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Quizzes > Science > Chemistry

Chemistry 101 Quiz: Challenge Your Chemistry Knowledge!

Think you can master this basic chemistry quiz? Tackle fun chemistry practice questions now!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration for Chemistry 101 quiz on dark blue background

This Chemistry 101 quiz helps you practice the basics - equations, reactions, the periodic table, and lab safety - so you can study smarter and spot gaps before a test. Take it at your pace and see what to review next. For more practice, try a basic quiz or review lab safety .

What does the atomic number of an element represent?
Number of neutrons
Number of protons
Number of isotopes
Atomic mass
The atomic number equals the number of protons in an atom's nucleus, which uniquely identifies an element. It does not count neutrons or include mass. This fundamental property orders the periodic table. .
Which element has the atomic number 1?
Hydrogen
Helium
Carbon
Oxygen
Hydrogen has an atomic number of 1 because it contains a single proton in its nucleus. Helium (atomic number 2) and others have more. This makes hydrogen the simplest element. .
Which group in the periodic table contains the noble gases?
Group 2
Group 16
Group 12
Group 18
The noble gases occupy Group 18 and are characterized by their full valence electron shells, making them very unreactive. Group 2 contains alkaline earth metals, while Groups 16 and 12 contain chalcogens and zinc group elements respectively. .
What is the chemical symbol for sodium?
Na
So
N
S
Sodium's chemical symbol is Na, derived from its Latin name 'natrium'. 'S' stands for sulfur, 'N' for nitrogen, and 'So' is not used. .
What is the molecular formula for water?
H2O2
H2O
HO2
OH2
Water consists of two hydrogen atoms bonded to one oxygen atom, giving the molecular formula H2O. H2O2 is hydrogen peroxide, and HO2 or OH2 are incorrect structures. .
A solution with a pH less than 7 is considered:
Acidic
Basic
Alkaline
Neutral
pH values below 7 indicate acidity due to higher hydrogen ion concentration. Values above 7 are basic or alkaline, and exactly 7 is neutral. This scale is logarithmic. .
Which subatomic particle carries a negative charge?
Proton
Electron
Neutron
Photon
Electrons carry a negative charge, while protons are positive, and neutrons are neutral. Photons are particles of light and have no charge. Electron behavior determines chemical bonding. .
What is the mass of one mole of carbon-12?
1 gram
12 atomic mass units
6.022×10^23 grams
12 grams
By definition, one mole of carbon-12 has a mass of exactly 12 grams. Avogadro's number (6.022×10^23) is the count of atoms, not the mass in grams. Atomic mass units are a different scale. .
What is the empirical formula of glucose (C6H12O6)?
C6H12O6
CH2O
C2H4O2
C3H6O3
The empirical formula is the simplest whole-number ratio of atoms: C6H12O6 reduces to CH2O. C2H4O2 and C3H6O3 are formulas for acetic acid and lactic acid, respectively. .
What term describes the coefficients in a balanced chemical equation?
Molecular weights
Percent yield
Stoichiometric coefficients
Limiting reagents
Stoichiometric coefficients indicate the relative number of moles of each substance in a balanced equation. Limiting reagents and percent yield describe reaction extents and efficiencies. Molecular weights are unrelated. .
What type of bond is formed when two atoms share electrons?
Ionic bond
Hydrogen bond
Metallic bond
Covalent bond
Covalent bonds result from atoms sharing electron pairs. Ionic bonds transfer electrons between atoms, metallic bonds occur between metal atoms, and hydrogen bonds are weak interactions. .
What is the mass percent of oxygen in water (H2O)?
50%
88.89%
66.67%
11.11%
Oxygen's atomic mass (16) divided by the molar mass of water (18) gives 16/18×100 ? 88.89%. The remaining 11.11% is from the two hydrogen atoms. .
A solution has [H+] = 1×10^-3 M. What is its pH?
11
7
3
-3
pH is calculated as -log[H+], so -log(1×10^-3)=3. A pH of 7 is neutral, and 11 or negative values do not apply here. .
In an exothermic reaction, heat is:
Released to the surroundings
Conserved within the system
Not involved
Absorbed from the surroundings
Exothermic reactions release heat into their surroundings. Endothermic reactions absorb heat. Heat conservation or lack of involvement is incorrect. .
Boyle's law describes which relationship at constant temperature?
Pressure is directly proportional to volume
Pressure is inversely proportional to volume
Volume is directly proportional to temperature
Pressure is directly proportional to temperature
Boyle's law states P?1/V at constant temperature. Charles's and Gay-Lussac's laws describe temperature and volume or pressure relationships. .
In the combustion of methane (CH4), how many moles of water are produced from 3 moles of CH4?
3
12
9
6
The balanced equation CH4 + 2O2 ? CO2 + 2H2O shows that 1 mole CH4 yields 2 moles H2O. Thus, 3 moles CH4 produce 3×2=6 moles of water. .
What is the conjugate base of H2SO4?
H3SO4+
SO4-
SO4^2-
HSO4-
When H2SO4 donates a proton, it forms HSO4-, making it the conjugate base. SO4^2- is formed after a second deprotonation. .
What is the oxidation number of sulfur in SO2?
+4
+2
+6
-2
Oxygen is -2 each, so 2×(-2) = -4. To balance to zero charge, sulfur must be +4. .
Which expression represents the equilibrium constant Kc for N2 + 3H2 ? 2NH3?
[N2]^2 [H2]^3 / [NH3]^2
[NH3]^2 / ([N2][H2]^3)
[NH3]^3 / ([N2][H2]^2)
([N2][H2]^3) / [NH3]^2
Kc = products^coefficients over reactants^coefficients: [NH3]^2 / ([N2][H2]^3). The other forms invert or misapply coefficients. .
What term describes the minimum energy required for a chemical reaction to proceed?
Enthalpy
Activation potential
Activation energy
Free energy
Activation energy is the energy barrier reactants must overcome to form products. Enthalpy is heat content, free energy indicates spontaneity, and activation potential is not standard. .
What is the pressure of 0.5 moles of an ideal gas in a 10 L container at 300 K? (R = 0.08206 L·atm/mol·K)
1.23 atm
0.12 atm
0.37 atm
12.3 atm
Using PV=nRT gives P=(0.5×0.08206×300)/10?1.23 atm. The other values result from calculation errors or unit mismatches. .
What is the molarity of a solution containing 0.5 moles of solute in 2 liters of solution?
4 M
0.5 M
0.1 M
0.25 M
Molarity is moles divided by volume in liters: 0.5 mol / 2 L = 0.25 M. The other options result from incorrect division. .
In a titration of 0.1 M HCl with 0.1 M NaOH, what is the pH at the equivalence point?
Depends on temperature
5
9
7
A strong acid-strong base titration yields a neutral solution at equivalence, so pH = 7 at 25°C. Temperature effects are minimal in ideal cases. .
Calculate the standard cell potential E° for a galvanic cell using Cu2+/Cu (+0.34 V) and Zn2+/Zn (-0.76 V) half-reactions.
-1.10 V
0.58 V
0.42 V
1.10 V
E°cell = E°cathode - E°anode = 0.34 V - (-0.76 V) = 1.10 V. Reversing signs or adding incorrectly yields other values. .
If the equilibrium constant K for a reaction at 25°C is 1×10^5, what is the sign of ?G°?
Cannot determine
Negative
Positive
Zero
?G° = -RT ln K. Since K > 1, ln K is positive, making ?G° negative and indicating spontaneity under standard conditions. .
0
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Study Outcomes

  1. Understand Atomic Structure -

    Identify the basic components of an atom, including protons, neutrons and electrons, and explain how their arrangement defines each element.

  2. Apply Periodic Table Principles -

    Use group and period trends to predict an element's properties, such as reactivity, atomic radius and ionization energy.

  3. Classify Chemical Reactions -

    Recognize and differentiate between synthesis, decomposition, single replacement and double replacement reactions.

  4. Interpret and Balance Equations -

    Translate word descriptions into chemical equations and balance them to reflect the law of conservation of mass.

  5. Analyze Molecular Formulas -

    Determine molecular composition and calculate molar mass from chemical formulas.

  6. Apply Laboratory Safety Protocols -

    Identify key safety symbols and best practices to handle chemicals and equipment responsibly.

Cheat Sheet

  1. Atomic Structure Basics -

    An atom's identity is defined by its proton count (atomic number) while its mass number sums protons and neutrons; for example, carbon's isotopes C-12 and C-14 share 6 protons but have different neutrons. Electrons occupy energy levels or orbitals around the nucleus following the Aufbau principle. Remember: "2n²" predicts the maximum electrons in a shell (n being the shell number).

  2. Periodic Table Trends -

    Trends like electronegativity, ionization energy, and atomic radius vary predictably across periods and groups. Electronegativity generally increases left to right and bottom to top, while atomic radius does the opposite. Use the mnemonic "FONClBrISCH" to remember high-electronegativity elements (Fluorine, Oxygen, Nitrogen, Chlorine, Bromine, Iodine, Sulfur, Carbon, Hydrogen).

  3. Chemical Bonding and Molecular Shapes -

    Ionic bonds form via electron transfer (e.g., NaCl), covalent bonds share electrons (e.g., H₂O), and metallic bonds pool electrons in a lattice. Lewis dot structures help visualize valence electrons and predict molecular shapes using VSEPR theory. Practice drawing NH₃ (trigonal pyramidal) or CO₂ (linear) to master bond angles.

  4. Reaction Types and Equation Balancing -

    Common reaction types include synthesis (A + B → AB), decomposition (AB → A + B), single replacement, and combustion. Balancing equations conserves mass; ensure the same number of each atom appears on both sides (e.g., 2H₂ + O₂ → 2H₂O). Use "OIL RIG" (Oxidation Is Loss, Reduction Is Gain) to track electron transfers in redox reactions.

  5. Essential Lab Safety Practices -

    Always wear safety goggles, gloves, and a lab coat to protect against chemical splashes and spills; know the locations of eyewash stations and fire extinguishers. Understand MSDS sheets for hazards and proper handling of each chemical. Follow the "no food or drink in the lab" rule to avoid accidental ingestion of toxic substances.

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