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States of Matter Glue the Following Table in Your Science Notebooks Complete the Table As the Slides Progress

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States of Matter Glue the Following Table in Your Science Notebooks Complete the Table As the Slides Progress States of Matter Glue the following table in your science notebooks Complete the table as the slides progress. Solid Liquid Gas Plasma Definite Shape Definite Volume Structure Particle Kinetic Energy Other Info Four States (Phases) of Matter Solid State • The particles of a solid are packed closely together and constantly vibrating in place. • The attractions between particles are strong, and solids have a fixed volume and shape. Liquid State • The attractive forces are strong enough to cause particles to cling together. • Liquids have a definite volume, but not a definite shape. Gas State • In a gas, the forces between particles are so weak that the particles no longer cling together. • Gases do not have a definite shape or volume. Plasma State • The most common state of matter in the universe is the plasma state. • Plasma is matter consisting of positively and negatively charged particles and does not have a definite shape or volume. Changing States Melting • The temperature at which a solid begins to melt is its melting point. • The amount of energy required to change 1 kg of a substance from a solid to a liquid at its melting point is known as the heat of fusion. Freezing • The heat of fusion is also the energy released when a liquid freezes. • The attractive forces are strong enough that the particles form an ordered arrangement. Vaporization • Vaporization occurs as a liquid changes into a gas. • Vaporization that occurs at the surface of a liquid is called evaporation. • Evaporation causes the temperature of the liquid to decrease. Boiling • The boiling point of a liquid is the temperature at which the pressure of the vapor in the liquid is equal to the external pressure acting on its surface. • The heat of vaporization is the amount of energy required for 1 kg of the liquid, at its boiling point, to become a gas. Condensation • The heat of vaporization is also the amount of energy released during condensation. Heating Curve for Water • This graph E 3500 n e 3000 shows the r g 2500 temperature y Heat of Vaporization --- J 2000 change of water o u 1500 l as thermal e 1000 s energy is added. 500 <---Heat of Fusion 0 -50 0 50 100 150 Temperature (° C ) Condensation • The average kinetic energy of the water molecules doesn’t change. Heating Curve for Water E 3500 n e 3000 r g • The temperature 2500 y Heat of Vaporization --- J remains constant 2000 o u during melting. l 1500 e s 1000 500 <---Heat of Fusion 0 -50 0 50 100 150 Temperature (° C ) Condensation • After the liquid water Heating Curve for Water E 3500 has changed n e 3000 completely into a gas, r g 2500 the temperature of y Heat of Vaporization --- J 2000 o the gas increases as u l 1500 energy is added. e (Does this graph s 1000 500 <---Heat of Fusion remind you of 0 anything?) -50 0 50 100 150 Temperature (° C ) Thermal Expansion The Thermal Expansion of Matter • The increased separation between the particles results in the expansion of the object, and the size of the object increases. • When a material cools, the particles in the material move more slowly and become closer together. Thermal Expansion of Liquids • The forces between the particles in liquids are weaker than the forces between the particles in a solid. • The same temperature increase usually causes liquids to expand much more than solids. Thermal Expansion of Gases • In a gas, the forces between particles are much weaker than they are in liquids. • Gases expand even more than liquids for the same increase in temperature..
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