The hybridization of carbon and oxygen in CO are respectively:(A) sp, sp(B) s{p^2}, sp (C) s{p^2}, s{p^2} (D) sp, s{p^2}

To determine the hybridization of carbon (C) and oxygen (O) in carbon monoxide (CO), we can follow these steps:

### Step 1: Determine the Lewis Structure
1. **Count Valence Electrons:**
- Carbon has 4 valence electrons.
- Oxygen has 6 valence electrons.
- Total = \(4 + 6 = 10\) valence electrons.

2. **Draw the Lewis Structure:**
- Carbon forms a triple bond with oxygen to satisfy the octet rule.
- The structure can be represented as:
\[
\text{C} \equiv \text{O}
\]
- There are two lone pairs on oxygen, and carbon has no lone pairs.

### Step 2: Determine Hybridization
1. **Carbon (C):**
- In CO, carbon forms one triple bond with oxygen, which consists of one sigma (σ) bond and two pi (π) bonds.
- For the sigma bond, one of the carbon's \(2s\) and one \(2p\) orbital hybridize to form two \(sp\) hybrid orbitals.
- Thus, the hybridization of carbon is **sp**.

2. **Oxygen (O):**
- Oxygen also participates in the triple bond, contributing one sigma bond and two pi bonds.
- In addition, oxygen has two lone pairs of electrons.
- The central atom in oxygen uses one \(2s\) and two \(2p\) orbitals for bonding, resulting in the formation of three hybrid orbitals.
- Thus, the hybridization of oxygen is **sp²**.

### Conclusion
Based on this analysis, the hybridization of carbon and oxygen in CO are:

- **Carbon:** sp
- **Oxygen:** sp²

### Final Answer
The correct option is **(D) sp, sp²**.