CBSE Class 10 Chemistry Periodic Classification Of Elements Worksheet Set B

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Worksheet for Class 10 Science Chapter 5 Periodic Classification of Elements

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Class 10 Science Worksheet for Chapter 5 Periodic Classification of Elements

Objective Questions

Question : Which type of compound is formed by the elements of group 1 and group 17? 
a. covalent compound
b. Organo-metallic compounds
c. coordinate compound
d. Ionic compound
Answer : D 
Explanation: Elements of group 1 can readily lose 1 electron to complete their octet.
Elements of group 17 need one electron to complete their octet. So, both of them combine with each other and form ionic compounds.
 
Question : Metallic character _________ down a group. 
a. remains the same in the group
b. decreases
c. First increase then decrease
d. Increases
Answer : D
Explanation: As we go down in a group, one more electron shell is added at each stage and size of the atom increases. The valence electrons become more and more far away from the nucleus and so the atom can lose electrons more easily to form positive ions. Therefore, metallic character increases down the group.
 
Question : Which one of the following is the most reactive? 
a. Bromine
b. Iodine
c. Chlorine
d. Fluorine
Answer : D
Explanation: Of all the halogens given, Fluorine is the most reactive as the reactivity of non-metals decreases on going down the group.
 
Question : Which of the following elements can be classified into group of triads?
a. Sr, Ca, Br
b. Cl, Br, I
c. Na, Cl, K
d. Cl, Ca, Br
Answer : B
Explanation: According to Dobereiner's law of triads, when elements are arranged in the order of increasing atomic masses, groups of three elements having similar chemical properties are obtained. The atomic mass of the middle element is equal to the arithmetic mean of the atomic masses of other two elements.
If we calculate the arithmetic mean of atomic masses of Cl and I , we would obtain the mass of Br.
35.5+127/2 = 81.2
 
Question : An element with atomic no 3 combines with another element with atomic number 17, What would be the formula of the compound? 
a. Lif
b. NaCl
c. LiCl
d. BeCl2
Answer : C 
Explanation: An element with atomic no 3 has electronic configuration 2,1 i.e. it can lose one electron readily to complete its duplet.
The element with atomic no 17 has electronic configuration 2,8,7 and is ready to accept one electron to complete its octet. 
 
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 : 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 : 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 : 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 : 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 : 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 : 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 : An element ‘X’ is placed in group 13 and third period of the Periodic Table. It burns in oxygen to form an oxide which is amphoteric in nature. Identify the chemical formula of its chloride
(a) CCl4
(b) BCl2
(c) GaCl3
(d) AlCl3
Answer : D 

Question : In the Modern Periodic Table calcium (Z = 20) is surrounded by the elements with atomic numbers 12, 19, 21, and 38 which of the following will have physical and chemical properties resembling calcium.
(a) 12, 20, 38
(b) 12, 19, 20, 38
(c) 19, 20, 38
(d) 12, 19, 20
Answer : A

Case Study Questions

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

Question : How electronegativity varies in a period?
(a) Increases down the group
(b) Decreasing down the group
(c) First increases then decreases down the group
(d) Vary independently
Answer : B

Question : Which element has highest electronegativity?
(a) C
(b) N
(c) O
(d) F
Answer : D

Question : What happens to tendency to gain electron in a period?
(a) Increases,
(b) Decreases,
(c) Remaining same,
(d) First increases then decreases.
Answer : A

Question : How electronegativity varies in a period?
(a) Increases from left to right
(b) Decreases from left to right
(c) First increases then decreases
(d) Vary independently
Answer : A

Question : Which of the following has least electronegativity?
(a) Li,
(b) Be,
(c) O,
(d) N
Answer : A

 

Very Short Answers

Question : What were the limitations of Döbereiner’s classification?
Answer : (a) All the existing elements were not classified.
(b) Döbereiner could identify only three triads from the elements.
Hence this system was not useful.

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

Answer :

CBSE Class 10 Chemistry Periodic Classification Of Elements Worksheet Set B-

Question : What were the criteria used by Mendeleev in creating his Periodic Table?
Answer : (i) Increasing order of atomic mass of the elements.
(ii) All elements in a group with similar properties.
(iii) The formula of oxides and hydrides formed by an element.

Question : How could the Modern Periodic Table remove various anomalies of Mendeleev’s Periodic Table?
Answer : Modern Periodic Table is based on the atomic number of elements, therefore
(i) problem of isotopes was solved because isotopes have same atomic number
(ii) wrong order of Ar, K, Co, Ni was removed.

Question : 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.

Answer :

CBSE Class 10 Chemistry Periodic Classification Of Elements Worksheet Set B-1

 
Question : The atomic radii of three elements A, B and C of a periodic table are 186 pm, 104 pm and 143 pm respectively. Giving a reason, arrange these elements in the increasing order of atomic numbers in the period.
Answer : Since atomic size decreases along a period and the atomic number increases. So, the element with smaller radii, has the highest atomic number. Hence, B has the highest atomic number followed by C and A i.e. A < C < B.
 
Question : Which is the main difference between Mendeleev's periodic table and long form of periodic table? 
Answer : Mendeleev's Periodic Table : Elements are arranged in increasing order of atomic masses.
Modern Periodic Table: Elements are arranged in increasing order of atomic numbers.
 
Question : How does the metallic character vary across the period? Explain.
Answer : Metallic character decreases as we move across a period in the periodic table from left to right. This occurs because as we move across a period, the nuclear charge increases and the tendency of the element to lose electrons decreases. 
 
Question : An element is present in a group IIA of the periodic table. Predict its two properties.
Answer :  Properties of group IIA element:
i. It has two electrons in the velence shell.
ii. It is of metallic nature.
 
Question : In the Modern Periodic Table, which are the metals among the first ten elements.
Answer : Lithium and beryllium are metals.

Question : Element X forms a chloride with the formula XCl2, which is 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) Al
(d) Si.
Answer : As the formula of chloride of element X is XCl2, it is a metal with valency 2 as it has a high melting point and is combining with Cl which is a non-metal having valency 1. Of the given elements, valency of (b) Mg is 2 (Atomic No. 12). Therefore, X will be in the same group as Mg in the Periodic Table. 

Question : Write the valency and usual number of valence electrons of group 18 of the periodic table. 
Answer :  18th group elements are known as noble gases or inert gases having 8 valence electrons, except Helium (2 valence electrons).
Therefore, Valency = 0 and
Usual number of valence electrons = 8.
 
Question : Give one reason for keeping both oxygen and sulphur in the same group of the periodic table. 
Answer :  Atomic number of oxygen is 8 and its electronic configuration is 2,6.
Atomic number of sulphur is 16 and its electronic configuration is 2,8,6.
Both oxygen and sulphur atoms have same number of electrons (6) in the valence shell of their atoms.
 
Question : Two elements ‘A’ and ‘B’ belong to group 1 and 2 respectively in the same period. Compare them with respect to size of their atoms.
Answer : Size of B will be smaller than the size of A because on moving from left to right in a period, the size of atoms decreases. When we move from left to right in a period, the number of electrons and protons increases. Due to the large positive charge on the nucleus, electrons are pulled more strongly towards the nucleus. 

Short Answers

Question. 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?

Answer : (a) Ne (2, 8) (b) Mg (2, 8, 2)
(c) Si (2, 8, 4) (d) B (2, 3)
(e) C (2, 4)

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 : (a) The atomic number of the element is 17.
(b) F(9) (2, 7) will be chemically similar to the given element.

Question. Nitrogen (atomic number 7) and phosphorous (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?

Answer : Nitrogen atomic number 7 → 2, 5
Phosphorus atomic number 15 → 2, 8, 5
Nitrogen with two shells will be more electronegative because it can easily gain electron due to its smaller size of atom, the nuclear charge attracts the electron easily to become negative ion.

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 : Ca atomic number — 20
Electronic configuration — 2, 8, 8, 2
Elements with atomic number 12 → 2, 8, 2
and atomic number 38 → 2, 8, 18, 8, 2
will resemble calcium as they all have same valence electrons and their chemical properties are also same.

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 element? 
Answer : The Modern Periodic table consists of 18 vertical columns or ‘groups’ and 7horizontal rows or ‘periods’. As we move from left to right along a period, we observe that the elements have the same number of valence shells but the number of valence electrons increases by one unit. Similarly, as we move down a group, we observe that elements have the same number of valence electrons but the number of shells increases by one. This proves that the Modern Periodic Table is based on electronic configuration of atoms of elements.

Question : Answer the following:
(A) Why do elements in a group show similar property?
(B) An element M is in the third group of the periodic table. Write the formulae of its chloride and oxide.
Answer : (A) All the elements present in a group have same electronic configuration of the atoms. The physical and chemical properties of elements depend on the number of valence electrons. Elements present in the same group have the same number of valence electrons. Therefore, elements present in the same group have similar physical and chemical properties. 

Question : An element X is in second period of group 16 of the periodic table. Is it metal or nonmetal? Give reason for your answer. 
Answer :  Second period suggests that there are two shells present in the element while group 16 suggests that there are 6 valence electrons. Thus, electronic configuration is 2, 6. It is a non-metal as it contains 6 valence electrons. The element is having atomic number 8 the element is Oxygen and the symbol is O.
 
Question : Locate the following group in the periodic table: 
a. Alkali metals
b. Halogens
c. Alkaline earth metals 
Answer :  a. Alkali metals : The alkali metals, found in group 1 of the periodic table, are highly reactive metals that do not occur freely in nature.
b. Halogens : The halogens are five non-metallic elements found in group 17 or VIIA of the periodic table.
c. Alkaline earth metals : The alkaline earth elements are metallic elements found in the second group of the periodic table.
 
Question : From the elements Li, K, Mg, C, Al, S identify the:
(a) elements belonging to the same group.
(b) element which has the tendency to lose two electrons.
(c) element which prefers sharing of electrons
Answer : (a) Li, K
(b) Mg
(c) C
(d) K
(e) S (strongly acidic, C (weakly acidic)
(f) Al
 
Question : 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 valance shell?
d. twice as many electrons in its second shell as in its first shell? 
Answer :  a. Neon
b. Magnesium
c. Silicon
d. Carbon 
 
Question : Class IXth and Xth students went on an education trip along with their respective class teachers in two separate buses. Class teacher of class IXth asked the students to make' a queue according to their height while boarding or deboarding the bus whereas class teacher of class Xth asked the students to make a queue for the same purpose but according to their role numbers.
Read the given passage and answer the following questions.
i. Name two scientists who arranged elements in the periodic table with different criteria?
ii. Which criteria of making queue was better in your view and why?
iii. What value do you associate with the class teachers?
Answer :  i. Mendeleev arranged elements on the basis of their atomic mass. He suggested that physical and chemical properties of elements are the periodic function of their atomic masses. While Moseley arranged elements on the basis of their atomic number. He suggested that physical and chemical properties of elements are the periodic function of their atomic numbers.
ii. I think the queue in order of role number was better as in this order it is easy to find out if a student missed the bus or not.
iii. Both the teachers are disciplined, organized and concerned towards student's safety. 
 
Question : Elements have been arranged in the following sequence on the basis of their increasing atomic masses: F, Na, Mg, Al, Si, P, S, Cl, Ar, K
(A) Pick two sets of elements which have similar properties.
(B) The given sequence represents which law of classification of elements? 
Answer : (A) In this sequence, the elements are arranged in increasing order of their atomic masses. According to Newlands’ law of octaves, every eighth element will show similar properties as that of the first element. Hence, F and Cl, Na and K will show similar properties. Therefore, set I is F and Cl and set II is Na and K. Note: Although Na and K have similar properties but they are not related as first and eighth element in the above sequence.
(B) The given sequence represents Newland’s law of octaves. In the given sequence, elements are arranged in increasing order of their atomic mass and each 8th element shows similar properties. So, it represents Newlands’ law of octaves. F Na Mg Al Si P S Cl Ar K

Long Answers

Question :  What is atomic radius? How do the atomic radii of the elements change in a group? 
Answer : Atomic radius: The atomic radius of an element is related to the atomic size and may be defined as the distance between the centre of the nucleus of an atom and the outermost shell of electrons.
Variation of atomic radii in a group: In a group, the atomic radii of the elements increase as we move down the group. The atomic radii of the alkali metals of group 1 are shown in the table. The last element Francium (Fr) is radioactive and unstable.
Therefore, its atomic radius has not been determined.
Table: Atomic radii of Alkali Metals in Group I

 A-30

Explanation: In a group, as we move downwards there is a regular addition of one new shell.
For example.

A-31
 
Since the number of electron shells increases, the size of the elements increases down a group.
 
Question : The electronic configuration of three elements X, Y and Z are given below: 
X = 2; Y = 2, 6; Z = 2, 8, 2
i. Which element belongs to the second period?
ii. Which element belongs to the eighteenth group?
iii. Which element belongs to the second group?
iv. What is the valency of Y?
v. Y and Z are metal or non-metal.
Answer :  i. Y belongs to the 2nd period because number of shells in Y is two that is K and L.
ii. X belongs to the 18th group also known as zero group because its first shell is completely filled. It is an inert gas iii. Z belongs to the 2nd group because the number of valence electrons is 2. It will be kept in third period.
iv. Valency of Y is 2, (8 - 6 = 2). But, valence electron will be 6 only.
v. Y - non-metal, Z-metal
 
 
 

Question : How many groups and periods are there in the Modern periodic table?

Question : What was the prediction of Mendeleev regarding the gaps in his periodic table?

Question : How is valence of an element determined?

Question : What will be the valence of an element having atomic number 16?

Question : How does valence vary in going down a group?

Question : Why inert gases have zero valences?

Question : What would be the valence of an atom containing 8 electrons in its outermost shell?

Question : How does the electronegative character of elements vary along a period of the periodic table?

Question : The present classification of elements is based on which fundamental property of elements?

Question : Among first ten elements in the modern periodic table name the metals present.

Question : Metals are on which side of Modern periodic table?

Question : Name two elements, other than Gallium, whose existence was predicted by Mendeleev.

Question : State Modern Periodic law.

Question : Write the name given to the vertical columns in a periodic table.

Question : What name is given to the horizontal rows in a periodic table?

Question : Why does silicon is classified as Metalloid?

Question : Name the scientist who proposed modern periodic law? On which fundamental property of elements it is based?

Question : Why could no fixed position be given to hydrogen in Mendeleev’s Periodic table?

Question : What are metalloids? Give two examples.

Question : In group 1 of periodic table three elements X, Y and Z have atomic radii 133pm , 95pm and 65pm respectively giving a reason, arrange them in the increasing order their atomic number.

Question : How and why does the atomic size vary as you go down the group?

Question : Arrange the following is descending atomic size Na, Mg, K.

Question : Give the name and electronic configuration of second alkali metal? 

Question : What is the similarity in the electronic configuration of Mg, Ca and Sr? 

Question : Which is bigger in size Na OR K? 

Question : Name three elements which behave as metalloids? 

Question : Alkali metals form positive ions why?

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

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