Periodic Table & Periodicity PYQs Set 9 (PDF)

Set 9 of 11 · Questions 241-270 of 322

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Mere Teacher · Previous Year Questions NEET Chemistry · Periodic Table & Periodicity · Set 9 (Q241-270)
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241. $Outermost electronic configurations of four elements A, B, C, D are given below: (A) 3 s^{2} (B) 3 s^{2} S p^{1} (C) 3 s^{2} 3 p^{3} (D) 3 s^{2} 3 p^{4} The correct order of first ionization enthalpy for them is:$ (1) $(A) < (B) < (C) < (D)$ (2) $(B) < (A) < (D) < (C)$ (3) $(B) < (D) < (A) < (C)$ (4) $(B) < (A) < (C) < (D)$ 242. $Amongst the elements with following electronic configurations, which one of them may have the highest ionisation energy?$ (1) $Ne [3 s^{2} 3 p^{2}]$ (2) $Ar [3 d^{10} 4 s^{2} 4 p^{3}]$ (3) $Ne [3 s^{2} 3 p^{1}]$ (4) $Ne [3 s^{2} 3 p^{3}]$ 243. $The electronic configuration of four elements are given below. Which elements does not belong to the same family as others?$ (1) $[X e] 4 f^{14} 5 d^{10} 6 s^{2}$ (2) $[K r] 4 d^{10} 5 s^{2}$ (3) $[N e] 3 s^{2} 3 p^{5}$ (4) $[Ar]3 d^{10} 4 s^{2}$ 244. $Which of the following compound CANNOT act as a Lewis base?$ (1) $NF_{3}$ (2) $PC l_{5}$ (3) $SF_{4}$ (4) $ClF_{3}$ 245. $Given below are the two statements: one is labeled as Assertion (A) and the other is labeled as Reason (R). Assertion (A): There is a considerable increase in covalent radius from N to P. However from As to Bi only a small increase in covalent radius is observed. Reason (R) : covalent and ionic radii in a particular oxidation state increases down the group.In the light of the above statement, choose the most appropriate answer from the options given below:$ (1) $(A) is false but (R) is true$ (2) $Both (A) and (R) are true but (R) is not the correct explanation of (A)$ (3) $(A) is true but (R) is false$ (4) $Both (A) and (R) are true and (R) is the correct explanation of (A)$ 246. $Which of the following statements are NOT true about the periodic table? A. The properties of elements are function of atomic weights. B. The properties of elements are function of atomic numbers. C. Elements having similar outer electronic configurations are arranged in same period. D. An element's location reflects the quantum numbers of the last filled orbital. E. The number of elements in a period is same as the number of atomic orbitals available in energy level that is being filled. Choose the correct answer from the options given below:$ (1) $A, C and E Only$ (2) $A and E Only$ (3) $B, C and E Only$ (4) $D and E Only$ 247. $Consider the following (I) The order of first ionisation enthalpy of first three elements of 3^{rd} period is Mg > Al > Na (II) The element with electronegativity of 3.5 is chlorine (III) The order of sizes of ions Mg^{2 +}, Na^{+}, F^{-} and O^{2 -} is Mg^{2 +} < Na^{+} < F^{-} < O^{2 -} (IV)The IUPAC name of the element with atomic number 106 is Bohrium. The correct statements are$ (1) $I & II only$ (2) $II & III only$ (3) $I & III only$ (4) $II & IV only$ 248. $Match List I with List II List - I A. Melting Point [K] B. Ionic Radius (M^{+ 3} / pm) C. Δ_{i} H_{1} (kJ mol^{- 1}) D. Atomic Radius [pm] List - II I . T 1 > In > Ga > A 1 > B II . B > T 1 > A 1 \approx Ga > In III . T 1 > In > A 1 > Ga > B IV . B > A 1 > T 1 > In > Ga Choose the correct answer from the options given below:$ (1) $A-II, B-III, C-IV, D-I$ (2) $A-IV, B-I, C-II, D-III$ (3) $A-I, B-II, C-III, D-IV$ (4) $A-III, B-IV, C-I, D-II$ 249. $B has a smaller first ionization enthalpy than Be . Consider the following statements: (I) It is easier to remove 2p electron than 2s electron. (II) 2p electron of B is more shielded from the nucleus by the inner core of electrons than the 2 s electrons of Be . (III) 2 s electron has more penetration power than 2 p electron. (IV) Atomic radius of B is more than Be . (atomic number B = 5, Be = 4) The correct statement are :$ (1) $(I), (II), (IV)$ (2) $(I), (III), (IV)$ (3) $(II), (III), (IV)$ (4) $(I), (II), (III)$ 250. $An element with atomic number 21 is a$ (1) $transition element$ (2) $alkali metal$ (3) $halogen$ (4) $representative element.$ 251. $Identify the correct statements about p-block elements and their compounds. (A) Non metals have higher electronegativity than metals.(B) Non metals have lower ionisation enthalpy than metals.(C) Compounds formed between highly reactive nonmetals and highly reactive metals are generally ionic.(D) The non-metal oxides are generally basic in nature.(E) The metal oxides are generally acidic or neutral in nature. Choose the correct answer from the options given below :$ (1) $(B) and (D) only$ (2) $(A) and (C) only$ (3) $(D) and (E) only$ (4) $(B) and (E) only$ 252. $Choose the INCORRECT statement$ (1) $CO_{2} is the most acidic oxide among the dioxides of group of 14 elements.$ (2) $Carbon exhibits negative oxidation states along with +4 and +2 .$ (3) $Carbon cannot exceed its covalency more than four.$ (4) $Among the isotopes of carbon,^{13} C is a radioactive isotope.$ 253. $Chalcogen group elements are :$ (1) $Se, Tb and Pu.$ (2) $Se, Te and Po.$ (3) $S,Te and Pm.$ (4) $O,Ti and Po.$ 254. $Identify the set of acidic oxides.$ (1) $Na_{2} O, CaO, BaO$ (2) $ZnO, PbO, BeO$ (3) $CO, NO, N_{2} O$ (4) $Mn_{2} O_{7}, CrO_{3}, V_{2} O_{5}$ 255. $Match List I with List II List - I (Elements) A. Cl, S B. Ge, As C. Fr, Ra D. F, O List - II (Properties in their respective groups) I . Elements with highest electronegativity II . Elements with largest atomic size III. Elements which show properties of both metals and non-metal IV. Elements with highest negative electron gain enthalpy Choose the correct answer from the options given below:$ (1) $A-II, B-I, C-IV, D-III$ (2) $A-III, B-II, C-I, D-IV$ (3) $A-IV, B-III, C-II, D-I$ (4) $A-II, B-III, C-IV, D-I$ 256. $The correct order of radii is:$ (1) $N < Be < B$ (2) $F^{-} < O^{2-} < N^{3-}$ (3) $Na < Li < K$ (4) $F e^{3 +} < F e^{2 +} < F e^{+ 4}$ 257. $The successive ionisation energy values for an element ' X' are given below: (i) 1 st ionisation energy = 410 kJ mol^{- 1} (ii) 2 nd ionisation energy = 820 kJ mol^{- 1} (iii) 3rd ionisation energy = 1100 kJ mol^{- 1} (iv) 4th ionisation energy = 1500 kJ mol^{- 1} (v) 5 th ionisation energy = 3200 kJ mol^{- 1} The number of valence electron in ' X' will be$ (1) $5$ (2) $4$ (3) $2$ (4) $3$ 258. $In comparison to boron, beryliumhas :$ (1) $lesser nuclear charge and lesser first ionization enthalpy.$ (2) $greater nuclear charge and lesser first ionization enthalpy.$ (3) $greater nuclear charge and greater first ionization enthalpy.$ (4) $lesser nuclear charge and greater first ionization enthalpy.$ 259. $When the first electron gain enthalpy (Δ_{e g} H) of oxygen is -141 kJ/mol, its second electron gain enthalpy is :$ (1) $almost the same as that of the first$ (2) $negative, but less negative than the first$ (3) $a more negative value than the first$ (4) $a positive value$ 260. $The characteristics of elements X, Y and Z with atomic numbers, respectively, 33,53 and 83 are:$ (1) $X and Y are metalloids and Z is a metal.$ (2) $X is a metalloid, Y is a non-metal and Z is a metal.$ (3) $X, Y and Z are metals.$ (4) $X and Z are non-metals and Y is a metalloid$ 261. $The effect of lanthanoid contraction in the lanthanoid series of elements by an and large means$ (1) $increase in atomic radii and decrease in ionic radii$ (2) $decrease in both atomic and ionic radii$ (3) $increase in both atomic and ionic radii$ (4) $decrease in atomic radii and increase in ionic radii$ 262. $The elements of Group 13 with highest and lowest first ionization enthalpies are respectively:$ (1) $B & Tl$ (2) $Tl & B$ (3) $B & In$ (4) $B & Ga$ 263. $Which statement is wrong?$ (1) $Bond energy of F_{2} > C l_{2}$ (2) $Electronegativity of F > Cl$ (3) $F is more oxidising than Cl$ (4) $Electron affinity of Cl > F$ 264. $The set that contains atomic numbers of only transition elements, is$ (1) $21, 32, 53, 64$ (2) $9, 17, 34, 38$ (3) $37, 42, 50, 64$ (4) $21, 25, 42, 72$ 265. $Identify the element which has highest second ionization enthalpy$ (1) $Carbon$ (2) $Phosphorus$ (3) $Nitrogen$ (4) $Oxygen$ 266. $The total number of rare-earth elements is:$ (1) $8$ (2) $10$ (3) $14$ (4) $32$ 267. $The correct decreasing order for metallic character is$ (1) $Na > Mg > Be > Si > P$ (2) $P>Si>Be>Mg>Na$ (3) $Si>P>Be>Na>Mg$ (4) $Be > Na > Mg > Si > P$ 268. $What is the value of electron gain enthalpy of Na+ if IE1 of Na = 5.1 eV ?$ (1) $-5.1 eV$ (2) $-10.2 eV$ (3) $+2.55 eV$ (4) $+10.2 eV$ 269. $In the periodic table, with the increase in atomic number, the metallic character of an element$ (1) $decreases in a period and increases in a group$ (2) $increases in a period and decreases in a group$ (3) $increases both in a period and the group$ (4) $decreases in a period and the group.$ 270. $The element having the highest first ionization enthalpy is$ (1) $Si$ (2) $Al$ (3) $N$ (4) $C$