Periodic Properties (Booklet Solution)

Periodic Properties (Booklet Solution) Foundation Builders (Objective). (B) Law of triads states that in the set of three elements arranged in increasing order of atomic weight, having similar properties, the atomic weight of middle element is the arithmetic mean of other two.. (C) Transition elements are those in which electron are filled in d orbitals. 3. (D) P block elements are also known as representative element. 4. (A) Covalent radii < crystal radii < vanderwaal radii. 5. (B) Noble gases are placed in zero group but has or 3 electrons in its valence shell. 6. (B) N 4e &CO 4e 7. (C) Fact 8. (C) Fourth period of periodic table has 3d electron filling, not 4d. 9. (D) Fe + has 4 unpaired electron. 0. (B) For compound to be coloured either cation or anion has unpaired electron. Cu : Ar 3d 9 9. (D) C & N + has 6 electrons in it.. (B) All the species has 4e in it. 3. (B) For iso electronic species, more negatively charged ion is more bigger in. 4. (C) Same as above. 5. (B) Same as above. 6. (D) For same atom more positive charged species is smaller one. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI #

7. (B) For an isoelectronic species, negatively charged species is more bigger than positively charged species. 8. (A) More is the P/e ratio smaller is the radius. 9. (B) r Na r F r Cl r r F Cl r S r r r r Na F Cl S 0. (B) Across a period, as Zeff increases. Atomic radii decreases.. (A) For isoelectronic species Radius of cation < radius of neutral Atom < radius of anion. (C) For same atom r r r cation atom anion 3. (A) Na > Mg (Across a period decreases) Na > Na + Mg > Mg + 4. (B) For an isoelectronic species, more positive charged ion, smaller in the. More is the negative charge on anion, more is the. 5. (D) Li Na K Be Mg Al 6. (C) Ionisation energy But in a period stable configuration is preferred as change is not very significant. 7. (B) Mg Mg e Mg mg e Mg Mg e H P 78kcal mol H P 348 kcal mol H H H = 78 + 348 CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI #

= 56 kcal mol 8. (B) P 5 is very high i.e removal of 5 th electron is very difficult. If means after removal of 4e species has acquired very stable configuration. 9. (B) I.E I.E I.E... I.E I.E n n n 30. (B) I.E for electron is 3P > 4P 3P 3 is half filled than p & p 3. (B) Mg Mg e I.E Mg,8,,8 Na Na e I.E Na,8,7 Inert gas configuration. I.E Na I.E Mg 3. (A) Electronegativity Ionisation Energy I. E is less for left side, metal as their is more, so they are more reactive. down the group. I. E decreases & hence reducing power decreases. 33. (C) B :S S P 34. (B) If I.E 5 4Be :S S : Full filled configuration is more stable. I.E > 6ev / atom, then lower oxidation state is more stable. 35. (D) For isoelectronic species, I.E S has maximum ionic radii & hence lowest I.E. 36. (C) I.E of Na is between Li & K. It I. E will also be in between the I.E. value of Li & K. 37. (C) I.E. increases tremendously when no. of reduces. I.E 4 >>> I.E 3, means valence electron is 3 CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 3

38. (A) Na Na e H I.E 39. (C) Na Na e Na H E.A H H 40. (A) e O O Heg ve e O O H eg ve e O O Heg ve total H eg Na for all element is positive. 0 N E.A E.A Repulsion offered to incoming O N e in 3P orbital will be very less as compared to P orbital. 4. (D) Negative anion species will repel incoming electron due to same charge repulsion. 4. (B) Be is more stable due to fulfilled as subshell. Be is formed over coming this stability, so more energy is taken by Be. Hence it is least stable. 43. (C) Electron affinity (E. A) E. A depends on repulsion to incoming electron mainly. E. A electronegativity 44. (B) Refer 39 45. (B) In C, electronic repulsion is very high. So EA is very less. For S & Se, repulsion difference is not significant. S Se S > Se > O 46. (C) In same period E.A electronegativity N < C < O < F 47. (C) Due to high electronegativity (E. A) F > (E. A) Br Fluorine undergo reduction easily than bromine, so it is better oxidizing agent. 48. (C) CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 4

Electronegativity decreases down the group, but decreases is less in case of alkali metal as compared to halogen groups. 49. (B) According to Pauling scale I.E E.A P where I.E & E.A is expressed in ev/atom. 5.6 50. (D) X X.8 m P X P : electronegativity on Pauling scale X m : electronegativity on Mulliken s scale. 5. (C) Electronegativity increases along a period and decreases down the group. 5. (A) X M I.P E.A I.P & E.A in ev/atom. 53. (A) More is the electronegativity difference, more is the ionic character. For same atom, electronegativity 0. 54. (D) charge Hydration energy 55. (A) 56. (D) Electronegativity difference increases, it means acidic strength of different element decreases. 57. (C) Group 3 th element oxides are generally amphoteric. FOUNDATION BUILDER SUBJECTIVE. Electronegativity differences of Mn +7 & O is not very high so Mn O 7 is acidic.. (I. E) K<< (I. E) Ag 3. g e F F Heg ve,7,8 g g e O O Heg ve g g e O O Heg ve H eg H eg e O O Heg ve CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 5

4. Refer diagonal relationship between Li and Mg 5. Due to inert pair effect, 6s electrons come closer to nucleus & hence (I.E) (I.E) >6 ev/atom for T. T is more stable than T 3. 6. Because it can loose n d as well as ns electrons 7. For isoelectronic species, atomic radii of more negatively charged species > neutral atom > cationic species 8. Anionic radii > atomic radii For atomic radii ; vanderwall radii > covalent radii II I III 9. Down the group shielding effect decreases. 0. For isoelectronic species Anion > atom > cation F > Ne > Na +. I.P Na Na Na e Na E.A I.P of Na = E.A of Na +. After first ionization, alkali metals achieves a noble gas configurations so, IP IP. Since it is true for alkaline earth metal after nd ionization. (I.P) 3 >> (I.P) 3. Fully filled subshell is more stable than half filled. 4. Poor shielding effect of 4f subshell. E.A I.P 5. x x x H I.P E.A 409 x x x E.A I.P 73.3 6. C :S S P B :S S P 6C: Zeff for C > B (I. P) for C > (I. P) for B 6C + : S S P 5B + : S S Completely filled S subshell 6 5 CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 6

7. I.P I.P I.P 3 3 4 Be :S S 4Be :S S 4Be :S 4Be :S Inert gas configuration. I.P I.P I.P 3 3 4 Be :S S 4Be :S S 4Be :S 4Be :S Inert gas configuration. 8. Achieving stable configuration on some time Noble gas configuration is the main reason for electron affinity 9. Be has fulfilled s subshell while N has half filled p subshell which are comparatively stable than Be & N 0. Let x gm of Mg converts into Mg x x x Mg Mg H 740 4 4 4 x x x Mg Mg H 740 450 L 4 4 H H 50kJ. x x 740 90 50 4 4 740x 90 90x 00 90x 740x 90 00 450x 990 99 0 x 45 0 x 0.687 % of Mg 0.37 in final mixture 00 3.7%. Na Fg Na g F g g H ev atom H 5.4eV 3.4eV ev atom 9 3.6 0 6.03 0 J mol.60 9 4. 0 45.88 Kcal mol. 6.030 3 3 Kcal mol 38. no. of moles of F ionized 68 38 no. of F atoms ionized N 68 3. In bonding electron of different subshell can participate. A CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 7

Get equipped for JEE Main. (D) Exception to aufbau s principle.. (D) Valency of X is Valency of Y is 3 3. (D) Oxygen group is known as chalcogens. 4. (B) M : Ar 3d 4s 3 0 0 3 M : Ar 3d 4s 4p. 5. (B) 6Fe : Ar 4s 3d 6Fe 6. (B) : Ar 3d 3 5 6 7. (C) Due to inert pair effect 8. (A) w.r.t oxygen halogen family : 7 oxygen family : O Nitrogen family : +5 Boron family : +3 9. (D) Valency of A is 3 Valency of B is compound formed is AB 3. 0. (C) I.E increases from left to right. 3 Bi is more stable as compared to +5 state for others.. (C) Zeff difference between consecutive elements in transition element is less as compared to s & p- block elements. Same is the case with lanthanide series, d orbitals electron offers less shielding effect as compared to s & p-block f orbitals electrons offers less shielding effect as compared to s, p & d block.. (D) Fe Co N ; Increase in effective atomic number is balanced by increase in repulsion between electrons. Ni Cu Zn Increase in zeff is overcomed by electronic repulsion increases. 3. (B) As P/e ratio increase, z eff increases so nd ionization energy is always higher than st I. E. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 8

4. (C) For alkali metal I.E I.E 5. (A) Atomic radius is determining factor for I. E down the group z eff and stable configuration important factor for I. E across period. 6. (B) Smaller of atoms, more is the I. E 7. (B) Hydration energy depends on ch arg e ratio. 8. (A) Metal oxide are basic while non metal oxides are acidic in nature generally. 9. (C) Cr : Ar 3d 4 3 5 6 4 V : Ar 3d 3 Mn : Ar 3d 5 Fe : Ar 3d b. Half-filled d orbitals are more stable than other configuration. 0. (B) More is the no. of unpaired electrons, more is the paramagnetism.. (D) Lawrencium 4 03Lr : Rn 7s 6d 5f.. (C) In a group, atomic number differ by, 8, 8, 8, 3. Etc. 3 (B) Isoelectronic species 4. (B) Li :s 3 4 5 Be :s s B :s s. I.E order Be B Li or Li B Be 5. (C) Difference between (I. E) 6 and (I. E) 7 is very large. So, there is 6e in valence shell of atom at this 6. (A) element. It belongs to th 6 group. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 9

II IV III I Inert gas configuration. Half filled configuration is disturbed subshell is fulfilled 7. (A) Ch arg e Hydrated radius K aq Na aq Li aq 8. (C) q q Lattice energy r R is least for NaF 9. (B) For alkaline, earth metal, 4,, 0, 38, 56, 78, 0. Achievement of inert gas configuration but repulsion is also there as electron is entering in nd shell. 30. (C) Less is electronegativity difference between atoms forming a bond, more is the covalent character. So X X X X, the m O bond break is polar solvent. If m C O H 3. (C) 3 00 Moles of X 7 3 00 Energy required 70kJ 7.3kJ. 3. (A) 33. (B) Cl is more stable than F 34. (B) 35. (C) I.E I.E Cl I.E I.E Cl I.E I.E F Cl F - (I.E) neutral atom > (I. E) anion.. Cl I.E CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 0

36. (B) I.E np I.E ns 37. (A) Electronegativity 38. (B) X X. A B is ionic bond A B <. A B is covalent bond theoretically. Practically X X.7 covalent bond will be formed A B >.7 Ionic bond is formed. 39. (B) According to Mulliken s scale I.E E.A x x Y I.E 40. (B) 4. (D) Hydration energy ch arg e 4. (D) O F isoelectronic species O F along period decreases. 43. (D) Be has maximum charge / ratio 44. (B) 45. (C) Nitrogen has half filled p orbitals. 46. (A) In a period decreases, So I. E increases. Magnesium has completely 3s subshell 47. (B) 48. (C) O 49. (B) e O e S S Incoming electron is repelled by anionic electrons. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI #

Heg is always endothermic Get equipped for JEE Advanced. (ABCD) (A) S is more stable than C (B) E.A E.A S (C) E.A E.A Cl F O As belongs to nitrogen family, so it has half filled subshell.. (BD) Argon (Ar) has stable configuration. 3. (ABCD) Refer theory 4. (ACD) (A) Zeff E.A (CD) I.E. For isoelectronic species r r r. cation atom anion 5. (CD) Zeff 6. (BD) For oxides, if electronegativity difference between elements increases, acid strength of different elements decreases. As positive change on any element increases, electronegativity increases. 7. (ABC) 8. (B) I.E I.E 3 + oxidation state of metal is more stable. 9. (B) Cl has large which results in less electronic repulsion and high electron affinity 0. (A) 3 6 X Ne :s s p.. (A) Refer Q. 6 of this exercise.. (ABCD) Element is made up of single type of atom 5 F :s s p 9 CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI #

3. (ABC) Halogens has most electron gain enthalpy. Alkaline earth metal has oxidation state 4. (ABC) I.E Along period half filled shell stability is considered 5. (B) Compounds of Mn oxidation state of Mn. MnO +4 KMnO +7 4 MnO + As oxidation state increase of atom decreases. 6. (ABCD) I.E Metallic radii > covalent radii 4 3 :s 0. He Due to poor shielding effect of electron in f orbital, is 7. (C) Due to inert pair effect 8. (C) 9. (ABD) Lattice energy Hydration energy 9 9 r ch arg e 0. (ABC) I.E along a period, I. E dereases. I.E I.E Na 4. (A) Ionic mobility Hydrated radius ch arg e Hydrated radius r Nb r Ta. (ABCD) Down the 4 th group, stability +4 oxidation state decreases as + increases. 4 For Pb : Pb Pb 3. (ABD) Refer theory. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 3

4. (A) r r r r x 5. (B) 6. (C) x metallic x covalent x 7. (B) M g 80 Kcal M g e 8. (ABC) Comprehension Type. (D) Metals undergo oxidation easily So I.E should be less.. (D) Non metals undergo reduction easily. So EA should be high. 3. (D) 4. (D) For E (I. E ) is less than others. 5. (A) If difference in two successive Ionisation energy is less than higher oxidation state is more stable. 6. (C) E. A for noble gas is positive. 7. (A) 8. (B) Lanthanides having +3 oxidation states are more stable. 9. (D) Species which undergo reduction easily is very string oxidizing agent. 4 3 Ce e Fe 0. (C) 3 ; ; ; For 0 th Period. (C) 6 7 CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 4

For e in each orbital maximum element in 4 th shell is 8. 8 For 3e in each orbital 3 7 Elements in 4 th shell.. (D) General electronic configuration of outer most shell of f block element is 4 0 n f n d ns 3. (C) For any shell / orbit no. n maximum electron in it is Maximum no. of possible elements in nature n n n n n n n n 6 n n n 3 4. (B) a z b 5. (D) b a z For Li : 4 a 3 b 8 3 0 a 3 b For Na : Na a z b 8 4 0 a b. () () ().. () 8 0 8a 8 a 0 8 3 b b For K 8 0 40 8 6 5 0 Hz 6. (B) E h 6.660 0 7 7.9 0 J. 34 6 7. (D) As electronegativity difference between element increases, acidic strength of oxide is decreases & vice versa for basic strength. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 5 n n.

8. (D) 9. (D) 0. (D) SO is an acidic oxide. Matrix Match:. A s B C K : Ar 4s 9 r p 3 Gd : Ti : Ar 4s 3d Ge : Ar 4s 3d 4p 0 Xe 6s 5d f 7 64 54 4. A p,q, r 3 4 :s s B p,q, r 39Kr6s C p,q Ba : Xe6s 3. A p B C D 4. A p,s 56 88 Ra : Rn 7s 5 p,q,s 3 p,q, r 35 p, r 85 p : Ne 3s 3p 3,Ga : Ar 4s 3d 3p 0 Br : Ar 4s 3d 3p 0 5 At : Xe 6s 4f 5d 6p 4 0 5 n n B.M n: no. of unpaired electron B p,s 0 diamagnetic C p, r D q c paramagnetic 5. A p,q, r B C 6. (A) 7. (A) 8. (A) Integer type: Nd : Xe 6s 5d 4f 60 p,s 9 p,s 90 3 U : Rn 7s 6d 5f 3 Th : Rn 7s 6d 5f D p,s Fm or 00 Uun : Rn 7s 6d 5f. n n.73 3. (+4) n 00 CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 6

Maximum oxidation state shown by any element is equal to the number of valence electrons 3. (+6) Same as above. 4. (4) Amphoteric oxide are AlO 3, PbO, SnO &BeO. (B) Unn : Rn 7s 5f 6d 06 86 4 4 WINDOW TO JEE MAIN. (C) Cu :s s p 3s 3p 3d 4s 9 6 6 0 3. (A) In a period, from left to hight, atomic radius decreases while E. A increases. 4. (A) Phosphorous exist as solid at room temperature. 5. (D) Ca :,8,8 0 6. (A) Mg Na F Al Isoelectronic with Ne has 3 shell i.e they have two filled shell 7. (B) E. A electronegativity of element 8. (D) For alkali earth metal I.E I.E 9. (B) I.E of Mg I.E. 3 of Na as Na has acquired noble gas configuration. 0. (A) All species are isoelectronic with argon i.e has 8e in them. (D) I. E electronegativity I.E I.E as p has half filled 3p subshell s p. (D) In alkali metal, electronegativity or I. E. decreases down the group. So, it oxidises easily. Hence reactivity increases down the group. In halogens, down the group, Hence E. A so reactivity decreases. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 7

3. (C) Fact 4. (B) Theory 5. (D) Anion > neutral > cation 6. (C) 7. (C) 8. (B) 9. (B) 0. (C). (C). (C) 3. (B) 4. (A) I.E 6 7 8 9 I.E C :s s p N :s s p C :s s p 3 F :s s p 4 O F N C. Hydration energy I.E N O WINDOW TO JEE ADVANCED half filled subshell is more stable. ch arg e 5. (A) Down the group increases as number of shell increases. 6. (C) 7. (A) Electronegativity 8. (D) For isoelectronic species r r r 9. (B) cation atom anion CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 8

I.E For comparative, half filled subshell are more stable. So I. E is more 0. (D) There are exception to Aufbau principle. Ex: Cr & Cu. (B) Due to inert pair effect.. (D) Fe has 4 unpaired electron. 3. (B) 4. (B) Isoelectronic speies. 5. (B) I. E 6. (B) e 4 Be 4 s s stable Be s s p. OBJECTIVE QUESTION (MCQ). (BCD) Refer theory. (ABC) The difference between the I. P is very large when there is change in no. of shell 3. (D) More is the positive charge on atom, smaller is its. Assertion and reasoning. (C) Additional e are repelled more effectively by e in F than 3pe in Cl.. (C) p 3 is more in energy than s 0 orbital. 3. (C) The lower oxidation states are more stable due to inert pair effect. Fill in the Blanks.. Electron affinity. Electronegativity I.E E.A CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 9

3. Higher zeff As p e increases zeff increases. 4. Inert pair effect T/F. (T) Density of IA metal decreases down the group.. (F) Less ionization potential means more reducing agent. 3. (F) E. A. Cl Br F. 4. (F) X X m 0 increases down the group, so basic nature increases. Subjective Questions.. (i) O F Na Mg (Isoelectronic species) (ii) Na Al Mg Si, the effect of half filled or fully filled subshell only extends upto neighbouring element (iii) Cl F O N F FO ON N As atomic radius increases bond length increases as bond multiplicity increases bond length decreases.. 3. 4. Ca Ar Cl S (Isoelectronic species) e 6C :s s p C :s s p.p 6 More zeff.p e C :s s 6 e e 5B:s s p.p B :s s s.p 5 B :s s 4 Less zeff than 6C Mg Na F O N (Isoelectronic species) 3 fulfilled s orbital i.e stable Configuration. 5. Cu I.P I.P Zn I.P I.P Zn. Cu 6. 3 Al Mg Li K 0 0 0 0 0.5A 0.66 A 0.68 A.33 A CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 0