Unlock hundreds more features
Save your Quiz to the Dashboard
View and Export Results
Use AI to Create Quizzes and Analyse Results

OR
Sign inSign in with Facebook
Sign inSign in with Google
Quizzes > Science > Chemistry

11th Grade Chemistry Quiz: Test Your Science Skills!

Dive into this 11th grade chemistry quiz online and challenge your knowledge!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art chemistry icons beaker atom test tube molecule model on coral background for 11th grade science quiz

This 11th grade chemistry quiz helps you practice atoms, elements, reactions, bonding, and balancing equations. You get instant feedback to spot gaps before a test and build strong skills. You also work with spectra and reaction rates. When you're set, open the quiz or start now .

What does the atomic number of an element represent?
The total number of protons and neutrons
The number of protons in the nucleus
The number of electrons in the atom
The number of neutrons in the nucleus
The atomic number is defined as the number of protons in an atom's nucleus. It uniquely identifies an element and determines its position on the periodic table. Electrons in a neutral atom equal the number of protons, but that is not the atomic number itself.
Which element is classified as an alkali metal?
Calcium (Ca)
Magnesium (Mg)
Sodium (Na)
Aluminum (Al)
Alkali metals occupy Group 1 of the periodic table and have a single valence electron. Sodium (Na) is the prototypical alkali metal, known for its high reactivity and soft metallic character. Calcium, magnesium, and aluminum belong to Groups 2 and 13 respectively and do not share these properties.
Which of these is the molecular formula for water?
CO2
CH4
N2
H2O
Water's molecular formula is H2O, indicating two hydrogen atoms bonded to one oxygen atom. Carbon dioxide (CO2) has one carbon and two oxygens, methane (CH4) has one carbon and four hydrogens, and nitrogen gas (N2) is a diatomic molecule of nitrogen. These formulas reflect different chemical properties and structures.
What is the pH of a neutral aqueous solution at 25°C?
14
1
7
4
At 25°C, pure water undergoes self-ionization producing equal concentrations of H+ and OH - ions, each 1×10?? M. The pH is defined as - log[H+], which in this case is 7. Solutions with pH less than 7 are acidic, while those above 7 are basic.
Which of the following is a noble gas?
Nitrogen (N2)
Fluorine (F2)
Oxygen (O2)
Neon (Ne)
Noble gases occupy Group 18 of the periodic table and are characterized by full valence electron shells, making them very unreactive. Neon (Ne) is one of these elements, whereas nitrogen, oxygen, and fluorine are diatomic nonmetals in other groups. This inertness leads to uses in lighting and welding.
How many valence electrons does an oxygen atom have?
6
2
4
8
Oxygen is in Group 16 of the periodic table, which means it has six valence electrons. These electrons are in the outermost shell and are involved in bonding and chemical reactions. Elements in the same group share the same valence electron count.
Who first proposed the periodic law leading to the modern periodic table?
Ernest Rutherford
Niels Bohr
Dmitri Mendeleev
John Dalton
Dmitri Mendeleev published the first recognizable periodic table in 1869, arranging elements by increasing atomic mass and grouping them by properties. His periodic law predicted the existence and properties of undiscovered elements. Rutherford and Bohr made key contributions to atomic structure, while Dalton proposed atomic theory.
What is the approximate value of Avogadro's number?
3.00×10^8 m/s
1.602×10^?19 C
6.022×10^23 mol^?1
9.81 m/s^2
Avogadro's number, 6.022×10^23, is the number of particles in one mole of substance. It provides the link between atomic scale measurements and macroscopic amounts of material. The other constants refer to the speed of light, the elementary charge, and gravitational acceleration.
Which element has the highest electronegativity on the Pauling scale?
Oxygen
Chlorine
Fluorine
Nitrogen
Fluorine is the most electronegative element with a Pauling value of 3.98. It has the strongest tendency to attract bonding electrons. Oxygen, chlorine, and nitrogen follow in decreasing electronegativity.
Which ion has the smallest ionic radius?
K?
Ca²?
Mg²?
Na?
Among these cations, Ca²? has the smallest ionic radius because it has a higher charge pulling electrons closer compared to the others. K?, Na?, and Mg²? have fewer protons per electron or lower charge density. Ionic radii decrease with increasing positive charge for ions of the same period.
In Boyle's law for an ideal gas, which variable remains constant?
Temperature
Number of moles
Pressure
Volume
Boyle's law states that for a fixed amount of gas at constant temperature, pressure and volume are inversely proportional. Temperature must remain constant for this relationship to hold. Changes in moles or temperature require other gas laws.
If 2 molecules of H? react with 1 molecule of O? to produce 2 molecules of H?O, how many molecules of H? are needed to produce 6 molecules of H?O?
3
9
12
6
The balanced equation shows a 1:1 molar ratio between H? and H?O. Thus, to produce 6 molecules of water, 6 molecules of hydrogen gas are required. Stoichiometry uses these ratios directly from the balanced reaction.
What are the units of the rate constant k for a second-order reaction?
mol/(L·s)
s?¹
unitless
L/(mol·s)
For a second-order reaction (rate = k[A]²), the rate constant k has units that make the rate (mol·L?¹·s?¹) match k[A]². Solving for k gives L/(mol·s). First-order reactions use s?¹.
Which of these is the strongest acid in aqueous solution?
Sulfuric acid (H?SO?)
Hydrochloric acid (HCl)
Hydrofluoric acid (HF)
Hydrobromic acid (HBr)
Sulfuric acid is a strong, diprotic acid that fully dissociates in its first proton release and is one of the strongest common laboratory acids. HCl and HBr are strong monoprotic acids but are slightly weaker than H?SO?'s first dissociation. HF is a weak acid due to strong H - F bond energy.
Which expression represents the equilibrium constant Kc for the reaction N? + 3H? ? 2NH??
([N?][H?]³)/[NH?]²
[NH?]³/([N?][H?]²)
[NH?]²/([N?][H?]³)
[NH?]/([N?]²[H?]³)
The equilibrium constant expression is products over reactants with each concentration raised to its stoichiometric coefficient. Therefore, Kc = [NH?]² ÷ ([N?][H?]³). The inverse or incorrect exponents do not match the balanced reaction.
Which compound can act as a Lewis acid?
Hydroxide ion (OH?)
Ammonia (NH?)
Boron trifluoride (BF?)
Water (H?O)
A Lewis acid is an electron-pair acceptor. BF? has an incomplete octet and can accept a pair of electrons. NH? and H?O are Lewis bases (electron-pair donors), and OH? donates electrons.
The carbon atoms in ethene (C?H?) each have which hybridization?
dsp²
sp²
sp³
sp
In ethene, each carbon forms three sigma bonds (two C - H and one C - C) and one ? bond. This trigonal planar arrangement corresponds to sp² hybridization. sp and sp³ hybridizations correspond to linear and tetrahedral geometries, respectively.
In an octahedral crystal field, which set of d orbitals experiences the highest energy?
e_g
d_xz
t?g
d_xy
In an octahedral field, the e_g orbitals (d_z² and d_x² - y²) point directly at ligand axes and experience greater repulsion, raising their energy above the t?g set. The t?g orbitals lie between axes and are lower in energy.
What is the oxidation state of manganese in the permanganate ion (MnO??)?
+6
+7
+4
+5
In MnO??, each oxygen is ?2, totaling ?8. The overall charge is ?1, so Mn must be +7 to balance: +7 + (?8) = ?1. Other oxidation states do not satisfy the charge balance.
Which solution will exhibit the highest boiling point elevation for a 1.0 m solution?
CaCl?
Glucose (C?H??O?)
NaCl
AlCl?
Boiling point elevation depends on the total number of solute particles (van 't Hoff factor). AlCl? dissociates into 4 ions, NaCl into 2, CaCl? into 3, and glucose into 1. Thus, 1 m AlCl? yields the greatest elevation.
What is the pH of a buffer solution where pKa = 4.76 and [A?]/[HA] = 1?
3.76
6.76
5.76
4.76
The Henderson - Hasselbalch equation is pH = pKa + log([A?]/[HA]). When the ratio [A?]/[HA] is 1, log(1) = 0, so pH = pKa. Here, pH = 4.76.
What is the standard cell potential E°?cell? for the galvanic cell Zn|Zn²? || Cu²?|Cu (E°Zn²?/Zn = ?0.76 V, E°C u²?/Cu = +0.34 V)?
0.34 V
0.42 V
1.10 V
-1.10 V
The standard cell potential is E°cell = E°cathode - E°anode = 0.34 V - ( - 0.76 V) = +1.10 V. Copper is reduced (cathode) and zinc is oxidized (anode). A negative sign would result from swapping electrodes.
According to the Arrhenius equation, if the activation energy increases at constant temperature, the rate constant k will:
Increase
Vary linearly with Ea
Decrease
Remain the same
The Arrhenius equation k = A·e^( - Ea/RT) shows that as the activation energy Ea increases, the exponential term decreases, reducing k. Temperature and frequency factor A held constant do not offset this. A higher barrier means fewer molecules can overcome it.
In a gas mixture at total pressure of 2 atm with nitrogen making up 25% of moles, what is the partial pressure of nitrogen?
2.0 atm
0.25 atm
0.5 atm
1.5 atm
Dalton's law states that partial pressure = mole fraction × total pressure. Nitrogen's mole fraction is 0.25, so its partial pressure is 0.25 × 2 atm = 0.5 atm. The others misapply the fraction or total.
What is the maximum number of electrons that can occupy the principal energy level n = 3?
6
8
32
18
The maximum number of electrons in a shell is given by 2n². For n = 3, this is 2 × 3² = 18 electrons. This includes the 3s, 3p, and 3d subshells.
0
{"name":"What does the atomic number of an element represent?", "url":"https://www.quiz-maker.com/QPREVIEW","txt":"What does the atomic number of an element represent?, Which element is classified as an alkali metal?, Which of these is the molecular formula for water?","img":"https://www.quiz-maker.com/3012/images/ogquiz.png"}

Study Outcomes

  1. Understand Periodic Table Trends -

    After completing the quiz, you'll interpret periodic trends like electronegativity, atomic radius, and ionization energy for various elements.

  2. Analyze Chemical Equations -

    Balance complex reactions, identify limiting reactants, and predict product formation to reinforce equation-solving skills.

  3. Apply Stoichiometry Concepts -

    Calculate molar relationships and reagent quantities to solve real-world stoichiometry problems with confidence.

  4. Evaluate Acid-Base and Redox Reactions -

    Classify and compare reactions by pH changes, redox processes, and reaction mechanisms in diverse scenarios.

  5. Interpret Molecular Formulas -

    Deduce compound composition and structure from molecular and empirical formulas to enhance formula-based reasoning.

  6. Strengthen Problem-Solving Skills -

    Tackle 11th grade science questions with improved strategies, boosting accuracy and exam readiness for high school chemistry.

Cheat Sheet

  1. Periodic Trends -

    Review how atomic radius, ionization energy, and electronegativity change across periods and groups. For example, ionization energy increases moving right across a period due to higher nuclear charge. A helpful mnemonic is FONClBrISCH to recall the most electronegative elements in order.

  2. Stoichiometric Calculations -

    Practice converting grams to moles and moles to particles using molar mass and Avogadro's number (6.022×1023). For instance, find moles of H2O in 36 g by dividing by 18 g/mol. Always balance the chemical equation before computing reactant-product relationships.

  3. Chemical Reaction Types -

    Classify reactions as synthesis, decomposition, single or double displacement, and redox. Use the OIL RIG mnemonic (Oxidation Is Loss, Reduction Is Gain) to identify electron transfer. Example: Zn + CuSO4 → ZnSO4 + Cu is a single-displacement redox reaction.

  4. Acid-Base Equilibria -

    Understand Brønsted - Lowry acids (H+ donors) and bases (H+ acceptors), and practice pH = -log[H+] calculations. For weak acids, apply the Henderson - Hasselbalch equation: pH = pKa + log([A−]/[HA]). Buffers maintain pH by shifting this equilibrium.

  5. Thermochemistry & Spontaneity -

    Review enthalpy (ΔH), entropy (ΔS), and Gibbs free energy (ΔG = ΔH − TΔS). A negative ΔG indicates a spontaneous process under constant conditions. For example, CH4 combustion has ΔH° = -890 kJ/mol, showing it's exothermic and thermodynamically favorable.

Make a Quiz (FREE) Copy & Edit This Quiz Create a Quiz with AI

Chemistry Quizzes

Powered by: Quiz Maker