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HESI Chemistry Practice Tests & Test Prep by Exam Edge - Exam Info



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The more you know about the HESI Chemistry exam the better prepared you will be! Our practice tests are designed to help you master both the subject matter and the art of test-taking to be sure you are fully prepared for your exam.

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HESI 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 Health Education Systems, Inc HESI Chemistry Certification Exam. Our comprehensive HESI 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 Health Education Systems, Inc HESI Chemistry Certification Exam. Our HESI 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 HESI 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 20 practice tests available, each with 50 questions and detailed explanations to help you study. Every exam is designed to cover all of the aspects of the HESI Chemistry exam, ensuring you have the knowledge you need to be successful!

HESI Chemistry - Additional Info Sample Questions

Which ion will have the smallest size?

Correct Answer:
b3+


to understand why b3+ has the smallest size among its other positively charged counterparts like b+, b2+, and another b3+, it's essential to delve into the concepts of atomic structure and ionic charge. atoms consist of a nucleus, containing protons and neutrons, surrounded by electrons in various orbitals. the number of protons in the nucleus determines the atomic number and the identity of the element.

when an atom loses electrons, it becomes a positively charged ion, known as a cation. the loss of electrons can occur due to energy interactions where the ion's electron(s) gain enough energy to overcome the electrostatic attraction exerted by the nucleus. in the case of boron (b), which originally has 5 electrons, losing one electron results in b+, losing two results in b2+, and losing three leads to b3+. each successive loss of an electron results in a higher positive charge.

the size of an ion is influenced primarily by two factors: the nuclear charge (number of protons in the nucleus) and the number of electrons around the nucleus. as more electrons are removed, the effective nuclear charge per electron increases. this means each remaining electron experiences a stronger pull from the nucleus, as there are fewer electrons to shield the attractive force from the nucleus. consequently, the electron cloud contracts, and the ion's radius decreases.

thus, among b+, b2+, and b3+, the b3+ ion, having lost the most electrons, has the highest positive charge. this results in the strongest effective nuclear charge experienced by the remaining electrons. the increased pull from the nucleus due to the higher positive charge leads to a smaller ionic radius in b3+ compared to b+, b2+, or even another b3+ ion. this principle of increasing nuclear attraction with increasing positive charge, leading to a decrease in size, is a fundamental concept in chemistry known as the "shielding effect" and "effective nuclear charge."

therefore, b3+ ion is correctly identified as the smallest among the given ions due to its higher positive charge and resultant stronger nuclear attraction, which tightly pulls the electrons closer to the nucleus, reducing the ion's overall size. this explanation aligns with the observed trend across the periodic table where ions with higher positive charges tend to be smaller due to stronger electrostatic attractions within the atom.