The stable oxidation state of Bismuth is

Options

A. `+1`
B. `+5`
C. `-3`
D. `+3`

Answer

To determine the stable oxidation state of Bismuth, we can follow these steps:

### Step 1: Identify the Group of Bismuth
Bismuth (Bi) is located in Group 15 of the periodic table, which includes the elements nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi).

**Hint:** Remember that elements in the same group often exhibit similar chemical properties, including common oxidation states.

### Step 2: Understand the Common Oxidation States
The common oxidation states for elements in Group 15 are typically +3 and +5. This is because they can lose three or five electrons from their outermost shell.

**Hint:** Oxidation states can be determined by the number of valence electrons an element has and how many it can lose or gain.

### Step 3: Consider the Electron Configuration
Bismuth has the electron configuration of [Xe] 4f14 5d10 6s2 6p3. The outermost electrons are in the 6s and 6p orbitals.

**Hint:** The electron configuration helps in understanding how many electrons can be involved in bonding and oxidation states.

### Step 4: Analyze the Inert Pair Effect
As we move down the group from nitrogen to bismuth, the stability of the +3 oxidation state increases due to the inert pair effect. This effect occurs because the s electrons (in the 6s orbital) become less available for bonding as they are held more tightly to the nucleus.

**Hint:** The inert pair effect explains why heavier elements in a group tend to favor lower oxidation states.

### Step 5: Determine the Most Stable Oxidation State
For bismuth, the +3 oxidation state is more stable compared to the +5 oxidation state due to the inert pair effect. Therefore, the stable oxidation state of bismuth is +3.

**Hint:** When considering oxidation states, always check for stability trends as you move down a group in the periodic table.

### Final Answer
The stable oxidation state of Bismuth is +3.

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