{"id":17577,"date":"2022-05-24T10:30:37","date_gmt":"2022-05-24T05:00:37","guid":{"rendered":"https:\/\/mcq-questions.com\/?p=17577"},"modified":"2022-05-16T15:25:07","modified_gmt":"2022-05-16T09:55:07","slug":"mcq-questions-for-class-11-chemistry-chapter-3","status":"publish","type":"post","link":"https:\/\/mcq-questions.com\/mcq-questions-for-class-11-chemistry-chapter-3\/","title":{"rendered":"MCQ Questions for Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties with Answers"},"content":{"rendered":"

Students are advised to practice the\u00a0NCERT MCQ Questions for Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties with Answers Pdf free download is available here. MCQ Questions for Class 11 Chemistry with Answers<\/a> are prepared as per the Latest Exam Pattern. Students can solve these Classification of Elements and Periodicity in Properties Class 11 MCQs Questions with Answers and assess their preparation level.<\/p>\n

Classification of Elements and Periodicity in Properties Class 11 MCQs Questions with Answers<\/h2>\n

Solving the Classification of Elements and Periodicity in Properties Multiple Choice Questions of Class 11 Chemistry Chapter 3 MCQ can be of extreme help as you will be aware of all the concepts. These MCQ Questions on Classification of Elements and Periodicity in Properties Class 11 with answers pave for a quick revision of the Chapter thereby helping you to enhance subject knowledge. Have a glance at the MCQ of Chapter 3 Chemistry Class 11 and cross-check your answers during preparation.<\/p>\n

Question 1.
\nThe group number, number of valence electrons, and valency of an element with the atomic number 15, respectively, are:
\n(a) 16, 5 and 2
\n(b) 15, 5 and 3
\n(c) 16, 6 and 3
\n(d) 15, 6 and 2<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) 15, 5 and 3
\nExplanation:
\nAtomic number (Z) = 15 = P \u2192 [Ne] 3s\u00b2 3p\u00b3
\nPhosphorus belongs to 15th group
\nNumber of valence electrons 3s\u00b2 3p\u00b3 = 5 and valency = 3 in ground state.<\/p>\n<\/details>\n

\n

Question 2.
\nThe d-block elements consists mostly of
\n(a) Monovalent metals
\n(b) All non-metals
\n(c) Elements which generally form stoichiometric metal oxide
\n(d) Many metals with catalytic properties<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) Many metals with catalytic properties
\nExplanation:
\nMany metals with catalytic properties because (i) They provide surface area for reaction to occur (ii) They decreases the ionisation energy. (iii) They have vacant d-orbitals.<\/p>\n<\/details>\n

\n

Question 3.
\nWhich of the following has the highest boiling point?
\n(a) Ne
\n(b) Xe
\n(c) Ar
\n(d) Kr.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Xe
\nExplanation:
\nXe has the highest atomic size and molecular weight. Hence, it has strong Vander Waals forces of attraction. Hence, it has the highest boiling point.<\/p>\n<\/details>\n

\n

Question 4.
\nThe chemistry of lithium is very similar to that of magnesium even though they are placed in different groups. Its reason is:
\n(a) Both are found together in nature
\n(b) Both have nearly the same size
\n(c) Both have similar electronic configuration
\n(d) The ratio of their charge and size (i.e. charge density) is nearly the same<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) The ratio of their charge and size (i.e. charge density) is nearly the same
\nExplanation:
\nThe chemistry of lithium is very similar to that of magnesium even though they are placed in different groups because of diagonal relationship.<\/p>\n<\/details>\n

\n

Question 5.
\nWhich one of the following groupings represents a collection of isoelectronic species? (At. nos: Cs-55, Br-35)
\n(a) Na+<\/sup>, Ca2+<\/sup>, Mg2+<\/sup>
\n(b) N3-<\/sup>, F–<\/sup>, Na+<\/sup>
\n(c) Be, Al3+<\/sup>, Cl–<\/sup>
\n(d) Ca2+<\/sup>, Cs+<\/sup>, Br<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) N3-<\/sup>, F–<\/sup>, Na+<\/sup>
\nExplanation:
\nIsoelectronic species are the neutral atoms, cations or anions of different elements which have the same number of electrons but different nuclear charge.
\nNumber of electrons in N3-<\/sup> = 7 + 3 = 10.
\nNumber of electrons in F–<\/sup> = 9 + 1 = 10
\nNumber of electrons in Na+<\/sup> = 11 \u2013 1 = 10.<\/p>\n<\/details>\n

\n

Question 6.
\nWhich of the following has the maximum number of unpaired electrons?
\n(a) Mg2+<\/sup>
\n(b) Ti3+<\/sup>
\n(c) V3+<\/sup>
\n(d) Fe2+<\/sup><\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) Fe2+<\/sup>
\nExplanation:
\nMg2+<\/sup>: 1s\u00b2 2s\u00b2 2p6<\/sup>: no unpaired electron
\nTi3+<\/sup>: 1s\u00b2 2s\u00b2 2p6<\/sup> 3s\u00b2 3p6<\/sup> 3d1<\/sup>: one unpaired electron
\nV3+<\/sup>: 1s\u00b2 2s\u00b2 2p6<\/sup> 3s\u00b2 3p6<\/sup> 3d1<\/sup>: two unpaired electrons
\nFe2+<\/sup>: 1s\u00b2 2s\u00b2 2p6<\/sup> 3s\u00b2 3p6<\/sup> 3d6<\/sup>: four unpaired electrons<\/p>\n<\/details>\n

\n

Question 7.
\nIn the periodic table, the element with atomic number 16 will be placed in the group
\n(a) Third
\n(b) Fourth
\n(c) Fifth
\n(d) Sixth<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) Sixth
\nExplanation:
\n16-1s\u00b22s\u00b22p6<\/sup>3s\u00b23p4<\/sup> there are 6e–<\/sup> in outer most shell therefore its group is VIth A<\/p>\n<\/details>\n

\n

Question 8.
\nRepresentative elements are those which belong to
\n(a) p and d – Block
\n(b) s and d – Block
\n(c) s and p – Block
\n(d) s and f – Block<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) s and p – Block
\nExplanation:
\nElements in which all the inner shells are complete but outer shell is incomplete is known as representative elements i.e. Those elements which have less than 8 electrons in outermost shell are representative.
\ns and p block elements except inert gas is known as representative elements.<\/p>\n<\/details>\n

\n

Question 9.
\nWhich pair of elements belongs to same group?
\n(a) Elements with atomic no. 17 and 38
\n(b) Elements with atomic no. 20 and 40
\n(c) Elements with atomic no. 17 and 53
\n(d) Elements with atomic no. 11 and 33<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Elements with atomic no. 17 and 53
\nExplanation:
\nAtomic no. 17(Cl) and 53 (I) are present in the same group<\/p>\n<\/details>\n

\n

Question 10.
\nThe most electronegative element of the periodic table is
\n(a) Iodine
\n(b) Sulphur
\n(c) Oxygen
\n(d) Fluorine.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) Fluorine.
\nExplanation:
\nFluorine is the most electronegative element. Fluorine has an electronegativity of 3.98 on the Pauling Electronegativity Scale and a valence of 1. A fluorine atom needs one electron to fill its outer electron shell and achieve stability, which is why free fluorine exists as the F–<\/sup> ion.<\/p>\n<\/details>\n

\n

Question 11.
\nIn the third period of the Periodic Table the element having smallest size is
\n(a) Na
\n(b) Ar
\n(c) Cl
\n(d) Si<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Ar
\nExplanation:
\nIn the third period of the Periodic Table the element having smallest size is Ar.<\/p>\n<\/details>\n

\n

Question 12.
\nThe element with highest second ionization energy is
\n(a) Cl
\n(b) S
\n(c) Na
\n(d) Mg<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) Na
\nExplanation:
\nSodium has 11 electrons which can be written as (2, 8, and 1). Its outer orbit has 1 electron When it is ionized for the first time, the outer most electron is removed very easily, so that it can form the electronic configuration of the nearest inert gas Neon (2, 8).
\nNeon has 8 electrons in its outermost orbit. Thus it is highly stable. Now, when the second electron is removed, a very very high amount of energy is required because it doesnt want to give away one of its outermost electron by disrupting its stability.
\nThus, second ionization energy of sodium is extremely high.<\/p>\n<\/details>\n

\n

Question 13.
\nWhich of the following properties generally decreases along a period?
\n(a) Ionization Energy
\n(b) Metallic Character
\n(c) Electron Affinity
\n(d) Valency.<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) Metallic Character
\nExplanation:
\nThe IE, EA increases along the period. The valency initially increases then decreases. The metallic character decreases along the period.<\/p>\n<\/details>\n

\n

Question 14.
\nIncreasing order of electronegativity is
\n(a) Bi < P < S < Cl
\n(b) P < Bi < S < Cl
\n(c) S < Bi < P < Cl
\n(d) Cl < S < Bi < P<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) Bi < P < S < Cl
\nExplanation:
\nIncreasing order of electronegativity is Bi < P < S < Cl.<\/p>\n<\/details>\n

\n

Question 15.
\nWhich of the following oxides is amphoteric in character?
\n(a) SnO2<\/sub>
\n(b) CO2<\/sub>
\n(c) SiO2<\/sub>
\n(d) CaO<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (a) SnO2<\/sub>
\nExplanation:
\nCaO is basic; CO2<\/sub> is acidic; SiO2<\/sub> is weakly acidic. SnO2<\/sub> is amphoteric.<\/p>\n<\/details>\n

\n

Question 16.
\nWhich of the following statement is correct with respect to the property of elements with an increase in atomic number in the carbon family (group 14)
\n(a) Atomic size decrease
\n(b) Ionization energy increase
\n(c) Metallic character decrease
\n(d) Stability of +2 oxidation state increase<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) Stability of +2 oxidation state increase
\nExplanation:
\nAs we go down the group inertness of ns\u00b2 pair increase hence tendency to exhibit +2 oxidation state increases and that of +4 oxidation state decreases.<\/p>\n<\/details>\n

\n

Question 17.
\nThe elements which occupy the peaks of ionisation energy curve, are
\n(a) Na, K, Rb, Cs
\n(b) Na, Mg, Cl, I
\n(c) Cl, Br, I, F
\n(d) He, Ne, Ar, Kr<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) He, Ne, Ar, Kr
\nExplanation:
\nAll the noble gases occupy the peaks of I.E. curve.<\/p>\n<\/details>\n

\n

Question 18.
\nAccording to the periodic law of elements, the variation in properties of elements is related to their
\n(a) nuclear neutron – proton number ratios
\n(b) atomic masses
\n(c) nuclear masses
\n(d) atomic numbers<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (d) atomic numbers
\nExplanation:
\nThe Periodic Law states that the physical and chemical properties of the elements recur in a systematic and predictable way when the elements are arranged in order of increasing atomic number.<\/p>\n<\/details>\n

\n

Question 19.
\nThe group number, number of valence electrons, and valency of an element with the atomic number 15, respectively, are:
\n(a) 16, 5 and 2
\n(b) 15, 5 and 3
\n(c) 16, 6 and 3
\n(d) 15, 6 and 2<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (b) 15, 5 and 3
\nExplanation:
\nAtomic number (Z) =15 =P \u2192 [Ne] 3s\u00b2 3p\u00b3
\nPhosphorus belongs to 15th group
\nNumber of valence electrons 3s\u00b2 3p\u00b3 = 5 and valency = 3 in ground state.<\/p>\n<\/details>\n

\n

Question 20.
\nA sudden large jump between the values of second and third ionisation energies of an element would be associated with the electronic configuration
\n(a) 1s\u00b2, 2s\u00b2p6<\/sup>, 3s1<\/sup>
\n(b) 1s\u00b2, 2s\u00b2p6<\/sup>, 3s\u00b2p1<\/sup>
\n(c) 1s\u00b2, 2s2p6<\/sup>, 3s\u00b2
\n(d) 1s\u00b2, 2s\u00b2p6<\/sup>, 3s2<\/sup>p\u00b2<\/p>\n

\nAnswer<\/span><\/summary>\n

Answer: (c) 1s\u00b2, 2s2p6<\/sup>, 3s\u00b2
\nExplanation:
\n1s\u00b2, 2s2p6<\/sup>, 3s\u00b2 – In III transition e–<\/sup> is to be removed from stable configuration.<\/p>\n<\/details>\n

\n

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Students are advised to practice the\u00a0NCERT MCQ Questions for Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties with Answers Pdf free download is available here. MCQ Questions for Class 11 Chemistry with Answers are prepared as per the Latest Exam Pattern. Students can solve these Classification of Elements and Periodicity in …<\/p>\n

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