HESI A2 · Chemistry section

HESI A2 Chemistry Practice Test: Atoms, Bonds, Reactions, Solutions and pH

Practice set 1 has 20 HESI A2 chemistry questions on an exam-style screen. They run from states of matter, atoms and the periodic table through bonds, balanced equations and moles to solutions, pH, oxidation and reduction, and radioactive decay. Each answer comes with an explanation and a note on every option, and a one-table chemistry review sits further down the page. Schools publish the section's details (Germanna Community College lists 30 chemistry questions). These questions are free, with no sign-up.

Start practice set 1 What the section covers

Practice sets

HESI A2 chemistry practice sets

Three sets of chemistry questions. Each opens on an exam-style test screen, one question at a time: answer, select Check answer, and see the correct answer, the explanation and a note on every option before you go on. Untimed, and your progress is saved in this browser.

Set 01Free

20 questions

Matter, atoms and the periodic table; bonds, equations and reactions; moles, solutions and concentration; acids, bases, redox and the nucleusNot started

Start set

Set 02Free

20 questions

Matter, atoms and the periodic table; bonds, equations and reactions; moles, solutions and concentration; acids, bases, redox and the nucleusNot started

Start set

Set 03Free

20 questions

Matter, atoms and the periodic table; bonds, equations and reactions; moles, solutions and concentration; acids, bases, redox and the nucleusNot started

Start set

Set 1 spreads its 20 questions over ten topics; the topic cards below show how many fall in each group. The chemistry section of Practice Exam 1 suggests about 60 seconds a question; your school or testing site sets the real timing (Texas State Technical College's library guide suggests 25 minutes for 25 chemistry items plus 5 pilot items). When the sets feel easy, take the full-length HESI A2 Practice Exam 1, with each section on its own clock.

Sample HESI A2 chemistry questionFrom practice set 1, with the answer and a note on every option

What is the name of a direct change from solid to gas?

1.Sublimation✓
2.Condensation
3.Vaporization
4.Deposition

Answer: Sublimation

Sublimation changes a solid directly into a gas. Deposition is the reverse change, from gas directly to solid.

Why each option is right or wrong

Sublimation: Correct. Sublimation skips the liquid phase.

Condensation: This describes gas changing to liquid.

Vaporization: This describes liquid changing to gas.

Deposition: This reverses the direction and describes gas changing to solid.

Matter, atoms and the periodic table · Matter and its states

Content

What the HESI A2 chemistry section covers

Schools describe the A2 chemistry section on their own pages. The practice sets here draw on the topics below, in four groups that run from states of matter to the atom's nucleus.

Questions: 25; In Practice Exam 1 here; Germanna lists 30
Suggested time: 25 min; Your school or testing site sets the limit
Per question: 60 s; At the suggested time
Calculator: None; In this section of the practice exam

Set 1 here: 6 of 20 questions

Matter, atoms and the periodic table

How particles behave in solids, liquids and gases, what happens when matter changes state, physical and chemical changes, and how a gas's pressure and volume trade off; the proton, neutron and electron counts behind an atomic number, a mass number and an ion's charge; isotopes and average atomic mass; and what an element's place in the periodic table says about its electrons, its size and how it reacts.

Matter and its states
Atomic structure and isotopes
The periodic table

Set 1 here: 4 of 20 questions

Bonds, equations and reactions

Ionic and covalent bonds, polar and nonpolar sharing, the formula an ionic compound takes and how many electrons a triple bond shares; then balancing an equation with coefficients, conservation of mass, the reaction types by their pattern, and whether a reaction gives off heat or takes it in.

Chemical bonding
Chemical equations and reaction types

Set 1 here: 4 of 20 questions

Moles, solutions and concentration

The arithmetic of chemistry: grams to moles and back, mole ratios from a balanced equation, percent by mass, molarity and dilution, and which solvent dissolves which solute. In the sets here, these questions give the molar masses they need, with numbers chosen to work by hand.

Moles and stoichiometry (simple)
Solutions and concentration

Set 1 here: 6 of 20 questions

Acids, bases, redox and the nucleus

Acids as proton donors, neutralization, buffers and the tenfold steps of the pH scale; oxidation numbers, which substance loses electrons and which gains them; and what alpha and beta decay do to a nucleus and how much of a sample is left after a number of half-lives.

Acids, bases and pH
Oxidation and reduction
Nuclear chemistry (half-life, types of radiation)

What schools say about the chemistry section

HESI A2 chemistry: published facts
Source	What its page says
Texas State Technical College (Library Guides)	Its HESI A2 study guide puts chemistry in a science part with biology, anatomy and physiology, and physics: 25 chemistry items plus 5 pilot items, with 25 minutes suggested. Its chemistry objectives include the parts of the atom and their mass and charge, bonds as shared or transferred electrons, patterns in the periodic table, particles in solids, liquids and gases, evaporation and condensation, balancing reactions (oxidation-reduction and acid-base among them), the pH scale, catalysts, enzymes as proteins, the chemical properties of water, kinds of energy, and the Sun as the main outside source of energy.
Germanna Community College (Academic Center for Excellence)	Its guide (updated January 2023) puts chemistry with anatomy and physiology in a science part, 30 questions each, and lists temperature, atomic structure and the periodic table, chemical equation terminology, solutions and concentrations, stoichiometry, chemical reactions, chemical bonding and nuclear chemistry. It mentions a basic on-screen calculator for the math portion only.
Central New Mexico Community College	Lists chemistry among its six sections (grammar, reading comprehension, vocabulary and general knowledge, biology, chemistry and math), without a question count. It hands out a calculator, pencils and paper but no periodic table or conversion table, and applicants to its nursing program need 75% on every sub-test and a 75% composite.
Tarrant County College	Does not offer biology or chemistry. Its five sections are reading comprehension, vocabulary, grammar and math (55 questions each) and anatomy and physiology (30).
Quincy College (Academic Division of Nursing)	Its guide (updated December 2024) lists only biology and anatomy and physiology in its science part, 30 items each; chemistry is not among its sections.
Chamberlain University	Its HESI A2 page mentions that Elsevier's review guide includes chemistry, along with math and physics, yet its BSN applicants sit only four exams: reading comprehension, vocabulary and general knowledge, biology, and anatomy and physiology.

Sources: Texas State Technical College Library Guides, Study Guide: HESI A2; Germanna Community College, HESI A2 Nursing Entrance Exam Preparation Guide (PDF, updated January 2023); Central New Mexico Community College, HESI A2 Exam; Tarrant County College, HESI A2 Exam Information; Quincy College Academic Division of Nursing, Preparing for the HESI A2 Admission Exam (PDF, updated December 2024); Chamberlain University, HESI Admission Assessment (A2) Exam

Question formats

How HESI A2 chemistry questions work

Each question here is right or wrong, with no partial credit. In Practice Exam 1 you can flag a question, see which are still blank and go back to any question in the section until you end it. Testing sites differ here: Germanna Community College's guide says its students cannot skip a question or go back to one they have already answered.

Chemistry question formats
Format	How you answer	In set 1 here
Multiple choice	Choose the one correct option of four	20 of 20

Every question in set 1 here is multiple choice with four options. Roughly half the questions across the chemistry sets here need a short calculation or a count: an average atomic mass, the electrons in a bond, a balanced coefficient, grams to moles, a molarity or a dilution, a pH, an oxidation number, or the nucleus left after alpha or beta decay. The rest ask you to name a change of state, a particle, a bond or a reaction type, or to choose the explanation that fits, such as why a gas compresses or why salt melts at a far higher temperature than ice.

Periodic table and calculator: ask your testing site

Central New Mexico Community College, which tests chemistry, says it hands out a calculator, pencils and paper but no periodic table or conversion table, and it allows no outside materials. Texas State Technical College's library guide and Germanna Community College's guide mention an on-screen calculator only for math. Check your own testing site's rules. The chemistry section of Practice Exam 1 here has no calculator and no periodic table, and the arithmetic in the sets here works on scratch paper.

Sources: Central New Mexico Community College, HESI A2 Exam; Texas State Technical College Library Guides, Study Guide: HESI A2; Germanna Community College, HESI A2 Nursing Entrance Exam Preparation Guide (PDF, updated January 2023)

Method

How to prepare for HESI A2 chemistry

What to study first and how to pace the section, for chemistry in particular.

01Learn the layout of the periodic tableYou may get no table on test day, so learn what an element's position tells you: one valence electron in group 1, two in group 2 and the group number minus 10 in groups 13 to 18 (helium, with two, is the exception); the period gives the highest occupied energy level; atoms generally grow larger down a group and smaller across a period. Learn where the alkali metals, the halogens and the noble gases sit and how each tends to react.
02Get every particle count from two numbersThe atomic number is the protons; the mass number minus the atomic number is the neutrons; the electrons equal the protons in a neutral atom and differ by the charge in an ion. A 2+ ion has two fewer electrons than protons, a 2− ion two more. Practice until an isotope or an ion takes seconds.
03Balance with coefficients and name the patternCount each kind of atom on both sides and change only the coefficients: changing a subscript changes the formula, and CO is not CO₂. Then sort reactions by their shape: two things becoming one (synthesis), one becoming two (decomposition), one element swapping in (single replacement), two compounds trading partners (double replacement), and a hydrocarbon burning in oxygen to give carbon dioxide and water (combustion).
04Send every mole problem through molesTurn grams into moles with the molar mass, use the coefficients of the balanced equation as a ratio, then turn moles back into grams. Write the unit beside every number; if the units do not cancel to the one the question asks for, a step is missing.
05Keep three concentration formulas readyMolarity is moles of solute per liter of solution; mass percent is the solute's mass over the whole solution's mass, times 100; and in a dilution the moles of solute stay the same, so M₁V₁ = M₂V₂, with both volumes in the same unit. For molarity, turn milliliters into liters before you divide.
06Use powers of ten for pH and OIL RIG for redoxEach pH unit is a factor of ten in hydrogen-ion concentration, so two units apart is a factor of 100, and at 25 °C pH and pOH add to 14. For redox, oxidation is loss of electrons and reduction is gain; work out an unknown oxidation number by making the numbers add up to the charge of the molecule or ion.
07Track the nucleus through decay and half-livesAlpha decay takes 4 from the mass number and 2 from the atomic number; beta-minus decay adds 1 to the atomic number and leaves the mass number alone. For half-life, halve the amount once for each half-life that passes: 100, 50, 25, 12.5.
08Pace at about 60 seconds a questionPractice Exam 1 here suggests 25 minutes for 25 chemistry questions; your school or testing site sets the real timing. Texas State Technical College's library guide suggests 25 minutes for 25 chemistry items plus 5 pilot items, closer to 50 seconds an item if the pilot items share that time. Definitions and trends take seconds, which leaves time for the problems with numbers; if one stalls, make your best choice and move on.

HESI A2 biology practice test, with a biology study guide in one table HESI A2 math practice test, for the fractions, ratios and conversions chemistry problems lean on Applying to TEAS schools too? TEAS science practice test, where chemistry is one of four areas

Chemistry review

HESI A2 chemistry review: the facts and formulas in one table

A summary written for this page, not a list of what the test asks: the particles, patterns, reactions and formulas behind the topics schools list for the section and the topics in the practice sets here, checked against the LibreTexts and US government pages named under the table.

HESI A2 chemistry review
Topic	What to know
States of matter	In a solid the particles are packed closely and vibrate in fixed positions, so a solid keeps its shape and volume. In a liquid they are still close but move past one another: a liquid has a definite volume but takes the shape of its container. A gas has no definite shape or volume; its particles are far apart and in rapid, random motion, and because a gas is mostly empty space it is easy to compress
Changes of state	Melting is solid to liquid and freezing the reverse; vaporization is liquid to gas (evaporation happens at the surface, boiling throughout the liquid) and condensation the reverse; sublimation is solid straight to gas and deposition the reverse. Melting, vaporization and sublimation absorb energy; freezing, condensation and deposition release it. While a pure substance melts or boils, its temperature stays constant until the change is complete
Physical and chemical changes	A physical change alters a material's form or state without changing what it is: ice melting, wood ground into sawdust. A chemical change makes new substances: wood burning, iron rusting. Signs of a chemical change include a color change, a gas, a precipitate (a solid forming in a solution) and a transfer of energy, often heat or light given off. A chemical property, such as iron's tendency to rust, shows only when a substance reacts; a physical property, such as density or melting point, can be observed without changing the substance
Gases	At constant temperature, the pressure and volume of a fixed amount of gas vary inversely (Boyle's law): P₁ × V₁ = P₂ × V₂, so tripling the volume cuts the pressure to a third. Heating a gas in a rigid container raises its pressure, because the faster particles hit the walls more often and with more force. Equal volumes of gases at the same temperature and pressure contain equal numbers of particles (Avogadro's hypothesis)
Temperature	Listed by Germanna Community College; the practice sets here do not test conversions. Temperature measures the average kinetic energy of a substance's particles. Kelvin = °C + 273.15 (often rounded to 273), and °F = (°C × 1.8) + 32. Water freezes at 0 °C (32 °F) and boils at 100 °C (212 °F) at standard pressure; absolute zero, 0 K, is the coldest possible temperature
The atom	Protons (positive charge) and neutrons (no charge) form the nucleus, which holds most of an atom's mass; electrons (negative charge, adding almost nothing to the mass) move around it. The atomic number is the number of protons; the mass number is protons plus neutrons. A neutral atom has as many electrons as protons; an ion does not, and its charge is the difference: 12 protons and 10 electrons make a 2+ ion
Isotopes and atomic mass	Isotopes of an element have the same number of protons but different numbers of neutrons, so different mass numbers: carbon-12, carbon-13 and carbon-14. An element's atomic mass is the average of its isotopes' masses, weighted by how common each is: chlorine is about 76% chlorine-35 and 24% chlorine-37, which gives about 35.45
Electrons and energy levels	Electrons occupy energy levels (shells) around the nucleus. The outermost electrons, the valence electrons, are the ones that take part in bonds and decide how reactive an atom is. When an electron drops to a lower energy level it gives off the difference in energy, often as light (a photon)
The periodic table	Elements are arranged in order of increasing atomic number, in rows (periods) and columns (groups). An element's period number is its highest occupied principal energy level. Elements in a group have similar properties, and in the main groups the same number of valence electrons: one in group 1, two in group 2, eight in group 18 (helium has two). The group 1 metals, the alkali metals, are very reactive and lose their one valence electron; the halogens of group 17 are one electron short of a full outer shell and very reactive; the noble gases of group 18 are essentially unreactive. Hydrogen sits in group 1 but is not an alkali metal. Metalloids such as silicon lie along the stair-step line between the metals and the nonmetals
Periodic trends	Atomic radius generally increases down a group, as each period adds an energy level, and decreases across a period, as more protons pull the electrons closer. Electronegativity, an atom's pull on the electrons in a bond, generally increases across a period and decreases down a group; fluorine's is the highest. A positive ion is smaller than its atom, a negative ion larger
Ionic bonds	A metal atom transfers electrons to a nonmetal atom, and the oppositely charged ions attract each other. Atoms tend to gain, lose or share electrons until they have eight valence electrons (the octet rule). An ionic compound has no overall charge: Na⁺ and Cl⁻ give NaCl, Mg²⁺ and Cl⁻ give MgCl₂, Mg²⁺ and O²⁻ give MgO. Ionic compounds have high melting points (sodium chloride melts at 801 °C) and conduct electricity when melted or dissolved in water, but not as solids
Covalent and metallic bonds	In a covalent bond, nonmetal atoms share pairs of electrons: a single bond shares one pair, a double bond two pairs and a triple bond three pairs (six electrons, as in N₂). Electrons shared equally, as between the two atoms of Cl₂, make a nonpolar bond; shared unequally, they make a polar bond, and the more electronegative atom takes a partial negative charge. Carbon forms four covalent bonds. In metallic bonding, positive metal ions sit in a sea of electrons that move freely
Water	Water is a polar molecule: the oxygen atom carries a partial negative charge and the hydrogen atoms partial positive charges. Hydrogen bonds, attractions between neighboring water molecules rather than bonds inside one, give water a very high boiling point for so small a molecule. Water dissolves many ionic and polar substances
Chemical equations	Reactants are written on the left of the arrow and products on the right. Matter is neither created nor destroyed in a chemical reaction (the law of conservation of mass), so an equation must be balanced: put coefficients in front of formulas and never change a subscript, which would change the formula itself (CO and CO₂ are different compounds). Balanced: 2H₂ + O₂ → 2H₂O
Reaction types	Combination (synthesis): A + B → AB. Decomposition: AB → A + B, as in CaCO₃ → CaO + CO₂. Single replacement: A + BC → AC + B, as when zinc reacts with hydrochloric acid. Double replacement: AB + CD → AD + CB, usually forming a precipitate, a gas or water. Combustion: a hydrocarbon burned in oxygen gives carbon dioxide and water. An exothermic reaction gives off heat, and its surroundings warm; an endothermic reaction absorbs heat, and its surroundings cool. A catalyst speeds up a reaction by lowering its activation energy and is not used up; enzymes are biological catalysts made of protein
The mole	One mole is 6.022 × 10²³ particles (Avogadro's number). Molar mass is the mass of one mole in grams, found by adding up the atomic masses in the formula: water, H₂O, is about 18.02 g/mol. Moles = mass ÷ molar mass, and mass = moles × molar mass
Stoichiometry	The coefficients of a balanced equation are mole ratios: in N₂ + 3H₂ → 2NH₃, 1 mole of nitrogen reacts with 3 moles of hydrogen to give 2 moles of ammonia. To go from grams of one substance to grams of another, convert grams to moles, apply the mole ratio, then convert moles back to grams. The limiting reactant is used up first and sets how much product forms; percent yield = actual yield ÷ theoretical yield × 100. Percent composition is each element's share of a compound's mass
Solutions	A solution is a homogeneous mixture of a solute dissolved in a solvent. Like dissolves like: many ionic and polar substances dissolve in water, which is polar; nonpolar substances dissolve in nonpolar solvents; and oil, being nonpolar, does not dissolve in water. A saturated solution holds as much solute as will dissolve at that temperature. Gases dissolve less in warmer water, and more when the pressure of the gas above the liquid rises
Concentration	Molarity (M) = moles of solute ÷ liters of solution. Mass percent = mass of solute ÷ mass of solution × 100, where the mass of the solution is the solute plus the solvent. Diluting a solution adds solvent and leaves the moles of solute unchanged, so M₁ × V₁ = M₂ × V₂
Acids and bases	Arrhenius: an acid produces hydrogen ions (H⁺) in water, and a base produces hydroxide ions (OH⁻). Brønsted–Lowry: an acid donates a proton (H⁺) and a base accepts one. A strong acid such as HCl ionizes completely in water; a weak acid such as acetic acid ionizes only slightly. An acid and a base neutralize each other to form a salt and water: HCl + NaOH → NaCl + H₂O. Acids turn blue litmus paper red; bases turn litmus blue
pH and buffers	The pH scale runs from 0 to 14: 7 is neutral, lower values are acidic and higher ones basic. Each whole pH unit is a tenfold change in hydrogen-ion concentration, so a solution at pH 3 has 100 times the H⁺ of one at pH 5. At 25 °C, pH + pOH = 14. A buffer, a weak acid with a salt of its conjugate base (acetic acid with acetate, for example), resists changes in pH when small amounts of acid or base are added
Oxidation and reduction	Oxidation is the loss of electrons, and the oxidation number rises; reduction is the gain of electrons, and the oxidation number falls (a memory aid: OIL RIG, oxidation is loss, reduction is gain). The two happen at the same time: the electrons one substance loses, another gains. The substance oxidized is the reducing agent and the substance reduced is the oxidizing agent: in 2Na + Cl₂ → 2NaCl, sodium is oxidized and is the reducing agent
Oxidation numbers	An element on its own has an oxidation number of 0 (O₂, Na). A monatomic ion's oxidation number is its charge (Cl⁻ is −1). Oxygen is usually −2 (−1 in peroxides) and hydrogen usually +1 (−1 in metal hydrides). The oxidation numbers in a neutral compound add up to 0, and in a polyatomic ion to the ion's charge: in CO₃²⁻, C + 3(−2) = −2, so carbon is +4
Radioactive decay	A radioactive isotope has an unstable nucleus that gives off radiation as it decays. Alpha decay emits 2 protons and 2 neutrons (a helium nucleus): the atomic number falls by 2 and the mass number by 4. In beta (beta-minus) decay a neutron becomes a proton and an electron is emitted: the atomic number rises by 1 and the mass number stays the same. Gamma rays are high-energy electromagnetic radiation and change neither number. Alpha particles are stopped by a sheet of paper or the skin and beta particles by a sheet of aluminum, while gamma rays need thick shielding of a dense material such as lead or concrete. A nuclear reaction can change one element into another; a chemical reaction cannot
Half-life	The half-life of a radioactive isotope is the time it takes for half of the radioactive atoms in a sample to decay. After n half-lives, (1/2)ⁿ of the original amount is left: after three half-lives, one eighth. Half-lives range from fractions of a second to billions of years
Energy	Listed by Texas State Technical College; the practice sets here do not test kinds of energy. Kinetic energy is the energy of motion and potential energy is stored energy; chemical potential energy is stored in the bonds of substances. The Sun is Earth's main source of energy

FAQ

HESI A2 chemistry: questions people ask

Is there chemistry on the HESI A2?

There can be, but each school picks the sections its applicants take. Central New Mexico Community College, Texas State Technical College and Germanna Community College include chemistry; Tarrant County College does not offer it, Quincy College's guide lists only biology and anatomy and physiology as its sciences, and Chamberlain University's four required exams leave it out. Ask your program which sections it counts before you plan your study time; Practice Exam 1 here lets you take only the sections you tick.

How many chemistry questions are on the HESI A2?

It depends on the school, and the figures come from schools' own pages: Germanna Community College's guide gives 30 chemistry questions, and Texas State Technical College's library guide counts 25 items plus 5 pilot items, for which it suggests 25 minutes. The chemistry section of Practice Exam 1 here has 25 questions and a suggested 25 minutes, close to 60 seconds each; the real limit is your testing site's.

What chemistry is on the HESI A2?

Schools list the topics. Germanna Community College's guide lists temperature, atomic structure and the periodic table, chemical equation terminology, solutions and concentrations, stoichiometry, chemical reactions, chemical bonding and nuclear chemistry, and Texas State Technical College's objectives add the pH scale, catalysts, the chemical properties of water and kinds of energy. The practice sets here cover states of matter; atoms and isotopes; the periodic table; bonding; equations and reaction types; moles and simple stoichiometry; solutions and concentration; acids, bases and pH; oxidation and reduction; and nuclear chemistry, from half-life to the types of radiation.

Is the HESI A2 chemistry section hard?

What makes it hard is the mix of facts to recall and short problems to work. Many questions in the sets here need a calculation, such as a molarity, a dilution, grams to moles or what is left after a few half-lives, and you may have no periodic table to look things up. Practice the formulas until they are routine.

Do you get a periodic table or a calculator for HESI A2 chemistry?

Ask your testing site, because the rules are local. Of the schools cited on this page, only Central New Mexico Community College says whether a periodic table is provided on test day, and it says it does not provide one. On calculators the pages differ: Central New Mexico Community College hands one out, while Texas State Technical College and Germanna Community College mention an on-screen calculator only under math. In Practice Exam 1 here, the chemistry section has neither.

How do you study for HESI A2 chemistry?

Begin with the parts everything else uses: the particles of the atom, the layout of the periodic table and the difference between ionic and covalent bonds. Then learn the formulas the problems use (moles, molarity, dilution, pH, half-life) by working problems on paper rather than rereading them. The chemistry review table on this page covers the facts. After each practice set, read the notes on the options you got wrong, and before test day take the timed chemistry section of a full practice exam.

What is a 70% on the HESI A2 chemistry section?

At some programs there is no chemistry score at all: Tarrant County College does not offer chemistry, and Quincy College's guide leaves it out. Where chemistry does count, the program's own minimum decides. Central New Mexico Community College requires 75% on every sub-test and on the composite, so a 70% in chemistry would miss its mark however strong your other sections are. Find the figure for your program on its admissions page; the HESI A2 practice test page explains scores further.

Is HESI A2 chemistry like TEAS science?

Only in part. The TEAS folds chemistry into its Science section: of the 44 scored questions in its 60-minute section, 8 are chemistry, so a TEAS taker meets a handful of chemistry items among the anatomy, biology and reasoning ones. A school that puts chemistry on its HESI A2 gives it a whole timed section of its own. Atoms, bonds, reactions and pH carry over between the two; for the TEAS, see the TEAS science practice test page.

Is there a free HESI A2 chemistry practice test?

Practice set 1 is free, with no sign-up. Beyond this page, HESI A2 Practice Exam 1 has a free chemistry section of 25 questions; it runs by itself if you tick only chemistry, with 25 minutes suggested. If you want a book, Chamberlain University's HESI page mentions that Elsevier's Admission Assessment Exam Review includes chemistry.

Are these real HESI A2 chemistry questions?

No. Every question here was made for this site from the topics schools publish for the chemistry section; none is copied from an Elsevier exam or book. NursePracticeTest is independent of Elsevier. Each comes with an explanation and a note on every option.

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Not affiliated with, endorsed by, or sponsored by Elsevier. HESI® is a trademark of Elsevier and is used here only to name the exam. Not affiliated with, endorsed by, or sponsored by Assessment Technologies Institute, LLC (ATI). ATI TEAS® and TEAS® are trademarks of ATI and are used here only to name the exam.

Pages this page relies on: Texas State Technical College Library Guides, Study Guide: HESI A2; Germanna Community College, HESI A2 Nursing Entrance Exam Preparation Guide (PDF, updated January 2023); Central New Mexico Community College, HESI A2 Exam; Tarrant County College, HESI A2 Exam Information; Quincy College Academic Division of Nursing, Preparing for the HESI A2 Admission Exam (PDF, updated December 2024); Chamberlain University, HESI Admission Assessment (A2) Exam; Western Technical College Library, Nursing: TEAS Prep Guide

Checked against the schools' pages and last reviewed November 4, 2026. Found an error? Tell us.