For each of the following sets of elements, arrange in order of decreasing atomic radius: Li , O , C , F
Rank from largest to smallest.
To rank the elements Li, O, C, and F in order of decreasing atomic radius, you need to compare their positions in the periodic table. The atomic radius generally decreases from left to right across a period and increases from top to bottom within a group.
First, let's locate these elements in the periodic table:
Li (Lithium) -> Group 1, Period 2
O (Oxygen) -> Group 16, Period 2
C (Carbon) -> Group 14, Period 2
F (Fluorine) -> Group 17, Period 2
Comparing these elements, we can see that they all belong to the same period (period 2). In period 2, the atomic radius decreases from left to right across the periodic table.
While comparing atoms in the same period, the number of protons and electrons increases as you move to the right. This leads to a stronger attraction between the protons in the nucleus and the electrons in the outer energy level, thus reducing the atomic radius.
Based on this information, we can determine the order of decreasing atomic radius:
Li > C > O > F
Lithium (Li) has the largest atomic radius because it is the farthest to the left in the period.
Carbon (C) has a smaller atomic radius than Li because it is to the right of Li.
Oxygen (O) has a smaller atomic radius than C because it is further to the right.
Finally, Fluorine (F) has the smallest atomic radius because it is the farthest to the right.
So, the correct order from largest to smallest atomic radius is Li > C > O > F.