States, Boiling Point, Melting Point, and Solubility
Solid Liquid Gas Defining States of Matter
● States of matter are defined by whether they hold SHAPE and VOLUME
Element (Au) Compound (NaCl) Mixture (Milk, Salt, etc)
ALL KEEP THE SAME SHAPE AND VOLUME = Solids Particle View of a Solid
● Particles in a solid are PACKED CLOSELY together and they are in a FIXED POSITION.
Particles vibrate in place Liquids
● Liquids – has definite VOLUME but no defined SHAPE
100 ml Particle View of a Liquid
● Packed CLOSELY (like a solid), but move FREELY around each other (must stay in contact). Gases
● Gases - do NOT have definite SHAPE or VOLUME.
Bromine gas fills up the entire volume of the container. Particle view of a Gas
● Particles can MOVE FREELY and will either fill up or squeeze into available space. Task
● Draw a diagram of
● A) Gas particles
● B) Liquid particles
● C) Solid particles Changes in States of Matter
● Thermal Energy – heat energy.
● More thermal energy = More particle movement Changing States
Increase Thermal Energy (Heat up)
point Solid Liquid Gas Melting Melting Boiling Point
Decrease Thermal Energy (Cool off) Melting point
● Melting - change from solid to liquid ● Melting point - SPECIFIC temperature when melting occurs. ● Each pure substance has a SPECIFIC melting point. ● Examples: ● M.P. of Water = 0°C (32°F) ● M.P. of Nitrogen = -209.9 °C (-345.81998 °F) ● M.P. of Silver = 961.93 °C (1763.474 °F) ● M.P. of Carbon = 3500.0 °C (6332.0 °F) Melting Point
● Particles of a solid vibrate so fast that they break free from their fixed positions.
Increasing Thermal Energy
Solid Liquid
Melting point Vaporization
● Vaporization – change from liquid to gas
● Vaporization happens when particles in a liquid gain enough energy to form a gas.
Increasing Thermal Energy
Liquid Gas
Boiling point Two Kinds of Vaporization
● Evaporation – vaporization that takes place only on the surface of the liquid
● Boiling – when a liquid changes to a gas BELOW its surface as well as above. Boiling Point
● Boiling Point – temperature at which a liquid boils ● Each pure substance has a SPECIFIC boiling point. ● Examples: ● B.P. of Water = 100°C (212°F) ● B.P. of Nitrogen = -195.79 °C (-320.42 °F) ● B.P. of Silver = 2162 °C (3924 °F) ● B.P. of Carbon = 4027 °C (7281 °F) Boiling Point
Increase Thermal Energy (Heat up)
Solid Liquid Gas
Decrease Thermal Energy (Cool off) Melting & Boiling Point
Melting Boiling Gas turns back into a Point Point liquid at its boiling point because it’s moving in the OTHER DIRECTION.
Metal becomes a liquid just above its Increase Thermal Energy (Heat up) melting point.
Solid Liquid Gas
Decrease Thermal Energy (Cool off) Boiling Point
Increase Thermal Energy (Heat up) ● Particles move the least under melting point (as a solid).
Solid Liquid Gas ● Tin is a metal. Describe the movement of particles AFTER Decrease Thermal Energy (Cool off) boiling point of Tin. ● The higher the boiling point, the more energy Which one required to boil! requires the most energy to boil? Boiling Point and Melting Point
Boiling point
Melting point Solubility
● Maximum amount of a substance that can be dissolved in a liquid (at a specific temperature).
● Soluble means it will dissolve. Insoluble means it will NOT dissolve.
● Stirring SPEEDS UP the dissolution process because you are increasing the movement and the energy of the particles. The War of Insolubility! Solubility can change…
● Increased Temp = Increased Solubility
● Different substances have different solubility curves NaCl Dissolving in H2O