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with Complete SolutionsQUESTION BANK
CLASS 10CHEMISTRY( )PART - 1
Strictly as per the Latest Syllabus and DesignPrescribed by SCERT Kerala Education Board
KERALA SSLC
FOR2017
EXAM
Based on Latest SCERT Textbook issued by Department of Education, Government of Kerala in 2016
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( 3 )
1. PERIODIC TABLE AND ELECTRONIC CONFIGURATION 5 - 21
Topic-1 : Bohr Atom Model – Shell and Subshell
Topic-2 : Electronic Configuration and Blocks
Topic-3 : Elements of s, p, d and f Blocks
Topic-3 : Periodic Trends in the Properties of Elements - Electronegativity and lonisation
2. MOLE CONCEPT 22 - 34
Topic-1 : Number and Mass
Topic-2 : Mole Concept and Avogadro's Low
Topic-3 : Mole Concept in Balanced Chemical Equations
3. RATE OF CHEMICAL REACTIONS AND CHEMICAL EQUILIBRIUM 35 - 46
Topic-1 : Speed of Chemical Reactions; Balanced Equations
Topic-2 : Le Chatelier's principle and Effect of Catalyst, Temperature and Pressure
4. REACTIVITY SERIES & ELECTROCHEMISTRY 47 - 56
Topic-1 : Displacement Reaction of Metals and Reactivity Series
Topic-2 : Chemical Effects of Electric Current
CONTENTS
( 4 )
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PREFACE
CHAPTER
1SyllabuS Bohr atom model – shell and subshell Subshell electronic configuration and blocks Periodic table Group number of s and p blocks elements Elements of d and f blocks Periodic trends in the properties of elements Electronegativity Ionisation energy
ToPiC-1
Bohr Atom Model – Shell and Subshell
QuICK REVIEW
Significance of Periodic Table : • The periodic table helps to simplify and systematize the study
of the elements, the basic units of all substances. • It is also useful in analyzing the millions of compounds formed
by the combination of elements. Elements are classified into 4 blocks. They are : • s block • d block • p block • f block
The basic reason for the periodicity in the properties of elements in the periodic table is their electronic configuration.
The properties of elements are influenced mainly by the electronic arrangement in their atoms. According to the Bohr scheme, electrons that move around the nucleus have definite paths. Bohr model of atom has shells K, L, M, N… etc. Shells can also be referred to as 1, 2, 3, 4.... energy levels respectively. Electrons present in each such shell or orbit have a definite energy. Therefore, shells are also known as energy
levels. An electron in the K shell has a fixed energy. To transfer an electron from the K shell to the L shell, a definite amount of energy has to be supplied. The energy of L shell is higher than that of K shell. Electrons are accommodated in shells in the increasing order of energy. Electrons are filled first in the lowest energy orbit and then in the next higher energy orbits. The shells in an atom are filled with electrons in the increasing order of their energy. The Bohr model provides a simple explanation of the electronic structure of an atom. The Bohr model became obsolete, as it was unable to explain the properties of elements of higher atomic numbers. Studies related to the position and properties of electrons in an atom led to the conclusion that the electrons in
each energy level are distributed in the various subenergy levels in it. These subenergy levels are called subshells. They are named s, p, d, f. s → sharp, p → principal, d → diffuse,
f → fundamental. The number of subshells in a shell is equal to the serial number of the shell. The first shell has only one subshell (s), the second has two (s, p), and so on.
PERioDiC TABLE AND ELECTRoNiC CoNFiGURATioN
TOPIC - 1Bohr Atom Model – Shell and Subshell .... P. 5
TOPIC - 2Electronic Configuration and Blocks .... P. 9
TOPIC - 3Elements of s, p, d and f Blocks .... P. 13
TOPIC - 4Periodic Trends in the Properties of Elements – Electronegativity and Ionisation .... P. 17
6 ] Oswaal Kerala SSLC Question Bank, Chemistry, Class – X
Each subshell can accommodate a fixed number of electrons. The s subshell can accommodate a maximum of 2 electrons. The K shell has only the s subshell and hence it can have only 2 electrons. To identify the shell to which the subshell belongs, the subshells are represented by including the shell number
also as 1s, 2s, 2p... etc. Each shell has definite energy. Intensive studies have proved that subshells in a shell differ slightly in their energy, as the energy of electrons
present in a shell may vary slightly. The increasing order of energy of subshells is represented as s < p < d < f....
Calledrepresentative
elements
Extreme leftof periodic
Table
s-block
Consist metalsnon-metals
and metalloids
Extreme rightof periodic
Table
p-block
Also calledtransitionmetals
In middleof periodic
Table
d-block
Consist of twoseries lanthanides
and actinoids
At the bottomof periodic
Table
f-block
Periodic Table
Periodic Table andElectronic Configuration
is the distribution of electionsin different subshells
Electronic Configuration
KNOW THE TERMS
Bohr atom model : Represented an atom consisting of a small, positively charged nucleus orbited by negatively charged electrons.
Electron shell : A grouping of electrons surrounding the nucleus of an atom. Electron subshells : A subdivision of electron shells separated by electron orbitals.
Bohr atomic model
Main energy levels Maximum number of electrons
accommodated
Number of electrons accommodated and
name of the subshell
Number of subshellsSI. No. of shell Shell
1 K 2 21s
1
2 L 8 2 62s 2p
2
3 M 18 2 6 103s 3p 3d
3
4 N 32 2 6 10 164s 4p 4d 4f
4
PERIODIC TABLE AND ELECTRONIC CONFIGURATION [ 7
Very Short Answer Type Questions (1 mark each)
Q. 1. What is common name of group 1 and 2 elements ? [TBQ]
Ans. s-block elements. 1 Q. 2. Do s-block element donate or receive electrons ?
[TBQ] Ans. They donate electrons. 1 Q.3. What does subshells s, p, d and f stand for ? Ans. s → sharp, p → principal, d → diffuse,
f → fundamental. 1 Q.4. What is the shape of s subshell ? Ans. The shape of s subshell is spherical. 1 Q.5. What is the shape of p subshell ? Ans. The p-subshells are dumb-bell shaped. 1 Q.6. How many orbitals are present in p subshell ? Ans. Three. 1 Q.7. How many orbital are present in d subshell ? Ans. Five. 1 Q.8. How many orbital are present in f subshell ? Ans. Seven. 1
Q.9. How many electrons are present in the M shell of argon which is its outermost shell ? [TBQ]
Ans. 18 Ar 2 8 8
K L M 1
Q.10. What is the basis of the classification of elements in the periodic table?
Ans. The classification of elements in the periodic table is done in such a way that their properties can be precisely and clearly analysed and predicted. 1
Q.11. How many subshell does K shell have ? Ans. 1 subshell i.e., s. 1 Q.12. How many subshell does L shell have ? Ans. 2 subshells i.e., s, p. 1 Q.13. How many subshell does M shell have ? Ans. 3 subshells i.e., s, p, d. 1 Q.14. How many subshell does N shell have ? Ans. 4 subshells i.e., s, p, d and f. 1 Q.15. Which subshell is common to all shells ? [TBQ] Ans. s. 1
Short Answer Type Questions-I (2 marks each)
Q. 1. A few subshells of an atom are given below.4d, 5s, 3f, 2p
(a) Which subshell is not possible ? (b) What is the reason for this ? [TBQ] Ans. (a) 3f. (b) The number of subshells in a shell is equal to
the serial number of the shell. The first shell has only one subshell (s), the second has two (s, p), the third subshell has (s, p, d), and so on. Each subshell can accommodate a fixed number of electrons. The maximum number of electrons that can be accommodated in the third subshell is 18, i.e., 3s2 3p6 3d10. Therefore, 3f subshell is not possible. 1+1
Q. 2. Look at the subshell electronic configuration of some atoms given below.
1s2 2s2 3s2
1s2 2s2 2p6 3s1
1s2 2s2 2p7
1s2 2s2 2p63s2 3p6 3d5
1s2 2s2 2p63s2 3p6 3d5 4s2
(a) Which are the wrong configurations ? (b) Give the reason. Ans. (a) 1s2 2s2 3s2
1s2 2s2 2p7
(b) 1s2 2s2 3s2 – The second shell has two subshells (s, p). Electrons are accommodated in shells in the increasing order of their energy i.e., s < p < d < f....
1s2 2s2 2p7 – Maximum number of electrons can accommodate in the second subshell is 8. 1+1
Q.3. Draw the shape of s subshell.
Ans.
y
z
x
s subshell 2 Q.4. Draw the shape of p subshell. Ans.
yx
py
z
yx
px
z
yx
pz
z
p subshell 2
8 ] Oswaal Kerala SSLC Question Bank, Chemistry, Class – X
Q.5. Explain the modern theories of atomic structure. Ans. according to modern theories of atomic structure,
electrons revolve in a three dimensional region around the nucleus. Each main energy level has sub levels or subshells. In these subshells, there are regions where there is high probability of finding electrons known as orbitals. 2
Q.6. Explain the Bohr model of the atom. Ans. According to the Bohr model of the atom, electrons
are arranged in different shells or energy levels around the nucleus in the increasing order of the energy. 2
Q.7. How can we identify the shell to which each subshell belongs ?
Ans. We can attach the serial number of the shell to the symbol of the subshell. For example, ‘1s’, to indicate the s subshell of the first shell and ‘2s’ for the s subshell of second shell and so on. 2
Short answer Type Questions-II (3 marks each)
Q. 1. Where are the d-block elements placed in periodic table ? From which period does it start ? Give two characteristics of d-block elements.
Ans. d-block elements lie in between of s-block and p-block elements.
d-block starts from third period.
(i) There are metals.
(ii) d-block elements show variable valency. 3
Q.2. Fill in the blanks in the below given table :
Shell Number 1 2 3 4
Subshell s s p s p d s p d f
Representation of the subshell
1s – – – 3p – – – 4d 4f
[TBQ] Ans. Shell Number 1 2 3 4
Subshell s s p s p d s p d f
Representation of the subshell
1s 2s 2p 3s 3p 3d 4s 4p 4d 4f
3
long answer Type Questions-I (4 marks)
Q. 1. If the subshell electronic configuration of an atom is 1s22s22p63s2, find answers to the following :
(i) How many shells are present in this atom ? (ii) Which is the subshell to which the last
electron was added ? (iii) What is the total number of electrons in the
atom.
(iv) What is its atomic number ? [TBQ] Ans. (i) Atom consist of 3 shell. (ii) Last electron added in s-subshell. (iii) Atom consist of 12 electrons. (iv) Atomic no. of element is 12. 4
long answer Type Questions-II (5 marks)
Q. 1. Analysis the given table and answer the following questions : [2016]
Element (Symbols are not real)
Atomic number
P 11
Q 18
R 17
S 26
(a) Identify the noble gas among these elements.
(b) Identify the element belonging to group 1. (c) Identify the type of compound formed by P
and R. (Electronegativity values P = 0.90 and R = 3.00)
(d) Which is the element showing variable valency ? Write the subshell electronic configuration of the element.
Ans. (a) Q (b) P (c) Ionic compound (d) Element S. 26S = 1s22s22p63s23p64s23d6 1+1+1+2
Multiple Choice Questions (1 mark each)
1. What is the maximum number of electrons that are permitted in a p subshell ?
(a) 2 (b) 3 (c) 6 (d) 10 Ans. (c) 6.
2. What is the maximum number of unpaired electrons in a d subshell ?
(a) 0 (b) 1 (c) 5 (d) 10 Ans. (c) 5.
PERIODIC TABLE AND ELECTRONIC CONFIGURATION [ 9
3. What is the maximum number of electrons that are permitted in an f subshell ?
(a) 5 (b) 6 (c) 10 (d) 14 Ans. (d) 14. 4. How many orbitals are there in f subshell ? (a) 3 (b) 4
(c) 5 (d) 7 Ans. (d) 7. 5. Shell number 2 contains _______ subshells. (a) s (b) s, p (c) s, p, d (d) s, p, d, f Ans. (b) s, p.
KNOW THE lINKS
http://chemphys.armstrong.edu/P1/AtmStr.htm http://science.jrank.org/pages/982/Bohr-Model.html
ToPiC-2
Electronic Configuration and Blocks
QuICK REVIEW
Electrons are accommodated in shells in the increasing order of their energy. When electrons are filled in a shell of an atom, they are actually accommodated in the respective subshells of the
shell. The number of electrons in an atom is equal to its atomic number (Z). Atomic number of hydrogen is 1. The subshell electronic configuration of hydrogen can be represented as 1s1. It is read as ‘one’s one’. The number at the right top shows the number of electrons. Atomic number of helium (He) is 2, i.e., number of electrons is 2. Therefore, the subshell electronic configuration
for helium is 1s2. Number of electrons in the atom of lithium (Li) is 3 and its subshell electronic configuration is 1s2 2s1. Be (Z = 4) - 1s2 2s2 and B (Z = 5) - 1s2 2s2 2p1
The outermost electron in helium fills in the s subshell. Therefore, it should have been placed in the s block. However, helium being a noble gas, it is placed in the p block along with other noble gases.
Electronic configuration of Cl (Z = 17) - 1s2 2s2 2p6 3s2 3p5, therefore, it belongs to p block. Electronic configuration of Ar (Z = 18) - 1s2 2s2 2p6 3s2 3p6, therefore, it belongs to p block. Atomic number of potassium is 19. Its shell-wise electronic configuration is 2, 8, 8, 1. In potassium the electron goes to 4s subshell in preference to 3d. This is the reason for potassium being an s block
element. The subshell electronic configuration of potassium is 1s2 2s2 2p6 3s2 3p6 4s1. Though electrons are filled in 3d subshell only after 4s, the subshells of the same shell are to be put together while
writing the electronic configuration. The electronic configuration of scandium (Z = 21) is 1s2 2s2 2p6 3s2 3p6 3d1 4s2. In the case of chromium (Z = 24), instead of the 2 electrons filling in the outermost 4s subshell, one of them goes
to 3d subshell. Its configuration, therefore, is 1s2 2s2 2p6 3s2 3p6 3d5 4s1. The electronic configuration of copper (Z = 29) also has such a rearrangement. Its configuration is 1s2 2s2 2p6 3s2
3p6 3d10 4s1. The d5 and d10 are stable electronic configurations in the d subshell. The rearrangement of electrons in Cr and Cu is to attain these stable electronic configurations.
KNOW THE TERMS
Electronic configuration : The representation of the arrangement of electrons distributed among the orbital shells and subshells.
Noble gas : The chemical elements in group 18 of the periodic table.
Oswaal Kerala SSLC Question Bank ForClass 10 Chemistry (Part-1) With
Complete Solutions For 2017 Exam
Publisher : Oswaal Books ISBN : 9789386177520 Author : Panel Of Experts
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