Periodic Table and Its Properties Mock Test

MOCK TEST SECTION - I : 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 2. (C) II, IV (D) I, III, IV The correct order of second ionisation potential of carbon, nitrogen, oxygen and flourine is : (A) C > N > O > F 3. (B) I, II, III, IV (B) O > N > F > C (C) O > F > N > C (D) F > O > N > C 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. PERIODIC TABLE AND ITS PROPERTIES SECTION - II : MULTIPLE CORRECT ANSWER TYPE 7. Which of the following statement(s) is/are true ? (A) ionisation energy  1 Screening effect (B) The first ionisation energies of Be and Mg are more than ionisation energies of B and Al respectively (C) Atomic and ionic radii of Niobium and Tantalum are almost same. (D) Metallic and covalent radii of potassium are 2.3Å and 2.03Å. 8. 9. Which of the following pair(s) represent(s) the isoelectronic species ? (A) S–2 and Sc+3 (B) SO2 and NO3– (C) N2 and CN– (D) NH3 and H3O+ The process(es) requiring the absorption of energy is/are : (A) Cl – Cl– (B) O– – O2– (C) Fe+3 – Fe+2 (D) Ar – Ar– SECTION - III : ASSERTION AND REASON TYPE 10. Statement – 1: Flourine has only one oxoacids, HOF because, Statement – 2 : Flourine has small size and high electronegativity. (A) Statement-1 is True, Statement-2 is True; Statement-2 is a correct explanation for Statement-1. (B) Statement-1 is True, Statement-2 is True; Statement-2 is not a correct explanation for Statement-1. (C) Statement-1 is True, Statement-2 is False. (D) Statement-1 is False, Statement-2 is True. 11. Statement – 1 : The 5th period of periodic table contains 18 elements not 32. Statement – 2 : n = 5, __= 0, 1, 2, 3. The order in which the energy of available orbitals 4d, 5s and 5p increases is 5s < 4d < 5p and the total number of orbitals available are 9 and thus 18 electrons can be accomodated. (A) Statement-1 is True, Statement-2 is True; Statement-2 is a correct explanation for Statement-1. (B) Statement-1 is True, Statement-2 is True; Statement-2 is not a correct explanation for Statement-1. (C) Statement-1 is True, Statement-2 is False. (D) Statement-1 is False, Statement-2 is True. 12. Statement – 1 : Manganese (atomic number = 25) has a less favourable electron affinity than its neighbours on either side because, Statement – 2 : The manganese has stable [Ar]18 3d5 4s2 electrons configuration. (A) Statement-1 is True, Statement-2 is True; Statement-2 is a correct explanation for Statement-1. (B) Statement-1 is True, Statement-2 is True; Statement-2 is not a correct explanation for Statement-1. (C) Statement-1 is True, Statement-2 is False. (D) Statement-1 is False, Statement-2 is True. 13. Statement – 1 : The ionisation energy of phosphorus is larger than sulphur. Statement – 2 : There is a larger amount of stability associated with filled s- and p- sub-shells (a noble gas elctron configuration) which corresponds to having eight electrons in the valence shell of an atom or ion. (A) Statement-1 is True, Statement-2 is True; Statement-2 is a correct explanation for Statement-1. (B) Statement-1 is True, Statement-2 is True; Statement-2 is not a correct explanation for Statement-1. (C) Statement-1 is True, Statement-2 is False. (D) Statement-1 is False, Statement-2 is True. 14. Statement – 1 : The electron gain enthalpies have large negative values towards the upper right of the periodic table precedign the noble gas. Statement – 2 : The effective nuclear charge increases from left to right across a period and consequently it will be easier to add an electron to a smaller atom since the added electron on an average would be closer to the positively charged nucleus. (A) Statement-1 is True, Statement-2 is True; Statement-2 is a correct explanation for Statement-1. (B) Statement-1 is True, Statement-2 is True; Statement-2 is not a correct explanation for Statement-1. (C) Statement-1 is True, Statement-2 is False. (D) Statement-1 is False, Statement-2 is True. SECTION - V : MATRIX - MATCH TYPE 15. Match the species/elements listed in column I with their characteristic listed in column II. Column I Column II –3 –2 (A) SO2, NO , CO3 (p) Semi-metals (B) Ge, As, Sb (q) Inert gases (C) Ar, Kr, Xe (r) Isoelectronic species (D) Ca, Sr, Ba (s) Alkaline earth metals 16. 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 –1  1H 1 ,  1H 2 , egH (in kJ mol ) , (A) 2372 5251 +48 (p) Elements which acts as a strong reducing agent (B) 419 (C) 1681 (D) 1008 17. 3051 3374 1846 -48 -333 -295 (q) Elements which exists as a monoatomic molecule (r) Least reactive non-metal (s) Elements which acts as a strong oxidising agent (t) Element which oxide is a stronger basic in nature Match the increasing order given in column I with the property(ies) given in column II. Column I (A) Na < F– < O2– < N3– (B) Li+ < Na+ < K+ < Rb+ < Cs+ (C) O < S < F < Cl (D) Cl– < K+ < Ca2+ < Sc3+ + Column II (p) Semi-metals (q) Mobility of hydrated ions (r) Ionic size (s) Electron affinity SECTION - IV : COMPREHENSION TYPE Read the following comprehensions carefully and answer the questions. Comprehension # 1 Read the following comprehension carefully and answer the following questions. Numerous forms of periodic table haev been revised from time to time. A modern version, which is most convinient and widely used is the long or extended form of periodic table.The afbau principle (electrons are filled in the progressive order of their increasing energy, i.e ny n+1 rule ) and the electronic cconfiguration of atom provide a theoritical foundation for the periodic classification. The horizontal rows are called periods. There are altogether seven periods. The first period consists of 2 elements. The subsequent periods consist of 8, 8, 18, 18 and 32 elements respectively. The seventh period is incomplete and like the sixth period would have the maximum of 32 elements. PERIODIC TABLE AND ITS PROPERTIES Elements having similar outer electronic configurations in their atoms are grouped together in vertical columns. These are reffered to as groups or families. According to the recommendation of IUPAC, the groups are numbered 1 to 18 replacing the older notifications of groups 0, IA, IIA........VII A,VIII, IB.........VII B. Each successive period in the periodic table is asssociated with the filling up next higher principal energy level following afbau principle. The number of eleementss in each period iss twice the number of atomic orbitals available in the energy level that is being filled. All the elements are classified into four blocks, i.e., s-block, p-block, d-block and f-block depending on the type of atomic orbitals that are being filled with their last electron of the element. 18. The element with atomic number 56 is likely to have the same outer shell configuration as the element with atomic number : (A) 12 19. (B) 18 (D) 20 If afbau rule iss not allowed, Ca will be placed in ______ block. (A) s- 20. (C) 14 (B) p- (C) d- (D) f- What is the position of the element in the periodic table satisfying the electronic configuration (n – 1) d 1 ns2 for n=4. (A) 3rd period and 3rd group (B) 4th period and 4th group (C) 3rd period and 2nd group (D) 4th period and 3rd group Comprehension # 2 The first (1H1) and second (1H2) ionisation enthalpies ( in kJ/mol) and the (egH) electron gain enthalpy ( in kJ/mol) of a few elements are given below : 21. Elements 1H1 1H2 egH (A) P 520 7300 -60 (B) Q 419 3051 -48 (C) R 1681 3374 -324 (D) S 1008 1846 -295 (5) T 2372 5251 +48 (6) U 738 1451 -40 The least reactive element is : (A) P 22. (C) R (D) T (C) S (D) U (C) P (D) U The most reactive element is : (A) P 23. (B) Q (B) Q The most reactive non-metal is : (A) R (B) S Comprehension # 3 The amount of energy required to remove the most loosely bound eleectron from as isolated gaseous atom is called as first ionization energy (IE1). Similarly the amount of energies required to knock out second, third etc. electrons from the isolated gaseous cation are called successive ionization energies and IE 3 > IE2 > IE1. (i) Nuclear charge (ii) Atomic size (iii) penetration effect of the electrons (iv) shielding effect of the inner electrons and (v) electronic configurations (exactly half filled and completely filled configurations are considerd extra stable) affect the ionisation energies. On the other hand, the amount of energy released when a neutral isolated gaseous atom accepts an extra electron to form a gaseous anion is called electron affinity. Exothermic O(g) + e–  O– (g) ; Heg = – 141 kJ mol–1 ........(i) 2– –1 Endothermic O(g) + e–   O (g) ; Heg = + 780 kJ mol ........(i) In (ii) the energy has to be supplied for the addition of second electron due to the electrostatic repulsion between an anion and extra electron ( same charged species ). The electron affinity of an elements depends upon (i) atomic size (ii) nuclear charge and (iii) electronic configuration. In general, ionisation energy and electron affinity increases as their atomic size decreases and nuclear chargee increases across a period. In general, in a group, ionisation energy and eleectron affinity decreasese as the atomic size increases down the group. The members of the third period have some higher ( e.g. S and Cl ) electron affinity values that the members of the second period ( e.g. O and F ) because second period elements have very small atomic size. Hence there is a tendency of electron-electron repulsion, which result in less evolution of energy in the formation of corresponding anion. 24. 25. The first ionization energy of Na, Mg, Al, Si are in the order of : (A) Na < Mg > Al < Si (B) Na > Mg > Al > Si (C) Na < Mg < Al > Si (D) Na > Mg > Al < Si Which one the following statements is correct ? (A) The elements like F, Cl, Br etc having high values of electronic affinity act as a strong oxidising agent. (B) The elements having low values of ionisation energies act as a strong reducing agent. (C) The formation of Be-(g) from Be (g) is an endothermic process. (D) All of these 26. Which one the following statements in incorrect in relation to ionisation enthalpy ? (A) Ionization enthalpy increase for each successive valence shell 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 on ionization enthalpy. (D) Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value. 27. Considering the elements F, Cl, O, and N, the correct order of their electron affinity values is : (A) F > Cl > O > S (B) F > O > Cl > S (C) Cl > F > S > O (D) O > F > S > Cl MOCK TEST 1. 6. 11. 15. 16. 17. 18. 23. C 2. C B 7. A,B,C,D A 12. A A  (r), B  (p), C  (q), D  (s) A  (q) ; B  (p,t) ; C  (s) ; D  (r) A  r); B  (q, r) ; C  s) ; D  (p, s) A 19. C 20. A 24. A 25. 3. 8. 13. D D D A,B,C,D D 4. 9. 14. 21. 26. D D B B,D A 5. 10. 22. 27. B C D A