Concepts of Matter | Waec Physics

Simple Structure of Matter

1. Matter is anything that occupies space and has mass.
2. Atoms are the fundamental building blocks of matter.
3. Molecules are formed by the chemical combination of two or more atoms.
4. Matter is composed of protons, neutrons, and electrons.
5. Protons and neutrons form the nucleus of an atom, while electrons orbit the nucleus.
6. The electron configuration determines the chemical properties of an atom.
7. Elements are pure substances consisting of one type of atom.
8. Compounds are substances formed by the chemical combination of different elements.
9. Matter can exist in three primary states: solid, liquid, and gas.
10. The structure of matter at the microscopic level explains its macroscopic properties.

The Three States of Matter

11. Solids have a definite shape and volume due to closely packed particles.
12. Liquids have a definite volume but take the shape of their container.
13. Gases have neither a definite shape nor volume and expand to fill their container.
14. Particles in solids vibrate around fixed positions.
15. In liquids, particles move more freely but remain close to one another.
16. Gas particles are widely spaced and move rapidly in random directions.
17. Plasma, the fourth state of matter, is an ionized gas found in stars.
18. The transition between states occurs through physical processes like melting, freezing, and condensation.
19. Solids resist compression due to strong intermolecular forces.
20. Liquids flow because intermolecular forces are weaker than in solids.
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Evidence of the Particle Nature of Matter

21. The particle nature of matter explains its discrete structure.
22. Diffusion demonstrates that matter is made up of particles.
23. Brownian motion is observable evidence of particle movement.
24. In the Brownian motion experiment, pollen grains in water move randomly.
25. Robert Brown first observed Brownian motion in 1827.
26. The random movement in Brownian motion results from collisions with water molecules.
27. Gases diffuse faster than liquids because of weaker intermolecular forces.
28. The zigzag path of particles in Brownian motion supports the kinetic theory.
29. Particle collisions are elastic, conserving energy in the system.
30. Diffusion rate depends on temperature, as heat increases particle speed.
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Kinetic Theory of Matter

31. The kinetic theory states that all matter is composed of small particles in constant motion.
32. The energy of particles determines the state of matter.
33. Temperature is proportional to the average kinetic energy of particles.
34. Higher temperatures increase particle speed and energy.
35. In solids, particles vibrate but remain bound by strong forces.
36. Liquids have more kinetic energy, allowing particles to slide past each other.
37. Gases possess the highest kinetic energy, leading to free particle movement.
38. Pressure in gases arises from collisions of particles with container walls.
39. Evaporation occurs when high-energy particles escape from a liquid surface.
40. Boiling involves the rapid conversion of liquid to gas at the boiling point.
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Use the Kinetic Theory to Explain States of Matter

41. Solids are rigid because their particles are held by strong intermolecular forces.
42. Liquids flow due to intermediate forces that allow particles to move freely.
43. Gases are compressible because particles are widely spaced.
44. Pressure in a gas increases with temperature due to more frequent collisions.
45. Evaporation happens below boiling point due to high-energy particles escaping.
46. Boiling involves vaporization occurring throughout the liquid at a specific temperature.
47. A rise in temperature provides energy to overcome intermolecular forces.
48. Cooling slows particles, leading to condensation or solidification.
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Cohesion, Adhesion, and Capillarity

49. Cohesion refers to the force of attraction between similar molecules.
50. Adhesion is the force of attraction between dissimilar molecules.
51. Surface tension arises from cohesive forces at the surface of a liquid.
52. Adhesion causes water to stick to surfaces, like glass.
53. Capillarity is the movement of liquid in narrow tubes due to adhesion and cohesion.
54. Water rises in a capillary tube because adhesion pulls the liquid up, while cohesion keeps it intact.
55. Capillarity is essential in plants for water transport in xylem vessels.
56. The balance between cohesion and adhesion explains droplet formation on surfaces.
57. Strong cohesive forces result in high surface tension.
58. Adhesive forces are responsible for the spreading of liquids on certain surfaces.
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Crystalline and Amorphous Substances

59. Crystalline substances have a well-ordered, repeating atomic structure.
60. Amorphous substances lack a regular atomic arrangement.
61. Examples of crystalline materials include salt, diamond, and quartz.
62. Glass and plastic are examples of amorphous substances.
63. Crystalline substances have sharp melting points.
64. Amorphous substances soften over a temperature range.
65. Crystalline materials exhibit anisotropy, meaning properties vary with direction.
66. Amorphous substances are isotropic, with uniform properties in all directions.
67. The orderly arrangement in crystalline solids leads to high strength and durability.
68. Amorphous substances are less rigid and more prone to deformation.
69. The internal arrangement of atoms determines the physical properties of substances.
70. Crystalline and amorphous structures influence material behavior in technology and manufacturing.

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