The most common oxidation state of VI A group elements is

Options

A. `-2`
B. `+2`
C. `+4`
D. `+6`

Answer

To determine the most common oxidation state of Group 16 (VI A) elements, we can follow these steps:

### Step 1: Identify the Group 16 Elements
Group 16 elements, also known as the chalcogens, include oxygen (O), sulfur (S), selenium (Se), tellurium (Te), and polonium (Po).

**Hint:** Remember that Group 16 elements are also known as chalcogens.

### Step 2: Understand the Electronic Configuration
The general electronic configuration for Group 16 elements can be represented as \( ns^2 np^4 \). This means they have six valence electrons (two in the s subshell and four in the p subshell).

**Hint:** Focus on the number of valence electrons to determine possible oxidation states.

### Step 3: Determine Possible Oxidation States
Group 16 elements can exhibit various oxidation states based on their ability to gain or lose electrons. The common oxidation states include:
- **-2:** This is the most stable oxidation state for elements like oxygen and sulfur when they gain two electrons to achieve a noble gas configuration.
- **+2, +4, +6:** These oxidation states are possible when elements lose their valence electrons. For example, sulfur can exhibit +4 and +6 oxidation states in compounds like sulfur dioxide (SO₂) and sulfur trioxide (SO₃).

**Hint:** Consider how elements can achieve stability by gaining or losing electrons.

### Step 4: Identify the Most Common Oxidation State
Among the oxidation states listed, the most common oxidation state for Group 16 elements is **-2**. This is particularly true for oxygen and sulfur, which frequently form oxides and sulfides.

**Hint:** Think about the stability of the oxidation states in common compounds formed by these elements.

### Conclusion
The most common oxidation state of Group 16 (VI A) elements is **-2**.