Classification Of Elements And Periodicity In Properties – Multiple Choice Questions

Q1. Identify the smallest ion among the following:

  1. Na+
  2. Mg2+
  3. K+
  4. Al3+

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Q2. For noble gases radius is measured as:

  1. Ionic radius
  2. Metallic radius
  3. van der Waals radius
  4. Atomic radius

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Q3. Among the following elements element with highest ionisation enthalpy is:

  1. O
  2. C
  3. N
  4. B

Answer :- (3)

Q4. The Latin word commonly used for the digit 9 is:

  1. Nil
  2. Quad
  3. Hex
  4. Enn

Answer :- (4)

Q5. Moseley performed experiments and studied the frequencies of which radiations emitted from the elements?

  1. Gamma rays
  2. X-rays
  3. Infra red rays
  4. UV rays

Answer :- (2)

Q6. How many valence electrons does a carbon atom have?

  1. 6
  2. 4
  3. 3
  4. 2

Answer :- (2)

Q7. Lithium shows diagonal relationship with which element?

  1. Beryllium
  2. Sodium
  3. Magnesium
  4. Silicon

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Q8. What is the relationship between the number of elements in each period and the number of atomic orbitals available in the energy level that is being filled?

  1. Number of elements is twice the number of atomic orbitals.
  2. Number of elements is same as the number of atomic orbitals.
  3. Number of elements is three times the number of atomic orbitals.
  4. Number of elements is half the number of atomic orbitals.

Answer :- (1)

Q9. In Na2O oxidation state of oxygen is:

  1. +2
  2. +1
  3. -1
  4. 0

Answer :- (1)

Q10. The systemic name for an element with atomic number (Z = 118) is:

  1. Unnilunium
  2. Ununhexium
  3. Ununoctium
  4. Unbinilium

Answer :- (2)

Q11. Oxygen exhibits +2 oxidation state in the compound:

  1. H2O
  2. Na2O
  3. OF2
  4. MgO

Answer :- (3)

Q12. The 3d transition series starts from which atomic number?

  1. 19
  2. 20
  3. 21
  4. 22

Answer :- (3)

Q13. Elements of Group-1 are called:

  1. Alkaline earth metals
  2. Chalcogens
  3. Alkali metals
  4. Halogens

Answer :- (3)

Q14. Elements in the same vertical group of the Modern Periodic Table have same:

  1. Number of electrons
  2. Atomic number
  3. Number of protons
  4. Electronic configuration of the outermost shell

Answer :- (1)

Q15. The p-block elements constitute elements belonging to which groups?

  1. Group 1 to 18
  2. Group 10 to 14
  3. Group 1 to 13
  4. Group 13 to 18

Answer :- (4)

Q16. The nature of bonds in the compounds of carbon is mostly:

  1. Covalent
  2. Electrovalent
  3. Covalent as well as electrovalent
  4. Metallic

Answer :- (1)

Q17. Lothar Meyer proposed that on arranging the elements in order of increasing atomic weights; similarities appear in which type of properties?

  1. In both physical and chemical properties
  2. Only physical properties
  3. Only chemical properties
  4. thermodynamic properties

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Q18. The fourth period involves the filling of  

  1. 5s, 4d, and 4p orbitals.
  2. 4s, 3d, and 4p orbitals.
  3. 3s, 4d, and 4p orbitals.
  4. 4s, 4d, and 4p orbitals.

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Q19. Electrons in an orbital are filled according to which rule?

  1. n+n
  2. L+m
  3. n + l
  4. m+l

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Q20. Electron gain enthalpy values of noble gases are positive because:

  1. They are all gases
  2. They have smallest size
  3. They are monoatomic
  4. They have stable electronic configuration

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Q21. Tendency of an atom in a molecule to attract the shared pair of electron towards itself is called:

  1. Periodicity
  2. Electronegativity
  3. Ionisation enthalpy
  4. Electron gain enthalpy

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Q22. The maximum covalence of the first member of each group is:

  1. 2
  2. 4
  3. 6
  4. 8

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Q23. Which of the following is isoelectronic with F?

  1. Ne
  2. Ar
  3. Mg+
  4. Cl

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Q24. The correct electronic configuration of an alkaline earth metal can be:

  1. [Ne]3s2 3p2
  2. [Ar]3d10 4s2
  3. [Ar]3d10 4s1
  4. [Ar] 4s2

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Q25. Anion O– is isoelectronic with:

  1. N2-
  2. F
  3. N3-
  4. Ne

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Q26. Johann Dobereiner classified elements in group of three elements called as

  1. Diads
  2. Triads
  3. Trinity
  4. Trials

Q27. What is the principal quantum number for second period?

  1. 1
  2. 3
  3. 2
  4. 4

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Q28. Which of the following elements will have the largest atomic radii?

  1. Li
  2. Al
  3. Ca
  4. Sr

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Q29. Elements of which group are called Halogens?

  1. Group 15
  2. Group 16
  3. Group 17
  4. Group 18

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Q30. Mendeleev predicted the existence of which element/elements in the periodic table?

  1. Gallium
  2. Sodium and germanium
  3. Gallium and germanium
  4. Germanium and Gold

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Q31. Group 2 elements are:

  1. Oxidizing agents
  2. Reducing agents
  3. Oxidizing as well as reducing agents
  4. Neither oxidizing nor reducing agents

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Q32. On moving down a group the number of valence electrons:

  1. Increases
  2. Remains the same
  3. Decreases
  4. Decreases and then increases

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Q33. The largest atomic radius among the following is of:

  1. Na
  2. K
  3. Mg
  4. Ca

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Q34. Among the following elements, an element that is named after a famous scientist is:

  1. Carbon
  2. Uranium
  3. Fermium
  4. Thorium

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Q35. Na+ is smaller than Na atom because:

  1. Nucleus in each case contains different nucleons.
  2. Sodium atom has one electron lesser than sodium ion.
  3. The effective nuclear charge is greater in case of sodium ion.
  4. Na+ is more stable than in Na atom.

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Q36. Which scientist proposed that atomic number is more fundamental property of an element than its atomic mass?

  1. Meyer
  2. Moseley
  3. Lothar Meyer
  4. Newlands

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Q37. Isoelectronic species have:

  1. Same number of electrons
  2. Same number of protons
  3. Same number of neutrons
  4. Same atomic mass

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Q38. Lothar Meyer arranged the elements in order of increasing:

  1. Atomic weight
  2. Atomic radii
  3. Atomic volume
  4. Density

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Q39. Sodium forms which types of oxides?

  1. Neutral
  2. Amphoteric
  3. Acidic
  4. Basic

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Q40. Consider the following reaction 2A + 3F2 → 2AF3.

What is the formula for the reaction product if we substitute iodine for fluorine?

  1. A2I3
  2. A3I2
  3. AI3
  4. AI

Answer :- ()

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