1. Chapter 6
PERIODIC TABLE

2. How does Electron Configuration relate to the Periodic Table?2 10 6 14 1 3 4 5 7 2 3 4

3. Do Now Which statement is true? (use Periodic Table)
Elements in the same column ↕ has same # of outer shell electrons
Elements in the same row ↔ has same # of outer shell electrons

4. Dmitri mendeleev (1869) Arrangement: Interesting observations:
produced the first periodic table for the known 63 elements
Arrangement:
Increasing atomic mass
kept similar elements in a column
left blanks for unknown elements
Interesting observations:
Mendeleev predicted the properties of the missing elements.

5. Mendeleev’s pt

6. Henry moseley (1914) Arrangement: Increasing atomic number
Interesting observations:
Discrepancies in Mendeleev’s table disappeared (Te before I)

8. Parts of periodic table
Vertical
Column
Row
Group
Period
Family

9. Same # of occupied energy levels

10. Groups or families
Same # of electrons in their outer orbital
Share similar chemical properties

11. Properties of Metals, Non-metals, & Metalloids
Conducts heat & electricity
Ductile
Malleable
Luster
Solid at room temp. (except Hg)
Forms cations (+)
Non-Metal:
Brittle
S/l/g at room temp.
Forms anions (-)
Metalloids
Semi-conductors
Properties of nonmetals and metals

12. Metals, non-metals, & metalloids
Note: Most elements are _________
metals

13. Tour of the Periodic Table
Main-group elements
Also called representative elements (s- and p-blocks)
E- config: regular & consistent
Group: same # of val. e-

14. Tour of the Periodic Table
Inner Transition Metals

15. Alkali Metal (Group 1, except H)
Hydrogen
Most common element in universe
charge: 1+ or 1-
Alkali Metal (Group 1, except H)
Highly reactive with water
Soft and can be easily cut
Charge:1+
Alkaline-earth metal (Group 2)
Less reactive than alkali metals
Harder than alkali metals
Charge: 2+

16. Transition metals (d-block)
No identical valence electrons (charge varies)
Less reactive than group 1 & 2
Inner Transition metals (f-block)
Nuclei are unstable – radioactive
(charge varies)

17. Halogens (Group 17) Most reactive group of non-metals
Likes to react with alkalis to produce salts
charge :1-

18. Noble gases (Group 18) Low chemical reactivity b/c very stable
Outermost energy level is full
Does not form ions
Glow brightly when an electric discharge is passed through them

19. Do now: Copy names into pg-2
Inner Transition Metals

20. Alkali Metals: Na loses 1 e-
Formation of ions
Octet rule:
atoms are most stable when they have 8 val. e-
CATION: (+) ions
Alkali Metals: Na loses 1 e-
1s22s22p63s s22s22p6
(Na) (Na+) Ne
E- config
Bohr Diagram

21. ANION: (-) ions Halogens: Cl gains 1 e-
1s22s22p63s23p s22s22p63s23p6
(Cl) (Cl-) Ar

22. As you look down a column, the outermost principle energy level __________________. (but the number of valence e-‘s stays the same) As more and more levels become filled with electrons, the nucleus becomes ______________ effective at attracting the outer electron(s). This is known as the “shielding effect.” (As you look down a column, even though the nucleus theoretically is stronger since it has more protons, it is NOT effective at holding onto the outer electrons.) Which energy level has NO shielding? ____________ Which atom holds onto the outer electron tighter, K or Rb? Why? ____ has one more filled level than ____ and therefore is _____ effective at holding onto the outermost (valence) electron.
INCREASES
LESS 1 Rb K
LESS
Pg-7

23. Is the shielding effect an issue with a row?_____ Row, Period , Series
Val n=2 n= n= n= n=2 n= n= n=2
energy level 
 filled ____ ____ ____ ___ ___ ____ ___ ____
Levels
The energy level is not changing. What is changing?
Is the nucleus getting stronger?_________. Is it effective?________
In a row, ___________ ___________(and not shielding) determines the trend. NO
2 b/c noble gas 1 1 1 1 1 1 1
# of electron & protons
YES
YES
NUCLEAR CHARGE
Pg-8

24. Recap: Column: the __________ _________ dictates the trends
Recap: Column: the __________ _________ dictates the trends. Row: the increasing strength of the __________ dictates the trends.
ELECTRON SHIELDING
NUCLEUS

25. Atomic Radius (pg-9) Distance from nucleus to outer electrons
Bond radius = ½ distance between nuclei of adjacent atoms.

26. Atomic Radius Down a Group: Increases Reason:
more energy levels
more shielding
Across a Period: Decreases
More nuclear charge (+) pulls outer most e- closer to nucleus

27. Ionic radii (pg-9) positive lose smaller gain negative larger
Metals tend to _________ electrons and become ____________ions. (gain or lose) positive or negative) ** (metal ions are ___________than metal atoms) (smaller or larger) Non- metals tend to _______ electrons and become __________ ions. (gain or lose) (positive or negative) ** (non-metal ions are ______________than non-metal atoms) (smaller or larger)
smaller
gain
negative
larger

28. Ionization Energy (IE) – pg10
Energy required to remove an electron from an atom or ion (form (+) ion).

29. Ionization Energy (IE)
Down a Group: Decreases (easier to remove an electron)
Reason:
1. more energy levels (outermost electrons are farther from nucleus)
2. more shielding (less attraction btw p+ & val. e-)
Across a Period: Increases (harder to remove an electron)
1. more nuclear charge, p+ ↑
2. radius decreases
Electron-shielding remains the same

30. Circle the correction answer & answer the last 2 questions
Ionization Energy pg-10
Circle the correction answer & answer the last 2 questions
Lower down in a column the atoms are larger / smaller and have more attractiveness / shielding so it is easier to remove an e- from the outer shell. It is harder/easier to remove an electron from a small atom with no shielding. It gets harder/easier to remove that electron as you move to the right as it approaches a perfect octet. Which column would be very difficult to go in and remove and electron from? Noble gases So the column with the highest Ionization Energy = Group # 18, Noble gases

31. IE
Which element has the least IE? the most?

32. #3 Electronegativity (pg-11)
the attraction of an atom to a pair of electrons in a bond
**EXCEPT NOBLE GASES
Fluorine has the highest value of “4.0”

33. Electronegativity (EN)
Down a Group: Decreases (less attraction towards bonding e-)
Reason:
1. more energy levels
2. more shielding
Across a Period: Increases (more attraction towards bonding e-)
1. radius decreases (val. e- closer to nucleus)
2. nuclear charge increases, p+ ↑

34. Which column does NOT bond with any element (because it has a perfect
Fluorine atom pulls harder on the shared pair of electrons. They are shared “unevenly”
Electronegativity of Fluorine is > , = , < the electronegativity of hydrogen
Chlorine atoms share the pair of electrons “evenly”
Electronegativity of Chlorine is > , = , < the electronegativity of Chlorine
In water, does Hydrogen or Oxygen pull harder on the shared pair of electrons? ____________
Which column does NOT bond with any element (because it has a perfect
octet)? ____________________ (No electronegativity values are assigned)
NOBLE GASES

35. MOLECULE/MOLE/MASS CONVERSIONS FOR DIATOMIC ELEMENTS
Atomic mass: mass in grams = 1 mole of that element Example: 12 g C = 1 mol C Molecular mass: mass of a molecule = 1 mole of that molecule Example: 32 g O2 = 1 mol O2 Diatomic Elements (BrINClHOF): Br2 I2 N2 Cl2 H2 O2 F2 Elements found in pairs