Answer:a) Al, b) S, c) Br, d) Na, e) O, f) Mg.
Step-by-step explanation:
To determine which atom in each pair has the largest atomic radius, we need to consider the periodic trend. Atomic radius generally increases as we move down a group and decreases as we move across a period from left to right.
a) Al B: Aluminum (Al) is larger than Boron (B) because Al is located below B in the same group (Group 13), and atomic radius generally increases down a group.
b) S O: Sulfur (S) is larger than Oxygen (O) because S is located below O in the same group (Group 16), and atomic radius generally increases down a group.
c) Br Cl: Bromine (Br) is larger than Chlorine (Cl) because Br is located below Cl in the same group (Group 17), and atomic radius generally increases down a group.
d) Na Al: Sodium (Na) is larger than Aluminum (Al) because Na is located to the left of Al in the same period (Period 3), and atomic radius generally decreases from left to right across a period.
e) O F: Oxygen (O) is larger than Fluorine (F) because O is located to the left of F in the same period (Period 2), and atomic radius generally decreases from left to right across a period.
f) Mg Ca: Magnesium (Mg) is larger than Calcium (Ca) because Mg is located to the left of Ca in the same period (Period 4), and atomic radius generally decreases from left to right across a period.
In summary, the atoms with the largest atomic radius in each pair are: a) Al, b) S, c) Br, d) Na, e) O, f) Mg.