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Quizzes > Science

Matter Quiz: What Is Matter in Chemistry?

Quick, free chemistry quiz on what is matter. Instant results.

Editorial: Review CompletedCreated By: Marketing DepartmentUpdated Aug 25, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art style chemistry quiz design with cutout molecules test tubes question blank on sky blue background

This matter quiz helps you check what is matter (any substance that occupies space and has mass) with quick, clear questions. Build confidence for class or exams, then go deeper with a classification of matter quiz, practice measurement in the mass volume and density quiz, or review phases in the states of matter quiz.

What is defined as any substance that occupies space and has mass?
Force
Field
Matter
Energy
Matter is anything that occupies space and has mass, distinguishing it from energy. This definition underpins all classical chemistry by defining what physical substances are composed of. Matter exists in different states like solids, liquids, and gases.
Which state of matter has a definite shape and volume?
Gas
Liquid
Solid
Plasma
A solid has particles packed closely in a fixed arrangement, giving it both a definite shape and volume. Unlike liquids and gases, solids resist deformation under small stresses. This rigidity arises from strong intermolecular forces.
In which state of matter do particles have a fixed volume but take the shape of their container?
Solid
Liquid
Plasma
Gas
Liquids have a definite volume because their particles are close together but can move past one another, allowing them to conform to the shape of their container. They are less compressible than gases. Intermolecular attractions are intermediate in strength between solids and gases.
Which state of matter has neither definite shape nor definite volume?
Gas
Liquid
Plasma
Solid
Gases have widely spaced particles that move independently, so they expand to fill any container. They have no fixed shape or volume. Their volume and pressure are highly sensitive to changes in temperature and pressure.
What is the SI base unit for mass?
Meter
Kilogram
Liter
Gram
The kilogram (kg) is the SI base unit for mass and is defined by a platinum - iridium alloy prototype. Other units like the gram are derived from the kilogram. Accurate mass measurement is crucial in quantitative chemistry.
What is the SI unit for volume?
Cubic meter
Newton
Gram
Liter
The cubic meter (m³) is the SI derived unit for volume. Liters (L) are commonly used in chemistry but are not the SI base unit. Volume measurement is key for reactions in solution.
Which of the following is a physical property of matter?
Reactivity
Density
Flammability
Oxidation
Physical properties can be observed without changing the substance's chemical identity. Density is the mass per unit volume and is intrinsic to the material. Reactivity and flammability involve chemical changes.
Which of the following is a chemical property of matter?
Color
Density
Reactivity
Odor
Chemical properties describe how a substance interacts with other substances to form new products. Reactivity indicates the tendency to undergo chemical reactions. Density, color, and odor are physical.
What is the ratio of mass to volume known as?
Specific heat
Molar mass
Viscosity
Density
Density (?) equals mass divided by volume and is an intensive property. It helps identify substances and affects buoyancy. Molar mass relates mass per mole, not per volume.
Matter that consists of two or more elements chemically combined in a fixed ratio is called?
Element
Compound
Mixture
Solution
A compound is a substance formed when two or more elements chemically bond in a fixed proportion. Elements are pure, single types of atom. Mixtures and solutions contain variable ratios.
A mixture that has uniform composition throughout is called?
Colloid
Heterogeneous mixture
Suspension
Homogeneous mixture
A homogeneous mixture has the same composition and properties throughout. Solutions are a type of homogeneous mixture. Heterogeneous mixtures have distinct regions.
Atoms of the same element with different numbers of neutrons are called?
Isotopes
Molecules
Ions
Allotropes
Isotopes are variants of the same element that differ in neutron count, giving different mass numbers. Ions differ by electron count. Allotropes are different structural forms.
How many particles are in one mole of a substance?
6.022×10^22
1.602×10^?19
9.81
6.022×10^23
Avogadro's number, 6.022×10^23, defines the number of entities in one mole. It allows conversion between moles and particle counts. This constant is fundamental in stoichiometry.
The basic unit of an element that can exist either alone or in combination is?
Molecule
Atom
Ion
Cell
An atom is the smallest unit of an element retaining its chemical properties. Atoms can bond to form molecules and compounds. Understanding atoms is key to chemical reactions.
Which is NOT a state of matter?
Liquid
Solution
Solid
Gas
Solutions are homogeneous mixtures, not fundamental states of matter. Solids, liquids, gases, and plasmas are the primary states. Recognizing this helps classify materials.
What is the smallest particle of a compound that retains all of the properties of that compound?
Molecule
Ion
Atom
Electron
A molecule is two or more atoms bonded together representing the smallest unit of a compound with its properties. Atoms alone may belong to an element. Recognizing molecules is vital in chemical formulas.
Which law states that mass is neither created nor destroyed in a chemical reaction?
Law of reciprocal proportions
Law of definite proportions
Law of conservation of mass
Law of multiple proportions
The law of conservation of mass asserts that the total mass of reactants equals the total mass of products in a chemical reaction. This principle is foundational in stoichiometry. It was established by Lavoisier in the 18th century.
What is the value of Avogadro's number?
9.109×10^?31
3.142×10^23
6.022×10^23
1.602×10^?19
Avogadro's number, 6.022×10^23, is the number of constituent particles in one mole of a substance. It allows chemists to relate macroscopic amounts to particle numbers. This constant is central to mole-based calculations.
According to the ideal gas law, PV = nRT, what does R represent?
Pressure
Temperature
Moles
Ideal gas constant
R is the ideal gas constant, relating pressure, volume, temperature, and moles in the ideal gas law. Its value depends on the units used (e.g., 0.08206 L·atm·K?¹·mol?¹). It is key for gas calculations.
What volume will 1 mole of an ideal gas occupy at STP (0°C and 1 atm)?
20.0 L
1.00 L
24.5 L
22.4 L
At STP (0°C, 1 atm), one mole of an ideal gas occupies 22.4 liters. This standard molar volume is used for comparing gas behaviors. Real gases may deviate slightly.
What is the formula to calculate density?
mass/volume
mass+volume
mass?volume
mass×volume
Density is defined as mass divided by volume (? = m/V). It describes how much matter is packed into a given space. It is an intensive property.
What is the empirical formula of a compound containing 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass?
CHO
C2H6O
C2H4O2
CH2O
Converting percentages to moles yields a simplest whole-number ratio of C:H:O = 1:2:1, giving CH2O. Empirical formulas reflect this ratio, not actual molecule size.
Which intermolecular force is the strongest?
Hydrogen bonding
London dispersion
Ionic bonding
Dipole-dipole
Hydrogen bonds, a strong type of dipole interaction, occur when H is bonded to N, O, or F. They are stronger than dipole-dipole and dispersion forces. Ionic bonds are not classified as intermolecular.
During which phase change is energy absorbed?
Condensation
Deposition
Melting
Freezing
Melting is an endothermic process where solids absorb energy to become liquids. Freezing and condensation release energy. Recognizing energy flow is essential in thermodynamics.
What is the pH of a neutral solution at 25°C?
1
0
7
14
At 25°C, pure water has [H?] = 1×10?? M, giving pH = -log(1×10??) = 7. Deviations occur with temperature changes. This is the neutral point on the pH scale.
A solution with pH less than 7 is considered?
Basic
Alkaline
Neutral
Acidic
Acidic solutions have higher [H?] than [OH?], giving pH < 7. Basic (alkaline) solutions have pH > 7. Understanding pH is key in many chemical processes.
An acid-base reaction where an acid reacts with a base to produce salt and water is called?
Neutralization
Polymerization
Hydrolysis
Oxidation
Neutralization reactions combine H? from the acid with OH? from the base to form water and a salt. They are exothermic and common in titrations.
In redox reactions, oxidation involves the ______ of electrons.
creation
gain
loss
sharing
Oxidation is defined as the loss of electrons by a species. Reduction is the gain of electrons. Remember the mnemonic OIL RIG (Oxidation Is Loss).
What does the atomic number of an element represent?
Atomic mass
Number of neutrons
Number of protons
Mass number
The atomic number (Z) equals the number of protons in an atom's nucleus. It defines the element's identity. Neutron count affects isotopes but not atomic number.
What is a cation?
Negatively charged ion
Neutral atom
Radical
Positively charged ion
A cation is formed when an atom or molecule loses electrons, resulting in a positive charge. Anions are negatively charged. Ion formation is fundamental to many chemical processes.
What is the mole fraction of a solute?
Mass of solute/total mass
Moles of solute divided by total moles
Molarity of solute
Volume of solute/total volume
Mole fraction (?) is the ratio of moles of one component to the total moles in the mixture. It is dimensionless and used in colligative properties.
The reaction rate is doubled if the concentration of a reactant is doubled suggests the reaction is?
Second order
Zero order
First order
Third order
In a first-order reaction, rate ? [A]^1, so doubling [A] doubles the rate. Zero-order rates are independent of concentration. Higher orders scale differently.
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of its ____?
Pressure
Temperature
Molar mass
Volume
Graham's law states that effusion rate ? 1/?M, where M is molar mass. Lighter gases effuse faster than heavier ones. This principle is applied in isotope separation.
Which term in the van der Waals equation accounts for intermolecular attractions?
b
R
a
V
In (P + a(n/V)²)(V - nb) = nRT, the term a(n/V)² corrects pressure for intermolecular attractions. Parameter b corrects volume for finite molecular size.
The boiling point elevation is classified as which type of property?
Colligative property
Physical property
Extensive property
Intensive property
Colligative properties depend on solute particle count, not identity. Boiling point elevation increases with solute concentration. It contrasts extensive properties that depend on amount.
If doubling the concentration of A doubles the reaction rate and doubling B has no effect, the rate law is?
rate = k[A]^1[B]^0
rate = k[A]^0[B]^1
rate = k[A]^1[B]^1
rate = k[A]^2[B]^0
A reaction first order in A doubles rate when [A] doubles; order zero in B means rate is independent of [B]. Rate laws define dependency on reactant concentrations.
Which parameter can be determined from the slope of an Arrhenius plot (ln k vs 1/T)?
Activation energy
Rate constant
Reaction order
Pre-exponential factor
The Arrhenius equation ln k = -Ea/(R)(1/T) + ln A shows a plot slope of -Ea/R. From the slope you can calculate activation energy. A is the pre-exponential factor.
When ice melts at 0°C under standard pressure, the entropy change ?S is ____?
positive
negative
zero
 
Melting increases disorder as a solid becomes liquid, so ?S > 0. Entropy measures system randomness. Phase changes often accompany significant entropy changes.
Which equation relates Gibbs free energy, enthalpy, and entropy?
?G = ?H + T?S
?G = ?H - T?S
?G = T?S - ?H
?G = ?S - T?H
The Gibbs free energy equation ?G = ?H - T?S defines spontaneity: negative ?G indicates a spontaneous process. It combines enthalpy and entropy terms.
In a galvanic cell, the overall cell potential is calculated by?
E°cell = E°cathode + E°anode
E°cell = E°anode - E°cathode
E°cell = E°anode + E°cathode
E°cell = E°cathode - E°anode
Standard cell potential equals the reduction potential at the cathode minus that at the anode. This determines the voltage a cell can produce. Proper sign usage is essential in electrochemistry.
Which equation modifies the Nernst equation at 25°C for a one-electron transfer?
E = E° + (0.0257/n) log Q
E = E° - (0.0591/n) log Q
E = E° - (0.0257/n) log Q
E = E° + (0.0591/n) log Q
At 25°C, the Nernst equation becomes E = E° - (0.0591/n) log Q. Here n is number of electrons transferred. It adjusts cell potential under nonstandard conditions.
The pH of a buffer solution can be calculated using which equation?
Beer's law
Van't Hoff
Arrhenius
Henderson-Hasselbalch
The Henderson-Hasselbalch equation, pH = pKa + log([A?]/[HA]), estimates buffer pH based on acid/base ratios. It's widely used in biochemistry.
At the equivalence point of a titration of a weak acid with a strong base, the pH is?
Equal to 7
Less than 7
Unpredictable
Greater than 7
Titrating a weak acid with a strong base yields a conjugate base on neutralization, producing a basic solution at equivalence (pH > 7). The salt hydrolyzes water.
UV-Vis spectroscopy measures transitions between which molecular levels?
Electronic energy levels
Vibrational energy levels
Rotational energy levels
Nuclear energy levels
UV-Vis spectroscopy involves electronic transitions when molecules absorb ultraviolet or visible light. Vibrational and rotational transitions occur at IR and microwave regions, respectively.
In the resonance hybrid of ozone (O3), how many equivalent Lewis structures are there?
1
3
4
2
Ozone has two equivalent resonance structures, each with one double bond and one single bond. The actual molecule is a hybrid of these. Resonance explains delocalized bonding.
What is the hybridization of the central atom in sulfur hexafluoride (SF6)?
sp3d2
sp2
sp3d
sp3
SF6 has an octahedral geometry, requiring six hybrid orbitals on sulfur. The sp3d2 hybridization accounts for six electron domains.
What is the molecular geometry of PCl5?
Trigonal planar
Trigonal bipyramidal
Tetrahedral
Square planar
PCl5 has five bonding pairs and no lone pairs, giving a trigonal bipyramidal shape. Three atoms form an equatorial plane, two are axial. VSEPR theory predicts this arrangement.
Which set of quantum numbers is not allowed for an electron in an atom?
n=2, l=1, m=1, s=-1/2
n=1, l=0, m=0, s=+1/2
n=0, l=0, m=0, s=+1/2
n=3, l=2, m=-2, s=+1/2
The principal quantum number n must be a positive integer (1,2,3,…), so n=0 is not allowed. Other sets follow quantum rules. Quantum numbers define electron orbitals.
According to molecular orbital theory, what is the bond order of O2?
1.5
1
2
0
O2 has 10 electrons in bonding MOs and 6 in antibonding MOs, giving bond order = (10-6)/2 = 2. Bond order predicts bond strength and length.
Which equation describes the relationship between vapor pressure and temperature for phase transitions?
Arrhenius equation
Clausius-Clapeyron equation
Nernst equation
Van't Hoff equation
The Clausius-Clapeyron equation ln(P2/P1) = -?Hvap/R (1/T2 - 1/T1) relates vapor pressure and temperature. It is key for phase equilibrium.
The Boltzmann distribution law gives the fraction of molecules in a state i as e^(?Ei/kT) divided by?
Average energy
Partition function
Activation energy
Degeneracy
The Boltzmann factor e^(?Ei/kT) normalized by the partition function Q gives population distribution across energy levels. This is fundamental in statistical thermodynamics.
Which IR absorption band around 1700 cm?¹ typically indicates?
N - H bending
Hydroxyl group
Carbonyl group
C - H stretching
A sharp, strong IR absorption near 1700 cm?¹ is characteristic of the C=O stretching vibration in carbonyl compounds. IR spectroscopy identifies functional groups by band positions.
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Study Outcomes

  1. Define Matter -

    Articulate that any substance that occupies space and has weight is known as matter, establishing a clear foundation for understanding chemistry concepts.

  2. Identify Key Properties -

    Recognize and describe the fundamental physical and chemical properties of matter as outlined in Milady Ch 12.

  3. Differentiate States of Matter -

    Distinguish between the solid, liquid, gas, and plasma states, explaining how each state relates to chapter 12 basics of chemistry.

  4. Recall Workbook Answers -

    Retrieve accurate chapter 12 Milady workbook answers to reinforce your grasp of core cosmetology chemistry topics.

  5. Apply Knowledge -

    Utilize your understanding of matter to correctly answer quiz questions and solidify key concepts.

  6. Analyze Performance -

    Evaluate your quiz results to pinpoint strengths and areas needing review, guiding further study of Milady Ch 12.

Cheat Sheet

  1. Definition of Matter -

    Any substance that occupies space and has weight is ______ - matter. According to IUPAC and ACS guidelines, matter includes solids, liquids, gases, and plasma, forming the basis for all cosmetic ingredients (see milady ch 12 overviews). Use the mnemonic "M-A-T-T-E-R" (Mass And Takes Up Room) to lock in this fundamental definition.

  2. States of Matter -

    Reputable sources like Khan Academy and university chemistry departments classify matter into solids, liquids, gases, and plasma, each with unique particle arrangements and energy levels. For example, water's transition from ice (solid) to steam (gas) illustrates energy-driven changes in molecular motion. Visualize particles as dancers: tightly packed for solids, loosely flowing for liquids, and wildly free for gases to cement these concepts.

  3. Physical vs. Chemical Properties -

    Physical properties (e.g., melting point, density, solubility) can be observed without altering composition, while chemical properties (e.g., reactivity, flammability) describe how substances transform in reactions. A simple mnemonic to remember chemical changes is "CLAP": Color change, Light emission, Action (gas release), Precipitate formation. Review tables of physical and chemical traits in your chapter 12 milady workbook answers for quick reference.

  4. Atomic Structure Essentials -

    Atoms consist of a nucleus (protons and neutrons) surrounded by electrons in shells - key for understanding bonding in cosmetic formulations. The mass number equals protons plus neutrons; atomic number equals protons, defining each element's identity (source: NIST). Practice writing the symbol for carbon-14 (¹❴₆C) to reinforce isotope notation and atomic structure.

  5. Cosmetic Chemistry Applications -

    Mastering matter principles helps you formulate and evaluate salon products: the pH scale, surfactant behavior, and emulsions all hinge on molecular interactions. Chapter 12 basics of chemistry cosmetology answers explore how acid - base balance affects hair cuticle health and product performance. Keep a log of formulation trials and observations to build confidence and speed in real-world salon scenarios.

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