ECAT Chemistry Chapter 12 Periodic Classification of Elements and Periodicity Online Test With Answers

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ECAT Chemistry Chapter 12 Periodic Classification of Elements and Periodicity Online Test

Sr. # Questions Answers Choice
1 Among the elements given below, the one with highest electropositivity is Cu Cs Cr Ba
2 The correct arrangement of increasing order of atomic radius among Na, K, Mg, Rb is Mg < K < Na < Rb Mg < Na < K < Rb Mg < Na < Rb < K Na < K < Rb < Mg
3 Alkali metals in each period have Smallest size Lowest IE Highest IE Highest electronegativity
4 The element with atomic number 55 belongs to which block of the periodic table s-block p-block d-block f-block
5 The attraction that an atom exerts on a pair of electrons that are being shared with another atom for forming covalent bond is referred to as its Electron affinity Electronegativity Ionisation energy Valency
6 Among O, C, F, Cl, Br, the correct order of increasing radii is F O C Cl Br F C O Cl Br F Cl Br O C C O F Cl Br
7 Among the following elements which one has the highest value of first ionization potential? Oxygen Argon Barium Cesium
8 The element with atomic number 26 will be found in group 2 8 6 10
9 Which of the following pair of atomic numbers represents s-block elements? 7, 15 6, 12 9, 17 3, 20
10 The valence shell electronic structure of an element is ns2np5. The element will along to the group of Alkali metals Inert metals Noble gases Halogen
11 The valency of noble gases, in general, is Zero One Three Two
12 Which among the following elements have lowest value of IE1? Pb Sn Si C
13 Of the given alkali metals, the one with smallest size is Rb Cs K Na
14 Which of the following elements is/are not liquid at 30°C? Ga Hg Ge Cs
15 Which of the following metal requires radiation of highest frequency to cause emission of electrons? Na Mg K Ca
16 Which of the following does not reflect the periodicity of elements? Bonding behaviour Electronegativity Ionisation potential Neutral/proton ratio
17 Which of the following has greatest tendency to lose electron? F Fr S Be
18 Which of the following elements is most electronegative? Oxygen Chlorine Nitrogen Fluorine
19 The alkali metal which is liquid at 15°C is K Cs Na None
20 Which of the following pairs are chemically dissimilar? Na and K Ba and Sr Zr and Hf Ca and Zn
21 Variable valency is generally exhibited by Normal elements Transition elements Metallic elements None of these
22 Which of the following statements is most appropriate about effective nuclear charge? It depends upon The shielding constant The atomic number The charge on the nucleus Both the nuclear charge and the shielding constant
23 Which of the following represents elements in order of increasing atomic size? I, Br, Cl Na, Mg, C C, N, O Li, Na, K
24 The chloride of element Q is hydrolysed by water to form an acidic solution and its oxide reacts with acid to form a salt.
What cold be the element Q
 Magnesium Aluminium Silicon Phosphorus
25 Which statement explains the observation that magnesium hydroxide dissolve in aqueous ammonium chloride, but not in aqueous sodium chloride The ionic radius of the NH<sub>4</sub><sup>+</sup>ion is similar to that of Mg<sup>2+</sup>but not that of Na<sup>+</sup> NH<sub>4</sub>Cl dissociates less fully than NaCl The ions Na<sup>+</sup>and Mg<sup>2+</sup>are isoelectronic (have the same number of electrons) The ion NH<sup>+</sup><sub>4</sub>acts as an acid
26 An element of the third period (Na to S) is heated in chlorine. The product is purified and then added to water. The resulting solution is found to be neutral. What is the element Sodium Aluminium Silicon Phosphorus
27 Which of the following oxides is unlikely to dissolve in aqueous hydroxide Al<sub>2</sub>O<sub>3</sub> MgO SO<sub>2</sub> SIO<sub>2</sub>
28 Which species represented by the following formula has the largest radius P<sup>3-</sup> Cl<sup>-</sup> A<sub>r</sub> K<sup>+</sup>
29 NaBH4and LialH4are Ionic hydrides Covalent hydrides Interposal hydrides Complex hydrides
30 Ionization potential increases in moving from left to right in a period Because nuclear charge increase Because atomic size decrease Both (a) and (b) Because atomic size increases
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