1. Organizing the Elements
Atomic Mass: the average mass of the isotopes (same element but different number of neutrons) of that element
Mendeleev original arrangement: increasing atomic mass- found that properties of the elements repeated
Periodic table: arrangement of elements – because of repetition of properties
Mendeleev predicted properties of elements not yet discovered
Modern arrangement of periodic table- increasing atomic number

2. Understanding the Atomic Structure
Parts of the atom: nucleus – protons +, neutrons 0, outside nucleus- electrons –
Atomic number: number of protons- every atom of a particular element has its unique number of protons
Protons and neutrons have the same mass (make up most of the mass of the atom)
Electrons are not nearly as massive as the protons and neutrons

3. Information found in the Periodic Table
Atomic number (number of protons)
Chemical symbol (abbreviation of name)
Name
Atomic mass (average mass of all isotopes of that element)

4. Periodic Table Made up of:
Rows called Periods ( 7 periods)- similar characteristics
Columns called Groups/ Families (18 groups)

5. Periodic Table
Properties can be predicted based of location in periodic table
Metals( left), nonmetals (right), metalloids (between)

6. Properties Change (left to right)
Majority of elements are metals
Good conductors of electricity and heat
Physical Properties
Luster: high luster= shinny and reflective
Malleability= ability to bend= can be hammered and rolled into flat sheets
Ductility: can be drawn into long wires
Conductivity: thermal- ability to transfer heat and electrical- ability to carry electric current
Chemical Properties :
Reactivity: the ease and speed with which an element reacts with other substances. React by losing electrons
Corrosion: deterioration of metals due to a chemical reaction in the environment

7. Chemical Families/Groups

8. Classification of Metals
Alkali Metals( group 1)- most reactive never found uncombined in nature, soft, low densities, low melting points
Alkali Earth Metals (group 2)- never found uncombined in nature- reactive but not as reactive as group 1) harder, denser and melt at higher temperatures than alkali
Transitions Metals (groups 3-12) hard and shinny solids, high melting points and high densities, less reactive than group 1 and 2
Some of the elements in groups are metals
Metals in Mixed Groups
Lanthanides
Actinides

9. Lanthanide and Actinide Metals
two rows below main part of periodic table

10. Transuranium those that follow uranium- atomic number above 95
unstable- decay radioactively into other elements

11. Periodic Table
Which of these elements has properties most similar to Magnesium: Sodium, Calcium, or Manganese? How do you know?
SC.8.P.8.6

12. Properties of Nonmetals
Lacks most of the properties of a metal
Right side of periodic table (exception: hydrogen)
Wider variety of properties- few in common
Most are poor conductors of electric and current and heat.
Solid nonmetals tend to be dull and brittle
Lower densities than metals
Chemical properties- usually gain or share electrons when they react with other atoms

13. Families Nonmetals Group 1 Groups 14-18
Carbon family, nitrogen family, oxygen family, the halogen family, noble gases and hydrogen

14. Nonmetals Group 14- carbon is the only nonmetal
Nitrogen family- 2 nonmetals – nitrogen (diatomic- two of the same atoms bonded together) and phosphorus
Oxygen family- 3 nonmetals- oxygen, sulfur and selenium
Halogens( group 17)- nonmetals- fluorine, bromine, chlorine, and iodine- very reactive; fluorine most reactive of all elements
Noble gas- group 18- nonreactive
Hydrogen- cannot be grouped- very different properties than any other element

15. Metalloids
Elements that have some properties of metals and some of nonmetals
Solid at room temperature
Brittle, hard and somewhat reactive
Silicone, germanium and arsenic – semiconductors- substances that can conduct electric current under some conditions but not under others

16. Acids, Bases, and Salts
Which substances reacted with baking soda to create a gas? Why?
Acids and Bases
What is created when a base (alkali) is added to an acid?
Can do one or both simulations. 1st simulation does not refer to salts at all. 2nd simulation refers to metals as bases and says that strong bases are corrosive which may be confusing but most of it is very good information so it can be overlooked.
SC.8.P.8.8

17. Electromagnetic Spectrum
Physical Science
Electromagnetic Spectrum

18. Benchmarks
SC.7.P.10.1: Students will identify, compare and contrast the variety of types of radiation present in radiation from the Sun.
SC.8.E.5.11: Students will identify and compare characteristics of the electromagnetic spectrum. Students will identify common uses and applications of electromagnetic waves.

19. Heating Damaging Coloring
Sun’s Radiation
Heating
Damaging
Coloring
Which word above relates to each of the types of Solar radiation: Infrared, Visible Light, and Ultraviolet?
SC.7.P.10.1

20. Electromagnetic SpectrumB
Which wave image (A or B) is accurate? Using the terms “wavelength” and “frequency” describe the trends in the waves within the EM Spectrum.
SC.8.E.5.11

21. Physical Science
Waves

22. Benchmarks
SC.7.P.10.3: Students will describe and explain that waves move at different speeds through different materials.
SC.7.P.10.2: Students will explain that light waves can be reflected, refracted, and absorbed.

23. Speed of Waves
Light Wave
What happens to the speed of the light as it travels from the air, through the glass, and then through the water?
SC.7.P.10.3

24. Reflect, Refract, Absorb
Label the images above with the correct term concerning the motion of light waves. Explain your choices
SC.7.P.10.2

25. Transformation of Energy
Physical Science
Transformation of Energy

26. Benchmarks
SC.7.P.11.2: Students will identify and describe the transformation of energy from one form to another.
SC.6.P.11.1: Students will differentiate between potential and kinetic energy. Students will identify and explain situations where energy is transformed between kinetic energy and potential energy.
SC.7.P.11.3: Students will identify and describe examples of the Law of Conservation of Energy.

27. Transformation of Energy
Energy Transformation
Think about:
What are some examples of each type of energy (chemical, thermal, electrical, mechanical, light, and nuclear)?
Good over all review of energy but gets into Renewable resources, Heat flow, etc… so save for later
SC.7.P.11.2

28. Potential vs Kinetic Energy
Energy in a Skate Park
Think about:
When is the skater’s potential energy the greatest? Where is the potential energy being transformed into kinetic energy?
SC.6.P.11.1

29. Law of Conservation of Energy
Energy of Springs
Think about:
What happens to the Total Energy as the spring bounces? Which types of energy make up the total energy? How to they relate to each other?
Be sure to click on “Show Energy of” buttons so students can see the bar graphs
SC.7.P.11.3

30. Physical Science
Heat Flow

31. Benchmarks
SC.7.P.11.4: Students will describe how heat flows in predictable ways.
SC.7.P.11.1: Students will explain that adding heat to or removing heat from a system may result in a temperature change and possibly a change of state.

32. Heat Flow B A C
Label the examples of heat flow above as either radiation, conduction, or convection. Explain your choices
SC.7.P.11.4

33. Adding and Removing Heat
Changing State
Think about:
When you “cool” the beaker, are you adding cold or removing heat? Explain
SC.7.P.11.1

34. Types of Forces Mass and Weight
Physical Science
Types of Forces
Mass and Weight

35. Benchmarks
SC.6.P.13.1: Students will identify and describe types of forces.
SC.6.P.13.2: Students will describe the relationship among distance, mass, and gravitational force between any two objects.
SC.8.P.8.2: Students will differentiate between mass and weight

36. Types of Forces Forces Think about:
What force works against an object traveling horizontally? What kind of force (balanced or unbalanced) changes an object’s motion?
Previews the next two slides as well
SC.6.P.13.1

37. Distance, Mass, and Gravity
Gravity Model
Think about:
What happens to the direction and magnitude of the force of gravity as you change the distance and/or masses?
SC.6.P.13.2

38. Weight vs Mass
An object is placed on the digital scale and spring scale below and the following readings are observed
9.5g
93.1 N
Which instrument is measuring the object’s mass and which is measuring the object’s weight? Why are the numbers different? Explain your thinking
SC.8.P.8.2

39. Balanced and Unbalanced Forces
Physical Science
Balanced and Unbalanced Forces

40. Benchmarks
SC.6.P.13.3: Students will describe and explain that an unbalanced force acting on an object changes its speed and/or direction.
SC.6.P.12.1: Students will interpret and analyze graphs of distance and time for an object moving at a constant speed.

41. Unbalanced Forces Unbalanced Forces Think about:
In order for the object to move, which force had to be overcome?
Simulation has a LOT of extras, can keep it very simple or go more in depth as needed
SC.6.P.13.3

42. Distance vs Time B C A
Technically benchmark is only for constant speed so C is not entirely appropriate, but it would be good to see if the students KNOW that C is not constant speed.
Describe the motion of the object during each section.
SC.6.P.12.1