q.413 the correct order of decreasing first ionisation

Q.413 The correct order of decreasing first ionisation potential is (A) Ca > K > Rb > Cs (B) Cs > Rb > K > Ca (C) Ca > Cs > Rb > K (D) K > Rb > Cs > Ca Q.414 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 Q.415 Which of the following atom has highest ionisation energy. (A) N (B) O (C) P (D) S Q.416 Select the correct increasing order of ionization enthalpy of S, P, As elements - (A) S < P < As (B) P < S < As (C) As < S < P (D) As < P < S Q.417 Which one of the following electronic configuration of an atom has the lowest ionisation

energy (A) 1s22s22p3 (B) 1s22s22p63s1 (C) 1s22s22p6 (D) 1s22s22p5 Q.418 Which of the following elements has the highest ionisation energy? (A) [Ne] 3s23p1 (B) [Ne] 3s23p3 (C) [Ne] 3s23p2 (D) 3d10, 4s2 4p3 Q.419 Consider following electronic configuration of atoms and select correct code in order of

increasing ionization energy [I] 1s2 2s2 2p6 3s2 [II] 1s2 2s2 2p6 3s1 [III] 1s2 2s2 2p4 [IV] 1s2 2s2 2p5 [V] 1s2 2s2 2p6 (A) [II] < [I] < [III] < [IV] < [V] (B) [II] < [III] < [IV] < [I] < [V] (C) [II] < [IV] < [III] < [I] < [V] (D) [II] < [III] < [I] < [IV] < [V] Q.420 Element which has minimum first ionisation energy is - (A) N (B) P (C) O (D) S Q.421 The ionisation energies for B, Tl and In are X,Y and Z kcal/mol respectively, Choose the

correct relationship between them - (A) Z > X = Y (B) X > Y > Z (C) X > Y = Z (D) X < Y > Z Q.422 Which of the following has maximum ionisation energy? (A) Li+ (B) He (C) Ne (D) Na Q.423 The first ionization energy is maximum for (A) Na (B) Mg (C) K (D) Kr Q.424 The set representing the correct order of first ionization potential is (A) K > Na > Li (B) Be > Mg > Ca (C) B > C > N (D) Ge > Si > C Q.425 Which of the following orders are correct for the ionization energies ? (i) Ba < Sr < Ca (ii) S2– < S < S2+ (iii) C < O < N (iv) Mg < Al < Si (A) i, ii and iv (B) i, iii and iv (C) i, ii and iii (D) i, ii, iii and iv Q.426 The order of first ionization 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 Q.427 The correct order of first IE is-

(A) He > O > F > N (B) N > F > O > He (C) He > F > N > O (D) F > O > N > He

Q.428 The set representing the correct order of first ionization potential is : (A) K > Na > Li (B) Be > Mg > Ca (C) B > C > N (D) Ge > Si > C

Nth ionization energy Q.429 Find the correct order of 2nd ionisation energy?

(A) A1 > Mg (B) Cr > Cr+ (C)P > S (D) S > C Q.430 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 Q.431 Second ionization potential of Li, Be and B is in the order (A) Li > Be > B (B) Li > B > Be (C) Li > Be Be > Li Q.432 The correct order of second I.P. (A) Na < Mg > Al < Si (B) Na > Mg < Al > Si (C) Na > Mg > Al < Si (D) Na > Mg > Al > Si Q.433 The correct order of second ionization potential of C, N, O and F is - (A) C > N > O > F (B) O > N > F > C (C) O > F > N > C (D) F > O > N > C Q.434 Which pair of elements has same order of 1st and IInd ionisation enrgy ? (A) Li, Be (B) N, O (C) C, N (D) Be, B Q.435 Which of the following statement is incorrect?

(A) The second ionization energy of sulphur is greater than that of chlorine (B) The second ionization energy of silicon is greater than that of aluminium (C) The first ionization energy of aluminium is lower than galium (D) The second ionization energy of boron is greater than that of carbon

Q.436 The third ionization energy is least for (A) Nitrogen (B) Phosphorus (C) Aluminum (D) Boron

Q.437 The correct order of decreasing second ionization energy of Li, Be, Ne, C, B (A) Ne > B > Li > C > Be (B) Li > Ne > C > B > Be (C) Ne > C > B > Be > Li (D) Li > Ne > B > C > Be

Q.438 Among the following, third ionisation energy is highest for (A) magnesium (B) boron (C) beryllium (D) aluminium Q.439 The 2nd ionisation potential of Mg is less than that of Na because (A) Atomic size of Mg is less than that of Na. (B) Atomic size of Mg is greater than that of Na. (C) 2nd electron removal from Na occur from inert gas configuration, while the same for Mg

results inert gas configuration. (D) Both are having same Zeff value for 3s electron.

Q.440 Which configuration represents atom having highest second ionization energy?

(A) (B)

(C) (D) Q.441 The incorrect statement among the following is (A) the first ionization potential of Al is less than the first ionization potential of Mg (B) the second ionization potential of Mg is greater than the second ionization potential of Na (C) the first ionization potential of Na is less than the first ionization potential of Mg (D) the third ionization potential of Mg is greater than third ionization potential of Al Q.442 Which of the following ionisation energy order is/are correct. (A) Be+ > B2+ (B) C3+ < B2+ (C) N4+ < O5+ (D) F6+ < C3+

2 2 41s ,2s ,2p 2 2 61s ,2s ,2p2 2 6 11s ,2s ,2p ,3s 2 2 6 21s ,2s ,2p ,3s

Q.443 Amongst the following, the incorrect order is (A) IE1 (Al) < IE1 (Mg) (B) IE1 (N(A) < IE1(Mg) (C) IE2 (Mg) > IE2 (Na) (D) IE3 (Mg) > IE3 (Al)

Q.444 IInd IP of which of the element is maximum– (A) Lithium (B) Oxygen (C) Nitrogen (D) Fluorine Q.445 The first five ionization energies of an element are 9.1, 16.2, 24.5, 35 and 205.7 eV

respectively. Then number of valence electron in the atom is (A) 2 (B) 3 (C) 4 (D) 5 Q.446 Which of the following set of elements are having strongest tendency to form cation? (A) I, Cl, Br (B) C, Sn, Se (C) Na, K, Sr (D) Mn, Ti, Fe Q.447 Ionisation energies of element X are given below (in kJ/mol) IE1 IE2 IE3 520 7,340 11,000 If ‘X’ reacts with different elements which compounds are possible (A) XF (B) X2O (C) X3N (D) All of above Q.448 The successive ionisation energies of an element (in eV/atom) are :

The outer electronic configuration of the element may be : (A) ns2 np0 (B) ns2np3 (C) ns2np1 (D) ns2np2 Q.449 Successive ionization enthalpies (in eV/atom) of an element are 5, 8, 9, 90, 100. The number

of valence electrons are : (A) 1 (B) 2 (C) 3 (D) 4 Q.450 For element, A there is large energy difference between 5th and 6th ionisation energy. This

element is member of (A) Pnictogen family (B) Chalcogen family (C) Halogen family (D) Noble gases Q.451 For an element the successive ionisation energy values (in eV atom–1) are given below

12.32, 26.84, 44.56, 65.63, 203.9, 251.12, 308.4 The element that satisfies the above values is : (A) Si (B) Ca (C) Al (D) S Q.452 For an element having only one valence shell electron, then which of the following ionisation

energy difference will have the maximum value - (A) IE2 – IE1 (B) IE3 – IE2 (C) IE3 – IE1 (D) can't predict Q.453 The element having maximum tendency to form ionic bonds is (A) Cs (B) Rb (C) K (D) Li Q.454 The strongest reducing agent in gaseous phase is (A) Li (B) Na (C) K (D) Cs Q.455 The five successive ionisation energies of an element ‘X’ are 800, 1427, 2658, 4500 and

5024 KJ mole–1 respectively. The valency of ‘X’ is (A) 3 (B) 5 (C) 1 (D) 2

Q.456 First, second and third I.P. values are 100 eV, 150 eV and 1500 eV. Element can be (A) Be (B) B (C) F (D) Na Q.457 The maximum tendency to form unipositive ion is for the elment with the electronic

configuration- (A) 1s2, 2s2, 2p6, 3s2 (B) 1s2, 2s22p6, 3s23p1 (C) 1s2, 2s22p6, 3s23p2 (D) 1s2, 2s22p6, 3s23p3 Q.458 Mg forms Mg(II) because of :- (A) The oxidation state of Mg is + 2 (B) Difference between I.P1 and I.P2 is greater than 16.0 eV (C) There are only two electrons in the outermost energy level of Mg (D) Difference between I.P1 and I.P2 is less than 11 Ev

Q.459 The correct order of stability of Al+, Al+2, Al+3 is- (A) Al+3 > Al+2 > Al+ (B) Al+2 > Al+3 > Al+ (C) Al+2 < Al+ > Al+3 (D) Al+3 > Al+ > Al+2 Q.460. Mg forms Mg(II) because of - (A) The oxidation state of Mg is +2 (B) Difference between I.P1 and I.P2 is greater than 16.0 eV (C) There are only two electrons in the outermost energy level of Mg (D) Difference between I.P1 and I.P2 is less than 11 eV Q.461 Successive ionization 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 (C) 1s2, 2s2 2p2 (D) 1s2, 2s2 2p6, 3s2 Q.462 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 IE1 IE2 (A) I 2372 5251 (B) II 520 7300 (C) III 900 1760 (D) IV 1680 3380 Q.463 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 Q.464 First, second and third IP values are 100eV, 150eV and 1500eV. Element can be - (A) Be (B) B (C) F (D) Na Q.465 Which represents alkali metals (i.e. 1st group metals) based on (IE)1 and (IE)2 values (in

kJ/mol) ? (IE)1 (IE)2 (IE)1 (IE)2 (A) X 500 1000 (B) Y 600 2000 (C) Z 550 7500 (D) M 700 1400

Q.466 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

(C) 1s2, 2s2 2p6, 3s2 3p2 (D) 1s2, 2s2 2p6 3s2

Q.467 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 , 2s22p6 , 3s2 3p2 (B) 1s2 , 2s1

(C) 1s2 , 2s22p2 (D) 1s2 , 2s22p6 , 3

Q.468 The strongest reducing agent among the following is :– (A) Na (B) Mg (C) Al (D) K Q.469 Values of first four ionisation potential of an elements are 68, 370, 400, 485. It belongs to which of the following electronic configuration:- (A) 1s2 2s1 (B) 1s2 2s2 2p1 (C) 1s2 2s2 2p6 3s1 (D) (A) and (C) both Q.471 In which case the maximum energy is needed in the formation of monopositive gaseous ion :- (A) 1 mole of Li atoms (B) 1 mole of Na atoms (C) 1 mole of Cs atoms (D) 1 mole of Be atoms 472. Which of the following electronic configuration belongs to least and most metallic character

respectively:-

(a) 1s2 2s1 (b) 5s2 5p5 (c) 3s2 3p6 4s1 (d) 1s2 2s2 2p5 (A) a, b (B) d, c (C) b, a (D) c, d 473. In the given process which oxidation state is more stable.

M(g) ¾® M(g)+ IE1 = 7.9 eV

M(g) + ¾®M(g)+2 IE2 = 15.5 eV

(A) M+ (B) M+2 (C) Both (D) None 474 Inert pair effect is prominent character of (A) p-block element (B) d-block element

(C) s-block element (D)f-block element 475 Which of the following is incorrect statement(s): (A) Tl3+ > Tl+ (Stability order) (B) Pb2+ > Pb4+ (Stability order) (C) Fe+ > Fe2+ > Fe3+ (Radius order) (D) O2– > F¯ > Na+ (radius order 476 Stability of ions of Ge, Sn and Pb will be in the order : (A) Ge2+ > Sn2+ > Pb2+ (B) Ge4+ > Sn4+ > Pb4+ (C) Sn4+ < Sn2+ (D) Pb2+ < Pb4+

477 The value of of an atom are respectively 7.5 eV, 25.6 eV, 48.6 eV and 170.6 eV. The electronic configuration of the atom will be

(A) (B)

(C) (D) 478 Which of the following ionization energy values for calcium show a sudden increase? (A) Third (B) Second (C) First (D) Fourth 479 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. 480 Sodium forms Na+ ion but it does not form Na+2 because - (A) Very low value of IE1 and IE2 (B) Very high value of IE1 and IE2 (C) High value of IE1 and low value of IE2 (D) Low value of IE1 and high value of IE2 481 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 482 If the graph is plotted between atomic numbers and ionisation potential. Which group of

element occupy the lowest position on the curve :– (A) Alkaline earth metal (B) Inert gas (C) Actinides (D) Alkali metals 483 In the plot of the first ionization energy against atomic number the peaks are occupied by :- (A) Inert gases (B) Alkali metals (C) Halogens (D) Transition elements 484 Which of the following statement is/are not correct:- (A) I.P. increases down the group (B) IP of s–block elements is less than corresponding d– block elements (C) If DIP > 16 eV higher oxidation state is more stable (D) IP of halogen elements is maximum in their respective period

485 Which one of the following statements is incorrect in relation to ionisation enthalpy ? (A) Ionization enthalpy increases for each successive electron. (B) The greatest increase in ionization enthalpy is experienced on removal of electron from core of 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 orbitals having higher n value.

2 2 6 11s ,2s ,2p ,3s 2 2 6 2 11s ,2s ,2p ,3s ,3p2 2 6 2 31s ,2s ,2p ,3s ,3p 2 2 6 21s ,2s ,2p ,3s

486. Which one of the following statements is incorrect in relation to ionisation enthalpy ? (A) Ionization enthalpy increases for each successive electron. (B) The greatest increase in ionization enthalpy is experienced on removal of electron from core of 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 orbitals having higher n value.

487 In the given process which oxidation state is more stable. M(g) → M(g)+ + e– IE1 = 7.9 eV

M(g)+ → M(g)+2 + e– IE2 = 15.5 eV (A) M+ (B) M+2 (C) Both (D) None

488 The electronic configuration of some neutral atoms are given below:- (A) 1s2 2s1 (B) 1s2 2s2 2p3 (C) 1s2 2s2 2p5 (D) 1s2 2s2 2p6 3s1 489 In which of these electronic configuration would you expect to have highest (i) IE1 (ii) IE2 (A) C, A (B) B, A (C) C, B (D) B, D 490. The sum of IE1 and IE2, IE3 and IE4 for element P and Q are given below:

IE1 + IE2 IE3 + IE4 (P) 2.45 8.82 (Q) 2.85 6.11 Then according to the given information the correct statement(s) is/are: (A) p2+ is more stable than Q2+ (B) p2+ is less stable than Q2+ (C) p4+ is more stable than Q4+ (D) p4+ is less stable than Q

491. Which one of the following represents the electronic configuration of the most electropositive element

(A) [He] 2s1 (B) [Xe] 6s1 (C) [He] 2s2 (D) [Xe] 6s2 492. 1/4th of Avogadro number of atoms of an element absorb energy ‘X’ kJ, the ionisation energy of per atom is,

(A) (B) (C) (D) 493 The first ionisation energies of the elements of the first transition series (Ti ® Cu) (A) increase as the atomic number increases (B) decrease as the atomic number increases (C) do not show any change as the addition of electrons takes place in the inner (n–1) d-

orbitals (D) increase from Ti to Mn and then decrease from Mn to Cu 494. Which of the following element has maximum, first ionisation potential (A) V (B) Ti (C) Cr (D) Mn 495 Which of the following has the lowest second ionisation energy? (A) Sc (B) Ti (C) V (D) Ca 496. The ionisation energy for ‘Sc’ , ‘Y’ and ‘La’ are x, y and z kcal/mol respectively. Choose the

correct relationship between them. (A) z > x » y (B) x > y > z (C) x > z » y (D) x < y > z 497. Element which has maximum ionisation energy. (A) Zn (B) Cu (C) Cd (D) Hg 498. Which of the following atoms has the highest first ionization energy? (A) Na (B) K (C) Sc (D) Rb

499. Which of the following element has highest value of ionisation energy- (A) Ti (B) Zr (C) Hf (D) None of these

0

2XN 0

4XN

04NX

0N4X

500. The correct order of ionisation energy of Al, K, Fe, Mg is (A) K < Al < Mg < Fe (B) K < Mg < Al < Fe (C) Mg < K < Al < Fe (D) Mg < Fe < Al < K 501. Which ionisation potential in the following equations involves the greatest amount of energy? (A) K+ → K2+ + e– (B) Ca+ → Ca2+ + e–

(C) Fe → Fe+ + e– (D) Li+ → Li2+ + e–

502. Which has the lowest IE :-

(A) 3d2 (B) 4s1 (C) 3p3 (D) 2p6 503 The incorrect statement among the following is : (A) The first ionisation energy of calcium is more than first ionisation energy of gallium (B) The second ionisation energy of copper is greater than that of potassium (C) The third ionisation energy of Mg is greater than the third ionisation energy of Al (D) The IE1 of Mg+ is less than the IE1 of Na+

504 Which of the following has the highest second ionisation energy? (A) Cr (B) Mn (C) Co (D) Fe 505 The incorrect order of IInd ionisation energy is (A) Cu > Zn (B) Cr > Mn (C) Na > Mg (D) Mg > Al

506. What is the correct order of ionisation energy : (A) K < Cu < Cu+ < K+ (B) K < Cu+ < Cu < K+ (C) Cu+ < K < Cu < K+ (D) K+ < Cu+ < Cu < K

507. Which one of these is expected to have the highest second ionization enthalpy? (A) Cr (B) V (C) Fe (D) Ni 508. Which of the following relation is correct with respect to first (I) and second (II) ionization

enthalpies of potassium and calcium ? (A) ICa > IIK (B) IK > ICa (C) IICa > IIK (D) IIK > IICa 509. The correct order of decreasing second ionisation enthalpy of Ti(2(B), V(2(C), Cr(2(D) and

Mn(25) (A) Cr > Mn > V > Ti (B) V > Mn > Cr > Ti (C) Mn > Cr > Ti > V (D) Ti > V > Cr > Mn 510. 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 511. The energy released when a neutral gaseous atom, takes up an electron and forms a uni negative ion is called its (A) effective nuclear charge (B) polarising power (C) electron affinity (D) ionization potential 512. Which of the following is as per the definition of electron-afiinity of element ? (A) X2(g) ® 2X– (g) (B) X(g) ® X– (g)

(C) X+(g) ® X (g) (D) X–(g) ® X2– (g) 513. Energy is absorbed when a second electron is added to oxygen. This is because (A) O- has stable configuration (B) O- has repulsion with electron to be added (C) O- has lower nuclear charge than O (D) O2- has unstable configuration

514. Second electron gain enthalpy ? (A) is always negative (B) is always positive (C) can be positive or negative (D) is always zero 515. Which of the following process is endothermic?

(A) Na(g) + 1e¯ ¾® Na¯(g) (B) O+ (g) + 1e¯ ¾® O(g) (C) O¯ (g) + 1e¯ ¾® O2– (g) (D) S + 1e¯ ¾® S¯(g)

516. Which of the following is incorrect? (A) For A(g) + e– ¾® A¯(g), DH may be positive (B) For A¯(g) + e– ¾® A2–(g), DH may be negative (C) For A¯(g) + e– ¾® A2–(g), DH must be positive (D) For A2+(g) + e– ¾® A+(g), DH must be negative

517. If the amount of energy required in the process X to X¯ is –5 kJ/mole then calculate how many energy is required in X to X+ process (A) –5 kJ/mole (B) > 5 kJ/mole (C) < 5 kJ/mole (D) 5 kJ/mole

518. Electron addition would be easier in - (A) O (B) O+ (C) O– (D) O+2

519. O(g) + 2e– ® DHeg = 744.7 KJ/mole. The positive value of DHeg is due to -

(A) Energy is released to add to 1 e– to O–1

(B) Energy is required to add to 1 e– to O–1 (C) Energy is needed to add on 1 e– to O (D) None of the above is correct

520 Second electron affinity of an element is - (A) Always exothermic (B) Endothermic for few elements (C) Exothermic for few elements (D) Always endothermic

521. For the processes K+(g) (")"# K(g)

("")"# K(s)

(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

522. The amount of energy which is released due to addition of extra electron to the outermost orbit of gaseous atom is called

(A) Electron capacity (B) Electron affinity (C) Ionisation potential (D) Electronegativity 523. Which of the following has electron affinity less than zero (DHeg = +ve) :- (A) O–2 (B) S–2 (C) (A) & (B) both (D) O+57. Energy absorbed in

524. The formation of the oxide ion requries first an exothermic and then an endothermic step as shown below:

This is because : (A) ion has comparatively larger size than oxygen atom (B) oxygen has high electron affinity (C) ion will tend to resist the addition of another electron. (D) Oxygen is more electronegative

525 When the first electron gain enthalpy (ΔegH) of oxygen is – 141 kJ/mol, its second electron gain enthalpy is :

(A) almost the same as that of the first (B) a positive value (C) a more negative value than the first (D) negative but less negative than the first

526 The process requiring the absorption of energy is - (A) F ® F– (B) Cl ® Cl– (C) O ® O2– (D) H ® H– EA and IE 527. If electron gain enthalpy of X(g) is – 4.0 eV, then the ionisation enthalpy of X(g) at the same

temperature may be : (A) 4.0 eV (B) 3.5 eV (C) 5.5 eV (D) any of these values

528. What is the value of Electron gain enthalpy of Na+ if IE1 of Na= 5.1 eV? (A) +2.55 eV (B) +10.2eV (C) – 5.1 eV (D) – 10.2 eV 529. Select correct relationship for Na atom.

(A) | I.E. of Na | < | E.A. of Na | (B) | I.E.of Na | > | I.E. of Na¯ | (C) | I.E. of Na | > | I.E. of Na+ | (D) | E.A. of Na | = | I.E.of Na+ |

530. For the process X(g) + e– ¾® X–(g), DH = x and X–(g) ¾® X(g) + e–, DH = y Select correct alternate : (A) Ionization energy of X–(g) is y (B) Electron affinity of X(g) is – x (C) Electron affinity of X(g) is +y (D) All are correct statements

531 Ionization energy of an element is : (A) Equal in magnitude but opposite in sign to the electron gain enthalpy of the cation of the element (B) Same as electron affinity of the element (C) Energy required to remove one valence electron from an isolated gaseous atom in its ground state (D) Equal in magnitude but opposite in sign to the electron gain enthalpy of the anion of the

element 532. 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– Factors affecting 533. The magnitude of electron affinity depends upon (A) electron affinity (B) Polarising power (C) ionization potential (D) the nuclear charge 534. The low electron affinity value of nitrogen is due to (A) small size (B) high nuclear charge (C) half-filled 2p sublevel (D) high metallic character 535. EA1 values of the following element has positive value (A) Be (B) Br (C) Mg (D) Cl The correct answer is (A) a and c (B) b and d (C) a , b and c (D) a, b and d 536. Which of the following will have positive DHeg (A) Chlorine (B) Oxygen (C) Magnesium (D) Sulphur

537. Adding electron a neutral gaseous atom usually leads to -

(A) Liberation of energy (B) Formation of anion (C) Proton/electron ratio decrease (D) Proton/electron ratio increase Code in - (A) (A), (D) (B) (B), (C), (D) (C) (A), (B), (D) (D) (A), (B), (C)

538 Whichofthefollowingconfigurationwillhaveleastelectronaffinity.

(A)ns2np5 (B)ns2np2 (C)ns2np3 (D)ns2np4539. Which of the following statement is correct.

(A) The 1st ionisation potential of N is greater than that of O+. (B) The 1st ionisation potential of N is equal to that of O+. (C) The 1st ionisation potential of N is less than that of O+. (D) The electron affinity of ‘N’ is greater than that of ‘O’.

540 The least stable anion is : (A) Li– (B) Be– (C) B– (D) C–

541. Which of the following is exothermic: (A) N(g) + 1e– ® N–(g) (B) P(g) + 1e– ® P–(g) (C) Na(g) ® Na+(g) + 1e– (D) 1e– + Be(g) ® Be–(g)

542. Addition of an electron to a gas phase Silicon (Si) atom results in the release of more energy than addition of an electron to a gas phase Phosphorus (P) atom. What is the best explanation for relative electron affinities ?

(A) The electron added to Si experiences less electron - electron repulsion than electron added to P

(B) the electron added to Si enters in lower energy subshell than the electron added to P (C) Si is more electronegative than P (D) Si is smaller than P 543. Which of the following process energy is liberated -

(A) Cl ® Cl+ + e– (B) HCl ® H+ + Cl– (C) Cl + e– ® Cl– (D) O– + e– ® O–2 544. Which of the following configuration will have least electron affinity -

(A) ns2np5 (B) ns2np2 (C) ns2np3 (D) ns2np4 EA left to right

545. Thecorrectorderofelectronaffinityis:- (A)Be<B<C<N (B)Be<N<B<C (C)N<Be<C B (C) Li > B (D) Li > C 547. Which element has highest Electron Affinity?

(A) Be (B) B (C) Li (D) C 548. Which of the following is incorrect order of electron affinity:

(A) Li < Na (B) Al > B (C) Si > C (D) Cl > F 549. Which of the following would require least energy?

(A) Si– (g) ¾¾® Si (g) + e– (B) P– (g) ¾¾® P (g) + e– (C) S– (g) ¾¾® S (g) + e– (D) Cl– (g) ¾¾® Cl (g) + e–

550. Which of the following process is associated with the energy release.

(A) Li ¾® Li+ (B) O¯ ¾® O2– (C) Cl+ ¾® Cl (D) Be ¾® Be¯

551. The electron affinity for inert gases is like to be (A) High (B) Small (C) Zero (D) Positive 552. The electron affinity of Be is almost similar to that of (A) Li (B) B (C) Na (D) Ne 553. Which of the following represents the correct order of electron affinities ? (A) F>Cl>Br>I (B)C<N<O<F (C) N<C<O<F (D)C<Si<P<N 554. In which case the energy released is minimum?

(A) Cl ® Cl– (B) P ® P– (C) N ® N– (D) C ® C–

555. In the process Cl (g) + e– ® Cl–(g) , DH is : (A) positive (B) negative (C) zero (D) none of these

556. 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

557. 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

558. TheamountofenergyreleasedfortheprocessX(g)+e–® X–(g)isminimumand

maximumrespectivelyfor:– (a)F (b)Cl (c)N (d)B Correctansweris:– (A)c&a (B)d&b (C)a&b (D)c&b

559. Whichofthefollowingelectronicconfigurationisexpectedtohavehighestelectronaffinity:-

(A)2s22p0 (B)2s22p2 (C)2s22p3 (D)2s22p1560. Which of the following pair has correct order of electron affinity (A) F>Fe (B) Ne> Na (C) Ba>Br (D) F=Fe 561. The energy released when an electron is added to a neutral gaseous atom would be highest if

the element belongs to (A) VII A group (B) V A group (C) VI A group (D) II A group 562. Highest electron-affinity is associated with the configuration - (A) 2s2, 2p0 (B) 2s2, 2p2 (C) 2s2, 2p3 (D) 2s2, 2p1 EA top to bottom 563. Fluorine has low electron affinity than chlorine because of -

(A) Smaller radius of fluorine, high electron density (B) Smaller radius of chlorine, high electron density (C) Bigger radius of fluorine, less electron density (D) Smaller radius of chlorine, less electron density

564. Among fluorine and chlorine, the electron affinity of the latter is high. This is due to (A) high electronegativity of fluorine (B) low dissociation energy of fluorine (C) fluorine repels with the added electron due to its small size (D) small size of Chlorine atom

565. Electron affinity of chlorine is -348 kJ/mol. Then the electron affinity of Fluorine is ...... in kJ/mol

(A) -333 (B) -348 (C) -384 (D) -428 566. The electron affinity order for halogen is (A) F < Cl Cl Br > I (D) F > Cl > Br > I 567. In which of the following process, maximum amount of energy involved.

(A) Cl ® Cl¯ (B) Br¯ ® Br (C) F¯ ® F (D) I¯ ® I 568. Select the correct order of electron affinity :

(A) F– > Cl– (B) F > Cl (C) Cl > F (D) F– > F 569. Select correct graph of first electon affinity values of oxygen family.

(A) (B)

( (C) (D) 570. Choose the incorrect statement.

(A) 2nd electron gain enthalpy for any element is (+) ve. (B) E.A. of an element µ Zeff (C) The ionisation energy order : F¯ > Cl¯ (D) The ionisation energy order : F¯ < Cl¯

571. Elementofwhichatomicnumberhashighestelectronaffinity:- (A)35 (B)17 (C)9 (D)53572. The order of electron gain enthalpy (magnitude) of O, S, Se and Te is :

(A) O > S > Se > Te (B) S > Se > Te > O (C) Se > S > Te > O (D) S > O > Se > Te

Mix 573. In which transition maximum amount of energy will be released.

(A) S(g) + 1e– ® S–(g) (B) O(g) + 1e– ® O–(g) (C) N(g) ® N+(g) + 1e– (D) He(g) + 1e– ® He–(g)

574. Which of the following represents correct order of electron affinity? (A) O < S < F < Cl (B) O < F < S < Cl (C) F > O > Cl > S (D) F > Cl > O > S

575. Which of the following has the lowest electron affinity? (A) O (B) S (C) F (D) Cl

576. The incorrect order of electron affinity is : (A) F < Cl (B) N > P (C) O < S (D) Cl > Br 577. Select incorrect order of E. A.

(A) Cl > F (B) O < S (C) N > P (D) C < Si 578. The correct order of electron affinity is

(A) N > P > S > Cl (B) P > N > S > Cl (C) Cl > N > P > S (D) Cl> S > P > N

579. The numerical value of energy involved in the given process ; S ® S– is less than, which of the following process : (A) S– ® S (B) Se ® Se– (C) S ® S+ (D) (B) and (C) both

580. Select the atom which has maximum electron affinity - (A) C (B) Si (C) N (D) P

581. Of the following elements, which possess the highest electron affinity? (A) As (B) O (C) S (D) Se

582. Increasing order of Electron affinity for following configuration. (a) 1s2, 2s2 2p3 (b) 1s2, 2s2 2p4 (c) 1s2, 2s2 2p6 3s2 3p4 (d) 1s2, 2s2 2p6, 3s2 3p3 (A) a < d < b < c (B) d < a < c < b (C) a < b < c < d (D) a < b < d < c

583. Which of the following case is endothermic - (A) Cl ® Cl– (B) P ® P– (C) N ® N– (D) C ® C–

584. Which of the following element is expected to have highest negative electron gain enthalpy - (A) 1s22s22p63s23p5 (B) 1s22s22p3 (C) 1s22s22p4 (D) 1s22s22p5

585. The electron affinity of - (A) Carbon is greater than oxygen (B) Sulphur is less than oxygen (C) Iodine is greater than bromine (D) Bromine is less than chlorine

586. Process in which maximum energy is released:-

(A) O ® O–2 (B) Mg+ ®Mg+2 (C) Cl ®Cl– (D) F ® F – 587. The element having highest electron affinity is (A) Fluorine (B) Nitrogen (C) Chlorine (D) Oxygen 588. Among the following electronic configurations which one will have highest electron affinity value (A) 1s2 (B) 1s2 2s2 (C) 1s2 2s2 2p4 (D) 1s2 2s2 2p5

589. Which statement is correct - (A) The E.A. of carbon is greater than oxygen (B) The E.A. of sulphur is less than oxygen (C) The E.A. of iodine is greater than bromine (D) The E.A. of bromine is less than chlorine 590. To which of the following atom, the attachment of electron is most difficult ? (A) Neon (B) Nitrogen (C) Oxygen (D) Radium 591. Which of the following order of electron affinity (E(A) is correct ? (A) S > O > Se (B) Cl > Br > F (C) N N > O 592. Which of the following represent the correct order of electron affinity:

(a) Cl > Br > F > I (b) Cl > S > O > P (c) F > O > C > N (d) Cl > P > S > Si (A) a,c,d (B) b,c,d (C) b,d (D) b,c

593. Arrange N, O and S in order of increasing electron affinity (A) S < O < N (B) N < S < O (C) N < O < S (D) O < N < S

594. Which of the following statement is correct ? (A) Electron gain enthalpy must be positive for all elements. (B) Second electron gain enthalpy always remains negative for all the elements. (C) ΔegH(K+) = –IE (Ar) (D) None of these

595. The increasing order of electron affinity is: (A) N < O < Cl < A1 (B) O < N < A1 < Cl (C) A1 < P < Si < Cl (D) Cl < N < O < A1

596. Which of the following will have the most negative electron gain enthalpy and which the least negative ? F, P, S, Cl. (A) P, Cl (B) Cl, F (C) Cl, S (D) Cl, P 597. The correct order of electron affinity is : (A) F > Cl > O (B) F > O > Cl (C) Cl > F > O (D) O > F > Cl 598. Which of the following has the highest electron affinity ? (A) F– (B) O– (C) O (D) Na 599. Which of them is correct order of electron affinity ? (A) F > I > Te > O (B) I > F > O > Te (C) Te > I > F > O (D) F > O > I > Te

q.413 the correct order of decreasing first ionisation

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