States of matter - Part 1
0 likes671 views
This document discusses states of matter and properties of matter. It defines the five known states of matter as solids, liquids, gases, plasma, and Bose-Einstein condensates. The three primary states are solids, liquids, and gases. The state that matter exists in depends on intermolecular forces, temperature, and pressure. Changes between states of matter are reversible physical changes, while chemical changes result in new substances. Key measurable gas properties discussed are mass, volume, temperature, pressure, density, and diffusion rate. Several gas laws relating these properties are also outlined.
More Related Content
What's hot (20)
Similar to States of matter - Part 1 (20)
Recently uploaded (20)
States of matter - Part 1
- 1. STATES OF MATTER & PROPERTIES OF MATTER Ms. Punam Dilip Bagad Assistant Professor, Dept. of Pharmaceutics GESs Sir Dr. M. S. Gosavi College of Pharm. Edu. & Research, Nashik-422005, INDIA 1
- 2. 2
- 3. Content as per syllabus State of matter, changes in the state of matter, Latent heats, vapour pressure, sublimation critical point, eutectic mixtures, Gases, Liquefaction of gases, aerosols inhalers, Relative humidity, liquid complexes, liquid crystals, glassy states, solid crystalline, amorphous(Methods of crystal analysis: X-Ray Diffraction, Braggs equation) Polymorphism (Definition, Different shapes of polymorphs, Example and its Pharmaceutical applications, Brief introduction of Detection techniques). 3
- 4. STATE OF MATTER Matter is the Stuff of the universe- the atoms, molecules and ions that make- up all physical substances. Matter is anything that has mass and takes up space. There are 5 known phases or states: Solids Liquids Gases Plasma Bose-Einstein Condensates 4
- 5. STATE OF MATTER Solid, liquid, and gases are the three primary states of matter or phases. The factors which usually determine the state in which matter exists are Intensity of intermolecular forces Temperature Pressure Solids have the strongest intermolecular forces and gases have the weakest. As the temperature of solid increased, the molecules acquire sufficient energy to break the ordered structure and pass into the liquid form. On further increasing the temperature, liquid changes to the gaseous state. 5
- 6. STATE OF MATTER Solid ice, liquid water, water vapor: All 3 states co-exist at the freezing point of water.. Solids with high vapor pressures, such as Iodine and Camphor, can pass directly from the solid to the gaseous state without melting at room temperature. This process is known as sublimation. 6
- 8. STATE OF MATTER A substance is a form of matter that has a constant composition. Physicochemical properties of a substance are dependent on the organizational arrangement of its constituent atoms. Example: n-butane and iso-butane (same chemical formula) 8 Physical properties n-butane iso-butane Boiling point 0属C 0属C Melting point -138属C -159属C density 0.622 g/ml 0.604 g/ml
- 9. 9
- 10. 10
- 11. 11
- 12. Changes in States of Matter Molecular interactions: keep the molecules together while the thermal energy provides motions to the molecules. K.E. based on thermal energy and intermolecular interactions based on pressure. These are responsible for intermolecular forces of attraction and decide physical state of the substance. Intermolecular forces are the forces of attraction between neighbouring molecules. Temperature and pressure decides the physical state of the substance. 12
- 13. 13
- 14. STATE OF MATTER Changes in the physical state: Changes in the physical state of substance are reversible in nature These are due to rearrangement of the molecules in a substance. Changes in the chemical state: Changes in the chemical state are due to change in specific orientation or arrangement of the atoms and groups of the substance. Changes may be irreversible Chemical changes always result in formation of a new compound having different properties. 14
- 15. Measurable properties of gases Characteristics of gases: 1) Mass 2) Volume 3) Temperature 4) Pressure 5) Density 6) Diffusion 15
- 16. Measurable properties of gases Mass: Each gas molecule has characteristic mass Mass of single gas molecule is negligibly small, Mass of one mole of gas molecule = 6.022*1023 Mass unit = gm/kg Volume: Gas occupies entire space available to it. Volume of gas is the volume of container in which it is stored. Unit : cm3/dm3/mL/L 16
- 17. Measurable properties of gases Pressure: It is the force exerted by the gas molecules per unit area on the walls of the container. Pressure measured by using Barometer or Mercury manometers Unit: Pascal, N/m2 Density: Mass/Volume Unit: Kg/m3 17
- 18. Measurable properties of gases Diffusion: The process of mixing of two or more gases to form homogeneous mixture is called diffusion. The rate at which gases diffuse depends on molar mass of gas Lighter gases diffuse faster than heavier gases. Unit = cm3/s or dm3/s ＄ = ｐ ＄ 18
- 19. Measurable properties of gases Temperature: = 9 5 + 32 19
- 20. Gas Laws Boyles Law: The pressure (P) of a given mass of a gas varies inversely as its volume (V) at constant temperature. 1 PV= K1 Gay- Lussac Law: Pressure of a given mass of gas varies directly with the temperature at constant volume. = Constant = K2 20
- 21. Gas Laws Charles Law: Volume of the given mass of the gas is directly proportional to absolute temperature at constant pressure. V= K3T By combining all three equations: PV=nRT 21