1. Do Now Sit SILENTLY and pull out your notebooks
Copy these questions and prepare to answer them while watching the video after role is called.
What was Newland’s initial theory/law called?
Who eventually streamlined the periodic table?
What was the element that proved the periodic table worked? Why?

2. Periodic
Table

3. He organized them by their increasing atomic masses.
Dmitri Mendeleev organized the known elements into a table called the periodic table.
He organized them by their increasing atomic masses.

4. Today we organize the elements by their increasing Atomic Number.

5. Insert copy of the periodic table.

6. Rows on the periodic table are called periods
Rows on the periodic table are called periods. All the elements listed in a row belong to the same period. There are 7 (seven) periods.

7. Columns in the periodic table are called groups or families
Columns in the periodic table are called groups or families. All elements in a group have similar properties.

8. Insert copy of the periodic table.
The columns have been given an Arabic number. The columns are numbered 1 – 18 starting at the left and moving to the right.

9. The outer most energy level is usually not full or complete .
Valence Electrons
The outer most energy level is usually not full or complete .
These electrons in the outer energy level are called Valence electrons.
Valence electrons are important because they determine how an element will react with other substance.

10. Insert picture of periodic table.
In group 1 and 2 the number of Valence electrons in the outer energy level will match the group number.

11. Insert picture of periodic table.
Groups 3 through 12 do not follow any particular rule to determine the number of Valence electrons.

12. Insert picture of periodic table.
In groups 13 to 18 – The Valence electrons for each of these is the group number minus 10. For example Group 14 – 10 = 4 Valence electrons.

13. Elements whose atoms gain, lose (ionic bonding) or share (covalent bonding) electrons are reactive, and they combine to form the many compounds we use in our daily lives.

14. Elements are categorized as metals, nonmetals or metalloids.
Metal: An element that has luster, is malleable and ductile, and is said to be a good conductor of heat and electricity.

15. What is luster, malleable and ductile?
Luster describes the way a surface reflects light…therefore metallic luster would be shiny like a metal object.
Malleable means to be able to press or pound the substance into sheets or different shapes.
Ductile means that the substance can be drawn out into thin wires.

16. Elements are categorized as metals, nonmetals or metalloids (cont’).
Nonmetals: Elements that are usually a gas or a brittle solid at room temperature. It is a poor conductor of heat and electricity.

17. Elements are categorized as metals, nonmetals or metalloids (cont’).
Metalloid: an element that shares some characteristics or properties with both metals and nonmetals.

18. Group 1 and 2 Elements:
These elements are so reactive that they are only found combined with other elements in nature.

19. Group 1: Alkali Metals Soft – can be cut with a knife3 Li
Lithium
6.941 11 Na
Sodium
22.990 19 K
Potassium
39.098 37 Rb
Rubidium
85.468 55 Cs
Cesium 87 Fr
Francium
Group 1: Alkali Metals
Soft – can be cut with a knife
Shiny and silver colored
Low Density (some will even float)
Most reactive of the metals
Valence electrons = 1
Reacts violently with water forming a hydrogen gas
Compounds from these are very useful such as NaCl

20. Silver colored Group 2: Alkaline- Earth Metals4 Be
Beryllium
9.012 12 Mg
Magnesium
24.305 20 Ca
Calcium
40.078 38 Sr
Strontium
87.62 56 Ba
barium 88 Ra
Radium
226
Group 2: Alkaline- Earth Metals
Very reactive but not as reactive as Alkali Metals.
Silver colored
More dense than Group 1 metals
Valence electrons = 2
Useful compounds include: Calcium compounds such as cement, plaster, chalk, and YOU.

21. Group 3 to 12: Transition Metals

22. Higher density and melting points (except mercury) than Group 1 and 2
Group 3 to 12: Transition Metals
Do not lose their valence electrons as easily as groups 1 & 2.
Less reactive than Alkali and Alkaline Earth metals
Shiny
Good conductors of electricity
Higher density and melting points (except mercury) than Group 1 and 2

23. Group 3 to 12: Transition Metals (cont’.)
Lanthanides: The first row underneath the periodic table: Shiny, reactive, many are used in the production of steel.
Actinides: The second row underneath the periodic table: These elements are all radioactive and unstable..
Note: Elements found after 94 (Plutonium) are man made and not found in nature

25. Solid at room temperature
Group 13: Boron Group
Reactive
Valence electrons = 3
Contains 1 Metalloid and 4 Metals
Solid at room temperature
Aluminum is the most abundant in this group and the most common in the Earth’s crust 5 B
Boron
10.811 13 Al
Aluminum
26.982 31 Ga
Gallium
69.723 49 In
Indium 81 Tl
Thallium

26. Reactivity varies in this group depending on the element6 C
Carbon
12.011 14 Si
Silicon
28.086 32 Ge
Germanium
72.64 50 Sn
Tin 82 Pb
Lead
207.2
Group 14: Carbon Group
Reactivity varies in this group depending on the element
Valence electrons = 4
This group contains 2 metals, 1 nonmetal and 2 metalloids.
Many forms found uncombined in nature such as diamonds
Compounds are very useful: proteins, fats, carbohydrates, computer chips.

27. Reactivity varies in this group depending on the element
Group 15: Nitrogen Group
Reactivity varies in this group depending on the element
Valence electrons = 5
Group contains 1 metal, 2 Nonmetals, and 2 metalloids
Phosphorous is very reactive and only found in nature combined with other elements.
All but nitrogen are solid at room temperature.
Nitrogen makes up 78% of our atmosphere.
Generally unreactive. 7 N
Nitrogen
14.007 15 P
Phosphorous
30.974 33 As
Arsenic
74.922 51
Sb Antimony 83 Bi
Bismuth

28. More reactive than group 15 Valence electrons = 6
Group 16: Oxygen Group
More reactive than group 15
Valence electrons = 6
Group contains 1 Metals, 3 Nonmetals and 1 Metalloids
Sulfur is found in nature and is used to make sulfuric acid, a very commonly used chemical in industry.
All but oxygen are solid at room temperature.
Oxygen makes up 21% of the Earth’s Atmosphere
Oxygen is very reactive and combines with many other elements especially metals
Rust is the result of the oxidation of metal. 8 O
Oxygen
15.999 16 S
Sulfur
32.065 34 Se
Selenium
78.96 52
Te Tellurium
127.60 84 Po
Polonium
209

29. Group 17: Halogen Group Very reactive Valence electrons = 7
Nonmetal group
Poor Conductors of electricity and heat
React violently with alkali metals to form salts
Never found uncombined in nature
Atoms of these elements only need to gain 1 electron to fill their outer shell
Chlorine and Iodine are both in this group and can be combined to make disinfectants. 9 F
Fluorine
18.998 17 Cl
Chlorine
35.453 35 Br
Bromine
79.904 53
I Iodine 85 At
Astatine
210

30. Group 18: Noble Gas Group Non-reactant Valence electrons = 82 He
Helium
4.003 10 Ne
Neon
21.180 18 Ar
Argon
39.948 36 Kr
Krypton
83.80 54
Xe Xenon 86 Rn
Radon
222
Group 18: Noble Gas Group
Non-reactant
Valence electrons = 8
Outermost energy shell is full
Colorless, odorless gases at room temp.
Under normal conditions they do not react with other elements
All found on Earth in very small amounts
Argon is the most common in the group
Their non-reactivity makes them very useful for light bulbs, helium for blimps and weather balloons.

31. Properties do not match the properties of any single group
Hydrogen Stands Alone:
Properties do not match the properties of any single group
Valence Electrons = 1
Easily looses that one valence electron
Physical properties are like the nonmetal group
Most abundant element in the Universe
Its reactive nature makes it useful as a fuel for rockets. 1 H
Hydrogen
1.008

32. Insert picture of periodic table.

33. Periodic Table Exit Ticket
Elements are arranged on the PTE by increasing what? Who came up with this organization?
What do the valence electrons have to do with bonding/reactivity of an atom?
What is a key characteristic of the noble gasses that makes them different from the other elements? (being a gas, is not the answer, think about how many valence electrons they have)

34. Elementals Homework
You will be assigned an element and you will need to do research on this element.
You will make a foldable, and on the front you will design the block of the periodic table that your element appears in so that it has the same information that can be found on the periodic table.
On the 2 sides of the open foldable, you will design and describe a superhero or super villain. That superhero/super villain needs to have properties or powers that line up with the properties of the element you were assigned.
Draw the hero/villain on the left side and write the description of their powers on the right.
Do this on colorful paper or use lots of colors in the drawing and fold the paper hamburger style not hot dog.
We will post this as a giant periodic table in the hallway so everyone can see

35. Chemical Bonds & Reactions- + + -

36. Chemical Bond
A force of attraction that holds two atoms together (electromagnetic force)
Has a significant effect on chemical and physical properties of compounds
involves the valence electrons
Valence Electrons – the electrons in the outermost energy level of an atom
This Lithium
Atom has one
valence electron

37. Counting Valence Electrons
Carbon
4 valence
electrons
Beryllium
2 valence
electrons
Oxygen
6 valence
electrons

38. Determining the Number of Valence Electrons by Using the Periodic Table
*Atoms of elements in Groups 1 and 2 have the same number of valence electrons as their group number.
*Atoms of elements in Group 3-12 do not have a general rule relating their valence electrons to their group number. However, they typically have between 1 or 2 valence electrons.
*Atoms of elements in Groups have 10 fewer valence electrons than their group number. (Exception - helium atoms have only 2 valence electrons, even though they are in group 18)

39. How Many Valence Electrons?
Hydrogen
Lead
Xenon
Sulfur
Rubidium
1 Valence
Electron
4 Valence
Electrons
8 Valence
Electrons
6 Valence
Electrons
1 Valence
Electron

40. CONSIDER EIGHT A HAPPY NUMBER FOR ATOMS!
The Octet Rule
Atoms will combine to form compounds in order to reach eight electrons in their outer energy level.
Atoms with less than 4 electrons tend to lose electrons.
Atoms with more than 4 electrons tend to gain electrons.
Be aware that there are some exceptions!
CONSIDER EIGHT A HAPPY NUMBER FOR ATOMS!

41. The Octet Rule In Action6 7
Notice how this chlorine atom has seven valence electrons, one away from eight. It will try to gain one more according to the Octet Rule. 5 + - 4 1 1 2 3
Notice how the sodium atom has one valence electron. It is this electron that it will try to get rid of according to the Octet Rule.
Where do you think Chlorine finds that one electron that it needs?

42. Lewis Structure (Electron Dot Diagram)
a way of drawing the outer energy level electrons (valence) of an atom
The symbol for the element surrounded by as many dots as there are electrons in its outer energy level (valence)
Examples
How many valence electrons do each of these atoms have?

43. Making an Electron Dot Diagram
Element “X” has 8 valence electrons
Write down the element’s symbol
and place the first two dots on any
side of the symbol. 1 2 3
If this were an atom of an element
from group 1, you would just place the
one dot on any side of the element.
Place the rest of the dots in either a
clockwise or counter clockwise manner around
the symbol, with no side receiving two dots
until each side gets one. 4 5 6 7

44. What Would the Electron Dot Diagram Look Like?
1 Valence Electron
6 Valence Electrons H O
How many valence
electrons does
each atom have? Ne Sr
8 Valence Electrons
2 Valence Electrons

45. Oxidation Number
The charge that an atom would have if it lost or gained electrons; ionic charge
Can be helpful in determining which atoms will interact or bond with each other
Example:
According to electron dot diagram for Magnesium, it has two valence electrons. Because Magnesium is “unhappy” with two, it will typically lose them. If this happens it will turn into a Magnesium ion. At this point it will have an oxidation number of +2. 2+ Mg

46. What Could the Oxidation Number Be?
+1 or -1 because it can
gain or lose one electron
-2 because it will
gain two electrons Ne Sr
0 because it will not
gain or lose electrons
+2 because it will
lose two electrons

47. 3 Types of Chemical Bonds
Ionic
Covalent
Metallic
What can you describe about each of these
bonds just by looking at the name?

48. IONIC BONDS
The force of attraction between oppositely charged ions.
Occurs after a transfer or loss/gain of electrons
Usually form between atoms of metals and atoms of non-metals
Resulting compounds have a name that usually ends in –ide 1- 1+ Cl Na
Which different groups or families
of elements will most-likely
interact to create these types
of bonds? -
Example - Sodium Chloride (NaCl)

49. COVALENT BOND
A force that bonds two atoms together by a sharing of electrons
Each pair of shared electrons creates a bond
Usually occurs between atoms of non-metals H O H - - - - + - + + - - - - -
Example – Water (H2O)

50. Types of Covalent Bonds
Different covalent bond types share a different number of electrons
Water (H2O)
Carbon Dioxide (CO2)
Nitrogen (N2)
Single Bonds Share 2 Electrons
Double Bonds Share 4 Electrons
Triple Bonds Share 6 Electrons

51. Chemical Bonds Exit Ticket
What do Lewis Dot diagrams represent and how can we use them to determine an atoms oxidation number?
What is the main difference between ionic and covalent bonding and why are there 3 types of covalent bonding?