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Chemistry Practice Questions: Classification of Elements, Periodic Table and Periodicity in Properties (Syllabus)

Genesis of Periodic Classification, Earlier Attempts of Classification of Elements, Mendeleev’s Periodic Law and Original Periodic Table, Modern Periodic Law and Long Form of Periodic Table, (Modified Form of Mendeleev’s Periodic Table), Naming the Elements, Periodic Table of Elements (Long Form representing Electron Configurations), Position of an Element on the Basis of Electronic Configuration, Nomenclature of Elements with Atomic Number > 100, Electronic Configurations of Elements and the Periodic Table, Periodic Trends in Properties of Elements or Atomic Properties or Periodic Properties of Elements, The Screening Effects or Shielding Effect, Effective Nuclear Charge, Ionisation Enthalpy or Ionisation Potential, Atomic Radii, Ionic Radii, Ionization Enthalpy, Electron Gain Enthalpy, Electron Affinity, Electronegativity, Valence, Electronic Configurations and Types of Elements: s, p, f-Blocks

Chemistry: Classification of Elements, Periodic Table and Periodicity in Properties

Multiple Choice Questions (MCQs) – Set 2 (Q. No. 11-20)

Question 11: Rare earths are generally
a. Actinides                            b. f-Block elements 
c. Inner transition elements   d. Lanthanides

Question 12: Amongst the elements with following electronic configurations, which one of them may have the highest ionization energy?
a. Ne [3s2 3p1]        b. Ne [3s2 3p3]  
c. Ne [3s2 3p2]        d. Ar [3d10 4s2 4p3]

Question 13: The ionisation energy will be higher when the electron is removed from _____ if other factors being equal.
a. s-orbital   b. p-orbital   c. d-orbital   d. f-orbital

Question 14: The elements with atomic numbers 10, 18, 36, 54 and 86 are all:
a. light metals   b. inert gases   c. halogens   d. rare-earths

Question 15: The starting element and last element in the largest period in modern periodic table are
a. Rb and Xe   b. Cs and I   c. Cs and Rn   d. Fr and Kr

Question 16: The first, second and third ionisation energies of Al are 578, 1817 and 2745 kJ mol- respectively. Calculate the energy required to convert all the atoms of Al to Al+3 present in 270 mg of Al vapours
a. 5140 kJ   b. 51.40 kJ   c. 2745 kJ   d. 514.0 kJ

Question 17: The set representing the correct order of first ionisation potential is:
a. K > Na > Li      b. Be > Mg > Ca  
c. B > C > N        d. Ge > Si > C 

Question 18: Which among the following element have lowest value of first ionization energy?
a. Pb   b. Sn   c. Si   d. C

Question 19: Which one of the following oxides is neutral?
a. CO     b. SnO2     c. ZnO     d. SiO2

Question 20: The correct order of the metallic character is:
a. Na > Mg > Al > Si        b. Mg > Na > Al > Si
c. Al > Mg > Na > Si        d. Si > Al > Na > Mg

Classification of Elements, Periodic Table and Periodicity in Properties
Solutions of Practice Questions Set 2 (Q. No. 11 - 20)

Answer 11: (d)   Answer 12: (b)   Answer 13: (a)   Answer 14: (b)   Answer 15:(c)   Answer 16:(b)     Answer 17: (b) Hint: Down the group the effective nuclear charge remains almost constant. But down the group with increasing atomic number the number of atomic orbits increases and there by atomic size increases. As a result, the distance of valence shell electron from nucleus increases and attraction between them decreases and therefore ionization energy decreases.
Answer 18: (b)   Answer 19: (a) Hint: CO is neutral towards litmus. SnO2 and ZnO are amphoteric as they form salts and water with acids and bases. SiO2 is acidic as it forms salts with bases.
SiO2 + 2NaOH → Na2SiO3 + H2O.
Answer 20: (a) Hint: The metallic character of the elements is highest at the extremely left (low ionisation energies) and then decreases across the period from left to right (ionisation energies increases across the period)

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