Exploring the Nature of Matter and Its Unique Physical Properties

Matter is anything that has mass and occupies space. Everything around us—air, water, rocks, plants, and even our bodies—is made up of matter. It exists in different states such as solid, liquid, gas, and plasma. Matter is made up of tiny particles called atoms and molecules, and it can change its form through physical or chemical processes.

1. •recognize that substances are
made up of smaller particles
•describe and/or make a
representation of the
arrangement, relative spacing,
and relative motion of the
particles in each of the three
phases of matter
LEARNING COMPETENCIES:

2. CHEMISTRY
•It is the study of matter, it’s
composition, it’s structure, it’s
properties, its transformation from
one form to another and the energy
that accompanies it’s transformation.

3. 5 Branches of Chemistry

4. Organic Chemistry
•Organic Chemistry is the study of
compounds that contain
the elements carbon and hydrogen.
–Petroleum
–Almost all medicine
–Food
•The organic chemist would take a sample of
scat and test it (NMR and IR tests) to see if
the animal was a vegetarian or carnivore
based on the various degraded foods present
in the scat.

5. Inorganic Chemistry
•The study of compounds that are made
of only one or no carbon elements.
–What we’ll focus on in Chem IB
–Most of what is not alive falls under this
category
•The inorganic chemist would take a
sample of scat and figure out if it is an acid
(like vinegar) or a base (like lye) by
dropping into a pH indicator liquid.

6. Physical Chemistry
•Chemistry that relies on a lot of physics
and math to study the changes in
energy that happen to matter.
–The study of the shape of non-living matter
and how that affects matter at the visible
scale.
•The physical chemist might take the
results that the organic chemist found
and get more information about the
degraded food. The physical chemist
would not touch the scat!

7. Analytical Chemistry
•Chemistry that detects & identifies if a
substance is present in a sample (qualitative
analysis) and how much is there
(quantitative analysis).
–CSI folk
–Determine if a white powder is cocaine or just
sugar.

•The analytical chemist would take a sample
of scat and calculate if the animal was
drinking clean or polluted water based on
the levels of pollution chemicals in the feces.
This chemist would also tell you the
quantities of everything that is in the scat.

8. Biochemistry
•Chemistry that deals with chemical
processes in living organisms.
–The study of digestion
–The study of bugs
–The study of cancer
•A biochemist would take a sample of scat and
test it to see if the animal was infected with any
kinds of worms or other intestinal parasites.
This chemist would also tell you how well the
animal was digesting his food.

13. atoms
molecules ions
the
smallest
particle
composed of
atoms
particles
with
charges

14. solid liquid gas
illustrate how the particles are distributed or arranged in each state of matter
using circles.

15. a. How separated are the
particles in each state of
matter?
b. How free are the
particles to move in each
state of matter?

16. classify the following
substances according to the
three states of matter:
a. Iron nail
b. Sugar
c. Syrup
d. Air
e. Ice
f. Alcohol
a. Solid
b. Solid
c. Liquid
d. Gas
e. Solid
f. Liquid

17. Matter

18. What is matter?
•Matter is everything around you, including you!
•Matter is what all things are made of.

19. Anything that occupies Anything that occupies
space and has massspace and has mass
MatterMatter

20. MassMass
•A measure of how much
matter is in an object.

21. WeightWeight
•A measure of the force of
gravity on an object.

22. VolumeVolume
•The amount of space that
matter occupies.

23. DensityDensity
•The measurement of how
much mass of a substance is
contained in a given volume.
•Mass/Volume

24. Freezing pointFreezing point
•The temperature at which
a liquid changes into a
solid.

25. Boiling pointBoiling point
•The boiling point of an
element or compound
means the temperature
at which the liquid form
of an element or
compound is at
equilibrium with the
gaseous form.
•the boiling point of water
is 100 degrees Celsius.

26. Melting pointMelting point
•The temperatures
at which the solid
form of the
element or
compound is at
equilibrium with
the liquid form.
•Basically the range
at which the solid
changes its state
into a liquid.
•The melting point of water is 0 degrees
Celsius

29. States of Matter
1. Solid
2. Liquid
3. Gas

30. These states of matter have
very different properties, or
ways they behave and appear.
Scientists use a model to
explain these different
properties called the particle
model.

31. According to the particle model:
• all substances are made up
of tiny particles.
• the particles are attracted
towards other surrounding
particles;
• the particles are always
moving;
• the hotter the substance
is the faster the particles
move. Soli d
Liquid
Gas

32. Solids
•A solid has its own
shape.
•A solid does not
change unless you
cut, bend, or break it.
•Solids take up space
and have mass.

34. Liquids
•Liquids do not have
their own shape.
•Liquids take the
shape of their
container.
•Liquids take up space
and have mass.

36. Gases
•Gases have no definite
size or shape.
•Gases take the shape of
its container.
•A gas will fill all the space
inside a container.
•Gases take up space and
have mass.

37. Water is matter.
Did you know it comes in all 3 forms?
A Solid A Liquid A Gas
ice water vaporwater

38. STATES OF MATTER
PLASMA
A plasma is an
ionized gas.
A plasma is a very
good conductor of
electricity and is
affected by
magnetic fields.
Plasmas, like gases
have an indefinite
shape and an
indefinite volume.
• Plasma is the
common state
of matter

39. Some places where plasmas are found…
1. Flames

40. 2. Lightning

41. 3. Aurora (Northern Lights)

42. The Sun is an example of a star in its
plasma state

43. Modern States

44. Modern States
•Bose–Einstein condensate: a phase in which a large number
of
 
bosons 
all inhabit the same 
quantum state, in effect
becoming one single wave/particle. This is a low energy
phase that can only be formed in laboratory conditions and in
very cold temperatures. It must be close to zero Kelvin, or
absolute zero.
 
Satyendra Bose 
and 
Albert Einsteinpredicted
the existence of such a state in the 1920s, but it was not
observed until 1995 by
 
Eric Cornell 
and 
Carl Wieman.
•Fermionic condensate: Similar to the Bose–Einstein
condensate but composed of
 
fermions, also known as Fermi-
Dirac condensate. The
 
Pauli exclusion principle 
prevents
fermions from entering the same quantum state, but a pair of
fermions can behave as a boson, and multiple such pairs can
then enter the same quantum state without restriction.

45. Modern States
•Excitonium
•Degenerate matter: matter under very high pressure, supported by the
 
Pauli exclusion principle.
–Electron-degenerate matter: found inside
 
white dwarf 
stars.
Electrons remain bound to atoms but are able to transfer to adjacent
atoms.
–Neutron-degenerate matter: found in
 
neutron stars. Vast
gravitational pressure compresses atoms so strongly that the
electrons are forced to combine with protons via inverse beta-decay,
resulting in a superdense conglomeration of neutrons. (Normally
 
free neutrons 
outside an atomic nucleus will 
decay 
with a half life of
just under 15 minutes, but in a neutron star, as in the nucleus of an
atom, other effects stabilize the neutrons.)
–Strange matter: A type of
 
quark matter 
that may exist inside some
neutron stars close to the
 
Tolman–Oppenheimer–Volkoff limit
 
(approximately 2–3 
solar masses). May be stable at lower energy
states once formed.

46. Modern States
•Photonic matter: Inside a quantum nonlinear
medium, photons can behave as if they had
mass, and can interact with each other, forming
photonic "molecules".
•Quantum: A state that gives rise to quantized
 
Hall voltage 
measured in the direction
perpendicular to the current flow.
–Quantum spin Hall state: a theoretical phase that may
pave the way for the development of electronic
devices that dissipate less energy and generate less
heat. This is a derivation of the quantum Hall state of
matter.

47. Modern States
•Superconductivity: is a phenomenon of exactly zero
 
electrical resistance 
and expulsion of 
magnetic fields
 
occurring in certain materials when 
cooled 
below a
characteristic
 
critical temperature. Superconductivity is
the ground state of many elemental metals.
•Superfluid: A phase achieved by a few
 
cryogenic 
liquids
at extreme temperature where they become able to flow
without
 
friction. A superfluid can flow up the side of an
open container and down the outside. Placing a
superfluid in a spinning container will result in
 
quantized vortices.
•Supersolid: similar to a superfluid, a supersolid is able to
move without friction but retains a rigid shape.

48. Modern States
•Quantum spin liquid: A disordered state in a system of interacting
quantum spins which preserves its disorder to very low
temperatures, unlike other disordered states.
•Heavy fermion materials:
 
Heavy fermion materials 
or strongly
correlated Fermi systems form a new state of matter that defines by
 
quantum phase transitions, and exhibits a universal
 
scaling 
behavior
of its
 
thermodynamic,
 
transport 
and 
relaxation 
properties. 
Quantum spin liquid,
 
quasicrystals, 2D
 
Fermi liquids,
 
heavy-fermion
 
metals and 
heavy-fermion superconductors 
can belong to the new
state of matter.
•String-net liquid: Atoms in this state have apparently unstable
arrangement, like a liquid, but are still consistent in overall pattern,
like a solid.
•Supercritical fluid: At sufficiently high temperatures and pressures
the distinction between liquid and gas disappears.

49. Modern States
•Dropleton: An artificial
 
quasiparticle, constituting a
collection of electrons and places without them inside a
semiconductor. Dropleton is the first known quasiparticle
that behaves like a liquid.
•Jahn–Teller metal: A solid that exhibits many of the
characteristics of an insulator, but acts as a conductor
due to a distorted crystalline structure. (The experiment
was not reproduced and confirmed by other scientists.)
•Time crystals: A state of matter where an object can
have movement even at their lowest energy state.
•Rydberg polaron: A state of matter that can only exist
at ultra-cool temperatures and consists of atoms inside
of atoms.

50. Very high energy
•Quark–gluon plasma: A phase in which
 
quarks 
become free and
able to move independently (rather than being perpetually bound
into particles, or bound to each other in a quantum lock where
exerting force adds energy and eventually solidifies into another
quark) in a sea of
 
gluons 
(subatomic particles that transmit
the
 
strong force 
that binds quarks together). May be briefly
attainable in
 
particle accelerators.
–For up to 10
−36
 
seconds after it , the energy density of the
universe was so high that the
 
four forces of
nature 
— 
strong,
 
weak,
 
electromagnetic, and
 
gravitational 
— are
thought to have been unified into one single force. The state of
matter in this time is unknown. As the universe expanded, the
temperature and density dropped and the gravitational force
separated, which is a process called
 
symmetry breaking.
–For up to 10
−12
 
seconds after the 
Big Bang, most scientists think
that the strong, weak and electromagnetic forces were unified.
The state of matter in this time is unknown.

51. Lesson 2
Properties of
Matter

52. Matter has certain properties.
•Matter can have color.
•Matter can be different sizes.
•Matter can have different shapes.
•Matter can have texture.
•Matter can be rigid or bendable.
•Matter also takes up space
and has mass.
Properties are the characteristics of
matter, how something looks or feels.

53. We can group objects by their properties.
How can we group these objects?

54. 1.Did you sort them by color?
One property is color.
Color
Red
Green
Yellow

55. Size
Large objects
Small objects
2. Did you sort them by size?
A second property is size.

56. Circles
Squares
Triangles
3. Did you sort them by shape?
A third property is shape.
Shape

57. We can group objects if they are
rigid or bendable.
•Bendable means that the matter can
bend, curve, or turn.
•Rigid means that the matter cannot bend,
it is stiff.
•Can you name something
that is rigid and something
that is bendable?

58. Which objects are rigid?
Which objects are bendable?

59. These objects
are rigid.
These objects
are bendable.

60. Centimeter
•Centimeter is a unit used to measure
length.
•Milliliter is a unit used to measure volume
of a liquid.

61. All substances have properties…All substances have properties…
Including people!Including people!
Example:
People can be
identified by
their …
Face
(shape,
expressions)
Voice Height Finger
prints
Eye colorHair colorTeeth DNA

62. Physical
Properties
Chemical
Properties
Extensive
Properties
Intensive
Properties

63. What are properties?
•Matter has observable and measurable
qualities.
•We can use general properties to identify
substances.
•Two basic types of properties of matter:
Physical properties and Chemical
properties:

64. answer the following questions:
•a. What is the
difference
between physical
properties and
chemical
properties?
•b. How do the
extensive
properties differ
from the intensive
properties?

65. Physical PropertiesPhysical Properties
•Physical properties are used to identify,
describe and classify matter.
–Characteristic of a substance that can be
observed (using your senses) without changing
the substance into something else.
Hardness Texture Color
Odor Taste Temperature

66. More EXAMPLES -
Physical
•size, shape, freezing point, boiling
point, melting point, magnetism,
viscosity, density, luster and many
more.
–Viscosity - The resistance of a liquid to
flowing.
–Examples:
–Low viscosity-water, rubbing alcohol
–High viscosity-honey

67. Chemical Properties
•Chemical properties are characteristics
involved when a substance interacts
with another substance to change its
chemical make-up.
Flammability Rusting Creating gas
bubbles
Creating a
new chemical
product
Reactivity with
water
pH

68. •Physical and chemical properties may
be intensive or extensive.

69. •Intensive properties such as density,
color, and boiling point do not depend on
the size of the sample of matter and can
be used to identify substances.

70. •Extensive properties such as mass and
volume do depend on the quantity of the
sample.

71. classify the following examples
as physical or chemical
properties:
•a. Melting of ice
•b. Evaporation of
water
•c. Rusting
•d. Digestion
a. Physical property
b. Physical property
c. Chemical property
d. Chemical property

72. classify the following examples
as intensive or extensive
properties:
•a. Boiling point
•b. Weight
•c. Volume
•d. Density
a. Intensive property
b. Extensive property
c. Extensive property
d. Intensive property