Classification of Elements and Periodicity in Properties

Q1. Which of the following elements will gain one electron more readily in comparison to other elements of their
group?

1. S(g)
2. Na(g)
3. O(g)
4. Cl(g)

Q2. Periodic classification of elements can be done on the basis of electronic configuration and is used to examine
the:

1. Periodic trends in physical properties of elements.
2. Periodic trends in chemical properties of elements.
3. Both (a) and (b).
4. None of the above.

Q3. An element belongs to 3 period and group-13 of the periodic table. Which of the following properties will be
shown by the element?

1. Good conductor of electricity.
2. Liquid, metallic.
3. Solid, metallic.
4. Solid, non metallic.

Q4. Mendeleev’s left the gap nder aluminium and a gap under silicon having atomic weights 68 and 72 respectively.
These elements respectively are:

1. Eka-aluminium and Eka-silicon.
2. Aluminium and silicon.
3. Eka-germanium and Eka-silicon.
4. Eka-aluminium and Eka-germanium.

Q5. Which of the following requires highest energy?

1. M(g) → M⁺ (g)
2. M(g) → M²⁺ (g)
3. M(g) → M³⁺ (g)
4. M(g) → M⁴⁺ (g)

Q6. According to IUPAC, total number of groups and periods in the periodic table respectively are:

1. 16, 9
2. 18, 7
3. 18, 9
4. 13, 7

Q7. Which of the following statements are correct?

1. Helium has the highest first ionisation enthalpy in the periodic table.
2. Chlorine has less negative electron gain enthalpy than fluorine.
3. Mercury and bromine are liquids at room temperature.
4. In any period, atomic radius of alkali metal is the highest.

Q8. The oxide formed by the element on extreme right and in the left of periodic table are generally:

1. Acidic, amphoteric respectively.
2. Acidic, basic respectively.
3. Neutral, amphoteric respectively.
4. Basic, neutral respectively.

Q9. What effect is observed, on the size of an atom when an electron is removed and in another case an electron is
added to the same atom?

1. Size increases and decreases respectively.
2. Size decreases and increases respectively.
3. Size increases in both cases.
4. Size decreases in both cases.

Q10. Which among the following sets of groups consist elements with high chemical reactivity?

1. Groups-1 and 11
2. Groups-11 and 17
3. Groups-1 and 17
4. Groups-11 and 18

Q11. The ions with the positive charge or negative charge will have the radius, respectively:

1. Smaller or greater.
2. Greater or smaller.
3. Remains same.
4. None of these.

Q12. The element with positive electron gain enthalpy is:

1. Hydrogen.
2. Sodium.
3. Oxygen.
4. Neon.

Q13. Choose the correct order of atomic radii of fluorine and neon (in pm) out of the options given below and justify
your answer.

1. 72, 160
2. 160, 160
3. 72, 72
4. 160, 72

Q14. Which of the following radii reflect an increase in size of an atom?

1. Van der Waals’ radius.
2. Metallic radius.
3. Covalent (non-metallic) radius.
4. Both (b) and (c).

Q15. Who developed the long form of the periodic table?

1. Niels Bohr.
2. Moseley.
3. Mendeleef.
4. Lothar Meyer.

Q16. Elements are classified into four blocks like s-block, p-block, d-block and f-block on the basis of:

1. Atomic number.
2. Atomic mass.
3. Atomic orbitals.
4. All of these.

Q17. 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?

1. 2
2. 13
3. 1
4. 17

Q18. Which of the following sequences contain atomic numbers of only representative elements?

1. 3, 33, 53, 87
2. 2, 10, 22, 36
3. 7, 17, 25, 37, 48
4. 9, 35, 51, 88

Q19. The nature of normal oxide formed by the element present on extreme left in the periodic table is:

1. Most acidic.
2. Most basic.
3. Amphoteric.
4. Neutral.

Q20. The ability of an atom in a chemical compound to attract shared electron is termed as:

1. Electron affinity.
2. Ionisation enthalpy.
3. Atomic attraction.
4. Electronegativity.

Q21. Which of the following groups of elements have highly negative electron gain enthalpy?

1. Group-16
2. Group-17
3. Group-14
4. Both (a) and (b).

Q22. Which of the following properties is inversely related to electronegativity?

1. Non-metallic properties.
2. Metalloid properties.
3. Ionic properties.
4. Metallic properties.

Q23. Ionic radii vary in:

1. Inverse proportion to the effective nuclear charge.
2. Inverse proportion to the square of effective nuclear charge.
3. Direct proportion to the screening effect.
4. Direct proportion to the square of screening effect.

Q24. Half the internuclear distance separating the metal cores in the metallic crystal is termed as:

1. Metallic radius.
2. Atomic radius.
3. Covalent radius.
4. Ionic radius.

Q25. The statement that is not correct for periodic classification of elements is:

1. The properties of elements are periodic function of their atomic numbers.
2. Non metallic elements are less in number than metallic elements.
3. For transition elements, the 3d-orbitals are filled with electrons after 3p orbitals and before 4s-orbitals.
4. The first ionisation enthalpies of elements generally increase with increase in atomic number as we go along
   a period.

Q26. The horizontal rows and the vertical columns in the periodic table are termed as respectively?

1. Periods, groups.
2. Groups, periods.
3. Series, periods.
4. Family, periods.

Q27. Which important property did Mendeleev use to classify the elements in his periodic table?

1. Atomic weight.
2. Atomic number.
3. Melting point.
4. None of these.

Q28. Why do elements in the same group have similar physical and chemical properties?

1. Because of same electronic configuration.
2. Because of same number of electrons.
3. Because of same number of protons.
4. Because of same valence electrons.

Q29. The symbol and name according to the IUPAC system for the element with atomic number = 120, respectively
are:

1. Ubn and unbinilium.
2. Ubn and unbiunium.
3. Ubn and unnilbium.
4. Ubn and unnilium.

Q30. In general second ionisation enthalpy of an atom will be:

1. Higher than the first ionisation enthalpy.
2. Equal to the first ionisation enthalpy.
3. Higher than the third ionisation enthalpy.
4. Equal to the third ionisation enthalpy.