Which one of the following elements shows both positive and negative oxidation states?

Options

A. Cesium
B. Fluorine
C. Iodine
D. Xenon

Answer

To determine which element shows both positive and negative oxidation states, we will analyze the given elements: cesium (Cs), fluorine (F), iodine (I), and xenon (Xe).

### Step 1: Analyze Cesium (Cs)
Cesium is known to be the most electropositive element in the periodic table. It typically exhibits an oxidation state of +1. Cesium cannot exhibit a negative oxidation state due to its high tendency to lose electrons rather than gain them.

**Hint:** Consider the position of cesium in the periodic table and its tendency to lose electrons.

### Step 2: Analyze Fluorine (F)
Fluorine is the most electronegative element. It predominantly exhibits an oxidation state of -1. Fluorine cannot show a positive oxidation state because it readily gains an electron to achieve a stable configuration.

**Hint:** Think about the electronegativity of fluorine and its ability to attract electrons.

### Step 3: Analyze Iodine (I)
Iodine is a halogen, like fluorine, but it is less electronegative. Iodine can exhibit multiple oxidation states, including both positive and negative states. For example, in compounds with fluorine, iodine can have oxidation states of +1, +3, +5, and -1. This variability is due to its ability to gain or lose electrons.

**Hint:** Look into the halogens and their ability to show variable oxidation states.

### Step 4: Analyze Xenon (Xe)
Xenon is a noble gas and typically does not form compounds. While it can exhibit positive oxidation states in some rare compounds, it does not show negative oxidation states.

**Hint:** Consider the characteristics of noble gases and their typical oxidation states.

### Conclusion
Based on the analysis, the element that shows both positive and negative oxidation states is **iodine (I)**.

**Final Answer:** Iodine (I) shows both positive and negative oxidation states.