Question

In general, as you go across a period in the periodic table from left to right:

1. the atomic radius _______;
2. the electron affinity becomes _______ negative; and
3. the first ionization energy ______.
A. increases, increasingly, decreases
B. decreases, increasingly, decreases
C. decreases, increasingly, increases
D. increases, increasingly, increases
E. decreases, decreasingly, increases

Answer 1

As you go across a period in the periodic table from left to right, the atomic radius increases, the electron affinity becomes increasingly negative, and the first ionization energy mostly increases.

Step-by-step explanation:

As you move across a period on the periodic table from left to right:

1. The atomic radius increases because the effective nuclear charge experienced by the electrons increases, pulling them closer to the nucleus.
2. The electron affinity becomes increasingly negative because electrons are placed into lower energy orbitals, closer to the nucleus, making the process more favorable.
3. The first ionization energy mostly increases because it is easier to remove an electron from a larger, higher energy orbital.

Note that there are exceptions to these trends when dealing with completely filled or half-filled subshells.