Periodic Table & Periodicity PYQs Set 6 (PDF)

Set 6 of 11 · Questions 151-180 of 327

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Mere Teacher · Previous Year Questions JEE Main Chemistry · Periodic Table & Periodicity · Set 6 (Q151-180)
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151. $The correct arrangement for the ions in the increasing order of their radii is$ (1) $Na^{+}, Cl^{-}, Ca^{2 +}$ (2) $Ca^{2 +}, K^{+}, S^{2 -}$ (3) $Na^{+}, Al^{3 +}, Be^{2 +}$ (4) $Cl^{-}, F^{-}, S^{2 -}$ 152. $Given below are two statements: Statement (I): According to the Law of Octaves, the elements were arranged in the increasing order of their atomic number. Statement (II): Meyer observed a periodically repeated pattern upon plotting physical properties of certain elements against their respective atomic numbers. choose the correct answer from the options given below:$ (1) $Both Statement (I) and Statement (II) are false.$ (2) $Both Statement (I) and Statement (II) are true.$ (3) $Statement (I) is false but Statement (II) is true.$ (4) $Statement (I) is true but Statement (II) is false.$ 153. $For elements B, C, N Li, Be, O and F, the correct order of first ionisation enthalpy is$ (1) $Li < Be < B < C < O < N < F$ (2) $B < Li < Be < C < N < O < F$ (3) $Li < Be < B < C < N < O < F$ (4) $Li < B < Be < C < O < N < F$ 154. $Which of the following ions has electronic configuration [Ar]3d6 ?$ (1) $Ni3+$ (2) $Mn3+$ (3) $Fe3+$ (4) $Co3+$ 155. $Which one of the following has largest ionic radius?$ (1) $L i^{+}$ (2) $O^{2-}$ (3) $B^{3 +}$ (4) $F^{-}$ 156. $Which of the following statements is incorrect?$ (1) $The enthalpy of atomisation decreases down a group in s-block elements$ (2) $The enthalpy of atomisation decreases down a group in p-block elements$ (3) $The enthalpy of atomisation decreases down a group in d-block elements$ (4) $The enthalpy of atomisation increases down a group in d-block elements$ 157. $The correct order of the metallic character of the elements Be, Al, Na, K is$ (1) $K > Na > Al > Be$ (2) $K > Al > Na > Be$ (3) $Al > K > Na > Be$ (4) $Na > K > Be > Al$ 158. $Which one of the following orders is not in accordance with the property stated against it?$ (1) $F_{2} > C l_{2} > B r_{2} > I_{2} : Bond dissociation energy$ (2) $F_{2} > C l_{2} > B r_{2} > I_{2} : Oxidising power$ (3) $H I > H B r > H C l > H F : Acidic property in water$ (4) $F_{2} > C l_{2} > B r_{2} > I_{2} : Electronegativity$ 159. $Given below are two statements : Statement I : The correct order in terms of atomic/ionic radii is Al > Mg > Mg^{2 +} > Al^{3 +} . Statement II : The correct order in terms of the magnitude of electron gain enthalpy is Cl > Br > S > O . In the light of the above statements, choose the correct answer from the options given below:$ (1) $Both Statement I and Statement II are false$ (2) $Both Statement I and Statement II are true$ (3) $Statement I is false but Statement II is true$ (4) $Statement I is true but Statement II is false$ 160. $Which of the following has the smallest size?$ (1) $A l^{3 +}$ (2) $F^{-}$ (3) $N a^{+}$ (4) $M g^{2 +}$ 161. $The group 14 elements A and B have the first ionisation enthalpy values of 708 and 715 kJ mol^{- 1} respectively. The above values are lowest among their group members. The nature of their ions A^{2 +} and B^{4 +} respectively is$ (1) $both reducing$ (2) $oxidizing and reducing$ (3) $both oxidizing$ (4) $reducing and oxidizing$ 162. $The third ionisation enthalpy is highest in$ (1) $alkali metals$ (2) $alkaline earth metals$ (3) $chalcogens$ (4) $pnictogens.$ 163. $The number of valence electrons present in an element with atomic number 117 is$ (1) $7$ (2) $8$ (3) $6$ (4) $5$ 164. $The number of valence electrons present in the metal among Cr, Co, Fe and Ni which has the lowest enthalpy of atomization is:$ (1) $10$ (2) $6$ (3) $9$ (4) $8$ 165. $Which one of the following arrangements represents the correct order of least negative to most negative electron gain enthalpy for C, Ca, Al, F and O ?$ (1) $Al < C a < O < C < F$ (2) $Al < O < C < C a < F$ (3) $C < F < O < A l < C a$ (4) $Ca < A l < C < O < F$ 166. $The set of elements that differ in mutual relationship from those of the other sets is:$ (1) $L_{i} - Mg$ (2) $B - Si$ (3) $Be - Al$ (4) $Li - Na$ 167. $The stability of dihalides of Si, Ge, Sn and Pb increases steadily in the sequence.$ (1) $S i X_{2} << G e X_{2} << S n X_{2} << P b X_{2}$ (2) $P b X_{2} << S n X_{2} << G e X_{2} << S i X_{2}$ (3) $G e X_{2} << S i X_{2} << S n X_{2} << P b X_{2}$ (4) $S i X_{2} << G e X_{2} << P b X_{2} << S n X_{2}$ 168. $Which one of the following elements will remain as liquid inside pure boiling water?$ (1) $Ga$ (2) $Br$ (3) $Li$ (4) $Cs$ 169. $The correct increasing order of the ionic radii is$ (1) $C l^{-} < C a^{2 -} < K^{+} < S^{2 -}$ (2) $K^{+} < S^{2 -} < C a^{2 +} < C l^{-}$ (3) $S^{2 -} < C l^{-} < C a^{2 +} < K^{+}$ (4) $C a^{2 +} < K^{+} < C l^{-} < S^{2 -}$ 170. $The correct option for the first ionisation enthalpy (in kJ mol^{- 1}) of Li, Na, K and Cs respectively is$ (1) $496, 520, 419, 374$ (2) $374, 419, 496, 520$ (3) $520, 496, 419, 374$ (4) $374, 419, 520, 496$ 171. $Lithium shows diagonal relationship with element ' X' and aluminum with Y . X and Y respectively are$ (1) $Mg, Be$ (2) $Be, Mg$ (3) $Na, Si$ (4) $B, Be$ 172. $Generally, the first ionization energy increases along a period. But there are some exceptions. One which is NOT an exception is$ (1) $N and O$ (2) $Na and Mg$ (3) $Mg and Al$ (4) $Be and B$ 173. $In general, the properties that decrease and increase down a group in the periodic table, respectively, are:$ (1) $atomic radius and electronegativity.$ (2) $electron gain enthalpy and electronegativity.$ (3) $electronegativity and atomic radius.$ (4) $electronegativity and electron gain enthalpy.$ 174. $The correct sequence which shows decreasing order of the ionic radii of the elements is:$ (1) $A l^{3 +} > M g^{2 +} > N a^{+} > F^{-} > O^{2-}$ (2) $N a^{+} > M g^{2 +} > A l^{3 +} > O^{2-} > F^{-}$ (3) $N a^{+} > F^{-} > M g^{2 +} > O^{2-} > A l^{3 +}$ (4) $O^{2-} > F^{-} > N a^{+} > M g^{2 +} > A l^{3 +}$ 175. $Identify the correct order of ionic radii of the following ions.$ (1) $Al^{3 +} > K^{+} > Mg^{2 +} > Li^{+}$ (2) $K^{+} > Mg^{2 +} > Al^{3 +} > Li^{+}$ (3) $K^{+} > Li^{+} > Mg^{2 +} > Al^{3 +}$ (4) $K^{+} > Mg^{2 +} > Li^{+} > Al^{3 +}$ 176. $Which among the following isoelectronic species has the smallest size? O^{2 -}, F^{-}, Ne, N a^{+}, M g^{2 +}, A l^{3 +}, S i^{4 +}$ (1) $F^{-}$ (2) $Ne$ (3) $Si^{4 +}$ (4) $Na^{+}$ 177. $The 71^{s} electron of an element X with an atomic numberof 71 enters into the orbital:$ (1) $6 p$ (2) $4 f$ (3) $5 d$ (4) $6 s$ 178. $Given two statements below : Statement I : In C 1_{2} molecule the covalent radius is double of the atomic radius of chlorine. Statement II: Radius of anionic species is always greater than their parent atomic radius. Choose the most appropriate answer from options given below:$ (1) $Both Statement I and Statement II are correct.$ (2) $Both Statement I and Statement II are incorrect.$ (3) $Statement I is correct but Statement II is incorrect$ (4) $Statement I is incorrect but Statement II is correct.$ 179. $Amongst the elements with following electronic configurations, which one may have the highest ionisation energy ?$ (1) $[Ne] 3s2 3p3$ (2) $[Ne] 3s2 3p2$ (3) $[Ar] 3d10, 4s2 4p3$ (4) $[Ne] 3s2 3p1$ 180. $Aluminium is usually found in + 3 oxidation state. In contrast, thallium exists in + 1 and + 3 oxidation states. This is due to:$ (1) $inert pair effect$ (2) $diagonal relationship$ (3) $lattice effect$ (4) $lanthanoid contraction$