The hybridization for both of the oxygen atoms will be sp2 and the hybridization of the carbon atom will be sp. Remember when there is a multiple bond you only count the attached atom as one atom, because the pi-bond will require unhybridized p orbitals. Thus each oxygen atom has a carbon atom and two non-bonded pairs for a total of three groups. The carbon atom has two atoms attached for a total of two groups.
The oxygen-carbon-oxygen bond angle is 180o.
The pi-bonds lie at right angles to each other because the two unhybridized p orbitals of the carbon atom are at right angles. In the following drawing, the non-bonded electron pairs for the oxygen atoms are shown as red hybrid orbitals with these in the plane of the paper for the oxygen atom on the left and coming out and going back of the plane of the paper for the oxygen atom on the right. The pi-bond shown in blue is in the plane of the paper and the pi-bond shown in green is perpendicular to the plane of the paper.
The electron-pair geometry is linear for the carbon atom and trigonal planar for both oxygen atoms.
The molecular geometry is linear.