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Quizzes > Science > Chemistry

Test Your Knowledge: Solids, Liquids & Gases Quiz

Dive into our Phases of Matter Quiz and master solids, liquids & gases!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration with solid liquid and gas shapes for a states of matter quiz on coral background

Calling all curious minds! Ready to explore solids, liquids & gases? Our free States of Matter Quiz is designed to challenge and educate students, hobbyists and budding chemists alike. Test your smarts with the ultimate 3 phases of matter assessment, dive into our Phases of Matter Quiz and a lively Matter States Quiz that covers everything from freezing points to vaporization. You'll learn how to spot each phase, brush up on key Chemistry States of Matter concepts, and tackle essentials of the Solids Liquids Gases Quiz. Think you have what it takes? Click play now and spark your scientific curiosity!

Which state of matter has a definite shape and a definite volume?
Gas
Plasma
Solid
Liquid
Solids are characterized by closely packed particles that vibrate in place, forming a rigid structure with a definite shape and volume. In contrast, liquids adapt to their container's shape and gases expand to fill all available space. This rigidity stems from strong intermolecular forces that hold the particles fixed. source
Which state of matter takes the shape of its container but has a fixed volume?
Solid
Gas
Plasma
Liquid
Liquids have particles that are close together but can move past one another, allowing the substance to flow and conform to the shape of its container while maintaining a fixed volume. The intermolecular forces in liquids are strong enough to keep the volume constant but weak enough to permit fluidity. source
Which state of matter has neither a definite shape nor a definite volume and fills its container completely?
Liquid
Plasma
Gas
Solid
Gases consist of particles that are far apart and move freely, causing them to expand and fill any container completely. The weak intermolecular forces allow particles to wander independently, eliminating any fixed shape or volume. This behavior distinguishes gases from solids and liquids. source
What is the term for the phase change in which a liquid turns into a gas?
Condensation
Vaporization
Sublimation
Melting
Vaporization is the process by which a liquid becomes a gas and includes both evaporation at the surface and boiling throughout the liquid. Condensation is the reverse process, while sublimation skips the liquid phase altogether. source
Which process describes the direct transition from a solid to a gas without passing through the liquid phase?
Vaporization
Deposition
Sublimation
Melting
Sublimation occurs when a solid changes directly into a gas without becoming a liquid first, as seen with dry ice (solid CO2). Deposition is the reverse process, where a gas turns directly into a solid. source
What is the normal boiling point of water at one atmosphere of pressure?
212°F
37°C
0°C
100°C
At one standard atmosphere of pressure, water boils at 100°C (212°F). This temperature is defined as the normal boiling point and is a key reference in physical chemistry. source
Which type of solid lacks a long-range, repeating atomic structure?
Crystalline
Amorphous
Metallic
Ionic
Amorphous solids, such as glass and many plastics, do not have a long-range, repeating atomic structure, unlike crystalline solids which form a regular lattice. Their disordered arrangement gives them unique mechanical and optical properties. source
What is the name of the substance's phase when it exists above its critical temperature and critical pressure?
Solid
Liquid
Supercritical fluid
Plasma
A supercritical fluid occurs when a substance is above its critical temperature and pressure, where the distinction between liquid and gas phases disappears. These fluids have properties of both liquids and gases, making them useful in extraction and cleaning processes. source
According to the kinetic molecular theory, what happens to the average kinetic energy of gas molecules as the temperature increases?
Stays the same
Increases
Becomes zero
Decreases
The kinetic molecular theory states that the average kinetic energy of gas molecules is directly proportional to the absolute temperature of the gas. As temperature rises, molecules move faster on average. source
In the van der Waals equation for real gases, which parameter accounts for intermolecular attraction?
T
b
R
a
In the van der Waals equation, the 'a' parameter corrects for intermolecular attractions that reduce the pressure exerted by a real gas compared to an ideal gas. The 'b' term accounts for the finite volume of gas molecules. source
At the triple point of a substance, which statement is true?
Only the gas phase exists
No phase changes occur
Only two phases coexist in equilibrium
Three phases coexist in equilibrium
The triple point of a substance is the unique set of conditions (temperature and pressure) at which its solid, liquid, and gas phases coexist in equilibrium. It is a fundamental reference point in thermodynamics. source
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Study Outcomes

  1. Identify Properties of Each State -

    Distinguish solids, liquids, and gases by their characteristic features such as shape, volume, and molecular arrangement.

  2. Differentiate Between Phases -

    Compare and contrast the structural differences and particle motion in each phase of matter.

  3. Explain Phase Transitions -

    Describe how matter changes between solid, liquid, and gas through processes like melting, freezing, and vaporization.

  4. Predict State Changes -

    Use temperature and pressure variables to anticipate how and when matter will transition between phases.

  5. Apply Concepts to Real-World Examples -

    Relate phase behavior to everyday phenomena such as cooking, weather patterns, and industrial processes.

  6. Evaluate Common Misconceptions -

    Correctly identify and address typical misunderstandings about the states and transformations of matter.

Cheat Sheet

  1. The Three States of Matter -

    In solids, particles vibrate about fixed positions, giving a rigid shape and volume; liquids maintain volume but adapt to container shapes due to freer particle movement; gases have both variable shape and volume as particles move independently at high speeds (NIST). A simple mnemonic is "SLG" (Solid, Liquid, Gas) to recall the order of increasing particle motion.

  2. Intermolecular Forces and State Stability -

    Ionic bonds, hydrogen bonding and van der Waals forces dictate how particles stick together, with stronger attractions raising melting and boiling points (Chemguide, University of Oxford). Remember "DIP" for Dispersion, Induction, and Polarization to cover London forces, dipole - induced dipole, and dipole - dipole interactions when comparing liquids like hexane versus water.

  3. Kinetic Molecular Theory & Gas Laws -

    The Kinetic Molecular Theory explains that a gas's average kinetic energy (KEavg) is directly proportional to temperature via KEavg = 3/2 kBT (University of Colorado). Use PV = nRT to relate pressure, volume, temperature, and moles - just think "Please Verify New Realms" to keep P, V, n, R, T in mind.

  4. Phase Transitions and Enthalpy -

    Endothermic processes like melting (ΔHfus) and vaporization (ΔHvap) absorb energy, while freezing and condensation release it; a standard heating curve shows flat regions where these changes occur (Khan Academy). For water, ΔHfus≈6 kJ/mol and ΔHvap≈40 kJ/mol at 1 atm - just remember "6 to 40" when you study these values.

  5. Triple Point and Critical Point -

    The triple point is where solid, liquid, and gas coexist in equilibrium (e.g., water at 0.01 °C and 611.7 Pa per IUPAC definitions); the critical point marks the end of the liquid - gas distinction (374 °C, 22.06 MPa for water). Picture the phase diagram's "vee" shape to lock in these landmark conditions.

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