Periodic Table MCQs Concise Class-10 ICSE Chemistry Selina Solutions Chapter-1. We Provide Step by Step Answer of MCQs, Exercise-1 Questions for ICSE Class-10 . The given Solutions is according to the Latest editions. Visit official Website CISCE for detail information about ICSE Board Class-10.
Periodic Table MCQs Concise Class-10 ICSE Chemistry Selina Solutions Chapter-1
| Board | ICSE |
| Book / Publication | Concise / Selina |
| Subject | Concise Chemistry |
| Class | 10th |
| Writer | Dr SP Singh |
| Chapter-1 | Periodic Table (Periodic Properties and Variations of Properties) |
| Topics | MCQs |
| Edition | 2025-2026 |
MCQs on Periodic Table with Questions and Answers
Page-15
Que-1: In the periodic table, alkali metals are placed in the group:
(a) 1
(b) 11
(c) 17
(d) 18
Ans: (a) 1
Hint- The elements placed in group 1 of the periodic table are known as alkali metals (except hydrogen) as they form strong alkalis with water.
Que-2: Which of the following properties does not match with the elements of the halogen family ?
(a) They have seven electrons in their valence shell.
(b) They are highly reactive chemically.
(c) They are metallic in nature.
(d) They are diatomic in their molecular form.
Ans: (c) They are metallic in nature.
Hint- Halogens are non-metallic in nature.
Que-3: With reference to the variation of properties in the Periodic Table, which of the following is generally true?
(a) Atomic size increases from left to right across a period.
(b) Ionization potential increases from left to right across a period.
(c) Electron affinity increases going down a group.
(d) Electronegativity increases going down a group.
Ans: (b) Ionization potential increases from left to right across a period.
Hint- On moving from left to right across a period, the atomic size decreases due to increase in the nuclear charge, and thus, more energy is required to remove the electrons. Hence, ionization potential increases from left to right across a period.
Que-4: An element in period 3 whose electron affinity is zero is :
(a) Neon
(b) Sulphur
(c) Sodium
(d) Argon
Ans: (d) Argon
Hint- Argon is the noble gas in period 3 having an electron affinity of zero.
Que-5: The number of electrons in the valence shell of a halogen is :
(a) 1
(b) 3
(c) 5
(d) 7
Ans: (d) 7
Hint- Halogens have 7 valence electrons.
Que-6: Among period 2 elements, the element which has highest electron affinity is :
(a) Lithium
(b) Carbon
(c) Chlorine
(d) Fluorine
Ans: (d) Fluorine
Hint- Electron affinity increases from left to right in a period. Out of the given options, Lithium, Carbon and Fluorine are period 2 elements in that order. Hence, Fluorine has the highest electron affinity among period 2 elements.
Que-7: Ionisation potential increases over a period from left to right because :
(a) Atomic radius and nuclear charge increase
(b) Atomic radius and nuclear charge decrease
(c) Atomic radius increases and nuclear charge decreases
(d) Atomic radius decreases and nuclear charge increases
Ans: (d) Atomic radius decreases and nuclear charge increases
Hint- On moving from left to right across a period, the atomic radius decreases due to increase in the nuclear charge, and thus, more energy is required to remove the electrons. Hence, ionization potential increases from left to right across a period.
Que-8: An element A belonging to period 3 and group II will have :
(a) 3 shells and 2 valence electrons
(b) 2 shells and 3 valence electrons
(c) 3 shells and 3 valence electrons
(d) 2 shells and 2 valence electrons
Ans: (c) 3 shells and 2 valence electrons
Hint- The number of shells present in an atom determines its period and valence electrons determine its group.
Que-9: Among the elements given below, the element with the least electronegativity is :
(a) Lithium
(b) Carbon
(c) Boron
(d) Fluorine
Ans: (a) Lithium
Hint- Lithium, Boron, Carbon, Fluorine is the order of given elements from left to right in period 2. As electronegativity increases from left to right in a period, hence, Lithium has the least electronegativity in the given elements.
Que-10: An element with atomic number 19 will most likely combine chemically with the elements whose atomic number is :
(a) 17
(b) 11
(c) 28
(d) 20
Ans: (a) 17
Hint- Element with atomic number 19 has an electronic configuration of 2, 8, 8, 1. It is a metal with one valence electron. Element with atomic number 17 has an electronic configuration of 2, 8, 7. It is a non-metal. Hence, element with atomic number 19 will donate its one valence electron to element with atomic number 17. Both will achieve stable octet. Hence, these two elements are most likely to combine chemically.
Que-11: Parts (i) to (iv) refer to changes in the properties of elements on moving from left to right across a period of the Periodic Table. For each property, choose the correct answer.
(i) The non-metallic character of the elements :
(a) decreases,
(b) increases,
(c) remains the same,
(d) depends on the period
(ii) The electronegativity :
(a) depends on the number of valence electrons,
(b) remains the same,
(c) decreases,
(d) increases
(iii) The ionization potential :
(a) goes up and down
(b) decreases
(c) increases
(d) remains the same
(iv) The atomic size :
(a) decreases,
(b) increases,
(c) remains the same,
(d) sometimes increases and sometimes decreases
Ans:
(i) increases.
Hint- On moving across a period from left to right, nuclear pull increases due to increase in atomic number and thus atomic size decreases. Hence, elements cannot lose electrons easily. Therefore, non-metallic character increases.
(ii) increases.
Hint- On moving across a period from left to right, nuclear charge increases due to an increase in atomic number. Hence, electronegativity increases from left to right in a period.
(iii) increases.
Hint- On moving from left to right across a period, the atomic radius decreases due to increase in the nuclear charge, and thus, more energy is required to remove the electrons. Hence, ionization potential increases from left to right across a period.
(iv) decreases.
Hint- On moving across a period from left to right, nuclear pull increases due to increase in atomic number and thus atomic size decreases.
Que-12: In the periodic table while going down in the halogen group :
(a) reactivity will increase
(b) electronegativity will increase
(c) ionic radius will increase
(d) ionisation potential will increase
Ans: (c) ionic radius will increase
Hint- On going down in the halogen group, number of shells increases, hence, ionic radius also increases. Reactivity, electronegativity and ionisation potential decreases while going down in the halogen group.
Que-13: Electron affinity is the :
(a) Power of an atom to attract an electron to itself.
(b) Energy released when an electron is added to an isolated atom in the gaseous state.
(c) Energy absorbed when an electron is added to an isolated atom in the gaseous state.
(d) Energy required to remove an electron from an isolated gaseous atom.
Ans: (b) Energy released when an electron is added to an isolated atom in the gaseous state.
Hint- The amount of energy released while converting a neutral gaseous isolated atom into a negatively charged gaseous ion (anion) by the addition of electron is called Electron Affinity (E.A.).
Que-14: Which of these statements gives the correct picture regarding halogens and alkali metals with respect to an increase in the atomic number ?
(a) Reactivity decreases in alkali metals but increases in halogens.
(b) Reactivity increases in both.
(c) Reactivity decreases in both.
(d) Reactivity increases in alkali metals but decreases in halogens.
Ans: (d) Reactivity increases in alkali metals but decreases in halogens.
Hint- Atomic number increases while going down the group in alkali metals and halogens. The tendency of losing electrons increases down the group. Reactivity of metals depends on tendency to lose electrons, thus reactivity of alkali metals increases while going down the group. Reactivity of non-metals depends on tendency to gain electrons, thus reactivity of halogens decreases while going down the group.
Que-15: The correct order of increasing ionisation energy of Be, Mg, Ca, Sr is :
(a) Be, Mg, Ca, Sr
(b) Ca, Mg, Be, Sr
(c) Sr, Ca, Mg, Be
(d) Mg, Ca, Sr, Be
Ans: (c) Sr, Ca, Mg, Be
Hint- Ionisation energy decreases on moving down the group.
Que-16: An element 13X combines with 17Y to form a compound. which of the following is true ?
P → X is a metal, Y is a metal.
Q → X is a metal, Y is a non-metal.
R → X losses electron(s), y gains electron(s).
(a) Only P
(b) Only Q
(c) Both P and Q
(d) Both Q and R
Ans: (d) Both Q and R
Hint- Element X with an atomic number of 13 is Aluminium (Al), which is a metal. Element Y with an atomic number of 17 is Chlorine (Cl), which is a non-metal.
X being a metal tends to lose electrons to achieve a stable electron configuration and Y being a non-metal tends to gain electrons to achieve stable electron configuration. Hence, statements Q and R are true whereas statement P is false.
Que-17:
Assertion (A): Second period consists of 8 elements.
Reason (R): Number of elements in each period is four times the number of atomic orbitals available in energy level that is being filled.
(a) Both A and R are true and R is the correct explanation of A.
(b) Both A and R are true but R is not the correct explanation of A.
(c) A is true but R is false.
(d) A is false but R is true.
Ans: (c) A is true but R is false.
Hint- The second period includes the elements from lithium (Z=3) to neon (Z=10): Li, Be, B, C, N, O, F, Ne → 8 elements. Hence assertion is true. Reason given is incorrect. In the first period, electrons are being added to the K electronic configuration.
The number of available electronic configuration or orbital for elements of first period is 1.
The number of elements present in the first period is 2, which is not four times the number of atomic orbitals available. Hence the (R) statement is false.
Que-18:
Assertion (A): In a Dobereiner’s triad, the three elements present have the same difference of atomic masses.
Reason (R): Elements in a triad have similar properties.
(a) Both A and R are true and R is the correct explanation of A.
(b) Both A and R are true but R is not the correct explanation of A.
(c) A is true but R is false.
(d) A is false but R is true.
Ans: (d) A is false but R is true.
Hint- In Dobereiner’s triads, the atomic mass of the middle element is approximately the average of the atomic masses of the other two. Hence, Assertion (A) is false.
Dobereiner grouped elements into triads because they had similar chemical properties. Hence, Reason (R) is true.
Que-19:
Assertion (A): Smaller the size of an atom greater is its electronegativity.
Reason (R): Electronegativity is the tendency of an atom to attract shared pair of electrons towards itself in a molecule.
(a) Both A and R are true and R is the correct explanation of A.
(b) Both A and R are true but R is not the correct explanation of A.
(c) A is true but R is false.
(d) A is false but R is true.
Ans: (b) Both A and R are true but R is not the correct explanation of A.
Hint- Assertion (A) is true because smaller atoms attract electrons more strongly. Reason (R) correctly defines electronegativity but does not explain why smaller atoms have higher electronegativity.
Que-20:
Assertion (A): Hydrogen is placed in group I.
Reason (R): Hydrogen can gain an electron to achieve noble gas configuration.
(a) Both A and R are true and R is the correct explanation of A.
(b) Both A and R are true but R is not the correct explanation of A.
(c) A is true but R is false.
(d) A is false but R is true.
Ans: (b) Both A and R are true but R is not the correct explanation of A.
Hint- Hydrogen is placed in Group I with alkali metals because, like them, it has one electron in its outermost shell and forms (H⁺) ions by losing this electron. Although hydrogen can also gain an electron to form the hydride ion (H⁻) similar to halogens. Hence, Both Assertion (A) and Reason (R) are true but Reason (R) is not the correct explanation of Assertion (A).
Que-21:
Assertion (A): Atomic size increases along a period.
Reason (R): Effective nuclear charge increases with atomic number.
(a) Both A and R are true and R is the correct explanation of A.
(b) Both A and R are true but R is not the correct explanation of A.
(c) A is true but R is false.
(d) A is false but R is true.
Ans: (d) A is false but R is true.
Hint- Atomic size decreases across a period (from left to right) in the periodic table. This is because, although electrons are being added, they are added to the same shell, and the increasing effective nuclear charge pulls the electrons closer to the nucleus. Hence, Assertion (A) is false.
As atomic number increases, the number of protons increases, which increases the effective nuclear charge. Hence, Reason (R) is true.
Que-22:
Assertion (A): Elements in the same vertical column have similar properties.
Reason (R): Properties depend upon the number of electrons in the valence shell.
(a) Both A and R are true and R is the correct explanation of A.
(b) Both A and R are true but R is not the correct explanation of A.
(c) A is true but R is false.
(d) A is false but R is true.
Ans: (a) Both A and R are true and R is the correct explanation of A.
Hint- Elements in the same vertical column i.e., a group in the periodic table, have the same number of valence electrons. Since chemical properties of elements depend upon the number of valence electrons, thus elements in the same group have similar properties. Hence, Reason (R) correctly explains the Assertion (A).
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