Anatomy & Physiology Exam Prep practice questions and answers 2026. Tap an option to test yourself — you'll see the correct answer and a plain-English explanation for every question. Free, no login.
Q1Refer to the table of elements below. Which element, essential for building bone tissue in the human body, has an atomic number of 20? Element Atomic Number Hydrogen 1 Carbon 6 Oxygen 8 Calcium 20
✓ Correct answer: D. Calcium
The element with an atomic number of 20 is Calcium. Calcium is essential for building and maintaining bone tissue in the human body.
Q2The main components contained within the nucleus of a human body cell are:
✓ Correct answer: C. DNA and proteins
The nucleus of a human body cell houses DNA (deoxyribonucleic acid) which contains genetic instructions, and proteins which help in maintaining its structure and regulating access to the DNA.
Q3In the context of human physiology, which category would a pure sample of oxygen atoms used for cellular respiration belong to?
✓ Correct answer: B. an element
Oxygen, when consisting of a pure sample of its atoms, is classified as an element because it is made up of only one type of atom. In human physiology, this distinction is important for understanding respiratory processes.
Q4In the structure of a water molecule, which subatomic particle of an oxygen atom determines that it is oxygen?
✓ Correct answer: E. Protons
An oxygen atom is defined as such because it has 8 protons. Protons are positively charged and have a significant role in defining the atomic number of an element, thereby determining its identity.
Q5Examine the following data on subatomic particles. Which particle defines the identity of an element by its number and possesses a positive charge? Particle Charge Mass (amu) Electron Negative 0.0005 Neutron Neutral 1 Proton Positive 1
✓ Correct answer: D. Proton
The number of protons in an atom's nucleus defines the identity of the element. Protons have a positive charge and a mass of one atomic mass unit, contrary to electrons which are negatively charged and neutrons which are neutral.
Q6What is an atomic orbital?
✓ Correct answer: C. The region around an atom's nucleus where electrons are likely to be found.
An atomic orbital is a region of space around the nucleus where there is a high probability of finding an electron. This concept helps explain the distribution of electrons in an atom and their role in chemical bonding and interactions.
Q7In a covalent bond formation, what is the maximum number of electrons that can fill the 3s orbital of an atom?
✓ Correct answer: B. 2
Each 's' orbital, including the 3s orbita, can hold a maximum of 2 electrons. During covalent bond formation, electrons occupy the lowest available energy orbitals, and no orbital can have more electrons than its capacity allows.
Q8Analyze the following biochemical reactions important for nerve function. Which element or compound is most likely to donate electrons? Consider the possible electron transfer roles listed. Substance Reaction Type Possible Electron Transfer Cu Redox Donates electrons Mg Redox Donates electrons N None Cl Acid-base Accepts electrons
✓ Correct answer: A. Mg
Mg is most likely to donate electrons because it is an alkaline earth metal, similar to strontium, and participates in redox reactions.
Q9Calculate the maximum number of electrons that can occupy the third electron shell for sulfur, given its atomic number is 16. Element Atomic Number Sulfur 16
✓ Correct answer: D. 18
The capacity of an electron shell is determined by $$2 \times n^2$$, where $$n$$ is the principal quantum number of the shell. For the third shell (n=3), the maximum number of electrons it can hold is $$2 \times 3^2 = 18$$. Sulfur does not use the full capacity of the third shell, but the question asks for the maximum potential number.
Q10Examine the following elements. Which element is most likely to form an ionic bond by losing an electron? Element Atomic Number Group Number Sodium (Na) 11 1 Calcium (Ca) 20 2 Nitrogen (N) 7 15 Chlorine (Cl) 17 17
✓ Correct answer: C. Sodium (Na)
Sodium (Na) is in Group 1, which means it has one valence electron. Elements in Group 1 readily lose one electron to achieve a stable noble gas electron configuration, making them likely to form ionic bonds.
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