The increasing order of the atomic radii of the
following elements is:
(a) C (b) O (c) F (d) Cl e) Br

The increasing order of atomic radii of the elements (a) C, (b) O, (c) F, (d) Cl, and (e) Br can be determined based on periodic trends in the periodic table.

Periodic Trends

1. Moving down a group: As we move down a group in the periodic table, the atomic radius increases. This occurs because additional electron shells are added, increasing the distance between the nucleus and the outermost electrons.

2. Moving left to right across a period: As we move from left to right across a period, the atomic radius decreases. This is due to the increasing nuclear charge, which pulls the outermost electrons closer to the nucleus.

Explanation of the Increasing Order of Atomic Radii

The elements F (fluorine), O (oxygen), and C (carbon) belong to the same period (Period 2). Within a period, the atomic radius decreases as we move from left to right. Therefore, the increasing order of atomic radii for these elements is:

F < O < C

Similarly, the elements F (fluorine), Cl (chlorine), and Br (bromine) belong to the same group (Group 17). Within a group, the atomic radius increases as we move down. Hence, the increasing order of atomic radii for these elements is:

F < Cl < Br

Final Increasing Order

By combining the trends for elements within the same period and group, the overall increasing order of atomic radii for the given elements is:

F < O < C < Cl < Br

Conclusion

The increasing order of atomic radii explains the periodic trends in atomic sizes effectively. Thus, the correct answer is option (d).