All elements commonly exhibit an oxidation state of 

Options

A. `+1`
B. `-1`
C. zero
D. `+2`

Explanation

To determine the common oxidation states exhibited by elements, we can analyze the options provided in the question. The options are: +1, -1, 0, and +2. Let's evaluate each option step by step.

### Step 1: Understanding Oxidation States
Oxidation states indicate the degree of oxidation (loss of electrons) of an atom in a compound. An oxidation state of 0 indicates that the element is in its elemental form.

### Step 2: Evaluating the Oxidation State of 0
- All elements in their native state (elemental form) exhibit an oxidation state of 0. For example, oxygen (O2), nitrogen (N2), and fluorine (F2) are all diatomic molecules where each atom has an oxidation state of 0.

### Step 3: Evaluating the Oxidation State of +1
- The +1 oxidation state is typically seen in alkali metals (like sodium, Na). However, these metals do not exhibit a +1 oxidation state in their elemental form; they are neutral. Therefore, +1 cannot be the common oxidation state for all elements.

### Step 4: Evaluating the Oxidation State of -1
- The -1 oxidation state is commonly found in halogens (like fluorine, F). However, fluorine exists as F2 in its elemental form, which means it has an oxidation state of 0. Thus, -1 cannot be the common oxidation state for all elements.

### Step 5: Evaluating the Oxidation State of +2
- The +2 oxidation state is typically seen in alkaline earth metals (like magnesium, Mg). However, these metals also exist in their elemental form with an oxidation state of 0. Therefore, +2 cannot be the common oxidation state for all elements.

### Conclusion
After evaluating all the options, the only oxidation state that all elements exhibit in their native state is 0.

### Final Answer
The correct answer is **0**.

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