Nature and Characteristics of Matter - Overview, Structure, Properties & Uses

Nature and Characteristics of Matter: What is, Examples, Particles

Edited By Shivani Poonia | Updated on Jul 02, 2025 07:37 PM IST

Chemistry is part of the science which embraces the investigation of the components of materials, their characteristics and the forms of their organization, the transformations that the given material passes through under the influence of certain circumstances, and the principles of such transformations. Chemistry is a core discipline of science and is related to other sciences on many occasions. Thus, it also has a significant role in our everyday life.

This Story also Contains

Importance of Chemistry And Nature of Matter
Some Solved Examples
Conclusion

Nature and Characteristics of Matter: What is, Examples, Particles

Importance of Chemistry And Nature of Matter

Chemistry deals with the composition, structure, and properties of matter. These aspects can be best described and understood in terms of basic constituents of matter: atoms and molecules. That is why chemistry is called the science of atoms and molecules.

Chemistry plays a central role in science and is often intertwined with other branches of science like physics, biology, geology, etc. Chemistry also plays an important role in daily life. Chemical principles are important in diverse areas, such as weather patterns, the functioning of the brain, and the operation of a computer. Chemical industries manufacturing fertilizers, alkalis, acids, salts, dyes, polymers, drugs, soaps, detergents, metals, alloys, and other inorganic and organic chemicals, including new materials, contribute in a big way to the national economy. Chemistry plays an important role in meeting human needs for food, healthcare products, and other materials aimed at improving the quality of life.

Anything which has mass and occupies some space is called matter. Based on shape, size, and volume, the matter can be classified into solids. liquids and gases.

Solids have definite volume and definite shape.
Liquids have a definite volume but no definite shape. They take the shape of the container in which they are placed.
Gases have neither a definite volume nor a definite shape. They completely occupy the container in which they are placed.

These three states of matter are interconvertible by changing the conditions of temperature and pressure.

Solid $\underset{\text { cool }}{\stackrel{\text { heat }}{\rightleftharpoons}}$ liquid $\underset{\text { cool }}{\stackrel{\text { heat }}{\rightleftharpoons}}$ Gas

On heating, a solid usually changes to a liquid, and the liquid on further heating changes to the gaseous ( or vapour) state. In the reverse process, a gas on cooling liquifies to the liquid, and the liquid on further cooling freezes to the solid.

Some Solved Examples

Example 1: Which of the following is known as dry ice?

1) Gaseous CO₂

2) Solid SiO₂

3) CH₄

4) Solid CO₂

Solution

Solid CO₂is called as dry ice.

Hence, the answer is the option (4).

Example 2: Which of the following exists as a solid at room temperature?

1)Cl₂

2)F₂

3) I₂

4) Br₂

Solution

F₂ and Cl₂ are gases, Br₂ is a liquid and I₂ exists as a solid at room temperature because of the difference in intermolecular forces that act on between individual molecules.

Iodine is present in solid form at room temperature, while chlorine is a gas at room temperature because of the difference in intermolecular forces that act between individual molecules.

Hence, the answer is an option (3).

Example 3:What is the state of water below 0^oC?

1) Solid

2) Liquid

3) Gas

4) Plasma

Solution

Water exists in three different forms i.e., solid, liquid, and gas. Below 0^oC, intermolecular hydrogen bonding is very strong between the different water molecules, thus water exists in solid form as ice.

Hence, the answer is the option (1).

Conclusion

The material world around us consists of an enormous variety of substances. Man has been curious to know about his surroundings ever since he came into existence. Science has been helping man to systematize his knowledge to describe and understand nature. Chemistry industries manufacturing fertilizers, acids, alkalies, salts, dyes, and other organic and inorganic chemicals including new materials have improved our national economy.

Frequently Asked Questions (FAQs)

1. Q. In how many ways matter can be classified?

Matter are classified in 2 ways

2. Q. What other name is given to the drug that is used to cure cancer?

Cisplatin and taxol

3. State the drug given to a victim of AIDS.

AZT (azidothymidine)

4. What is the matter?

Limiting the definition simply to something that has mass and occupies space will suffice as the definition of matter.

5. Q. What is removed to decrease your temperature in severe conditions?

Antipyretics drugs are use to decrease the high temp.

6. What is matter?

Matter is anything that has mass and occupies space. It is the physical substance that makes up everything in the universe, from the tiniest atom to the largest galaxy. Matter can exist in different states, such as solid, liquid, or gas, and can undergo changes in form or composition.

7. How do we know that all matter is made up of particles?

We know that all matter is made up of particles through various scientific observations and experiments. For example, Brownian motion (the random movement of particles suspended in a fluid) provides evidence for the existence of particles. Additionally, the behavior of gases, the process of diffusion, and the success of atomic theory in explaining chemical reactions all support the particulate nature of matter.

8. What are the three main states of matter?

The three main states of matter are 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 neither a fixed shape nor volume, expanding to fill their container.

9. Can matter be created or destroyed?

According to the law of conservation of mass, matter cannot be created or destroyed in chemical reactions. However, in nuclear reactions and certain high-energy physics processes, matter can be converted to energy and vice versa, following Einstein's famous equation E=mc².

10. What is the difference between an element and a compound?

An element is a pure substance made up of only one type of atom, while a compound is a substance made up of two or more different elements chemically bonded together in a fixed ratio. For example, hydrogen is an element, while water (H2O) is a compound.

11. How does the kinetic molecular theory explain the behavior of gases?

The kinetic molecular theory states that gas particles are in constant, random motion, colliding with each other and the container walls. This theory explains gas properties such as pressure (caused by particle collisions with container walls) and the relationship between temperature and particle speed.

12. What is the relationship between pressure and volume in gases?

The relationship between pressure and volume in gases is described by Boyle's Law, which states that for a fixed amount of gas at constant temperature, pressure and volume are inversely proportional. As pressure increases, volume decreases, and vice versa. This relationship is due to the compressibility of gases and the space between gas particles.

13. What is the significance of Lewis structures in understanding molecular bonding?

Lewis structures are diagrams that show how valence electrons are arranged among atoms in molecules. They help visualize chemical bonds, predict molecular geometry, and understand reactivity. By representing shared and unshared electron pairs, Lewis structures provide insights into a molecule's polarity, bond angles, and potential reaction sites.

14. What is the relationship between bond order and bond strength?

Bond order refers to the number of electron pairs shared between two atoms in a molecule. Generally, as bond order increases, bond strength increases. For example, a triple bond (bond order of 3) is stronger than a double bond (bond order of 2), which is stronger than a single bond (bond order of 1). This concept helps explain differences in bond lengths and dissociation energies.

15. How does the VSEPR theory explain molecular geometry?

The Valence Shell Electron Pair Repulsion (VSEPR) theory predicts molecular geometry based on the arrangement of electron pairs around a central atom. It states that electron pairs repel each other and arrange themselves to minimize repulsion, determining the shape of molecules. This theory helps explain and predict the three-dimensional structure of molecules, which influences their properties and reactivity.

16. How does the concept of chirality relate to molecular structure?

Chirality refers to the property of a molecule that is not superimposable on its mirror image. Chiral molecules have the same chemical formula and bonding sequence but different spatial arrangements of atoms. Understanding chirality is crucial in organic chemistry and biochemistry, as it can significantly affect a molecule's properties and reactivity, especially in biological systems.

17. What is the relationship between molecular structure and spectroscopic properties?

Molecular structure directly influences a substance's spectroscopic properties. Different types of spectroscopy (IR, NMR, UV-Vis) interact with specific aspects of molecular structure, such as bond vibrations, nuclear spin environments, or electronic transitions. Understanding this relationship allows chemists to use spectroscopic data to determine molecular structures and identify compounds.

18. How does the concept of formal charge help in determining molecular structure?

Formal charge is a way to keep track of electrons in Lewis structures. It helps determine the most likely structure among several possible Lewis structures for a molecule or ion. The structure with the smallest formal charges and formal charges closest to zero is usually the most stable. This concept is crucial for predicting the most probable arrangement of atoms in a

19. How do atoms differ from molecules?

Atoms are the smallest unit of an element that retains its chemical properties. Molecules, on the other hand, are formed when two or more atoms bond together. For instance, an oxygen atom (O) is different from an oxygen molecule (O2), which consists of two oxygen atoms bonded together.

20. What is the relationship between temperature and particle movement?

Temperature is a measure of the average kinetic energy of particles in a substance. As temperature increases, particles move faster and have more kinetic energy. Conversely, as temperature decreases, particle movement slows down. This relationship explains why substances expand when heated and contract when cooled.

21. How does the arrangement of particles differ in solids, liquids, and gases?

In solids, particles are tightly packed in a fixed arrangement with strong intermolecular forces. In liquids, particles are close together but can move around each other with weaker intermolecular forces. In gases, particles are far apart and move freely with minimal intermolecular forces.

22. What is meant by the term "phase change"?

A phase change refers to the transition of matter from one state to another, such as from solid to liquid (melting) or liquid to gas (vaporization). During a phase change, the temperature remains constant while energy is absorbed or released to change the arrangement and behavior of particles.

23. How does density relate to the nature of matter?

Density is a measure of mass per unit volume and is determined by how closely packed the particles of a substance are. It helps explain why some substances float or sink in others. For example, ice floats in water because it has a lower density due to its crystal structure, which creates more space between water molecules.

24. What is the difference between physical and chemical properties of matter?

Physical properties are characteristics that can be observed without changing the substance's chemical composition, such as color, shape, or boiling point. Chemical properties describe how a substance interacts with other substances to form new substances, such as flammability or reactivity with acids.

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

Intermolecular forces are attractions between molecules that influence a substance's physical properties. Stronger intermolecular forces result in higher boiling points, surface tension, and viscosity. For example, water has strong hydrogen bonds, which contribute to its high boiling point and surface tension compared to other liquids of similar molecular mass.

26. What is the difference between homogeneous and heterogeneous matter?

Homogeneous matter has a uniform composition throughout, such as pure water or air. Heterogeneous matter has a non-uniform composition, with visible boundaries between its different components, such as a salad or granite rock. Understanding this difference is crucial for identifying mixtures and pure substances.

27. What is meant by the term "allotropes" in chemistry?

Allotropes are different structural forms of the same element. They have the same type of atoms but different arrangements, resulting in different physical properties. For example, diamond and graphite are allotropes of carbon with vastly different properties due to their different crystal structures.

28. How does the concept of matter relate to energy?

Matter and energy are interrelated, as described by Einstein's famous equation E=mc². This equation shows that matter can be converted to energy and vice versa. In chemical reactions, energy is often absorbed or released as bonds between atoms are broken or formed, demonstrating the close relationship between matter and energy.

29. What is the significance of Avogadro's number in understanding matter?

Avogadro's number (approximately 6.022 x 10²³) represents the number of particles (atoms, molecules, or formula units) in one mole of a substance. It provides a way to connect the microscopic world of atoms and molecules to the macroscopic world we can measure, allowing chemists to relate atomic-scale properties to observable quantities.

30. How do subatomic particles contribute to the properties of matter?

Subatomic particles (protons, neutrons, and electrons) determine an atom's identity and behavior. The number of protons defines the element, while electrons are responsible for chemical bonding and many physical properties. Neutrons affect an atom's mass and stability. The arrangement and interaction of these particles give rise to the diverse properties of matter we observe.

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

Intensive properties do not depend on the amount of matter present, such as density, melting point, or color. Extensive properties, on the other hand, do depend on the amount of matter, such as mass, volume, or heat capacity. Understanding this distinction is crucial for characterizing and comparing different substances.

32. How does the arrangement of atoms in a crystal structure affect its properties?

The crystal structure, or the regular, repeating arrangement of atoms in a solid, greatly influences its properties. For example, the tetrahedral arrangement of carbon atoms in diamond results in its hardness, while the layered structure of graphite makes it soft and slippery. Crystal structure affects properties like hardness, conductivity, and optical characteristics.

33. How does the concept of polarity affect the properties of molecules?

Polarity refers to the uneven distribution of electrical charge in a molecule. Polar molecules, like water, have slightly positive and negative ends, which leads to properties such as higher boiling points, solubility in other polar substances, and the ability to form hydrogen bonds. Non-polar molecules, like methane, lack this charge separation and behave differently.

34. What is the significance of the periodic table in understanding matter?

The periodic table organizes elements based on their atomic structure and properties. It reveals patterns in electron configuration, reactivity, and other characteristics across elements. This organization helps predict an element's behavior, its compounds' properties, and how it will interact with other elements, making it a fundamental tool for understanding matter.

35. How do isotopes differ, and why are they important in chemistry?

Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons. They have identical chemical properties but different physical properties due to their different masses. Isotopes are important in radioactive dating, nuclear chemistry, and as tracers in biological and environmental studies.

36. What is the difference between covalent and ionic bonding in matter?

Covalent bonding involves the sharing of electrons between atoms, typically in molecules or network structures. Ionic bonding involves the complete transfer of electrons, resulting in oppositely charged ions held together by electrostatic forces. These different bonding types lead to distinct properties in the resulting substances, such as melting point, solubility, and conductivity.

37. How does the concept of entropy relate to the nature of matter?

Entropy is a measure of the disorder or randomness in a system. In the context of matter, entropy helps explain why certain processes occur spontaneously, such as the mixing of gases or the melting of ice. As temperature increases, the entropy of matter generally increases as particles gain more energy and freedom of movement.

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

The mole is a unit that allows chemists to work with manageable numbers of particles. One mole contains Avogadro's number of particles. This concept bridges the gap between the atomic scale and the macroscopic world, enabling calculations involving mass, volume, and number of particles in chemical reactions and everyday quantities of substances.

39. How do intermolecular forces differ from intramolecular forces?

Intramolecular forces are the strong chemical bonds within a molecule, such as covalent or ionic bonds. Intermolecular forces are weaker attractions between molecules, such as hydrogen bonding or van der Waals forces. While intramolecular forces determine a molecule's structure, intermolecular forces influence physical properties like boiling point and solubility.

40. What is the relationship between chemical formula and molecular structure?

A chemical formula shows the types and numbers of atoms in a molecule or compound, while molecular structure describes how these atoms are arranged in three-dimensional space. For example, C2H6O could represent ethanol (CH3CH2OH) or dimethyl ether (CH3OCH3), which have the same formula but different structures and properties.

41. How does the concept of resonance contribute to understanding molecular structure?

Resonance describes a molecule or ion that can be represented by multiple valid Lewis structures. It occurs when electrons are delocalized over several atoms. Understanding resonance is crucial for explaining the stability, reactivity, and properties of many molecules, such as benzene or the carbonate ion, which cannot be accurately described by a single Lewis structure.

42. What is the difference between empirical and molecular formulas?

An empirical formula shows the simplest whole-number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms in a molecule. For example, the empirical formula of glucose is CH2O, while its molecular formula is C6H12O6. Understanding this difference is crucial for interpreting chemical analysis results and determining molecular composition.

43. How does the concept of oxidation state relate to the nature of matter?

Oxidation state (or oxidation number) is a concept that describes the degree of oxidation of an atom in a chemical compound. It helps track electron transfers in redox reactions and understand the behavior of elements in different compounds. For example, the oxidation state of carbon ranges from -4 in methane (CH4) to +4 in carbon dioxide (CO2).

44. How do quantum numbers describe the nature of electrons in atoms?

Quantum numbers (principal, azimuthal, magnetic, and spin) describe the energy, shape, orientation, and spin of electron orbitals in atoms. They arise from the wave nature of electrons and the quantum mechanical model of the atom. Understanding quantum numbers is crucial for explaining atomic structure, spectral lines, and chemical bonding.

45. What is the significance of electronegativity in understanding chemical bonding?

Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. It helps predict the type of bond formed between atoms (ionic, polar covalent, or nonpolar covalent) and explains properties like bond polarity and molecular polarity. Understanding electronegativity is crucial for predicting chemical behavior and reactivity.

46. How does the concept of hybridization explain molecular structure?

Hybridization is the mixing of atomic orbitals to form new hybrid orbitals of equal energy. It explains the geometry of molecules that cannot be accounted for by simple atomic orbital theory. For example, the tetrahedral structure of methane (CH4) is explained by sp³ hybridization of carbon's orbitals. Understanding hybridization is crucial for predicting molecular shapes and bonding patterns.

47. What is the relationship between intermolecular forces and phase changes?

Intermolecular forces determine the strength of attraction between molecules. During phase changes, these forces are overcome or formed. For example, during vaporization, intermolecular forces are broken as molecules gain enough energy to escape the liquid phase. The strength of these forces affects properties like boiling point, melting point, and heat of vaporization.

48. What is the significance of bond angles in molecular structure?

Bond angles are the angles formed between chemical bonds around an atom. They are determined by electron pair repulsion and hybridization. Bond angles influence a molecule's shape, polarity, and reactivity. For example, the 104.5° bond angle in water contributes to its bent shape and polar nature, which are crucial for its unique properties.

49. How does the concept of resonance energy contribute to molecular stability?

Resonance energy is the difference between the actual stability of a molecule and the stability predicted by its most stable Lewis structure. Molecules with resonance are more stable than would be expected from a single Lewis structure. This concept explains the enhanced stability of molecules like benzene and the carbonate ion, which have delocalized electrons.

50. How does the concept of aromaticity relate to the stability of certain molecules?

Aromaticity is a property of cyclic, planar molecules with delocalized electrons that follow Hückel's rule (4n+2 π electrons). Aromatic compounds, like benzene, are unusually stable due to this electron delocalization. Understanding aromaticity is crucial for predicting the reactivity and stability of many organic compounds, especially in the field of organic synthesis.

51. What is the significance of molecular orbital theory in understanding bonding?

Molecular Orbital (MO) theory describes chemical bonding by considering the combination of atomic orbitals to form molecular orbitals. It provides a more accurate picture of electron distribution in molecules than Lewis structures or Valence Bond theory. MO theory explains phenomena like paramagnetism in O2 and the stability of H2+, which other theories struggle to explain.