Statement: The halogens have high electron affinity values.

Explanation:
- Electron affinity refers to the energy change that occurs when an electron is added to a neutral atom to form a negative ion.
- It is a measure of the atom's ability to attract and hold an additional electron.
- A higher electron affinity value indicates a greater attraction for electrons and a stronger tendency to gain an electron.
- The halogens, which include elements such as fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At), are known to have high electron affinity values.

Reasons why the halogens have high electron affinity values:
1. Effective nuclear charge: The halogens have a high effective nuclear charge, which refers to the positive charge experienced by an electron in the outermost energy level. The greater the effective nuclear charge, the stronger the attraction for an additional electron, resulting in a high electron affinity.

2. Small atomic size: The halogens have relatively small atomic sizes, which means that the incoming electron will be closer to the nucleus. This proximity results in a stronger attractive force between the electron and the nucleus, leading to a high electron affinity.

3. Atomic stability: The halogens have electron configurations that are close to achieving a stable noble gas configuration. By gaining an electron, they can achieve a full outer electron shell, which increases their stability. This drive for stability contributes to their high electron affinity values.

4. Shielding effect: The shielding effect refers to the repulsion between electrons in different energy levels. In the halogens, the outermost electron is shielded from the full positive charge of the nucleus by the inner electrons. This shielding effect reduces the attraction between the nucleus and the incoming electron, allowing the halogens to have a relatively higher electron affinity compared to elements with similar effective nuclear charge but larger atomic sizes.

In conclusion, the halogens have high electron affinity values due to their high effective nuclear charge, small atomic size, atomic stability, and shielding effect. Thus, option B, "The halogens have high electron affinity values," is the correct answer.