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Quizzes > Science

General Chemistry Quiz: Test Your Knowledge

Quick, free general chemistry 1 quiz to test your knowledge. Instant results.

Editorial: Review CompletedCreated By: Ninocka HajtnikUpdated Aug 25, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art of atoms, molecules, flasks and compounds on golden yellow background for a free chemistry quiz

This general chemistry quiz helps you check your understanding of atoms, bonding, reactions, and periodic trends with instant feedback. Warm up with a chemistry practice test, try a chemistry 101 quiz, or have fun with a chemistry trivia quiz, then come back to measure progress.

What is the atomic number of oxygen?
6
8
16
7
The atomic number represents the number of protons in an element. Oxygen has 8 protons in its nucleus, giving it an atomic number of 8. You can find more details about oxygen's properties here: .
Which of the following is a noble gas?
Nitrogen
Oxygen
Hydrogen
Helium
Noble gases are elements in Group 18 of the periodic table that are inert under standard conditions. Helium is a noble gas with a full outer electron shell. For more, see .
What is the chemical formula for water?
H2O2
HO
CO2
H2O
Water consists of two hydrogen atoms bonded to one oxygen atom, giving the formula H2O. Hydrogen peroxide (H2O2) is a different compound with an extra oxygen. More information at .
What is the pH of a neutral solution at 25°C?
1
0
7
14
At 25°C, the pH of pure water, which is neutral, is defined as 7. This is because [H+] equals [OH-] at 1×10^-7 M. More on pH scale here: .
Which subatomic particle has a negative charge?
Neutron
Proton
Electron
Photon
Electrons carry a negative charge, protons carry a positive charge, and neutrons are neutral. Photons are particles of light with no charge. See for more.
What is the molar mass of CO2?
28 g/mol
12 g/mol
32 g/mol
44 g/mol
Carbon dioxide (CO2) has one carbon atom (12.01 g/mol) and two oxygen atoms (2 × 16.00 g/mol), giving a total of about 44.01 g/mol. Reference: .
What is the chemical symbol for sodium?
Na
S
N
So
The symbol 'Na' comes from the Latin name 'Natrium' for sodium. S is sulfur, N is nitrogen, and 'So' is not an element symbol. More at .
What is the oxidation state of sulfur in H2SO4?
+2
+3
+4
+6
In H2SO4, hydrogen is +1 each (total +2) and oxygen is - 2 each (total - 8), so sulfur must be +6 to balance to zero. For more, see .
Which type of chemical bond involves the sharing of electron pairs between atoms?
Covalent bond
Hydrogen bond
Metallic bond
Ionic bond
Covalent bonds form when atoms share electron pairs to achieve stable electron configurations. Ionic bonds transfer electrons, metallic bonds involve a sea of delocalized electrons, and hydrogen bonds are intermolecular attractions. See .
What is the empirical formula of glucose (C6H12O6)?
CH2O
C2H4O2
CHO
C6H6
The empirical formula is the simplest whole-number ratio of atoms: C6H12O6 reduces to CH2O. It represents the ratio but not the actual molecule. More at .
Which gas is produced when acids react with carbonates?
Hydrogen
Nitrogen
Oxygen
Carbon dioxide
Acid - carbonate reactions produce carbon dioxide gas, water, and a salt. For instance, HCl + CaCO3 yields CO2, H2O, and CaCl2. See .
Which of these elements is an alkali metal?
Calcium
Magnesium
Aluminum
Lithium
Alkali metals occupy Group 1 of the periodic table; lithium is in that group. Magnesium is an alkaline earth metal, calcium is also Group 2, and aluminum is a post-transition metal. More info: .
What is the molecular geometry of methane (CH4)?
Trigonal planar
Tetrahedral
Linear
Octahedral
Methane has four bonding pairs around carbon with no lone pairs, giving a tetrahedral shape according to VSEPR theory. Bond angles are approximately 109.5°. See .
What is the conjugate base of hydrochloric acid (HCl)?
Cl?
H2Cl
H2O
Cl2
When HCl donates a proton (H?), the remaining species is Cl?, its conjugate base. Conjugate bases form when acids lose protons. More at .
In the periodic table, elements in the same group share which property?
Atomic radius
Number of energy levels
Number of valence electrons
Atomic mass
Elements in the same group have the same number of valence electrons, giving them similar chemical reactivity. Atomic mass and radius vary down a group, and energy levels increase. More: .
What is the pKa of acetic acid?
4.76
9.25
7.21
2.87
Acetic acid has a pKa of 4.76, meaning it is a weak acid that partially dissociates in solution. pKa is the negative log of the acid dissociation constant. More at .
In a redox reaction, the species that gains electrons is called the:
Oxidizing agent
Spectator ion
Catalyst
Reducing agent
The oxidizing agent is reduced by gaining electrons, causing another species to be oxidized. The reducing agent loses electrons. More: .
What is the product of the electrophilic bromination of benzene using Br2/FeBr3?
Cyclohexane
Bromobenzene
Phenol
Benzene tribromide
Electrophilic aromatic substitution of benzene with bromine and FeBr3 yields bromobenzene. The catalyst polarizes Br2 to form the electrophile. See .
Calculate the percent composition of oxygen in H2SO4.
65.3%
50.0%
47.0%
53.3%
H2SO4 has molecular mass ?98.08 g/mol; oxygen contributes 4×16.00 = 64.00 g. Percent = (64.00/98.08)×100 ?65.3%. More: .
Which compound is amphoteric, reacting both as an acid and a base?
Al(OH)3
H2SO4
NaOH
HCl
Aluminum hydroxide can donate protons in strong base and accept protons in strong acid, making it amphoteric. NaOH is only basic, HCl and H2SO4 are strong acids. See .
For the reaction 2A + B ? products, the rate doubles when [A] doubles and quadruples when [B] doubles. What is the rate law?
Rate = k[A][B]
Rate = k[A]^2[B]
Rate = k[A]^2[B]^2
Rate = k[A][B]^2
If rate doubles with [A] doubling, reaction is first order in A. If rate quadruples with [B] doubling, it is second order in B. Thus rate = k[A]^1[B]^2. More: .
Which orbital type corresponds to an angular momentum quantum number l = 2?
f orbital
p orbital
s orbital
d orbital
Quantum number l = 0,1,2,3 correspond to s, p, d, f orbitals respectively. Therefore l = 2 is a d orbital. More: .
What is the hybridization of the central atom in SF6?
sp3
sp3d
d2sp3
sp3d2
SF6 has six bonding domains around sulfur and adopts an octahedral shape, requiring sp3d2 hybridization. This uses one s, three p, and two d orbitals. More at .
Which molecule exhibits cis - trans isomerism?
Butane
2-Butene
Propane
Methane
Cis - trans isomerism requires a double bond with two different substituents on each carbon. 2-Butene fits this criterion, yielding cis and trans forms. See .
In the Born - Haber cycle for NaCl, which step is exothermic?
Ionization of Na
Bond dissociation of Cl2
Enthalpy of sublimation of Na
Lattice energy of NaCl
Lattice energy release occurs when gaseous Na+ and Cl? ions combine to form solid NaCl, releasing a large amount of energy. Other steps like sublimation and ionization are endothermic. More: .
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Study Outcomes

  1. Analyze Atomic and Molecular Structure -

    Identify the roles of protons, neutrons and electrons in atoms and distinguish common molecular geometries through questions featured in the general chemistry quiz.

  2. Evaluate Periodic Trends -

    Predict and compare atomic radius, ionization energy and electronegativity by interpreting periodic trends quiz items.

  3. Explain Chemical Bonding Principles -

    Differentiate ionic, covalent and metallic bonding types and apply bonding theories to challenges in the chemical bonding quiz.

  4. Balance Chemical Equations -

    Balance chemical equations by adjusting coefficients to uphold mass conservation in reaction problems.

  5. Solve Stoichiometric Problems -

    Perform stoichiometric calculations to determine reactant and product quantities, strengthening skills tested in the basic chemistry test.

Cheat Sheet

  1. Periodic Trends and Element Properties -

    Master trends like atomic radius, ionization energy, and electronegativity to predict element behavior in reactions. Use the mnemonic "FONCl - BrISCH" to remember Fluorine, Oxygen, Nitrogen, Chlorine, Bromine, Iodine, Sulfur, Carbon, Hydrogen - techniques recommended by IUPAC and top university courses. As you prep for your general chemistry quiz, these patterns help you gauge reactivity, bond strength, and ion formation.

  2. Chemical Bonding and VSEPR Theory -

    Differentiate ionic, covalent, and metallic bonds by electronegativity differences; for instance, ΔEN>1.7 typically indicates ionic bonding (Chemistry LibreTexts). Apply VSEPR to Lewis structures - CO₂'s linear O=C=O shape is a classic example from MIT OpenCourseWare. Grasping these fundamentals powers your chemical bonding quiz skills.

  3. Stoichiometry and Balancing Equations -

    Ensure mass and charge balance using the conservation of atoms: 2 H₂ + O₂ → 2 H₂O illustrates simple stoichiometric ratios, as featured in Zumdahl's textbooks. Convert between moles, mass, and molecules using Avogadro's number (6.022×10²³), a staple in every basic chemistry test. Accurate stoichiometry underpins yield predictions and reagent calculations in any chemistry knowledge quiz.

  4. Acid-Base Equilibria and pH Calculations -

    Know how to compute pH and pOH via pH=−log[H❺] and the Henderson - Hasselbalch equation for buffer systems, concepts detailed by the Royal Society of Chemistry. Recognize strong vs. weak acids (e.g., HCl vs. CH₃COOH) and practice titration curves - key for acid - base chemistry trivia questions. These calculations boost confidence on any periodic trends quiz section involving solution chemistry.

  5. Thermochemistry: Enthalpy and Calorimetry -

    Apply q=mcΔT to determine heat flow in calorimetry experiments, a formula emphasized by Khan Academy and respected journals. Memorize that ΔH°f values allow you to calculate reaction enthalpies via Hess's law, combining steps from standard tables. Solid thermodynamics knowledge will help you ace questions on energy changes in your general chemistry quiz.

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