1. Matter

2. Matter vs. Energy The universe is made up of matter and energy.
Has mass and takes up space (volume)
Is usually a “thing”
Energy:
Does not have mass or take up space
Energy moves matter!!!!!!
** Energy is the ability to make things move. Light, heat, sound, motion, and electricity are all forms of energy.

3. Properties of Matter All matter has characteristics, or properties
These properties can either be:
Chemical
Physical

4. Physical Properties
Physical property- any property of matter that can be observed or measured without changing the identity of the matter
Examples
color
shape
taste
density
state/phase
malleability
D = M V

5. Volume and Density Volume= length X width X height Density= mass (g)
volume (mL or cm3)
1 mL = 1 cm3
Which is more dense?

7. Physical Properties States of matter: Bose-Einstein Solid Liquid Gas
Plasma
(Newest State)

8. Bose-Einstein Condensate
Exist at extremely cold temperatures (around absolute zero or -460 oF)
Particles are super unexcited
Particles lock or “clump” together so firmly that they move as a single unit

9. Solid Particles are tightly compact
Particles vibrate without the ability to move freely
Definite shape and volume
Solid Animation

10. Liquid
Particles are tightly compact, but able to move around close to each other
No definite shape, but definite volume
Liquid Animation

11. Gas Particles can easily spread out or move close together
Particle move freely and with a lot of energy
No definite shape or volume
Gas Simulation

12. Plasma
Particles broken apart and move freely with extremely high energy
Exist at extremely high temps (several million degrees Celsius)
Not too common on earth, but the most common form of matter in the universe
Examples: Florescent and neon lights, lightning, fire
Why do you think this is the most common form/state of matter in the universe?

13. Physical Properties
Physical states of matter result from the amount of energy that the particles composing the matter have.
More energy = more movement for the particles
If you were to compare an ice cube and the steam created from boiling water, which would you think has more energy?

14. Types of Energy Potential- stored energy
Kinetic energy- energy a moving object has
Temperature-average kinetic energy of all atoms in a substance
Thermal energy- sum of both the kinetic and potential energy of the atoms of a substance

15. Physical Properties What about this states of matter continuum could
be considered a little misleading?
Taken from:

16. Changes in States (Physical Changes)
Why do you think Bose-Einstein and plasma are not equally distanced from the other three states of matter?
Plasma
Disposition
Vaporization
(Evaporation/Boiling)
Gas
Liquid
Condensation
Melting
Solid
Freezing
Sublimation
Bose-Einstein
All changes in state require a change in energy

17. Heating Curve The heating curve below shows how adding
more thermal energy results in changes in the
states of water
boiling point
melting point

18. Thermal Expansion
Thermal expansion- the increase in the size of a substance when the temperature is increased.
Hot air balloons rise due to the thermal expansion of air
Colder water will contract and sink
Density and temp
The exception of this is water because when it becomes ice it expands and floats

19. Physical Properties of Fluids
Fluid- any substance that can flow, like a liquid or gas
Buoyancy- the ability of a fluid to exert an upward force on an object immersed in it.
Archimedes principle-the buoyant force on an object is equal to the weight of the fluid displaced by that object

20. Density and Buoyancy Density= mass (g) volume (mL or cm3)
Because saltwater has the additional mass of salt in the water and is more dense, things are more buoyant in saltwater than fresh
Generally if an object is more dense than the fluid, it will sink
If an object is less dense it will float

21. Physical Properties of Fluids
Pascals principle- pressure applied to a fluid is transmitted throughout the fluid
P (Pascals)= Force (Newton)
Area (m2)
where one Pascal is a N/m2

22. Check for Understanding
As you sit here, atmospheric pressure from the air is pushing on you
If the atmospheric pressure at sea level is 101 kPa (or N/m2), and the average human’s area is 1.80 m2, with how much force does the atmosphere push on the average human?

23. Check for Understanding
As you sit here, atmospheric pressure from the air is pushing on you
If the atmospheric pressure at sea level is 101 kPa (or N/m2), and the average human’s area is 1.80 m2, with how much force does the atmosphere push on the average human?
P = F so F = PA A
F (N) = 101 kPa X 1.80 m2 = 101,000Pa X 1.80 m2
F (N) = 182,000 Pa m2 = 182,000 N

24. Physical Properties of Fluids
Bernoulli’s principle- fluid velocity increases when the flow of the fluid is restricted

25. Physical Properties of Fluids
Viscosity- the resistance of a fluid to flowing.
Maple syrup is very viscous, even more so cold than when warm
Water is not viscous at all

26. Physical Properties of Gases
Boyle’s Law- decrease the volume of a container of gas and hold the temp constant, pressure from the gas will increase
Conversely, increase the volume of a container of gas holding the temp constant, pressure from the gas will decrease

27. Boyle’s Law Boyle’s Law as an equation:
PiVi = PfVf where i=initial and f=final
If a weather balloon has a volume of 100L when it is released at sea level where the pressure is 101 kPa, what will be the balloon’s volume when it reaches an altitude where the pressure is 43 kPa?
PiVi = PfVf so = PiVi = Vf Pf
Vf = 100L X 101,000Pa = 235L
43,000 Pa

28. Check for Understanding
Boyle’s Law as an equation:
PiVi = PfVf where i=initial and f=final
If a balloon has a volume of 11L when it is released at sea level where the pressure is 101 kPa, what will be the balloon’s volume when it reaches an altitude where the pressure is 86 kPa?

29. Check for Understanding
Boyle’s Law as an equation:
PiVi = PfVf where i=initial and f=final
If a balloon has a volume of 11L when it is released at sea level where the pressure is 101 kPa, what will be the balloon’s volume when it reaches an altitude where the pressure is 86 kPa?
PiVi = PfVf so = PiVi = Vf Pf
Vf = 11L X 101,000Pa = 12.9L
86,000 Pa

30. Physical Properties of Gases
Charles’s Law- the volume of a gas increases with increasing temperature as long as the pressure on the gas is constant

31. Charles’s Law Charles’s Law as an equation:
Vi = Vf where i=initial and f=final
Ti Tf
and temperature must be measured in Kelvin
K = oC + 273
Remember:
0K is absolute zero
273K is the freezing point of water
373K is the boiling point of water

32. Charles’s Law
A 2L balloon at room temperature (20.0oC) is placed in a refrigerator at 3.0oC. What will be the balloon’s volume be after it cools?
K = oC + 273
So Ti = 293K and Tf = 276K
Vi = Vf so Vi X Tf = Vf
Ti Tf Ti
Vf = 2L X 276K = 1.89 L (it shrinks!)
293K

33. Check for Understanding
What would be the final volume if the balloon was put in a -18oC freezer?

34. Check for Understanding
What would be the final volume if the balloon was put in a -18oC freezer?
K = oC + 273
So Ti = 293K and Tf = 255K
Vi = Vf so Vi X Tf = Vf
Ti Tf Ti
Vf = 2L X 255K = 1.7 L (it shrinks smaller!)
293K

35. Physical Properties of Solids
Malleable- able to be hammered or pressed out of shape without breaking
This is a property of many metals

36. Composition of Matter All matter has a composition, what it’s made of
Different kinds of composition are:
Pure substances- type of matter with a fixed composition that can’t be separated physically
Element
Compound
Mixture- can be separated physically
Solutions
Colloids
Mechanical mixture

37. MATTER PURE SUBSTANCES (non-mixtures) MIXTURES COLLOIDS ELEMENTS
COMPOUNDS
SOLUTIONS
SUSPENSIONS
HOMOGENEOUS
MECHANICAL MIXTURES
HETEROGENEOUS

38. Pure Substances
Element- made up of one kind of atom that can’t be broken down into simpler substances by physical or chemical means
90 occur naturally on Earth
25 were synthesized (made) by scientists

39. Pure Substances
Compound- substance composed of two or more different elements (atoms) that are chemically combined
Examples:
H2O, CO2,CO, NO2,

40. characteristics of these
Mixtures
Mixtures- combination of two or more substances that do not combine chemically, but remain the same individual substances;
Can be separated by physical means
Two types:
Heterogeneous
Homogeneous
Based on the prefixes
“hetero” and “homo,”
what do you think are
characteristics of these
two types of mixtures?

41. Heterogeneous Mixtures
“Hetero” = different
Consists of visibly different substances or phases (solid, liquid, gas)
Mechanical mixture- visibly not wholly one
Example:
Notice the visibly different
substances in these mechanical mixtures
Pizza
Trail Mix

42. Heterogeneous Mixtures
Suspension- special type of heterogeneous mixture of larger particles that eventually settle

43. Heterogeneous Mixtures
Colloids- heterogeneous mixture with particles that never settle
Milk and paint
Have a foggy appearance because its particles are large enough to scatter light, unlike a solution

44. Homogeneous Mixtures “Homo” = same
Has the same uniform appearance and composition throughout; maintain one phase (solid, liquid, gas)
Commonly referred to as solutions
Example:
Notice the
uniform
appearance
Salt Water

45. Homogeneous Mixtures
Solution- a mixture of two or more substances that is identical throughout
Can be physically separated
Composed of solutes and solvents
Salt water is considered a solution. How
can it be
physically separated?
the substance in the smallest
amount and the one that dissolves in the solvent
the substance in the larger
amount that dissolves the solute
Iced Tea Mix
(solute)
Water
(solvent)
Iced Tea
(solution)
Colloids (milk, fog, jello) are considered solutions

46. Solutes Change Solvents
The amount of solute in a solution determines how much the physical properties of the solvent are changed
Examples:
Lowering the Freezing Point
Raising the Boiling Point
The freezing point of a liquid solvent
decreases when a solute is dissolved in it.
Ex. Pure water freezes at 320F (00C), but when salt is
dissolved in it, the freezing point is lowered.
This is why people use salt to melt ice.
The boiling point of a solution is higher
than the boiling point of the solvent.
Therefore, a solution can remain a liquid at
a higher temperature than its pure solvent.
Ex. The boiling point of pure water is 2120F (1000C),
but when salt is dissolved in it, the boiling
point is higher. This is why it takes salt water
longer to boil than fresh water.

47. Concentration
Concentration- the amount of solute dissolved in a solvent at a given temperature
Described as dilute if it has
a low concentration of
solute
Described as saturated if it
has a high concentration of
Described as supersaturated if
contains more dissolved solute
than normally possible

48. Solubility
The amount of solute that dissolves in a certain amount of a solvent at a given temperature and pressure to produce a saturated solution
Influenced by:
What do we call things that are not soluble?
Temperature
Pressure
Solids increased temperature causes
them to be more soluble and vice versa
Gases increased temperature causes
them to be less soluble and vice versa
Ex. Iced Coffee
Solids increased pressure has no
effect on solubility
Gases increased pressure causes them
to be more soluble and vice versa
Ex. Soda, “The Bends”

49. Chemical Properties
Chemical property- any property of matter that describes a substance based on its ability to change into a new substance
Examples
flammability
reactivity with vinegar
reactivity with oxygen
Iron + Oxygen  Iron oxide (rust)
2Fe + 3O2  Fe2O3

50. Chemical or Physical Property?
Paper is white
Boiling point of H2O is 100oC
Zinc reacts with hydrochloric acid and creates hydrogen gas
Nitrogen does not burn
Sulfur smells like rotten eggs
Physical Property
Physical Property
Chemical Property
Chemical Property
Physical Property

51. Comparing Physical and Chemical Properties
Substance/Matter
Physical Property
Chemical Property
Helium
Less dense than air
Nonflammable
Wood
Grainy texture
Flammable
Baking soda
White powder
Reacts with vinegar to produce bubbles
Powdered sugar
Does not react with vinegar
Rubbing alcohol
Clear liquid
Red food coloring
Red color
Reacts with bleach and loses color
Iron
Malleable
Reacts with oxygen

52. Changes in Matter Matter is constantly changing
There are two types of changes in matter:
Chemical
Physical

53. Physical changes are not indicative of a chemical reaction
Physical change- a change in shape, size, color, or state a change without a change in chemical composition
Examples
tearing paper
cutting your hair
change in state
Some mixtures can be separated based on their physical properties
The Mixtures Lab
Physical changes are not indicative of a chemical reaction

54. Changes in States (Physical Changes)
Why do you think Bose-Einstein and plasma are not equally distanced from the other three states of matter?
Plasma
Disposition
Vaporization
(Evaporation/Boiling)
Gas
Liquid
Condensation
Melting
Solid
Freezing
Sublimation
Bose-Einstein
All changes in state require a change in energy

55. Physical Changes Simulation 1 Simulation 2 Chemistry of Chocolate
This is what happens when energy is added and taken away

56. Chemical Changes
Chemical change- a change in which a substance becomes another substance having different properties
A change that is not reversible using ordinary physical means
Changes that usually cause, heat, sound, light, odor, fizzing/foaming, color changes
Examples
mixing vinegar & baking soda
burning a piece of wood
soured milk
A chemical analysis is the only 100% way to know a
chemical change has occurred.

57. Chemical Changes
Chemical reaction- the process by which a chemical change occurs
Types of chemical reactions
Synthesis (creating)
Decomposition (separating)
Combustion (burning)
Displacement/Replacement (switching of atoms)

58. Chemical Changes
During chemical changes, atoms are rearranged, and chemical bonds are broken and reformed
One or more substances change to produce one or more different substances
What does
H2 & O2 gas
create?
Out of the four types of reactions, which would describe the chemical reaction taking place to the right? H2 O2

59. Chemical or Physical Change?
Bending a Paper Clip
Baking a cake
The sublimation of carbon dioxide
Crushing an aluminum can
Vinegar and baking soda combining to create salt and water
Physical Change
Chemical Change
Physical Change
Physical Change
Chemical Change

60. Law of Conservation of Mass
Proposed by Antoine Lavoisier
In a chemical reaction, atoms are neither created nor destroyed
All atoms present in the reactants are also present in the products
Chemical equations must be balanced to show the conservation of mass
In its present form, does this chemical equation show a
conservation of mass? 2
H2 + O2  2
H2O
Reactants
Products
How would you balance this equation to
show the conservation of mass?
H  2
O  2 4 2
H  2
O  1 4 2