (iii) Group 18
CBSE Class 10 Science Periodic Table VBQs
(c) Krypton has a stable electronic configuration, with 8 electrons in its valence shell. Hence, it does not lose, gain or share electron(s) with another atom. 

Question. Elements magnesium and oxygen respectively belong to group 2 and group 16 of the Modern Periodic Table. If the atomic numbers of magnesium and oxygen are 12 and 8 respectively, draw their electronic configuration and show the process of formation of their compound by transfer of electrons.
Answer: Atomic number of magnesium = 12
∴ Electronic configuration = 2, 8, 2
Valency of magnesium (Mg) = 2
Similarly, for oxygen (O) atomic number = 8
Electronic configuration = 2, 6
Valency of oxygen = 8 – 6 = 2
Formation of their compound will be as follows : 

CBSE Class 10 Science Periodic Table VBQs

Question. Calcium is an element with atomic number 20. Stating reason answer each of the following questions :
(i) Is calcium a metal or non-metal?
(ii) Will its atomic radius be larger or smaller than that of potassium with atomic number 19?
(iii) Write the formula of its oxide.
Answer: Given that, atomic number of calcium is 20.
So, its electronic configuration = 2, 8, 8, 2
(i) As, it has 2 valence electrons in the outermost shell which can be easily lost, so it is a metal.
(ii) Atomic number of K (potassium) is 19 so, it is placed before Ca(20) in the same period.
On moving from left to right in a period, the atomic radius decreases.
Hence, atomic radius of Ca(20) will be smaller than that of K(19).
(iii) The valency of calcium as well as oxygen is 2 thus, the formula of the oxide will be CaO.

Question. What is meant by periodicity of properties of elements? Why are the properties of elements placed in the same group of the periodic table similar?
Answer: When elements are arranged in increasing order of their atomic numbers, elements with similar chemical properties are repeated at definite intervals. This is known as periodicity of properties of elements.
Elements placed in the same group of the periodic table have similar properties because they have same number of outermost electrons and hence, show same valency. Thus, they all will form similar type of compounds.

Question. Based on the group valency of elements state the formula for the following giving justification for each:
a. Oxides of 1st group elements,
b. Halides of the elements of group 13, and
c. Compounds formed when an element of group 2 combines with an element of group 16.
Answer : a. M2O
b. MCl3
c. CaO

Question. The atomic number an element is 17. Predict:
a. its valency.
b. whether it is a metal or a non-metal?
c. its relative size with respect to other members of the group.
Justify your answer in each case.
Answer : 2, 8, 7 is the electronic configuration.
a. Its valency is equal to 1 because it can gain 1 electron to become stable.
b. Non-metals because it can gain an electron to form anion.
c. It is bigger in size than F (1st element) but smaller than all other members because it has 3 shells, F has 2 shells, others have more than 3 shells.

Question. In the following table, six elements A, B, C, D, E and F (here letters are not the usual symbols of the elements) of the Modern Periodic Table with atomic  numbers 3 to 18 are given as follows:
CBSE Class 10 Science Periodic Classification Of Elements Worksheet_15
a. Which of these is (i) a noble gas, (ii) a halogen?
b. If B combines with F, what would be the formula of the compound formed?
c. Write the electronic configurations of ‘C’and’E’.
Answer : a. (i) G is a noble gas, (ii) F is a halogen.
b. BF is the formula of compound.
c. C: 2, 8, 2 E: 2, 8, 6

Question. An element X (atomic number 17) reacts with an element Y (atomic number 20) to form a compound.
a. Write the position of these elements in the modern periodic table.
b. Write the formula of the compound formed.
Justify your answer in each case.
Answer : a. X: 2, 8, 7 belongs to 3rd period, group 17, because it has 3 shells and 7 valence electrons.
Y: 2, 8, 8, 2 belongs 4th period, group 2, because it has 4 shells and 2 valence electrons.
b. YX2, is the formula of the compound, because Y has valency 2, X has valency 1.

Question. What is meant by ‘group’ in the modern periodic table? How do the following change on moving from top to bottom in a group?
a. Number of valence electrons.
b. Number of occupied shells.
c. Size of atoms.
d. Metallic character of elements.
e. Effective nuclear charge experienced by valence electrons.
Answer : The vertical column of the periodic table is called group.
a. Number of valence electrons remains the same in a group.
b. Number of occupied shells goes on increasing down a group.
c. Size of atom increases down the group.
d. Metallic character of element increases down the group.
e. Effective nuclear charge decreases down the group.

Question. Two elements X and Y have atomic number 11 and 16 respectively.
a. Write the electronic configuration of both.
b. Write the formula of the compound formed by their combination (in terms of X and Y).
Answer : a. X(11): 2, 8, 1; Y(16): 2, 8, 6
b. X2Y is the formula of compound formed.

Question. In the following table, are given eight elements A, B, C, D, E, F, G and H (here letters are not the usual symbols of the elements) of the Modem Periodic Table with the atomic numbers of the elements in parenthesis.
CBSE Class 10 Science Periodic Classification Of Elements Worksheet_16
a. What is the electronic configuration of‘F?
b. What is number of valence electrons in ‘F’?
c. What is number of shells in *F’?
d. Arrange E, F, G, H in decreasing order of atomic size.
e. State whether F is a metal or a non¬metal.
f. Out of three elements B, E and F, which one has biggest atomic size.
Answer : a. 2, 8, 2 is the electronic configuration of F.
b. No. of valence electrons = 2.
c. Three shells are present in F.
d. H > G > F > E is the decreasing order of atomic size.
e. F is a metal.
f. B has biggest atomic size.

Question. (a) Name metals among the first five elements of the Modern Periodic Table.
(b) Write their symbols.
(c) Write the formula of their oxides.
Answer : a. Lithium and Beryllium are metals among first five elements.
b. Lithium (Li), Beryllium (Be).
c. Li2O and BeO are the formulae of their oxides.

Question. The atomic number of three elements are given below:
Element (symbol)   A   B   C
Atomic number       5   7   10
Write the symbol of element which belongs to (a) group 13, (b) group 15 of the periodic table. State the period to which these elements belongs to. Give reason for your answer.
Answer : a. A(2, 3) belongs to group 13 because it has 3 valence electrons.
b. B(2, 5) belongs to group 15 because it has 5 valence electrons. It belongs to 2nd period because it has 2 shells.

Question. The electronic configuration of 4 elements A, B, C and D are given as under:
A-2, 1; B-2, 2; C-2, 8, 2; D-2
a. Which amongst them belongs to the same group? Name it.
b. Which amongst them belong to the same period? Name it.
c. Which amongst them is an inert element? Name it.
Answer : a. B and C belong to the same group, 2nd group; Be and Mg.
b. A and B belong to the same period, 2nd period; Li and Be.
c. D is the inert; It is Helium (He).

Question. The atomic number of an element X’is 20.
a. Determine the position of the element “X’ in the periodic table.
b. What would be the nature (acidic or basic) of the compound formed? Justify your answer.
Answer : X(20): 2, 8, 8, 2; Y(8): 2, 6
a. It belongs to group 2, 4th period because its valence electrons are 2 and no. of shells = 4
b. Compound formed will be basic because “X’ is a metal.

Question. a. How are the following related?
i. Number of valence electrons of different elements in the same group.
ii. Number of shells of elements in the same period.
b. How do the following change?
i. Number of shells of elements as we go down a group.
ii. Number of valence electrons of elements on moving from left to right in a period.
iii. Atomic radius in moving from left to right along a period.
iv. Atomic size as we go down a group.
Answer : a. i. Same number of valence electrons.
ii. Number of shells remains the same in a period.
b. i. Number of shells goes on increasing down the group.
ii. Number of valence electrons goes on increasing in a period from left to right.
iii. Atomic radius decreases along a period from left to right.
iv. Atomic size increases down a group.

Question. The electronic configuration of two elements A and B are 2, 8, 7 and 2, 8, 8, 2 respectively. Write the atomic number of these elements. What will be formula of the compound formed and the nature of bond between them when these two elements chemically combine together?
Answer : A - 2 + 8 + 7 = 17 is its atomic number.
B - 2 + 8 + 8 + 2 = 20 is its atomic number.
A(2, 8, 7) B(2, 8, 8, 2)
CBSE Class 10 Science Periodic Classification Of Elements Worksheet_17
The nature of bond is ionic bond.

Question. How does valency of the elements vary
a. in going down a group, and
b. in going from left to right in a period of the periodic table?
Answer : a. It remains the same.
b. It first increases till middle, then decreases.

Question. In the periodic table, how does the tendency of atoms to lose electrons change on going from
a. left to right across a period?
b. top to bottom in a group?
Answer : a. Tendency to lose electron(s) decreases across the period from left to right.
b. Tendency to lose electron(s) increases down in a group.

Question. Given below are some elements of the modern periodic table:
      4Be, 9F, 14Si, 19K, 20Ca
a. Select the element that has one electron in the outermost shell and write its electronic configuration.
b. Select two elements that belong to the same group. Give reason for your answer.
c. Select two elements that belong to the same period. Which one of these two has bigger atomic size?
Answer : a. 19K: 2, 8, 8, 1
b. 4Be, 20Ca belong to the same group because both have same number of valence electrons.
     Be: 2, 2; Ca: 2, 8, 8, 2
c. 4Be, 9F belong to the same period. 4Be has bigger atomic size than 9F.

Question. The atomic number of these elements are given below:
Element (symbol)   A   B   C
Atomic number       3   6   9
Write the symbol of element which belongs to
a. group 1,
b. group 14 of the periodic table.
State the period of the periodic table to which these elements belong to. State reason to support your answer.
Answer : c. A(3) has electronic configuration 2, 1. It belongs to group 1. Hence the number of valence electrons is 1.
d. B(6) has electronic configuration 2, 4. It belongs to group 14, valence electrons = 4.
They belong to second period because they have 2 shells.

Question. An element X’ is placed in 13th group and 3rd period of Modern Periodic Table. Answer the following stating reason for your answer.
a. Write the electronic configuration of the element X’.
b. Will oxide of this element be acidic or basic?
Answer : X is Aluminium (13); Y(17) 2, 8, 7
a. 2, 8, 3
b. It will be amphoteric i.e., it is acidic as well as basic.

Question. Na/Mg and A1 are the elements having one, two and three valence electrons respectively. Which of these elements (a) has the largest atomic radius, (b) is least reactive? Justify you answer stating reason for each.
Answer : Na has largest atomic radii due to 11 protons and 11 electrons and least effective nuclear charge. Na is most reactive because it can lose an electron easily due to its large size and least effective nuclear charge.

Question. How the electronic configuration of the atom of an element is related to its position in the modern periodic table? Explain with one example.
Answer : Period No. = Number of shells
Group No. = Number of valence electrons or valence electrons +10.
Example
Na(11): 2, 8,1. It has 1 valence electron, it belongs to group 1. Also Al (13): 2, 8, 3. It has 3 shells, therefore it belongs to 3rd period.

Question. The elements Li, Na and K each having one valence electron, are in period 2, 3 and 4 respectively of modern periodic table.
a. In which group of the periodic table should they be placed?
b. Which one of them is least reactive?
c. Which one of them has the largest atomic radius?
d. Give reason to justify your answer in each case.
Answer : a. They belong to group 1 because they have one only valence electron.
b. Lithium (Li) is the least reactive because it is smallest in size, has least tendency to lose electrons.
c. K has largest atomic radius because it has maximum number of shells.

Question. The position of three elements A, B and C in the Periodic Table is shown below:
CBSE Class 10 Science Periodic Classification Of Elements Worksheet_18
Giving reasons, explain the following:
a. Element A is a non-metal.
b. Atoms of element C has a larger size than atoms of element A.
c. Element B has a valency of 1.
Answer : a. A is a non-metal because it can gain one electrons to form anion.
b. C has more number of shells i.e., it has 3 shells because it belongs to 3rd period whereas A has 2 shells as it belongs to 2nd period.
c. B can lose 1 electron to become stable, therefore its valency is equal to 1.

Question. (a) State modern periodic law.
(b) How many groups and periods are present in the modern periodic table?
(c) State how the problem of placing (a) hydrogen,
(b) isotopes of an element has been solved in this periodic table.
Answer : a. Properties of elements are a periodic function of their atomic numbers’.
b. There are 18 groups and 7 periods.
c. (i) Hydrogen is placed along with group 1 as well as halogens because it resembles with both of them.
(ii) Isotopes do not need a separate place as they have the same atomic number.

Question. The element Be, Mg and Ca are placed in the second group of the periodic table. Their atomic numbers are 4, 12, 20 respectively a. Write the electronic configuration of these elements.
b. Write the valency exhibited by them,
c. Which three elements will be the most reactive?
Answer : a.
CBSE Class 10 Science Periodic Classification Of Elements Worksheet_19
b. Valency is 2.
c. Ca is the most reactive metal.

Question. Two elements M and N belong to group 1 and 2 respectively and are in the same period of the periodic table. How do the following properties of M and N vary?
a. Sizes of their atoms.
b. Their metallic character.
c. Their valencies in forming oxides.
d. Formulae of their chlorides.
Answer : a. M has bigger size than N.
b. M has more metallic character than N.
c. M has valency equal to 1, N has valency equal to 2.
d. MCl and MCl2 are formula of their chlorides.

Question. On the basis of electronic configuration, how will you identify the first and the last element of a period?
Answer : 1st element will have 1 valence electron whereas last element will have 8 valence electrons except in first period in which last element has 2 electrons.

Question. Lithium, Sodium, Potassium are placed in the same group on the basis of their similar properties. List three such similar properties.
Answer : a. All of them are reactive metals.
b. They have 1 valence electron and form positive ions with +1 charge.
c. They are largest in size in their respective periods.

Question. The atomic number of K and Ca is 19 and 20 respectively and they belong to same period.
a. Which amongst them would have smaller atomic size?
b. Which one would be more electro¬positive?
c. To which group would each one belong to? 
Answer : a. Ca has smaller atomic size.
b. K is more electropositive.
c. K belongs to group 1, Ca belongs to group 2.

Question. The atomic number of three elements, X, Y and Z are 9, 11 and 17 respectively. Which two of these elements will show similar chemical properties? Why?
Answer : X(9) : 2, 7
Y(11) : 2, 8, 1
Z(17) : 2, 8, 7
X and Z have similar chemical properties because they have the same number of valence electrons.

Question. The position of elements A, B, C, D, E, F and G in the Modern Periodic Table is given as under:
CBSE Class 10 Science Periodic Classification Of Elements Worksheet_20
a. In which group are inert elements placed?
b. What type of ions would ‘B’, ‘C’, ‘E’ and ‘F’will form?
c. Which element would have chemical properties similar to ‘C’?
d. How many shells do ‘A’ have?
e. What is the similarity between ‘A’ and ‘D’?
f. Identify the most abundant element in the earth crust.
Answer : a. Group 18
b. They will form anions.
c. F will have similar properties to ‘C’.
d. A has only one shell.
e. A and D both are inert elements.
f. C is the most abundant element in the Earth crust.

Question. a. What is meant by periodicity in properties of elements with reference to the periodic table?
b. Why do all the elements of the same group have similar properties?
c. How will the tendency to gain electrons change as we go from left to right across a period. Why?
Answer : a. The repetition of similar properties after regular intervals is called periodicity in properties.
b. It is because they have the same number of valence electrons.
c. Tendency to gain electrons increases from left to right across the period due to decrease in atomic size.

Question. What physical and chemical properties of elements were used by Mendeleev in creating his periodic table? List two observations which posed a challenge to Mendeleev’s Periodic Law.
Answer : a. Increasing order of atomic mass was the physical property.
b. Formulae of oxides and hydrides was the chemical property.
i. Increasing order of atomic mass could not be maintained.
ii. Position of isotopes posed a challenge for the classification of elements.

Question. a. Identify the elements among the following which will belong to the same group: H, He, Li, B, C.
b. State the group number of the recognised elements.
c. Name another one element belonging to the same group.
Answer : a. H and Li belong to the same group.
b. They belong to group 1.
c. Na (sodium) also belong to this group.

Question. Choose from the following: 4Be, 9F, 19K, 20Ca 
a. The element having one electron in the outermost shell.
b. Two elements of the same group.
Answer : a. 19K(2,8,8,1) has one valence electron,
b. 4Be(2, 2) and 20Ca(2, 8, 8, 2) belongs to the same group.

Question. The following table shows the elements represented by the letters A, B, C, D, E, F, G and H.
Group      1  2  13  14  15  16  17  18
Element  A   B   C   D    E    F    G    H
a. Which of the elements has the atomic size (i) biggest and (ii) smallest?
b. Which element has valency equal to (i) 3 and (ii) zero?
Answer : a. (i) A has the biggest size. (ii) G has the smallest size.
b. (i) C has valency equal to 3. (ii) H has valency equal to zero.

Question. a. State Modern Periodic Law
b. Elements A, B, C and D have atomic number 1, 8, 11, 19 respectively. Choose the odd element and give reason for your answer.
Answer : a. Modern Periodic Law: It states ‘properties of elements are a periodic function of their atomic number’.
b. B(8): 2, 6 is an odd element because it has 6 valence electrons whereas others have 1 valence electron.

Question. The atomic number of an element is 19.
a. Write the electronic configuration of this element and determine (i) the valency of this element, and (ii) whether this element is a metal or a nonmetal?
b. Write the formula of the oxide of this element.
c. Is this element more reactive or less reactive than Na (atomic number 11)? Justify your answer, giving example.
Answer : a. 2, 8, 8, 1
i. Valency = 1
ii. It is a metal.
a. X2O
b. It is more reactive than Na(11) because it is large in size and it can lose electrons easily due to less effective nuclear charge.
K reacts more vigorously with H2O than Na.

Question. An element has atomic number 13.
a. What is the group and period number to which this element belongs to?
b. Is the element a metal or a non-metal? Justify your answer.
Answer : a. It belongs to group 13, 3rd period because it has 3 valence electrons and 3 shells.
b. It is a metal because it can lose 3 electrons to become stable.

Question. Why is atomic number considered to be a more appropriate parameter than atomic mass for the classification of elements in a periodic table? How does the metallic character of elements vary as we move (a) from left to right in a period, and (b) top to bottom in a group of the modem periodic table? Give reasons to justify your answer.
Answer : It is because chemical properties depend upon the number of valence electrons which is determined with the help of atomic number.
a. Metallic character decreases from left to right because atomic size decreases, tendency to lose electrons decreases,
b. Metallic character increases from top to bottom in a group because atomic size increases due to which effective nuclear charge decreases.

Question. Arrange the following elements in descending order of their atomic size and give reason for your answer.
Mg(12), P(15), Cl(17), Ar(18)
Answer : Mg > P > Ar > Cl
As we move from left to right, atomic size decreases due to increase in effective nuclear charge. Ar is bigger than Cl due repulsion between 8 valence electrons.

Question. In the figure given below the first 20 elements are jumbled up. Carefully observe the figure and answer the following questions:
CBSE Class 10 Science Periodic Classification Of Elements Worksheet_21
a. Pick out the two elements which are known as alkali metals.
b. Pick out the two elements which have valency of 4.
c. Pick out two elements which belong to group 16 of the periodic table.
Answer : a. Na, K are alkali metals.
b. C, Si have valency equal to 4
c. O and S belongs to group 16.

Question. Why does the reactivity of metals increases and that of non-metals decreases as we move down the group?
Answer : Reactivity of metals depends on the tendency to lose electrons. If the atomic size increases, the valence electrons are easily removed thereby forming positive ion. In case of metals the atomic size increases as we move down the table. Reactivity of non-metals depends on the tendency to gain electrons. As we move down the group, the tendency to gain electrons decreases because the atomic size increases, the nuclear force decreases.

Question. What physical and chemical properties of elements were used by Mendeleev in creating his Periodic Table? List two observations which posed a challenge to Mendeleev’s Periodic Law.
Answer : The physical property used was the atomic mass of an element.
The chemical property used was the nature of oxide and hydride formed i.e. similarity in chemical properties were used by Mendeleev. The two observations that posed
challenge in Mendeleev Periodic Law were:
(i) Arranging elements according to the increasing order of atomic mass could not be maintained. Chemical properties do not depend on atomic mass.
(ii) Isotopes were not given any place in the table as they have different atomic mass but same chemical properties.

Question. List the elements present in 2nd period. Write their atomic number and electronic configuration.
Answer : Elements → Li     Be     B     C     N      O       F     Ne
Atomic No. →                3      4      5     6      7      8       9     10
Electronic
configuration →           2, 1  2, 2  2, 3  2, 4  2, 5  2, 6   2, 7  2, 8

Question. Lithium, sodium potassium belong to same group called alkali metals. Why?
Answer : Lithium, sodium and potassium have same valence electron i.e. 1, hence they belong to same group. The group is called alkali metals group because all these elements form oxides which dissolve in water to form alkali.

Question. (a) What is meant by periodicity in properties of elements with reference to the Periodic Table?
(b) Why do all the elements of the same group have similar properties?
(c) How will the tendency to gain electrons change as we go from left to right across a period? Why?
Answer : (a) The repetition of same properties after definite interval is called periodicity in properties.
(b) All elements in group have same valence electrons.
(c) Tendency to gain electrons increases from L → R in the period because the atomic size goes on decreasing and nuclear charge increases, which can attract the nearby electron.

Question. What are the merits of Mendeleev’s Periodic Table?
Answer : Merits of Mendeleev’s Periodic Table are:
(i) Mendeleev left some gaps in his table. Predicted the chemical properties of these 3 elements which were discovered later and had same properties as predicted by
Mendeleev, they were gallium, germanium and scandium.
(ii) He arranged the elements very systematically in periods and groups.

Question. Carbon with atomic number 6 and silicon with atomic number 14 belong to same group although carbon is non-metal and silicon is semi-metal.
Answer : Carbon with atomic number 6, shows electronic configuration 2, 4. Silicon with atomic number 14 shows electronic configuration 2, 8, 4.
Both the elements have same valence electrons, hence they are placed in same group.

Question. Why are noble gases placed in a separate group?
Answer : All noble gases show same valency i.e. ‘0’, all of them are inert gases, the chemical properties are same and hence they are placed in same group.

Question. Table given below shows a part of the Periodic Table.
H                                        He
Li    Be   B   C   N  O  F    Ne
Na  Mg  Al   Si  P  S  Cl    Ar
Using this table explain why?
(a) Li and Na are considered as active metals.
(b) Atomic size of Mg is less than that of Na.
(c) Fluorine is more reactive than chlorine.
Answer : (a) Li and Na can readily lose electrons due to bigger size of atom.
(b) Mg has more number of protons than Na which attracts the electrons thereby reducing the size of Mg.
(c) Fluorine readily accepts/gains electrons to become F– ion due to its small atom size as compared to chlorine.

Long Answer Type Questions :

Question. (a) Consider three elements Na, Cl, Ar and answer the following.
(i) Discuss their metallic and non-metallic character.
(ii) Discuss the acid-base character of their oxides.
(b) The element with atomic number 14 is hard and forms acidic oxide and a covalent halide.
To which of the categories does the element belong?
Answer: (a) The electronic configurations of these elements are Na : 2, 8, 1 ; Cl : 2, 8, 7 and Ar : 2, 8, 8
(i) Sodium has only 1 electron in its valence shell which it can lose easily. Therefore it is a typical metal, chlorine has even electrons in its outermost shell, it can easily accept one
electron to get noble gas configuration, hence it is a typical non-metal. Ar is a noble gas.
(ii) The oxide of Na i.e. Na2O dissolves in water to form NaOH which is a strong base. The oxide of chlorine i.e. Cl2O7 dissolves in water to give HClO4 which is a strong acid.
Ar does not form any oxides.
Na2O + H2O → 2NaOH
Cl2O7 + H2O → 2HClO4
Hence, both metallic character of the elements and basic character of oxides decreases from left to right across a period.
(b) Non-metal, because it forms acidic oxide and covalent halide which are characteristics of non-metals.

Question. In the table given below, some of the elements of the periodic table with atomic numbers from 3 to 18 are given. These are represented by letters, which are not the usual symbols of the elements. 38
(a) Which of these
(i) is an alkaline earth metal?
(ii) are alkali metals?
(iii) is an element with valency 4?
(b) If A combines with F, what would be the formula of the resulting compound?
(c) What is the electronic arrangement of G?
Answer: (a) (i) C is an alkaline earth metal.
(ii) A and B are alkali metals.
(iii) D is an element with valency 4.
(b) If A combines with F, the formula of the resulting compound will be A+F –., i.e., AF.
(c) The electronic arrangement of G is 2, 8.

Question. (a) The modern periodic table has been evolved through the early attempts of Dobereiner, Newlands and Mendeleev. List one advantage and one limitation of all the three attempts.
(b) Name the scientist who first of all showed that atomic number of an element is a more fundamental property than its atomic mass.
(c) State Modern periodic law.
Answer: (a) Advantage of Dobereiner’s triads : It recognised a relationship between properties of elements and their atomic weights.
Limitation of Dobereiner’s triads : Dobereiner could identify only three triads. He was not able to prepare triads of all the known elements.
Advantages of Newland’s law of octaves : This law provided a basis for the classification of elements into groups of elements having similar properties.
Limitation of Newlands’ law of octaves : This law worked only for the lighter elements. All the element discovered at that time could not be classified into octaves.
Advantages of Mendeleev’s periodic table : He classified all the 63 elements discovered at that time on the basis of similarities in their properties.
Limitation of Mendeleev’s periodic table : Increasing order of atomic masses could not be maintained in all cases e.g., cobalt with higher atomic mass was placed before nickel.
(b) Henry Moseley, an English physicist, showed that atomic number of an element is a more fundamental property than its atomic mass.
(c) Modern periodic law states that the physical and chemical properties of elements are the periodic function of their atomic numbers.

Question. The table below shows the electronic configuration of six elements. 39
(a) Give the letter (s) of (i) two elements that are in the same period of the periodic table.
(ii) two elements that are in the same group of the periodic table.
(iii) a noble gas.
(iv) group VII non-metals.
(v) element which forms positive ion.
(b) (i) Give the formula of the compound formed between elements P and S.
(ii) What type of bonding would you expect in the compound formed?
Answer: (a) (i) P, Q and R (two electron shells) or S and T (three electron shells).
(ii) P and U (one valence electron) or R and S (seven valence electrons).
(iii) T (completely filled valence shell).
(iv) R or S (seven valence electrons).
(v) P or U (one valence electron).
(b) (i) PS
(ii) ionic bonding.

Question. (a) How does metallic character of elements in Modern Periodic Table vary on moving from
(i) left to right in a period
(ii) top to bottom in a group?
Explain with the help of an example in each case.
(b) If an element X is placed in group-14, what will be the nature of bond in its chloride?
Write the chemical formula of the compound formed.
(c) An element X has mass number = 35 and number of neutrons = 18. What is the atomic number of X? Write electronic configuration of X and determine its valency.
Answer: (a) In the Modern periodic table, there are 18 vertical columns called groups and 7 horizontal rows called periods.
Trend of metallic character :
(i) Along the period from left to right : Metallic character of elements decreases as we move from left to right in a period.
Metallic character depends on the electropositive character (tendency to lose electrons) of the elements. As we go across the period from left to right, one electron is added to same
shell at every stage which increases the effective nuclear charge and hence, valence electrons becomes more and more closer to the nucleus. Due to this, the tendency of atoms
to lose valence electrons and form positive ions decreases.
Hence, electropositive character decreases resulting in decrease of metallic character.
Example :
Variation of metallic character across the period : 
CBSE Class 10 Science Periodic Table VBQs
(ii) Down the group : Metallic character of elements increases on moving down the group as the electropositive character increases down the group.
Example :
Variation of metallic character down the group :
(b) Since element ‘X’ is placed in group 14, therefore, its valency is 14 – 10 = 4. Further, since it is difficult to either lose all the four valence electrons or gain four more electrons,
therefore, it prefers to share these four electrons to acquire the stable electronic configuration of the nearest inert gas.
Thus, the nature of the bond of chloride of element ‘X’ is covalent and the chemical formula is XCl4.
(c) Mass number of X = 35
Number of neutrons = 18
∴ Number of electrons = Number of protons
= (Mass number – Number of neutrons)
= 35 – 18 = 17
Number of electrons of X = Atomic number of X = 17
Thus, electronic configuration of X = 2, 8, 7
As it has 7 electrons in the outermost shell, so it belongs to 17th group. Moreover the electrons are present in three shells, so it belongs to 3rd period.
Valency of X = 8 – 7 = 1

Please refer to the link below for CBSE Class 10 Science VBQs - Periodic Table

Chapter 01 Chemical Reactions and Equations
CBSE Class 10 Science Chemical Reactions and Equations VBQs
Chapter 02 Acids Bases and Salts
CBSE Class 10 Science Acids Bases and Salts VBQs
Chapter 03 Metals and Non metals
CBSE Class 10 Science Metals and Non metals VBQs
Chapter 04 Carbon and its Compounds
CBSE Class 10 Science Carbon and its Compounds VBQs
Chapter 05 Periodic Classification of Elements
CBSE Class 10 Science Periodic Table VBQs
Chapter 07 Control and Coordination
CBSE Class 10 Science Control and Coordination VBQs
Chapter 08 How do the Organisms Reproduce
CBSE Class 10 Science How Do Organisms Reproduce VBQs
Chapter 09 Heredity and Evolution
CBSE Class 10 Science Heredity and Evolution VBQs
Chapter 10 Light Reflection and Refraction
CBSE Class 10 Science Light Reflection and Refraction VBQs
Chapter 11 Human Eye and Colourful World
CBSE Class 10 Science Human Eye and Colourful World VBQs
Chapter 13 Magnetic Effects of Electric Current
CBSE Class 10 Science Magnetic Effects of Electric Current VBQs
Chapter 16 Sustainable Management of Natural Resources
CBSE Class 10 Science Sustainable Management of Natural Resources VBQs

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