1. Elements and the Periodic Table
Chapter 4

2. The Atom
Chapter 4.1 pg
Cornell Notes

3. Essential Questions What is the structure of the atom?
What are the 3 subatomic particles?
What particles make up the nucleus?

4. 1. The Atom Atom: the smallest particle of an element (pg:124-125)
Nucleus: the center of an atom; also where the protons and neutrons can be found (pg:128)

5. electron clouds nucleus
Surrounding the nucleus is a cloud-like region of moving electrons.
electron clouds
nucleus
At the center of the atom is a tiny nucleus containing protons and neutrons.

6. A. Proton
Proton: positively charged particles in an atom’s nucleus; mass = 1 amu (atomic mass unit)
Number of protons identifies the element
Number of protons and identifies the element = atomic number

7. B. Neutron
Neutron: Particles with no charge in the nucleus; mass = 1 amu
# of protons + the # of neutrons = mass number/atomic mass
Adding or taking away neutrons DOES NOT change the atom, it makes different isotopes

8. Isotopes- atoms of the same element that have different numbers of neutrons.
Example: Carbon-12 = 6 neutrons, Carbon-13 = 7 neutrons, and Carbon-14 = 8 neutrons (pg: 130)

9. Isotopes or different elements?
T has 20 protons and 20 neutrons
Z has 20 protons and 21 neutrons
T and Z are isotopes
same # of protons, different # of neutrons
A has 31 protons and 39 neutrons
E has 32 protons and 38 neutrons
A and E are different elements
different # of protons

10. C. Electron
Electron: negatively charged particles in the electron cloud; mass = 0 amu (very small It takes electrons to equal the mass of 1 proton)
# of electrons = # of protons in a neutral atom
Valence Electron- The electron(s) in the shell farthest from the nucleus

11. electron clouds nucleus Protons (+) Neutron (0) Valence Electrons (-)

12. Protons (+) Neutron (0) Valence electrons Electron (- ) P+ N
A simplified slide P+ N
Neutron (0)

13. With your partner: Protons Neutrons Electrons
Can you name the charge, location and mass
Neutrons
Electrons

14. The electrons are arranged in a particular order
The electrons are arranged in a particular order. The electrons fill the energy shells closest to the nucleus first and then fill outward:
The first energy shell can hold up to 2 electrons
The second energy shell can hold up to 8 electrons
The third energy shell can hold up to 18 electrons
The fourth energy shell can hold up to 32 electrons

15. Electron Shell Diagram – *
First Energy Level
2 electrons
Second Energy
Level 8 electrons
Third Energy
Level 18 electrons
Fourth Energy
Level 32 electrons

16. Sub-Atomic Particle Review
Atomic mass in atomic mass units
charge
location
Proton
1 amu +
positive
nucleus
Neutron
neutral
Electron
0 amu _
negative
Orbits around nucleus in electron cloud

17. Section 1 Review 7 10 10 8 Oxygen O 1 Hydrogen H 6 Carbon C 7 N Neon
Proton number
Atomic number
Element
Symbol 8
Oxygen O 1
Hydrogen H 6
Carbon C 7 N
Neon Ne 7
Nitrogen 10 10

18. Review 6 12 11 23 14 28 8 16 C Carbon Na Sodium Si Silicon O Oxygen
Element
Atomic number
Proton number
Atomic mass
(rounded)
Neutrons
Electrons C
Carbon 6 12 Na
Sodium 11 23 Si
Silicon 14 28 O
Oxygen 8 16

19. Organizing the elements
Chapter 4.2
Cornell Notes

20. 4.2 Essential Questions
How is the Periodic Table of the Elements (PTE) arranged?

21. 1. Mendeleev
-Russian Chemist who looked for patterns of properties of the elements.
-He grouped the elements according to the patterns and by increasing atomic mass.
-This allows us to predict the properties of missing elements.

22. 2. Atomic Weight
The average of all the masses of all the isotopes of an element

23. 3. Using the periodic table
The properties of an element can be predicted from its location on the periodic table
Elements are arranged in order of increasing atomic weight

24. 4. How to read the Periodic Table
Atomic Number- number of protons
Atomic Symbol
First letter always capitalized, second never C
Atomic Mass- protons +neutrons 6
12.011

25. 4. How to read the Periodic Table (partner review)Li 3
6.941

26. 5. Periods Horizontal rows (pg. 134-135)
The properties gradually change as you move left to right across the Periodic Table.
Indicates the number of electron shells

27. 5. Periods

28. 6. families or Groups Vertical Columns (pg 134-135)
Similar Physical and Chemical properties
Indicates the number of Valence Electrons

29. 6. Families or Groups

30. Review: With your partner
How is the PTE organized?
Vertical columns?
Horizontal rows?
What order are the elements in?

31. Metals, Nonmetals, inert gasses, and semimetals
Chapter 4.3 & 4.4
Cornell Notes

32. Essential Questions
Where are metals, nonmetals and semi metals on the PTE?
What are the properties of metals, nonmetals and semimetals?
What are the properties of elements in each family?

33. Metals, Nonmetals, and Semimetals
• Metals and nonmetals are separated by a stair-step line on the right side of the table.
• Metals are found to the left of the line and nonmetals are found to the right of the line.
• Elements that border the line on both sides are called semi-metals.

34. The Periodic Table
Semimetals
Metals
Nonmetals

35. A. Metals 1. Found on the left of the periodic table.
2. Have only a few electrons in outer shell.
3.Most are solid, shiny, good conductors of heat and electricity, malleable, are ductile.
4. Alkali metals – Family/Group 1
5. Alkaline earth metals – Family/Group 2
6. Transition metals – Families/Groups 3-12

36. B. Nonmetals 1.Found on the right side of periodic table
2. Most are dull, not malleable or ductile, not good conductors of heat or electricity.
3.Valence electron shell is mostly or completely full

37. C. Semi-Metals (metalloids)
1.Found along the zig-zag (stair step) line on the periodic table; also called metalloids
2. They are semi-conductors that have properties of both metals and non-metals.
3.The outer electron shell is about half full.

38. With your partner
Can you identify where the metals, non metals and semimetals are on the PTE
What are the properties of metal?
What are the properties of a nonmetal?
What are the properties of a semimetal?

39. Valence Electrons Electrons that are in the outer shell
Valence Electrons determine reactivity
A full shell is stable
The valence shell is complete with 8 electrons

40. reactivity Empty or Full Half full or half empty
non reactive (inert)
Close to full or close to empty
very reactive
Half full or half empty
not as reactive

41. Boron Family Alkali Metals
Halogen Family
Inert / Nobel Gases
Lanthanides
Actinides
Oxygen Family
Nitrogen Family
Transition Metals
Boron Family
Carbon Family
Alkaline Earth Metals
Alkali Metals

42. A. Alkali Family (1 Valence Electron)
The most reactive metals
Shiny and soft
Can be cut with a knife

43. B. Alkaline Earth Metals (2 Valence Electrons)
Very Reactive
Silver colored metals, more dense than family #1

44. C. Transition Metals Have 1-2 Valence electrons
Includes many common metals such as copper, iron, gold, and silver

45. D. Boron Family (3 valence electrons)
Reactive Solids

46. E.Carbon Family (4 Valence electrons)
Reactivity varies
All are solids
Carbon based molecules make up all living things

47. F.Nitrogen Family (5 valence electrons)
Reactivity varies
Nitrogen is the most common element in the atmosphere

48. G. Oxygen Family (6 valence electrons)
Reactive

49. H. Halogen Family (7 valence electrons)
-These are the
MOST REACTIVE NONMETALS
-Some are used as cleaners

50. I.Inert Gases (Noble Gases) (8 valence electrons)
Stable – Not reactive!!
All are nonmetals, and all are gases
Helium only has 2 valence electrons because it only HAS 2 electrons total

51. Lanthanide and Actinide Families (2 valence electrons)
These are a part of the transition element family

52. Liquids, gases and semi metals
The majority of elements are solids (so we are not labeling those)
Find and mark (be creative) the liquids
Find and mark (be creative) the gases
Darken the stair step line for metalloids and outline the boxes of elements that are semi- metals