CBSE Class 10 Chemistry Periodic Classification Of Elements Worksheet Set A

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Worksheet for Class 10 Science Chapter 5 Periodic Classification of Elements

Class 10 Science students should refer to the following printable worksheet in Pdf for Chapter 5 Periodic Classification of Elements in Class 10. This test paper with questions and answers for Class 10 will be very useful for exams and help you to score good marks

Class 10 Science Worksheet for Chapter 5 Periodic Classification of Elements

Question : An element X (2, 8, 2) combines separately with (SO4)2–and (PO4)3– radicals. The chemical formulae of the compounds are
(a) X2SO4 : X3(PO4)2
(b) XSO4 : X3(PO4)2
(c) X(SO4)2 : X2(PO4)3
(d) XSO4 : X3(PO4)
Answer : B

Question : In the Modern Periodic Table, the metals among the first ten elements are—
(a) Be, Na
(b) Li, Be
(c) Be, Li, Na
(d) Li, Na
Answer : D

Question : Arrange the following elements into the increasing order of their metallic character along a period.
(a) S < Si < P < Al
(b) S < P < Si < Al
(c) Si < P < S < Al
(d) Si < S < P < Al
Answer : B

Question : How many elements did Mendeleev classify? 
(a) 30.0
(b) 63.0
(c) 92.0
(d) 60.0
Answer : B
Explanation: In his periodic table, Mendeleev arranged all the then known 63 elements in the order of increasing atomic masses.
 
Question : Match the following with correct response.
A-32
(a) 1-A, 2-C, 3-B, 4-D
(b) 1-B, 2-D, 3-A, 4-C
(c) 1-D, 2-A, 3-C, 4-B
(d) 1-C, 2-B, 3-D, 4-A
Answer : C
Explanation: As the atomic size across a group increases, so the energy required to knock out the electron i.e. Ionization enthalpy decreases.
Across a group, the atomic size increases with the increase in atomic number.
Metals readily lose electrons to form positive ions, so they have high electropositive character.
Non-metals readily gain electrons to form negative ions, so they have high electronegative character.
 
Question : Give the symbol for the most reactive non-metal of group 17. 
(a). Br
(b) I
(c) F
(d) Cl
Answer : C 
Explanation: On going down the group of the periodic table, the electronegative character of non-metals decreases.
Therefore, Fluorine being on the top in group 17 elements have the most electronegative character.
 
Question : Match the following with correct response.
A-33
(a) 1-C, 2-B, 3-D, 4-A
(b) 1-D, 2-A, 3-C, 4-B
(c) 1-A, 2-C, 3-B, 4-D
(d) 1-B, 2-D, 3-A, 4-C
Answer : B
Explanation: Valency is the combining capacity of an element.
On moving down in a group, the valency of elements remains same. On moving from left to right in a period, the atomic size decreases.
Elements on the left hand side of the periodic table are metals. 
 
Question : Elements having same valence electrons are placed in same group but there is an exception with- 
(a) He
(b) Ar
(c) Ne
(d) Xe
Answer : A
Explanation: All the elements of group 18 have 8 valence electrons each in their atoms, except helium which has only 2 valence electrons in its atom as its duplet is complete.
 

Multiple choice questions 

Question : The properties of Eka-aluminium predicted by Mendeleev are the same as the properties of later discovered element:
(a) Scandium
(b) Germanium
(c) Gallium
(d) Aluminium
Answer : C

Question : The arrangement of elements in the Modem Periodic Table is based on their
(a) increasing atomic mass in the period
(b) increasing atomic number in the horizontal rows
(c) increasing atomic number in the vertical columns
(d) increasing atomic mass in the group
Answer : B

Question : Element ‘X’ forms a chloride with the formula XCl2, which is a solid with high melting point. X would most likely be in the same group of the periodic table as:
(a) Si
(b) Mg
(c) Al
(d) Na
Answer : B

Question : What is the atomic number of element of period 3 and group 17 of the Periodic Table?
(a) 10
(b) 4
(c) 17
(d) 21
Answer : C

Question : An element X from group 2 of the Periodic Table reacts with Y from group 17 to form a compound. Give the formula of the compound.
(a) XY2
(b) XY
(c) X2Y
(d) (XY)2
Answer : A

Question : A metal ‘M’ is in the first group of the Periodic Table. What will be the formula of its oxide? (a) MO
(b) M2O
(c) M2O3
(d) MO2
Answer : B

Question : An element X has mass number 40 and contains 21 neutrons in its atom. To which group of the Periodic Table does it belong?
(a) Group 1
(b) Group 4
(c) Group 2
(d) Group 3
Answer : A

Question : What is the other name for group 18th elements?
(a) Noble gases
(b) Alkali metals
(c) Alkali earth metals
(d) Halogens
Answer : A

Question : The atom of an element has electronic configuration 2, 8, 7. To which of the following elements would it be chemically similar?
(a) 7N
(b) 15P
(c) 11Na
(d) 9F
Answer : D

 

Case study questions

Modern periodic table has 18 vertical columns known as groups and 7 horizontal rows known as periods. First period contains 2 elements second and third period contain 8 elements. 4th and 5th period contains 18 elements and 6th and 7th period contains 32 elements. The graph is plotted between atomic number and atomic radius of group 17 and group 1 elements.

""CBSE-Class-10-Chemistry-Periodic-Classification-Of-Elements-Worksheet-Set-A

Question. What happens to atomic radii in a group from top to bottom?
(a) Increases
(b) Decreases
(c) First decreases then increases
(d) Number of shells remains the same
Answer : A

Question. Which group elements will have largest atomic size?
(a) Group 1
(b) Group 2
(c) Group 3
(d) Group 18
Answer : A

Question. Which element in group 17 has smallest size?
(a) Flourine
(b) Bromine
(c) Chlorine
(d) Iodine
Answer : A

Question. Which group elements will gain electrons to form negative ions?
(a) Group 1
(b) Group 2
(c) Group 17
(d) Group 18
Answer : C

Question. Atomic size decreases from left to right in a period because
(a) Effective nuclear charge increases
(b) Number of shells remains the same
(c) Force of attraction between the nucleus and valence electrons increases
(d) All of these
Answer : D

 

 

Assertion Reason type Questions

In the following questions a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
(A) Both assertion and reason are true and the reason is the correct explanation of assertion.
(B) Both assertion and reason are true and the reason is not the correct explanation of assertion.
(C) Assertion is true but the reason is false.
(D) Both assertion and reason are false.
(E) Assertion is false but reason is true.

Question. Assertion: Properties of an atom and its corresponding ion remains the same.
Reason: Electronic configurations of both atom and ion remain same.
Answer : D

Question. Assertion: Elements in the same vertical column have similar properties.
Reason: The properties of elements are periodic functions of their atomic numbers.
Answer : B

Question. Assertion: Fluorine is more reactive than Chlorine.
Reason: The chemical reactivity of non-metals increases down the group.
Answer : C

Question. Assertion: Group 18 elements are inert.
Reason: They have completely filled valence shell.
Answer : A

Question. Assertion: Isotopes of an element were given separate places in Mendeleev’s periodic table.
Reason: Isotopes of an element have different atomic masses.
Answer : E

Question. Assertion : In Mendeléev Periodic Table, cobalt was placed before nickel.
Reason : The atomic mass of cobalt is less than nickel
Answer : C

Question. Assertion : According to Mendeleev, periodic properties of elements is a function of their atomic number.
Reason : Atomic number is equal to the sum of number of protons and neutrons.
Answer : D

Question. Assertion: Li,Na,K belong to Dobereiner’s triads
Reason: The atomic mass of Na is the average of atomic masses of Li and K
Answer : A

Question. Assertion : Atomic size decreases along a period.
Reason : Effective nuclear charge decreases as the atomic number increases resulting in the increased attraction of electrons to the nucleus
Answer : C

Question. Assertion: Mendeleev left some gaps in his Periodic Table
Reason: Mendeleev believed that some elements would be discovered later
Answer : A

 

Very Short Answers

Question : How does valency of an element vary across a period?
Answer : The valency of an element first increases and then decreases across a period.
 
Question : The atomic number of three elements A, B and C are 11, 14 and 17 respectively.
i. State the group to which these elements belong in the modern periodic table.
ii. Write the formula of the compound formed when the element A reacts with C. (1)
Answer : i. A, B, C belongs to the group number 1 ,14 and 17 respectively which belongs to alkali metals, carbon family and halogens respectively.
ii. Formula for A and C will be AC or NaCl.
 
Question : 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? 
Answer : Elements with atomic numbers 12 and 38 have the similar chemical and physical properties of calcium. 
 
Question : State the Periodic Law on which the Modern Periodic Table is based.
Answer : Periodic Law on which the Modern Periodic Table is based is termed as Modern Periodic Law. According to Modern Periodic Law—The properties of elements are a periodic function of their atomic numbers.
 
Question : Chlorine, bromine and iodine form a Dobereiner's triad. The atomic masses of chlorine and iodine are 35.5 and 126.9, respectively. Predict the atomic mass of bromine. 
Answer : According to Dobereiner’s triad, when three elements in a traid were written in the order of increasing atomic masses, the atomic mass of the middle element is roughly the average of the atomic masses of the other two elements.
Thus, the atomic mass of bromine
A-36
 
Question : The electronic configuration of an element X is 2, 8, 8, 2. To which period and group of the modern periodic table does X belong? State its valency. Justify your answer in each case. 
Answer : Period - 4, as number of shells are 4 and group - 2 as valence shell has 2 electrons.
 
Question : State the common characteristic of the following elements: Boron, Silicon, Germanium and Arsenic 
Answer : Boron, silicon, Germanium and Arsenic elements are metalloids. They possess the properties of both metals and non-metals. zag line separates metals from non-metals and the borderline elements show the properties of left hand side elements (metals) and right hand side elements (non-metals and are called metalloids or semi-metals). 

Question : Give one example of Döbereiner’s Triad.
Answer :  Li,   Na,     K
         7    23      39

Question : What is the limitation of Döbereiner triads?
Answer : He failed to arrange all the elements in triads having same chemical properties.

Question : Give two limitations of Newlands’ law of Octaves.
Answer :  Two limitations of Newlands’ law of octaves are:
(i) The law was applicable only upto calcium.
(ii) In order to fit elements into his table, Newlands adjusted two elements in wrong slot, and grouped unlike elements in same groups.

Question : Which two chemical properties were considered by Mendeleev for grouping of elements?
Answer : The two chemical properties are:
(a) The nature of compounds formed by elements with oxygen.
(b) The nature of compounds formed by elements with hydrogen.

Question : Define ‘groups and periods’.
Answer : The vertical columns in a Periodic Table are called groups and the horizontal rows are called periods.

Question : Name three elements discovered later, which filled gaps left by Mendeleev for them.
Answer :  Scandium, gallium and germanium.

Question : How many groups and periods are present in the Modern Periodic Table?
Answer : Modern Periodic Table has 18 groups and 7 periods.

Question : State Modern Periodic Law.
Answer :  ‘Properties of elements are a periodic function of their atomic number’.

Question : Fluorine (F) atomic number 9 and chlorine (Cl) atomic number = 17 are placed in group number17, what are the number of valence electrons present in them.
Answer :  Fluorine atomic number 9 = 2, 7
Chlorine atomic number 17 = 2, 8, 7
Both of them show 7 valence electron.

 

Short Answers

Question : List the limitations of Newlands’ Law of Octaves?
Answer : Limitations of Newlands’ Law of Octaves:
(1) It was not applicable for all the elements. It was applicable only till calcium, as after calcium every eighth element did not possess properties similar to that of the first. 
(2) It was assumed by Newlands that only elements existed in nature and no more elements would be discovered in the future. But, later on, several new elements were discovered, whose properties did not fit into the Law of Octaves.
(3) Cobalt and nickel are placed in the group of halogens with the elements fluorine and chlorine (F, Cl) which have different properties and it was not explained for the same.
(4) Placing of iron far away from cobalt and nickel, which have similar properties as iron, could also not be explained. Thus, Newlands’ Law of Octaves worked well with lighter elements only.
 
Question : Answer the following:
(A) Name any three halogens.
(B) Mention the group to which they belongMand their valency.
(C) What type of compounds will they form with elements of group 1?
Answer : (A) Three halogens are Fluorine, Chlorine and Bromine.
(B) They belong to the Halogen group or Group 17 of the periodic table. Their valency is 1.
(C) All the alkali metals react vigorously with halogens to produce salts, the most industrially important of which are NaCl and KCl.
2Na(s) + Cl2(g) → 2NaCl(s)
 
Question : 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)
Answer : Chlorine has the electronic configuration 2, 8, 7.
a. Atomic number of element is 17.
b. F (9). ( 2, 7)
 
Question : On the basis of the electronic configuration, how will you identify: Chemically similar elements. 
Answer :  Chemically similar elements can be identified with the help of the valence shell configuration of their atoms. The atoms having same valence shell configuration are chemically similar. For example Mg (Z = 12) and Ca (Z = 20) are chemically similar because the valence shell of both these elements have two electrons.

Question : Out of lithium and potassium, which one has stronger metallic character and why?
Answer : On going down in a group of the periodic table, the metallic character of elements increases. Therefore, potassium has stronger metallic character than Lithium. The reason behind is that as we go down in a group of the periodic table, one more electron shell is added. As a result, the size of the atom increases. The valence electrons move away from the nucleus at regular intervals. The holding capacity of the nucleus on valence electrons decreases. Due to this the atom can lose valence electrons more easily to form positive ions, and hence the metallic character increases. 

Question : Write the number of valence electrons present in a nitrogen atom (147N).
Answer : Valence electrons present in a nitrogen atom (14 7N) = Number of electrons in outermost or valence shell 147N
7—Atomic number
14—Mass number Atomic number = Number of protons = Number of electrons
 Number of electrons in nitrogen 7
Electronic configuration k L 2 5
Hence, valence electrons present in nitrogen are 5.
 
Question : Calcium is an element with Z = 20.
a. Is it a metal or a non-metal?
b. Will its size be bigger or smaller than that of potassium?
c. write the formula of its chloride. 
Answer :  Z = 20 is 2, 8, 8, 2
a. It is a metal which has two valence electrons, it is present in group 2
b. Both potassium (K) and calcium (Ca) are present in fourth period. Since atomic size decreases along a period calcium is slightly smaller in size than K whose electronic configuration is 2, 8, 8, 1
c. The valency of calcium is 2 and formula of its chloride is CaCl2
 
Question :  In the following pairs, choose the atom having bigger size: 
Mg (At. No. = 12) or Cl (At. No. = 17)
Answer : The electronic configurations of the two elements are
Mg (Z = 12) = 2, 8, 2
Cl (Z = 17) = 2, 8, 7
Both the elements belong to the third period. Since the atomic number of Cl is more than that of Mg, it comes after Mg in its period. Now, the atomic size decreases along a period. Therefore, Mg has bigger atomic size than Cl.

Question : An element X has mass number 35 and the number of neutrons is 18. Identify the group number and period of X. 
Answer : Mass no. = Sum of protons + Sum of neutrons
35 = Sum of protons + 18
Sum of protons = 35 – 18
Sum of protons = 17
Hence, we can say that the atomic number of element X is 17.
Its electronic configuration will be 2, 8, 7.
Thus it is clear that element X belongs to the 3rd Period and the 17th Group

Question : List two anomalies of Mendeleev’s periodic table which were solved by modern periodic table law.
Answer : (i) Position of isotopes were not justified in Mendeleev’s periodic table but it is justified in the modern periodic table.
(ii) Increasing order of atomic masses could not be followed but increasing order of atomic numbers has been followed.

Question : Predict the maximum number of valence electrons possible for the elements in the first period of periodic table.
Answer : 2 valence electrons are present in the last element ‘Helium’ of 1st period.

Question : (a) Among the following elements identify the one that would form anions:
K, O, Na, F, Ca, Cl, Hg
(b) Write the electronic configuration of the anions identified above.
Answer : (a) O, F, Cl will form anions.
(b) O2–(10)         2, 8
       F–(10)          2, 8
      Cl–(18)          2, 8, 8.

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

Question : An element belongs to third period and second group of the periodic table:
(a) State number of valence electrons in it. (b) Is it a metal or non-metal?
(c) Name the element. (d) Write the formula of its oxide.
Answer : (a) 2, 8, 2 is the electronic configuration. The number of valence electrons = 2
(b) It is a metal
(c) Magnesium
(d) MgO is the formula of its oxide.

Question : Why lithium with atomic number 3 and potassium with atomic number 19 are placed in group one?
What will be atomic numbers of first two elements of second group?
Answer :  K L M N
Li(3)          2, 1
K(19)        2, 8, 8, 1
Li and K are placed in Group 1 because both have 1 valence electron.
Be(4) and Mg(12) are first two elements of Group 2.

Question : State the reasons for the following:
(a) The elements of the same group have similar chemical properties.
(b) The elements of the same period have different properties.
Answer : (a) It is because they have the same number of valence electrons.
(b) It is because they differ in the number of valence electrons.

Question : How it can be proved that the basic structure of the Modern Periodic Table is based on the electronic configuration of atoms of different elements?
Answer : Position of element in periodic table is decided with the help of electronic configuration e.g. group number is decided on the basis of valence electrons e.g., elements having valence electrons 1,2,3,4,5,6,7,8, belong to Group 1, 2, 13, 14, 15, 16, 17 and 18 respectively. Period is equal to number of shells e.g. 2,8,3 belong to third period.

Question : Choose from the following: 6C, 8O, 10Ne, 11Na, 14Si
(a) Elements that should be placed in the same period.
(b) Elements that should be placed in the same group.
State the reason for your selection in each case. 
Answer : (a) 6C, 8O, 10Ne belong to the same period because all these have 2 shells. 11Na, 14Si belong to the same period because both of these have 3 shells.
(b) 6C and 14Si belong to the same group because they have the same number of valence electrons and valency.

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) It belongs to Group 14, third period.
(b) Silicon is the element. It is a metalloid, forms covalent bond. It is a semiconductor.

Question : An element ‘X’ has atomic number 13.
(a) Write its electronic configuration.
(b) State the group to which ‘X’ belong.
(c) Is ‘X’ a metal or non-metal?
(d) Write the formula of its bromide.
Answer : (a) 2, 8, 3, (b) Group 13, (c) Metal, (d) AlBr3

Question : (a) Predict the following which will form anions and which will form cations:
(i) Na (ii) Al (iii) Cl (iv) O
(b) Name two elements that are inert.
Answer : (a) Cl and O will form anions
Na and Al will form cations
(b) He, Ne are inert

Question : (a) State two main characteristics of elements on which modern periodic table is based.
(b) No fixed position can be assigned to hydrogen in the periodic table. Why?
Answer : (a) (i) Atomic number, (ii) No. of valence electrons
(b) It is because hydrogen resembles with Group 1 as well as Group 17 elements, therefore no fixed position can be assigned to it.

Question : The electrons in the atoms of four elements A, B, C and D are distributed in three shells having 1, 3, 5 and 7 electrons in the outermost shell respectively. State the period in which these elements can be placed in the modern periodic table. Write the electronic configuration of the atoms A and D and the molecular formula of compound formed when A and D will combine.
Answer : They belong to third period because these have 3 shells.
A has electronic configuration 2, 8, 1, valence electron 1, valency = 1
D has electronic configuration 2, 8, 7, valence electron 7, valency = 1
Formula: AD or A+D

Question : Name the element which has
(a) the electronic configuration 2, 8, 1
(b) a total of two shells, with 4 electrons in the valence shell.
(c) total of three shells, with 3 electrons in valence shell.
(d) One shell which is completely filled with electrons.
(e) twice as many electrons in the second shell as in the first shell.
Answer : 1. (a) Sodium (2, 8, 1)
(b) Carbon (2, 4)
(c) Aluminium (2, 8, 3)
(d) Helium (2)
(e) Carbon (2, 4)

Long Answers

Question : The element of a period of the periodic table are given below in order, from left to right with one of its element missing. 
Li Be B C O F Ne
i. To which period to these elements belong?
ii. One element of this period is missing. Which is the missing element and where should it be placed?
iii. Which one of these elements in the period shows the property of catenation?
iv. Which one of the above elements belongs to the halogen series?
v. Identify the noble gas.
Answer : i. All of these elements belongs to the 2nd period. Second period consists of 8 elements in total.
ii. Nitrogen (N) is missing from these elements. It should be placed between carbon and oxygen in the V A group.
iii. Carbon (C) shows the property of catenation.
iv. Fluorine (F) belongs to the halogen series
v. Neon (Ne) is the noble gas.
 
Question : An element P (atomic number 20) reacts with an element Q (atomic number 17) to form a compound.
Answer the following questions giving reason:
Write the position of P and Q in the Modern Periodic Table and the molecular formula of the compound formed when P reacts with Q.
Answer : Atomic number of element P = 20
Electronic configuration of element P = 2, 8, 8, 2
Atomic number of element Q = 17
Electronic configuration of element Q = 2, 8, 7
The position of P in the Modern Periodic Table
Period (Number of shells) = 4
Group (Electrons in outer-most shell) = 2
The position of Q in the Modern Periodic Table
Period (Number of shells) = 3
Group (Electrons in outer-most shell) = (10 + 7) = 17
When P reacts with Q, it loses the two valence electrons (valency 2).
These two valence electrons are accepted by two Q atoms (valency 1).
Hence, the formula of the compound formed between P and Q is PQ2.
 
Question : Consider two elements A (atomic number = 17) and B (atomic number = 19). 
i. Write the positions of these elements in the modern periodic table giving justification.
ii. Write the formula of the compound formed when A combines with B.
iii. Draw the electron dot structure of the compound and state the nature of the bond formed between the two elements.
Answer : i. Atomic number of A = 17 . Atomic no 17 is of element chlorine (Cl) which belongs to VII A group, Halogen group and 3rd period. It is a non-metal and lacks one electron in its outer most shell for its octet to complete. Electronic configuration of A = 2, 8, 7 .
ii. Atomic number of B = 19 . Atomic no. 19 is of element potassium (K) latin name kalium which belongs to I A group, group of Alkali metals and 4th period. It is a very reactive metal and has 1 electron in its outermost shell.
Electronic configuration of B = 2, 8, 8, 1
Position of the elements in the periodic table:
A-34
 
iii. Atomic number of A = 17, E.C. of A =2, 8, 7
=> Valency = 1
Atomic number of B = 19, E.C. of B = 2, 8, 8, 1
=> Valency = 1
  Symbol A B
 Valency 1 1
Hence, the formula of compound is AB.
iv. The electron dot structure of compound AB will be
A-35
The nature of bond will be electrostatic. Thus, compound of these two is AB.
 
Question : From the elements 1939A, 1428B, 816C and 1840D identify:
(a) the most electropositive element.
(b) a noble gas.
(c) a metalloid.
(d) an element which will gain 2 electrons to attain nearest noble gas configuration.
(e) formula of compound formed between A and C.
(f) elements belonging to same period.
Answer : 
(a) 1939A is most electropositive element
(b) 1840D is noble gas
(c) 1428B is metalloid
(d) 816C will gain 2 electrons to attain nearest noble gas configuration

 

Question : The atomic numbers of the three elements X, Y and Z are 2 ,6 and 10 respectively.

(i)Which two element belong to the same group?

(ii)Which two elements belong to the same period?Give reasons.

Question : An element X belongs to 3rd period and group 2 of the periodic table. State

(a) Number of valance electrons.

(b) Valency

(c) Metal or non-metal.

(d) Name of the element.

Question : An element X is in group 2 of the periodic table

(a) What will be the formula of its chloride.

(b)What will be the formula of its oxide.

Question : An element X has mass number 40 and contains 21 neutrons in its atom.To which group of the periodic table does it belong?

Question : Find the neutral atom in the periodic table which has the same number of electrons as K+ and Cl-. What is this number?

Question : The elements X, Y and Z belong to group 2, 14 and 16 respectively of the periodic table

(a) Which two elements will form covalent bond?

(b) Which two elements will form an ionic bond?

Question : The elements A, B, C and D belong to groups 1, 2, 14 and 17 respectively of the periodic table. Which of the following pairs of elements would produce a covalent bond?

(i) A and D (ii) C and D (iii) A and B (iv) B and C

Question : A metal X is in the first group of the periodic table.What will be the formula.

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Worksheet for CBSE Science Class 10 Chapter 5 Periodic Classification of Elements

We hope students liked the above worksheet for Chapter 5 Periodic Classification of Elements designed as per the latest syllabus for Class 10 Science released by CBSE. Students of Class 10 should download in Pdf format and practice the questions and solutions given in the above worksheet for Class 10 Science on a daily basis. All the latest worksheets with answers have been developed for Science by referring to the most important and regularly asked topics that the students should learn and practice to get better scores in their class tests and examinations. Expert teachers of studiestoday have referred to the NCERT book for Class 10 Science to develop the Science Class 10 worksheet. After solving the questions given in the worksheet which have been developed as per the latest course books also refer to the NCERT solutions for Class 10 Science designed by our teachers. We have also provided a lot of MCQ questions for Class 10 Science in the worksheet so that you can solve questions relating to all topics given in each chapter.

Where can I download latest CBSE Printable worksheets for Class 10 Science Chapter 5 Periodic Classification of Elements

You can download the CBSE Printable worksheets for Class 10 Science Chapter 5 Periodic Classification of Elements for latest session from StudiesToday.com

Is there any charge for the Printable worksheets for Class 10 Science Chapter 5 Periodic Classification of Elements

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Are there any websites that offer free test sheets for Class 10 Science Chapter 5 Periodic Classification of Elements

Yes, studiestoday.com provides all latest NCERT Chapter 5 Periodic Classification of Elements Class 10 Science test sheets with answers based on the latest books for the current academic session

What topics are covered in CBSE Class 10 Science Chapter 5 Periodic Classification of Elements worksheets?

CBSE Class 10 Science Chapter 5 Periodic Classification of Elements worksheets cover all topics as per the latest syllabus for current academic year.

How can I use worksheets to improve my Class 10 Science scores?

Regular practice with Class 10 Science worksheets can help you understand all concepts better, you can identify weak areas, and improve your speed and accuracy.