2. • People describe objects in many ways
using size, shape, colors, and textures.
Describing objects by using
> size
> shape
> color
> texture

3. • A property describes how an object
looks, feels, or acts

4. Properties of all objects
• Objects take up space.
• All objects take up space. Your computer is taking up space on the desk.
You are taking up space on the chair.
• Objects have mass.
• Mass is how much there is of an object.. Mass and weight are two different
things. The unit for mass is a gram. A nickel has the mass of about one
gram.
• Objects that take up space and have mass are called matter. Everything
around you is made up of matter.
• If you are having trouble understanding matter, look all around you. You can
see matter makes up the walls of your house and your classroom. Matter is
large and matter is small. Do you get it yet?

5. • . Anything you see and can feel is made of atoms.
• All atoms are too small to be seen with the naked eye or
even a microscope, although there are some new types
of microscopes that are now able to see larger atoms
such as gold.
• All matter is the same because all matter is made up of
atoms. Matter is also different because objects can be
made up of different kinds of atoms.
• Gold is made of one kind of atom-gold atoms. Salt is
made up of two different kinds of atoms-sodium atoms
and chloride atoms.

6. Properties of Matter
• Remember all objects take up space and have mass. You use your sense
of taste and smell to tell the difference between spinach and an orange.
• Physical properties- The measurement of mass and other
characteristics that can be seen without changing how that object
looks are its physical properties.
• Mass, color, shape, volume, and density are some physical properties. The
answers to the question about the present are physical properties.
• Density is an important physical property. Density is the mass of a
substance per unit volume. Volume is the amount of space an object
occupies.
• Chemical properties- These are properties that can only be observed
by changing the identity of the substance. A piece of paper burns and
turns to a black substance. After the flame goes out you can no longer
burn the new substance. The chemical properties have been changed.

7. Intensive
– Intensive - Properties that do not depend on
the amount of the matter present.
• Color
• Odor
• Luster - How shiny a substance is.
• Malleability - The ability of a substance to be
beaten into thin sheets.
• Ductility - The ability of a substance to be drawn
into thin wires.

8. • Conductivity - The ability of a substance to allow
the flow of energy or electricity.
• Hardness - How easily a substance can be
scratched.
• Melting/Freezing Point - The temperature at
which the solid and liquid phases of a substance
are in equilibrium at atmospheric pressure.
• Boiling Point - The temperature at which the
vapor pressure of a liquid is equal to the pressure
on the liquid (generally atmospheric pressure).
• Density - The mass of a substance divided by its
volume

9. Extensive
Extensive - Properties that do depend on
the amount of matter present.
• Mass - A measurement of the amount of
matter in a object (grams).
• Weight - A measurement of the
gravitational force of attraction of the earth
acting on an object.
• Volume - A measurement of the amount of
space a substance occupies.
• Length

10. Chemical Property
• Cannot be determined apart from
Chemical reaction

11. gas liquid solid
assumes the shape and assumes the shape of retains a fixed volume
volume of its container the part of the container and shape
particles can move past which it occupies rigid - particles locked
one another particles can move/slide into place
past one another
compressible not easily compressible not easily compressible
lots of free space little free space between little free space between
between particles particles particles
flows easily flows easily does not flow easily
particles can move past particles can move/slide rigid - particles cannot
one another past one another move/slide past one
another

12. Solids
• A substance in a solid phase is relatively
rigid, has a definite volume and shape.
• The atoms or molecules that comprise a
solid are packed close together and are
not compressible.
• Because all solids have some thermal
energy, its atoms do vibrate. However, this
movement is very small and very rapid,
and cannot be observed under ordinary
conditions.

13. Kinds of Solids
• Amorphous solids
Amorphous solids do not have a definite melting point or
regular repeating units. An amorphous solid is a solid in
which there is no long-range order of the positions of the
atoms unlike those in crystalline solids. An example of
an amorphous solid is window glass. In addition many
polymers such as polystyrene are amorphous.
• Amorphous solids can exist in two distinct states, the
'rubbery' state and the 'glassy' state. The temperature at
which they transition between the glassy and rubbery
states is called their glass transition temperature or Tg.

14. Liquids
• Liquids have a definite volume, but are
able to change their shape by flowing.
• Liquids are similar to solids in that the
particles touch. However the particles are
able to move around.
• Since particles are able to touch, the
densities of liquid will be close to that of a
solid.
• Since the liquid molecules can move, they
will take the shape of their container.

15. Properties of liquids
• Viscosity --The resistance of a liquid to flow is called its
viscosity
• Surface Tension -- The result of attraction between
molecules of a liquid which causes the surface of the
liquid to act as a thin elastic film under tension. Surface
tension causes water to form spherical drops.
• Vapor Pressure -- The pressure that a solid or liquid
exerts when it is in equilibrium with its vapor at a given
temperature.
• Boiling Point -- when vapor pressure = atmospheric
pressure.

16. Gases
• Gases have no definite volume or shape.
If unconstrained gases will spread out
indefinitely.
• If confined they will take the shape of their
container. This is because gas particle
have enough energy to overcome
attractive forces. Each of the particles are
well separated resulting in a very low
density.

17. Plasma
• Plasma is an ionized gas, a gas into which sufficient energy is
provided to free electrons from atoms or molecules and to allow both
species, ions and electrons, to coexist.
• In effect a plasma is a cloud of protons, neutrons and electrons
where all the electrons have come loose from their respective
molecules and atoms, giving the plasma the ability to act as a whole
rather than as a bunch of atoms.

18. • Plasmas are the most common state of matter in the
universe comprising more than 99% of our visible
universe and most of that not visible. Plasma occurs
naturally and makes up the stuff of our sun, the core of
stars and occurs in quasars, x-ray beam emitting
pulsars, and supernovas.
• On earth, plasma is naturally occurring in flames,
lightning and the auroras. Most space plasmas have a
very low density, for example the Solar Wind which
averages only 10 particles per cubic-cm. Inter-particle
collisions are unlikely - hence these plasmas are termed
collisionless.

19. Bose- Einstein Condesates
• The collapse of the atoms into a single quantum state is known as Bose
condensation or Bose-Einstein condensation is now considered a 5th state
of matter.
• Recently, scientists have discovered the Bose-Einstein condensate, which
can be thought of as the opposite of a plasma. It occurs at ultra-low
temperature, close to the point that the atoms are not moving at all.
• A Bose-Einstein condensate is a gaseous superfluid phase formed by
atoms cooled to temperatures very near to absolute zero. The first such
condensate was produced by Eric Cornell and Carl Wieman in 1995 at the
University of Colorado at Boulder, using a gas of rubidium atoms cooled to
170 nanokelvins (nK). --Under such conditions, a large fraction of the atoms
collapse into the lowest quantum state, producing a superfluid. This
phenomenon was predicted in the 1920s by Satyendra Nath Bose and
Albert Einstein, based on Bose's work on the statistical mechanics of
photons, which was then formalized and generalized by Einstein.

20. States of Matter
• States of matter are the distinct forms that different phases of matter take on. Three states of matter are known in everyday
experience: solid, liquid, and gas. Other states are possible; in scientific work, the plasma state is important. Further states are
possible but do not normally occur in our environment: Bose-Einstein condensates, neutron stars. Other states, such as quark-
gluon plasmas, are believed to be possible. Much of the baryonic matter of the universe is in the form of hot plasma, both as
rarefied interstellar medium and as dense stars.
• Historically, the distinction is made based on qualitative differences in bulk properties. Solid is the state in which matter maintains
a fixed volume and shape; liquid is the state in which matter maintains a volume which can vary only slightly, but adapts to the
shape of its container; and gas is the state in which matter expands to occupy whatever volume is available.
• This diagram shows the nomenclature for the different phase transitions.
• The state or phase of a given set of matter can change depending on pressure and temperature conditions, transitioning to other
phases as these conditions change to favor their existence; for example, solid transitions to liquid with an increase in temperature.
• A state of matter is also characterised by phase transitions. A phase transition indicates a change in structure and can be
recognized by an abrupt change in properties. A distinct state of matter can be defined as any set of states distinguished from any
other set of states by a phase transition. Water can be said to have several distinct solid states.[1] The appearance of
superconductivity is associated with a phase transition, so there are superconductive states. Likewise, ferromagnetic states are
demarcated by phase transitions and have distinctive properties. When the change of state occurs in stages the intermediate
steps are called mesophases. Such phases have been exploited by the introduction of liquid crystal technology.
• More recently, distinctions between states have been based on differences in molecular interrelationships. Solid is the state in
which intermolecular attractions keep the molecules in fixed spatial relationships. Liquid is the state in which intermolecular
attractions keep molecules in proximity, but do not keep the molecules in fixed relationships. Gas is the state in which molecules
are comparatively separated and intermolecular attractions have relatively little effect on their respective motions. Plasma is a
highly ionized gas that occurs at high temperatures. The intermolecular forces created by ionic attractions and repulsions give
these compositions distinct properties, for which reason plasma is described as a fourth state of matter.[2][3]
• Forms of matter that are not composed of molecules and are organized by different forces can also be considered different states
of matter. Superfluids (like Fermionic condensate) and the quark–gluon plasma are examples.

22. • Solid
• A crystalline solid: atomic resolution image of strontium titanate. Brighter atoms are Sr and darker
ones are Ti.
• Main article: Solid
• The particles (ions, atoms or molecules) are packed closely together. The forces between
particles are strong enough so that the particles cannot move freely but can only vibrate. As a
result, a solid has a stable, definite shape, and a definite volume. Solids can only change their
shape by force, as when broken or cut.
• In crystalline solids, the particles (atoms, molecules, or ions) are packed in a regularly
ordered, repeating pattern. There are many different crystal structures, and the same substance
can have more than one structure (or solid phase). For example, iron has a body-centred cubic
structure at temperatures below 912 C, and a face-centred cubic structure between 912 and
1394 C. Ice has fifteen known crystal structures, or fifteen solid phases, which exist at various
temperatures and pressures.[4]
• Glasses and other non-crystalline, amorphous solids without long-range order are not thermal
equilibrium ground states; therefore they are described below as nonclassical states of matter.
• Solids can be transformed into liquids by melting, and liquids can be transformed into solids by
freezing. Solids can also change directly into gases through the process of sublimation.

23. • Liquid
• Structure of a classical monatomic liquid. Atoms have many nearest neighbors in contact, yet no long-range order is present.
•
• Main article: Liquid
• A liquid is a nearly incompressible fluid that conforms to the shape of its container but retains a (nearly) constant volume independent of
pressure. The volume is definite if the temperature and pressure are constant. When a solid is heated above its melting point, it becomes
liquid, given that the pressure is higher than the triple point of the substance. Intermolecular (or interatomic or interionic) forces are still
important, but the molecules have enough energy to move relative to each other and the structure is mobile. This means that the shape of
a liquid is not definite but is determined by its container. The volume is usually greater than that of the corresponding solid, the most well
known exception being water, H2O. The highest temperature at which a given liquid can exist is its critical temperature.[5]
• Gas
• The spaces between gas molecules are very big. Gas molecules have very weak or no bonds at all. The molecules in "gas" can move
freely and fast.
• Main article: Gas
• A gas is a compressible fluid. Not only will a gas conform to the shape of its container but it will also expand to fill the container.
• In a gas, the molecules have enough kinetic energy so that the effect of intermolecular forces is small (or zero for an ideal gas), and the
typical distance between neighboring molecules is much greater than the molecular size. A gas has no definite shape or volume, but
occupies the entire container in which it is confined. A liquid may be converted to a gas by heating at constant pressure to the boiling
point, or else by reducing the pressure at constant temperature.
• At temperatures below its critical temperature, a gas is also called a vapor, and can be liquefied by compression alone without cooling. A
vapor can exist in equilibrium with a liquid (or solid), in which case the gas pressure equals the vapor pressure of the liquid (or solid).
• A supercritical fluid (SCF) is a gas whose temperature and pressure are above the critical temperature and critical pressure respectively.
In this state, the distinction between liquid and gas disappears. A supercritical fluid has the physical properties of a gas, but its high
density confers solvent properties in some cases, which leads to useful applications. For example, supercritical carbon dioxide is used to
extract caffeine in the manufacture of decaffeinated coffee.[6]
• State Symbols

24. • Plasma (ionized gas)
• Main article: Plasma (physics)
• Plasmas or ionized gases can exist at temperatures starting at several thousand degrees
Celsius, where they consist of free charged particles, usually in equal numbers, such as ions and
electrons. Plasma, like gas, is a state of matter that does not have definite shape or volume.
Unlike gases, plasmas may self-generate magnetic fields and electric currents, and respond
strongly and collectively to electromagnetic forces. The particles that make up plasmas have
electric charges, so plasma can conduct electricity. Two examples of plasma are the charged air
produced by lightning, and a star such as our own sun.
• As a gas is heated, electrons begin to leave the atoms, resulting in the presence of free
electrons, which are not bound to nuclei, and ions, which are chemical species that contain
unequal number of electrons and protons, and therefore possess an electrical charge. The free
electric charges make the plasma electrically conductive so that it responds strongly to
electromagnetic fields. At very high temperatures, such as those present in stars, it is assumed
that essentially all electrons are "free," and that a very high-energy plasma is essentially bare
nuclei swimming in a sea of electrons. Plasma is the most common state of non-dark matter in the
universe.
• A plasma can be considered as a gas of highly ionized particles, but the powerful interionic forces
lead to distinctly different properties, so that it is usually considered as a different phase or state of
matter.