In chemistry at your level, sometimes you just have to settle for learning traits without delving too deeply the origins of rules, because the answers require a deep understanding of physical chemistry.
Oxygen likes to form two bonds, and silicon, like carbon, likes to form four. However unlike carbon, silicon does not like to form double bonds because it is a bigger atom and the p orbitals responsible for forming pi bonds are more diffuse, and so overlap between p orbitals on adjacent nuclei is poor. For this reason, CO2 is a small molecular gas with formula O=C=O, whereas silica, which has the same type of (SiO2) forms an extended structure characterized by single bonds between silicon and oxygen atoms. It is the only structure available that minimizes the number of pi bonds formed with silicon atoms.
Looking at your other options: (A) can't form easily an extended structure because halogens like chlorine typically (though not always) only bond 1 time each, so SiCl4 is a small molecule. This logic also extends to (C) and (D). (E) is likewise excluded because hydrogen usually only bonds once as well, and (F) involves fluorine, another halogen that is only available for a single bond to another atom. So with the exception of (B), all do not offer the ability to form extended structures because to do so would involve more bonds than the atoms involved would typically be happy to form.