Assignment periodic table JH sir 3575 kho tài liệu bách khoa

Periodic Table & Periodicity Contents Topic Page No Theory 01 - 06 Exercise - 07 - 14 Exercise - 15 - 22 Exercise - 22 - 24 Exercise - 25 - 27 Answer Key 28 - 29 Syllabus Periodic Table & Periodicity Modern Periodic law and present form of the periodic table, s, p, d and f block elements, periodic trends in properties of elements atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states and chemical reactivity Name : Contact No ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # PERIODIC TABLE & PERIODICITY DOBEREINER TRIAD RULE [1817] He made groups of three elements having similar chemical properties called TRIAD NEWLAND OCTAVE RULE [1865] He arranged the elements in the increasing order of their atomic mass and observe that properties of every 8th element was similar to the 1st one like in the case of musical vowels notation Sa Re Ga Ma Pa Dha Ne Sa LOTHER MEYER’S CURVE [1869] He plotted a curve between atomic wt and atomic volume of different elements The following observation can be made from the curve (a) Most electropositive elements i.e alkali metals (Li, Na, K, Rb, Cs etc.) occupy the peak positions on the curve (b) Less electropositive i.e alkaline earth metal (Be, Mg, Ca, Sr, Ba) occupy the descending position of the curve (c) Metalloids (B, Se, As, Te, At etc.) and transition metals occupy bottom part of the curve MENDELEEV’S PERIODIC TABLE [1869] Mendeleev’s Periodic’s Law According to him the physical and chemical properties of the elements are the periodic functions of their atomic masses This table was divided into nine vertical columns called groups and seven horizontal rows called periods The groups were numbered as I, II, III, IV, V, VI, VII, VIII and Zero group MODERN PERIODIC TABLE (MODIFIED MENDELEEV PERIODIC TABLE) (i) It was proposed by Moseley (ii) Modern periodic table is based on atomic number (iii) Moseley did an experiment in which he bombarded high speed electron on different metal surfaces and obtained X-rays He found out that (iv)   Z where  = frequency of X-rays Modern Periodic Law - The physical & chemical propeties of elements are a periodic function of the atomic nubmer LONG FORM/PRESENT FORM OF MODERN PERIODIC TABLE It consist of horizontal periods and 18 vertical columns (groups) IA, IIIA, IIIB, IVB, VB, VIB, VIIB, VIII |—————| 10 IB, IIB IIIA, IVA, VA, VIA, VIIA 11 12 ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 13 14 15 16 17 18 PERIODIC TABLE & PERIODICITY ADVANCED # S–Block p–Block Elements Elements IA 18 VIII A H 1.007 Li 6.941 11 Na 22.98 19 K 39.08 37 Rb 85.46 55 Cs 132.90 Be 9.012 12 Mg 24.30 20 Ca 40.078 38 Sr 87.62 56 Ba 137.27 87 Fr 223 88 Ra 226 d –Block Elements II A III B IV B VB 21 22 23 Sc Ti V 44.959 47.88 50.9415 39 40 41 Y Zr Nb 88.905 91.224 92.906 57 72 73 La* Hf Ta 138.905 178.49 180.947 89 Ac** 227 VI B 24 Cr 51.996 42 Mo 95.94 74 W 183.85 104 105 106 Rf Ha Sg 261.11 262.114 263.118 13 III A 14 IV A 15 VA B C N 10.811 12.011 14.006 13 14 15 10 11 12 Al Si P VII B VIII VIII VIII IB II B 26.981 28.085 30.973 25 26 27 28 29 30 31 32 33 Mn Fe Co Ni Cu Zn Ga Ge As 54.938 55.84 55.933 58.693 63.546 65.39 69.723 72.61 74.921 43 44 45 46 47 48 49 50 51 Tc Ru Rh Pd Ag Cd In Sn Sb 98 101.07 102.905 106.42 107.868 112.411 114.82 118.710 121.757 75 76 77 78 79 80 81 82 83 Re Os Ir Pt Au Hg Tl Pb Bi 186.207 190.2 192.22 195.08 196.666 200.59 204.383 207.2 207.980 107 Bh 262.12 108 Hs 265 109 Mt 266 110 Uun 269 16 VI A 17 VII A O 15.999 16 S 32.006 34 Se 78.96 52 Te 127.60 84 Po 209 F 18.998 17 Cl 35.452 35 Br 79.904 53 I 126.904 85 At 210 He 4.002 10 Ne 20.179 18 Ar 39.948 36 Kr 83.80 54 Xe 132.29 86 Rn 222 69 Tm 168.934 101 Md 258 70 Yb 173.04 102 No 259 71 Lu 174.967 103 Lr 260 114 Uuq Inner - Transition Metals (f-Block elements) *Lanthanides **Actinides 58 59 60 Ce Pr Nd 140.115 140.907 144.24 90 91 92 Th Pa U 232.038 231 238.028 61 Pm 145 93 Np 237 62 63 64 Sm Eu Gd 150.36 151.965 157.25 94 95 96 Pu Am Cm 244 243 247 65 Tb 158.925 97 Bk 247 66 Dy 162.50 98 Cf 251 67 Ho 164.930 99 Es 252 68 Er 167.26 100 Fm 257 Classification of the Elements : s-block elements : When shells upto (n – 1) are completely filled and the last electron enters the s-orbital of the outermost (nth) shell, the elements of this class are called s-block elements p-block elements : When shells upto (n – 1) are completely filled and differentiating electron enters the porbital of the nth orbit, elements of this class are called p-block elements d-Block elements : When outermost (nth) and penultimate shells (n – 1)th shells are incompletely filled and differentiating electron enters the (n – 1) d orbitals (i.e., d-orbital of penultimate shell) then elements of this class are called d-block elements (1) Ist transition series i.e 3d series contains 10 elements and starts from 21Sc – 30Zn Filling of electrons takes place in 3d sub-shell (2) IInd transition series i.e 4d series contains 10 elements and starts from 39Y – 48Cd Filling of electrons takes place in 4d sub-shell (3) IIIrd transition series i.e 5d series contains 10 elements and starts from 57La, 72Hf – 80Hg Filling of electrons takes place in 5d sub-shell (4) IVth transition series i.e 6d series contains 10 elements and starts from 89Ac, 104Rf – 112Uub Filling of electrons takes place in 6d sub-shell (incomplete series) f-Block elements : When n, (n – 1) and (n – 2) shells are incompletely filled and last electron enters into forbital of antepenultimate i.e., (n – 2)th shell, elements of this class are called f-block elements General electronic configuration is (n – 2) f1-14 (n – 1) d0-1 ns2 The elements of f-blocks have been classified into two series st inner transition or f-series, contains 14 elements 58Ce to 71Lu Filling of electrons takes place in 4f subshell IInd inner transition or f-series, contains 14 elements 90Th to 103Lr Filling of electrons takes place in 5f subshell ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # PERIODIC PROPERTIES : VALENCY : It is defined as the combining capacity of the elements The word valency is derived from an Italian word “Valentia” which menas combining capacity DENSITY : (a) In a group volume of an atom increases along with atomic weight but atomic weight increases more than atomic volue, So density increases in a group Mass M Density (D) = = Volume V (b) In period - Density first increases till maximum and then decreases (s-block to d-block increases, d-block to p-block decreases) (c) In group - From top to bottom in a group density increases regularly e.g In VIIA gp F and Cl are gases (Low density) Br is liquid (density 3.19 gm/cm–3) I is solid (density 4.94 gm/cm–3) Effective nuclear charge : Between the outer most valence electrons and the nucleus of an atom, there exists number of shells containing electrons Due to the presence of these intervening electrons, the valence electrons are unable to experience the attractive pull of the actual number of protons in the nucleus These intervening electrons act as shield between the valence electrons and protons in the nucleus Thus, the presence of intervening (shielding) electrons reduces the electrostatic attraction between the protons in the nucleus and the valence electrons because intervening electrons repel the valence electrons The concept of effective nuclear charge helps in understanding the effects of shielding on periodic properties The effective nuclear charge (Zeff) is the charge actually felt by the valence electron Zeff is given by Zeff = Z – , (where Z is the actual nuclear charge (atomic number of the element) and  is the shielding (screening) constant) The value of  i.e shielding effect can be determined using the Slater’s rules Atomic radius : Covalent radius : It is one-half of the distance between the centres of two nuclei (of like atoms) bonded by a single covalent bond as shown in figure dA  A (b) For heterodiatomic molecules in which electronegativity remains approximately same dA – B = rA + rB (a) For homodiatomic molecules dA–A = rA + rA or 2rA so, rA = For heteronuclear diatomic molecule, A–B, where difference between the electronegativity values of atom A and atom B is relatively larger, dA – B = rA + rB – 9.0  This formula was given by Stevenson & Schomaker Electronegativity values are given in Pauling units and radius in picometers  = XA – XB where XA and XB are electronegativity values of high electronegative element A and less electronegative element B ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # Vander Waal’s radius (Collision radius) : It is one-half of the internuclear distance between two adjacent atoms in two nearest neighbouring molecules of the substance in solid state as shown in figure Vander Waal’s radius does not apply to metal and its magnitude depends upon the packing of the atoms when the element is in the solid state Metallic radius (Crystal radius) : It is one-half of the distance between the nuclei of two adjacent metal atoms in the metallic crystal lattice as shown in figure Thus, the covalent, vander Wall’s and metallic radius magnitude wise follows the order, rcovalent < rcrystal < rvander Walls IONISATION POTENTIAL OR IONISATION ENERGY OR IONISATION ENTHALPY : (i) Minimum energy required to remove most loosly held outer most shell e– in ground state from an isolated gaseous atom is known as Ionisation Potential (ii) Successive I.E (a) For an atom M, successive ionisation energies are as follows M + E1 M+ + e– E1 = IP1 M+ + E2 M+2 + e– E2 = IP2 M+2 + E3 M+3 + e– E3 = IP3 IP3 > IP2 > IP1 (b) e– can not be removed from solid state of an atom, it has to convert in gaseous form, Energy required for conversion from solid state to gaseous state is called Sublimation energy (c) IP is always an endothermic process (H = +ve) In a period : In a period atomic size decreases and zeff increases so removal of electron become difficult and IE increases Li Be B C N O F Ne            atomic size decreases, zeff increases IE increases IE = Ne > F > N > O > C > Be > B > Li ELECTRON AFFINITY / ELECTRON GAIN ENTHALPY The amount of energy released or absored when electron is added to the valence shell of an isolated gaseous atom X + e– X– + E.A known as Electron affinity ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # Mostly energy is released in the process of first E.A X + e– X– + EA1 If EA1 is exothermic then (eg H (electron gain enthalpy) = – ve) – EA1 is mostly positive In period : Electron affinity increases along the period due to increase in Zeff and decrease in atomic size Li Be B C N O F Ne Na Mg Al Si P S Cl Ar Zero Less zero F > O > C > B > N > Be > Ne Cl > S > Si > Al > P > Mg > Ar In Group : Electron affinity of 3rd period element is greater than electron affinity of 2nd period elements of the respective group F 2s22p5 Cl 3s23p5 Due to small size of fluorine, electron density around the nucleus increses The incoming electron suffers more repulsion In case of chlorine electron density decreases due to large size, decreasing order of electron affinity of halogen Cl > F > Br > I S>O>P>N Si > C > P > N N & P have low electron affinity due to stable half filled configuration Difference between EN and EA Electronegativity – Tendency of an atom in a molecule to attract the bonded electrons – Relative value of an atom – – (i) (ii) (iii) (iv) It regularly changed in a period or group It has no unit – Electron Affinity Energy released when an electron is added to neutral isolated gaseous atom Absolute value of an atom – It does not changes regularly – It is measured in eV/atom or KJ mol–1 or K.cal mole–1 – ELECTRONEGATIVITY (EN) The tendency of an atom to attract shared electrons towards itself is called electronegativity EN and EA both have tendency to attract electrons but electron affinity is for isolated atoms Where as electronegativity is for bonded atoms A polar covalent or ionic bond of A – B may be broken as (a) A – B A– : + B+ (EN A > EN B) or (b) A – B A+ + :B– (EN A < EN B) depending on their tendency to attract bonded electron There is no unit of electronegativity as EN is tendency of a bonded atom not an energy H 2.1 Li Be B C N O F 1.0 1.5 2.0 2.5 3.0 3.5 4.0 Na Mg Al Si P S Cl 0.9 1.2 1.5 1.8 2.1 2.5 3.0 K Br 0.8  Rb  0.8 I Cs  0.7   Fr  0.7  – Small atoms are normally having more EN than larger atoms ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # PART - I : OBJECTIVE QUESTIONS * Marked Questions are having more than one correct option Section (A) : Atomic and Ionic Radius A-1 A-2 A-3 A-4 The correct order of atomic size of C, N, P, S follows the order (A) N < C < S < P (B) N < C < P < S (C) C < N < S < P Match list-I with list-II List -I Ion (I) Li+ (II) Na+ (III) Br– (IV) I– Codes : I II (A) a b (B) b c (C) c d (D) d c (D) C < N < P < S and select the correct answer using the codes given below List-II Radius (in pm) (a) 216 (b) 195 (c) 60 (d) 95 III d a b b IV c d a a The ionic radii of N3–, O2– and F– are respectively given by (A) 1.36, 1.40, 1.71 (B) 1.36, 1.71, 1.40 (C) 1.71, 1.40, 1.36 The screening effect of d-electrons is (A) Equal to the p-electrons (C) Same as f-electrons (D) 1.71, 1.36, 1.40 (B) Much more than p-electrons (D) Less than p-electrons A-5 In which of the following compounds manganese shows maximum radius (A) MnO2 (B) KMnO4 (C) MnO (D) K3[Mn(CN)6] A-6 Arrange in the increasing order of atomic radii of the following elements O, C, F, Cl, Br (A) F < O < C < Cl Ni > Pd (D) Pd > Pt > Ni Which group of atoms have nearly same atomic radius (A) Na, K, Rb, Cs (B) Li, Be, B, C (C) Fe, Co, Ni (D) F, Cl, Br, I In the ions P3–, S2– and Cl– the increasing order of size is (A) Cl– < S2– < P3– (B) P3– < S2– < Cl– (C) S2– < Cl– < P3– (D) S2– < P3– < Cl– Atomic radii of Fluorine and Neon in Angstrom units are given by (A) 0.72, 1.60 (B) 1.60, 1.60 (C) 0.72, 0.72 (D) None of these Which of the following has largest radius (A) 1s2, 2s2, 2p6, 3s2 (C) 1s2, 2s2, 2p6, 3s2, 3p3 (B) 1s2, 2s2, 2p6, 3s2, 3p1 (D) 1s2, 2s2, 2p6, 3s2, 3p5 Arrange the elements in increasing order of atomic radius Na, Rb, K, Mg (A) Na < K < Mg < Rb (B) K < Na < Mg < Rb (C) Mg < Na < K < Rb (D) Rb < K < Mg < Na ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # A-13 Arrange the following in order of increasing atomic radii Na, Si, Al, Ar (A) Na < Si < Al < Ar (B) Si < Al < Na < Ar (C) Ar < Al < Si < Na (D) Na < Al < Si < Ar A-14 Consider the isoelectronic series : K+, S2–, Cl– and Ca2+, the radii of the ions decrease as (A) Ca2+ > K+ > Cl– > S2– (B) Cl– > S2– > K+ > Ca2+ 2– – + 2+ (C) S > Cl > K > Ca (D) K+ > Ca2+ > S2– > Cl– A-15 Which of the following is not isoelectronic series(A) Cl–, P3–, Ar (B) N3–, Ne, Mg+2 (C) B+3, He, Li+ (D) N3–, S2–, Cl– A-16 In the isoelectronic species the ionic radii (Å) of N3–, Ne and Al+3 are respectively given by (A) 1.36, 1.40, 1.71 (B) 1.36, 1.71, 1.40 (C) 1.71, 1.40, 1.36 (D) 1.71, 1.36, 1.40 A-17 The size of the following species increases in the order : (A) Mg2+ < Na+ < F– (B) F– < Na+ < Mg2+ (C) Mg < F– < Na+ (D) Na+ < F– < Mg2+ Highest size will be of(A) Br– (B) I (D) I+ A-18 (C) I– A-19 Element Hg has two oxidation staters Hg+1 & Hg+2, the right order of radii of these ions (A) Hg+1 > Hg+2 (B) Hg+2 > Hg+1 (C) Hg+1 = Hg+2 (D) None of these A-20 The correct order of increasing atomic size of element N,F, Si & P (A) N < F < Si N < P < Si (C) F < N < P < Si (D) F < N < Si < P The correct order of atomic / ionic size (A) N < Li < B (B) Cl < Mg < Ca (D) Na+ < Mg+2 < Cl¯ A-21 (C) Ca+2 < S–2 < Cl¯ Section (B) : Ionization Energy or Potential B-1 Correct orders of Ist I.P are (i) Li < B < Be < C (ii) O < N < F (iii) Be < N < Ne (A) (i), (ii) (B) (ii), (iii) (C) (i), (iii) (D) (i), (ii), (iii) B-2 The maximum tendency to form unipositive ion is for the elment with the electronic configuration(A) 1s2, 2s2, 2p6, 3s2 (B) 1s2, 2s22p6, 3s23p1 2 2 (C) 1s , 2s 2p , 3s 3p (D) 1s2, 2s22p6, 3s23p3 B-3 The second ionisation potentials in electron volts of oxygen and fluorine atoms are respectively given by : (A) 35.1., 38.3 (B) 38.3, 38.3 (C) 38.3, 35.1 (D) 35.1, 35.1 B-4 A sudden large jump between the values of 2nd and 3rd IP of an element would be associated with the electronic configuration(A) 1s2, 2s2 2p6, 3s1 (B) 1s2, 2s2 2p6, 3s2 3p5 2 2 (C) 1s , 2s 2p , 3s 3p (D) 1s2, 2s2 2p6 3s2 B-5 The ionization energy of sodium is 495 kJ mol–1 How much energy is needed to convert atoms persent in 2.3 mg of sodium into sodium ions (A) 4.95 J (B) 49.5 J (C) 495 J (D) 0.495 J B-6 Ionisation energy increases in the order (A) Be < B < C < N (B) B < Be < C < N (C) C < N < Be < B ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 (D) N < C < Be < B PERIODIC TABLE & PERIODICITY ADVANCED # B-7 IP and IP of Mg are 178 and 348 K.cal mol –1 The enthalpy required for the reqction Mg  Mg2+ + 2e– is (A) + 170 K.cal (B) + 526 K.cal (C) – 170 K.cal (D) – 526 K.cal B-8 Highest ionisation potential in a period is shown by (A) Alkali metals (B) Noble gases (C) Halogens (D) Representative elements B-9 In which of the following electronic configuration ionisation energy will be maximum (A) [Ne] 3s2 3p1 (B) [Ne] 3s2 3p2 (C) [Ne] 3s2 3p3 (D) [Ar] 3d10 4s2 4p3 B-10 The ionization energy will be maximum for the process (A) Ba  Ba++ (B) Be Be++ (C) Cs  Cs+ (D) Li  Li+ The correct order of second I.P (A) Na < Mg > Al < Si (B) Na > Mg < Al > Si (D) Na > Mg > Al > Si B-11 B-12 (C) Na > Mg > Al < Si Amongst the following, the incorrect statement is (A) IE1 (Al) < IE1 (Mg) (B) IE1 (Na) < IE1(Mg) (C) IE2 (Mg) > IE2 (Na) (D) IE3 (Mg) > IE3 (Al) Section (C) : Electron affinity or Electron Gain Enthalpy C-1 In which case the energy released is minimum (A) Cl  Cl– (B) P  P– (C) N  N– (D) C  C– C-2 In the formation of a chloride ion, from an isolated gaseous chlorine atom, 3.8 eV energy is released, which would be equal to (A) Electron affinity of Cl– (B) Ionisation potential of Cl (C) Electronegativity of Cl (D) Ionisation potential of Cl– C-3 The correct order of electron affinity is (A) Be < B < C < N (B) Be < N < B < C (C) N < Be < C < B (D) N < C < B < Be C-4 Electron addition would be easier in (A) O (B) O+ C-5 (C) O– (D) O+2 H In the process Cl(g) + e–  Cl–(g), H is (A) Positive (B) Negative (C) Zero (D) None C-6 2 O(g) + 2e–  O ( g ) Heg = 744.7 KJ/mole The positive value of Heg is due to (A) Energy is released to add to e– to O–1 (B) Energy is required to add to e– to O–1 – (C) Energy is needed to add on e to O (D) None of the above is correct C-7 Which of the following process energy is liberated (A) Cl  Cl+ + e– (B) HCl  H+ + Cl– (C) Cl + e–  Cl– C-8 Second electron affinity of an element is (A) Always exothermic (C) Exothermic for few elements (D) O– + e–  O–2 (B) Endothermic for few elements (D) Always endothermic C-9 The element having very high ionization enthalpy but zero electron gain enthalpy is(A) H (B) F (C) He (D) Be C-10 The electron affinity values for the halogens shown the following trend (A) F < Cl > Br > I (B) F < Cl Cl > Br > I (D) F < Cl > Br < I C-11 The process requiring the absorption of energy is (A) F  F– (B) Cl  Cl– (C) O  O2– C-12 (D) H  H– Which of the following configuration will have least electron affinity (A) ns2np5 (B) ns2np2 (C) ns2np3 (D) ns2np4 ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # PART - I : MIXED OBJECTIVE Single choice type Which of the following element has highest metallic character Element IP (A) P 17 eV (B) Q eV (C) R 10 eV (D) S 13 eV The electronic configuration of an element is 1s2 2s2 2p6 3s2 3p4 The atomic number and the group number of the element ‘X’ which is just below the above element in the periodic table are respectively (A) 24 & (B) 24 & 15 (C) 34 & 16 (D) 34 & Choose the s-block element from the following: (A) 1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s1 (B) 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s1 (C) 1s2, 2s2, 2p6, 3s2, 3p6, 4s1 (D) all of the above False statement for periodic classification of elements is (A) The properties of the elements are periodic function of their atomic numbers (B) No of non-metallic elements is less than the no of metallic elements (C) First ionization energy of elements does not increase regularly with the increasing of atomic number in a period (D) d-subshell is filled by final electron with increasing atomic number of inner transition elements Pick out the isoelectronic species from the following: CH 3 I +CH3 II H3O+ III NH3 IV (A) I and II (B) III and IV (C) I and III (D) II, III and IV If there were 10 periods in the periodic table then how many elements would this period can maximum comprise of (A) 50 (B) 72 (C) 32 (D) 98 Among the following which species is/are paramagnetic (i) Sr2+ (ii) Fe3+ (iii) Co2+ (iv) S2– (A) i, iv, v (B) i, ii, iii (C) ii, iii (v) Pb2+ (D) iv, v If each orbital can hold a maximum of three electrons, the number of elements in 9th period of periodic table (long form) are (A) 48 (B) 162 (C) 50 (D) 75 Atomic radii of F & Ne in Angstrom are respectively given by : (A) 0.72, 1.60 (B) 1.60, 1.60 (C) 0.72, 0.72 (D) 1.60, 0.72 Which one of the following is the smallest in size ? (A) N  (B) O  (C) F  (D) Na + 10 11 Which one of the following is correct order of increase in size ? (A) Mg < Na+ < O2– < Al (B) Na+ < Al < Mg < O2– (C) Na+ < O2– < Al < Mg (D) Na+ < O2– < Mg < Al ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 15 12 13 The first Ionization energy of Na, Mg, Al & Si are in the order : (A) Na < Mg > Al < Si (B) Na > Mg > Al > Si (C) Na < Mg < Al > Si (D) Na > Mg > Al < Si The first ionisation energy in eV of N & O are respectively given by : (A) 14.6, 13.6 (B) 13.6, 14.6 (C) 13.6, 13.6 (D) 14.6, 14.6 14 As one move down the group from top to bottom then which one among the following will not be observed? (A) Ionisation energy increases (B) Electron affinity decreases (C) Electronegativity decreases (D) Atomic radii increase 15 Which of the following relation is correct with respect to first (I) and second (II) ionization energies of sodium and magnesium ? (A) IMg = IINa (B) INa > IMg (C) IIMg > IINa (D) IINa > IIMg 16 The ionization energy will be higher when the electron is removed from if other factors being equal (A) s-orbital (B) p-orbital (C) d-orbital (D) f-orbital 17 Which of the following isoelectronic ion has the lowest 1st ionization energy ? (A) Na+ (B) F– (C) Mg2+ (D) O2– 18 A large difference between the third and fourth ionization energies indicates the presence of : (A) valence electrons in an atom (B) valence electrons in an atom (C) valence electrons in an atom (D) valence electrons in an atom 19 The second ionization energies of elements are always higher than their first ionization energies because: (A) the cation is smaller than its parent atom (B) it is easier to remove electron from cation (C) ionization is an endothermic process (D) cation formed always have stable half filled or completely filled valence shell electron configuration 20 Which is a true statement ? (A) Larger is the value of ionisation energy easier is the formation of cation (B) Larger is the value of electron affinity easier is the formation of anion (C) Larger is the value of ionisation energy as well as electron affinity the smaller is the electronegativity of atom (D) Larger is the Zeff larger is the size of atom 21 Which of the following is the correct order of ionisation energy ? (A) O2– < F– < Na+ < Mg2+ (B) F– < O2 – < Na+ < Mg2+ (C) O2 – < Na+ < F– < Mg2+ (D) Mg2+ < Na+ < F– < O2 – 22 Values of E1, E2 and E3 of an element are 9.32, 18.21 and 553.83 eV What informations these data convey ? (A) The element has two electrons in the valence shell (B) The element has two p–electrons in the valence shell (C) (A) and (B) both (D) None of the two 23 The electron gain enthalpies of halogens are as given below F = – 332, Cl = – 349, Br = – 324,  = – 295 kJ mol–1 The less negative value for F as compared to that of Cl is due to : (A) strong electron-electron repulsions in the compact 2–p sub shell of F (B) strong electron -electron repulsions in the bigger 3–p sub shell of Cl (C) higher electronegativity value of Cl (D) higher effective nuclear charge of F ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 16 24 The formation of the oxide ion O2– (g) requires first an exothermic and then an endothermic step as shown below O(g) + e– = O– (g) ; egH = – 142 kJmol–1 – – 2– O (g) + e = O (g) ; egH = 844 kJmol–1 This is because : (A) O– ion will tend to resist the addition of another electron on account of same charge (B) oxygen has high electron affinity (C) oxygen is more electronegative (D) O– ion has comparatively larger size than oxygen atom 25 26 27 28 For electron affinity of halogens which of the following is correct ? (A) Br > F (B) F > Cl (C) Br < Cl (D) F > I Which of the following is the correct order of ionisation energy ? (1) Be+ > Be (2) Be > Be+ (3) C > Be (A) 2, (B) 3, (C) 1, (4) B > Be (D) None of these The correct order of electronegativity is : (A) F > Cl I (B) F > O > N > C (D) All (C) S < O < Se < Te The electronegativity of the following elements increases in the order : (A) C, N, Si, P (B) N, Si, C, P (C) Si, P, C, N (D) P, Si, N, C 29 Consider the following statements E(I) of nitrogen atom is more than E(I) of oxygen atom Electron affinity of oxygen is less than sulphur atom Electronegativity of an atom has no relation with its ionization enthalpy and electron gain enthalpy Which of the above statements are correct ? (A) 1, (B) 1, (C) 2, (D) 1, & 30 Which of the following statement is wrong ? (A) Vander Waal’s radius of iodine is more than its covalent radius (B) All isoelectronic ions belong to same period of the periodic table (C) I.E(I) of N is higher than that of O while I.E(II) of O is higher than that of N (D) The electron affinity of N is less than that of P 31 The IP1, IP2, IP3, IP4 and IP5 of an element are 7.1, 14.3, 34.5, 46.8, 162.2 eV respectively The element is likely to be (A) Na (B) Si (C) F (D) Ca 32 With reference to ionisation potential which one of the following sets is correct (A) Li > K > B (B) B > Li > K (C) Cs > Li > K (D) Cs < Li < K 33 Successive ionisation energies of an element ‘X’ are given below (in K.Cal) : IP1 IP2 IP3 IP4 165 195 556 595 Electronic configuration of the element ‘X’ is (A) 1s2, 2s2 2p6, 3s2 3p2 (B) 1s2, 2s1 2 (C) 1s , 2s 2p (D) 1s2, 2s2 2p6, 3s2 34 The ionistion energy of B and Al as compared to Be and Mg are (A) Lower (B) Higher (C) Equal (D) None of these Which of the following has 2nd IP < Ist IP (A) Mg (B) Ne (D) None 35 (C) C ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 17 36 Among the following elements (Whose electronic configuration is give below) the one having the highest ionisation energy is (A) [Ne] 3s2 3p3 (B) [Ne] 3s2 3p4 (C) [Ne] 3s2 3p5 (D) [Ne] 3s2 37 The correct order of decreasing first ionization energy is (A) Si > Al > Mg > Na (B) Si > Mg > Al > Na (C) Al > Si > Mg > Na (D) None of these 38 Which of the following transitions involves maximum amount of energy 3+ (A) M–(g)  M(g) (B) M(g)  M+(g) (C) M+(g)  M2+ (D) M2+ (g) (g)  M (g) 39 Element X, Y and Z have atomic numbers 19, 37 and 55 respectively Which of the following statements is true (A) Their ionisation potential would increase with the increasing atomic number (B) ‘Y’ would have an ionisation potential in between those of ‘X’ and ‘Z’ (C) ‘Z’ would have the highest ionisation potential (D) ‘Y’ would have the highest ionisation potential 40 The first (IE1) and second (IE2) ionization energies (kJ/mol) of a few elements designated by Roman numerals are given below Which of these would be an alkali metal ? IE1 IE2 (A) I 2372 5251 (B) II 520 7300 (C) III 900 1760 (D) IV 1680 3380 41 The decreasing order of the ionization potential of the following elements is (A) Ne > Cl > P > S > Al > Mg (B) Ne > Cl > P > S > Mg > Al (C) Ne > Cl > S > P > Mg > Al (D) Ne > Cl > S > P > Al > Mg 42  K(g)  K(s)For the processes K+(g) (A) Energy is released in (I) and abosrbed in (II) (B) Energy is absorbed in (I) and released in (II) (C) Energy is absorbed in both the processes (D) Energy is released in both the processes 43 The order of first ionisation enthalpies of the elments Li, Be, B, Na is (A) Li > Be > B > Na (B) Be > B > Li > Na (C) Na > Li > B > Be (D) Be > Li > B > Na 44 Arrange the elements S, P, As in order of increasing ionization enthalpy (A) S N > O > F (B) O > N > F > C (C) O > F > N > C (D) F > O > N > C 46 First, second and third IP values are 100eV, 150eV and 1500eV Element can be (A) Be (B) B (C) F (D) Na 47  M+(g) + e–,   H = 100 eV M(g)   M2+(g) + 2e–, H = 250 eV M(g)  Which is incorrect statement ? (A) IE1 of M(g) is 100 eV (C) IE2 of M(g) is 250 eV 48 I II (B) IE1 of M+(g) is 150 eV (D) IE2 of M(g) is 150 eV I.P of sodium is 5.14 eV then I.P of potassium will be (A) Equal to sodium (B) 5.68 eV (C) 4.34 eV (D) 10.28 eV mol–1) 49 The correct values of ionization enthalpies (in kJ of Si, P, Cl and S respectively are (A) 786, 1012, 999, 1256 (B) 1012, 786, 999, 1256 (C) 786, 1012, 1256, 999 (D) 786, 999, 1012, 1256 50 Consider the following changes A  A+ + e– : E1 and A+  A2 + e– : E2 The energy required to pull out the two electrons are E1 and E2 respectively The correct relationship between two energies would be (A) E1 < E2 (B) E1 = E2 (C) E1 > E2 (D) E1  E2 ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 18 51 Electron affinity is a (A) Relative strength to attract the shared electron pair (B) Necessary energy required to remove the electron from the ultimate orbit (C) Energy released when an electron is added to the outermost shell (D) Energy released when an electron is added to the inner shell 52 The electron affinityes of , O, S and Cl are such that (A) N < O < S < Cl (B) O < N < Cl < S (C) O  Cl < N  S (D) O < S < Cl < N The correct order of electron affinity of B, C, N, O is (A) O > C > N > B (B) B > N > C > O (C) O > C > B > N (D) O > B > C > N 53 54 The correct order of electron affinity for the different families is (A) Halogen > carbon > nitrogen > oxygen (B) Halogen > oxygen > nitrogen > carbon (C) Halogen > nitrogen > carbon > oxygen (D) Halogen > oxygen > carbon > nitrogen 55 Highest electron-affinity is associated with the configuration (A) 2s2, 2p0 (B) 2s2, 2p2 (C) 2s2, 2p3 (D) 2s2, 2p1 56 Adding electron a neutral gaseous atom usually leads to (i) Liberation of energy (ii) Formation of anion (iii) Proton/electron ratio decrease (iv) Proton/electron ratio increase (A) (i), (iv) (B) (ii), (iii), (iv) (C) (i), (ii), (iv) (D) (i), (ii), (iii) 57 Which statement is correct (A) The E.A of carbon is greater than oxygen (C) The E.A of iodine is greater than bromine (B) The E.A of sulphur is less than oxygen (D) The E.A of bromine is less than chlorine 58 Fluorine has low electron affinity than chlorine because of (A) Smaller radius of fluorine, high density (B) Smaller radius of chlorine, high density (C) Bigger radius of fluorine, less density (D) Smaller radius of chlorine, less density 59 Which of the following element is expected to have highest electron gain enthalpy (A) 1s22s22p63s 23p5 (B) 1s22s22p3 (C) 1s22s22p4 (D) 1s22s22p5 60 Arrange N, O and S in order of decreasing electron affinity (A) S > O > N (B) O > S > N (C) N > O > S (D) S > N > O 61 Which of the following set of elements exhibits positive and negative oxidation states(A) O, Cl, H (B) F, Li, Be (C) Na, Mg, Al (D) H, Ba, Ne 62 A, B and C are hydroxy-compounds of the elements X, Y and Z respectively X, Y and Z are in the same period of the periodic table A gives an aqueous solution of pH less than seven B reacts with both strong acids and strong alkalis C gives an aqueous solution which is strongly alkaline Which of the following statements is/are true: I : The three elements are metals II : The electronegativities decrease from X to Y to Z III : The atomic radius decreases in the order X, Y and Z IV : X, Y and Z could be phosphorus, aluminium and sodium respectively : (A) I, II, III only correct (B) I, III only correct (C) II, IV only correct (D) II, III, IV only correct 63 The correct set of decreasing order of electronegativity is (A) Li, H, Na (B) Na, H, Li (C) H, Li, Na (D) Li, Na, H Increasing order of electronegativity is (A) Bi F > N > C (B) F > N > C > O (C) C > F > N > O ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 (D) F > O > N > C PERIODIC TABLE & PERIODICITY ADVANCED # 19 More than one choice type 66 M(g)  M+ (g) + e– ; H = 100 eV M(g)  M2+ (g) + 2e– ; H = 250 eV Which is/are correct statement(s) ? (A) IE1 of M(g) is 100 eV (C) IE2 of M(g) is 250 eV (B) IE1 of M+ (g) is 150 eV (D) IE2 of M(g) is 150 eV 67 In halogens, which of the following increases from iodine to fluorine? (A) Bond length (B) Electronegativity (C) The ionization energy of the element (D) Oxidizing power 68 Which of the following have isoelectronic structures? (i) CH3+ (ii) H3O+ (iii) CH–3 (A) (i) and (ii) (B) (i) and (iii) (C) (iii) and (iv) (iv) NH3 (D) (ii), (iii) and (iv) Which among the following are isostructural pairs? (A) NF3 and H3O+ (B) NO–3 and BF3 (C) NF3 and NO–3 (D) NF3 and NH3 69 70 Which of the following statements are correct? (A) F is the most electronegative and Cs the most electropositive element (B) The electronegativity of halogens decreases from F to I (C) The electron affinity of Cl is higher than that of F though their electronegativities are in the reverse order (D) The electron affinity of noble gases in almost zero 71 Which of the following species are isoelectronic with Ne? (A) N3– (B) Mg2+ (C) Al3+ (D) Ca2+ 72 In which of the following are the orders of electron affinity of the elements or ions shown correctly? (A) S > O– (B) O > S– (C) O– > S– (D) N– > P 73 Which of the following salts does not undergo hydrolysis ? (A) NaCl (B) KCN (C) KClO4 (D) Na2CO3 Which of the following halides are soluble in water? (A) AlF3 (B) AgI (C) AgCl (D) AgF Which of the following pairs have approximately the same atomic radii? (A) Pd and Pt (B) Al and Mg (C) Al and Ga (D) Na and Ne 74 75 76 77 The ionic bonds X+ Y– are formed when the : (A) electron affinity of Y is high (C) lattice energy of XY is high (B) ionization energy of X is low (D) lattice energy of XY is low Which of the following pairs not show the inert-pair effect? (A) Cu and Au (B) Si and Ge (C) TI and Pb (D) Bi and Sn PART - II : SUBJECTIVE QUESTIONS Elements A, B, C, D and E have the following electronic configurations : A : 1s 2s 2p1 B : 1s 2s 2p6 3s 3p1 C : 1s 2s 2p6 3s 3p3 D : 1s 2s 2p6 3s 3p5 2 6 E : 1s 2s 2p 3s 3p 4s Which among these will belong to the same group in the periodic table ? An element X with Z = 112 has been recently discovered What is the electronic configuration of the element ? To which group and period will it belong ? ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 20 What is the effective nuclear charge at the periphery of nitrogen atom when a extra electron is added during the formation of an anion Compare the value of Zeff when the atom is ionized to N+ X – X bond length is 1.00 Å and C–C bond length is 1.54 Å If electronegativities of X and C are 3.0 and 2.0 respectively, then C–X bond length is likely to be ? (using Stevension & Schomaker formula) Atomic radius of Li is 1.23 Å and ionic radius of Li+ is 0.76Å Calculate the percentage of volume occupied by single valence electron in Li Select from each group the species which has the smallest radius stating appropriate reason (a) O, O–, O2– (b) P3+ , P4+ , P5+ Mg2+ is smaller than O2– in size, though both have same electronic configuration Explain ? From each set, choose the atom which has the largest ionization enthalpy and explain your answer with suitable reasons (a) F, O, N (b) Mg, P, Ar First and second ionisation energies of magnesium are 7.646 eV and 15.035 eV respectively The amount of energy in kJ needed to convert all the atoms of magnesium into Mg2+ ions present in 12 mg of magnesium vapour will be ? [Given eV = 96.5 kJ ml–1] 10 Consider the elements N, P, O and S and arrange them in order of increasing negative electron gain enthalpy 11 Why halogens have high electron gain enthalpies (i.e –egH) ? 12 The amount of energy when million atoms of iodine are completely converted into I– ions in the vapour state according to the equation, I (g) + e– (g)  I– (g) is 5.0 × 10–13 J Calculate the electron gain enthalpy of iodine in terms of kJ mol–1 and eV per atom 13 Account for the large decrease in electron affinity between Li and Be despite the increase in nuclear charge 14 Calculate the electronegativity of carbon from the following data : EH–H = 104.2 kcal mol–1 , EC–C = 83.1 kcal mol–1 EC–H = 98.8 kcal mol–1| , X H = 2.1 15 Arrange the following in decreasing basic nature LiOH, NaOH, KOH, CsOH LiOH, NaOH, KOH, CsOH 16 Arrange the following compounds in increasing order of acidic strength Al2O3, SiO2, P2O3 and SO2 Al2O3, SiO2, P2O3 SO2 17 A M2+ ion derived from a metal in the first transition metal series has four electrons in 3d subshell What element might M be ? 18 Following are the valence shell electronic configurations of some elements (i) 3s 3p5 (ii) 3d10 4s (iii) 2s 3p6 4s (iv) 1s 2s Find out the blocks to which they belong in the periodic table ? 19 Find out the group of the element having the electronic configuration, 1s 2s 2p6 3s 3p6 3d6 4s ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 21 20 Arrange the following ions in the increasing order of their size : Be2+ , Cl–, S2– , Na+ , Mg2+ , Br– ? 21 The (IE1) and the (IE2) in kJ mol–1 of a few elements designated by Roman numerals are shown below: I II III IE1 403 549 1142 IE2 2640 1060 2080 Which of the above elements is likely to be a (a) non-metal 22 (b) alkali metal (c) alkaline earth metal ? Ionisation energy and electron affinity of fluorine are respectively 17.42 and 3.45 eV Calculate electronegativity of fluorine atom 23 Select neutral, acidic,basic and amphoteric oxides from the following CO, BeO, Na2O , N2O5 24 Why the electron gain enthalpy values of alkaline earth metals are lower (i.e less negative) or positive ? PART - I : IIT-JEE PROBLEMS (PREVIOUS YEARS) Which one of the following has largest size ? (A) Na (B) Na+ (C) Na– [IIT-1993] (D) None of these The decreasing order of the second ionization energy of K, Ca and Ba is (At Nos K = 19, Ca = 20, Ba = 56) [IIT-1993] (A) K > Ca > Ba (B) Ca > Ba > K (C) Ba > K > Ca (D) K > Ba > Ca Element Hg has two oxidation states Hg+1 & Hg+2 The right order of radii of these ions - [IIT-1994] (A) Hg+1 > Hg+2 (B) Hg+2 > Hg+1 (C) Hg+1 = Hg+2 (D) Hg+2  Hg+1 Which has most stable + oxidation state : (A) Sn (B) Pb [IIT-1995] (C) Fe (D) Ag Moving from right to left in a periodic table, the atomic size is(A) Increased (B) Decreased (C) Remains constant [IIT-1995] (D) None of these The increasing order of electronegativity in the following elements(A) C, N, Si, P (B) N, Si, C, P (C) Si, P, C, N (D) P, Si, N, C [IIT-1995] One element has atomic weight 39 Its electronic configuration is 1s2, 2s2 2p6, 3s2 3p6 4s1 The true statement for that element is[IIT-1995] 38 (A) More (IE)1 (B) Transition element (C) Isotone with 18Ar (D) Stable oxide M2O The number of paired electrons in oxygen is (A) (B) 16 Which of the following oxide is neutral ? (A) CO (B) SnO2 [IIT-1995] (C) (D) 32 [IIT-1996] (C) ZnO ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 (D) SiO2 PERIODIC TABLE & PERIODICITY ADVANCED # 22 10 Which of the following has the maximum number of unpaired electrons (A) Mg2+ (B) Ti3+ (C) V3+ (D) Fe2+ 11 The incorrect statement among the following is [IIT-1997] (A) the first ionisation potential of Al is less than the first ionisation potential of Mg (B) the second ionisation potential of Mg is greater that the second ionisation potential of Na (C) the first ionisation potential of Na is less than the first ionisation potential of Mg (D) the third ionisation potential of Mg is greater than the third ionisation potential of Al 12 The correct order of radii is (A) N < Be Na > Li (B) Be >Mg > Ca (C) B > C > N The correct order of acidic strength is (A) Cl2O7 > SO3 > P4O10 (C) Na2O > MgO > Al2O3 [IIT-1996] [IIT-2001] (D) Ge > Si > C [IIT-2000] (B) CO2 > N2O5 < SO3 (D) K2O > CaO > MgO Identify the least stable ion amongst the following(A) Li¯ (B) Be¯ (C) B¯ [IIT-2002] (D) C¯ Identify the correct order of acidic strengths of CO2, CO, CuO, CaO, H2O – (A) CaO < CuO < H2O < CO2 (B) H2O < CuO < CaO < CO2 (C) CaO < H2O < CuO < CO2 (D) H2O < CO2 < CaO < CuO [IIT-2002] PART - II : AIEEE PROBLEMS (PREVIOUS YEARS) The correct order of ionic radius is (1) Ce > Sm > Tb > Lu (3) Tb > Lu > Sm > Ce [AIEEE-2002] (2) Lu > Tb > Sm > Ce (4) Sm > Tb > Lu > Ce Ce3+, La3+, Pm3+ and Yb3+ have ionic radii in the increasing order as – (1) La3+ < Ce3+ < Pm3+ < Yb3+ (2) Yb3+ < Pm3+ < Ce3+ < La3+ 3+ 3+ 3+ 3+ (3) La = Ce < Pm < Yb (4) Yb3+ < Pm3+ < La3+< Ce3+ According to the Periodic Law of elements, the Variation in properties of elements is related to their ? [AIEEE-2003] (1) Nuclear masses (2) Atomic numbers (3) Nuclear neutron-proton number ratio (4) Atomic masses The reduction in atomic size with increase in atomic number is a characteristic of elements of [AIEEE-2003] (1) d-block (2) f-block (3) Radioactive series (4) High atomic masses Which one of the following groups represent a collection of isoelectronic species ? (At no Cs = 55, Br = 35) [AIEEE-2003] (1) N3–, F–, Na+ (2) Be, Al3+, Cl– (3) Ca2+, Cs+, Br (4) Na+, Ca2+, Mg2+ The atomic numbers of vanadium (V) Chromium (Cr), manganese (Mn) and iron (Fe) respectively 23, 24, 25 and 26 Which one of these may be expected to have the higher second ionization enthalpy? [AIEEE-2003] (1) Cr (2) Mn (3) Fe (4) V Which one of the following sets of ions represents the collection of isoelectronic species ? [AIEEE-2004] (1) K+, Cl–, Mg2+, Sc3+ (2) Na+, Ca2+, Sc3+, F– (3) K+, Ca2+, Sc3+, Cl– (4) Na+, Mg2+, Al3+, Cl– ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 [AIEEE-2002] PERIODIC TABLE & PERIODICITY ADVANCED # 23 Which one of the following ions has the highest value of ionic radius ? (1) O2– (2) B3+ (3) Li+ [AIEEE-2004] (4) F– Among Al2O3, SiO2, P2O3 and SO2 the correct order of acid strength is : (1) Al2O3 < SiO2 < SO2 < P2O3 (2) SiO2 < SO2 < Al2O3 < P2O3 (3) SO2 < P2O3 < SiO2 < Al2O3 (4) Al2O3 < SiO2 < P2O3 < SO2 [AIEEE-2004] 10 2 The formation of the oxide ion O g  requires first an exothermic and then an endothermic step as shown below : [AIEEE-2004] O(g) + e– = O–(g) H° = – 142 kJ mol–1 O–(g) + e– = O2–(g) H° = 844 kJ mol–1 This is because of : (1) O– ion will tend to resist the addition of another electron (2) Oxygen has high electron affinity (3) Oxygen is more electronegative (4) O– ion has comparatively larger size than oxygen atom 11 In which of the following arrangements the order is NOT according to the property indicated against it ? [AIEEE-2005] (1) Al3+ < Mg2+ < Na < F– – increasing ionic size (2) B < C < N < O – increasing first ionization enthalpy (3) I < Br < F < Cl – increasing electron gain enthalpy (with negative sign) (4) Li < Na < K < Rb – increasing metallic radius 12 Which of the following oxides is amphoteric in character ? (1) SnO2 (2) SiO2 (3) CO2 13 Pick out the isoelectronic structure from the following : I +CH3 II H3O+ III NH3 IV CH3– (1) I and II (2) III and IV (3) I and III [AIEEE-2005] (4) CaO [AIEEE-2005] (4) II, III and IV 14 The lanthanide contraction is responsible for the fact that [AIEEE-2005] (1) Zr and Y have about the same radius (2) Zr and Nb have similar oxidation state (3) Zr and Hf have about the same radius (4) Zr and Zn have the same oxidation state 15 Which of the following factors may be regarded as the main cause the lanthanide contraction ? [AIEEE-2005] (1) Poor shielding of one of 4f electron by another in the subshell (2) Effective shielding of one of 4f electrons by another in the subshell (3) Poorer shielding of 5d electrons by 4f electrons (4) greater shielding of 5d electrons by 4f electrons 16 The increasing order of the first ionization enthalpies of the elements B, P, S and F (lowest first) is– [AIEEE-2006] (1) F < S < P < B (2) P < S < B < F (3) B < P < S < F (4) B < S < P < F 17 Which one of the following sets of ions represents a collection of isoelectronic species ? [AIEEE-2006] (1) N3–, O2–, F–, S2– (2) Li+, Na+, Mg2+, Ca2+ (3) K+, Cl–, Ca2+, Sc3+ (4) Ba2+, Sr2+, K+, Ca2+ 18 lanthanoid contraction is caused due to [AIEEE-2006] (1) The same effective nuclear charge from Ce to Lu (2) The imperfect shielding on outer electrons by 4f electrons from the nuclear charge (3) The appreciable shielding on outer electrons by 4f electrons from the nuclear charge (4) The appreciable shielding on outer electrons by 5d electrons from the nuclear charge 19 Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se and Ar ? [AIEEE-2013] (1) Ca < S < Ba < Se < Ar (2) S < Se < Ca < Ba < Ar (3) Ba < Ca < Se < S < Ar (4) Ca < Ba < S < Se < Ar 20 The first ionisation potential of Na is 5.1 eV The value of electron gain enthalpy of Na+ will be :[AIEEE-2013] (1) – 2.55 eV (2) – 5.1 eV (3) – 10.2 eV (4) +2.55 eV ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 24 NCERT QUESTIONS What is the basic theme of organisation in the periodic table? Which important property did Mendeleev use to classify the elements in his periodic table and did he stick to that? What is the basic difference in approach between the Mendeleevís Periodic Law and the Modern Periodic Law? On the basis of quantum numbers, justify that the sixth period of the periodic table should have 32 elements In terms of period and group where would you locate the element with Z = 114? Write the atomic number of the element present in the third period and seventeenth group of the periodic table Which element you think would have been named by (i) Lawrence Berkeley Laboratory (ii) Seaborgis group? Why elements in the same group have similar physical and chemical properties? What does atomic radius and ionic radius really mean to you? 10 How atomic radius vary in a period and in a group? How you explain the variation? 11 What you understand by isoelectronic species? Name a species that will be isoelectronic with each of the following atoms or ions (i) F– (ii) Ar (iii) Mg2+ (iv) Rb+ 12 Consider the following species : N3–, O2–, F–, Na+, (a) What is common in them? (b) Arrange them in the order of increasing ionic radii Mg2+ and Al3+ 13 Explain why cation are smaller and anions larger in radii than their parent atoms? 14 What is the significance of the terms - 'isolated gaseous atom' and 'ground state' while defining the ionization enthalpy and electron gain enthalpy? Hint : Requirements for comparison purposes 15 Energy of an electron in the ground state of the hydrogen atom is – 2.18 × 10–18 J Calculate the ionization enthalpy of atomic hydrogen in terms of J mol–1 Hint: Apply the idea of mole concept to derive the answer 16 Among the second period elements the actual ionization enthalpies are in the order Li < B < Be < C < O < N < F < Ne Explain why (i) Be has higher iH than B (ii) O has lower iH than N and F? ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 25 17 How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium? 18 What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group? 19 The first ionization enthalpy values (in kJ mol–1) of group 13 elements are : B Al Ga In Tl 801 577 579 558 589 How would you explain this deviation from the general trend ? 20 Which of the following pairs of elements would have a more negative electron gain enthalpy? (i) O or F (ii) F or Cl 21 Would you expect the second electron gain enthalpy of O as positive, more negative or less negative than the first? Justify your answer 22 What is the basic difference between the terms electron gain enthalpy and electronegativity? 23 How would you react to the statement that the electronegativity of N on Pauling scale is 3.0 in all the nitrogen compounds? 24 Describe the theory associated with the radius of an atom as it (a) gains an electron (b) loses an electron 25 Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer 26 What are the major differences between metals and non-metals? 27 Use the periodic table to answer the following questions (a) Identify an element with five electrons in the outer subshell (b) Identify an element that would tend to lose two electrons (c) Identify an element that would tend to gain two electrons (d) Identify the group having metal, non-metal, liquid as well as gas at the room temperature 28 The increasing order of reactivity among group elements is Li < Na < K < Rb < Cs whereas that among group 17 elements is F > CI > Br > I Explain 29 Write the general outer electronic configuration of s-, p-, d- and f- block elements 30 Assign the position of the element having outer electronic configuration (i) ns2np4 for n = (ii) (n - 1)d2ns2 for n = 4, and (iii) (n - 2) f (n - 1)d1ns2 for n = 6, in the periodic table 31 The first (iH1) and the second (iH2) ionization enthalpies (in kJ mol–1) and the (egH) electron gain enthalpy (in kJ mol–1) of a few elements are given below : Elements H1 H2 eg1H I 520 7300 – 60 II 419 3051 – 48 III 1681 3374 – 328 IV 1008 1846 – 295 V 2372 5251 + 48 VI 738 1451 – 40 Which of the above elements is likely to be : (a) the least reactive element (b) the most reactive metal (c) the most reactive non-metal (d) the least reactive non-metal (e) the metal which can form a stable binary halide of the formula MX2(X = halogen) (f) the metal which can form a predominantly stable covalent halide of the formula MX (X = halogen)? ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 26 32 Predict the formulas of the stable binary compounds that would be formed by the combination of the following pairs of elements (a) Lithium and oxygen (b) Magnesium and nitrogen (c) Aluminium and iodine (d) Silicon and oxygen (e) Phosphorus and fluorine (f) Element 71 and fluorine 33 In the modern periodic table, the period indicates the value of : (a) atomic number (b) atomic mass (c) principal quantum number (d) azimuthal quantum number 34 Which of the following statements related to the modern periodic table is incorrect? (a) The p-block has columns, because a maximum of electrons can occupy all the orbitals in a p-shell (b) The d-block has columns, because a maximum of electrons can occupy all the orbitals in a d-subshell (c) Each block contains a number of columns equal to the number of electrons that can occupy that subshell (d) The block indicates value of azimuthal quantum number () for the last subshell that received electrons in building up the electronic configuration 35 Anything that influences the valence electrons will affect the chemistry of the element Which one of the following factors does not affect the valence shell? (a) Valence principal quantum number (n) (b) Nuclear charge (Z ) (c) Nuclear mass (d) Number of core electrons 36 The size of isoelectronic species : F–, Ne and Na+ is affected by : (a) nuclear charge (Z) (b) valence principal quantum number (n) (c) electron-electron interaction in the outer orbitals (d) none of the factors because their size is the same 37 Which one of the following statements is incorrect in relation to ionization enthalpy? (a) Ionization enthalpy increases for each successive electron (b) The greatest increase in ionization enthalpy is experienced on removal of electron from core noble gas configuration (c) End of valence electrons is marked by a big jump in ionization enthalpy (d) Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value 38 Considering the elements B, Al, Mg, and K, the correct order of their metallic character is : (a) B > Al > Mg > K (b) Al > Mg > B > K (c) Mg > Al > K > B (d) K > Mg > Al > B 39 Considering the elements B, C, N, F, and Si, the correct order of their non-metallic character is : (a) B > C > Si > N > F (b) Si > C > B > N > F (c) F > N > C > B > Si (d) F > N > C > Si > B 40 Considering the elements F, Cl, O and N the correct order of their chemical reactivity in terms of oxidizing property is : (a) F > Cl > O > N (b) F > O > Cl > N (c) Cl > F > O > N (d) O > F > N > Cl ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 27 Exercise-1 PART - I A-1 (A) A-2 (C) A-3 (C) A-4 (D) A-5 (C) A-6 (A) A-7 (A)* A-8 A-15 B-1 B-8 C-3 C-10 C-17 (C) (D) (D) (B) (B) (A) (A) A-9 A-16 B-2 B-9 C-4 C-11 C-18 (A) (C) (B) (C) (D) (C) (C) A-10 A-17 B-3 B-10 C-5 C-12 D-1 (A) (A) (C) (B) (B) (C) (A) A-11 A-18 B-4 B-11 C-6 C-13 D-2 (A) (C) (D) (B) (B) (C) (B) A-12 A-19 B-5 B-12 C-7 C-14 D-3 (C) (A) (D) (C) (C) (C) (C) A-13 A-20 B-6 C-1 C-8 C-15 D-4 (B) (C) (B) (C) (D) (B) (A) A-14 A-21 B-7 C-2 C-9 C-16 D-5 (C) (B) (B) (D) (C) (A) (B) D-6 (D) D-7 (D) D-8 (D) D-9 (B) D-10 (A) (C) (B) (C) 26 (A) PART - II (B) (D) 12 14 16 18 20 27 (D) (A) 10 (A) q ; (B) s, t ; (C) r ; (D) p (A) s ; (B) q ; (C) p ; (D) r (A) q ; (B) p ; (C) s ; (D) r (A) r ; (B) s ; (C) p ; (D) q (C) 21 (A) 22 (A) 28 T 29 (C) (A) (B) 11 13 15 17 19 23 30 (A) s ; (B) r; (C) p (D) q (A) t ; (B) q, t ; (C) s ; (D) p, r, s (A) r ; (B) s ; (C) q ; (D) p (A) q ; (B) s ; (C) p ; (D) r (A) r ; (B) (s) ; (C) p, q ; (D) q (A) 24 (C) 25 (C) T 31 F 32 F (C) T Exercise-2 PART - I (B) (D) (C) (D) (D) (B) (C) (D) (A) 10 (D) 11 (B) 12 (A) 13 (A) 14 (A) 15 (D) 16 (A) 17 (D) 18 (C) 19 (A) 20 (B) 21 (A) 22 29 36 43 50 57 64 70 76 (A) 23 (A) 30 (C) 37 (B) 44 (A) 51 (D) 58 (A) 65 (ABCD) 71 (AB) 77 (A) (B) (B) (C) (C) (A) (D) (AC) (AB) 24 31 38 45 52 59 66 72 (A) (B) (D) (A) (A) (A) (ABD) (AB) 25 32 39 46 53 60 67 73 (C) (B) (B) (A) (C) (A) (BCD) (AC) 26 33 40 47 54 61 68 74 (C) (D) (B) (C) (D) (A) (CD) (AD) 27 34 41 48 55 62 69 75 (B) (A) (B) (B) (B) (C) (AB) (AC) 28 35 42 49 56 63 (C) (D) (D) (C) (D) (C) PART - II Out of these, elements A and B will belong to the same group of the periodic table because they have same outer electronic configuration, ns np1 (a) The electronic configuration of element X is [Rn]86 5f 14 6d107s (b) It belongs to d-block as last electron enters in d subshell (c) As number of electrons in (n – 1)d subshell and valence shell is equal to twelve i.e 10 + So it belongs to group 12 (d) It belongs to period of the periodic table as principal quantum number of valence shell is (i.e., 7s 2) 4.25 C–X bond length = 18 Å 76.4% (a) O is having smallest radius Anion is larger than its parent atom Also the anion of the same atom with higher negative charge is bigger in size as compared to anion with smaller negative charge as proton to electron ratio decreases thus attraction between valence shell electrons and nucleus decreases Hence electron cloud expands (b) The ionic radius decreases as more electrons are ionized off that is as the valency increases So the correct order is P5+ < P4+ < P3+ ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 28 10 11 12 13 14 15 16 17 18 19 Mg2+ and O2– both are isoelectronic i.e., have same number of electrons But Mg2+ having 12 protons in its nucleus exerts higher effective nuclear charge than O2– having protons and thus valence shell as well as inner shells electrons are more strongly attracted by the nucleus in Mg2+ resulting smaller size than O2– (a) Fluorine (F) has the largest ionization enthalpy because in moving from left to right in a period, atomic size decreases and electrons are held more tightly Since F has the smallest size and maximum nuclear charge It has the largest ionization enthalpy among these elements (b) Argon (Ar) has the largest ionization enthalpy as argon has extra stable fully filled configuration 1.0943 kJ Order of increasing negative electron gain enthalpy is N < P < O < S For detail refer text The valence shell electronic configuration of halogens is ns2np5 and thus they require one electron to acquire the stable noble gas configuration ns2np6 Because of this they have strong tendency to accept an additional electron and hence have high electron gain enthalpies –3.12 The electron configurations of Li and Be are [He]2s1 and [He]2s2, respectively The additional electron enters the 2s orbital of Li but the 2p orbital of Be and hence is much less tightly bound In fact, the nuclear charge is so well shielded in Be that electron gain is endothermic 2.5 The basic nature of hydroxides of elements of group 1st increases on descending the group with increase in size of cation as CsOH > RbOH > KOH > NaOH > LiOH Al2O3 < SiO2 < P2O3 < SO2 Electron configuration of M2+ is : [Ar]18 4s0 3d4  Electron configuration of M is : [Ar]18 4s1 3d5 (and not 4s2 3d4) So total number of electrons = 24 Hence, metal M is chromium (Cr) 22 (i) p-block (ii) d-block (iii) s-block (iv) s-block As last electron enters in d-subshell, therefore this belongs to d-block For d-block element the group number is equal to the number of valence shell electrons + number of electrons in (n-1) d-subshell So, group number = + = Be2+ < Mg2+ < Na+ < Cl– < S2– < Br– (a) non-metal(III) – Due to highest ionisation energy, (IE1) and (IE2) (b) alkali metal (I) – Due to lowest ionisation energy, (IE1) and there is quite high jump in (IE2) due to inert gas configuration (c) alkaline earth metal (II) – There is little difference in (IE1) and (IE2) and the value of (IE1) is slightly greater than(I) due to stable configuration(ns2) P = 3.726 23 BeO is amphoteric and reacts with acids and bases forming salts 20 21 CO is neutral as it is neutral towards litmus Na2O is basic and dissolves in water forming base (NaOH) 24 N2O5 is acidic and dissolves in water forming acid (HNO3) The general valence shell electron configuration of alkaline earth metals is ns2 (stable configuration) The extra electron must enter np subshell, which is effectively shielding by the two ns electrons and the inner electrons Consequently, the alkaline earth metals have little or no tendency to pick up an extra electron Exercise-3 PART - I 15 (C) (A) (B) 16 (A) (A) (A) 10 (A) (D) 11 (B) (B) 12 (A) (B) 13 (C) (B) 14 (C) (A) 14 (3) (3) PART - II (1) (1) (2) (4) 10 (2) (1) 11 (2) (2) 12 (1) (1) 13 (1) (4) 15 (3) 16 (4) 17 (3) 18 (2) 19 (3) 20 (2) ETOOS ACADEMY Pvt Ltd F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor, BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel : +91-744-242-5022, 92-14-233303 PERIODIC TABLE & PERIODICITY ADVANCED # 29