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



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OAE Chemistry - Additional Information

At ExamEdge.com, we focus on making our clients' career dreams come true by offering world-class practice tests designed to cover the same topics and content areas tested on the actual Ohio Assessments for Educators OAE Chemistry (009) Certification Exam. Our comprehensive OAE Chemistry practice tests are designed to mimic the actual exam. You will gain an understanding of the types of questions and information you will encounter when you take your Ohio Assessments for Educators OAE Chemistry Certification Exam. Our OAE Chemistry Practice Tests allow you to review your answers and identify areas of improvement so you will be fully prepared for the upcoming exam and walk out of the test feeling confident in your results.

Because our practice tests are web-based, there is no software to install and no need to wait for a shipment to arrive to start studying. Your OAE Chemistry practice tests are available to you anytime from anywhere on any device, allowing you to study when it works best for you. There are 15 practice tests available, each with 125 questions and detailed explanations to help you study. Every exam is designed to cover all of the aspects of the OAE Chemistry exam, ensuring you have the knowledge you need to be successful!

OAE Chemistry - Additional Info Sample Questions

Which element has the lowest enthalpy of atomization?

Correct Answer:
zn


to determine which element among zn (zinc), sc (scandium), cu (copper), and cr (chromium) has the lowest enthalpy of atomization, it is important to understand what enthalpy of atomization is and how it relates to electronic configuration.

enthalpy of atomization is the amount of energy required to convert a mole of a solid substance into free gaseous atoms. this process involves breaking all the metallic bonds in one mole of metal. the strength of metallic bonding, and hence the enthalpy of atomization, depends significantly on the electronic configuration of the element, particularly its valence electrons.

zinc (zn) has the electronic configuration [ar] 3d^10 4s^2. this configuration represents a completely filled d-subshell and an s-subshell. the presence of a filled d-subshell adds stability to the electronic structure of zinc, and the fully filled shells do not provide additional delocalized electrons that could enhance metallic bonding. this reduced availability of electrons for bonding generally results in weaker metallic bonds compared to elements with partially filled d-subshells.

in contrast, scandium (sc) has the electronic configuration [ar] 3d^1 4s^2. this setup with a partially filled 3d subshell means that scandium can provide more delocalized electrons for metallic bonding compared to zinc, resulting in stronger metallic bonds and a higher enthalpy of atomization.

copper (cu), with an electronic configuration of [ar] 3d^10 4s^1, despite having a fully filled d-subshell like zinc, has an additional electron in the 4s orbital which is available for metallic bonding. this availability of an extra delocalized electron compared to zinc generally leads to stronger metallic bonds in copper, thus increasing the enthalpy of atomization.

similarly, chromium (cr) with the electronic configuration [ar] 3d^5 4s^1 features a half-filled d-subshell, which is known for its relative stability and ability to provide multiple delocalized electrons for bonding. this characteristic significantly enhances the strength of the metallic bonds in chromium, leading to a relatively high enthalpy of atomization.

therefore, among the given elements, zinc, with its fully filled 3d and 4s orbitals and lesser availability of delocalized electrons for bonding, exhibits the weakest metallic bonding. consequently, zinc has the lowest enthalpy of atomization among the options provided. this aligns with the concept that elements with fewer available electrons for metallic bonding typically have lower enthalpies of atomization.