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Periodic Table
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2. Good morning! Take out your notes from yesterday and be ready to start
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Todays agenda – November 8, 2016
Cornell notes Periodic Table
Periodic Table Questions Review
Element Bingo
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3. Standard
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SPS4 Students will investigate the arrangement of the Periodic Table.
a. Determine the trends of the following:
Number of valence electrons
Types of ions formed by representative elements
Location of metals, nonmetals, and metalloids
Phases at room temperature
b. Use the Periodic Table to predict the above properties for representative elements.
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4. Essential Question How and why is the periodic table arranged?
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How and why is the periodic table arranged?
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5. Organization of the Elements
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Periodic Table 1st organized by Dmitri Mendeleev in the 1860’s
There were only 60 known elements
First organized by atomic mass and chemical properties, now by atomic number
There were gaps in the table because other elements had not yet been discovered
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6. Periodic Law
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Elements are organized by atomic number and similar chemical properties
Also organized by metals, metalloids, nonmetals
Metals tend to be solids at room temperature
Nonmetals tend to be gases at room temperature
Exception – Hydrogen is a gas at room temperature
Metalloids are also called Semiconductors
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7. Periods Each row is a period
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Each row is a period
From left to right elements become less metallic
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8. Groups Each column Each group has the same number of valence electrons
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Each column
Each group has the same number of valence electrons
Because of the valence electrons each group has similar properties
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9. Periodic Table Labeling
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Need periodic table
We are going to label it
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10. Ion Formation and Oxidation Numbers
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Ion Formation and Oxidation Numbers
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11. Octet Rule Octet Rule What do they do if they don’t have 8 electrons?
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Octet Rule
Elements want 8 electrons to be stable and happy
What do they do if they don’t have 8 electrons?
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12. Ions
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Elements will either lose or gain electrons from other elements in order to get the number of electrons they need to be stable
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13. Ions
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The number of electrons lost or gained depends upon the number of valence electrons
Easier to lose a few electrons
Group 1 – gives up its 1 electron easily
Group 17 – wants to gain 1, not lose 7
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14. Ions
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As an electron is lost or gained, the number of electrons no longer equal to the number of protons (atomic number)
This causes the element to have either a positive or negative charge = Ion
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15. Lose Electron Lose an electron get a positive charge
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Lose an electron get a positive charge
Ex: Lithium, valence electron = 1, Li+
Ex: Beryllium, valence electron = 2, Be+2
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16. Gain Electron Gain and electron get a negative charge
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Gain and electron get a negative charge
Ex: Fluorine, valence electrons = 7, F-
Ex: Oxygen, valence electrons = 6, O2-
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17. Oxidation Numbers
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Oxidation Number = the number of electrons an element needs to gain or lose
This is opposite of Ion Charge!
Group 1 = -1
Group 2 = -2
Group 3 = -3
Group 4 = -4 or +4
Group 5 = +3
Group 6 = +2
Group 7 = +1
Group 8 = 0 (already has all it needs)
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18. Where does it go? Group 1 and Group 7 often go with each other – why?
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Group 1 and Group 7 often go with each other – why?
Which Group often goes with Group 2? Why?
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