This PDF is the Sample PDF taken from our Comprehensive Study Material for NEET & AIIMS To purchase the books, go through the link below- http://www.etoosindia.com/smartmall/bookList.do ETOOS Comprehensive Study Material For NEET & AIIMS 08 CHAPTER PERIODIC TABLE If you memorize the periodic table it will speed you up if you're a chem- ist, but by and large, the reason you have a periodic table is so that you can store that information outside of your body. That way it frees up some part of your brain to do something else. “BILL NYE” INTRODUCTION T he chapter gives an insight to the contribution made by different scientists to ar- range the known elements in a manner which could be smooth and informative and the elements properties could justify its position. Thus what we see in the form of modern periodic table today follow a logical sequence of electronic configuration capable enough to explain the trend in physical and chemical properties of the ele- ments. At present 118 elements are known. of them, the recently discovered elements are man made. Efforts to synthesise new elements are continuing. With such a large number of elements it is very difficult to study individually the chemistry of all these elements and their innumerable compounds individually. To ease out this problem, scientists searched for a systematic way to organise their knowledge by classifying the elements. PHYSICS FOR NEET & AIIMS (a) Along a period acidic nature increases. (b) Down the group basic nature increases Li Be B C N O F Na Mg Al Si P S Cl  X – X > 2.3 X – X = 2.3 X – X < 2.3 A O A O A O Basic Amphoteric Acidic ie. when in periodic table the distance between the element and oxygen increases, basic character increases. NO > ZnO > KO 2 2  acidic character decreases ETOOS KEY POINTS Note: BeO, AlO, ZnO, SnO, PbO, SnO, PbO, SbO etc. are amphoteric oxides. 2 3 2 2 2 3 CO, HO, NO, NO etc. are neutral oxides. 2 2 Acidic strength of oxide and oxyacid  Electronegativity BO CO NO 2 3 2 2 5  EN increase, acidic nature increasse. SO SeO TeO HNO H CO  H BO HClO > HBrO > HIO 3 3 3 3 2 3 3 3 4 4 4 H SO H SeO H TeO H PO > H AsO > H SbO N O > P O > As O 2 4 2 4 2 4 3 4 3 4 3 4 2 5 2 5 2 5 H SO H SeO H TeO HOF > HOCl > HOBr > HOI N O > P O > As O > Sb O 2 3 2 3 2 3 2 3 2 3 2 3 2 3 Acidic nature oxidation state Acidic properties increases with increasing oxidation state of an element HClO > HClO > HClO > HClO HNO > HNO 4 3 2 3 2 HSO > HSO NO > NO 2 4 2 3 2 5 2 3 SO > SO SbO > SbO 3 2 2 5 2 3 (I) Hydrolysis of AX : Where A = Other element and X = Halogen (a) If electronegativity of X > Electronegativity of A then on hydrolysis product will be HX. Ex. (BCl), Electronegativity of Cl > Electronegativity of B 3 Cl H OH B Cl + H OH 3HCl + B(OH) Cl H OH 3 PCl + 3HOH  3HCl + HPO 3 3 3 PCl. Cl + HO  2HCl + POCl 3 2 2 3 POCl + 3HOH  3HCl + HPO 3 3 4 (b) If electronegativity of X < electronegativity of A then on hydrolysis product will be HOX (hypohalous acid) Cl Ex. ClO O Here electronegativity of O > Cl 2 Cl So On hydrolysis – Cl HO– H+ O + 2HOCl + HO Cl HO– H+ 2 etoosindia.com 27 India’s No. 1 Online Coaching Institute IIT-JEE | PRE-MEDICAL | CBSE | FOUNDATION PERIODIC TABLE important facts to remember 1. Lowest electronegativity : Cs 2. Highest electronegativity : F 3. Highest ionisation potential : He 4. Lowest ionisation potential : Cs 5. Lowest electron affinity : Noble gases 6. Highest electron affinity : Chlorine 7. Least electropositive element : F 8. Lowest m. pt. metal : Hg 9. Highest m. pt. and b. pt. metal : W (Tungsten) 10. Lowest m. pt. and b. pt. non metal : He 11. Notorious element : Hydrogen 12. Lightest element : Hydrogen 13. Smallest atomic size : H 14. Largest atomic size : Cs 15. Largest anionic size : I– 16. Smallest cation : H+ 17. Most electropositive element : Cs 18. Element with electronegativity next to Fluorine : Oxygen 19. Group containing maximum no. of gaseous elements in periodic table : Zero group 20. Total number of gaseous elements : in periodic table : 11 (H, N, O, F, Cl, He, Ne, Ar, Kr, Xe, Rn) 21. Total number of liquid elements in periodic table : 6 (Ga, Br, Cs, Hg, Fr, Uub) 22. Liquid element of radioactive nature : Fr 23. Total number of radioactive elements in periodic table : 25 24. Volatile d block elements : Zn, Cd, Hg, Uub 25. Element containing no neutron : H 26. Most abundant element on earth : Oxygen 27. Most abundant metal on earth : Al 28. Element having maximum tendency for catenation : Carbon 29. Non metal having highest m. pt., b.pt. : Carbon (dimond) 30. Metals showing highest oxidation number : Os (+8), Ru 31. Most electrovalent compound : CsF 32. Most stable carbonate : CsCO 2 3 32 etoosindia.com Study with Best Etoos Faculties of Kota IIT-JEE | PRE-MEDICAL | CBSE | FOUNDATION PERIODIC TABLE SOLVED EXAMPLE Ex. 1 Following are the valence shell electronic Ex. 5 In Column-I, there are given electronic configurations of some elements. configurations of some elements. Match these (i)3s2 3p5 (ii)3d10 4s2 with the correct metals given in Column-II : (iii)2s2 3p6 4s1 (iv) 1s2 2s2 Column-I Column-II Find out the blocks to which they belong in the (A) ns2, np5 (p) Chromium periodic table ? (B) (n – 1) d10 , ns1 (q) Copper Ans. (i) p-block (ii) d-block (iii)s-block (iv) s-block (C) (n – 1) d5 , ns1 (r) Krypton Sol. The block of the elements depend on the type of (D) (n – 1) d10 , ns2 , np6 (s) Bromine sub-shell which receive the last electron. In case of Ans. (A)  (s) ; (B)  (q) ; (C) (p) ; (D) (r). (i) it enters in 3p-subshell, Sol. (A) ns2np5 is general valence shell electron (ii) z it enters 3d-subshell, configuration of halogens. So this configuration (iii)it enters 4s-subshell and belongs to bromine. (iv) it enters 2s-subshell. (B) (n – 1) d1-10 ns1-2 ; This is electron configuration Ex. 2. A M2+ ion derived from a metal in the first transition of d-block elements. As it contains (n – 1) d10ns1 metal series has four electrons in 3d subshell. What configuration it belongs to copper. element might M be ? (C) (n – 1) d1-10 ns1-2 ; This is electron configuration Ans. Chromium of d-block elements. As it contains (n – 1) d5 ns1 Sol. Electron configuration of M2+ is configuration it belongs to chromium. [Ar]18 4s0 3d4 (D) Noble gases has valence shell electron  Electron configuration of M is configuration ns2 np6, so it belongs to krypton. [Ar]18 4s1 3d5 (and not 4s2 3d4) So total number of electrons = 24. Ex. 6 Match the metals given in Column-II with their Hence, metal M is chromium (Cr). type given in Column-I : Column-I Column-II Ex. 3 Find out the group of the element having the electronic configuration, 1s2 2s2 2p6 3s2 3p6 3d6 (A) Metalloid (p) Sulphur 4s2 . (B) Radioactive (q) Gold Ans. As last electron enters in d-subshell, therefore (C) Transition metal (r) Arsenic this belongs to d-block. For d-block element the group number is equal to the number of valence (D) Chalcogen (s) Uranium shell electrons + number of electrons in (n-1) d- Ans. (A)  (r) ; (B)  (s) ; (C) (q) ; (D) (p) subshell. Sol. (A) Arsenic is a metalloid because it behaves as So, group number = 6 + 2 = 8. metal (forming cation, As3+ -AsCl ) as well as 3 Ex. 4 Arrange the following ions in the increasing order nonmetal (forming anion, As3– -AsH). 3 of their size : Be2+ , Cl–, S2– , Na+ , Mg2+ , Br– ? (B) Uranium is a radioactive element. Ans. Be2+ < Mg2+ < Na+ < Cl– < S2– < Br– (C) Those elements which in their neutral atoms or Sol. Be2+ is smaller than Mg2+ as Be2+ has one shell in most common oxidation state have partially filled where as Mg2+ has two shells. d-orbitals are called as transition elements. Gold in Mg2+ and Na+ are isoelectronic species : Ionic its +3 oxidation state has electron configuration radius  1/nuclear charge. [Xe]54, 5d86s0 . Cl– and S2– are isoelectronic species : Ionic radius (D)16th group elements like oxygen and sulphur are  1/nuclear charge. ore forming elements and therefore are called as Cl– is smaller than Br– as Cl– has three shells chalcogens. where as Br– has four shells. etoosindia.com 35 Study with Best Etoos Faculties of Kota IIT-JEE | PRE-MEDICAL | CBSE | FOUNDATION PHYSICS FOR NEET & AIIMS Exercise # 1 SINGLE OBJECTIVE NEET LEVEL 1. Which of the following statement is not correct for 11. Which cation has smallest radius the element having electronic configuration (A) K+ (B) Na+ 1s2,2s2p6,3s1 (C) Li+ (D) Be2+ (A)It is a monovalent electropositive 12. The radii of F, F–, O and O–2 are in the order of (B) It forms basic oxide (A) O2 F OF (B) O2 F FO (C) It is a non-metal (D) It has low electron affinity (C) F O2 FO (D) O2 OF F 2. Which of these dose not reflect the periodicity of 13. Which of the following has the smallest size the elements (A) Na+ (B) Mg+2 (A) Bonding behaviour (B) Electronegativity (C) Cl– (D) F– (C) Ionization energy (D) Neutron/proton ratio 14. Which of the following is largest 3. If an atom has electronic configuration (A) Cl– (B) S2– 1s22s22p63s23p63d34s2, it will be placed in (C) Na+ (D) F– (A)Second group (B) Third group 15. Which of the following property displays (C) Fifth group (D) Sixth group progressive increase down a group in the Bohr's periodic table 4. All the s-block elements of the periodic table are (A) Electronegativity (B) Electron affinity placed in the groups … (A) IA and IIA (B) IIIA and IVA (C) Ionization potential (D) Size of the atom (C)B sub groups (D) VA to VIIA 16. Atomic radii of fluorine and neon in angstrom units 5. The electronic configuration of halogen is are respectively given by (A) ns2np6 (B) ns2np3 (A) 0.762, 1.60 (C) ns2np5 (D) ns2 (B) 1.60, 1.60 (C) 0.72, 0.72 6. The ratio between radii of He+ ion and H atom is (D)None of these values 1 (A) (B) 1 17. Which ion has greatest radius in the following 2 (A) H– (B) F– 3 (C) Br– (D) I– (C) (D) 2 2 18. Which has the maximum atomic radius 7. The smallest among the following ions is (A) Al (B) Si (A) Na+ (B) Mg2+ (C) P (D) Mg (C) Ba2+ (D) Al3+ 19. Which one of the following ions has the highest 8. Which is smallest in size value of ionic radius (A) O2– (B) C4– (A) O2– (B) B3+ (C) F– (D) N3– (C) Li+ (D) F– 9. Which of the following has largest size 20. On going down a main sub-group in the periodic table (example Li to Cs in IA or Be to Ra in IIA), the (A) Al (B) Al+ expected trend of changes in atomic radius is a (C) Al+2 (D) Al+3 (A) Continuous increase 10. Of the following, the one with largest size is (B)Continuous decrease (A) Cl– (B) Ar (C) Periodic one, an increase followed by a decrease (C) K+ (D) Ca2+ (D) A decrease followed by increase 38 etoosindia.com India’s No. 1 Online Coaching Institute IIT-JEE | PRE-MEDICAL | CBSE | FOUNDATION PERIODIC TABLE Exercise # 2 SINGLE OBJECTIVE AIIMS LEVEL 1. Atomic number of Ag is 47. In the same group, the 9. Match the correct atomic radius with the element : atomic numbers of elements placed above and S.No. Element Code Atomic radius (pm) below Ag in Long form of periodic table will be : (i) Be (p) 74 (A) 29, 65 (B) 39, 79 (ii) C (q) 88 (C) 29, 79 (D) 39, 65 (iii) O (r) 111 2. Element with electronic configuration as [Ar] 3d5 (iv) B (s) 77 (v) N (t) 66 4s1 is placed in ___ in Modern periodic table : (A) (i) – r, (ii) – q, (iii) – t, (iv) – s, (v) – p (A) IA (1st group), s-block (B) (i) – t, (ii) – s, (iii) – r, (iv) – p, (v) – q (B)IB (7th group), d-block (C) (i) – r, (ii) – s, (iii) – t, (iv) – q, (v) – p (C) VIB (8th group), d-block (D) (i) – t, (ii) – p, (iii) – r, (iv) – s, (v) – q (D) VIB (6th group), d-block 10. Select correct statement(s) about radius of an atom: 3. In modern periodic table, the element with atomic (A)Values of Vander waal's radii are larger than number Z = 118 will be : those of covalent radii because the Vander waal's forces are much weaker than the forces (A) Uuo ; Ununoctium ; alkaline earth metal operating between atoms in a covalently (B) Uno ; Unniloctium ; transition metal bonded molecule. (C) Uno ; Unniloctium ; alkali metal (B) The metallic radii are smaller than the Vander (D) Uuo ; Ununoctium ; noble gas waal's radii, since the bonding forces in the metallic crystal lattice are much stronger than 4. Which of the following is not an actinoid : the Vander waal's forces. (A) Curium (Z = 96) (B) Californium (Z = 98) (C) Both (A) & (B) (C) Uranium (Z = 92) (D) Terbium (Z = 65) (D)None of these 5. Which of the following statements is not correct 11. Which of the following order of atomic / ionic radius regarding hydrogen : is not correct ? (A) It resembles halogens in some properties. (A) F < Cl < Br <  (B) Y3+ > Sr2+ > Rb+ (B) It resembles alkali metals in some properties. (C) Nb  Ta (D) Li > Be > B (C) It can be placed in 17th group of Modern periodic table. 12. The size of isoelectronic species F–, Ne and Na+ is (D) It cannot be placed in 1st group of Modern affected by : (A) nuclear charge (Z) periodic table. (B) valence principal quantum number (n) 6. The order of screening effect of electrons of s, p, d and (C) electron-electron interaction in the outer orbitals f orbitals of a given shell of an atom on its outer shell (D) none of the factors because their size is the electrons is same. (A) s > p > d > f (B) f > d > p > s 13. Which of the following order of radii is correct : (C) p < d < s > f (D) f > p > s > d (A) Li < Be < Mg (B) H+ < Li+ < H– 7. Which of the following is/are generally true (C) O < F < Ne (D) Li < Na < K < Cs < Rb regarding effective nuclear charge (Z ) : eff 14. Which one of the following statements is incorrect (A) It increases on moving left to right in a period. in relation to ionisation enthalpy ? (B) It remains almost constant on moving top to (A) Ionization enthalpy increases for each bottom in a group. successive electron. (C) For isoelectronic species, as Z increases, Z (B)The greatest increase in ionization enthalpy is eff decreases. experienced on removal of electron from core (D) Both (A) and (B). of noble gas configuration. (C) End of valence electrons is marked by a big 8. Which of the following is the correct order of size of jump in ionization enthalpy. the given species : (D) Removal of electron from orbitals bearing lower (A)I > I– > I+ (B)I+ > I– > I n value is easier than from orbitals having higher (C)I > I+ > I– (D)I– > I > I+ n value. 42 etoosindia.com Study with Best Etoos Faculties of Kota IIT-JEE | PRE-MEDICAL | CBSE | FOUNDATION PHYSICS FOR NEET & AIIMS Exercise # 3 PART - 1 MATRIX MATCH COLUMN 1. Match the electronic configurations of the elements given in column-(I) with their correct characteristic(s) ( i.e. properties for given configuration) given in column-(II). Column-I Column-II (A) 1s2 (p) Element shows highest negative oxidation state. (B) 1s2 2s2 2p5 (q) Element shows highest first ionisation enthalpy. (C)1s2 2s2 2p6 3s2 3p5 (r)Element shows highest electronegativity on Pauling scale. (D) 1s2 2s2 2p2 (s) Element shows maximum electron gain enthalpy (most exothermic). 2. Match Column–I (atomic number of elements) withColumn–II (position of element in periodic table) and select the correct answer using the codes given below : Column-I Column-II (A) 19 (p) p-block (B) 22 (q) f-block (C) 32 (r) d-block (D) 64 (s) s-block 3. Match the species/elements listed in column I with their characteristic listed in column II. Column I Column II (A) SO, NO–3, CO–2 (p) Semi-metals 2 3 (B) Ge, As, Sb (q) Inert gases (C) Ar, Kr, Xe (r)Isoelectronic species (D) Ca, Sr, Ba (s) Alkaline earth metals 4. Match the values of ionization energy and electron gain enthalpi listed in column I with characteristic(s) of elements listed in column II. Column I Column II H , H ,  H(in kJ mol–1) , 1 1 1 2 eg (A) 2372 5251 +48 (p) Elements which acts as a strong reducing agent (B) 419 3051 -48 (q) Elements which exists as a monoatomic molecule (C) 1681 3374 -333 (r) Least reactive non-metal (D) 1008 1846 -295 (s)Elements which acts as a strong oxidising agent (t) Element which oxide is a stronger basic in nature 46 etoosindia.com India’s No. 1 Online Coaching Institute IIT-JEE | PRE-MEDICAL | CBSE | FOUNDATION PERIODIC TABLE Exercise # 4 PART - 1 PREVIOUS YEAR (NEET/AIPMT) 1. Correct order of Ist ionisation potential (IP) among 7. Which of the following electronic configuration of following elements Be, B, C, N, O is an atom has the lowest ionisation enthalpy ? [CBSE AIPMT 2001] [CBSE AIPMT 2007] (A) B < Be < C < O < N (A) 1s2, 2s22p5 (B) 1s2, 2s22p3 (B) B < Be < C < N < O (C) 1s2, 2s22p5, 3s1 (D) 1s2, 2s22p6 (C) Be < B < C < N < O 8. The correct order of decreasing second ionisation (D) Be < B < C < O < N enthalpy of Ti(22), Cr(24) and Mn(25) is 2. An atom has electronic configuration 1s2, 2s22p6, [CBSE AIPMT 2008] 3s23p63d3, 4s2, you will place it in (A) Cr > Mn > V > Ti [CBSE AIPMT 2002] (B) V > Mn > Cr > Ti (A) fifth group (C) Mn > Cr > Ti > V (B) fifteenth group (D) Ti > V > Cr > Mn (C)second group 9. Which of the following oxides is not expected to (D) third group react with sodium hydroxide? 3. Which of the following order is wrong ? [CBSE AIPMT 2009] [CBSE AIPMT 2002] (A) BO (B) CaO 2 3 (A)NH < PH < AsH – Acidic (C) SiO (D) BaO 3 3 3 2 (B) Li < Be < B < C – 1st Ionisation potential 10. Which one of the elements with the following outer (C) AlO < MgO < NaO < KO – Baisc 2 3 2 2 orbital configurations may exhibit the largest number (D)Li+ < Na+ < K+ < Cs+ – Ionic radius of oxidation states? [CBSE AIPMT 2009] 4. The ions O2–, F–, Na+ Mg2+ and Al3+ are isoelectronic. (A) 3d3, 4s2 (B) 3d5, 4s1 Their ionic radii show (C) 3d5, 4s2 (D) 3d2, 4s2 [CBSE AIPMT 2003] 11. Amongst the elements with following electronic (A) an increase from O2– to F– and then decrease configurations, which one may have the highest from Na+ to Al3+ ionisation energy ? [CBSE AIPMT 2009] (B) a decrease from O2– to F– and then increase (A) [Ne] 3s23p3 (B) [Ne] 3s23p2 from Na+ to Al3+ (C) [Ar] 3d10, 4s2 4p3 (D) [Ne] 3s2 3p1 (C) a significant increase from O2– to Al3+ (D) a significant decrease from O2– to Al3+ 12. Which of the following represents the correct order of increasing electron gain enthalpy with negative 5. Ionic radii are [CBSE AIPMT 2004] sign for the elements O, S, F and Cl? (A) inversely proportional to effective nuclear [CBSE AIPMT 2010] charge (A) Cl < F < O < S (B) inversely proportional to square of effective nuclear charge (B) O < S < F < Cl (C) directly proportional to effective nuclear charge (C) F < S < O < Cl (D) directly proportional to square of effective (D) S < O < Cl < F nuclear charge 13. The correct order of the decreasing ionic radii among 6. Identify the correct order of the size of the following. the following isoelectronic species is [CBSE AIPMT 2007] [CBSE AIPMT 2010] (A)Ca2+ < K+ < Ar < S2– < Cl– (A) Ca2+ > K+ > S2– > Cl– (B)Ca2+ < K+ < Ar < Cl– < S2– (B)Cl– > S2– > Ca2+ > K+ (C) Ar < Ca2+ < K+ < Cl– < S2– (C) S2– > Cl– > K+ > Ca2+ (D)Ca2+ < Ar < K+ < Cl– < S2– (D) K+ > Ca2+ > Cl– > S2– 48 etoosindia.com Study with Best Etoos Faculties of Kota IIT-JEE | PRE-MEDICAL | CBSE | FOUNDATION PHYSICS FOR NEET & AIIMS MOCK TEST STRAIGHT OBJECTIVE TYPE 1. Consider the following statements; (I)Rutherford name was associated with the developement of periodic table. (II) A metal M having electronic configuration 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s1 is d-block element. (III) Diamond is not an element. (IV) The electronic configuration of the most electronegative element is 1s2, 2s2, 2p5, and select the correct one from the given codes. (A) I, II, IV (B) I, II, III, IV (C) II, IV (D) I, III, IV 2. The correct order of second ionisation potential of carbon, nitrogen, oxygen and flourine is : (A) C > N > O > F (B) O > N > F > C (C) O > F > N > C (D) F > O > N > C 3. The electron gain enthalpies of halogens in kJ/mol are as given below. F = –332, Cl = –349, Br = –324, I = –295 The less negative value for F as compared to that of Cl is due to : (A)strong electron-electron repulsions in the compact 2p-subshell of F. (B) weak electron-electron repulsions in the compact 2p- subshell of Cl (C) smaller electronegativity value of F than Cl (D)(A) and (B) both 4. Which of the following statement is not correct ? (A) The first ionisation energies (in kJ/mol) of carbon, silicon, germaniu, tin and lead are 1086, 786, 761, 708 and 715 respectively. (B) Down the group, electronegativity decreases from B to Tl in boron family. (C) Among oxides of the elements of carbon family, CO is neutraql, GeO is acidic and SnO is amphoteric. (D) The 4f- and 5f- inner transition elements are placed separately at the bottom of the periodic table to maintain its structure. 5. Which of the following order is correct ? (A) F > N > C > Si > Ga – non-metallic character. (B) F > Cl > O > N – oxidising property. (C) C < Si > P > N – electron affinity value. (D) All of these. 6. If the same element is forming oxides in different oxidation state then : (A) that oxide will be neutral in nature in which element will be in its highest oxidation state. (B) that oxide will be highest acidic in nature in which element will be in the highest oxidation state. (C) that oxide will be amphoteric in nature in which element will be in the highest oxidation state. (D) that oxide will be higly basic in nature in which element will be in the highest oxidation state. 7. What will be the order of Ist ionisation energy (A) Li > Na > K (B) K > Li > Na (C) Na > Li > K (D) Li > K > Na 8. Which of the following configurations represents atoms of the elements having the highest second ionization energy (A)1s22s22p4 (B)1s22s22p6 (C)1s22s22p63s1 (D)1s22s22p63s2 9. The first ionization potentials in electron volts of nitrogen and oxygen atoms are respectively given by (A) 14.6, 13.6 (B) 13.6, 14.6 (C) 13.6, 13.6 (D) 14.6, 14.6 10. The elements which occupy the peaks of ionisation energy curve, are (A) Na,K, Rb,Cs (B) Na, Mg,Cl,I (C) Cl, Br,I,F (D) He, Ne,Ar,Kr etoosindia.com 51 India’s No. 1 Online Coaching Institute IIT-JEE | PRE-MEDICAL | CBSE | FOUNDATION