States of Matter and KMT PPT Slides PDF

Section 11.1 http://www.slideshare.net/WongSookYen/stpm-form-6-chemistry-mole-and-avogadro ! Two factors determine the state of a substance: ! The forces holding the particles together ! The kinetic energy of the particles (which tends to pull them apart) ! The particle theory states that...

Section 11.1 http://www.slideshare.net/WongSookYen/stpm-form-6-chemistry-mole-and-avogadro ! Two factors determine the state of a substance: ! The forces holding the particles together ! The kinetic energy of the particles (which tends to pull them apart) ! The particle theory states that there are attractive forces between particles ! The weaker the attractive forces the freer the particles are to move ! States: All substances contain entities that are in constant random motion ! How do we know this? ! Scottish scientist Robert Brown (1773-1858) ! Examined pollen under the microscope and was amazed at what he saw https://www.youtube.com/watch?v=4m5JnJBq2AU ! Explains why you can smell cookies baking in the kitchen in your bedroom  Solids Liquids Gases Types of Motion vibrational vibrational, vibrational, rotational, and rotational, and translational translational Strength of strongest intermediate weakest Attraction Organization of Highly organized Intermediate level Least organized entities of organization ! Temperature – a measure of the average kinetic energy of the entities of a substance ! A hotter substance with high kinetic energy is more likely to overcome attractive forces between molecules and exist as a gas ! A cooler substance is more likely to be a liquid or a solid ! The volume of an individual gas molecule is negligible compared to the volume of the container holding the gas. ! There are neither attractive nor repulsive forces between gas molecules. ! Gas molecules move randomly in all directions, in straight lines. ! When gas molecules collide there is no loss of kinetic energy. ! The average kinetic energy of gas molecules is directly related to the temperature. The greater the temperature, the greater the average motion of the molecules and the greater their kinetic energy. ! The KMT describes a hypothetical gas called an ideal gas ! In an ideal gas, the gas particles take up hardly any space ! Particles in an ideal gas do not attract each other ! Of course no gas is “ideal” ! Does allow us to calculate mathematically, with high degree of accuracy how real gases behave under varying conditions ! Read textbook pages 514-519 ! Do questions 1-10 page 519