1. The Atom and Periodic Table
Physical Science

2. Element verse Atom ATOM ELEMENT Smallest particle of an element
A substance that cannot be broken down into simpler substances
Ex: Neon, Gold, Helium
ATOM
Smallest particle of an element
Counting unit of elements

3. History of the Atomic Model
Democritus
--believed in the atom
J.J. Thomson
--found the electron
John Dalton
--made the theory on atoms
Ernest Rutherford
--found the nucleus

4. History of the Atomic Model
Neil Bohr
--established energy levels
Electron Cloud Model
--the current model of the atom

5. 3 Subatomic Particles Atoms can be broken into:
Electrons
Negatively charged
Symbol = e-
Extremely small mass
Protons
Positively charged
Symbol = p+
Mass = 1
Neutrons
No charged (neutral)
Symbol = n
Mass = 1

6. Parts of an Atom Nucleus Energy Levels/Shells/Orbitals
Center of the atom
Small, dense, positively charged
Where Protons and Neutrons remain
Energy Levels/Shells/Orbitals
Around the nucleus
Contains the electrons

7. Atomic Number The Identify of the element Number of Protons
Top of the Element Block
SECRET: Also the number of electrons

8. Mass Number The sum of the Protons and Neutrons
Bottom Number of the element block
Round to the Nearest Whole Number

9. Understanding an Element Block
ATOMIC NUMBER 10 Ne
Element Symbol
1st letter is upper case
2nd letter is lower case
NEON
Element Name
20.18
Mass NUMBER

10. How do you Find Items Number of Protons = Atomic Number
Number of Electrons = Number of Protons
(Because Atoms are neutral which means positive equals negative)
Number of Neutrons =
Mass Number subtract Atomic Number

11. Electron, Protons, Neutrons Example Practice
Name
Symbol
Atomic Number
Mass Number
Number of Protons
Number of Electrons
Number of Neutrons
NEON
BORON

12. End Day ONE

13. ISOTOPES
Atoms of the same element that have the same atomic number but different mass numbers
# of protons stays the same
# of neutrons change

14. How Isotopes are Written
Elements name/symbol dash mass number
Ex:
Oxygen— p+= n =
Oxygen— p+= n =
O— p+= n =

15. Why is Mass Number a Decimal?
Mass Number is the weighted average of all the isotopes of an atom
The isotope whom mass number is closest to the actual mass number is more abundant

16. IONS Charged Particles Negative Charge = gains electrons
Positive Charge = lose electrons

17. End Day TWO

18. The Periodic Table
An arrangement of elements in columns based on properties that repeat from row to row
Modern Periodic Table arranged by Henry Moseley
Arranged by increasing atomic number

19. Parts of the Periodic Table
ROWS
Called Periods
Go across
COLUMNS
Called Groups
Go up and down

20. Periods 7 periods Elements in the same period have:
Same number of energy levels or shells or orbitals

21. Groups 18 groups Elements in the same group have the same: Properties
Valence Electrons
Oxidation Numbers

22. Valence Electrons Code:
Number of electrons on the outermost (last) energy level
Code:
1, 2, 3, 4, 5, 6, 7, 8
Number next to “A” at the top of the column

23. Know Your Roman Numerals
I = 1
II = 2
III = 3
IV = 4
V = 5
VI = 6
VII = 7
VIII = 8

24. Oxidation Number
Number of electrons an atom will gain or lose to become stable
Stable = 8 electrons on last shell
Code:
+1, +2, +3, ±4, -3, -2, -1, 0
“+” means lose electrons
“—” means gain electrons

25. Labeling the Periodic Table

26. End Day Three

27. Bohr’s Model Focuses On Electrons Places electrons into energy levels
Developed by Neil Bohr

28. Components of Bohr’s Model
Circles
DOTS
Number of Circles = Period Number = Number of Energy Level
Go on the Last Circle
Number of Dots = Number of Valence Electrons
Important Note
First energy level has a max of 2 electrons
All other energy levels have a max of 8 electrons

29. Steps to Draw Bohr’s Model
Place a dot to be Nucleus
Place circles around Nucleus
Place dots on last circle in correct order
EXAMPLE Oxygen

30. Bohr Model Practice
NEON
Boron
Helium

31. Electron Dot Diagrams
Model of an atom in which each dot represents the valence electrons
AKA: Lewis Dot Diagrams

32. Steps to Draw Dot Diagrams
Identify the number of valence electrons
Write the element’s symbol
Place dots around the symbol equal to valence electrons in correct order
Example
NEON

33. Dot Diagram Practice
Fluorine
Sodium
Carbon

34. End Day Four

35. Classifying Elements
Elements are classified as metals, nonmetals, or metalloids based on properties and location on the periodic table

36. Metals Most elements are them Malleable: hammer into sheets
Good Conductors of electricity/heat
Solid at room temperature (except Mercury)
Ductile: turn into thin wire
Luster: reflect light
Malleable: hammer into sheets
High Melting Point
Left side of the stair step
Francium: Most reactive metal
High Boiling Point

37. Nonmetals Dull Brittle Poor Conductors of electricity/heat
Most are gas at room temperature
Low Melting Point
Low Boiling Point
Right Side of Stair Step
Fluorine: most reactive nonmetal

38. Metalloids Have BOTH characteristics of metals and nonmetals
Found on the stair-step line
What are the Metalloids
B, Si, Ge, As, Sb, Te, Po, At

39. Periodic Trend Reactivity
As you go left to right across a period, the less reactive elements become

40. End Day Five

41. THE FAMILIES AND GROUPS OF THE PERIODIC TABLE

42. Alkali Metals Group IA 1 valence electron
Reactivity increases from top to bottom
Francium is most reactive metal

43. Alkaline Earth Metals Group IIA 2 valence electrons
Ca: is in your bones, teeth, shells

44. Transitional Metals THE MIDDLE OF THE PERIODIC TABLE Groups 3B-12B
Vary in oxidation numbers
Brightly colored
Likes to combine with Oxygen

45. BORON FAMILY Group IIIA 3 valence electrons
Al: most abundant metal in Earth’s crust

46. Carbon Family Group IVA 4 valence electrons
Carbon is the element of life

47. Nitrogen Family Group VA 5 valence electrons N is 78% of air
Main component of fertilizer

48. Oxygen Family Group VIA 6 valence electrons
O: most abundant element in Earth’s crust

49. The Halogens Group VIIA 7 valence electrons Salt formers
Reactive with metals
Fluorine: most reactive nonmetal

50. Noble Gases Group VIIIA 8 valence electrons Stable = not reactive
Inert Gases
All Shells are full

51. End UNIT