Under the influence of strong the ligands the electrons can be forced______against the_____ rule of__________ .

Answer

To fill in the blanks in the statement "Under the influence of strong ligands, the electrons can be forced ______ against the ______ rule of ________," we can derive the answer from the explanation provided in the video transcript.

### Step-by-Step Solution:

1. **Identify the Concept**: The question revolves around the behavior of electrons in coordination compounds, specifically when influenced by strong field ligands.

2. **Understand Strong Field Ligands**: Strong field ligands, such as cyanide (CN⁻), have a strong ability to attract electrons and can cause pairing of electrons in the d-orbitals of the metal ion.

3. **Recall Hund's Rule**: Hund's rule states that electrons will fill degenerate orbitals singly first before pairing up, in order to maximize the number of unpaired electrons.

4. **Analyze the Example**: In the example of the complex ion Fe(CN)₆²⁻, the presence of the strong field ligand (CN⁻) leads to the pairing of electrons in the d-orbitals of iron (Fe). Normally, in a d⁶ configuration, there would be unpaired electrons, but the strong field ligand forces them to pair.

5. **Fill in the Blanks**:
- The first blank should be "pair up" because the electrons are forced to pair.
- The second blank should be "Hund's" because we are referring to Hund's rule.
- The third blank should be "maximum multiplicity" because Hund's rule is about maximizing the number of unpaired electrons (multiplicity).

### Final Statement:
"Under the influence of strong ligands, the electrons can be forced **pair up** against the **Hund's** rule of **maximum multiplicity**."