STATES OF MATTER

1. STATES OF MATTER

2. MATTER Matter is anything that takes up space and has mass. Matter does not have to be visible. Air is matter.

3. States of Matter • Three states of matter common on Earth: • Solids • Liquids • Gases • States of matter in the Universe • Plasma • Bose-Einstein Condensate 1995 • Fermionic Condensate 2004

4. The Fifth State of Matter • Bose-Einstein Condensation in a gas: a new form of matter at the coldest temperatures in the universe... It is the ability to slow down light. • Atoms move faster than photons. • Predicted 1924... • ...Created 1995 • A. Einstein S. Bose

5. The Sixth State of Matter • Scientists have created a new form of matter, which they say could lead to new ways of transmitting electricity and communication to the Moon and other planets. • The fermionic condensate is a cloud of cold potassium (P -40) atoms forced into a state where they behave strangely. It is considered a super cooled, strange superparticle and a superfluid.

6. Sixth State of MatterThe fermionic condensate

7. Solid • Solid is matter with a define shape and volume. • Particles that make up all types of matter are in constant motion.

8. Crystalline Solids • Particles are arranged in repeating three-dimensional patterns, called crystal.

9. Amorphous Solids • Solids with large particles arranged randomly. • Example: plastic, rubber.

10. Surface Tension • Uneven forces acting on the particles of the surface of the liquid. • The surface of the liquid acts as a thin film were stretched across its surface. Ex: floating an insect on the surface of water.

11. Gases • Matter does not have a definite shape or volume. Vapor Matter that exist in the gas state but is generally a liquid or solid at room temperature . Ex: water is a liquid. water vapor is a gas.

12. States of Matter. Particles Solid Liquid Gas

13. Levels of Energy in Particles Addition of energy, creates a change in state

14. Changes of State of Matter • Kinetic Energy is the total energy of motion. • Particles of matter are at constant motion. • The amount of motion depends of the kinetic energy of the particles. • Particles moving slowly have less kinetic energy. ( solids) • Particles moving faster have more kinetic energy. ( gases)

15. Temperature • The average kinetic energy of the particles that make up a substance.

16. Heat • The movement of thermal energy from a substance at a higher temperature to one at a lower temperature is called heat.

17. Specific Heat • The specific heat of a substance is the amount of heat required to raise the temperature of 1 Kg. of a substance in 1 Celsius degree.

18. Matter .- Materials that have a low specific heat • Metals Sand • Aluminum, Gold

19. Materials that have high specific heat • Water

20. Melting • The change from a solid to the liquid state.

21. Freezing • The change from the liquid state to the solid state.

22. Vaporization • The change from a liquid to gas. • As liquid water is heated ,its temperature rises until it reaches 100 Celsius. And liquid water changes into water vapor.

23. Evaporation • The conversion of water from a liquid into a gas. • Water is transferred from the surface to the atmosphere through evaporation, the process by which water changes from a liquid to a gas.

24. Evaporation

25. Condensation • It is the opposite process of vaporization. • A gas condenses to a liquid. • The decrease in energy changes the arrangements of the particles.

26. Sublimation • This is a drawing of what the surface of a comet might look like. This is a picture of dry ice (frozen CO2) sublimating.

27. Sublimation • Sublimation of an element or compound is a transition from the solid to gas phase so rapidly that the liquid phase cannot be observed. Sublimation is a phase of transition where solid gain enough energy to transform in gas.

28. Deposition • The process of a gas changing directly into a solid is called deposition or desublimation. • For example, water vapor in sub-freezing air can transform into ice • without going through • the liquid phase, which is • how snow and frost are formed.

29. Viscosity • Some liquids flow more easily than others. • A liquid resistance to flow is known as viscosity. • Slower the liquid flow, higher the viscosity. • High viscosity pure honey.

30. Behavior of Fluids • Pressure is the force exerted on a surface divided by the total area over which the force is exerted. • P= F/ A • Force is measure in Newtons N. • Area is measured in m2 ( square meter) • N/m2 the unit is called Pascal ( Pa)

31. Pressure • Steam machine. Pumps water out of mines. ( Thomas Savery 17th century )

32. Pressure • Crushing a can is applying pressure.

33. Pascal Principle • Atmospheric pressure at the sea level is 101.3 KPa ( kilopascals). This means that air exerts a force about 101,000 N ( Newtons).

34. Atmospheric Pressure • Changes with altitude. • Altitude is the height above the sea level. • As altitude increases, atmospheric pressure decreases.

36. Buoyant Force/Archimede’s Principle • The difference in pressure results in an upward force on an object immerse in a fluid. • The buoyant force is equal to the weight of the object.

37. Buoyancy • Sink or float

38. Archimedes’Principle • Density is mass divided by volume • D= m/v • Understanding density can help you predict whether an object will float or sink.

39. Pascal’s principle • When a force is applied to a confined fluid, an increase in pressure is transmitted equally to all parts of the fluid. • This relationship is known as Pascal’s Principle.