An element of 3d-transition series shows two oxidation states x and y, differing by two units. Then:

Options

A. compounds in oxidation state x are ionic if `xgty`
B. compounds in oxidation state x are ionic if `xlty`
C. compounds in oxidation state y are covalents if `xlty`
D. compounds in oxidation state y are covalents if `xgty`

Answer

To solve the problem regarding the oxidation states of an element from the 3d-transition series, we can follow these steps:

### Step 1: Identify the Oxidation States
Given that the element shows two oxidation states, \( x \) and \( y \), which differ by two units, we can denote them as:
- \( x = n \)
- \( y = n + 2 \) (or \( y = n - 2 \))

### Step 2: Determine the Nature of Compounds
In transition metals, the nature of the compounds (ionic or covalent) formed depends on the oxidation state:
- Lower oxidation states (like +2) tend to form ionic compounds.
- Higher oxidation states (like +3) tend to form covalent compounds.

### Step 3: Analyze the Given Options
We need to analyze the options based on the relationship between \( x \) and \( y \):
- If \( x < y \) (where \( x \) is the lower oxidation state), then compounds in oxidation state \( x \) are likely ionic, and those in oxidation state \( y \) are likely covalent.
- If \( x > y \), the same logic applies but in reverse.

### Step 4: Conclusion
From the analysis:
- If \( x < y \):
- Compounds in oxidation state \( x \) are ionic.
- Compounds in oxidation state \( y \) are covalent.
- If \( x > y \):
- Compounds in oxidation state \( y \) are ionic.
- Compounds in oxidation state \( x \) are covalent.

### Final Answer
Based on the information provided in the video transcript, we conclude that:
- Compounds in the lower oxidation state are ionic.
- Compounds in the higher oxidation state are covalent.