What are the ions present in the compound CO2?C4+, 2 O2-C2+, 2 O-C2+, O2-C2+, O22-no ions present

To analyze the ions present in the compound $\text{CO}_2$, we first consider the chemical structure and the types of particles involved.

1. Understanding Carbon Dioxide Structure: The molecular formula $\text{CO}_2$ represents carbon dioxide, which consists of one carbon atom (C) and two oxygen atoms (O).

2. Ion Analysis:

   • Carbon (C) typically forms a +4 oxidation state when it bonds with oxygen in $\text{CO}_2$.
   • Oxygen (O) typically forms a -2 oxidation state.
   • In the compound itself, there are no free ions present as it exists as a neutral molecule. Thus, although carbon can be thought to be in a +4 state and oxygen in a -2 state, they do not exist as separate ions in $\text{CO}_2$.

3. Evaluating Given Options: Now, let’s evaluate the provided options:

   • C4+: Represents a carbon ion, which is not present in $\text{CO}_2$.
   • 2 O2-: This suggests the presence of two oxide ions, which does not exist separately in the molecule form.
   • C2+: Again, a carbon ion is not separately present.
   • 2 O-: Indicates oxide ions, which also do not exist separately.
   • O2-: Refers to a peroxide ion, unrelated to $\text{CO}_2$.
   • O22-: Refers to a peroxide ion form (e.g., $\text{O}_2^{2-}$), also not relevant to $\text{CO}_2$.
   • No ions present: This correctly identifies that $\text{CO}_2$ is a neutral molecule without free ions.

Final Answer

The correct choice is "no ions present" since carbon dioxide exists as a molecular compound without free ions, despite the oxidation states of the elements involved.