The atomic radii of the elements of the second period are given below:

Second period elements	$B$	$Be$	$O$	$N$	$Li$	$F$	$C$
Atomic Radii $(pm)$	$88$	$111$	$66$	$74$	$152$	$64$	$77$

$(i)$ Arrange these elements in decreasing order of their atomic radii.
$(ii)$ Are the elements now arranged in the pattern of a period in the periodic table?
$(iii)$ Name the element which has the $(a)$ smallest and $(b)$ largest atomic number.
$(iv)$ From the above data, infer how the atomic size or atomic radius of the elements changes as we move from left to right in a period.
$(v)$ Name one metal, one non-metal, and a metalloid out of these elements.
$(vi)$ Why does atomic radius decrease as we move from left to right in a period?

(N/A) $(i)$ The decreasing order of atomic radii is: $Li (152) > Be (111) > B (88) > C (77) > N (74) > O (66) > F (64)$.
$(ii)$ Yes, the elements are now arranged in the order of a period in the periodic table (from left to right).
$(iii)$ $(a)$ The element with the smallest atomic number is $Li$ (atomic number $3$).
$(b)$ The element with the largest atomic number is $F$ (atomic number $9$).
$(iv)$ From the data, we can infer that the atomic radius decreases as we move from left to right in a period.
$(v)$ Metal: $Li$ (Lithium), Non-metal: $F$ (Fluorine), Metalloid: $B$ (Boron).
$(vi)$ As we move from left to right in a period, the nuclear charge increases due to the addition of protons in the nucleus. This increased nuclear charge pulls the valence electrons closer to the nucleus, resulting in a decrease in atomic radius.