Periodic Properties (Booklet Solution)

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1 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 #

2 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 r r F r S r r r r Na F 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 H P 78 kcal mol Mg mg e Mg Mg e H P 348 kcal mol H H H = CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI #

3 = 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 in 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 4 Be :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

4 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 (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 undergoes reduction easily than bromine, so it is better oxidizing agent. 48. (C) CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 4

5 Electronegativity decreases down the group, but decrease 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 (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) I.P E.A XM I.P & E.A in ev/atom. 53. (A) More is the electronegativity difference, more is the ionic character. For same atom, electronegativity (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. 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 M : Ar 3d 4s 4p. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 5

6 5. (B) 6Fe : Ar 4s 3d 6Fe 6. (B) : Ar 3d (C) Due to inert pair effect 8. (A) w.r.t oxygen halogen family : 7 oxygen family : O Nitrogen family : +5 Boron family : (D) Valency of A is 3 Valency of B is compound formed is AB (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 Ni ; Increase in effective atomic number is balanced by increase in repulsion between electrons. Ni Cu Zn Increase in Z eff 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. 4. (C) I.E I.E For alkali metal 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) CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 6

7 Metal oxide are basic while non metal oxides are acidic in nature generally. 9. (C) Cr : Ar 3d 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 differs by, 8, 8, 8, 3. Etc. 3 (B) Isoelectronic species 4. (B) Li :s 3 4 Be :s s 5 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 element. It belongs to th 6 group. 6. (A) 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 Achievement of inert gas configuration but repulsion is also there as electron is entering in nd shell. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 7

8 r is least for NaF 9. (B) For alkaline, earth metal, 4,, 0, 38, 56, 78, (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 Energy required 70kJ 7.3kJ. 3. (A) 33. (B) is more stable than F I.E I.E 34. (B) 35. (C) I.E 36. (B) I.E I.E I.E I.E F F - (I.E) neutral atom > (I. E) anion.. I.E np ns I.E 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 39. (B) B >.7 Ionic bond is formed. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 8

9 40. (B) 4. (D) According to Mulliken s scale I.E E.A X X Y I.E 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 e O e S S Incoming electron is repelled by anionic electrons. 49. (B) Heg is always endothermic. (B) Unn : Rn 7s 5f 6d WINDOW TO JEE MAIN. (C) Cu :s s p 3s 3p 3d 4s (A) In a period, from left to right, atomic radius decreases while E. A. increases. 4. (A) Phosphorous exist as solid at room temperature. 5. (D) 0 Ca :,8,8 CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 9

10 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 I.E s p as p has half filled 3p subshell. (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, 3. (C) Fact Hence E. A so reactivity decreases. 4. (B) Theory 5. (D) Anion > neutral > cation 6. (C) 7. (C) For isoelectronic species as number of protons increase attraction between outer most orbit electron and nucleus increases that is decreases. 8. (B) Down the group ionization energy decreases. 9. (B) For isoelectronic species as number of protons increase attraction between outer most orbit electron and nucleus increases that is decreases. 0. (C) Down the group ionization energy decreases. CENTERS : MUMBAI /DELHI /AKOLA /LUCKNOW /NASHIK /PUNE /NAGPUR /BOKARO /DUBAI # 0

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