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OAE Chemistry (009) Practice Tests & Test Prep by Exam Edge - Review



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OAE Chemistry - Reviews


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Based on 110 reviews

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See why our users from 154 countries love us for their exam prep! Including 110 reviews for the OAE Chemistry exam.

Exam Edge is an industry leader in online test prep. We work with institutional partners to offer a wide array of practice tests that will help you prepare for your big exam. No matter how niche your field of interest might be, we're here to help you prepare for test day.

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OAE Chemistry - Test Reviews Sample Questions

Which of the following has the same carbon as that in the hybrid state of the C atom in C2H2 ?

Correct Answer:
co2


to understand the hybrid state of carbon in different compounds, it is essential to know about orbital hybridization. orbital hybridization is a concept in molecular chemistry where atomic orbitals mix to form new hybrid orbitals which can influence molecular geometry and bonding properties.

in the molecule acetylene, c2h2, each carbon atom is bonded to the other carbon atom via a triple bond, and each carbon also bonds to a hydrogen atom. the type of hybridization involved in c2h2 is sp hybridization. in sp hybridization, one s orbital and one p orbital mix to form two equivalent sp hybrid orbitals. this hybridization results in a linear arrangement of atoms with bond angles of approximately 180 degrees.

now, let's analyze the options provided: 1. **c2h6 (ethane)**: in ethane, each carbon is sp3 hybridized. this involves the mixing of one s orbital and three p orbitals to form four sp3 hybrid orbitals. these orbitals are oriented tetrahedrally with bond angles of about 109.5 degrees. therefore, the hybridization in c2h6 differs from the sp hybridization in c2h2. 2. **co2 (carbon dioxide)**: in carbon dioxide, the carbon atom forms two double bonds with two oxygen atoms. the hybridization of carbon in co2 is sp, similar to that in c2h2. the molecule is linear with bond angles of 180 degrees. hence, co2 has the same sp hybridization as observed in c2h2. 3. **benzene**: in benzene, each carbon atom is sp2 hybridized. this involves the mixing of one s orbital and two p orbitals to form three sp2 hybrid orbitals arranged in a trigonal planar geometry with bond angles of about 120 degrees. the remaining unhybridized p orbital participates in pi bonding. thus, the hybridization in benzene (sp2) is different from the sp hybridization in c2h2. 4. **c (diamond)**: in diamond, each carbon atom is sp3 hybridized, similar to ethane, forming a tetrahedral structure with bond angles of 109.5 degrees. this is different from the sp hybridization in c2h2.

based on this analysis, 2, where the carbon atom is sp hybridized, matching the hybridization state of carbon in c2h2.