This document discusses the three states of matter - solids, liquids, and gases. It describes their characteristic properties, including the arrangement and movement of particles in each state. Key concepts covered include kinetic theory, vapor pressure, boiling point, phase changes, allotropes, and triple points. The document provides definitions and explanations of these essential concepts relating to states of matter and phase changes.

1. Chapter 13
States of Matter and Changes

2. Solid Liquid Gas
Mass Definite
Shape
Indefinite
shape
Indefinite
shape
Volume Definite Definite indefinite
Particles Vibrate in
place
Strong
bonds
Can flow
Loose
bonds
No bonds

3. 13.1 The Nature of Gases
• The word kinetic refers to
motion.
• The energy an object has
because of motion is
called kinetic energy.

4. Kinetic Theory
• 1. The particles in a gas are
considered to be small, hard
spheres with an insignificant
volume.
• 2. The motion of the particles in
a gas is rapid, constant and
random.
• 3. All collision between particles
in a gas are perfectly elastic.

5. 1
• Particles are far apart.
• Between the particles there
is empty space.
• Motion is independent.
• No attractive or repulsive
forces are present.

6. 2•
Gases fill their container
regardless of their shape.
• Uncontained gases can
spread without limit.
• Particles only change
direction when rebounding
off objects.
• Particles move at random.

7. 3•
Kinetic energy is
transferred without
loss from one particle
to another.
•Total kinetic energy
remains constant.

9. Gas Pressure
• Gas pressure results from the force
exerted by a gas per unit surface area of
an object.
• Gas pressure is a result of simultaneous
collisions of billions of rapidly moving
particles in a gas with an object.
• An empty space with no particles and no
pressure is called a vacuum.
• Atmospheric pressure results from the
collisions of atoms and molecules in the air
with objects.
• A barometer is device that is used to
measure atmospheric pressure.

12. MATH MONKEY MOMENT
1 atm=760 mm Hg= 101.3
Practicek cPoanverting units
of pressure.
What pressure, in
kilopascals and in
atmospheres, does a gas
exert at 385 mm Hg?
The pressure at the top of
Mount Everest is 33.7 kPa.
Is that pressure greater or
less than .25 atm?
Pg. 387

13. Can you convert easily? Or did I just pull your tail 1. 51.3 kPa, .507
atm 2. 33.7 kPa is greater than .25 atm.

14. Vocabulary Cards
• Definite
• Indefinite
• Uniform
• Kinetic energy
• Gas pressure

15. SUM IT UP- What’s
happening in this clip on
the next slide?

17. Kinetic Energy and
Temperature
• As a substance is heated, its particles
absorb energy.
• Some gets stored in the particles as
potential energy.
• The rest of the energy speeds up the
particles thus increasing their kinetic
energy.
• Average kinetic energy is the
measurement of kinetic energy for a
substance regardless of physical state.

19. Kinetic Energy and
Temperature
• Absolute zero is the theoretical point
at which all motion stops and kinetic
energy is zero.
• It has never been produced in a
laboratory but scientists have come
close in a vacuum.
• The Kelvin temperature of a
substance is directly proportional to
the average kinetic energy of the
particles of the substance.

20. 13.2 The Nature of Liquids
• Particles in liquids have kinetic energy
like a gas.
• Substances that flow are referred to as
liquids.
• The key difference between liquids and
gases, is that liquids have attractions
between the particles and gases don’t.
• The interplay between the disruptive
motions of particles in a liquid and the
attractions among the particles
determine the physical properties of
liquids.

21. Evaporation
• The conversion of a liquid to a gas is
called vaporization.
• When the conversion occurs at the
surface of a liquid that is not boiling, it is
called evaporation.
• Most of the molecules in a liquid don’t
have enough kinetic energy to overcome
attractive forces and escape into a
gaseous state.
• During evaporation, only those molecules
with a certain minimum kinetic energy
can escape the surface of the liquid.

23. Vapor Pressure
• Vapor Pressure is a measure of the force
exerted by a gas above a liquid.
• Over time, the number of particles entering
the vapor increases and some of the
particles condense back into a liquid.
• In a system at constant vapor pressure, a
dynamic equilibrium exists between the
rate of evaporation and the rate of
condensation.
• An increase in the temperature of the liquid
increases the vapor pressure.

24. • Animation

25. Boiling Point
• The rate of evaporation of a liquid from an
open container increases as the liquid is
heated.
• When a liquid is heated to a temperature
at which particles throughout the liquid
have enough kinetic energy to vaporize,
the liquid begins to boil.
• The temperature at which the vapor
pressure of the liquid is just equal to the
external pressure on the liquid is the
boiling point.

26. Vapor pressure less than
atmospheric pressure
Vapor pressure more than
atmospheric pressure

27. Boiling Point and Pressure
Changes
• Liquids don’t always boil at the same
temperature all the time.
• Change in altitude affects the boiling
point.
• Higher altitudes decrease boiling
point.
• Lower altitudes (under water)
increase boiling points.
• Normal boiling point is at standard
pressure of 101.3 kPa.

28. Vocabulary Cards
• Potential energy
• Average kinetic energy
• Evaporation
• Vaporization
• Vapor pressure
• Equilibrium
• Boiling point

29. POST IT UP
When will a liquid evaporate?
I GOT THIS!
I NEED HELP!

30. 13.3 The Nature of Solids
• The general properties of solids reflect
the orderly arrangement of their particles
and the fixed locations of their particles.
• When you heat a solid, its particles
vibrate more rapidly as their kinetic
energy increases.
• The melting point is the temperature at
which a solid changes into a liquid.
• The melting and freezing points are at the
same temperatures and the solid and
liquid phases are in equilibrium.

32. Allotropes
• Some solid substances can exist in
more than one form.
• Allotropes are two or more different
molecular forms of the same
element in the same physical state.
• Carbon is one example.
• Carbon can exist as a diamond,
graphite and as fullerene.

34. 8 allotropes of carbon

35. 13.4 Changes of State
• Sublimation occurs in solids with vapor
pressures that exceed atmospheric
pressure at or near room temperature.
• Examples are iodine and carbon dioxide.
• A phase diagram is a visual
representation of boiling, melting and
triple points.
• The triple point is a point in which all three
states of matter exist at one time.
• Boiling and melting points vary with
atmospheric pressure.

38. Science Swag

39. Science Swag
• Research an allotrope of carbon.
• You may choose any type.
• Write a one page type I paper about
your research.
• Things you could include: examples,
pictures, experiments, history,
discoveries, past/present/future of
allotropes……..etc etc…

40. POST IT UP
What is the triple point?
I GOT THIS!
I NEED HELP!