1. Big Idea 8: Properties of Matter
Atomic theory, properties of matter, atoms, compounds, mixtures, & solutions

2. Benchmark Number & Descriptor
SC.8.P.8.5
Recognize that there are a finite number of elements and that their atoms combine in a multitude of ways to produce compounds that make up all of the living and nonliving things that we encounter.
SC.8.P.8.6
Recognize that elements are grouped in the periodic table according to similarities of their properties.
SC.8.P.8.7
Explore the scientific theory of atoms (also known as atomic theory) by recognizing that atoms are the smallest unit of an element and are composed of sub-atomic particles (electrons surrounding a nucleus containing protons and neutrons).
SC.8.P.8.8
Identify basic examples of and compare and classify the properties of compounds, including acids, bases, and salts.
SC.8.P.8.9
Distinguish among mixtures (including solutions) and pure substances.
Benchmark Number & Descriptor
SC.8.P.8.1
Explore the scientific theory of atoms (also known as atomic theory) by using models to explain the motion of particles in solids, liquids, and gases.
SC.8.P.8.2
Differentiate between weight and mass recognizing that weight is the amount of gravitational pull on an object and is distinct from, though proportional to, mass.
SC.8.P.8.3
Explore and describe the densities of various materials through measurement of their masses and volumes.
SC.8.P.8.4
Classify and compare substances on the basis of characteristic physical properties that can be demonstrated or measured; for example, density, thermal or electrical conductivity, solubility, magnetic properties, melting and boiling points, and know that these properties are independent of the amount of the sample.

3. MATTER Everything in the world is made up of matter.
Matter is defined as anything that takes up space and has mass.
Atoms are the building blocks of matter.
Matter can exist as solids, liquids, gases and plasma.
Matter has both physical and chemical properties.

4. SOLIDS, LIQUIDS and GASES

5. SOLIDS Characteristics: Definite shape Definite volume
Atoms are packed tightly together with very little movement.

6. LIQUIDS Characteristics: Definite volume Indefinite shape
Liquids will take the shape of the container they are in.
Atoms within a liquid are loosely packed together and have fluid movement within the container.

7. GAS Characteristics: Indefinite shape
Gases will take the shape of the container they are placed into.
Indefinite volume
Gases will spread out in order to fill their containers.
Atoms within a gas are in constant free movement. They will spread out and fill the space they are contained in.

8. Take a Look…
View this clip to see solids, liquids and gasses in action.
chool.com/activity/st ates_of_matter/

9. Don’t Forget, PLASMA Characteristics: Indefinite shape
Indefinite volume
Particles can move past one another.
Plasma consists of a sea of ions and electrons and is a very good conductor of electricity and is affected by magnetic fields.
Plasmas are heated to over 100 million degrees.

10. Knowledge Check
1. Identify and describe the particle arrangement in the state of matter that has no definite shape but does have a definite volume?
How do the particles of a gas differ from a solid?
3. Which phase consists of electrically charged particles at very high temperatures?

11. Knowledge Check
1. Identify and describe the particle arrangement in the state of matter that has no definite shape, but does have a definite volume?
Liquid; particles have some movement within their containers.
How do the particles of a gas differ from a solid?
Gas particles have much more movement. Indefinite
shape and volume
3. Which phase consists of electrically charged particles at very high temperatures?
Plasma

12. PHYSICAL vs. CHEMICAL PROPERTIES
What is the difference?

13. PHYSICAL PROPERTIES Physical Property What it Means Density
The amount of matter in a given volume
Boiling Point
The temperature at which a substance changes from a liquid to a gas
Melting Point/Freezing Point
The temperature at which a substance changes from a solid to a liquid (liquid to solid)
Solubility
The ability to dissolve in another substance
Are observed with the senses and can be determined without destroying the object.
Does not depend on how much of the substance you have – if it is the same substance it should have the same properties.

14. CHEMICAL PROPERTIES Chemical Property What it Means Flammability
A. Indicates how a substance reacts with something else
B. The original substance is changed into something new.
Chemical Property
What it Means
Flammability
The ability to burn
Reactivity
Ability to react with oxygen, acid, water, or other substances

15. Let’s Review…

16. Another Identification Method DENSITY
Amount of mass per unit volume
Density = Mass / Volume
No matter how much of a sample you have of a specific substance, the same substances will have the same densities.

17. Densities of Common Materials (computed in grams per cubic centimeter)
Water ………………………1.00
Glass………………………2.60
Granite…………………2.650
Bone……………………….1.85
Human Body………………0.995
Butter…………………….0.94
SulfuricAcid……1.840
Ice……………………0.91
Carbon………………2.60
Kerosene…………0.80
Chalk……………………2.36
Salt……………………2.20
Coal………………………1.50
Sand…………………2.80
Cork…………………0.25

18. WEIGHT vs. MASS Weight Mass
the force which a given mass feels due to the gravity at its place
Weight is measured in units of Force like Newton (which is the SI unit of Force).
The weight of an object will change due to its location (gravitational pull).
Mass
the amount of matter present in an object
Mass of an object is measured by balancing it equally with another known amount of mass.
The mass of an object does not change due to its location.

19. KNOWLEDGE CHECK Distinguish from the list below which are
physical and chemical changes.
Boiling point
Flammability
Reacts with acid
Bitter taste
Ice melting
Iron rusting
Solubility
Milk sours
Wood rots

20. KNOWLEDGE CHECK Distinguish from the list below which are
physical and chemical changes.
Boiling point - Physical
Flammability - Chemical
Reacts with acid - Chemical
Bitter taste - Physical
Ice melting - Physical
Iron rusting - Chemical
Solubility - Physical
Milk sours - Chemical
Wood rots - Chemical

21. ATOMIC THEORY
What makes up matter?

22. What’s an atom? Atoms are the building blocks for matter.
They are so small that the naked eye cannot even see one.
Atoms contain three particles.
Protons
Electrons
Neutrons

23. 3 Little Particles…

24. If we can’t see atoms, how do we know about them?
460 BCE: Democritus
Stated the smallest piece matter can be broken into was an “atom.”
From the Greek word, atomos, which means “indivisible.”
1807 : John Dalton (British chemist)
1st modern scientist to discuss the atom.
Stated that an atom was similar to a billiard ball – round, indestructible, solid sphere

25. If we can’t see atoms, how do we know about them?
1898: Sir Joseph John Thompson (British physicist)
Stated that inside an atom was a mixture of protons and electrons mixed together
His idea is referred to as the “Plum Pudding Model.”
1911: Ernest Rutherford (British physicist)
Stated that atoms are mostly empty space
Discovered the positive charged nucleus of an atom
Suggested that electrons circle the nucleus
Conducted the gold foil experiment

26. If we can’t see atoms, how do we know about them?
1913: Niels Bohr (Danish physicist)
Stated that electrons did not just randomly circle the nucleus. Instead, the circled in orbits
Each orbit contained a certain number of electrons and were located a specific distances from the nucleus.
Current Atomic Model
Based upon Bohr’s model
Orbits of electrons are referred as the electron cloud.

27. KNOWLEDGE CHECK Match each scientist to their Atomic Theory Model
Democritus A. Proposed that electrons were located throughout an atom like plums in plum pudding
John Dalton B. Atom model had electrons surrounding the nucleus at a specific distance.
J.J. Thompson C. Stated atoms were the smallest piece of matter
Ernest Rutherford D. Electrons surround the nucleus in an electron cloud.
Niels Bohr E. Atoms of the same element are alike, and atoms of different elements are different.
Current Atomic Theory F. Electrons move around the nucleus in certain paths.

28. KNOWLEDGE CHECK Match each scientist to their Atomic Theory Model
Democritus - C A. Proposed that electrons were located throughout an atom like plums in plum pudding
John Dalton - E B. Atom model had electrons surrounding the nucleus at a specific distance.
JJ Thompson - A C. Stated atoms were the smallest piece of matter
Ernest Rutherford - B D. Electrons surround the nucleus in an electron cloud.
Niels Bohr - F E. Atoms of the same element are alike, and atoms of different elements are different.
Current Atomic Theory - D F. Electrons move around the nucleus in certain paths.

29. Put the atoms together and what do you get?
Everything around you!

30. Combination of ATOMS
When atoms are combined together, they create elements.
All known elements are located on the periodic table.
Dmitri Mendeleev, a Russian chemist, was the original founder of the periodic table.
* Arranged elements in order of increasing mass
Henry Moseley, a British scientist, is know as the founder of the modern day periodic table.
* Arranged elements in order of increasing atomic number

31. MODERN PERIODIC TABLE

32. PERIODIC TABLE SET-UP COLUMNS ROWS Also called families and groups
There are 18 columns.
Columns are vertical on the periodic table.
Elements in the same column have similar physical/chemical properties.
Also called periods
There are 7 rows.
Rows are horizontal on the periodic table.
As you travel across a row, the properties of elements gradually change.
COLUMNS
ROWS

33. Types of substances created from the periodic table
Compounds
2 or more elements that have combined in a fixed ratio.
Can have different properties than the elements that make them up.
Example – water
Water is different than the elements hydrogen and oxygen.
Molecules
Smallest particle of a substance with the same properties of that substance
Diatomic – simplest molecule
Some elements are naturally diatomic; H, O, Cl

34. Types of substances created from the periodic table
Mixtures
Combination of 2 or more substances that have not combined chemically.
Substances are not combined in the same ratio
Substances can be broken apart and have their own identity
Example: A supreme pizza. Every piece has a different ratio of toppings. I can pick them of and each piece is its own entity.
Solutions
Combination of 2 or more substances that have been combined chemically
The solution has the same properties throughout
A solution does not have to be liquid.
Example: Bronze is a solution. In order to be created a specific ratio of copper and tin must be mixed together. If you look at a piece of bronze, you cannot tell that there are two different elements present.

35. Types of substances created from the periodic table
BASES
Produce OH- ions in water
Taste bitter, chalky
Are electrolytes
Feel soapy, slippery
React with acids to form salts and water
ACIDS
Produce H+ (as H3O+) ions in water
Produce a negative ion (-) too
ion – an atom that has gained or lost an electron
Taste sour
Corrode metals
React with bases to form salts and water

36. KNOWLEDGE CHECK Compare a period and a group on the periodic table.
Are the properties of Potassium, K, more like those of
calcium, Ca, or Sodium, Na?
3. Draw the Ph scale. Label where acids and bases are found.
4. Label the following as a compound, mixture, or solution:
a. Water
b. Salt Water
c. Fruit Salad

37. KNOWLEDGE CHECK Compare a period and a group on the periodic table.
Rows are horizontal; groups run vertical.
Elements in the same group have similar properties.
Are the properties of Potassium, K, more like those of
calcium, Ca, or Sodium, Na?
Sodium, Na. Both these elements are in the same group.
3. Draw the Ph scale. Label where acids and bases are found.
1,2,3,4,5,6,7,8,9,10,11,12,13,14
A C I D S B A S E S
4. Label the following as a compound, mixture, or solution:
a. Water - Compound
b. Salt Water - Solution
c. Fruit Salad - Mixture