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Vocabulary Preview
Prefixes/Suffixes/Roots
OctEight
MultiMany
DiTwo
NonNot
SemiSomewhat
ElectrHaving to do with electricity
Key Vocab
1. Group
2. Period
3. Periodic Table
4. Atomic Shells
5. Valence Electrons
6. Atomic Number
7. Symbol
8. Average Atomic Mass
9. Oxidation Number
10. Octet Rule
11. Multivalent
12. Diatomic
13. Metals
14. Nonmetals
15. Metalloids
16. Electron Configuration
17. Periodic Law
18. Halogen
19. Noble Gas
20. Alkali Metal
21. Alkaline Earth Element
22. Transition Metal
23. Lanthanide
24. Actinide
25. Semiconductor
26. Atomic Radii
27. Ionization Energy
28. Electronegativity
29. Ionic Radius
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Read p. 155. How did chemists begin the process of organizing
elements?
How many elements had been identified by 1700?
Read p. 156. What method did Mendeleev use to develop his
periodic table?
Mendeleev arranged the elements in his periodic table in order
of increasing _______________________.
Why did Mendeleev leave question marks, or spaces, in his
periodic table?
Read p. 157. What problem occurred with Mendeleev’s
periodic table?
Moseley arranged his periodic table in order of increasing
_______________________.
Whose periodic table is the one we have today – Mendeleev or
Moseley?
What is the periodic law?
Mrs. C Check
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Organization of the PT
Periods
 _____________ are called periods.
 All of the elements in a period have the same
number of _______________________.
 As we increase the atomic number, the electrons fill
the energy levels.
 Energy levels are labeled…
Groups
 The _______________ of the PT are called groups.
 The elements in a group have the same number of
________________________.
 Valence electrons are the
 They are very important to _______________.
 Every element in the first column (Group 1) has
_____ electron in its outer shell. Every element in
the second column (Group 2) has _____ electrons
in its outer shell. Etc.
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Symbols on the Periodic Table
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K
39.1
Let’s Label the PT
1. Oxidation number =
 Relates to…
 To become stable an atom wants ____ electrons
 THE OCTET RULE:
2. Multivalent –
3. Diatomic Molecules –
o Only diatomic when ___________!
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4. Metals, Nonmetals, & Metalloids
TYPE
LOCATION
PROPERTIES
Metal
Nonmetal
Metalloid
6.2 Classifying the Elements
Groups of the Periodic Table
Group 1: Alkali Metals



Very Soft

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Group 2: Alkaline Earth Elements


Not Found in Nature
Group 3 – 10: Transition Metals

 Electrons they use to bond are in more than one
shell (MULTIVALENT)

Metalloids


 Semiconductors
Group 17: Halogens

 Exist as all three states of matter at room
temperature

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Group 18: Noble Gases
 Contain 8 electrons in outer shell (oxidation
number of 0) = STABLE

Lanthanides (57-71) & Actinides (89-103)
 Most are synthetic, or man-made

Actually in Period 6 & 7

6.3 Periodic Trends
Periodic Trends
Activity Series of Metals –
 Most Reactive =
 WHY? The further to the left and down you go, the
easier it is for ______________ to be given or
taken away.
Activity Series of Nonmetals –
 Most Reactive =
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 WHY? The further right and up you go, the
stronger the element can “grab” other
________________ or ______________.
Atomic Radii
 Calculated by finding…
 PERIOD TREND: Atomic radius
____________________ as you go left to right
across a period.
 WHY?
o Determined by the strength of the attraction
between the nucleus and the outermost
electrons
o __________________ the attraction,
__________________ the size of the atom
o More Protons =
 GROUP TREND: Atomic radius
____________________ as you go down a group
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 WHY? There is a significant jump in the
________________________________ as well as
the _____________________________________.
Ions
 An atom or group of atoms with…
o Cation =
o Anion =
Ionization Energy
 Energy required to ______________ an electron
from the neutral atom to form a positively charged
ion _______________
 PERIOD TREND: Ionization energy
____________________ as you go left to right
across a period.
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 WHY?
o Metals (left)_____________ to get rid of
their electrons, therefore it …
o Nonmetals (right) ___________________ to
get rid of their electrons, therefore it…
 GROUP TREND: Ionization energy
____________________ as you go down a group
 WHY?
o Shielding Effect – Caused by an increasing
number of electrons between the outer level
and the nucleus
o Blocks the ___________________ of the
nucleus for the ________________.
o Causes…
 Ionization energy relates to…
o The highest ionization energy = the most active nonmetal (Fluorine)
o The lowest ionization energy = the most active metal
(Francium)
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 As electrons are removed, the ionization energy
___________________.
 Large jumps of energy indicate a removal of an
electron from a new shell.
 Example: For Na the IE for each successive
electron are 496 kJ/mol, 4562 kJ/mole, 4912
kJ/mol, and 5544 kJ/mol. How many valence
electrons does Na have?
Ionic Size
 Cations are always __________________ than the
atoms from which they form.
 Anions are always ___________________ than the
atoms from which they form.
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Electronegativity
 Ability of an atom to …
 Discovered by ____________________.
 PERIOD TREND: Electronegativity
____________________ as you go left to right
across a period.
 WHY?
o Elements on the left side have
_________________________ that they
would rather give away than “grab” another
element’s electrons, so they have _________
electronegativity
o Elements on the right side only need a few
electrons they want to “grab” another atom’s
electrons giving them ___________
electronegativity.
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 GROUP TREND: Electronegativity
____________________ as you go down a group
 WHY?
o Elements near the top of the PT have
__________________________ to begin
with so they have a stronger desire to acquire
more electrons
_____________________________.
o Elements near the bottom have so many
electrons already, that gaining or losing an
electron is no big deal
_____________________________.
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Additional Notes
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