InterviewSolution
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InterviewSolution
This section includes InterviewSolutions, each offering curated multiple-choice questions to sharpen your knowledge and support exam preparation. Choose a topic below to get started.
| 51. |
`N_(0)//2` atoms of X(g) are converted into `X^(+)` (g) by energy `E_(1) . N_(0)//2` atoms of X(g) are converted into `X^(-)` (g) by the energy `E_(2)` . Hence ionisation potential and electron affinity of X(g) are :A. `(2E_(1))/(N_(0)) , (2(E_(1) - E_(2)))/(N_(0))`B. `(2E_(1))/(N_(0)) , (2E_(2))/(N_(0))`C. `((E_(1) - E_(2)))/(N_(0)) , (2E_(2))/(N_(0))`D. `(E_(1))/(N_(0)) , (2E_(2))/(N_(0))` |
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Answer» Correct Answer - B |
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| 52. |
According to Moseley, a straight line graph is obtained on plotting:A. the frequencioes of characteristic line graphB. the square of the frequencies of characteristic X-rays of elements against their atomic numbersC. the square root of the frequencies of characteristis X-rays of elements against their atomic numbers.D. the reciprocal of the frequencies of characteristic X-rays of elements against their atomic numbers |
| Answer» Correct Answer - C | |
| 53. |
In the modern periodic table, the block indicates the value of `………………` for the last subshell that received electrons in building up the electronic configuration. Fill in the blank with appropriate optionA. Atomic numberB. Aximuthal quantum numberC. Principal quantum numberD. Atomic mass |
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Answer» Correct Answer - 2 The block indicates value of azimuthal quantum number `(l)` for the last sub`-` shell that received electrons in building up the electronic configuration. For examples group 1 and group 2 elements belong to `s-` block as last electron enters in `s-` subshell. |
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| 54. |
A `M^(2+)` ion derived from a metal in the first transition metal series has four electrons in `3d` subshell. What element might `M` be? |
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Answer» Correct Answer - Chromium `{:(,"Electron configuration of "M^(2+)is:,,[Ar]^(18)4s^(@)3d^(4)),( :.,"Electron configuration of"M is:,,[Ar]^(18)4s^(1)3d^(5)("and not" 5s^(2)3d^(4))):}` So total number of electrons `= 24`. Hence, metal `M` is chromium `(Cr)`. |
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| 55. |
Using the periodic table predict the formula of compound which might be formed by the following pair of elements: silicon and bromineA. `SiBr_(2)`B. `SiBr_(4)`C. `Si_(2)Br_(8)^(4-)`D. `Si_(3)Br_(8)^(2-)` |
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Answer» Correct Answer - B Br is more EN than Si and Br needs one electron to complete its octete while Si needs 4 hence the formula of compound will be `SiBr_(4)`. |
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| 56. |
Predict the position of an element with atomic number 55 in the periodic table and explain the chemical behaviour of tha element. |
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Answer» (i) electronic configuration of the element and predict group and period (ii) correlation between the position of the element ltbegt in the periodic table and its chemical behaviour |
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| 57. |
There is a sharp decrease in the ionisation energies from boron to aluminium but it is almost the same from aluminium to gallium. Justify. |
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Answer» Among IIIA group elements, boron has the highest ionisation potential due to smaller size. The sharp decrease in ionisation energy from boron to aluminium is due to increase in atomic radius. The atomic radius increases due to decrease in effective nuclear charge. In gallium contraction in atomic size is significant due to the presence of completely filled d-electrons in the penultimate shell. Thus. The effective nuclear charge increases. Hence, both aluminium and gallium have almost equal ionisation energy values. |
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| 58. |
Therr elements A, B and C have atomic numbers as x,x + 1 and x + 2. The atomic size of C is greater than that of B but positions of B is less than that of A. Predict the positions of A, B amd C in the periodic table and justify the trend in atomic size. |
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Answer» As the atomic numbers of A,B and C differ by 1 unit each they must be belonging to adjacent group. Along a period the atomic size decreases till the VII A group and then increases till the zero group. As the atomic size of C is greater than B though it differs by one unit in its atomic number it must be a zero group element. Though the atomic number of B is greater than A, it has smaller size than Band this shows that B is a halogen, that is VII A group and A chalcogen, that is, VI A group. |
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| 59. |
Lanthanoids are-A. 14 elements in the seventh period (Atomic no. =58 to 71) that are filling 4f subshellB. 14 elements in the sixth period (atomic no. = 90 to 103) that are filling 4f subshellC. 14 elements in the seventh period (atomi no. = 90 to 103) that are filling 5f subshellD. 14 elements in the sixth period (atomic no = 58 to 71) that are filling 4f subshell |
| Answer» Correct Answer - D | |
| 60. |
For the process `X(g) +e^(-) rarr X^(-)(g), DeltaH = x` and `X^(-)(g) rarr X(g) +e^(-), DeltaH = y` Select correct alternate :A. ionisation energy of `X^(-)(g)` is yB. electron affinity of `X(g)` is xC. electron affinity of `X(g)` is yD. all are correct statements |
| Answer» Correct Answer - D | |
| 61. |
Sodium forms `Na^(+)` ion but it does not form `Na^(+2)` because -A. Very low value of `IE_(1)` and `IE_(2)`B. Very high value of `IE_(1)` and `IE_(2)`C. High value of `IE_(1)` and low value of `IE_(2)`D. Low value of `IE_(1)` and high value of `IE_(2)` |
| Answer» Correct Answer - D | |
| 62. |
For the process `X(g) +e^(-) rarr X^(-)(g), DeltaH = x` and `X^(-)(g) rarr X(g) +e^(-), DeltaH = y` Select correct alternate :A. Ionization energy of `X^(-)(g)` is yB. Electron affinity of `X(g)` is xC. Electron affinity of `X(g)` is -yD. All are correct statements |
| Answer» Correct Answer - D | |
| 63. |
The actinoids exhibit more number of oxidation states in general than the lanthanoids. This is becauseA. the 5f orbitals are more buried than the 4f orbitalsB. there is a similarly between 4f and 5f orbitals in their angular part of the wave functionC. the actinoids are more reactive than the lanthanoidsD. the 5f orbitals extend farther from the nucleus than the 4f orbitals |
| Answer» Correct Answer - D | |
| 64. |
Which of the following is not a representative elementA. SodiumB. BoronC. CalciumD. Chromium |
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Answer» Correct Answer - D |
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| 65. |
Whichone of the following is not the representative element ?A. FeB. KC. BaD. N |
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Answer» Correct Answer - 1 Elements of group `1,2,13,14,15,16,17` are reperesentative elements. |
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| 66. |
Which of the following statements are correct?A. Helium has the highest first ionisation enthalpy in the periodic tableB. Chlorine has less negative electron gain enthalpy than fluorineC. Mercury and bromine are liquids at room temperatureD. In any period, atomic radius of alkali metal is the highest |
| Answer» Correct Answer - A::C::D | |
| 67. |
Which of the following is not the electronic configuration of a representative elementA. `ns^(2)`B. `ns^(2)np^(5)`C. `ns^(2)np^(1)`D. `ns^(2)np^(6)` |
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Answer» Correct Answer - D |
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| 68. |
Which of the following elements will gain one electron more readily in comparison to other elements of their group?A. `S(g)`B. `Na(g)`C. `O(g)`D. `CI(g)` |
| Answer» Correct Answer - A::D | |
| 69. |
The grneral electronic configuration of representative elements isA. (a) `ns^(1-2) np^(1-6)`B. (b) `ns^(1-2) np^(1-5)`C. (c) `ns^(1-2) (n-1)p^(1-5)`D. (d) `ns^(1-2) (n-1)p^(1-6)` |
| Answer» Correct Answer - C | |
| 70. |
Which of the following sequences contain atomic numbers of only representative elements?A. 3,33,53,87B. 2,10,22,36C. 7,17,25,37,48D. 9,35,51,88 |
| Answer» Correct Answer - A::D | |
| 71. |
The dominating factor responsible for the decreasing ionisation energies of the elements on moving down the group is `:`A. atomic radiusB. type of electron to be removedC. the valence shell electron configurationD. all of these |
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Answer» Correct Answer - 1 As size of atom increases the distance between the nucleus and valence shell electron increases. As a result of this the attraction between nucleus and valence shell electron decreases. Hence less energy is required for the removal of the valence shell electron. So down the group ionisation energies decreases. |
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| 72. |
Those elements impart colour to the flame on heating in it, the atoms of which require low energy for the ionisation (i.e., absorb energy in the visible region of spectrum). The elements of which of the following groups will impart colour to the flame?A. 2B. 13C. 1D. 17 |
| Answer» Correct Answer - A::C | |
| 73. |
Those elements impart colour to the flame on heating in it, the atoms of which require low energy for the ionisation (i.e. absorb energy in the visible region of spectrum). The elements of which of the following groups in Modern periodic table will impart colour to the flame?A. 2B. 13C. 1D. 17 |
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Answer» Correct Answer - A::C Elements of Group 1 & 2 have low `IE` have. So they impart colour to flame. `E.g. Li, Na, K, Ca, Ba`, etc. |
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| 74. |
Which of the following would require least energy?A. `Si^(-)(g) rarr Si(g)+e^(-)`B. `P^(-)(g)rarr P(g)+e^(-)`C. `S^(-)(g) rarr S(g) +e^(-)`D. `CI^(-)(g) rarr CI(g) +e^(-)` |
| Answer» Correct Answer - B | |
| 75. |
Which of the following will have the most negative electron gain enthalpy and which the least negative? `P, S, Cl, F`. Explain your answer.A. `F,CI`B. `CI,F`C. `CI,S`D. `CI,P` |
| Answer» Correct Answer - D | |
| 76. |
Which is least for an elementA. `I_(1)`B. `I_(2)`C. `I_(3)`D. `I_(4)` |
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Answer» Correct Answer - A |
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| 77. |
In a given energy level, the order of penetration effect of different orbitals isA. `f lt p lt d lt s`B. `s lt p lt d lt f`C. `f lt d lt p lt s`D. `s = p = d = f` |
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Answer» Correct Answer - C The order of penetration effect of different orbitals depends upon the different energies of the various subshells for the same energy level, e.g. electrons in s-subshell will have lowest energy and thus will be closest to the nucleus and will have highest penetration power, while p-subshell electrons will penetrate the electron cloub to lesser extent and so on. |
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| 78. |
Screening effect is not observed in :A. `He^(+)`B. `Li^(2+)`C. `Be^(3+)`D. In all cases |
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Answer» Correct Answer - D `He^(+),1s^(1), Li^(2+), 1s^(1), Be^(3+), 1s^(1)`. All these ions have only one electron. So they do not have any inner orbital and thus do not experience any screening effect. |
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| 79. |
The screening effect of `d`-electron isA. Equal to the p-electronsB. Much more than the p-electronsC. Same as f-electronsD. Less than the p-electrons |
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Answer» Correct Answer - D |
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| 80. |
The screening effect of `d`-electron isA. equal to the p-electronsB. much more than p-electronC. same as f-electronsD. less than p-electrons |
| Answer» Correct Answer - D | |
| 81. |
Which of trhe following statements is not correct?A. The first inoisation energies (in ` KJ "mol"^(-1)`) of carbon, silicon , germanium , tin, and lead are 1086, 786,761,708 and 715 respectively:B. Down the group , electronegativity dereases from B to T1 in boron family.C. Among oxides of the elements of carbon family CO is neutral , GeO is acidic and SnO is amphoteric.D. The 4f and 5f inner transition elements are placed seperately at the bottom of the periodic table to maintain its struction. |
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Answer» Correct Answer - A::C::D |
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| 82. |
Due to screening effect of electrons in an atomA. Decrease in the ionisation energyB. Increases in the ionisation energyC. No effect on the ionisation energyD. Increases in the attraction of the nucleus to the electrons |
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Answer» Correct Answer - A The attraction of the nucleus with the electron decreases so it becomes easy to extract the electron. |
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| 83. |
The screening effect of d-electrons isA. Less than p - electrons but more than s and f - electronsB. Less than p and s - electrones but more than f - electronsC. Less than f - electrons but than s and p - electronsD. Equal to s and p - electrons |
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Answer» Correct Answer - B |
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| 84. |
The screening effect of inner electrons of an atom can causeA. decrease in ionization energyB. increase in effective nuclear chargeC. increase in ionisation energyD. decrease in atomic size |
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Answer» Correct Answer - A::B |
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| 85. |
Calculate the lattice energy of `NaCI` crystal from the following data by the use of Born-Haber cycle. Sublimation energy of `Na = 26 kcal//g`atom, dissociation energy of `CI_(2) = 54 kcal//"mole"`, ionisation energy of `Na(g) = 117 kcal//"mol"`, electron affinity for `CI(g) = 84 kcal//g` atom, heat of formation of `NaCI =- 99 kcal//"mole"`. |
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Answer» Correct Answer - `[-185 kcal//"mole"]` `[(DeltaH)_("formation") = (DeltaH)_("sub") +I.E. +(DeltaH)_(eg) +1//2 (DeltaH)_("diss") +U]` |
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| 86. |
The correct order of atomic radii of the following element `Sm(z=62), Eu (z=63), Gd (z=64), Lu(z=71)`A. `Sm gt Eu gt Gd gt Lu`B. `Sm lt Eu lt Gd lt Lu`C. `Eu gt Sm gt Gd gt Lu`D. `Sm gt Gd gt Lu gt Lu` |
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Answer» Correct Answer - C |
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| 87. |
Unniltrium belongs to which block and group of the periodic table?A. d-block, group -10B. f-block,group 3C. p-block, group-13D. d-block,group-11 |
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Answer» Correct Answer - B `Z = 103` is an actinide |
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| 88. |
Which element has the greatest electrical conductivity?A. AsB. GeC. PD. Sn |
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Answer» Correct Answer - D Sn is a metal (good coductor of electricity) |
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| 89. |
Which of the following elements posses zero electron affinity (theriotically) and zero electronegativity values?A. HalogensB. Alkali metalsC. ChalcogensD. Rare gases |
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Answer» Correct Answer - D |
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| 90. |
An atom with atomic number 21 belongs to the category ofA. s- block elementsB. p-block elementsC. d-block elementsD. f-block elements |
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Answer» Correct Answer - C |
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| 91. |
How many of the following are more electronegativity than Boron. `H, Li, Be, C, N, O, F` |
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Answer» Correct Answer - 5 `H, C, N, O, F` |
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| 92. |
The correct order of electronegativity on Pauling scale is:A. `F gt CI gt O gt S`B. `Li gt Na gt L gt Rb gt Cs`C. `Be lt B lt N lt C`D. Both `(A)` and `(B)` |
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Answer» Correct Answer - B Electronegativity of elements generally across the period (less increase) and decreases down the group (more decreases.) |
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| 93. |
Fluorine has the highest electronegativity among the `ns^(2) np^(5)` group on the Pauling scale, but the elctron affinity of fluorine is less than that of chlorine because `:`A. The atomic number of fluorine is less than that of chlorineB. fluorine being the first member of the family behaves in an unusual manner.C. chlorine can accommodate an electron better than fluorine by utilising its vacant `3d-`orbitalD. small size, high electron density and an increased electron repulsion makes addition of an electron to fluorine less favourable than that in the case of chlorine in isolated stage. |
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Answer» Correct Answer - 4 There is more interelectronic repulsion in `2p-` subshell of fluorine than chlorine `(3p)`. So extra electron will added easily in `3p-` subshell of chlorine as compared to `2p-` subshell of fluorine. |
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| 94. |
Pauling scale of electronegativity of elements helps to determineA. Covalent nature of an elementB. Position of an element in EMF seriesC. Dipole moment of moleculesD. Polarity of bond |
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Answer» Correct Answer - C |
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| 95. |
Regarding the electronegativity (i) The element with maximum electornegativity: Fluorine (ii) In Pauling scale, the reference element is: Silicon (iii) Elements with stable configuration have high electronegativity (iv) the electron with maximum electronpositivity: HydrogenA. Only (i) correctB. Only (ii) correctC. only (iii) correctD. Only (iv) is correct |
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Answer» Correct Answer - A |
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| 96. |
Consider the following statements. Statement-1: Fluorine does not form any polyhalide as it has low F-F bond energy. Statement-2: The chlorine has the most negative electron gain enthalpy. Statement-3: The first ionization potentials of N and O atoms are 14.6 and 13.6eV respectively. Which of the above statements are correct?A. Statements 1,2 and 3B. Statement 1 and 2C. Statement 1 and 3D. Statements 2 and 3 |
| Answer» Correct Answer - A | |
| 97. |
Which of the following are the correct statements (I) EA of noble gases is endothermic (II) EA of Fluorine is less than chlorine (III) EA of oxygen is less than sulphur (IV) EA of N is more than phosphorous The correct answer isA. I,II,III and IVB. I, II and IIIC. II and IVD. I and IV |
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Answer» Correct Answer - B |
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| 98. |
Why is electron affinity of chlorine more than that of fluorine? |
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Answer» (i) factors affecting electron affinity (ii) electronic configuration of chlorine and fluorine (iii) comparison of the number of valence electrons with respect to the atomic size between chlorine and fluorine |
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| 99. |
The electron affinity of bromine atom is equal to the..........of bromide ionA. ionisation potentialB. Electron affinityC. effective nuclear chargeD. electron negative |
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Answer» Correct Answer - A |
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| 100. |
Which systematic diagram representsthe correct sequence of physical properties ? No Property 1) Electronegativity 2) Metallic property 3) Atomic radiusA. `Li underset((2,3) "Decrease")overset((1)"Increase")rarrBe` `{:((1)"Decrease" ,(1) "Increase "),((2,3)"Increase",(2,3)"Decrease"):}` `Cunderset((2,3)"Increase")overset((1)"Decrease")rarr B`B. `Li underset((2,3) "Increase")overset((1)"Decrease")rarrBe` `{:((1)"Increase" ,(1) "Decrease"),((2,3)"Decrease",(2,3)"Increase"):}` `Cunderset((2,3)"Increase")overset((1)"Decrease")rarr B`C. `Li underset((2,3) "Decrease")overset((1)"Increase")rarrBe` `{:((1)"Decrease" ,(1) "Increase "),((2,3)"Increase",(2,3)"Decrease"):}` `Cunderset((2,3)"Decrease")overset((1)"Increase")rarr B`D. `Li underset((2,3) "Increase")overset((1)"Decrease")rarrBe` `{:((1)"Decrease" ,(1) "Increase "),((2,3)"Increase",(2,3)"Decrease"):}` `Cunderset((2,3)"Increase")overset((1)"Decrease")rarr B` |
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Answer» Correct Answer - C |
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