Chemistry Quiz

11 – 27 Questions 10 min

This chemistry quiz focuses on core general chemistry concepts, including atoms, molecules, reactions, and simple calculations that practicing chemists and students use every day. Questions check your ability to interpret formulas, balance equations, predict products, and reason with units, which helps high school and college learners, lab technicians, and pre health students solidify foundations.

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Part 1 — Questions

Answer each question on paper. Do not turn the page until you are ready to check your work.

In a basic chemistry quiz, which subatomic particle in an atom carries a negative electric charge?

Proton
Electron
Nucleus
Neutron

An element is defined by the number of protons in the nucleus of its atoms.

True
False

A student compares sodium and potassium during a general chemistry quiz. Both are in Group 1, but potassium is below sodium. Which statement about their first ionization energies is most accurate?

Potassium has a higher first ionization energy because it is more reactive.
Sodium has a lower first ionization energy because it is smaller.
Their first ionization energies are identical because they are in the same group.
Potassium has a lower first ionization energy because its outer electron is farther from the nucleus.

In a general chemistry quiz, a sample of solid sodium chloride is heated and does not melt until a very high temperature. What best explains this high melting point?

Its atoms form a continuous network of covalent bonds like in diamond.
Its ions are held together by strong electrostatic attractions in a crystal lattice.
Its molecules are held together only by weak London dispersion forces.
Its particles are bonded by metallic bonding among sodium atoms only.

A solution at 25 °C has a hydrogen ion concentration [H⁺] of 1.0 × 10⁻⁹ M. How would this solution be classified in a basic chemistry quiz?

Strongly acidic
Basic
Neutral
Weakly acidic

Liquid water in an open beaker is heated from 25 °C to 80 °C at constant pressure. Which property of the water definitely increases during this process?

Average kinetic energy of molecules
Molar mass
Density
Chemical composition

Solid sodium chloride conducts electricity well because its ions can move freely within the crystal lattice.

True
False

A student completely reacts 2.0 mol of O₂ with excess H₂ according to the balanced equation 2 H₂ + O₂ → 2 H₂O. How many moles of water are produced?

2.0 mol
4.0 mol
3.0 mol
1.0 mol

A flexible balloon is filled with helium gas at room temperature and atmospheric pressure, then placed in a freezer while the outside pressure remains the same. What happens to the gas in the balloon?

Its mass decreases.
The pressure inside the balloon increases.
The number of moles of gas increases.
Its volume decreases.

10.

A student observes that a reaction mixture becomes noticeably warmer to the touch as the reaction proceeds. Which description of the reaction is most appropriate?

The reaction has zero enthalpy change because temperature increases are not energy changes.
The reaction has a positive enthalpy change and releases heat to the surroundings.
The reaction has a positive enthalpy change and absorbs heat from the surroundings.
The reaction has a negative enthalpy change and releases heat to the surroundings.

11.

In a displacement reaction used in a general chemistry quiz, a strip of zinc metal is placed in a solution of copper(II) sulfate and copper metal forms. Which species is oxidized in this reaction?

SO₄²⁻(aq)
H₂O(l)
Cu²⁺(aq)
Zn(s)

12.

In a chemical reaction, the reactant that is completely consumed first is called the limiting reagent.

True
False

13.

As you move from left to right across a single period of the periodic table for main group elements, which of the following general trends occur? Select all that apply.

A.Metallic character generally increases.
B.First ionization energy generally increases.
C.Atomic radius generally decreases.
D.The number of valence electrons stays the same.
E.Nuclear charge increases.

14.

A student is performing a basic acid–base titration of an acid in a flask with a standardized base in a buret. Arrange the following steps in the correct order.

Put these in the correct order (write 1–5 beside each):

____Slowly add base from the buret while swirling the flask.
____Stop adding base at the first persistent color change in the flask.
____Add a few drops of indicator to the acid in the flask.
____Fill the buret with the standardized base solution.
____Measure a known volume of the acid solution into an Erlenmeyer flask.

15.

In a basic chemistry lab, a student dissolves 5.8 g of NaCl in water and dilutes the solution to a final volume of 500 mL. Approximately what is the molarity of the NaCl solution? (Molar mass of NaCl ≈ 58.5 g/mol.)

1.0 M
0.20 M
0.50 M
0.10 M

16.

A sealed container holds a mixture of colorless N₂O₄(g) and brown NO₂(g) at equilibrium: N₂O₄(g) ⇌ 2 NO₂(g). The container is suddenly compressed, decreasing the volume at constant temperature. What is the most likely observable change?

The equilibrium shifts toward NO₂, and the gas mixture becomes darker in color.
The equilibrium does not shift because temperature is constant.
The equilibrium shifts toward N₂O₄, and the gas mixture becomes lighter in color.
The reaction stops because the container volume changed.

17.

In an introductory chemistry titration, a strong monoprotic acid is titrated with a strong base at 25 °C. At the equivalence point, which statements are true? Select all that apply.

A.The concentrations of acid and base in the flask are equal.
B.The moles of H⁺ originally present equal the moles of OH⁻ added.
C.The solution contains only pure water.
D.The pH is approximately 7.

18.

A covalent liquid has a relatively high boiling point, mixes well with water, and does not conduct electricity as a pure liquid. Ignoring the universal presence of London dispersion forces, which intermolecular forces are most likely important between its molecules? Select all that apply.

A.London dispersion forces
B.Metallic bonding
C.Dipole–dipole forces
D.Hydrogen bonding

19.

A student mixes aqueous sodium carbonate with aqueous calcium chloride and observes a white solid form. Considering the net ionic equation for this precipitation reaction, which species appear in that net ionic equation? Select all that apply.

A.Na⁺(aq)
B.CO₃²⁻(aq)
C.Cl⁻(aq)
D.CaCO₃(s)
E.Ca²⁺(aq)

Part 2 — Answer key

Compare your answers after you have finished Part 1.

In a basic chemistry quiz, which subatomic particle in an atom carries a negative electric charge?
Electron
An element is defined by the number of protons in the nucleus of its atoms.
True
A student compares sodium and potassium during a general chemistry quiz. Both are in Group 1, but potassium is below sodium. Which statement about their first ionization energies is most accurate?
Potassium has a lower first ionization energy because its outer electron is farther from the nucleus.
In a general chemistry quiz, a sample of solid sodium chloride is heated and does not melt until a very high temperature. What best explains this high melting point?
Its ions are held together by strong electrostatic attractions in a crystal lattice.
A solution at 25 °C has a hydrogen ion concentration [H⁺] of 1.0 × 10⁻⁹ M. How would this solution be classified in a basic chemistry quiz?
Basic
Liquid water in an open beaker is heated from 25 °C to 80 °C at constant pressure. Which property of the water definitely increases during this process?
Average kinetic energy of molecules
Solid sodium chloride conducts electricity well because its ions can move freely within the crystal lattice.
False
A student completely reacts 2.0 mol of O₂ with excess H₂ according to the balanced equation 2 H₂ + O₂ → 2 H₂O. How many moles of water are produced?
4.0 mol
A flexible balloon is filled with helium gas at room temperature and atmospheric pressure, then placed in a freezer while the outside pressure remains the same. What happens to the gas in the balloon?
Its volume decreases.
A student observes that a reaction mixture becomes noticeably warmer to the touch as the reaction proceeds. Which description of the reaction is most appropriate?
The reaction has a negative enthalpy change and releases heat to the surroundings.
In a displacement reaction used in a general chemistry quiz, a strip of zinc metal is placed in a solution of copper(II) sulfate and copper metal forms. Which species is oxidized in this reaction?
Zn(s)
In a chemical reaction, the reactant that is completely consumed first is called the limiting reagent.
True
As you move from left to right across a single period of the periodic table for main group elements, which of the following general trends occur? Select all that apply.
First ionization energy generally increases.; Atomic radius generally decreases.; Nuclear charge increases.
A student is performing a basic acid–base titration of an acid in a flask with a standardized base in a buret. Arrange the following steps in the correct order.
Correct order: Fill the buret with the standardized base solution. → Measure a known volume of the acid solution into an Erlenmeyer flask. → Add a few drops of indicator to the acid in the flask. → Slowly add base from the buret while swirling the flask. → Stop adding base at the first persistent color change in the flask.
In a basic chemistry lab, a student dissolves 5.8 g of NaCl in water and dilutes the solution to a final volume of 500 mL. Approximately what is the molarity of the NaCl solution? (Molar mass of NaCl ≈ 58.5 g/mol.)
0.20 M
A sealed container holds a mixture of colorless N₂O₄(g) and brown NO₂(g) at equilibrium: N₂O₄(g) ⇌ 2 NO₂(g). The container is suddenly compressed, decreasing the volume at constant temperature. What is the most likely observable change?
The equilibrium shifts toward N₂O₄, and the gas mixture becomes lighter in color.
In an introductory chemistry titration, a strong monoprotic acid is titrated with a strong base at 25 °C. At the equivalence point, which statements are true? Select all that apply.
The moles of H⁺ originally present equal the moles of OH⁻ added.; The pH is approximately 7.
A covalent liquid has a relatively high boiling point, mixes well with water, and does not conduct electricity as a pure liquid. Ignoring the universal presence of London dispersion forces, which intermolecular forces are most likely important between its molecules? Select all that apply.
Dipole–dipole forces; Hydrogen bonding
A student mixes aqueous sodium carbonate with aqueous calcium chloride and observes a white solid form. Considering the net ionic equation for this precipitation reaction, which species appear in that net ionic equation? Select all that apply.
CO₃²⁻(aq); CaCO₃(s); Ca²⁺(aq)

1In a basic chemistry quiz, which subatomic particle in an atom carries a negative electric charge?

2An element is defined by the number of protons in the nucleus of its atoms.

True / False

3A student compares sodium and potassium during a general chemistry quiz. Both are in Group 1, but potassium is below sodium. Which statement about their first ionization energies is most accurate?

4In a general chemistry quiz, a sample of solid sodium chloride is heated and does not melt until a very high temperature. What best explains this high melting point?

5A solution at 25 °C has a hydrogen ion concentration [H⁺] of 1.0 × 10⁻⁹ M. How would this solution be classified in a basic chemistry quiz?

6Liquid water in an open beaker is heated from 25 °C to 80 °C at constant pressure. Which property of the water definitely increases during this process?

7Solid sodium chloride conducts electricity well because its ions can move freely within the crystal lattice.

True / False

8A student completely reacts 2.0 mol of O₂ with excess H₂ according to the balanced equation 2 H₂ + O₂ → 2 H₂O. How many moles of water are produced?

9A flexible balloon is filled with helium gas at room temperature and atmospheric pressure, then placed in a freezer while the outside pressure remains the same. What happens to the gas in the balloon?

10A student observes that a reaction mixture becomes noticeably warmer to the touch as the reaction proceeds. Which description of the reaction is most appropriate?

11In a displacement reaction used in a general chemistry quiz, a strip of zinc metal is placed in a solution of copper(II) sulfate and copper metal forms. Which species is oxidized in this reaction?

12In a chemical reaction, the reactant that is completely consumed first is called the limiting reagent.

True / False

13As you move from left to right across a single period of the periodic table for main group elements, which of the following general trends occur? Select all that apply.

Select all that apply

14A student is performing a basic acid–base titration of an acid in a flask with a standardized base in a buret. Arrange the following steps in the correct order.

Put in order

1Slowly add base from the buret while swirling the flask.

2Stop adding base at the first persistent color change in the flask.

3Add a few drops of indicator to the acid in the flask.

4Fill the buret with the standardized base solution.

5Measure a known volume of the acid solution into an Erlenmeyer flask.

15In a basic chemistry lab, a student dissolves 5.8 g of NaCl in water and dilutes the solution to a final volume of 500 mL. Approximately what is the molarity of the NaCl solution? (Molar mass of NaCl ≈ 58.5 g/mol.)

16A sealed container holds a mixture of colorless N₂O₄(g) and brown NO₂(g) at equilibrium: N₂O₄(g) ⇌ 2 NO₂(g). The container is suddenly compressed, decreasing the volume at constant temperature. What is the most likely observable change?

17In an introductory chemistry titration, a strong monoprotic acid is titrated with a strong base at 25 °C. At the equivalence point, which statements are true? Select all that apply.

Select all that apply

18A covalent liquid has a relatively high boiling point, mixes well with water, and does not conduct electricity as a pure liquid. Ignoring the universal presence of London dispersion forces, which intermolecular forces are most likely important between its molecules? Select all that apply.

Select all that apply

19A student mixes aqueous sodium carbonate with aqueous calcium chloride and observes a white solid form. Considering the net ionic equation for this precipitation reaction, which species appear in that net ionic equation? Select all that apply.

Select all that apply

Frequent Concept Mistakes on General Chemistry Quiz Problems

Stoichiometry and unit handling

Many learners plug numbers into mole and molarity formulas without checking units. They mix grams, kilograms, and milliliters in one calculation. Convert all quantities to base units first, such as grams, liters, and moles. Track units algebraically, and cancel them step by step so the final unit matches the question.

Balancing and interpreting equations

Some test takers balance chemical equations by changing subscripts instead of coefficients. This changes the identity of the substance. Always adjust only coefficients. After balancing, check that both atoms and total charge match on each side. Do a quick ratio check to see which reactant limits the reaction before computing theoretical yield.

Atomic structure and periodic trends

Students often confuse atomic number with mass number. Atomic number is the proton count. Mass number is protons plus neutrons. Another frequent slip is to memorize periodic trends without context. Relate trends like atomic radius and ionization energy to effective nuclear charge, and compare elements within the same period or group.

Acids, bases, and pH reasoning

Quiz takers may treat pH as a linear scale. It is logarithmic. A solution with pH 3 is one hundred times more acidic than pH 5. Use pH = -log[H⁺] and [H⁺] = 10^-pH. Check whether the prompt expects a qualitative comparison or a calculated hydrogen ion concentration.

Physical versus chemical changes

Another error is to label dissolving, melting, or boiling as chemical changes. These are physical changes because particle identity stays the same. Focus on whether new substances form. If only spacing or arrangement of particles changes, classify the process as physical, not chemical.

Printable General Chemistry Quick Reference Sheet

How to use this sheet

Use this general chemistry quick reference while you work through chemistry quiz questions. Print it or save as a PDF so you can annotate key formulas, constants, and patterns as you practice calculations and conceptual problems.

Core quantities and constants

Avogadro constant: N_A ≈ 6.02 × 10²³ particles per mole.
Mole definition: n = mass (g) ÷ molar mass (g mol^-1).
Density: ρ = m ÷ V, units often g mL^-1 or g cm^-3.

Stoichiometry and solutions

Moles from volume of solution: n = M × V, where M is molarity (mol L^-1) and V is volume in liters.
General stoichiometry steps:
1. Write and balance the equation.
2. Convert given quantities to moles.
3. Use mole ratios from coefficients.
4. Convert moles of target substance to required units.
Dilution: M₁V₁ = M₂V₂.

Gas relationships

Ideal gas law: PV = nRT, with P in atm, V in L, n in mol, T in K.
Common gas constant: R = 0.0821 L atm mol^-1 K^-1.
Convert Celsius to Kelvin with T(K) = T(°C) + 273.

Energy and thermochemistry

Heat: q = m c ΔT, where m is mass, c is specific heat, ΔT is temperature change.
Exothermic: system releases heat, ΔH < 0. Endothermic: system absorbs heat, ΔH > 0.

Acids, bases, and pH

pH = -log[H⁺].
[H⁺] = 10^-pH.
At 25 °C, neutral water has pH 7, [H⁺] = 1.0 × 10^-7 M.

Periodic trends and bonding

Across a period: atomic radius decreases, ionization energy and electronegativity increase.
Down a group: atomic radius increases, ionization energy generally decreases.
Ionic bonds form between metals and nonmetals. Covalent bonds form between nonmetals.
Polar covalent bonds have unequal electron sharing due to electronegativity difference.

Worked General Chemistry Quiz Question Examples with Stepwise Reasoning

Example 1: Moles from mass and mole ratio

Question: How many moles of CO₂ form when 11.0 g of C react completely with excess O₂? Equation: C + O₂ → CO₂.

Find moles of C: molar mass of C ≈ 12.0 g mol^-1. n(C) = 11.0 g ÷ 12.0 g mol^-1 ≈ 0.917 mol.
Use mole ratio: Coefficients are 1 C to 1 CO₂. Moles of CO₂ = 0.917 mol.
Answer: About 0.92 mol of CO₂ are produced.

Example 2: Solution molarity

Question: What is the molarity of a NaCl solution made by dissolving 5.85 g NaCl in enough water to make 250. mL of solution?

Convert mass to moles: molar mass NaCl ≈ 58.5 g mol^-1. n = 5.85 g ÷ 58.5 g mol^-1 = 0.100 mol.
Convert volume to liters: 250. mL = 0.250 L.
Apply molarity formula: M = n ÷ V = 0.100 mol ÷ 0.250 L = 0.400 M.
Answer: The solution is 0.400 M NaCl.

Example 3: Predicting relative atomic size

Question: Which atom is larger, Na or K?

Locate on the periodic table: Na and K are in the same group, with K below Na.
Recall trend: Atomic radius increases down a group because additional energy levels are added.
Answer: K has the larger atomic radius compared with Na.

General Chemistry Quiz Practice FAQ

What topics does this general chemistry quiz focus on?

The quiz centers on basic atomic structure, periodic trends, bonding, stoichiometry, gases, simple thermochemistry, and introductory acids and bases. You will see both conceptual items and short calculations that reflect common questions in a first high school or college general chemistry course.

How challenging are the chemistry quiz questions?

Difficulty ranges from easy identification questions, such as classifying changes as physical or chemical, to multi step calculations, such as mole conversions and solution molarity. The quiz targets learners who already know core terms and want to check how fluently they can apply them without a formula sheet.

What math skills do I need for this chemistry quiz?

You should be comfortable with scientific notation, unit conversions, ratios, and rearranging simple equations. A calculator helps for gas law and stoichiometry questions. The focus is on setting up relationships correctly, not on advanced algebra, so careful unit tracking matters more than heavy computation.

How can I use this quiz to study more effectively?

First complete a quiz mode without notes so you see your current level. Then review every missed or guessed question. Identify which formulas, definitions, or trends you misused. Rewrite a correct solution in your own words, and create a small practice set that targets that specific weakness.

Who benefits most from taking a general chemistry quiz like this?

High school and college students in an introductory chemistry course gain quick feedback on core topics before tests. Pre health and engineering majors can refresh prerequisite material. Teachers and tutors can use results to spot common trouble areas and build focused practice sets for their classes.