Complete Whole Notebook

The Learning Goal for this assignment is: Differentiate among the 4 states
of matter
Take note over the following chapter. Use the Headings provided to organize your notes. Define and
number all highlighted vocabulary (total 23 ) as well 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
should be 3 pages and should be saved as a pdf before you submit it into Angel.
Chapter 13 States of Matter
Pages 420 - 439
13.1 The Nature of Gases
Kinetic Theory and a Model for Gases
The energy an object has because of its motion is called
kinetic energy 1 . According to the kinetic theory 2 , all matter
consists of tiny particles that are in constant motion. The
particles in a gas are considered to be small, hard spheres with an insignificant volume. Within a gas,
the particles are relatively far apart compared with the distance between particles in a liquid or solid.
The motion of the particles in a gas is rapid, constant, and random. As a result, gases fill their
containers regardless of the shape and volume of the containers. All collisions between particles in a
gas are perfectly elastic. During an elastic collision, kinetic energy is transferred without loss from one
particle to another.
Gas Pressure
Gas pressure 3 results from the force exerted by a gas per unit surface area of an object. An empty
space with no particles and no pressure is called a vacuum 4 . The collisions of atoms and molecules
in air with objects results in atmospheric pressure 5 . A barometer 6 is a device that is used to measure
atmospheric pressure. The SI unit of pressure is the pascal(Pa) 7 . One standard atmosphere(atm) 8 is
the pressure required to support 760 mm of mercury in a mercury barometer at 25 o C. Moving bodies
exert a force when they collide with other bodies. Although a single particle in gas is a moving body,
the force it exerts is extremely small. Gas pressure is the result of billions of rapidly moving particles
in a gas simultaneously colliding with an object. If no particles are present, no collisions can occur.
Consequently, there is no pressure.
Kinetic Energy and Temperature
The particles in any collection of atoms or molecules at a given temperature have a wide range of
kinetic energies. Most of the particles have kinetic energies somewhere in the middle of this range.
Therefore, we use average kinetic energy when discussing the kinetic energy of a collection of
particles in a substance. The Kelvin temperature scale reflects the relationship between temperature
and kinetic energy. The Kelvin temperature of a substance is directly proportional to the average
kinetic energy of the particles of the substance. For example, the particle in helium gas at 200 K have
twice the average kinetic energy as the particles in helium gas at 100K. The effects of temperature on
particle motion in liquids and solids are more complex than in gases.
Pg110