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Quizzes > Science

AP Chemistry Chapter 1 Quiz: Chemical Foundations

Quick, free quiz for your AP Chemistry chapter 1 test prep. Instant results.

Editorial: Review CompletedCreated By: Elisabeth HeniscaUpdated Aug 27, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art molecules flasks atoms periodic table on teal background for AP Chemistry Chapter 1 foundations quiz

This quiz helps you practice AP Chemistry Chapter 1 topics like atoms, molecules, and measurement, with instant feedback on each question. Use it to check what you know before a unit test and spot gaps fast. For more practice, try the intro to chemistry quiz, move on to the chemistry chapter 2 quiz, or challenge yourself with a chapter 4 chemistry test.

Which of the following is a chemical change?
Dissolving sugar in water
Cutting a sheet of paper
Melting ice
Rusting iron
Rusting iron involves oxidation and the formation of new compounds (iron oxides), which is characteristic of a chemical change. Physical changes, like melting or cutting, do not form new substances. Dissolving sugar is a physical process because the sugar molecules remain chemically unchanged.
Which SI unit measures the amount of substance?
Liter (L)
Ampere (A)
Gram (g)
Mole (mol)
The mole is the SI base unit for the amount of substance, defined by Avogadro's number of entities. Grams measure mass, liters measure volume, and amperes measure electric current. Understanding SI units is fundamental in chemistry measurements.
How many significant figures are in the measurement 0.00420?
1
3
2
4
Leading zeros do not count as significant figures, but all nonzero digits and any zeros between or after them do. In 0.00420, the digits 4, 2, and the trailing zero are significant, giving three significant figures. Proper sig-fig practice ensures accurate reporting of measurements.
What is the density of an object with a mass of 10 g and a volume of 2 cm³?
0.2 g/cm³
2 g/cm³
20 g/cm³
5 g/cm³
Density is mass divided by volume (d = m/V). For a mass of 10 g and volume of 2 cm³, the density is 10 g ÷ 2 cm³ = 5 g/cm³. This property is intrinsic to the material and helps in substance identification.
Which of the following is a homogeneous mixture?
Air
Granite
Oil and water
Tossed salad
A homogeneous mixture has a uniform composition throughout. Air is a single-phase mixture of gases, making it homogeneous. Salad and granite have visibly distinct components, and oil and water form separate layers.
What is the empirical formula of a compound containing 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass?
CH2O2
CH2O
C2H4O
CHO
Convert percentages to moles: C:40/12=3.33, H:6.7/1=6.70, O:53.3/16=3.33. The ratio is 1:2:1 for C:H:O, giving CH?O as the empirical formula. Empirical formulas show the simplest whole-number ratio.
Which quantum number indicates the shape of an atomic orbital?
Magnetic (m?)
Azimuthal (l)
Principal (n)
Spin (m?)
The azimuthal quantum number (l) defines an orbital's shape (s, p, d, f, etc.). The principal quantum number determines energy level, m? gives orbital orientation, and m? describes electron spin. Orbital shapes arise from solutions to the Schrödinger equation.
If an atom has 20 neutrons and a mass number of 40, what is its atomic number?
40
60
0
20
Atomic number equals the number of protons, which is mass number minus neutrons: 40 ? 20 = 20. The atomic number defines the element's identity on the periodic table. Neutrons add to mass but do not affect charge.
How many moles of an ideal gas occupy 22.4 L at STP?
0.5 mol
1.0 mol
2.0 mol
4.0 mol
At standard temperature and pressure (0 °C, 1 atm), one mole of an ideal gas occupies 22.4 L by definition. This is a cornerstone of gas stoichiometry and the ideal gas law.
Which element has the electron configuration [Ne]3s²?
Sulfur (S)
Sodium (Na)
Aluminum (Al)
Magnesium (Mg)
The configuration [Ne]3s² indicates two electrons in the 3s orbital following neon, which corresponds to magnesium (atomic number 12). Sodium has one 3s electron, aluminum has 3p, and sulfur involves 3p electrons.
What is the percent composition of hydrogen in H?O?
33.3%
66.7%
11.2%
88.8%
The molar mass of H?O is 18.02 g/mol (2×1.01 + 16.00). Hydrogen contributes 2.02 g, so H% = (2.02/18.02)×100 ? 11.2%. Percent composition helps in determining empirical formulas.
According to the Brønsted - Lowry definition, why is NH? considered a base?
It has a pH below 7
It donates a proton (H?)
It donates an electron pair
It accepts a proton (H?)
A Brønsted - Lowry base is defined as a proton (H?) acceptor. NH? accepts a proton to form NH?? in aqueous solution. Arrhenius and Lewis definitions differ, but the Brønsted - Lowry concept is broader.
What mass of CaCl?·2H?O (molar mass ?147 g/mol) is required to prepare 250 mL of a 0.200 M solution?
3.68 g
7.35 g
14.70 g
29.4 g
Moles needed = 0.250 L × 0.200 M = 0.0500 mol. Mass = moles × molar mass = 0.0500 mol × 147 g/mol = 7.35 g. Stoichiometry calculations are essential for solution preparation.
Using the Bohr model and the Rydberg formula, what is the wavelength of the photon emitted when an electron in hydrogen transitions from n = 3 to n = 2?
656 nm
486 nm
121 nm
434 nm
The wavelength is found using 1/? = R (1/2² ? 1/3²), giving ? ? 6.56×10?? m or 656 nm. This transition is part of the Balmer series in hydrogen's emission spectrum.
Calculate the average atomic mass of an element with two isotopes: 75% has mass 10 amu and 25% has mass 12 amu.
11.5 amu
10.0 amu
11.0 amu
10.5 amu
Average atomic mass = (0.75×10) + (0.25×12) = 7.5 + 3.0 = 10.5 amu. Natural isotopic abundances yield the weighted average seen on periodic tables.
What is the hybridization of the sulfur atom in SF??
sp³d
sp³
sp³d²
sp²d
SF? has five electron domains (four bonding pairs and one lone pair) around sulfur, requiring sp³d hybridization. The molecular shape is seesaw as predicted by VSEPR theory.
Which principle states that no two electrons in an atom can have the same set of four quantum numbers?
Pauli exclusion principle
Aufbau principle
Heisenberg uncertainty principle
Hund's rule
The Pauli exclusion principle holds that each electron in an atom must have a unique set of four quantum numbers. This rule explains the arrangement of electrons in orbitals. Aufbau and Hund's rules govern filling order and spin distribution.
In a mixture of ideal gases, if the partial pressure of gas A is 40 kPa and gas B is 60 kPa, what is the mole fraction of gas A?
0.40
0.67
1.00
0.60
Mole fraction equals partial pressure divided by total pressure. Total pressure = 40 + 60 = 100 kPa, so ?_A = 40/100 = 0.40. Dalton's law relates partial pressures and mole fractions in ideal gases.
What is the wavelength (in nm) of a photon with energy 4.00×10?¹? J?
497 nm
625 nm
400 nm
656 nm
Use E = hc/?, so ? = (6.626×10?³? J·s × 3.00×10? m/s) / 4.00×10?¹? J ? 4.97×10?? m = 497 nm. This is in the visible spectrum (blue-green light). Photon energy - wavelength relationships are central to spectroscopy.
A sample contains two isotopes: 20% at 100 amu and 80% at 102 amu. What is the average atomic mass?
101.6 amu
102.0 amu
100.4 amu
101.2 amu
Weighted average = (0.20×100) + (0.80×102) = 20.0 + 81.6 = 101.6 amu. Real atomic masses reflect natural isotopic abundances on the periodic table. Precise average calculations are crucial in high-accuracy mass spectrometry.
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Study Outcomes

  1. Understand Atomic Structure -

    Describe the roles of protons, neutrons, and electrons and explain how isotopes differ based on mass number.

  2. Analyze Periodic Trends -

    Interpret patterns in atomic radius, ionization energy, and electronegativity across the periodic table.

  3. Apply Dimensional Analysis -

    Use conversion factors to solve unit conversion problems and ensure accurate chemical calculations.

  4. Calculate Molar Relationships -

    Compute molar masses of compounds and convert between mass, moles, and number of particles with precision.

  5. Interpret Significant Figures -

    Determine the correct number of significant digits in measurements and apply rules for rounding during calculations.

  6. Evaluate Chemical Formulas -

    Recognize and write formulas for ionic and molecular compounds, connecting composition with formula representation.

Cheat Sheet

  1. Atomic Structure and Subatomic Particles -

    Every atom is made of protons, neutrons, and electrons - protons and neutrons in the nucleus and electrons in orbitals around it (ACS Fundamentals). Remember that the atomic number equals the number of protons, which defines the element's identity. Think of the Bohr model as a solar system where electrons "orbit" at fixed energy levels (Khan Academy reference).

  2. Isotopes and Average Atomic Mass -

    Isotopes are atoms of the same element with different neutron counts; use the formula average atomic mass = Σ (fractional abundance × isotopic mass) to calculate the weighted mean (IUPAC guidelines). For example, chlorine has two major isotopes, ³❵Cl and ³❷Cl, so you'd compute 0.7578×34.969 + 0.2422×36.966. Mnemonic: "Mass matters, count matters" to recall that both abundance and mass factor into the average.

  3. Periodic Trends and Predicting Properties -

    Understand that atomic radius increases down a group and decreases across a period, while ionization energy and electronegativity follow the opposite trend (University chemistry curricula). A popular mnemonic for electronegativity order is "FONCl BrISCH" (Fluorine, Oxygen, Nitrogen, Chlorine, Bromine, Iodine, Sulfur, Carbon, Hydrogen). Use these trends to predict reactivity, bond polarity, and more in the chemistry chapter 1 test.

  4. Mole Concept, Avogadro's Number & Molar Mass -

    The mole links microscopic particles to macroscopic mass via 6.022×10²³ entities per mole (Avogadro's number, as defined by NIST). Convert between grams and moles with n = mass (g) ÷ molar mass (g/mol); for instance, 18.02 g of H₂O equals 1.00 mol. Practice dimensional analysis to ensure units cancel correctly - this skill is vital for success on the chemistry chapter 1 test.

  5. SI Units, Significant Figures & Scientific Notation -

    Master SI prefixes (kilo-, centi-, milli-) and always express measurements with the correct number of significant figures (nonzero and captive zeros count, leading zeros don't). For example, 0.00450 m has three significant figures, and you'd write 4.50×10❻³ m in scientific notation. Reliable unit conversions and precision are foundational for answering any chemical foundations quiz accurately.

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