Thus a hybrid orbital having more s- character will be more close to the nucleus and thus, more electronegative this give us the answer we why sp carbon is more electronegative than sp2 and sp3 carbon....It is better than the parents because it is directly unlike s-orbital

Why is sp more electronegative than sp2?

Introduction
Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. It is influenced by various factors such as atomic size, effective nuclear charge, and electron configuration. In the case of carbon, the electronegativity increases as the hybridization state of the carbon atom changes from sp3 to sp2 to sp. This can be explained by considering the following factors:

1. Bond Strength
The electronegativity of an atom is related to the strength of the bonds it forms. The strength of a bond is determined by the overlap of atomic orbitals involved in bond formation. In sp hybridized carbon, the two hybrid orbitals (formed by mixing one s and one p orbital) have a greater degree of overlap compared to sp2 hybridized carbon, which has three hybrid orbitals (formed by mixing one s and two p orbitals). The greater overlap in sp hybridization leads to stronger bonds, making sp hybridized carbon more electronegative.

2. Electron Density
The electronegativity of an atom is also influenced by its electron density. In sp hybridization, the two hybrid orbitals are directed towards opposite sides of the carbon atom, resulting in a linear arrangement. This linear arrangement causes the electrons to be held closer to the carbon nucleus, leading to higher electron density and increased electronegativity. On the other hand, in sp2 hybridization, the three hybrid orbitals are arranged in a trigonal planar geometry, causing the electron density to be spread out over a larger region. This results in lower electron density and lower electronegativity compared to sp hybridization.

3. Effective Nuclear Charge
The effective nuclear charge experienced by an atom also affects its electronegativity. In sp hybridization, the two hybrid orbitals are closer to the carbon nucleus, experiencing a higher effective nuclear charge. This higher effective nuclear charge attracts electrons more strongly towards the carbon atom, increasing its electronegativity. In sp2 hybridization, the three hybrid orbitals are farther from the nucleus, experiencing a lower effective nuclear charge, and therefore, a lower electronegativity.

Conclusion
In summary, sp hybridized carbon is more electronegative than sp2 hybridized carbon due to factors such as stronger bond strength, higher electron density, and a higher effective nuclear charge. These factors contribute to the increased ability of sp hybridized carbon to attract electrons towards itself in a chemical bond.