Put the following elements in order of increasing atomic size: Ca, O, B, Be
B < O < Be < Ca
Ca < Be < B < O
O < B < Be < Ca
Be < B < O < Ca
https://www.angelo.edu/faculty/kboudrea/periodic/trends_atomicradius.htm
Be < B < O < Ca
To determine the order of increasing atomic size for the elements Ca, O, B, and Be, we need to consider their positions in the periodic table. Atomic size generally increases as you move down a group (vertical column) in the periodic table and decreases as you move across a period (horizontal row) from left to right.
First, let's locate the elements in the periodic table:
Ca - Calcium is located in group 2 and period 4.
O - Oxygen is located in group 16 and period 2.
B - Boron is located in group 13 and period 2.
Be - Beryllium is located in group 2 and period 2.
Comparing the atomic size of the elements, we can see that Be and Ca are both in the same period (period 2), so we need to consider their position in the group. Since Ca is in group 2 and Be is in group 2 as well, Ca has a larger atomic size than Be because atomic size generally increases as you move down a group.
Next, let's compare the atomic sizes of B and O. O is in period 2, while B is also in period 2. However, O is in group 16 and B is in group 13. Atomic size generally decreases as you move across a period from left to right, so B has a larger atomic size than O.
Based on these comparisons, we can determine the order of increasing atomic size:
B < O < Be < Ca