Properties of Matter and Their Measurement: Types and Material

Edited By Shivani Poonia | Updated on Aug 16, 2025 02:33 PM IST

The study of properties of matter and their measurement is an important aspect of the science that relates to the field of chemistry as well as physics. The properties of matter include mass, volume, temperature, and density. All these help us to understand the physical behavior of the substance. The matter was first ever explored by Aristotle who proposed the existence of the fundamental elements of life earth, water, air, and fire.

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Properties of Matter and Their Measurement
Some Solved Examples
Practice more Questions from the link given below:
Conclusion

Properties of Matter and Their Measurement

Antoine Lavoisier, the father of modern chemistry made his important contribution to the law of conservation of masses and developed the systematic method for the naming of chemical substances. Afterward, lots of scientist discovered the different measuring techniques of physical substances over some time. The measurement is very important as it gives the quantitative idea of how to elucidate the data or helps in predicting the nature of matters. By doing all these studies scientists make precise measurements, which are better to understand such physical properties. These discoveries continued to the 19th and 20th centuries for understanding measurement on a more advanced level.

Properties of Matter and Their Measurement

Physical and chemical properties :

Every substance has unique or characteristic properties. These properties can be classified into two categories – physical properties and chemical properties.

Physical properties are those properties that can be measured or observed without changing the identity or the composition of the substance.

Some examples of physical properties are color, odor, melting point, boiling point, density, etc.

The measurement or observation of chemical properties requires a chemical change to occur. Examples of chemical properties are characteristic reactions of different substances; these include acidity or basicity, combustibility, etc.

Measurement of physical properties :

Many properties of matter such as length, area, volume, etc. are quantitative in nature. Any quantitative observation or measurement is represented by a number followed by units in which it is measured. For example, the length of a room can be represented as 5 m; here 5 is the number and m denotes meter – the unit in which the length is measured.

The International System of Units (SI) :

The SI system has seven base units and they are listed in Table 1.1. These units pertain to the seven fundamental scientific quantities. The other physical quantities such as speed, volume, density, etc. can be derived from these quantities.

Base physical Quantities and their Units

Definition of SI Base Units

Prefixes used in SI system

Mass and Weight :

The mass of a substance is the amount of matter present in it while weight is the force exerted by gravity on an object. The mass of a substance is constant whereas its weight may vary from one place to another due to change in gravity.

Volume:

Volume has the units of (length)³. So, in the SI system, the volume has units of m³. But again, in chemistry laboratories, smaller volumes are used. Hence, the volume is often denoted in cm³ or dm³ units.

A common unit, litre (L) which is not an SI unit, is used for measurement of the volume of liquids.

1 L = 1000 mL , 1000 cm³ = 1 dm³ . In the laboratory, the volume of liquids or solutions can be measured by a graduated cylinder, burette, pipette, etc. A volumetric flask is used to prepare a known volume of a solution.

Density :

The density of a substance is its amount of mass per unit volume. So SI units of density can be obtained as follows:

S.I unit of density $= \frac{S.I unit of mass}{S.I unit of volume} = \frac{kg}{m^{3}}$

This unit is quite large and chemists often express density in g cm^-3. where mass is expressed in grams and volume is expressed in cm^-3.

Temperature :

There are three common scales to measure temperature ^oC (degree Celsius), ^oF (degree Fahrenheit), and K (Kelvin). Here, K is the SI unit. The thermometers are based on these scales. Generally, the thermometer with the Celsius scale is calibrated from 0^o to 100^o where these two temperatures are the freezing point and the boiling point of water respectively. The Fahrenheit scale is represented between 32^oto 212^o.

The temperatures on the Fahrenheit and degree Celcius scales are related to each other by the following relationship:

^oF = (9/5)(^oC) + 32

The Kelvin scale is related to the Celsius scale as follows :

K =^oC + 273.15

It is interesting to note that the temperature below 0 °C (i.e. negative values) are possible in the Celsius and Fahrenheit scales but on the Kelvin scale, a negative temperature is not possible.

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Some Solved Examples

Example 1:

S.I unit of luminous intensity is:

1) Mole

2) Ampere

3) Candela

4) Metre

Solution:

Candela is the S.I. unit of luminous intensity.

Hence, the answer is the option (3).

Example 2:

Chromium is added to steel to impart strength and shine. If the density of chromium is 5.24g/cm³ then the expression in S.I. unit (kg/m³) is:

1) 5240

2) 5.24

3) 0.524

4) 52400

Solution:

1kg = 1000g and 1m³ = 10⁶cm³5.24 g/cm³ = (5.24 x 10^-3 Kg)/10^-6m³ = 5240 Kg/m³.

Hence, the answer is the option (1).

Example 3:

The density of a certain metal is $10.5 g / {cm}^{3}$ . If a cube of this metal weighs 630g, what is the length of one side of the cube?

1) 3 cm

2) 4 cm

3) 5 cm

4) 6 cm

Solution:

The volume of the cube is equal to the length of one side cubed. Therefore, the volume of the cube is $(4 cm)^{3} = 64 {cm}^{3}$ . Since the density of the metal is $10.5 g / {cm}^{3}$ , the mass of the cube can be calculated as $10.5 g / {cm}^{3} \times 64 {cm}^{3} = 672 g$ . But we know that the actual weight of the cube is 630 g. So, we can calculate the actual volume of the cube. Thus, the length of one side of the cube is $\sqrt[3]{60 {cm}^{3}} \approx 4 cm$

Hence, the answer is the option (2).

Example 4:

Assertion: Water boils at a higher temperature at higher altitudes.

Reasoning: Atmospheric pressure decreases with an increase in altitude.

1) Both assertion and reasoning are true, and reasoning is the correct explanation of the assertion.

2) Both assertion and reasoning are true, but reasoning is not the correct explanation of the assertion.

3) Assertion is true, but reasoning is false.

4) Assertion is false, but reasoning is true.

Solution:

At higher altitudes, the atmospheric pressure decreases. As a result, the boiling point of water decreases because the pressure on the liquid decreases, and it requires less energy to change into vapor. This is the reason why water boils at a higher temperature at higher altitudes, both the assertion and reasoning are true, and reasoning is the correct explanation of the assertion.

Hence, the answer is the option (1).

Example 5:

Which of the following gases have the highest average velocity at the same temperature?

1) Hydrogen (H₂)

2) Oxygen (O₂)

3) Nitrogen (N₂)

4) Argon (Ar)

Solution:

According to Graham's law of diffusion, the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. This means that at the same temperature, lighter gases will have higher average velocities compared to heavier gases. The molar mass of hydrogen (H₂) is the lowest among the given options, so it will have the highest average velocity at the same temperature.

Hence, the answer is the option (1).

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PROPERTIES OF MATTER AND THEIR MEASUREMENT

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Conclusion

In conclusion, comprehending the properties of matter and learning their measurement is fundamental to scientific progress. From ancient theories to modern techniques, the path shows how curiosity and precision shape our knowledge of the physical world. Accurate measurements of mass, volume, temperature, and density not only help elucidate data but also explains the behavior of substances in varied conditions. As science continues to progress, these theories remains the spine of discovery, innovation, and practical application across fields.

Frequently Asked Questions (FAQs)

1. What is matter and how is it defined in chemistry?

Matter is anything that has mass and occupies space. In chemistry, matter is defined as any physical substance that can be observed and measured. It includes all solids, liquids, and gases that make up the universe.

2. How do we classify matter based on its physical state?

Matter is classified into three main physical states: solid, liquid, and gas. Solids have a fixed shape and volume, liquids have a fixed volume but take the shape of their container, and gases have no fixed shape or volume and expand to fill their container.

3. What is the difference between intensive and extensive properties of matter?

Intensive properties are independent of the amount of matter present, such as density, melting point, and boiling point. Extensive properties depend on the amount of matter, such as mass, volume, and heat capacity.

4. How does the concept of density relate to the properties of matter?

Density is an intensive property that relates mass to volume. It's calculated by dividing an object's mass by its volume (density = mass/volume). Density explains why some objects float or sink in fluids and helps identify unknown substances.

5. What are physical properties, and how do they differ from chemical properties?

Physical properties are characteristics that can be observed without changing the substance's chemical composition, such as color, shape, and melting point. Chemical properties describe how a substance reacts with other substances, like flammability or reactivity with acids.

6. What is the importance of stoichiometry in chemical reactions?

Stoichiometry describes the quantitative relationships between reactants and products in chemical reactions. It's crucial for predicting reaction yields, determining limiting reagents, and balancing chemical equations.

7. What is the importance of isotopes in understanding atomic structure and properties?

Isotopes are atoms of the same element with different numbers of neutrons. They help us understand atomic structure, nuclear stability, and have applications in radioactive dating and nuclear medicine.

8. What is the significance of Le Chatelier's principle in understanding chemical equilibrium?

Le Chatelier's principle states that when a system at equilibrium is disturbed, it will shift to counteract the change. This helps predict how changes in concentration, pressure, or temperature will affect chemical equilibria.

9. What is the relationship between bond energy and chemical reactivity?

Bond energy is the energy required to break a chemical bond. Stronger bonds are generally more stable and less reactive. Understanding bond energies helps predict the likelihood and energy changes of chemical reactions.

10. What is the importance of oxidation states in understanding chemical reactions?

Oxidation states indicate the degree of oxidation of an atom in a compound. They help balance redox reactions, predict reactivity, and understand the behavior of elements in different compounds.

11. How does the concept of resonance affect molecular structure and properties?

Resonance occurs when a molecule's structure can't be represented by a single Lewis structure. It affects bond lengths, strengths, and molecular stability, influencing properties like reactivity and spectroscopic behavior.

12. What is the significance of activation energy in chemical reactions?

Activation energy is the minimum energy required for a chemical reaction to occur. It affects reaction rates and helps explain why some reactions occur spontaneously while others require energy input.

13. How do we use the concept of half-life in understanding radioactive decay?

Half-life is the time it takes for half of a radioactive sample to decay. It's constant for each isotope and used to date materials, predict decay rates, and understand the behavior of radioactive substances.

14. What is the importance of buffer solutions in maintaining pH?

Buffer solutions resist changes in pH when small amounts of acid or base are added. They're crucial in biological systems, industrial processes, and laboratory work for maintaining stable pH conditions.

15. How does the concept of hybridization explain molecular geometry?

Hybridization is the mixing of atomic orbitals to form new hybrid orbitals. It explains the geometry of molecules, bond angles, and certain physical and chemical properties of compounds.

16. What is the significance of the aufbau principle in electron configuration?

The aufbau principle describes how electrons fill orbitals in atoms, starting with the lowest energy levels. It's crucial for understanding electron configurations, periodic trends, and chemical bonding.

17. How do we use the concept of limiting reagents in chemical reactions?

The limiting reagent is the reactant that's completely consumed in a reaction and determines the amount of product formed. Understanding limiting reagents is crucial for predicting reaction yields and optimizing industrial processes.

18. What is the importance of the Heisenberg uncertainty principle in quantum mechanics?

The Heisenberg uncertainty principle states that we cannot simultaneously know both the exact position and momentum of a particle. It's fundamental to understanding the quantum nature of matter and energy.

19. How does the concept of chirality affect the properties of molecules?

Chiral molecules are non-superimposable mirror images of each other. Chirality can significantly affect a molecule's biological activity, optical properties, and reactivity, especially important in pharmaceutical chemistry.

20. What is the significance of the Pauli exclusion principle in atomic structure?

The Pauli exclusion principle states that no two electrons in an atom can have the same set of quantum numbers. It's crucial for understanding electron configurations, chemical bonding, and the structure of matter.

21. How do we use the concept of standard reduction potentials in electrochemistry?

Standard reduction potentials measure the tendency of chemical species to be reduced. They help predict the direction of redox reactions, calculate cell potentials, and understand the reactivity of different elements and compounds.

22. What is the importance of the Hund's rule in electron configuration?

Hund's rule states that electrons in orbitals of the same energy will occupy separate orbitals before pairing up. It's important for understanding electron configurations, magnetic properties, and chemical bonding.

23. How does the concept of conjugation affect the properties of organic compounds?

Conjugation involves the alternation of single and multiple bonds in a molecule. It affects properties like color, reactivity, and stability, and is crucial in understanding the behavior of many organic compounds, including dyes and biological molecules.

24. How do we measure the volume of irregularly shaped solids?

The volume of irregularly shaped solids can be measured using the displacement method. The solid is submerged in a known volume of liquid in a graduated cylinder, and the increase in liquid volume equals the solid's volume.

25. What is the significance of the melting point in identifying substances?

The melting point is the temperature at which a solid changes to a liquid. It's an intensive property unique to each pure substance, making it useful for identifying unknown materials and assessing their purity.

26. How does pressure affect the properties of gases?

Pressure significantly affects gas properties. As pressure increases, gas volume decreases (if temperature is constant), and vice versa. This relationship is described by Boyle's Law and is crucial in understanding gas behavior.

27. What is the difference between homogeneous and heterogeneous mixtures?

Homogeneous mixtures have uniform composition throughout, like salt dissolved in water. Heterogeneous mixtures have visibly different components, like oil and water or a fruit salad.

28. How does temperature affect the solubility of substances?

Generally, the solubility of solids in liquids increases with temperature, while gas solubility in liquids decreases. This is why warm soda loses carbonation faster than cold soda.

29. What is the importance of significant figures in measurements?

Significant figures indicate the precision of a measurement. They include all certain digits plus one uncertain digit, ensuring that calculations and reported results reflect the actual precision of the measurements taken.

30. How do we convert between different units of measurement in chemistry?

Unit conversion involves using conversion factors and dimensional analysis. Multiply the original quantity by a conversion factor (a ratio of equivalent units) that cancels out the original unit and leaves the desired unit.

31. What is the difference between accuracy and precision in measurements?

Accuracy refers to how close a measurement is to the true value, while precision refers to how close repeated measurements are to each other. A measurement can be precise (consistent) without being accurate (close to the true value).

32. How does surface tension affect the properties of liquids?

Surface tension is the tendency of liquid surfaces to shrink into the minimum surface area possible. It causes water droplets to form, allows some insects to walk on water, and influences capillary action in plants.

33. What is the relationship between temperature and kinetic energy of particles?

Temperature is a measure of the average kinetic energy of particles in a substance. As temperature increases, particles move faster, increasing their kinetic energy. This relationship is fundamental to understanding heat and thermal energy.

34. How do intermolecular forces affect the properties of matter?

Intermolecular forces (like hydrogen bonding and van der Waals forces) influence properties such as boiling point, melting point, and solubility. Stronger intermolecular forces generally result in higher boiling and melting points.

35. What is the difference between heat and temperature?

Heat is the transfer of thermal energy between objects due to temperature differences. Temperature is a measure of the average kinetic energy of particles in a substance. Heat flows from higher to lower temperature objects.

36. How does the concept of specific heat capacity relate to the properties of matter?

Specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. It's unique to each substance and affects how quickly materials heat up or cool down.

37. What is the importance of the periodic table in understanding material properties?

The periodic table organizes elements based on their atomic structure and properties. It helps predict chemical behavior, reactivity, and physical properties of elements and their compounds based on their position in the table.

38. How do allotropes demonstrate the relationship between structure and properties?

Allotropes are different structural forms of the same element, like diamond and graphite for carbon. They demonstrate how atomic arrangement can dramatically affect properties, even when the chemical composition is identical.

39. What is the role of electron configuration in determining material properties?

Electron configuration determines an element's chemical behavior and many of its physical properties. It influences bonding capabilities, reactivity, and properties like conductivity and magnetism.

40. How does crystalline structure affect the properties of solids?

Crystalline structure determines many physical properties of solids, including hardness, melting point, and optical properties. Different crystal structures of the same substance (polymorphs) can have vastly different properties.

41. What is the significance of phase diagrams in understanding material behavior?

Phase diagrams show how temperature, pressure, and composition affect the physical state of a substance. They help predict phase transitions and are crucial in materials science and engineering.

42. How do we determine the empirical and molecular formulas of compounds?

The empirical formula shows the simplest whole-number ratio of atoms in a compound, determined from its composition by mass. The molecular formula shows the actual number of atoms in a molecule, often a multiple of the empirical formula.

43. How does polarity affect the properties of molecules?

Polarity, caused by uneven electron distribution, affects properties like solubility, boiling point, and intermolecular forces. Polar molecules tend to dissolve in polar solvents and have higher boiling points than similar non-polar molecules.

44. What is the relationship between bond type and material properties?

The type of chemical bonding (ionic, covalent, metallic) greatly influences material properties. Ionic compounds are often brittle and have high melting points, covalent compounds vary widely, and metals are typically malleable and conductive.

45. How do we use spectroscopy to analyze material properties?

Spectroscopy uses the interaction between matter and electromagnetic radiation to analyze material composition and structure. Different spectroscopic techniques (like IR, NMR, mass spectroscopy) provide information about molecular structure and composition.

46. What is the significance of the mole concept in chemistry?

The mole is a unit representing 6.022 × 10^23 particles (Avogadro's number). It allows chemists to relate microscopic particles to macroscopic quantities, crucial for stoichiometric calculations and understanding chemical reactions.

47. How does the concept of electronegativity relate to chemical bonding and material properties?

Electronegativity is an atom's ability to attract electrons in a chemical bond. It influences bond polarity, which affects molecular properties like solubility, boiling point, and reactivity.

48. How do we use the ideal gas law to predict gas behavior?

The ideal gas law (PV = nRT) relates pressure, volume, amount of gas, and temperature. It's used to predict how gases will behave under different conditions, though it assumes ideal behavior and has limitations for real gases.

49. How does the concept of entropy relate to the properties of matter?

Entropy is a measure of the disorder or randomness in a system. It helps explain why certain processes occur spontaneously and affects properties like phase transitions and chemical reactivity.

50. How do we use colligative properties to understand solution behavior?

Colligative properties depend on the number of dissolved particles, not their nature. They include boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure, and help us understand solution behavior.