1. Structure of the Atom
&
The Periodic Table

2. Atomic Structure Goals
Examine the structure of the atom in terms of
proton, electron, and neutron locations.
atomic mass and atomic number.
atoms with different numbers of neutrons (isotopes).
Develop and use models to compare and contrast the structure of atoms, ions and isotopes. Analyze data to the number of valence electrons.
Chemistry

3. TedEd: Just How Small is an Atom?

4. Matter This will be our FOCUS Mixture Pure Substance Compound Element
Intro Clip

5. What is an Element? Elements are the building blocks for all matter.
One of the ~118 known “Pure”, un-cutable substances. ….that still retain the properties of that substance.

6. What is an Atom?
Smallest piece of matter that still retains the properties of that matter.
What are they composed of?

7. TedEd: The 2,400-year search for the atom

8. 7
Subatomic Particles
Protons
Neutrons
Electrons
Nucleus

9. 8

10. What makes one element different from another element?
Number of protons. 9

12. Protons Positive Charge
The number of protons determines which element it is.
All elements have different numbers of protons
Mass= 1amu

13. Electrons Smallest subatomic particle. 1/1800 the mass of a proton.
Orbit nucleus.
Negative Charge

14. Electrons are found in different levels around the nucleus.
These are called Energy Levels or shells.

16. Electrons are found in the
Electron cloud
Surrounding
the nucleus.

17. Each Energy Level Can Hold A Certain Numbers of Electrons!
Only TWO on the first level!

18. Each Energy Level Can Hold A Certain Numbers of Electrons!
Different atoms have different numbers of electrons!
Each Energy Level Can Hold A Certain Numbers of Electrons!
Eight on the 2nd and 3rd levels!
Review Clip
Add:
Valence Electrons: Outermost electrons.

19. Neutrons No Charge- Neutral Found in the nucleus
Same size as a protons
Mass= 1amu

20. Atomic Number and Mass Number
How to find the number of Protons & Neutrons

21. How do you find # of Neutrons???
Atomic Number
Number of Protons 1 H
Atomic Mass
Sum of Protons & Neutrons 1
How do you find # of Neutrons???

22. How can I find out how many electrons an atom has?
An atom is neutral
So, the number of protons = electrons.
Atomic number tells you the number of protons
So, it also tells you the number of electrons!

23. Do Starter #3

24. Practice (on notebook paper)
Elements
Hydrogen
Carbon
Sulfur
Fluorine
Neon
Silicon
Aluminum
Magnesium 4 Be
9.01
Beryllium
Practice (on notebook paper)
Outside
Inside
At #____
At mass____
#p=____
#e=____
#n=____
VE=______

26. 20
Isotopes

27. Isotopes
Isotopes are atoms that have the same number of protons and differ only in the number of neutrons. 21
Most isotopes are stable but radioactive isotopes are unstable and break down into more stable forms by emitting particles and energy (radiation).
Radiation can be detected, so radioactive isotopes are useful as labels in scientific research and medical diagnostic procedures.

28. Still have the same # of protons, so they are still the SAME element.
Isotopes of Helium 22
Isotopes of Carbon
Isotope Video Clip
Still have the same # of protons, so they are still the SAME element.

29. 23 Isotope Notation Mass Number Atomic Number Symbol
Protons + Neutrons
Symbol
Atomic Number
Protons

30. 24
Some isotopes are more abundant on earth than others.

31. Review: Isotopes

32. 25
Electron Dot Diagrams
Shows the number of valence electrons an element has
Examples:
Hydrogen
Beryllium
Oxygen
Sulfur

33. Periodic
Table
Element Song

34. Determine the trends of the following:
Number of valence electrons
Location of metals, nonmetals, and metalloids
Phases at room temperature
2. Use the Periodic Table to predict the above properties for representative elements.

35. Dmitri Ivanovitch Mendeléev
Grouped elements on the basis of similar chemical properties. 
Left blank spaces open to add new elements where he predicted they would occur. 
Accepted minor inversions when placing the elements in order of increasing atomic mass. 
Predicted properties for undiscovered elements.

36. The genius of Mendeleev's periodic table

37. Groups or Families
increasing atomic number
periods

38. Add to notes. Bottom pf P.3
Ions
When an atom gains or loses electrons to become stable. The atom then has a positive or negative charge.

39. When Atoms gain or lose electrons, they are called Ions.
Add to notes
When Atoms gain or lose electrons, they are called Ions. 3P 3P 3P
Anion 3P 3P 3P
Cation

41. Alkali Metals Soft Metals, solids @room temp
Clip
Soft Metals, temp
Very reactive metals that do not occur freely in nature.
Only one valence electron
malleable, ductile, and are good conductors of heat and electricity.
Cesium and francium are the most reactive elements in this group.
Can explode if they are exposed to water.

42. Alkaline Earth Metals Two valence electron Form +2 ions
Because of their reactivity, the alkaline metals are not found free in nature.
Form many compounds with 6A

43. Alkaline Earth Metals- Group 2A

44. Transition Metals All solids @ room temp.
Are both ductile and malleable, and conduct electricity and heat.
The interesting thing about transition metals is that their valence electrons change.
There are three noteworthy elements in the transition metals family. -iron, cobalt, and nickel, and they are the only elements known to produce a magnetic field.
Form positive ions

45. Transition Metals
The other metals…Clip

46. Metalloids
Clip
Metalloids have properties of both metals and non-metals.
Some of the metalloids, such as silicon and germanium, are semi-conductors. This means that they can carry an electrical charge under special conditions. This property makes metalloids useful in computers and calculators
All solids at room temperature

47. Halogens "halogen" means "salt-former" and compounds containing
CLIP
"halogen" means "salt-former" and compounds containing
halogens are called "salts".
All have 7 valence
electrons.
Form -1 ions
Form many compounds with the alkali metals.
exist, at room temperature, in all three states of matter:
Solid- Iodine, Astatine
Liquid- Bromine
Gas- Fluorine, Chlorine

49. Noble Gases All (but one) have 8 valence electrons Chemically inert
Clip
All (but one) have 8 valence electrons
Chemically inert
All gases at room temp.
They all have very low boiling and melting points.
Do not form ions
They all put out a color in the visible wavelengths when a low pressure of the gas is put into a tube and a high voltage current is run through the tube. This type of tube is called a neon light whether the tube has neon in it or not.

50. Rare Earth Metals
-The thirty rare earth elements are composed of the lanthanide and actinide series.
One element of the lanthanide series and most of the elements in the actinide series are called trans-uranium, which means synthetic or man-made.
All of the rare earth metals are found in group 3 of the periodic table, and the 6th and 7th periods.
All rare earth elements have 3 valence electrons and are solid at room temp.

51. Lanthanide Series

52. Actinide Series

55. Allotropes
Different forms of the same element. They have different molecular structures.
Same formula- different structure

56. A molecule that consist of 2 atoms of the same element Br Br I I
A molecule that consist of 2 atoms of the same element
Never found in nature alone.
Where are these found on the Periodic table?

57. Metals vs. Nonmetals
Lose their valence electrons easily.
Form positive ions
Good electrical conductors and heat conductors.
Malleable & Ductile
Solid at room temperature
Gain or share valence electrons easily.
Poor conductors of heat and electricity.
Brittle - if a solid.
Nonductile.
Solids, liquids or room temp.
Metallic bonding: e- move freely among a metal’s positive charges ions

58. Metals lose electrons to become stable.
Nonmetals gain electrons to become stable.
Add to notes

59. Electron Donors
Electron Acceptors

60. Periodic Trends

61. Atomic Radii
The greater the number of protons present, the stronger the attraction that holds the electrons closer to the nucleus, and the smaller the size of the shells.

66. Periodic Table Review