1. Periodic Patterns

2. The Periodic Table

3. Design of the Periodic Table
Classification of Element
By looking at where a element is on the periodic table, you can tell about it’s chemical and physical properties
Columns (18)
Up and down
Called Families/Groups
Elements in Families have similar properties
Rows (7)
Side to Side
Called Periods
Elements in periods DO NOT have similar properties

5. The first two and last six columns are numbered 1A-8A, relates to the # of electrons in their OUTER shell. 1A 2A
3A 4A 5A 6A 7A 8A

7. Properties of the metals
These elements are metals:
Physical Properties
Luster- Shininess
Ductile and malleable- able to be drawn into wires and hammered into sheets
Chemical Properties
Corrosive- wearing down due to chemical reaction
Easily lose electrons

8. Alkali Metals Group 1 Very reactive Form +1 ions Cations
Examples: H, Li, Na

9. Alkaline Earth Metals Group 2 Reactive Form 2+ ions Cations
Examples: Be, Mg, Ca, etc

10. Transition Metals Groups 3B-12B on the Periodic Table
Much less reactive than Alkali or Alkaline Earth Metals
Only 1 that is a liquid at room temp
Mercury – Hg
Examples: Cr, Co, Ni, Fe, Cu, Ag, Au

11. Properties of non-metals
These elements are non-metals:
Physical Properties
No Luster
Not ductile or malleable
Chemical Properties
Tend to gain electrons

12. Nonmetals Not good conductors
Found on right side of periodic table – AND hydrogen
Usually brittle solids or gases

13. Halogens Group 17 Very reactive Form 1- ions Anions
Examples: F, Cl, Br, etc

14. Properties of Noble Gases
These Elements are Noble gases:
Group 18
Unreactive, inert, “noble”
Have a 0 charge, no ions
Examples: He, Ne, Ar, Kr, etc

15. Properties of Metalloids
These Elements are metalloids
Form the “stairstep” between metals and nonmetals
Properties
Can have both of metals and non metals
Sometimes called semiconductors
Example:
Can be shiny or dull, malleable or not…

16. Properties of rare Earth metals
These Elements are rare Earth metals:
Properties:
The rare earths are silver, silvery-white, or gray metals.
The metals have a high luster, but tarnish readily in air.
The metals have high electrical conductivity.
Lanthanides - part of period 6
Actinides - part of period 7

17. Atoms Inside the Atom Elements are made of particles called atoms
Atoms are the smallest pieces of matter that contain all the properties of a specific element
Each element contains only one type of atom
Inside the Atom
Atoms are made up of smaller particles
These particles are found in different regions of the atom

18. Neutron Protons Electron Neutral particles found in nucleus of atom
Positively charged particles found in nucleus of atom
Have an electrical charge of +1
Mass of 1 a.m.u.
Neutron
Neutral particles found in nucleus of atom
Have no electrical charge
Electron
Negatively charged particles found in electron cloud
Have an electrical charge of -1
Constantly moving around outside nucleus
Have essentially no mass

19. Structure of the Periodic Table
Atomic number – Tells us how many protons and electrons are in an atom
The number of protons defines the identity of the atom
Atomic Mass – gives the mass of a single atom in atomic mass units (amu)
Atomic mass = # p+ + n0
Oxidation Number – tells us what the atom wants to do with electrons

20. Structure of the Periodic Table
The Periodic Table also tells us about the electron structure of an atom
Each Period represents an energy level in the electron cloud
Ex: Na is in the 3rd Period, therefore its electron cloud will consist of 3 Energy levels
The Group number represents the number of electrons in the outer energy level
Ex: Na is in a Group 1 element, therefore it has one electron in the outer energy level
The number of boxes in each period indicate the number of electrons that the energy level can hold

23. Comprehension Check
How many energy levels does aluminum’s electron cloud have? 3
How many electrons are in aluminum’s 2nd energy level? 8
How many electrons are in aluminum’s 3rd energy level?

24. Symbols Elements are listed by their chemical symbols
Symbols are usually either one capital letter like C for Carbon, or one capital and one lowercase letter like Ne for Neon

25. Periodic Table
The periodic table gives much information we need to learn more about the atom of each element

26. Atomic Mass Mass # = # p+ + # n0
The average atomic mass is the number at the bottom of this square
Found by averaging the natural abundances of its isotopes
Mass # = # p+ + # n0

27. Atom Math
Atomic Number
Symbol
Element Name
Atomic Mass

28. Atom Math
Protons
Electrons
Protons
Neutrons

29. Practice # n0 = Mass # - Atomic # Zn Oxygen Lithium 8 30 3 15.999
65.39
6.941 8 30 3 35 8 4 8 30 3
# n0 = Mass # - Atomic #

30. Mass # Atomic # Isotopes Nuclear symbol: Hyphen notation: carbon-12
Atoms of the same element with different mass numbers.
Nuclear symbol:
Mass #
Atomic #
Hyphen notation: carbon-12

31. Isotopes
© Addison-Wesley Publishing Company, Inc.

32. How many eggs go in an egg carton?

33. The Role of Electrons in Bonding
The sharing or transfer of electrons is what holds atoms together in a compound
Typically, only the electrons in the outer energy level are used for bonding.
These electrons are called Valence Electrons
The outer energy level is called the Valence Shell
Octet Rule: atoms want to have a full valence shell (8 valence electrons)
Atoms react with one another in an attempt to gain or lose electrons to fill their valence shell
During a reaction, electrons can be shared or completely transferred

34. Comprehension Check How many valence electrons does phosphorus have?5
How many electrons does phosphorus have to gain or lose in order to fill its valence shell?
Lose 5, Gain 3

35. Comprehension Check- To Gain or Not to Gain
nitrogen
beryllium
xenon
carbon
Gain 3
Lose 2
None
Gain/Lose 4
oxygen
lithium
chlorine
boron
Gain 2
Lose 1
Gain 1
Lose 3

36. Types of Bonds
Ionic Bonds – Results from the complete transfer of electrons
Results in a formation of two charged atoms called ions
The atom that gains electrons becomes negatively charged and is called an anion
The atom that loses electrons becomes positively charged and is called a cation
The attraction of the positive and negative charges results in a very weak bond
Covalent Bonds – Results from the sharing of electrons
The shared electrons create a very strong bond
These are the bonds that make molecules possible

37. Oxidation Numbers
Oxidation Numbers tell us how many electrons an atom is willing to lose or gain
Positive oxidation numbers indicate that the atom can lose that many electrons
Negative oxidation numbers indicate that the atom can gain that many electrons
Some atoms have more than one possibility