Question

Consider the elements: \(Cs\), \(Ne\), \(I\) and \(F\)

1. Identify the element that exhibits only negative oxidation state. 
2. Identify the element that exhibits only postive oxidation state. 
3. Identify the element that exhibits both positive and negative oxidation states.
4. Identify the element which exhibits neither the negative nor does the positive oxidation state.

Answer 1

 Consider the elements: Cs, Ne, I and F

1. Element that exhibits only negative oxidation state:
   Fluorine (F)
   Explanation: Fluorine is the most electronegative element and always shows an oxidation state of −1 in its compounds.
2. Element that exhibits only positive oxidation state:
   Cesium (Cs)
   Explanation: Cesium is an alkali metal and always loses one electron to form Cs⁺, showing only +1 oxidation state.
3. Element that exhibits both positive and negative oxidation states:
   Iodine (I)
   Explanation: Iodine can show negative oxidation state (−1) as well as positive oxidation states (+1, +3, +5, +7) in different compounds.
4. Element that exhibits neither negative nor positive oxidation state:
   Neon (Ne)
   Explanation: Neon is a noble gas with a completely filled valence shell and generally does not form compounds, so its oxidation state is 0.