Matter Particles Characteristics - Properties, Particle theory, FAQs

Edited By Team Careers360 | Updated on Jul 02, 2025 04:57 PM IST

Our beautiful earth is the third among the total nine planets which orbits the sun. About two third of the earth surface is covered by water in the form of seas, rivers, lakes, glaciers Etc. Only one third of the surface of earth is available for human beings, animal kingdom, trees and plants to occupy. Entire earth is surrounded by earth’s atmosphere, consisting of a mixture of gases, mainly nitrogen, oxygen, carbon dioxide and other gases.

This Story also Contains

Characteristics of matter
Physiochemical characteristics of matter
Physical properties of matter
Chemical properties of matter
Particle theory of matter

We are living and surviving on the solid earth because we are drowned in the atmosphere. Marine life exists because they are drowned in water in which oxygen is dissolved. Oxygen and water are the two essential things without which life is impossible. In general earth exists in three states. The inner central core of earth is in molten state and has a temperature of about 4000 degrees. Water on the surface of earth and below it is also in liquid state.

The atmosphere is in gaseous state. Matter is simply anything that comprises space and has mass. In general, all the matter in the universe exists in three states, solid, liquid and gas. It is intended to study matter, physicochemical characteristics, it’s fundamental theories and all about particles and much more.

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State the characteristics of particles of matter.

Characteristics of matter

Density
Color
Mass
Volume
Malleability
Melting point
Boiling point
Temperature

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Physiochemical characteristics of matter

The physicochemical properties of matter are classified as extensive and intensive properties.
Extensive properties: any property of matter that depends on the quantity of matter that is being measured.
For example, mass and volume.
Intensive properties: any property of matter that can be determined by altering a matter’s molecular structure.

Physical properties of matter

Physical properties of matter are the characteristics that can be observed without altering the chemical behavior of matter. Some physical properties of matter are given below.

Density is an intensive property of matter.
Color is an intensive property of matter.
Mass is an extensive property of matter.
Volume is an extensive property of matter.
Physical constants that are melting point and boiling point are intensive properties of matter.

Chemical properties of matter

Chemical property of a matter is the ability of a matter to undergo chemical change under certain chemical behavior. Some of the chemical properties of matter are listed below.

Flammability implies whether a compound will catch fire when exposed to flame.
Heat of combustion is the energy released when a substance undergoes complete burning in presence of oxygen.
Chemical stability implies whether a substance will react in presence of air or water.
Oxidation states, the lowest energy oxidation state is the preferred state for a metal to undergo chemical changes.

Particle theory of matter

A long time ago in Greece, Democritus pointed out that matter comprises very small particles too tiny for the naked eye.

After much time gone, scientists using Democritus idea plus adding some statements created a theory called Particle theory of matter which consists of following five points

Matter is divisible in nature that is, it is made up of smaller and smaller particles.

Oxygen atom and Water Molecule

Particles of matter are continuously moving or we can say that all particles of matter are in continuous random motion. At higher temperatures the movement is quite faster because of the increase in kinetic energy with increase in temperature.

carbon, Nitrogen and Oxigen Atom

Related Topics Link,

The particles of matter are attractive in nature, they attract each other.

colder and warner

All particles of matter comprise space in between them which is much larger in comparison to the particles itself.

identical particles in one substance.

The particles of a matter are pure that is there are

identical particles in one substance.

Composite particles

Composite particle is a subatomic particle that consists of one or more elementary particles. The best examples of composite particles are the protons and neutrons which are present in the nucleus which is the central core of the atom, as they are composite, they consist of quarks. Quarks are nothing but the building blocks of matter. There are two main types of quarks: the up quark and the down quark. The proton consists of two up quark and quark and one up quark.

Coarse particle

Coarse particles are the relatively bigger particles which are found in air mainly produced by the mechanical breaking of even bigger particles. Coarse particles range in the size from 2.5 to 10 micrometer, which is the differentiating point between other particulate matter known as ultrafine particles and fine particles which range in the diameter of 0.1 to 2.5 micrometer. Some of the examples of bigger airborne particulate matter are pollen, dust, spores, and fly ash.

Evidence for particles in matter

The evidence of the presence of particles in matter comes from the diffusion experiments which consist of mixing of different substances on their own which shows the zig-zag movement of the tiny particles suspended in a gas or liquid referred to as Brownian movement or motion.

Also Read:

Matter occupies space

What is matter? Matter is any form of object that has a suitable weight and even has a volume. Now as stated above there are three states of matter that are solid, liquid and gas, and if something is solid, it should have a definite shape and volume. The volume of a compound or an object implies the space it occupies.

The particles of matter are constantly moving

We are aware of the fact that particles are always in a state of continuous random motion, the reason behind this fact is that the particles which are in a state of motion have some kinetic energy that helps in the continuous movements or motions. Some of the best examples which illustrate the above fact are chemicals in a glass beaker, burning of paper or wood which gives off flying ashes etc.

Activity to show that particles of matter are in a continuous motion

Take two glass beakers and fill each of them with water.
Put a drop of blue ink in one glass beaker and leave it for some time undisturbed.
In the second glass beaker a teaspoon of salt and leave it undisturbed.
After sometime you will observe that the blue ink in one beaker spreads completely throughout the water present inside the beaker.
And in the second beaker too the salt completely dissolves throughout the water present inside the beaker.
This happens because the molecules are in a state of a complete random motion and when the temperature is raised to a certain limit this movement of particles happens to occur faster, which is due to the presence of kinetic energy.

Also check-

NCERT Chemistry Notes:

Frequently Asked Questions (FAQs)

1. What are the properties of particles of matter?

Density
Volume
Temperature
Color
Malleability

2. How small are these particles of matter?

The size of the particles is too small, preferably not visible to the naked eye. For example, the size of the coarse particles range in diameter from 0.1 to 2.5 micrometers.

3. Particles meaning in Tamil?

a tiny piece of anything.

ஏதாவது ஒரு சிறிய துண்டு

give any five points on particle theory.

Matter is divisible in nature.
All the particles of a matter are in a continuous state of random motion.
All particles of matter attract each other.
All particles of matter comprise space in between them.
All particles of a single compound are pure, that is they are identical.

4. What is the meaning of coarse particle?

Coarse particles are relatively bigger particles which are found in air, mainly produced by the mechanical breaking of even bigger particles.

5. state why the particles of matter constantly moving?

the particles of matter are in constant motion because they some amount of kinetic energy which help them in continuous random motion

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

The aufbau principle states that electrons fill orbitals from lowest to highest energy. This principle helps predict electron configurations of atoms and ions, which in turn explain chemical behavior and spectroscopic properties.

7. How do metallic, covalent, and ionic substances differ in their properties?

Metallic substances have free-flowing electrons, leading to good electrical and thermal conductivity. Covalent substances often form discrete molecules with lower melting points. Ionic substances form crystal lattices with high melting points and conduct electricity when molten or in solution.

8. What is the relationship between an atom's electron configuration and its spectral lines?

An atom's electron configuration determines the energy levels electrons can occupy. When electrons move between these levels, they absorb or emit specific wavelengths of light, producing characteristic spectral lines unique to each element.

9. What is the significance of Hund's rule in electron configuration?

Hund's rule states that electrons in the same subshell prefer to occupy separate orbitals with parallel spins before pairing up. This minimizes electron repulsion and explains patterns in electron configuration and magnetic properties of atoms.

10. How do isotopes affect the average atomic mass of an element?

The average atomic mass of an element is a weighted average of its isotopes' masses based on their natural abundance. This explains why atomic masses on the periodic table are often not whole numbers.

11. What is the significance of the valence shell in an atom?

The valence shell is the outermost electron shell of an atom. It's crucial for chemical bonding and reactivity. Atoms tend to gain, lose, or share electrons to achieve a full valence shell, which is generally more stable. This tendency drives many chemical reactions.

12. What is the relationship between an element's electron configuration and its position in the periodic table?

An element's electron configuration determines its position in the periodic table. Elements in the same group (column) have similar outer electron configurations, leading to similar chemical properties. The period (row) corresponds to the highest occupied energy level.

13. What is the significance of the octet rule in chemical bonding?

The octet rule states that atoms tend to gain, lose, or share electrons to achieve a full outer shell of eight electrons (like noble gases). This rule helps predict the formation of chemical bonds and the stability of compounds, although there are exceptions, especially for larger atoms.

14. Why do different substances have different properties?

Different substances have different properties because of variations in their atomic and molecular structures. The number and arrangement of protons, neutrons, and electrons in atoms, as well as how atoms bond together, determine a substance's unique characteristics.

15. How does atomic size change across a period and down a group in the periodic table?

Atomic size generally decreases across a period (left to right) due to increasing nuclear charge pulling electrons closer. It increases down a group due to additional electron shells, which outweigh the increased nuclear charge.

16. What is matter made up of at its most basic level?

At its most basic level, matter is composed of tiny particles called atoms. Atoms are the smallest unit of an element that retains the properties of that element. They consist of even smaller subatomic particles: protons, neutrons, and electrons.

17. How does atomic mass differ from atomic number?

Atomic mass is the total number of protons and neutrons in an atom's nucleus, while the atomic number is only the number of protons. For example, a carbon-12 atom has 6 protons and 6 neutrons, giving it an atomic mass of 12 and an atomic number of 6.

18. What are isotopes and how do they differ?

Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons. They have the same atomic number but different mass numbers. For example, carbon-12, carbon-13, and carbon-14 are all isotopes of carbon with 6, 7, and 8 neutrons respectively.

19. What is the difference between an atom and a molecule?

An atom is the smallest unit of an element that retains its properties. A molecule is formed when two or more atoms bond together. For example, an oxygen atom (O) is different from an oxygen molecule (O₂), which consists of two oxygen atoms bonded together.

20. What is the significance of the atomic number?

The atomic number is the number of protons in an atom's nucleus. It determines the element's identity and its position in the periodic table. For example, all carbon atoms have 6 protons, so carbon's atomic number is 6.

21. How do subatomic particles contribute to an atom's mass and charge?

Protons and neutrons, located in the nucleus, contribute significantly to an atom's mass. Protons have a positive charge, neutrons are neutral, and electrons (which contribute negligibly to mass) have a negative charge. In a neutral atom, the number of protons equals the number of electrons.

22. How do intermolecular forces differ from intramolecular forces?

Intramolecular forces hold atoms together within a molecule (like covalent bonds). Intermolecular forces act between molecules (like hydrogen bonds or van der Waals forces). Intermolecular forces are generally weaker and influence properties like boiling point and solubility.

23. What is the relationship between an element's electron configuration and its chemical reactivity?

An element's electron configuration, especially its valence electrons, largely determines its chemical reactivity. Elements with similar outer electron configurations (e.g., same group in the periodic table) tend to have similar chemical properties and reactivity.

24. How does the quantum mechanical model differ from the Bohr model?

The quantum mechanical model describes electrons as existing in probability clouds (orbitals) rather than fixed orbits. It accounts for the wave-like nature of electrons and provides a more accurate representation of electron behavior, including the concept of electron spin.

25. What is the significance of atomic orbitals?

Atomic orbitals are regions in an atom where electrons are likely to be found. They come in different shapes (s, p, d, f) and help explain chemical bonding, molecular geometry, and spectroscopic properties of elements.

26. How does the particle theory explain the states of matter?

The particle theory explains states of matter based on the arrangement and movement of particles. In solids, particles are tightly packed and vibrate in fixed positions. In liquids, particles are close but can move around each other. In gases, particles are far apart and move freely in all directions.

27. How do electrons contribute to chemical bonding?

Electrons, especially those in the outermost shell (valence electrons), play a crucial role in chemical bonding. Atoms can share, gain, or lose electrons to form covalent, ionic, or metallic bonds, respectively. These bonds determine the properties and behavior of substances.

28. How does the Bohr model explain electron energy levels?

The Bohr model depicts electrons orbiting the nucleus in fixed energy levels or shells. Electrons can jump between these levels by absorbing or emitting specific amounts of energy. This model helps explain atomic spectra and the stability of atoms.

29. 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. This principle explains electron configuration patterns and the structure of the periodic table.

30. What is the relationship between bond angle and molecular geometry?

Bond angles are determined by the arrangement of electron pairs (both bonding and non-bonding) around a central atom, as described by VSEPR theory. Understanding this relationship helps predict and explain molecular shapes and their properties.

31. What is the difference between covalent and ionic bonding?

Covalent bonding involves sharing of electrons between atoms, typically between non-metals. Ionic bonding involves the complete transfer of electrons, usually from a metal to a non-metal, resulting in oppositely charged ions that attract each other.

32. How does electronegativity affect chemical bonding?

Electronegativity is an atom's ability to attract electrons in a chemical bond. Differences in electronegativity between bonded atoms determine bond polarity. Large differences lead to ionic bonds, while smaller differences result in polar covalent bonds.

33. How does the concept of electron shielding affect atomic properties?

Electron shielding occurs when inner electron shells partially block the nuclear charge felt by outer electrons. This effect influences atomic size, ionization energy, and electron affinity, explaining trends in the periodic table.

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

Hybridization involves the mixing of atomic orbitals to form new hybrid orbitals. This concept explains the geometry of molecules that don't conform to simple VSEPR predictions, such as the tetrahedral shape of methane (CH₄).

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

Bond order is the number of electron pairs shared between atoms. Higher bond orders (e.g., double or triple bonds) generally result in stronger, shorter bonds. This concept helps explain differences in bond energies and molecular reactivity.

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

Resonance occurs when a molecule's structure can be represented by multiple valid Lewis structures. The actual structure is a hybrid of these resonance forms, often resulting in greater stability than any single structure would suggest.

37. What is the significance of the noble gas configuration in chemical bonding?

The noble gas configuration (full outer shell) is generally very stable. Many atoms form chemical bonds to achieve this configuration, explaining why noble gases are less reactive and why other elements often gain, lose, or share electrons to mimic this stable arrangement.

38. How do quantum numbers describe an electron's state in an atom?

Quantum numbers (n, l, ml, ms) describe an electron's energy, angular momentum, magnetic moment, and spin, respectively. They provide a complete description of an electron's quantum state and explain atomic spectra and chemical behavior.

39. What is the relationship between molecular polarity and intermolecular forces?

Molecular polarity, resulting from uneven electron distribution, influences intermolecular forces. Polar molecules can engage in stronger intermolecular interactions (like hydrogen bonding), affecting properties such as boiling point and solubility.

40. How does the concept of effective nuclear charge explain periodic trends?

Effective nuclear charge is the net positive charge experienced by an electron, accounting for shielding by inner electrons. It increases across a period and explains trends in atomic size, ionization energy, and electron affinity.

41. How do atomic emission spectra provide evidence for quantized energy levels in atoms?

Atomic emission spectra show discrete lines of specific wavelengths, rather than a continuous spectrum. This indicates that electrons can only exist at specific energy levels and emit or absorb specific amounts of energy when transitioning between these levels.

42. What is the relationship between an element's position in the periodic table and its electron affinity?

Electron affinity generally increases across a period and decreases down a group. This trend is related to atomic size and effective nuclear charge, with smaller atoms and higher effective nuclear charges typically having higher electron affinities.

43. How does the concept of electronegativity explain bond polarity?

Electronegativity differences between bonded atoms determine bond polarity. Larger differences lead to more polar bonds, with the more electronegative atom attracting the shared electrons more strongly. This concept helps predict molecular polarity and reactivity.

44. What is the significance of the lanthanide and actinide contractions?

The lanthanide and actinide contractions refer to the smaller-than-expected increase in atomic radius across these series. This is due to poor shielding by f-electrons and affects the properties of elements following these series in the periodic table.

45. How do molecular orbital theory and valence bond theory differ in explaining chemical bonding?

Valence bond theory focuses on the overlap of atomic orbitals, while molecular orbital theory considers the formation of molecular orbitals from linear combinations of atomic orbitals. Molecular orbital theory better explains some phenomena like paramagnetism in O₂.

46. What is the relationship between an atom's ground state and excited states?

The ground state is an atom's lowest energy configuration. Excited states occur when electrons occupy higher energy levels. Understanding this relationship is crucial for explaining atomic spectra and photochemical processes.

47. How does the concept of ionization energy relate to an atom's electron configuration?

Ionization energy is the energy required to remove an electron from an atom. It generally increases across a period and decreases down a group, reflecting the stability of electron configurations and the strength of electron-nucleus attractions.

48. What is the significance of the aufbau principle exceptions in transition metals?

Some transition metals have electron configurations that seem to violate the aufbau principle (e.g., Cr, Cu). These exceptions are due to the stability gained from half-filled or fully filled d-subshells and help explain the unique properties of transition metals.

49. How do relativistic effects influence the properties of heavy elements?

In heavy elements, inner electrons move at speeds approaching the speed of light, leading to relativistic effects. These effects can alter orbital energies and sizes, influencing chemical and physical properties, especially noticeable in elements like gold.

50. How does the concept of hybridization explain the bonding in molecules like ethene (C₂H₄)?

In ethene, carbon atoms undergo sp² hybridization, forming three sp² hybrid orbitals and leaving one unhybridized p orbital. This explains the planar structure of ethene and the formation of a pi bond, which is crucial for understanding its reactivity.

51. What is the significance of Fajan's rules in predicting the covalent character of ionic compounds?

Fajan's rules predict the degree of covalent character in predominantly ionic bonds. They consider factors like the charge and size of ions, helping explain why some compounds behave more covalently than their classification as ionic compounds might suggest.

52. How do atomic and ionic radii trends differ in the periodic table?

While atomic radii generally decrease across a period and increase down a group, ionic radii trends can be more complex. Cations are smaller than their parent atoms, while anions are larger, affecting how these radii change across the periodic table.

53. What is the relationship between molecular geometry and dipole moment?

A molecule's geometry, combined with the polarity of its bonds, determines its overall dipole moment. Symmetrical molecules with polar bonds can have a net dipole moment of zero if the bond dipoles cancel each other out due to their arrangement.

54. How does the concept of electron delocalization contribute to the stability of aromatic compounds?

Electron delocalization in aromatic compounds involves the sharing of electrons over a cyclic π system. This delocalization provides extra stability (resonance energy) to aromatic molecules, explaining their unique reactivity and physical properties.

55. What is the significance of the lanthanide series in understanding electron configurations?

The lanthanide series involves the filling of 4f orbitals, which are lower in energy than the 5d orbitals. This explains the similar chemistry of lanthanides and challenges in separating them. It also demonstrates the limitations of the simple aufbau principle in predicting electron configurations.