1. Organization of The Periodic Table
Open to page 112 and 113.

2. Nucleus Center of the atom. Makes majority of the atom’s mass.
Made of protons and neutrons.

3. Protons
Part of the nucleus
Have positive (+) charge

4. Neutrons
Part of the nucleus
Have neutral charge

5. Electrons
Orbit around the nucleus
Have negative (-) charge

6. Atomic Number Definition: the number of protons in the nucleus
Tells us the identity of the element.
Mass
Every element is defined by the number of protons in its nucleus

7. Isotopes
Atoms with the same number of protons but different numbers on neutrons
Example: Carbon
So you can change the number of neutrons and the element still maintains its identity

8. Questions 1) What particles make up an atom?
2) What are the charges on these particles?
3) What particles make up the nucleus?

9. Questions 1) What is Oxygen’s atomic number?
2) How many protons does Oxygen have?
3) If I have 4 protons what element am I?
4) If I have 4 neutrons what element am I?

10. Reading the Periodic Table
Mass

11. Atomic Mass Definition: the mass of one atom of an element
Tells us how much one atom weighs in atomic mass units.
Mass

12. Organization of The Periodic Table
Group/Family
Period
Ordered by atomic mass. Columns arranged to form groups with similar properties

13. Assessment Which element has the greatest atomic mass? Lithium Sodium
Potassium
Rubidium
Rubidium

14. Reactivity
The ease and speed with which an element combines, or reacts, with other elements or compounds
Pure sodium reacts explosively
with air

15. Groups/families of elements have similar reactivity
Group 1: metals that react violently with water
Group 18: Gases that barely react at all
Why do groups/families of elements react the same way?

16. Atoms have neutral charge
# of Protons (+) = # of Electrons (-) = 0 charge
Example: Hydrogen
How many electrons does C have?
carbon has 6 electrons.

17. Question How many electrons does an oxygen have?
Which group is oxygen most likely to react with?

18. Question For the first 3 periods:
1) Which group is least likely to react with any other group?
2) Which groups are the most likely to react with one another?

19. Take home message
The properties of an element can be predicted from its location on the Periodic Table
This is largely a result of the number of electrons.

20. Assignment Read p. 109 – 117 Complete Section 2 Assessment
(No Writing in Science)

21. Metals, Metalloids, and Nonmetals

22. Metals Shiny Solids (at room temp) Malleable – can be hammered flat
Ductile – can be pulled into wire
High Conductivity – ability to transfer heat or electricity to another object

23. Reactivity of Metals Low High
Metals will usually lose electrons when they react with other elements

24. Magnesium reacting to water.
Sodium reacting to water.

25. Alkali Metals Metals in Group 1
Often lose an electron when they react with other elements
Rare to find them in their pure form because they are so reactive
Very shiny and soft
Example: Lithium batteries
Potassium in its pure form

26. Alkaline Earth Metals Group 2
Hard, gray-white, good conductor of electricity
Lose 2 electrons when they react with other elements
Hard to find in pure form.
Example: Calcium in your teeth
and bones.
Calcium in its pure form

27. Transition Metals Groups 3 – 12
Hard, shiny, good conductors of electricity
Can form colorful compounds
Less reactive
Examples: iron, gold, copper, nickel
Pure iron
Pure copper

28. Groups 13-15 Only some are metals Not very reactive
Examples: aluminum, tin, lead
Pure aluminum
Pure lead

29. Lanthanides 1st row below the Periodic Table
Soft, malleable, shiny metals
Often mixed with other metals to make alloys
Pure cerium
Pure Samarium

30. Actinides 2nd row below the Periodic Table
Only the first six naturally occur on Earth
The other elements are synthetic and unstable
Some only exists for a few seconds after being made
Depleted uranium

31. Assignment P. 125 Section 3 Questions
Complete on a separate piece of paper
Skip the “At-Home Activity”

32. Assignment Go on a metal scavenger hunt at your house, school, etc…
Make a list of 10 metals you find
Identify each metal and the group it belongs to.
You cannot write down the same metal more than twice!
Example
Item
Type of Metal
Group
Mom’s wedding ring
Gold, Transition Metal 11

33. Nonmetals Sulfur Opposite of properties of metals Not shiny
Poor conductors
Mostly gases (at room temperature)
Solids are brittle
Sulfur

34. Reactivity of Nonmetals
Low
Low
High
Nonmetals will usually gain or share electrons when they react with other elements

35. Some Important Nonmetals
Carbon – important element for making up living organisms
Noble Gases – group 18 – very nonreactive. Have full outer shells.

36. Metalloids Inbetween metals and nonmetals Solids (at room temp)
brittle and hard
Semiconductors – can conduct electricity under some conditions but not others.
very important for computer chips
Most common example – Silicon – in sand and glass

37. Assessment The atomic number is the number of valence electrons.
neutrons.
protons in the nucleus.
electrons in the nucleus.
Protons in nucleus

38. Assessment
The periodic table is a chart of the elements that shows the repeating pattern of their
energies.
properties.
element symbols.
names.
properties

39. Assessment
Which piece of information cannot be found in a square on the periodic table?
Atomic mass.
Chemical symbol.
Atomic number.
Number of neutrons.
Number of neutrons

40. Assessment Which element will have properties most similar to Calcium?
Potassium.
Scandium.
Magnesium.
Bromine.
Magnesium.

41. Assessment
Which group is most likely to lose/share 2 electrons in a chemical reaction? 1 2 17 18
Magnesium.

42. Assessment
Which side of the periodic table contains most of the nonmetals?
Left side
Right side
Middle
Magnesium.

43. Assessment Which is not a property of nonmetals? Brittle Nonmalleable
High conductivity
Most are gases at room temperature
Magnesium.

44. Assessment Which metal is probably the most reactive? Potassium
Calcium
Scandium
Titanium
Potassium

45. Assessment Which nonmetal is probably the most reactive? Nitrogen
Oxygen
Fluorine
Neon
Flourine