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The Learning Goal for this assignment is:<br />
Differentiate among the four states of matter.<br />
Take note over the following chapter. Use the Headings provided to organize your notes. Define and number all highlighted vocabulary (total 23 ) as well<br />
as summarize the sections. You may add pictures where needed. The pictures should be an appropriate size. Use Arial 12 for all text. This document<br />
should be 3 pages and should be saved as a pdf before you submit it into Angel.<br />
13.1 The Nature of Gases<br />
Chapter 13 States of Matter<br />
Pages 420 - 439<br />
Kinetic Theory and a Model for Gases<br />
Kinetic energy 1 refers to the energy of an object because of its motion. Kinetic theory 2 states that all matter<br />
consists of particles in constant motion. There are a few fundamentals about gasses. 1.) The particles in<br />
gasses are typically considered to be small hard spheres with insignificant volume. The empty space<br />
between these particles is vast (on a molecular level; compared to liquids and solids) and they are not<br />
attracted or repulsed. 2.) The motion of these particles are rapid, constant, but unpredictable. For this<br />
reason, gasses fill the volume of the container they are put in. This is a property unique to gasses. Liquids will<br />
take the shape of their containers, but depending on the mass, they won’t necessarily expand to the entire<br />
container. Solids of course, don’t take the shape or volume of their containers. If gasses don’t have a<br />
container, then they can expand into vast areas (like the air). Anyways, Gas particles are also constantly<br />
colliding with other particles and objects as well. 3.) All collisions between particles in gas are elastic. What<br />
this basically means is that during collisions, kinetic energy is passed from particle to particle without any loss.<br />
Gas Pressure<br />
Gas pressure 3 is a result of the force (per unit surface area of an object) by billions of individual<br />
particles colliding with each other or other objects. On an individual basis, this does not create this<br />
much force, the scale of billions create this pressure. On the other hand, a Vacuum 4 is an empty<br />
space with no particles and no pressure. In vacuum cleaners, the partial vacuum utilizes differences<br />
in air pressure to create a vacuum. Low air pressure sucked up with suction interacts with high<br />
pressure in the vacuum bag to create a partial vacuum. Anyways, atmospheric pressure 5 is the result<br />
of molecules in air colliding with objects. A barometer 6 is used to measure atmospheric pressure. It<br />
uses mercury. The SI unit of pressure is the pascal 7 . One standard atmosphere (atm) 8 is the pressure<br />
required to support 760 mm of mercury in a barometer.<br />
Kinetic Energy and Temperature<br />
Particles in any given substance have varying kinetic energies. Regardless of temperature or physical<br />
state, particles have the same average kinetic energy. The average kinetic energy of a particle is<br />
directly correlated to the temperature. As temperature rises, there is an increase in avg. kinetic<br />
energy and vice versa. As there is a decrease in avg. kinetic energy, the substance cools, and vice<br />
versa. That’s why since ice is cold, the particles in the water would slow down and and turn it into a<br />
solid. When water is heated up, the particles pick up the pace and turn into steam: a gas.<br />
13.2 The Nature of Liquids<br />
A Model of Liquids<br />
The property gases and liquids have to flow allows them to adopt the shape of their container. While<br />
gas particles are not attracted to each other, the particles in liquids are. The intermolecular attraction
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