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