Which of the following arrangements of elements is correct in terms of increasing atomic radius?

On moving down a group, atomic radius increases as the number of shells increases. Li (Z = 3), Be (Z = 4) and B (Z = 5) belong to the 2^nd period. On moving across the period from Li to B, size will decrease. So, their correct order in terms of increasing atomic radius is B < Be < Li. Moreover, N (Z = 7), O (Z = 8) and F (Z = 9) belong to the 2^nd period. On moving from N to F, atomic radius will decrease. So, their correct order is F < O < N. Similarly, Na (Z = 11), Mg (Z = 12) and Al (Z = 13) belong to the 3^rd period. On moving from Na to Al, atomic radius will decrease. So, their correct order is Al < Mg < Na. F (Z = 9), Cl (Z = 17) and Br (Z = 35) belong to the 17^th group and from F to Br, the atomic radius will increase. So, their correct order in terms of increasing atomic radius is F < Cl < Br. Therefore, only option (4) is correct.